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Thank you Dr for the detailed explanation for group VIA. This is my summary for Group VIA.

-Group VIA is known as Chalcogens Group:
-It Metallic characteristic increase going down the group.

OXYGEN
-Exist as atmospheric gaseos
- Form 2 allotropes Oxygen,O2 and Ozone,O3.
Preparation :
Commercial form:
Fractional distillation of liquid air to separate O2.
In Lab:
-Heating of KClO3.
-Decomposition of H2O2.
-Electrolysis of water, H2O
Ozone,O3
-colourless gass
-blue colour in liquid form
-used as detergent
Oxide
-form normal oxide, high oxide, suboxide and mix-oxide (spinel compund)
Hydide
-polar molecule
-act as ligand
-act as oxidizing and reducing agent

Sulfur
-exist as S8 molecule
-2 allotropes rhombic sulphur and monoclinic sulphur.
-It is extracted by Frasch Process.
-Compound which is oxide, oxoacids, halides.

# data[].attributes.body
Thank you dr for the explanations in the lectures. Here is my summary of Group VIA:
- Group VIA is also known as the Chalcogens Group.
-Valence electron : 6
- Metallic characteristics increases as going down the group
- ionization energy decreases as going down the group due to the decreased shielding effect
Oxygen
-  Exists in the atmospheric gaseous
- Has 2 allotropes : Oxygen gas & Ozone
-Oxygen gas:  colourless gas while in liquid form  is blue coloured
- Ozone : a blue coloured gas while in has a dark blue colour in liquid state
- Water, H2O is a colouless in solid, liquid & gas state
- water is an amphoteric compound
Sulfur
-Has 2 allotropes
Extracted by  using a porcess called Frasch process
- A odourless, tasteless & non-metallic solid with a light yellow colour.
- Sulfur is used in making black gunpowder and a main component in vulcanization of natural rubber
-2 types of sulfur oxide : Sulfur dioxide & sulfur trioxide
-Reaction of SO2 with water can cause H2SO4(acid rain)
-Sulfuric acid is used as fertilizers, a dehydrating agent & to produce hydrochloric acid

# data[].attributes.body
Thank you dr for the class on group IVA. This will be my summary for this chapter.
Group VIA
Characteristic:
- Metallic character increase down the group
- IE decrease down the group
- Oxidation state -2 are stable for O
Oxygen,O2
- Anionic mineral in earth crust
- Form 2 allotropes
Oxygen, O2
Ozone, O3
Preparation
1. Commercial
- Fractional distillation of liquid air
2. In lab
- Heating of KCiO3
- Decomposition of H2O2
- Electrolysis of water uses graphite as electrodes
Characteristics
- Colourless gas
- Blue liquid
- Paramagnetic with unpaired electrons
- Reactive and combine with most of elements
Uses
- Producing "fuel cell"
- Respiration
- Welding industries
Ozone,O3
Characteristics of ozone
- Blue gas
- Dark blue liquid
- Strong oxidising agent
Testing for mercury
- Use Hg
Uses of O3
- Substitue Cl2 in water treatment
- Detergent, deodorizer and preservative
- Ozone treatment
Compound of oxygen
- Oxide
- Peroxide
- Superoxide
Sulphur
- Exist as free element
- Ores: pyrite, galena, sphalerite
Extraction of Sulphur
- Frasch Process (obtain with 99.5% purity)
Properties of Sulphur
- Odourless, tasteless
- Cannot dissolved by water
- Reactive element
- Burn in blue flame
Uses
- Produce H2SO4
- Uses in black gun powder
- Vulcanization of natural rubber
- Bleaching
Compund of Sulphur
- Metallic sulphide(ionic)
- Non-metallic sulphide(covalent)
Oxides of Sulphur
1. Sulphur dioxide
- React with water form acid solution
- Reducing agent
- Oxidizing agent
- React with alkali form sulphite salt
Source
- Volcanoes activities
- Combustion of sulphide ores, coal and oil
- Roasting anhydride CaSO4 with coke
- Reaction of sulphite salt with acid
- Reaction of metal with conc sulphuric acid
2. Sulphur trioxide
- Form SO3 crystal when cooled
- Reaction with sulphuric acid form oleum

# data[].attributes.body
Thank you Dr for the lessons,
here are my summary for group IVA

-known also as chalcogens group
-the metallic character increase,IE and shielding effect decrease down the group
-stble oxidatuion state for o is -2,while other members -2 to +6
-oxygen different from thers member based on electronegativity and  strong forming bond.

OXYGEN
-2 allotropes: oxygen(o2),ozones(o3)
oxygen
-preparation: commercial-from frictional distillation liquid air
lab-heating of KClO3,decomposition of H2O2,electrolysis of water
O2 is paramagnetic
-uses:producing fuel cell, respiratin,welding industries.
ozone
-formation- directly,photochemical decomposition of NO2,industrial involved electrical discharged O2 gaseous
-strong oxidation agent
-dark blue liquid
-mercury was uses to test the presence of o3.
-uses:detergent,deodorizer, preservatives
OXIDES
oxides:paramagnetic
peroxide:diamagnetic
superoxide:paramagnetic
-oxide,high oxide,suboxide,mix-oxide
HYDRIDES- water (act as ligand)
HYDROGEN PEROXIDE-book shaped structure,bleaching agent

SULPHUR
exist as S8 molecule (crown shape)
-2 allotropes:
rhombic sulphur,monoclinic sulphur
-extraction by Frasch Process
-odourless,not readily wetted,high degree of solubility
-uses: to produce sulphuric acid
COMPOUND OF SULPHUR
-metallic sulfide (ionic sulfide)
-non-metallic sulfide (covalent sulfide):hydrogen sulfide,carbon disulfide
OXIDES
-SO3 - preparation by contact process,heating of ferum(III) sulfate,dehydration of conc.H2SO4
OXOACIDS
-sulfurous acid (H2SO3), salt obtained by reacting acid with alkali
-sulfuric acid (H2SO4) ,dibasic acid,strong acid,uses for fertilization,dehydrating agent,chemical detergent,industrial manufacture :contact process
HALIDES
-disulphur dihalides-S2F2,S2Cl2,S2Br2
-sulphur tetrahalides,SX4
-sulphur hexahalides,SX6

thiosufuric acid is not stable ,uses for quantitative analysis iodometry ,used to removed silver (I) salt

# data[].attributes.body
Thank you very much for today’s lessons Dr.

Here summary for Group VIA

Down the group:

metallic character increases

IE decrease

Compounds form

ionic (Group IA & IIA)

covalent (most elements)

Oxygen different

very high electronegativity

forming strong ppi-ppi bonds with O, C, N

Oxygen, O2

exist in the atmospheric gaseous

anionic mineral in earth crust

form 2 allotropes (O2 & O3)

Preparation:

Commercial:

From fractional distillation of liquid air - separate O2

Laboratory:

Heating KClO3

decomposition H2O2

Electrolysis of water use graphite as electrode

Characteristics:

colourless gas

liquid form (blue liquid)

paramagnetic with 2 unpaired e-

reactive at elevated temperature and combine directly with most elemnts (except noble gas)

Uses:

producing fuel cell

respiration

welding industries

Ozone, O3

Formation

O + O2 ---> O3

Photochemical decomposition of NO2

Industrial - electrical discharged of O2 gaseous

Characteristics

blue gaseous

dark blue liquid

smelly

strong oxidizing agent

Uses:

in susbtitute of Cl2 in water treatment - kill bacteria

as detergent, deodorizer, preservative

in atmosphere: prevent high energy UV from reach earth

Oxides

Oxide (O2-) - paramagnetic

Peroxide ((O2)2-) - diamagnetic

Superoxide ((O2)-) - paramagnetic

Properties:

Natural of bonding

acid-base

Acid-base:

Oxidation increase, acidity increase

Hydrides

H2O - water

Properties:

colourless liquid, gas, solid

polar molecule --> solvent for most ionic

density solid < liquid

neutral oxide -> change to acid/base depend on compound reacted (Amphoteric)

act as ligand

oxidizing and reducing agent

H2O2 - hydrogen peroxide

open book structure

Properties:

colourless syrupy liquid -> HB

thermally unstable and decompose in presence of finely divided metal catalyst

strong oxidizing agent

reducing agent

Uses:

bleaching agent

antiseptic, disinfectant and germicide

MgO2 & CaO2 as mild oxidant in toothpaste

Sulfur

exists as free element, S

ores : pyrite, galena, sphalerite

S8 molecule ( puckered ring form)

Allotropes: alpha-rhombic S and beta-monoclinic S

Extraction:

By Frasch Process : due to low melting point & low density

Properties:

odourless, tasteless, light yellow non-metallic solid

not readily wetted or dissolved by water

reactive element, combine with all other element (except inert gas, gold, platinum)

rhombic & monoclinic sulfur are soluble in organic solvents

high degree of solubility in CS2 -> dissolve rhombic sulfur

flammable & burn in air with blue flame

Uses:

to produced sulfuric acid, H2SO4

component of black gunpowder

used in vulcanization of natural rubber

used in bleaching of dried fruits and paper products

Chemical prop:

Reaction with O2 (combustion)

Heating with metal -> metal sulfides

Reaction with conc. acid

Compounds:

Metallic sulfides (ionic)

Solid and dark/black excp ZnS & PbS -> yellow

Anionic sulfide from highly electropositive metals undergo hydrolysis -> basic solution

Solid insoluble in water

React with acid --> H2S gas evolves

2) Non-metallic sulfide (covalent)

Hydrogen sulfide, H2S

colourless gas

foul smelling

extrmely toxic gas

dissolve in water --> acidic solution

easily oxidized

reducing agent

Carbon disulfides, CS2

colourless liquid, fouling smell

solvent S, P, I2, rubber, wax

hydrolyze in water

Oxides

SO2

Chemical prop:

React with water --> acidic solution (acid rain)

React with alkali --> sulfite salt ((SO3)2-) Reducing agent

Oxidizing agent

Sources:

volcanoes activities

combustion of sulfide ores, coal, oil

roasting anhydride CaSO4 with coke

reaction of sulfite salt with acid

reaction of metal with conc. sulfuric acid

* SO3

Preparation:

Contact/Touch Process

Heating of ferum(III) sulfate

dehydration of conc. H2SO4 by solid P2O5

Properties:

Forming SO3 crstal when cooled

alpha-SO3 : crystal trimetric form

beta-SO3 : cube, transpareny crystal, meta stable

gamma-SO3 : needle-like, most stable

Reaction with water

Reaction with sulfuric acid --> produced oleum

Oxoacid

H2SO3 (Sulfurous acid)

Derived from SO2

Salt : sulfite anion (SO3)2-

Properties:

Ionization

Sulfite salt obtained by react acid with alkali

dissollves in water undergo hydrolysis

H2SO4 (Sulfuric acid)

Derived from SO3

Salt : sulfate anion (SO4)2-

Properties:

dibasic acid, strong acid

viscous liquid -> HB between molecule

high bp -> HB

conc. acid: Dehydrating agent

dilute concentration: acid

conc. and hot: oxidizing agent

sulfonation agent

as catalyst - H2SO4 absorb water

H2SO4 (Sulfate salt)

obtained by react H2So4 with

alkali

metal oxide

Metal

carbonate/bicarbonate

Uses sulfuric acid

Fertilizers

Chemical for detergent, ether, ester

Dehydrating agent -> remove water from gas, liquid, solid

pigment -> TiO2, TiOSO4: white glow pigment in paint

produce conc. HCl

Industrial of sulfuric acid

Contact Process

Combustion S --> SO2

Oxidation SO2 --> SO3

SO3 transformation to H2SO4

- Dissolution of SO3 into H2SO4 --> oleum

- Addition of water to H2S2O7 --> H2SO4

Halides

exists for:

: X = F & Cl

: X = Br - only a few

: X = I - not exist

disulfur dihalide, S2X2

S2F2 - gas

S2Cl2 - yellow liquid

S2Br2 - unstable liquid

( decrease in stability )

hydrolysis in water

S2Cl2 react further with Cl2 --> SCl2

SCl2 reacts with ethene give mustard gas

Sulfur tetrahalide, SX4

Structure: Trigonal bipyramidal

Reactions:

Hydrlysis in water and alkali

Able to expend the octet

Sulfur hexahalides, SX6

Synthesis:

S react directly with all halogen exp iodine

Properties;

colourless, odorless, tastesless, non-toxic, thermally stable, insoluble in water

Not Lewis base, no available non-bonding

Despite +6 it is not oxidizing agent - F atoms protect S

Much better insulator than air

Thiosulfuric acid (H2S2O3) & salts (S2O3 2-)

H2S2O3 not stable

Important salt --> Na2S2O3.5H2O

Uses:

Quantitative analysis in Iodometry: titration method, use starch as indicator (blue --> decolorize)

In photography

# data[].attributes.body
Thank you Dr.Sheela for today's lecture.
Group IVA summary :

Characteristic

O, S (non metallic, insulators); Se, Te (metalloid, semiconductors); Po (metal, conductor)

IE decreases down group <- decreased shielding effect (d10, f14 inner shells_Se, Te, Po)

Form ionic bond with GIA & GIIA-form M2- ions

Form covalent bond with most elements-two covalent bonds (e.g. H2O, (CH3)2S)

Form MR- ions (e.g. OH-, HS-)

Form onium salts (e.g. H3O+, R3S+)

Form hypervalents (MR4, MR6 except O - no d orbitals)

O

Exist in atmospheric gas 21%

Anionic mineral in earth crust (carbonate, nitrate, sulphate, oxides)

Blue (l)

2 allotropes: O2, O3

Reactive at high temp.

Combine w most elements except GVIII

Very high electronegativity;

-form ionic M-O bond
-form H bond in compounds with O-H

Form strong pπ-pπ bonds with O, C, N

-e.g. O=O, O=C=O, O=N-O

Other group members:

Form rings & chains (√single bonds, metallic lattices)

Form dπ-pπ type multiple bonds (hypervalents)

*pπ-pπ bond is stronger than pπ-dπ bond

Preparation
Commercial

Separate O2 by factional distillation air(l)

Lab

Heat KClO3(s)

Decompose H2O2

Uses

Produce fuel cell

Respiration

Welding industries

O3, Ozone

Dark blue (l)

Strong oxidation agent

Formation

1. O + O2 h> O3

2. Photochemical decomposition of NO2

3. Industrial production (chemical discharged of O2(g) -> cooling to (l) -> distillation)

Testing
Mercury: bright shining -> tarnish, stick to glass surface
Uses

Substitute Cl in water treatment;

-high cost
-does not react w HC (Cl2 does -> carcinogenic)
-does not produce smell/taste to water
Prevent high E UV(involved in both formation & destruction of O3) from reaching earth

Ozone treatment

Oxides

O²-, Oxides, Paramagnetic, 12e-; 2O²- =diamagnetic, 16e-

O2²-, Peroxide, Diamagnetic, 14e-

O2-, Superoxide, Paramagnetic, 13e-

*Bond length O²- < O2- < O2²-

Oxides (follow valence rule)

High oxide (O content > actual)

Suboxide (O content < actual)

Mix-oxide: spinel compound

Properties

Bonding: Ionic, covalent, intermediate

Acid-base: Strong acidic, neutral, amphoteric, strong base

*Oxidation state is directly proportional to acidity

Water, H2O

sp³, bent

Polar: solvent for most ionic & polar compounds <- form H bond

Density (s) < (l)

Amphoteric: change to acid / base depends on compound reacted

Act as:

-ligand
-oxidizing & reducing agent

Hydrogen Peroxide, H2O2

Book-shaped structure

Colourless syrupy liquid <- H bond

Miscible w water, soluble in alcohol

Thermally unstable:

-decomposes in presence of finely divided metal
2H2O -> 2H2O + O2

Strong oxidizing agent, reducing agent

Uses

Bleaching agent ( wool, hair, teeth)

Antiseptic, disinfectant, germicide

MgO2, CaO2: mild oxidant in toothpaste

S: brimestone

Exist as:

1. Free element <- volcanic gas, H2S

2. Ores: FeS, PbS, ZnS

3. S8 molecule (crown shape):

alpha-rhombic S --97°C--> beta-monoclinic S
*Both limitedly soluble in most organic solvents
*CS2 √high degree solubility (often used to dissolve rhombic S)

Extraction

Mined by Frasch Process (low m.p): 99.5% purity:

3 concentric pipes:

1. Pump superheated water down outermost pipes

2. Pump compressed air down innermost pipes

3. Mixture (hot water + molten S + air) comes up middle pipe

Properties

Odorless, tasteless

Light yellow

Float on water

Flammable, blue flame

Uses

Produce H2SO4

Component of black gun powder (mixture: KNO3, C, S)

Vulcanisation of natural rubber

S compounds - bleaching (dried fruits, paper products)

Compounds

Metallic sulfide

Solid (soluble in water), dark except ZnS, PbS: yellow

Anionic sulfide fr highly electropositive metals --hydrolysis--> basic solution

S²- + acid -> H2S

Non-metallic sulfide

Colourless, foul smelling, extremely toxic

Dissolve in water -> acidic soln

Easily oxidized -> reducing agent

CS2

Colourless (l), foul smelling

Solvent: S, P, I2, rubber, wax

Hydrolyze in water -> CO2 + H2S

Oxides
SO2

sp³, bent

chocking smell, poisonous gas

Oxidizing & reducing agent

React w:

Water -> acidic soln (acid-rain)

Alkali -> sulfide salt, SO3³-

Sources

Volcanoes activities -> emission of SO2 <- high temp from rotten earth

Combustion: sulfide ores, coal, oil

Roasting: anhydride CaSO4 + coke; sulfite salt + acid; metal + {H2SO4}

SO3

Form SO3 crystal when cooled to ~-83°C

Alpha-SO3:cyclic trimeric, m.p 290K

Beta-SO3: cube, meta stable, m.p 305K

Gamma-SO3: needle like crystal, most stable

Rxn

+ water -> H2SO4

+ H2SO4 -> H2S2O7, Oleum

Preparation
Commercial

Touch/Contact Process

SO2 + O2 --V2O5--> SO3

Heat Fe(III) sulphate

Dehydration of {H2SO4} by P2O5(s)

Oxoacid
H2SO3, sulphorous acid/sulfuric(IV) acid

From SO2 + H2O

Dibasic acid

Salt: sulfite anion, SO3²- (H2SO3 - 2H+)

From H2SO3 + alkali

Dissolve in water -> hydrolysis

Sulfonation agent

H2SO4, sulphuric acid/sulfuric(VI) acid

From SO3 + H2O

Dibasic, strong acid

{H2SO4}: viscous (l) & high b.p <- H bond

Salt: sulfate anion, SO4²-

From H2SO4: - 2H+; +alkali; +oxide; +metal; +carbonate/bicarbonate

1. {H2SO4}: dehydrating agent

2. Dilute H2SO4: dilute metal

3. {hot H2SO4}: oxidizing agent

Uses

Produce {HCl}

Fertilisers: (NH4)2SO4

Dehydrating agent: remove water fr gas, solid, liquid

TiOSO4: white glow pigment

Industrial manufacture

Contact Process:

Combustion: S + O2 -> SO2
Oxidation: SO2 + O2 --V2O5--> SO3

Transformation:

Dilute SO3 + {H2SO4} -> H2S2O7 + certain amount H2O (avoid fog formation) -> H2SO4 w known conc.

Halides

Hydrolysis in water

React further w Cl2 ->SCl2

React w ethane, C2H4 -> mustard gas S(C-²CH2CL)2

Exist for: F & Cl

A few: Br

Not exist: I

DiSulfide dihalide, S2X2

Stability: S2F2 (g) > S2Cl2 yellow(l) > S2Br2 unstable(l)

Trihalide, SX4

Distorted trigonal bypiramidal

Preparation

Cl; /F

S(l) + X2 --/-73°C(inert atmosphere)--> SX4

Rxn

Hydrolysys -> SO2 + -X

+ OH- -> SO3- + 4X + 3H2O

Able to expand octet

SF4 + F2 -> SF6

Hexahalides, SX6

Synthesis directly w all haligens except I

Thermally stable, insoluble in H2O

Not lewis base <- no available lone pair e-

Not oxidizing agent <- F holds S very closely

Much better insulator than air

Thiosulfuric acid, H2S2O3

S: sp³

Not stable

Salt: S2O3²-

Important salt: Na2S2O3.5H2O

Uses

Iodometry: Quantitative analysis- titration method w starch as indicator

I: blue -> decolorize

Photograohy: remove Ag(I) salt not reduced by Ag

# data[].attributes.body
Thank you dr for the lesson and here is my summary for group VIA:
-O&S --> non-metal
Se&Te --> metalloid
Po--> metal
OXYGEN
-electronegativity very high

-strong pπ  - pπ  bonds with itself, carbon and nitrogen

-forms 2 allotropes (O2 and O3)
Oxygen(O2)
-colorless gas
-blue liquid
-paramagnetic
Ozone(O3)
-blue gaseous in color
-dark blue liquid
-strong oxidation agent
-use of mercury to test the presence of O3
-used in water treatment
-as detergent, deodorizer and preservative
-O3 layer prevent high energy UV from reaching the earth
Oxides

Oxide, O²⁻

Peroxide, O₂ ²⁻

Superoxide, O²⁻

Hydrides

Water, H2O

-sp3 hybridization (O atom)
-bent shape
-colourless liquid, solid and gas
-polar
-amphoteric character
-ligand

Hydrogen Peroxide, H2O2

-book- shaped structure
-colourless syrupy liquid due to hydrogen bonding
-strong oxidizing agent and also reducing agent
-bleaching agent
-antiseptic, disinfectant and germicide
SULPHUR
-exists as S8 molecule
-2 allotropes of sulphur

Rhombic sulphur

Monoclinic sulphur

-mined by Frasch Process
-odourless, tasteless, light yellow non-metallic solid
-flammable
-produce H2SO4
-component of black gunpowder
-used in vulcanization of natural rubber
Sulphides

Metallic Sulphide (Ionic Sulphide)

Non-Metallic Sulphide (Covalent Sulphide) eg:H2S&CS2

Oxides

Sulphur dioxide, SO2

Sulphur trioxide, SO3

Halides
-X = I – does not exist

Disulphur dihalide, S2X2

Sulphur tetrahalide, SX4

Sulphur Hexahalides, SX6

Oxoacids

Sulphuric(IV) acid,H2SO3

-dibasic acid

Sulfuric(VI) acid,H2SO4

-prepared by Contact process
-dibasic acid, strong acid

# data[].attributes.body
Thank you for today's class Dr!
summary for group VIA:
- metallic character increases, IE and shielding effect decreases down the group.
-Oxidation state of -2 are stable for O and other members -2 to +6.

-O different from other members because the electronegativity of oxygen is very high and O also differs markedly from the rest in forming strong ppi-ppi bonds with itself.
OXYGEN
- anionic mineral in the earth crust.
- form 2 allotropes which is O2 & O3.

Preparation:

*From fractional distillation of  liquid air to separate O2 (Commercial)
*Heating of KClO3, Decomposition of H2O2 and electrolysis of water uses graphite as electrodes (in lab)

- colourless gas and blue liquid
-O2 is paramagnetic with 2 unpaired electrons according to MOT.
- Reactive at elevated temperature.

-USES: producing "fuel cell' , respiration and for welding industries
- ozone form by direct reaction, photochemical decomposition of NO2 and electrical discharged of O2 gaseous.
-use mercury for testing for O3
-OXIDES: normal oxide, high oxide, suboxide, mix-oxide
-acidity increase as the oxidation number of the same element increase.

SULFUR
-exist as free element, S which form by bacterial action on volcanic gas.
- PROPERTIES: odourless, tasteless, light yellow non-metallic solid.
- Sulfur is not readily wetted or dissolved by water.
- Sulfur is flammable and burn air with blue flame.
-USES:Most of the sulfur produced is to produce sulfuric acid.
-CHEM PROPERTIES: react with O2, Heating with metal becomes metal sulfide and reaction with conc. acid.
- COMPUND SULFUR

metallic sulfide(ionic sulfide)

non-metallic sulfide(covalent sulfide)

-CHEM PROPERTIES SO2:

react with water to form acid solution

react with alkali

reducing agent

oxidizing agent

- PREPARATION SO3

contact process(commercial)

dehydration of conc H2SO4 by solid P2O5.

-OXOACID, H2SO4
-Halides of sulfur, SX4, SX6 and Thiosulfuric acid and its salts

# data[].attributes.body
Thank you Dr for class today :)

Summary for group VIA:

As go  down the group metallic character increases, IE decreases.

Form ionic and covalent compounds

Oxygen

Electronegativity very high

Forming strong pπ-pπ bond with itself , carbon and nitrogen

From 2 alloptropes oxygen and ozone

Colourless gas and blue liquid

Reactive at elevated temperature and combine directly with most element except noble gas

Uses : producing “ fuel cell “ , respiration , welding industries

Ozone , O₃

Blue gaseous in colour, smell and strong oxidizing agent

For testing of ozone uses mercury

In substitute of Cl₂ in water treatment

Ozone prevent high energy UV

Compound of oxygen :

Oxides (oxide , peroxide and superoxide)

Normal oxide = follow valence rule

High oxide  = oxides with more oxygen

Suboxide = less content of oxygen

Mix-oxide = mix of 2 different of oxides

Hydrides (water)

Colourless liquid , solid and gas

Polar molecule

Neutral oxide but changes to acid or base depends on the compound being reacted

Acts as ligand

Hydrogen peroxide

Book-shaped structure

Colourless liquid due to hydrogen bond

Uses : bleaching agent, antiseptic

Sulfur

Exists as free element

S₈ molecule in crown shape

Odourless, tasteless, light yellow non metallic solid

Not readily wetted or dissolved in water

Reactive element

High degree of solubility and flammable

Uses : produce sulfuric acid, used in vulcanization

Oxide ( SO₂ , SO₃)

SO₂ react with water to form acid solution and react with alkali form sulfite salt

Volcanoes activities

SO₃ prepared by contact process

Forming SO₃ crystal when cooled

Oxaacids (H₂SO₃, H₂SO₄)

The salt of H₂SO₃ is sulfite anion. H₂SO₃ is dibasic acid

The salt of H₂SO₄ is sulfate anion. H₂SO₄ is dibasic acid , strong acid. It viscous liquid due to hydrogen bond.

H₂SO₄ is sulfonation agent

H₂SO₄ uses as fertilizers , to produce HCl

Halides

Exist (F and Cl) , Br only a few and I does not exist

As go down , the halides of sulfur decrease in stability

Thiosulfuric acid

H₂S₂O₃ is not stable

Uses in quantitative analysis in iodometry and photography

# data[].attributes.body
Thank you Dr for today class, this is my summary for Group IVA (halogen)
-Metallic characteristic in INCREASES down the group
-Ionization energy decreases steadily because of shielding effect
GPIVA + GPIA/GPIIA = ionic , others = covalent bonds (to achieve noble gas electronic configuration)
Why Oxygen is different?
-electronegativity very high (hydrogen bond present)
-forming strong ppai-ppai bonds with carbon,nitrogen
Oxygen
2 alltropes -O2 , O3
Preparation
1)Fractional distillation of liquid air – separate O2 (commercial)
2)Heating KCLO3
3) Decomposition H2O2
4) Electrolysis of H2O -graphite electrode
Characteristic
-colourless gass
-blue liquid
-O2 paramanegtic (attracted to magnetic field w 2 unpaired electron)
-Reactive at elevated temperature and combine directly w most element (except noble gas)
Uses
-producing “fuel cell”
-respiration
-welding industries
OZONE (O3)
-blue gasses, dark blue liquid, smell bad, strong oxidation agent
Use in water treatment to kill bacteria (not produce smell, expensive), detergent, deodorizer, preservative , prevent UV ray.
COMPOUNDS
Oxide
-oxide, peroxide, superoxide
-higher bond order, shorten bond length, stronger interaction.
Hydrides of oxygen, H2O
-colourless (all phase) , polar molecules (hydrogen bond exist)
-neutral oxide but change to
Acid (accept H+)/base (donates H+)-> amphoteric character
-act as ligand – form comples
-act as oxidizing agent and reducing agent.
Hydrogen Peroxide, H2O2
-book-shaped structure
-strong oxidizing agent , reducing agent.
-uses as bleaching agent, antiseptic, disinfectiont, mild in toothpaste
SULFUR
-exist as free element.
-allotrope, alpha and beta rombic
-extracted from Frash Process
-not readiy reacted by water
-reactive element
-high degree of solubility
-blue flame
-uses – sulfuric acid, black gunpowder, vulcanization.
Oxide
-SO2
-colourless gas, chocking smell, poisonous gas
-volacnoes activities, combustion of sulfie ores, coal and oil.
SO3
-touch process, heating of ferum (III) sulfate
-react with water form H2SO4
OXOACIDS -h2so3
-sulfurous acid
-ionization – dibasic acid
-sulfite salt is obtained reacting the acid w alkali
-touch process
Halides Sulfur
-F, CL, Br
-decreases stability

# data[].attributes.body
Summary of Group VIA (chalcogens group)

O and S is non-metal, Se and Te is metalloid, Po is metal

O atom

anomalous:
- electronegativity is very high
- form strong ppi - ppi bond with O, C and N

Preparation:
- from fractional distillation of liquid air
- heating of KClO₃
- decomposition of H₂O₂
- electrolysis of H₂O

Compounds: O₃, oxide, H₂O and H₂O₂

- oxidation increases, acidity increases

S atom

- exists as S₈ molecule in the form 0f puckered ring in crown shape
- has 2 forms: alpha-rhombic S and beta-monoclinic S
- yellow solid
- burn in air with blue flame

Compounds: metallic sulfide,  covalent sulfide, CS₂, SO₂, SO₃, sulfur oxoacids, sulfur halides and thiosulfuric acid

# data[].attributes.body
Thank you Dr for today's class. Below is my summary for Group VIA

Characteristics
- Metallic character increases down the group
- IE decreases down the group
- Oxidation state: O= -2 (stable), -1 (peroxo)
- Tupe of compounds formed: ionic (E + Group IA and IIA) and covalent (most of the elements)

OXYGEN
- Exist in atmospheric gaseous (21%)
- Form 2 allotropes: O2 and O3
- Prepared from fractional distillation of liquid air and heating of KClO3
- Colourless gas, paramagnetic with 2 unpaired electrons
- Uses: produce fuel cell and respiration

OZONE
- Formed by photochemical decomposition of NO2
- Characteristics: blue gaseous, smell and strong oxidation agent
- Uses: detergent, deodorizer

OXIDES
- Oxide, peroxide and superoxide

H2O
- Colourless liquid, solid and gas
- Act as oxidizing and reducing agent

H2O2
- Colourless syrup liquid
- Strong oxidizing agent

SULPHUR
-  Odourless, tasteless
- Reactive element
- Flammable and burn in air with blue flame
- Uses: vulcanization of natural rubber
- Ionic sulphide: solid and dark in colour, solid insoluble in H2O
- Covalent sulphide: colourless gas, extremely toxic gas

SO2
- React with H2O to form acid solution
- Reducing agent and oxidizing agent
- Sources: volcanoes activities, combustion of sulfide ores, coal and oil

SO3
- Prepared by Touch process
- Forming SO3 crystal when needed

H2SO3
- Derived of SO2
- Sulfite salt is obtained by reacting acid and alkali

H2SO4
-  Conc. sulphuric acid is viscous liquid
- High bp due to hydrogen bond
- Uses: fertilizers, chemicals for detergent, ether, ester

# data[].attributes.body
Thankyou for the lesson Dr ❤
Summary for group VIA :
-Also known as halcogens group
-The metallic character ⬆ when down the group
-IE ⬇ down the group owing to the  decrease shielding effect
-Oxidation state ,O :(-2)stable, -1(peroxo) & other is between -2 to +6
-2nd highest electronegativity in periodic table

OXYGEN
🐾OXYGEN
-forms 2 allotropes which is oxygen and ozone
-Preparation
1)In commercial-fractional distillation of liquid air to separate O2
2)In laboratory-Heating of KClO3 [catalyst=MnO2],Decomposition of H2O2[catalyst=MnO2],Electrolysis of water uses graphite
-Colourless gas
-Blue liquid
-Paramagnetic with 2 unpaired electron according to MOT

🐾OZONE
-O2(g) + O2(g) ➡ O3(g)
-Photochemical decomposition of NO2
-blue gaseous in colour
-dark blue liquid
-strong oxidation agent
-use mercury,Hg for testing of O3
-use as detergent,deodorizer and etc

Compound of Oxygen:
🐬OXIDES(oxide,peroxide & superoxide)
-Normal oxide follow valence rule
-High oxide is oxide with more oxygen
-Suboxide is less content of oxygen
-Mix-oxide is mix of 2 different of oxides

🐬HYDRIDES ,H2O
-polar molecule
-act as ligand
-act as oxidizing agent and reducing agent
-colourless in all phase

🐬HYDROGEN PEROXIDE
-book-shaped structure
-colourless liquid due to hydrogen bond
-use as bleaching agent,antiseptic

SULFUR
-Exist as free element
-Allotropes :alpha-rhombic S and Beta-monodinic S
-Extracted by Frasch Process
-Properties
>odourless,tasteless,light-yellow non-metallic solid
>reactive element
>high degree of solubility
>flammable and burn in air with blue flame
-Uses
>produce H2SO4
>component of black gun powder
>use in vulcanization of natural rubber
-Chemical properties
>reaction with O2(combustion)
>heating with metal to become metal sulfide
>reaction with conc.acid

Compound of Sulfur:
◀Metallic Sulfides(ionic sulfides)
>all are solid & dark/black in colour except ZnS & PbS (yellow solid)
>react with acid
◀Non-Metallic Sulfide(covalent sulfide)
>colourless gas
>foul smelling like rotten eggs
>extremely toxic gas>act as reducing agent

Compound of Sulfur :
OXIDE
🦋SO2
-sp2
-bend shape
-AX2E
-poisonous gas
-react with water to form acidic solution
-react with alkali forming sulfite salt
-act as reducing and oxidizing agent
🦋SO3
-sp2
-trigonal planar shape
-AX3
-reaction with H2SO4 ➡ oleum
-preparation[ by contact/touch process] & [heating of ferum(III) sulfate]

OXOACID
🦋H2SO3
-dibasic acid
-acid + alkali ➡ sulfite salt
-salt when dissolve in H2O undergo hydrolysis
🦋H2SO4
-dibasic acid,but strong acid because extra H
-high B.P
-In dilute concentration acts as acid
-In conc. & hot act as oxidizing agent
-sulfonation agent
-act as catalyst in esterification and etc
-mostly use in making fertilizers

HALIDE
🦋SX6(sulfur hexhalides)
-sp3d2
-not a lewis base because its donate electron
-not oxidizing agent because F protect the S
-much better insulator than air
🦋H2S2O3(Thiosulfuric acid)
-not stable
-sp3
-use in quantitative analysis in Iodometry
-use in photography

# data[].attributes.body
GROUP VIA
oxygen , sulphur , selenium , tellerium, polonium
Characteristics
-the metallic characteristic increases down the group
-IE decreases down the group

OXYGEN

-Exist in amphoteric gaseous
-Anionic mineral in earth's crust
-Form 2 allotrotypes ; O2,O3
-Preparation ;
1.From fractional distillation of liquid air
2. Heating KClO3
3.Decomposition H2O2
4.Electrolysis of water
Characteristic
-colourless gas
-O2 is paramagnetic
Uses
-producing fuel cell
-respiration
--welding industries
Ozone (O3)
- O + O2 -----> O3
-blue gaseous in color
-dark blue liquid
-strong oxidation agent
Use O3
-substitute Cl2 in water treatment to kill bacteria
-as detergent
Properties of water
- colourless liquid
- form amphoteric character
-act as ligand
Properties H2O2
-colourless syrupy liquid
-Redox reaction
SULPHUR
Properties
- odourless
-tasteless , nonmetallic solid
-Rhombic and monoclinic sulphur are soluble
-high degree solubility
Uses
-produce H2SO4
-Used in valcunation of natural rubber
Compound sulphur
1. Metallic sulphide
-all solid and dark black
-insoluble in water
2. Non-metallic sulfide
-colourless gas
-foul smelling
-toxic gas
SO3
preparation
-touch process
-heatinng ferum (II) sulphate

# data[].attributes.body
Thank you dr for your explanation. Here are my summary

Oxygen
- the electronegativity is very high
- oxygen can form strong p-pi p-pi bonds with itself, carbon and nitrogen
- have two allotropes
*oxygen, O2
*ozone,O3
- can be prepared by fractional distillation of liquid air to separate O2 (commercial)
- heating of KClO3, decomposition of H2O2, electrolysis of water uses graphite as electrodes (laboratory)
- it is a colourless gassand in blue liquid
- it is a paramagnetic with 2 unpaired electron
- can combine directly with most of the elements except for noble gas
USES
- as producing "fuel cell"
- carbohydrate
- in respiration
- in welding industries
OZONE
- prepared by direct reaction of oxygen atom and oxygen gas, photochemical decomposition of NO2 and electrical discharged of O2 and followed by cooling to liquid oxygen and distills.
- it is a blue gaseous in colour, and dark blue in liquid, have smell and strong oxidation agent
- can test the presence of O3 by react Hg and O3 , if bright shining of Hg turn to tarnish, then there is O3
H2O2, hydrogen peroxide
- have open book shaped
- colourless syrup liquid (hydrogen bonding miscible with water, soluble in alcohol)
- thermally unstable and decomposes in the presence of finely divided metal catalyst
- strong oxidizing agent
- a reducing agent
- use as bleaching agent, antiseptic, disinfectant and germicide

Sulfur
- have two allotrope which are a-rhombic S and B-monoclinic S
- sulfur is odourless, tasteless, light-yellow non metallic solid
- not readily wetted or dissolved by water
a reactive element, combines with all element except for inert gases, gold and platinum.
- rhombic and monoclinic sulfur are soluble to a limited extent in most organic solvents
- high degree of solubility
- flammable and burn in air with blue flame
- use to produce sulfuric acid and a component of black gunpowder, vulcanization of natural rubber.

ionic sulfide
- all metallic sulfide are solid and dark black in colour except for ZnS and PbS (yellow colour)
- solid insoluble in water
react with acid H2S gas evolved

sulfur trioxide
- can be prepared by Touch/Contact process, heating of ferum (III) sulfate and dehydration of conc. H2SO4 by solid P2O5
- forming SO3 crystal when cooled
- react with water to form H2SO4
- react with sulfuric acid to produced oleum

H2SO4, sulfuric acid
- derived from SO3 , salt - sulfate ion
- dibasic and strong acid
- conc. sulfuric acid is viscous liquid due to the hydrogen bond between the molecules
- high b.p due to hydrogen bond between the molecules
uses of sulfuric acid
- as fertilizers
- chemicals for detergent, ether and ester
- dehydrating agent
as pigment
to produce conc. HCl

# data[].attributes.body
Thank you for today's lecture, the music video was very interesting XD. Below is my summary of Group IVA;
- Going down, the metallic character increases and the IE & shielding effects decreases.
- Oxidation number; O is -2 (stable) & -1 (peroxo), other elements -2 to +6.
- Type of compound formed: Ionic with Group IA & IIA & Covalent with most of the elements.

1. Oxygen
- Oxygen has very high electronegativity and strong ppi-ppi bonds with itself, carbon, and nitrogen.
- Anionic mineral in the earth's crust.
- Found in water.
- 2 allotropes: oxygen (O2) & ozone (O3)
- Preparation: Commercial (fractional distillation of liquid air) & in Lab (Heating KCLO3, Decomposition of H2O2, & Electrolysis of water using graphite as electrodes).
- Properties: Colorless gas, blue liquid, paramagnetic with 2 unpaired electrons, reactive at elevated temperature, & combine directly with most elements excepts noble gas.
- Uses: Fuel cell, respiration, welding industry.

a) Ozone (O3)
- Preparation: O(g) + O2 -> O3(g), Photochemical decomposition of NO2, & electrical discharge of O2 (industrial).
- Properties: Blue gas, dark blue liquid, smell present, strong oxidation agent.
- Testing of O3 uses mercury.
- Uses: Subtitute of Cl2 in water treatment, detergent, deodorizer, preservative, O3 layer in the atmosphere to prevent entry of high energy UV, & ozone treatment.

b) Oxygen (O2)
- Diamagnetic, 12e-
- Bond order 2, bond length 121pm

c) Peroxide (O2^2-)
- Diamagnetic, 14e-
- Bond order 1.5, bond length 128pm

d) Superoxide (O2^-)
- Paramagnetic, 13e-
- Bond order 1, bond length 148pm

e) Oxide (2O^2-)
- Diamagnetic, 16e-
- No bond order and bond length
- Normal, high, sub, mix-oxide
- Properties: Ionic, covalent, intermediate bonding. Strong acid, neutral, amphoteric, strong base.

f) Water (H2O)
- sp3 hybridization, bend, AX2E2.
- Properties: Colorless gas, liquid, solid, Polar molecule, liquid form more dense, neutral but changes depending on compound being reacted (amphoteric character), act as ligand, act as oxidizing and reducing agent.

g) Hydrogen peroxide (H2O2)
- Open book-like structure.
- Properties: Colorless syrupy liquid, miscible with water & soluble in alcohol, thermally unstable, decomposed if there's finely divided meta; catalyst, strong oxidizing agent, reducing agent.
- Uses: Bleaching agent for wool, hair, teeth, etc, Antiseptic, disinfectant, germicide.

2. Sulfur
- Exist as free element and S8 molecule in a crown-like form.
- Pyrite, Galena, Sphalerite ores.
- 2 allotropes: a-rhombi S & B-monoclinic S.
- Extraction: Mined using the Frasch Process.
- Properties: Odorless, tasteless, light yellow, non-metallic solid, not readily wetter or dissolved in water, reactive if combined with other elements except inert gases, gold, & platinum, flammable in air with blue flame.
- Uses: Sulfuric acid, black gunpowder, vulcanization of natural rubber, blecahing dried fruits and paper products.
- Metallic sulfide: solid, dark/black (except ZnS & PbS=yellow solid), anionic sulfide from highly electropositive metals undergo hydrolysis=basic solution, solid insoluble in water.
- Non-Metallic sulfide:
a) H2S: Colorless gas, foul smell, extremely toxic, dissolve in water=acidic solution, easily oxidized, reducing agent.
b) CS2: Colorless liwuid, foul smell, hydrolysed in water.

a) Oxides of Sulfur
- SIVO2: sp2 hybrid, bend, AX2E, colorless gas, choking smell, poisonous gas.
- SIVO3: sp2 hybrid, trigonal planar, AX3, colorless gas, dissolve in water=sulfuric acid, reaction with sulfuric acid=oleum.
- Properties of SO2: +water=acidic solution, +alkali=sulfite salt, reduing agent, oxidizing agent.
- Source of SO2: Volcano activities, Combustion of sulfide ores, coal, oil, Roasting anhydride CaSO4 with coke, Sulfite salt with acid, Metal with conc. sulfuric acid.
- Preparation of SO3: Contact/Touch Process, Heating of ferum(III) sulfate, Dehydration of conc. H2SO4 by solid P2O5.
- Properties of SO3: crystal when cooled, a-SO3, B-SO3, y-SO3, +water=H2SO4, +sulfuric acid=oleum.

b) Oxoacids of Sulfur
- Oxoacid H2SO3: Sulfurous acid, SO2 + H2O -> H2SO3
- Properties of H2SO3: dibasic acid.
- Oxoacid H2SO4: Sulfuric acid, SO3 + H2O -> H2SO4
- Properties of H2SO4: dibasic acid, strong acid, conc. H2SO4 is viscous liquid, high b.p. acid in dilute concentration, oxidizing agent in conc. & hot, sulfonation agent, catalyst.
- Sulfate salts are obtained by reacting H2SO4 with alkali, metal, & carbonate/bicarbonate.
- Uses of H2SO4: Fertilizers, chemical detergent, ether, ester, dehydrating agent, pigment, production of conc. HCl.
- Industrial manufacture of H2SO4 by Contact/Touch Process.

c)Halides of Sulfur
- Sulfur halides: F & Cl exists, Br a few, I does not exist.
- Disulfur dihalide (S2X2): F2-gas, Cl2-yellow liquid, Br2-unstable liquid structure.
- sp3 hybrid, hydrolysis in water, +Cl2=SCl2, +ethylene C2H4=mustard gas.
- Sulfur tetrahalide, SX4: Distorted trigonal bipyramidal, preparation by +Cl2 or +F2 in inert atmosphere, hydrolysis in water & alkali, able to expand the octet.
- Sulfur hexahalide, SX6: sp3d2 hybrid, reacts readily w halogen except Iodine, SF6 is colorless, tasteless, non-toxic, thermally stable, insoluble in water.
- Thiosulfuric acid (H2S2O3) is not stable.
- Uses: Quantitative analysis in iodometry (titration method using starch as indicator) & in photography.

# data[].attributes.body
Thank you Dr for the explaination for this subtopic.Here is my summary.
Characteristics Group VIA
-metallic character decrease down the group due to the electrical properties of elements
-Ionization energy decrease down the group due to the decreasing of shielding effects
-Ionic to group IA and IIA and covalent to most of the element(M²- ions, two covalent bond for water and (CH3)S, MR- ions, onium salts, hypervalents
Unique of Oxygen than others
-higher electronegativity
-forming strong pπ-pπ bonds with itself, C and N
OXYGEN
-Anionic mineral in earth crust(carbonate,nitrate,sulfate,oxides)
In water
Form allotropes: oxygen and ozone
Preparation of oxygen
Comercial:Fractional distillation of liquid air to separate oxygen
In Laboratory:Heating of KClO3 solid
Decomposition of H2O2
Electrolysis of water
Characteristic: Colorless gas, blue liquid
-oxygen is paramagnetic with 2 unpaired electrons(according MOT)
Uses : -producing fuel cell
- respiration
OZONE
FORMATION :-O (g) + O2 → O3 (g)
-Photochemical
decomposition of NO2
- Industrial production of O3
CHARACTERISTICS:
-gas :blue, liquid: dark blue
-Strong oxidation agent
USES :-Deodorize air, purify water, and treat
industrial wastes
-ozone treatment
-ozone layer prevent UV from reach
the earth
OZONE TEST :
-Use Mercury,Hg . The bright shining Mercury will become tarnish and starting to stick to the surface of glass due to presence of ozone
OXIDE (normal oxide, high oxide, suboxide and mid-oxide)
ACID BASE OXIDE :
-metal and non-metal
-oxidation state which is acidity increase when oxidation increase, e.g : N2O (N=+1) is neutral, N2O5 (N=+5) is strong acid
HYDRIDES OF OXYGEN :
- WATER, H2O  (bent shape with hybridization sp3)

-PROPERTIES :
i) polar molecule

ii) neutral oxide but change to acid/alkali (develope  amphoteric character)

iii)act as ligand

iv) act as reducing agent and oxidizing agent

-HYDROGEN PEROXIDE ,H2O2  (has book shape structure)
-PROPERTIES :
i) colourless syrupy liquid due to hydrogen bonding and soluble in alcohol
ii)thermally unstable and decompose when finely divided metal cattalyst present
iii)strong oxidizing agent and also a reducing agent

-USES :
i) as bleaching agent for wool, hair and teeth
ii) as antiseptic, disinfectant and germicide.
SULFUR(exist as free element
-Ores :phyrite, galena and sphalarite
-Exist as S8 molecule(crown shape)
-Allotrope of sulfur : alpha-rhombic S and gamma-monoclinic S
Extraction of Sulfur:
-Frasch Process due to low m.p. & low density
-Superheated water (115°C) pumped down outer-most 3 concentric pipe
-Compress air pump down the inner pipe
-Mixture of hot water, molten sulfur & air comes up the middle
-Sulfur obtaines has 99.5% purity
-Properties:
-odorless, tasteless and reactive element combine with all except inert gases, gold and platinum
-not readily wetted or dissolve in water
-used to produce H2SO4
-High degree of solubility
&
-Flammable and burn in air with blue flame

Uses:
-Component of black gunpowder
-use in vulcanization of natural rubber,as a fungicide & fumigant
-Use as bleaching agent for dried fruit and for paper product
-Chemical property:
-Reaction with O2(combustion)
-Heating with metal become metal sulfide
-reaction with conc. acid
-Metallic sulfide (ionic sulfide)
-All metallic sulfides are solid and dark color(Except Zn & Pb (yellow)
-Anionic sulfide from highly electropositive metals undergo hydrolysis; resulting basic solution
-Solid insoluble in water
-react with acid; H2S gas evolves
NON-METALLIC SULFIDE (COVALENT SULFIDE)
-Hydrogen Sulfide (sp3)
has foul smell and extremely toxic
Dissolved in water form acidic solution
easily to oxidize, act as reducing agent
Carbon Disulfide (sp)
Solvent for S, P, I2, rubber and wax
Hydrolyze in water
OXIDE ( SO2 and SO3)
-SO2 (S=+4)
hybridization= sp2 with bend shape
Colorless gas with choking smell
Poisonous gas
-PROPERTIES :
i) react with water to form acidic solution (phenomeon acidic rain)
ii) react with alkali form sulfite salt (SO32-)
iii) act as reducing agent and oxidizing agent
-SOURCES OF SO2 (air pollution) :
i) Volcanoes activities (emission of SO2 from the higher temperature of the molten earth)
ii) Combustion of sulfide ores, coal and oil
iii) Roasting anhydride calcium sulfate, CaSO4 with coke
iv) Reaction of sulfide salt with acid
v) Reaction of metal with concentrated H2SO4
-SO3 (S=+6)
Hybridization=sp2 with trigonal planar shape
Usage : dissolve in water form sulfuric acid, H2SO4
React with sulfuric acid form oleum, H2S2O7
PREPARATION :
i) Contact Process, SO2 + O2 🡪 SO3
ii) Heating of Fe2(SO4)3
iii) Dehydration of concentrated H2SO4 by solid P2O3
PROPERTIES :
i) Form SO3 crystal when cooled to 195K
Alpha-SO3, cyclic trimetric form
Beta-SO3, cube, transparent crystal , cross-linked of SO4 into layers
Gamma-SO3, needle-like crystal with infinite helical chains of SO4
ii) Reaction SO3 with water form H2SO4
iii) Reaction SO3 with H2SO4 form oleum, H2S2O7
OXOACID (SULFUROUS ACID, H2SO3)
SO2(g) + H2O(l) -->H2SO3(aq)
sulfite anion, SO32-
-Properties :
i)dibasic acid
ii)sulfite salt obtained by reacting acid with alkali
iii)salt dissolve in water umdergo hydrolysis
H2SO4
-Properties:
i)concentrated acid is dehydrating agent
ii)diluted concentration act as acid
iii)concentrated and acid H2SO4 as oxidizing agent
H2SO4 can sulfate salt form by react with alkali, oxide, metal and carbonate or bicarbonate
-Uses:
i)chemicals for detergent, ether and ester
ii)pigment TiO2, TiOSO4 as white glow pigment in paint
INDUSTRIAL MANUFACTURE OF H2SO4
Touch/Contact Process
i)combustion of S
ii)oxidation of SO2
iii)SO3 transformation to H2SO4
-dissolution of SO3 into oleum
-addition of a certain amount of water to oleum to form H2SO4
HALIDES
-Disulfur dihalide(S2X2) can undergo hydrolysis in water, S2Cl2 react with excess Cl2 form SCl2 and S2Cl2 react with ethane give mustard gas which used as war weapon but banned due to its hazardous
-Sulfur Tetrahalides
SCl4 can be prepared react S with Cl2
and SF4 can be prepare by react S with Cl2 with -73°C and in inert atmosphere
Reaction : i)hydrolysis in water and alkali
ii)able to expand to the octet(SF6)
-Sulfur Hexahalides
can synthesis with S directly with all halides except I to form SX6
Properties :
i)colorless, odorless, tasteless, non-toxic, thermally stable and insoluble im water
H2SO3 AND (S2O3)2-
-can be used as quantitative analysis in iodometry and in photography

# data[].attributes.body
GROUP VIA (CHALCOGENS)

metallic character increases

ionization engergy decreases

form ionic compound with Group IA & IIA and covalent with others

why oxygen different ?
- electronegativity high (form ionic character and hydrogen bond

- forming p(pi)-p(pi) bonds with itself, C & N

OXYGEN(O2)

# fractional  distillation of liquid air to separate O2
# heaating KClO3
# decomposition H2O2
# electrolysis H2O

colouless gas

blue liquid

paramagnetic

reactive at high temp

uses

produce "fuel cell"

welding industries

respiration

OZONE(O3)

# directly from O & O2
# photochemical decomposition NO2
# electrical charged of O2 gaseous

blue gasesous

dark blue liquid

smell

strong oxidation agent

uses

substitute Cl2 in water treatment to kill bacteria

atmosphere

detergent

Testing O3 : use mercury, Hg
> bright shining mercury becime tarnish & Hg stic at glass surface

compounds of oxygen

Oxide

(oxide, peroxide, superoxide)

Hydrides (H2O)

Hydrogen Peroxide (H2O2)

SULPHUR

free element  (brimestone)

ores : pyrite(FeS), galena(PbS), sphalerite(ZnS)

S8 molecules (crown shape)

form S8 ring (alpha-rhombic S & beta-monoclinic S)

extraction

Frasch Process (low melting point &  density)

properties

odourless, tasteless, logh yellow non-metallic

not readily wetted, not dissolved in water

flammable & burn in air with blue flame

chemical properties

reaction with oxygen (combustion)

heating with metal

reaction with conc. acid

uses

produce H2SO4

vulcanization of rubber

component of black gunpowder

bleaching dried fruit/paper product

METALLIC SULFIDE (IONIC)

all solid & dark/black colour except ZnS & PbS (yellow solid)

anionic sulfide from highly electropositive metals undergo hydrolysis > basic soln.

soluble in water

react with acid > H2S gas envolve

NON-METALLIC SULFIDE (COVALENT)

hydrogen sulfide, H2S

carbon disulfide, CS2

compounds of sulfur

Oxide

- SO2
chemical properties

1.  react with water > acid soln.

2.  react with alkali > sulfide salt

3.  reducing & oxidizing agent

sources
# volcanoes activities
# combustion anhydride CaSO4 with coke
# reaction with sulfide salt with acid
# reaction of metal with conce. H2SO4
# combustion sulfide ores, coal, oil

- SO3
# Touch Process
# heating ferum (III) sulfate
# dehyfration conc. H2SO4
properties
form SO3 when cooled
(alpha-SO3, beta-SO3 & gamma-SO3)

Oxoacid

- H2SO3
- H2SO4
industrial manufacture H2SO4 (contact/touch process)

1. combustion of S > SO2

2.  oxidation SO2 > SO3

3. SO3 transformation to H2SO4

- dissolution SO3 into conc. H2SO4 > oleum
- addition of H2O to oleum > H2SO4

Halides

- sulfur tetrahalide, SX4

- sulfur hexahalide, SX6

thiosulfuric acid (H2S2O3) and
salts (S2O3 ²⁻)
- H2S2O3 nit stable
- important salt : Na2S2O3.5H2O

thankyou dr for today lesson :)

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The Calcogens Group

Characteristics

·         The metallic character increase down the group

·         IE decrease down the group

·         Attain a noble gas electronic configuration

How Oxygen differ from other member

·         Electronegativity is very high

·         Differ in forming p-pi p-pi bond

OXYGEN

·         Exist in atmospheric gaseous

·         Anionic mineral in earth crust

Preparation in commercial:

-from fractional distillation of liquid air to separate o2

Preparation in laboratory

-heating of KCIO3 (g)

-decomposition of H2O2

-electrolysis of water uses graphite as electrodes

Characteristic

-colourless gas

-blue liquid in liquid form

Paramagnetic with 2 unpaired electron

Uses

-producing ‘fuel cell’

-respiration

-welding industries

OZONE

Formation

-O +O2 ----> O3

-photochemical decomposition of NO2

-Industrial production of O3 involved electrical discharge of O2 gaseous

Uses

-to kill bacteria

-as detergent

COMPOUND OF OXYGEN

OXIDE

-normal oxide

-High oxide

-Suboxide

-mix oxide

Properties

-nature of bonding

(ionic, covalent, intermediate, strong acidic)

-acid-base

(strong acidic, neutral, amphoteric, strong base)

HYDRIDES

Properties of water

-colorless liquis, solid and gas

-density of solid<liquid

-act as ligand

-act as oxidizing and reducing agent

Properties of H2O2

-colourless syrupy liquid due to hydrogen bonding

-the molecule thermally stable

-strong oxidizing agent

-Also act as reducing agent

SULFUR

·         Exist as free element

Properties of sulphur

-a high degree of solubility

Sulphur is flammable and burn in air with blue flame

Uses

-used in vulcanization of natural rubber

-used in the bleaching of dried fruits and for paper product

Chemical properties

-reaction with o2- combustion

-heating with metal

-reaction with conc. Acid

Compound of sulphur

1.       Metallic sulphide

2.       2. Non-metallic sulphide

COMPOUNDS OF SULPHUR

OXIDES OF SULPHUR

-O2, O3

Chemical properties

-react with water to form acid solution

-react with alkali forming sulphite salt

-act as reducing agent

- act as oxidizing agent

OXOACIDS OF SULPHUR

Properties H2SO3

-sulfurous acid is dibasic acid

-the sulphite salt is obtained by reacting the acid with alkali

Properties H2SO4

-dibasic acid, strong acid

-conc. Sulphuric acid is viscous liquid due to the hydrogen bond between the molecule

-high b.p due to hydrogen bond between molecules

Uses

-act as fertilizers

-chemicals for detergent , ether, ester

-dehydrating agent

To produce concentrated HCL

Industrial manufacturer of H2SO4

-by CONTACT/TOUCH PROCESS

1. combustion of Sà SO2

2. oxidation os SO2à SO3

3. SO3 tranformation to H2SO4

HALIDES OF SULPHUR

·         Structure: distorted trigonal bipyramidal

Uses

-quantitative analysis in iodometry

-used in photography

question:
1. dr, can i have again a short explanation about quantitative analysis in iodometry? what to prove from the experiment?

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Summary for Group VIA
- metallic character increase down the group
- IE decrease down the group

OXYGEN
- form 2 allotropes
i) O2
ii) O3

i) O2
- colourless gas
- oxygen is paramagnetic with 2 unpaired electrons
-uses :
~ producing " fuel cell"
~ respiration
~ welding industries

ii) O3
- blue gaseous in colour
- dark blue liquid
- strong oxidation agent
- formation of ozone :
~ O react with O2
~ photochemical decomposition of NO2
~ industrial production of O3 involved electrical discharged of O2 gaseous followed by cooling to liquid oxygen and distills.
- uses :
~ as detergent, deodorizer and preservative
~ ozone layer prevent high energy uv from reaching the earth

- compound of oxygen
i) oxide ( diamagnetic)
ii) peroxide (diamagnetic)
iii) superoxide (paramagnetic)

- properties of water :
- colourless liquid, solid and gas
- neutral oxide but changes to acid or base depending on the compound being reacted (amphoteric character)
- act as ligand
- act as oxidizing agent and reducing agent

- properties of H2O2 :
- colourless syrupy liquid due to hydrogen bonding, miscrible with water, soluble in alcohol
- the molecule is thermally unstable and decomposes in the presence of finely divided metal catalyst
- strong oxidizing agent
- reducing agent

uses :
- as bleaching agent for wool, hair, teeth
- as antiseptic, disinfectant and germicide

SULFUR
- exist as free element, brimstone
- S8 molecule in the form of a puckered ring in crown shape
- allotrope of sulfur:
~ a-rhombic S
~B-monoclinic S

extraction of sulfur
- Frasch Process
- superheated water is pumped down the outermost of three concentric pipes
- compressed air is pumped down the innermost pipe
- a mixture of hot water, molten sulfur and air comes up the middle pipe
- sulfur obtained has 99.5% purity.

properties of sulfur
- odourless, tasteless, light yellow non-metallic solid
- not readily wetted or dissolved by
- reactive element
- high degree of solubility
- flammable and burn in air with blue flame

uses:
- used to produced sulfuric acid
- vulcanization of natural rubber
- bleaching dried fruits and paper product

chemical properties of SO2:
- react with water to form acid solution
- react with alkali
- reducing agent
- oxidizing agent

preparation of SO3:
- contact process by heating of ferum(III) sulfate
- dehydration of concentrated h2so4 by solid p2o5

uses of sulfuric acid:
- fertilizer
- chemical for detergent, ether,ester
- dehydrating agent
- pigment
- to produce concentrated hcl

# data[].attributes.body
Thankyou Dr for today’s lesson and pre-recorded class. Summary for group VIA:

-Down the group, metallic character increases while IE decreases down the group- shielding effects decreases along Se, Te and Po

-Oxidation state: (-2 stable, -1 peroxo) (other elements: -2 to +6)

-Oxygen is different from others due to

- electronegativity is very high -form ionic and hydrogen bonding

- strong p-pi—p-pi bonds

Oxygen

- Form 2 allotropes (O2; oxygen & O3; ozone)

- Preparation – fractional distillation of liquid air (commercial)

- O2 paramagnetic with 2 unpaired electron

- Reactive (high temp) & combine directly with most of elements except noble gas

- Uses- producing “fuel cell”, respiration & welding industries

- Ozone (O3) -strong oxidation agent & testing for O3 by using Hg

- Uses - water treatment, detergent, deodorizer, prevent high energy UV from reaching earth

- Oxide - (oxide - paramagnetic, peroxide -diamagnetic & superoxide -paramagnetic) & (normal oxide, high oxide, suboxide & mix oxide) & Acid-base oxide (oxidation increases, acidity increases)

- H2O (can accept or donates H+) & H2O2 (easily decomposed)-bleaching agent, antiseptic & mild oxidant in toothpaste

Sulfur

- Ores- pyrite, galena & sphalerite

- Allotrope- alpha-rhombic S & beta-monoclinic S

- Extraction- Frasch process – obtained 99.5% purity of S

- Reactive element & combine all other elements except inert gases, gold & platinum

- High degree of solubility

- All metallic sulfides are solid and dark/black except ZnS & PbS (yellow)

- Non-metallic sulfides: H2S – extremely toxic gas and easily oxidized & CS2 – solvent for S, P, I2, rubber, wax

- Oxide: SO2- react with water to form acid solution & SO3 – Contact/Touch process & forming alpha-SO3, beta-SO3 & gamma-SO3

- Oxoacid- H2SO3 (derived from SO2) & H2SO4 (derived from SO3) – dibasic acid & strong acid

- Industrial manufacture of H2SO4 – contact/touch process

- Halide- exist for F & Cl, only a few for Br & does not exist for I

- Thiosulfuric acid – not stable & important salt (S2O32-) & Uses – analysis in Iodometry & in photography

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Group VIA
- metallic increases down the group
- IE increases down the group (decreased shielding effects)
- -2 to +6 except O
- forms both ionic and covalent
- O is different
high electronegativity

forms pπ - pπ bonds with itself, C, N

OXYGEN
- 2 allotropes: O₂ & O₃
- prep. ind.: fractional distillation
prep. lab: heating KClO₃, decomposition of H₂O₂, electrolysis of water
- char.: colourless gas, blue liquid, O₂ paramagnetic
- uses: producing fuel cell, respiration, welding industries
O ₃
- resonance structure
- formation: O + O₂ -> O₃, photochemical decomposition of NO₂
- char.: blue gaseous, dark blue liquid, smell, strong oxidation agent
- testing for O₃ use Hg
- uses: water treatment, detergent, deodorizer, preservative, prevent high energy UV from penetrating
Oxides
- Normal, high, sub, mix
- prop.: ionic/covalent/intermediate, strong acidic/neutral/amphoteric/strong base
Hydrides
H ₂ O
- prop.: colorless in all states, polar, density solid < liquid, neutral oxide with amphoteric character, ligand, oxidation & reduction agent
H ₂ O ₂
- book-shaped
- colorless syrupy liquid (H-bonding), thermally unstable, strong oxidizing agent, reducing agent
- uses: bleaching agent, antiseptic, disinfectant, germicide

Sulphur
- exists as free element (brimstone), S₈ molecule
- allotrope (S8 arranged differently): α-rhombic S &
β-monoclinic S
- extraction: Frasch Process (99.5% purity)
- prop.: odourless, tasteless, light yellow, not readily dissolved by water, reactive except with inert gases, gold & platinum, rhombic & monoclinic soluble in select organic solvents, flammable with blue flame
- uses: prod. H₂SO₄, black gunpowder, vulcanization of natural rubber, fungicide, fumigant, bleaching of dried fruits
- chem. prop.: react with O₂, metal & conc. acid
Ionic sulfide
- solid, dark colour except with Zn & Pb, solid insoluble, react with acid evolves H₂S gas
Covalent sulfide
- H2S: colorless, foul smell, toxic, soluble in water, easily oxidized, reducing agent
- CS2: colourless liquid, foul smell, solvent, hydrolize in water
Oxides
SO ₂
- sp², bend, colourless gas, choking smell, poisonous
- reacts with water & alkali, reducing & oxidizing agent
- sources: volcanic activity, combustion of sulfide ores, roasting anhydride CaSO4, react sulfite salt & acid, metal & conc. sulfuric acid
SO ₃
- sp², trigonal planar, colourless gas, soluble in water, produces oleum when react with H₂SO₄
- prep.: Contact process, heating Fe₂(SO₄)₃, dehydration of conc. H₂SO₄ by solid P₂O₅
- prop.: forms crystals when cooled (α, β, γ)
Oxoacids
H ₂ SO ₃
- dibasic acid, react with alkali to get sulfite salt, salt dissolves in water
H ₂ SO ₄
- strong dibasic acid, viscous liquid & high BP (H-bond), dehydrating agent (conc.), oxidizing agent (hot & conc.), sulfonation agent
- uses: fertilizers, detergent, ether, ester, dehydrating agent, pigment, prod. conc. HCl
- Contact Process: Combustion of S, Oxidation of SO₂, SO₃ to H₂SO₄
Halides
- exists for F, Cl and a few for Br
S ₂ X 2
- exists for all but becomes increasingly unstable
- hydrolize in water, S2Cl2 react further to get SCl2
SX ₄
- distorted trigonal bipyramid
- prep.: direct reaction for Cl, direct reaction under inert atmosphere and -73°C for F
- hydrolize, able to expand octet
SX ₆
- prep.: reacts readily except I
- prop.: colorless, odorless, tasteless, non-toxic, thermally stable & insoluble in water
- not a Lewis base (no available non-bonding lone pair electron)
- not oxidizing agent (F aroms protect S)
- better insulator than air
H ₂ S ₂ O ₃
- not stable
- important salt : Na₂S₂O₃.5H₂O
- uses: quantitative analysis in iodometry

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Group VIA summary
-metallic character increase down the group
-IE decrease down the group

Oxygen
-preparation
i)commercial- fractional distillation of liquid air to separate O2 from N2 and Ar
ii) lab-heating KClO3, decomposition of H2O2 and electrolysis of water using graphite electrodes
character -colourless gas, blue liquid
uses- producing fuel cell, respiration ,welding industries

Ozone
Formation
1)photochemical decomposition of NO2
2)industrial-involve electrical discharged of O2 followed by cooling liquid O2 and distills

character-blue gaseous, dark blue liquid

uses- substitute Cl2 in water treatment, detergent, atmosphere

Oxides
normal oxide
Peroxide
Superoxide

Hydride
1)H2O
2)H2O2

Sulphur
allotropes
-alpha rhombic
-beta monoclinic
Extract- Frasch Process

Properties
-odourless, tasteless, light yellow solid
-not readily wetted or dissolve in water
Compound
1)metallic sulphide
-dark black colour except ZnS & PbS
-anionic sulphide
solid insoluble n water
2)Non-metallic silphide
H2S-hydrogen Sulphide
-colourless, foul smell, extreme toxic

CS2- Carbon Disulphide
- colourless liquid
-foul smell
-solvent for S, P, I2, rubber and wax

Oxide
SO2
properties
-react with H2O -> H2SO4
Alkali -> sulfite salt
-  reducing agent
-oxidizing agent

source- volcanoes activity, combustion of sulphide ores, roasting anhydride  CaSO4 with coke

SO3
preparation- Contact/Touch Process

properties -SO3 crystal when cooled to  -195 K

Oxoacid
H2SO3 (sulphurous acid)
H2SO4 (sulphuric acid)
-properties- dibasic acid
- sulphonation agent
-as catalyst
-Uses- fertilizer
- dehydrating agent
- detergent
Halide
Disulphur dihalide , S2X2
S2F2-gas
S2Cl2- yellow liquid
S2Br2- unstable

Sulphur tetrahalide SX4
Sulphur Hexahalide SX6

Thiosulphuric Acid (H2S2O3)
used in Iodometry and photography

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Thank you dr for today's class and the other pre-recorded videos :))

Here summary for Group VIA
Down the group:
- metallic character increases
- IE decreases
Compounds form:
- ionic (Group IA & IIA)
- covalent (most elements)
Why oxygen different than others?
1) very high electronegativity
2) forming strong ppi-ppi bonds with O, C, N

Oxygen, O2

- exist in the atmospheric gaseous
- anionic mineral in earth crust
- form 2 allotropes (O2 & O3)
Preparation:
Commercial:
1) From fractional distillation of liquid air - separate O2
Laboratory:
1) Heating KClO3
2) decomposition H2O2
3) Electrolysis of water use graphite as electrode
Characteristics:
- colourless gas
- liquid form (blue liquid)
- paramagnetic with 2 unpaired e-
- reactive at elevated temperature and combine directly with most elemnts (except noble gas)
Uses:
- producing fuel cell
- respiration
- welding industries
Ozone, O3
Formation
1) O + O2 ---> O3
2) Photochemical decomposition of NO2
3) Industrial - electrical discharged of O2 gaseous
Characteristics
- blue gaseous
- dark blue liquid
- smell
- strong oxidizing agent
Uses:
- in susbtitute of Cl2 in water treatment - kill bacteria
- as detergent, deodorizer, preservative
- in atmosphere: prevent high energy UV from reach earth

Oxides
1) Oxide (O2-) - paramagnetic
2) Peroxide ((O2)2-) - diamagnetic
3) Superoxide ((O2)-) - paramagnetic
Properties:
1) Natural of bonding
2) acid-base
Acid-base:
Oxidation increase, acidity increase

Hydrides
H2O - water
Properties:
- colourless liquid, gas, solid
- polar molecule --> solvent for most ionic
- density solid < liquid
- neutral oxide -> change to acid/base depend on compound reacted (Amphoteric)
- act as ligand
- oxidizing and reducing agent

H2O2 - hydrogen peroxide
- open book structure
Properties:
- colourless syrupy liquid -> HB
- thermally unstable and decompose in presence of finely divided metal catalyst
-strong oxidizing agent
- reducing agent
Uses:
- bleaching agent
- antiseptic, disinfectant and germicide
- MgO2 & CaO2 as mild oxidant in toothpaste

Sulfur

- exists as free element, S
- ores : pyrite, galena, sphalerite
- S8 molecule ( puckered ring form)
- Allotropes: alpha-rhombic S and beta-monoclinic S

Extraction:
- By Frasch Process : due to low melting point & low density

Properties:
- odourless, tasteless, light yellow non-metallic solid
- not readily wetted or dissolved by water
- reactive element, combine with all other element (except inert gas, gold, platinum)
- rhombic & monoclinic sulfur are soluble in organic solvents
- high degree of solubility in CS2 -> dissolve rhombic sulfur
- flammable & burn in air with blue flame

Uses:
- to produced sulfuric acid, H2SO4
- component of black gunpowder
- used in vulcanization of natural rubber
- used in bleaching of dried fruits and paper products

Chemical prop:
- Reaction with O2 (combustion)
- Heating with metal -> metal sulfides
- Reaction with conc. acid

Compounds:
1) Metallic sulfides (ionic)
- Solid and dark/black excp ZnS & PbS -> yellow
- Anionic sulfide from highly electropositive metals undergo hydrolysis -> basic solution
- Solid insoluble in water
- React with acid --> H2S gas evolves
2) Non-metallic sulfide (covalent)
Hydrogen sulfide, H2S
- colourless gas
- foul smelling
- extrmely toxic gas
- dissolve in water --> acidic solution
- easily oxidized
- reducing agent
Carbon disulfides, CS2
- colourless liquid, fouling smell
- solvent S, P, I2, rubber, wax
- hydrolyze in water

Oxides
SO2
- hybridization: sp2
- geometry: bend
- type: AX2E
- colourless gas
- chocking smell
- poisonous gas
SO3
- hybridization: sp2
- geometry: trigonal planar
- colourless gas
- dissolves in water --> sulfuric acid
- react with sulfuric acid --> oleum

SO2

Chemical prop:
- React with water --> acidic solution (acid rain)
- React with alkali --> sulfite salt ((SO3)2-)
- Reducing agent
- Oxidizing agent
Sources:
- volcanoes activities
- combustion of sulfide ores, coal, oil
- roasting anhydride CaSO4 with coke
- reaction of sulfite salt with acid
- reaction of metal with conc. sulfuric acid

SO3

Preparation:
1) Contact/Touch Process
2) Heating of ferum(III) sulfate
3) dehydration of conc. H2SO4 by solid P2O5
Properties:
1) Forming SO3 crstal when cooled
- alpha-SO3 : crystal trimetric form
- beta-SO3 : cube, transpareny crystal, meta stable
- gamma-SO3 : needle-like, most stable
2) Reaction with water
3) Reaction with sulfuric acid --> produced oleum

Oxoacid
H2SO3 (Sulfurous acid)
- Derived from SO2
- Salt : sulfite anion (SO3)2-
Properties:
1) Ionization
2) Sulfite salt obtained by react acid with alkali
- dissollves in water undergo hydrolysis
H2SO4 (Sulfuric acid)
- Derived from SO3
- Salt : sulfate anion (SO4)2-
Properties:
- dibasic acid, strong acid
- viscous liquid -> HB between molecule
- high bp -> HB
- conc. acid: Dehydrating agent
- dilute concentration: acid
- conc. and hot: oxidizing agent
- sulfonation agent
- as catalyst - H2SO4 absorb water

H2SO4 (Sulfate salt)
- obtained by react H2So4 with
: alkali
: metal oxide
: metal
: carbonate/bicarbonate
Uses sulfuric acid
- fertilizers
- Chemical for detergent, ether, ester
- Dehydrating agent -> remove water from gas, liquid, solid
- pigment -> TiO2, TiOSO4: white glow pigment in paint
- prodece conc. HCl
Industrial of sulfuric acid
Contact Process
1) Combustion S --> SO2
2) Oxidation SO2 --> SO3
3) SO3 transformation to H2SO4
- Dissolution of SO3 into H2SO4 --> oleum
- Addition of water to H2S2O7 --> H2SO4

Halides
- exists for:
: X = F & Cl
: X = Br - only a few
: X = I - not exist
- disulfur dihalide, S2X2
S2F2 - gas
S2Cl2 - yellow liquid
S2Br2 - unstable liquid
( decrease in stability )
- hydrolysis in water
- S2Cl2 react further with Cl2 --> SCl2
- SCl2 reacts with ethene give mustard gas

Sulfur tetrahalide, SX4
Structure: Trigonal bipyramidal
Reactions:
- Hydrlysis in water and alkali
- Able to expend the octet

Sulfur hexahalides, SX6
Synthesis:
- S react directly with all halogen exp iodine
Properties;
- colourless, odorless, tastesless, non-toxic, thermally stable, insoluble in water
- Not Lewis base, no available non-bonding
- Despite +6 it is not oxidizing agent - F atoms protect S
- Much better insulator than air

Thiosulfuric acid (H2S2O3) & salts (S2O3 2-)
- H2S2O3 not stable
- Important salt --> Na2S2O3.5H2O
Uses:
- Quantitative analysis in Iodometry: titration method, use starch as indicator (blue --> decolorize)
- In photography
: S2O3 2- , to remove silver(I) salt that not reduce by Ag

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SUMMARY GROUP VIA

- characteristic

- metallic characteristic increase

- IE decreased due to increasing shielding effect

- oxidation state = O(-2,-1), others (-2 to +6)

- types of compound form

- ionic = E + group IA, IIA

- covalent = with most of the element

- attain a noble gas electronic structure include the formation of

-M²⁻ ion

-2 covalent bond

- MR- ion

- onium salt

- hypervalents

Why oxygen is different ?

- electronegativity is very high

- can form strong p(pi)-p(pi) bond with itself, N or C

OXYGEN

- exist in the atmospheric gaseous (21% O₂)

- anionic mineral in the earth crust

- carbonate, nitrate, sulphate, oxides

-exist in water

- as allotrope (O₂ , O₃)

Preparation

- fraction distillation of liquid air

- reaction of KClO₃

- decomposition of H₂O

- electrolysis of water (C as electrode)

Characteristic

- colourless gas, blue liquid

- paramagnetic with 2 unpaired electron

- reactive at elevated temperature and combine directly with

most element except noble gas

Uses

- production of fuel cell

- respiration

- welding industries

Ozone (O₃)

Formation

- O + O₂ --> O₃

- photochemical decomposition of NO₂

- electrical discharged of oxygen gaseous followed by cooling to

Liquid oxygen and distilled

Characteristic

- blue gaseous, dark blue liquid, smell, strong oxidizing agent

Testing O₃

- use mercury (bright shining mercury becomes tarnish and stick

To the surface of glass )

Uses

- substitute Cl₂ in water treatment to kill bacteria

- as detergent, deodorizer, preservative

- prevent UV ray from reaching earth

COMPOUNDS
Oxides

- oxide, peroxide, superoxide

- normal oxide

- follow valence rule (MgO, Na₂O)

- high oxide

- more than actual according to valence rule (Mn₂O, PbO₂)

- suboxide

- less content of oxygen according to valence rule

- mix-oxide

- known as spinel compound Pb₃O₄ (2PbO.PbO₂)

- acid-base oxide

- metal and non-metal

- oxidation state = oxidation increase , acidity increase

Hydrides (H₂O)

Characteristic

- colourless liquid, solid gas

- polar molecule

- density solid < water

- neutral oxide but changes to acid or base depend on the compound being reacted

- act as a ligand

- as oxidizing and reducing agent

Hydrogen Peroxide (H₂O₂)

Book-shaped structure

Characteristic

- colourless syrupy liquid, miscible with water, soluble in alcohol

- thermally unstable and decomposes in the presence of finely divided metal catalyst

- strong oxidizing and reducing agent

Uses

- bleaching agent

- antiseptic, disinfectant, germicide

- MgO₂ and CaO₂ as mild oxidant in toothpaste

SULFUR

- exist as free element, brimstone which are formed by bacterial action on volcanic gas

- ores (pyrite, galena, sphalerite)

- Allotrope

- alpha-rhombic S

- beta-moniclinic S

Extraction

Mined by Frasch process

- superheated water pumped down the outer-most of 3 pipes

- compressed air pumped down to inner-most pipe

Properties

- odourless, tasteless, light-yellow non metallic solid

- not readily wetted or dissolved in water

- rhombic and monoclinic sulfur are soluble to a limited extent in most organic solvent

- high degree solubility is attained in carbon disulfide

- flammable and burn in air with blue flame

Uses

- to produce sulfuric acid

- in vulcanization of natural rubber

- bleaching of dried fruit and paper product

Compounds

1) Metalliic sulfide

- solid and dark/ black (ZnS/PbS yellow)

- anionic sulfide form highly electropositive metals undergo hydrolysis

- solid insoluble

- react with acid to evolve H₂S gas

2) Non metallic sulfide

H₂S

- colourless gas, foul smelling, extremely toxic gas

- dissolve in water to produce acidic solution

- easily oxidized

- as reducing agent

CS₂

- colourless liquid with fouling smell

- solvent for S, P, I₂ , rubber and wax

- hydrolyze in water

COMPOUNDS

Oxides

SO₂

- colourless gas, choking smell, poisonous gas

SO₃

- colourless gas, dissolve in water to form sulfuric acid, react with sulfuric acid to form oleum

SO₂

- react with water to form acid

- react with alkali to form sulfite salt

- as reducing and oxidizing agent

Sources of SO₂

- volcanoes activities

- combustion of sulfide ores, coal and oil

- roasting anhydride CaSO4 with coke

- reaction of sulfite salt with acid

- reaction of metal with conc. Sulfuric acid

SO₃

Preparation

- contact process

- heating Ferum (III) sulfate

- dehydration of conc. H₂SO₄ by solid P₂O₅

Properties

- form SO3 crystal when cooled

- react with water to form sulfuric acid

- react with sulfuric acid to form oleum

Oxoacid

H₂SO₃

- derived form SO₂

Properties

- dibasic acid, sulfite salt obtained by reacting acid with alkali

H₂SO₄

- derived form SO₃

Properties

- dibasic acid, strong acid

- conc. Sulfuric acid is viscous liquid due to HB

- High BP due to HB

- conc acid as dehydrating agent

- dilute acid as an acid

- hot and con as oxidizing agent

H₂SO₄ ---> sulfate salt

- obtained by reacting the acid with = alkali, metal oxide, metal, carbonate/ dicarbonate

Uses

- fertilizer, as detergent, dehydrating agent, pigment, to produce conc. HCl

Industrial Manufacturer of H₂SO₄

- touch process

1) Combustion S ---> SO₂

2) Oxidation SO₂ ---> SO₃

3) SO₃ transformation to H₂SO₄

I) Dissolution of SO₃ with H₂SO₄ ---> oleum

II) Added amount of water to oleum ---> conc. H₂SO₄

Halide

- exist for F, Cl, Br

- S₂F₂ = gas

S₂Cl₂ = yellow liquid

S₂Br = unstable liquid structure

- hydrolyze in water

- S₂Cl₂ further react with Cl₂ ---> SCl₂

- SCl₂ react with ethane ---> mustard gas

Sulfur tetrahalide

Reaction

- hydrolysis in water and alkali

- able to expand the octet

Sulfur hexahalide

Reaction

- S react with all halogen except Iodine

Properties

- colourless, odourless, tasteless, non toxic, thermally stable, insoluble in water

Thiosulfuric acid

- not stable, salt is the important part (Na₂S₂O₃.5H₂O)

- uses for quantitative analysis in iodometry, also in photography

# data[].attributes.body
Thank you dr for the class. Here are some summary for group IVA:
Group IV
- metallic character increases down the group but IE and shielding effect decreased
- different between oxygen and other elements: electronegativity O very high, can form p(pi)-p(pi) bonds with itself, C and N
OXYGEN
- preparation: by fractional distillation of liquid air for commercial and heating of KCLO3, decomposition of H202, electrolysis of water in laboratory
-characteristic: colourless gas, blue liquid in liquid form, paramagnetic
-use: producing fuel cell, respiration, welding industries
• OZONE
- formation: photochemical decomposition of NO2, electrical discharge of O2 followed by cooling liquid oxygen
- characteristic: blue gaseous, and dark blue in liquid form, smell, strong oxidation agent
-testing: by using mercury
- use: water treatment, detergent, deodorant, prevent UV ray in atmosphere
COMPOUNDS:
• oxides
- form oxide, peroxide, superoxide
-properties: nature of bonding and acid-base
• hydride
- water,H2O
- properties: colourless liquid, solid, gas, polar molecules, neutral oxide
- properties: act as ligand, oxidizing and reducing agent
-H2O2
-book shaped structure
- properties: colourless syrup liquid, strong oxidizing agent and reducing agent
- use: bleaching agent, antiseptic
SULFUR
- free element (brimstone) formed by bacterial action
- exists as S8 molecule in form of puckered ring
- allotrope: alpha and beta rombhic sulphur
- extraction: frasch process
- properties: odourless, tasteless, light yellow non metallic solid, flammable with blue flame
- use: to produce H2SO4, as components of black gunpowder, bleaching dried fruit
COMPOUNDS
1. Metallic sulfide
- solid and dark colour, insoluble in water, react with acid
2. Non- metallic sulfide
-H2S:  colourless gas, foul smelling, toxic gas
- CS2: colourless liquid with fouling smell, hydrolyze in water
• OXIDE
1.  SO2: colourless gas, chocking smell, poisonous gas
- properties: react with water form acid solution, reducing and oxidizing agent
- sources: volcanoes activity, combustion of sulfide ore, roasting anhydride CaSO4
2. SO3: colourless gas, dissolved in water to form sulfuric acid
- preparation: contact process, heating of ferum(III) sulfate
- properties: forming SO3 crystal when cooled, reaction with water, reaction with sulfuric acid
• OXOACID
1. H2SO3: sulfurous acid
- properties: dibasic acid, obtained salt when react with alkali
2. H2SO4: sulfuric acid
- properties: dibasic acid, strong acid, viscous liquid, high boiling point
- obtain sulfate salt by react H2SO4 with alkali, metal oxide, metal, carbonate
- use: chemical detergent, produce conc. HCL
• HALIDE
- exist for F and Cl, a few for Br and not exist with I
- disulfur dihalide: sp3 hybridization, can hydrolysis in water
- sulfur tetrahalide: sp3d hybridization
- reaction: hydrolysis in water and alkali, able to expand the octet
- sulfur hexahalide: sp3d2 hybridization
- properties SF6: colourless, odorless, tasteless and non toxic
• Thiosulfuric acid ( H2S2O3)
- not stable, has sp3 hybridization
- use: quantitative analysis in iodometry and in photography

# data[].attributes.body
Thank you Dr.for today lesson.Here my summary:
OXYGEN
-Metallic character increase down the group
-IE decrease due to shielding effect
-electronegativity is very high form ionic character,form hydrogen bonding
ALLOTROPE
i)O2
ii)O3
i)-preparation: from fractionally distillation of liquid air to seperate O2(commercially)
-in liquid form:blue liquid
-uses:producing fuel cell,respiration
-ii)preparation:O+O2-------O3
-dark blue,smell
-as detergent,deodorizer.
OXIDES
-oxide(diamagnetic)
-peroxide(diamagnetic)
-superoxide(paramagnetic)
HYDRIDE(H2O)
-polar molecule
-amphoteric character,act as ligand
(H2O2)(hydrogen peroxide)
-syrup liquid due to hydrogen bond
-bleaching agent,antiseptic
SULPHUR
ALLOTROPE
i)alfa rhombic
ii)beta monoclinicS
EXTRACTION:
-Frasch process
-reactive element
-not readily welted
-flammable and burn in air with blue flame
-produce H2SO4,component black powder,bleaching of dried fruit
OXIDE(acid rain)
-SO2+H2O-----H2SO3
-Volcanoes activities form emmision SO2 from increase temperature
-SO3(contact/touch process)
-SO2+O2------SO3
-forming SO2 crystal
-OXOACID
H2SO3(dibasic acid)
-salt:sulfite ion
-H2SO4
-dibasic acid,strong acid,vicous liquid due to hydrogen bond,as catalyst
-contact/touch process:SO3 not dissolve directly to H2O to avoid fog formation
HALIDE
-only I does not exist
-Disulphur dihalide
-sulphur tetrahalide(distorted trigonal bipyramidal)
-sulphur hexahalide
-S directly react with halide except I,non-toxic,
-thiosulphuric acid
-not stable,uses starch as indicator

# data[].attributes.body
Thankyou Dr fon the lesson .

Group IVA (chalcogens group)

🔴Down group Metallic character increase
🔴Down group IE decrease,
🔴Oxidation state O
(-2 stable - 1 perox)
Others : - 2  to +6
🔴Ionic when react IA & IIA
Covalent M2-,
Two covalent,
Mr- ion,
onium salt
Hypervalents MR4 & MR6(exc O does not has d orbital)

ELEMENT OXYGEN

🔴Reasons Different from others
1)very high electronegativity (ionic character and hydrogen bonding)
2)form strong p pi - p pi with O,C,N (double bond)  while others form rings and chain
🔴Form allotrope
1)O2 oxygen
2)O3 ozone
🔴O2 OXYGEN
⚪Preparation
1) commercial
Fractional distillation of liquid air
2)laboratory
- heating KlCo3(s) with MnO4
-decomposition of H2O2 with MnO4
-electrolysis of water (graphite as electrode)  O2 formed at cathode
⚪Characteristic
1)in Gas colourless, in liquid blue form
2)O2 paramagnetic : 2 unpaired electron (according MOT)
3)Combine with most element exc noble gas
⚪ USES
1)Fuel cell (generate energy)
2)respiration
3)welding industry
🔴OZONE O3
⚪ have resonance structures
⚪Formation of ozone
1)O+O2->O3
2)photochemical decomposition NO2
3)industrial production
Electrical discharge O2(g) followed cooling to liquid oxygen and distill
⚪ Characteristics
Blue gaseous, dark blue liquid
Smell
Strong oxidation agent
⚪Testing O3
using Mercury, from bright shining Mercury to tarnish and Hg stick to surface
⚪Uses
1)Water treatment to kill bacteria
O3 better than Cl2
2)Detergen, deodorizer, presevertive
3)prevent high energy uv to reach earth
4)ozone treatment
🔴Compoud
⚪OXIDE
1)in form  oxide, Peroxides   Superoxide
2)Proven diamagnetic/paramagnetic from MOT
3)class oxide
- normal oxide
-high oxide(excess O content)
-suboxide(less O content)
-mix oxide(mix 2 diff oxide)
5)properties
-Nature of bonding: ionic, covalent, intermediate
-Acid base : strong acid, strong base, neutral, amphoteric
6)acid base oxide
-metal& non metal
-oxidation state same element increase, acidity increase
⚪ hydride
-H2O, water
-Sp3,bend, AX2E2
-Properties
1)polar molecule
2)colourless in (l) (s) (g)
3)density solid<liquid
4)neutral oxide (but can change acid or base depend compound react)
5)ligand
6)oxidising and reducing agent
⚪Hydrogen peroxide
-book shapes structure (open book)
-properties
1)colourles syrupy liquid(HB)
2)thrmally unstable and decompose
3)strong oxidizing agent
4)as reducing agent
-Uses
1)bleaching agent
2)antiseptic, disinfectant, germicide

ELEMENT SULFUR

🔴Free element S, Brimstone and Exists as S8molecule crown shape)
🔴allotrope
Alpha-rhombic and B-monoclinic S
🔴S8 ring arranged differently (granulated and another is needle like form)
🔴Extraction by Frasch Process
🔴Properties
-odorless, tasteless, light yellow non-metallic solid
-not dissolved by water (floating)
-rhombic and monoclinic soluble in most organic solvent
-high Solubility
-flammable and burn in air (blue flame)
🔴Uses in H2SO4, black gun powder, vulcation of natural rubber
🔴sulphur compound
1)Metallic sulphide-ionic
2)Non metallic sulfide-covalent
-H2S
-CS2
🔴Compound
⚪Oxide.
1)SO2
2)SO3
Prepare by Touch Process or heating of ferum(II) Sulfate or dehydration of conc H2SO4
Form So3 crystal
⚪OXOACIDS
1)H2SO3 sulphurous acid +4,
anion So3 2-
2)H2SO4 sulphuric acid +6
Anion: So4 2-, dibasic strong acid
3)industrial manufacture.
CONTACT/TOUCH PROCESS
⚪Halides
For F, Cl, few Br, I not exist
S2F2-gas
S2Cl2-yellow liquid
S2Br2 - unstable liquid structure

1)SX4 (sulfur tetrahalide) , For perpare if X:F =73 c, inert atmosphere
2)SX6 (sulfur hexahalide) direct with halogen exc Iodine
3)Thiosulphate (H2SO2O3 not stable & S2O3 2-)
Salt : Na2S2O3.5H2O

# data[].attributes.body
Thank you Dr. for the lesson. Here is my summary for Group VIA :-
Going down the group :

Metallic characteristic increases shown by electrical properties of the elements

IE decrease due to decrease shielding effect.

Oxidation state : - 2 to +6 except oxidation state for O : -2 & -1
The reason why oxygen is different from other members :-

High electronegativity

Strong ppi-ppi bond with itself , carbon and nitrogen.

Oxygen

- Form 2 Allotropes

Oxygen, O2

Preparation
-Commercial : Fractional distillation of liquid air to separate O2
-In laboratory :

Heating KClO3

Decompostion of H2O2

Electrolysis of water uses graphite as electrodes

Characteristic :
-Colourless gas , blue liquid and paramagnetic.
Uses :
- Producing "fuel cell"
-Respiration
-Welding industries

Ozone,O3

Formation :

Directly form from O and O2

Photochemical decomposition of NO2

Industrial production : Discharged of O2 gaseous followed by cooling to liquid oxygen and distills.

Characteristic :
-Blue gaseous , dark blue liquid , smell and strong oxidizing agent .
Testing :  Use mercury
- Mercury will become tarnish and stick to the surface of the glass.
Uses :-
-Water treatment.
- As detergent , deodorizer and preservative.
-Prevent UV from reaching the earth.
Compound of oxygen
Oxides

1. Oxide - paramagnetic

2. Peroxide - diamagnetic

3. Superoxide - paramagnetic

4 types of oxides :-
- Normal Oxide
-High Oxide
-Suboxide
-Mix-oxide
Properties depends on :-
- Nature of bonding and acid-base.
Hydrides
Water, H2O
Properties :
- Colourless liquid, gas and solid , polar molecule , solid state is less dense than liquid state , give amphoteric characteristic , act as ligand and act as oxidizing agent and reducing agent.
Hydrogen peroxide , H2O2,
Properties :
- Colourless syrupy liquid , thermally unstable and decomposes in the presense of finely divided metal catalyst, strong oxidizing agent and reducing agent.

Sulfur
Allotropes:-
-Alpha-rhombic S
-Beta-monoclinic S
Extraction :

Frasch Process

Properties :
-Odourless, tasteless ,light yellow non-metallic solid, reactive element when combines with other elements except inert gasses, gold and platinum.
Uses :
-Used to produced sulfuric acid
-Component of black gunpowder.
-Used in the vulcanization of natural rubber
-Used in the bleaching of dried fruits.
Compounds of Sulfur.
1. Metallic sulfide (Ionic sulfide)
2. Non-metallic sulfide (Covalent sulfide)- H2S & CS2
Oxides

SO2

Oxidation state : +4
Properties :  Colourless gas , chocking smell and poisonous gas.
Sources :
-Volcanoes activities
- Combustion of sulfide ores , coal and oil.
-Roasting anhydride CaSo4 with coke
-Reaction of sulfite salt with acid
-Reaction of metal with conc. sulfuric acid.

SO3

Preparation :
-Commercial : Touch process
-Dehydration of conc. H2SO4 by solid P2O5.
Properties : Colourless gas , dissolve in water produce sulfuric acid and react with sulfuric acid to produce oleum.
Oxoacids

Sulfurous acid/ Sulfuric(IV) acid , H2SO3

-Derived from SO2
-Salt : Sulfite anion.
Properties : - Dibasic acid , sulfite salt is obtained by reacting the acid with alkali.

Sulfuric acid or Sulfuric(VI) acid , H2SO4

-Derived from SO3
-Salt: Sulfate anion.
Properities:
-Dibasic acid, conc H2SO4 is viscous liquid and dehydrating agent , high boiling point , in dilute concentration acts as acid and conc and hot as oxidizing agent.
Uses :
-Fertilizers , chemicals for detergent , ether , ester , dehydrating agent , used as white glow pigment and to produce conc. HCl .
Industrial Manufacture : Touch Process
Halides

Sulfur halides & Disulfur halides
- Only exists for F , Cl and Br.

Sulfur tetrahalide

Sulfur Hexahalides

Thiosulfuric acid and its Salt
-Thiosulfuric acid is not stable
Uses : Quantitative analysis in Iodometry and in photography .

# data[].attributes.body
Thank you Dr for today lesson, here is my summary for Group VIA:

-when down the group:
metallic character increase
IE decrease
-Oxygen is different from others due to high EN and strong p pi p pi bond

Oxygen:
- preparation, characteristics and uses

Ozone:
- formation, characteristics, testing of ozone (by Hg) and uses of O3 (H20 treatment and ozone treatment)

Compounds of oxygen:
- monoxide, peroxide and superoxide
- oxides can divided into normal oxide, high oxide, suboxide, and mix-oxide
- properties of oxide compound

Hydride of oxygen:
- H2O ( properties)
- H2O2 (properties and uses)

Sulphur
- allotrope, extraction, properties and uses

compound of sulphur:
- metallic sulphide, and non metallic sulphide

Oxide of sulphur:
- SO2 (properties and sources) and SO3 (properties)

Oxoacids: H2SO3 and H2SO4
-structure, properties, salt uses, and preparation of H2SO4

Halide of Sulpbur, sulphur tetrahalide and sulphur hexahalides

Thiosulphuric acid and the use of its salt

# data[].attributes.body
Summary Group IVA:
-Down the group, metallic character increases while IE decreases.
-Oxidation state : O : -2(stable)
others : -2 to +6
OXYGEN
1. Different form other members in group because the electronegativity of o2 is very high and can form strong ppi-ppi bonds.
2. Preparation :
-Fractional distillation of liquid air to
separate O2.
-Heating of KClO3.
-Decomposition of H2O2.
-Electrolysis of H20 uses graphite as
electrodes
3. Compound of Oxygen- OXIDE
i) form normal oxide, high oxide, suboxide and mix-oxide (spinel compund).
ii) Properties :
- Nature of bonding
- Acid-Base
4. Compound of Oxygen- HYDRIDES
(H2O)
i) Properties : - polar molecule
- act as ligand
- act as oxidizing and
reducing agent
5. HYDROGEN PEROXIDE- H2O2
i) open book structure.
ii)Properties:
- Colourless syrupy liquid.
-Thermally unstable & easily decompose
-Strong oxidizing agent.
- As reducing agent.
iii) Used as bleaching agent, as antiseptic and used in mild oxidant.

SULFUR
1. Ring in crown shape.
2. Allotrope : Rhombic & Monoclinic
3. Extraction : Frasch process
4. Chemical properties :
- Combustion.
- Heating with metal.
- Reaction with conc. acid
5. Compound of Sulfur- OXIDES
i) Chemical properties:
- react with H2O to form acid solution
- react with alkali
- reducing agent
- oxidizing agent
6.Compound of Sulfur- OXOACIDS
i) Derived from SO2
ii) The salt : sulfite ion, (SO3)2-
iii) Uses of H2SO4
- fertilizers
-chemical for detergent
- dehydrating agent
- white glow pigment
- produce conc. HCl
7. Compound of Sulfur- HALIDES
i) sp3 hybridization
ii) Preparation :
-hydrolysis in water
- S2Cl2 react further with Cl2
- SCl2 react with ethane
iii) Uses :
- qualitative analysis in iodometry
- in photography

# data[].attributes.body
Thank you for the lecture dr <3
Summary of Group VIA
Oxygen
1)Metallic character increases ,IE decrease down the group
2)The types of compounds formed are ionic (E+ Group IA&IIA) and covalent with most of the elements
3)Its different from other members because it has high electronegativity and it forms strong ppi-ppi bond with itself ,C,N.
Preparation
- Commercial: Fractional distillation of liquid air
-Laboratory
: Heating of KCl
:Decomposition of  H2O2                  :Electrolysis of water using graphite as electrodes
4)Has characteristics such as colorless gas, blue liquid form, paramagnetic
5)Has usage such as producing fuel cell ,respiration, welding industries
6)The compounds of oxygen are such as oxides(normal oxide, high oxide, suboxide, mix-oxide),Hydrides(water)

Sulfur
1)Exist as a brimstone (S)
2)The ores are :pyrite, galena , sphalarite
3)Sulfur is extracted through Frasch Process
4)The properties of sulfur are such as odorless, tasteless, non-metallic solid, not readily wetted or dissolved by water, reactive element except when it is combined with(inert gases, gold, platinum)
5)Uses are such as production of H2SO4, component of black gunpowder, vulcanization of natural rubber
6)Chemical properties:
- Reaction with oxygen
-Heating with metal becomes metal sulfides
-Reaction with conc. acid
7)Compounds of sulfur are (ionic, covalent sulfide), oxides(so2,so3), oxoacids(H2SO3, H2SO4) halides(SX4,SX6)
~ For halides it does not exist for I

# data[].attributes.body
SUMMARY GOURP IVA
DOWN THE GROUP:

·Metallic character INCREASE

-O & S: non-metallic and insulator

-Se & Te: metalloid & semiconductors

-Po:truly metal and conductor

·IE DECREASE:decrease shielding shielding effects

· Oxidation state:

§  O: -2(stable),-1(peroxo)

§  Other element: -2 to +6
Type of compound form;

·Ionic: E + Group IA and IIA

·Covalent: most of element

i.M2-ions

ii.Two covalent bonds

iii.MR- ions

iv.Onium salts

v. Hypervalents  MR4 and MR6 (except O)
Oxygen different from other;
1.Electronegativity of O high

i.Form ionic character on M-O bonds

ii.Form hydrogen bond
2.Form strong p-p bonds with itself,C & N

OXYGEN
·Exist in atmospheric gaseous (21% )

·Anionic mineral in earth crust(carbonate,nitrate,sulfate,oxides)

·In water
.Form allotropes
Preparation;
Comercial:Fractional distillation of liquid air to separate  from  and Ar
In Laboratory:

·Heating (s)

·Decomposition of

·Electrolysis of water uses graphite as electrodes
Characteristic;

·Colorless gas
· in liquid form:Blue liquid

·is paramagnetic with 2 unpaired electrons (according MOT)

ACID BASE OXIDE :
-metal and non-metal
-oxidation state which is acidity increase when oxidation increase
HYDRIDES OF OXYGEN :
- WATER, H₂O  (bent shape with hybridization sp³)
~PROPERTIES :
i) polar molecule
ii) neutral oxide but change to acid/alkali (develope  amphoteric character)
iii)act as ligand
iv) act as reducing agent and oxidizing agent
-HYDROGEN PEROXIDE ,H₂O2  (has book shape structure)
~PROPERTIES :
i) colourless syrupy liquid due to hydrogen bonding and soluble in alcohol
ii)thermally unstable and decompose when finely divided metal catalyst
present
iii)strong oxidizing agent and also a reducing agent
~USES :
i) as bleaching agent for wool, hair and teeth
ii) as antiseptic, disinfectant and germicide.

SULFUR
`Exist in free element and S8 molecule;granulated form and needle form
Extraction of sulfur;
`mined by Frasch process
Properties of sulfur;
`odourless,tasteless,light yellow non-metallic solid
`not readily wetted or dissolve in water
`high degree of solubility
`flammable and burn in air with blue flame
Uses;
produce sulfuric acid
`component of black gunpowder
`use in vulcanization of natural rubber,fungicide and fumigant.
`bleaching dried fruits and paper product
Chemical properties;
`Reaction with O2(combustion)
`heating with metal become metal sulfide
`reaction with conc.acid
Compound of sulfur
1.metallic sulfide
`all metallic sulfide in dark/black except ZnS & PbS (yellow)
`solid insoluble in water
`react with acid
2.Nonmetallic sulfide(covalent sulfide)
H2S;
`colorless gas,foul smell(like rotten egg smell),extremely toxic gas,dissolve in water,easily oxidize,reducing agent.
CS2;
`colorless liquid,fouling smell,solvent for,S,P,I2,rubber wax
`hydrolyse in water
Oxide of sulfur;
SO2;
`Colorless,chocking smell,poisonous gas
`react w water form acid solution,react w alkali,reducing agent,oxidizing agent.
`source;volcanoes activity,combustion sulfide ores,coil and oil,roasting anhydride CaSO4 with coke,reaction of metal w conc.sulfuric acid,reaction sulfite salt w acid.
SO3;
`Preparation:touch process,heating ferum(III) sulfate,dehydration of conc.H2SO4 by solid P2O5
`Properties;forming SO3,reaction w water
H2SO3;
`Salt; sulfate anion
`properties;ionazation,sulfate salt
H2SO4;
`salt;sulfate anion
`properties;dibasic acid,strong acid,high b.p.,sulfonate agent
`sulfate salt;obtained by reacting H2SO4;Alkali,metal oxide,metal,carbonate/bicarbonate
`Uses;fertilizers,chemical for detergent,ether and ester,dehydrating agent,pigment,produce conc. HCl
Contact process;
`combustion of S
`oxidation of SO2
`SO3 transformation to H2SO4
Halide of sulfur
`SX4
`SX6
`Thiosulfuric acid and its salt
-uses;quantitative analysis in iodometry,in photography.

thank you dr!

# data[].attributes.body
Thank you dr for your well explainations . Here are my summary about group IVA :
OXYGEN
# Exist in the atmospheric gaseous
# Form 2 allotropes
- oxygen O2, ozone O3
# Preparation
- from fractional distillation of liquid air
- heating of KClO3
- decomposition of H2O
- electrolysis of water (graphite-electrodes)
# Colourless, liquid(blue), paramagnetic(2 unpaired e)
# Uses
- producing fuel cell
- respiration
- welding industries
# Formation of ozone
- blue gaseous , smell, strong oxidation agent
- mercury ( becomes tarnish)
- substitute of Cl2 (water treatment)
- layer prevent high energy UV
#Oxides
- form oxide(paramagnetic), peroxide(diamagnetic), superoxide(paramagnetic)
#Hydrides (H2O)
- sp3, bent , AX2E2
-colourless liquid , solid and gas
- polar molecule and neutral oxide
- act as ligand
_ oxidizing & reducing agent
-H2O2 (bleaching agent ,colourless,thermally unstable , strong oxidising agent, reducing agent)

SULFUR
# exist as free element (brimestone)
# formed 2 S8 ring
# odourless,tasteless,light yellow
# high degree of solubility
# used in the vucanization of natural rubber, fungicide, furnigant
#Chemical properties
- combustion (O2)
- heating with metal (metal sulphide)
- reaction with conc. acid
#Oxides
-SO2
react with water, alkali.Reducing & oxidizing agent.
-SO3
prepared by Touch process & heating Fe2(SO4)3
#Oxoacids
1)sulfurous acid H2SO3
- derived from SO2
- dibasic acid & sulphite acid
2) sulfuric acid H2SO4
- derived from SO3
- dibasic acid & strong acid
- dehydrating agent
- sulphate salt by react with alkali, metal oxides, metal, carbonate/bicarbonate
- fertilizers
-CONTACT/TOUCH PROCESS
# Halides
-hydrolysis in water
- able to expend the octet
- S react directly with all halogen
- quantitative analysis in Iodometry
- photography decolorize

# data[].attributes.headline
NUR QISTINA IZZATI BINTI MOHD FITRINAZRIN POON

# data[].attributes.subject
NUR QISTINA IZZATI BINTI MOHD FITRINAZRIN POON

# data[].attributes.body
Group VIA
Oxygen ,Sulphur, Selenium, Tellurium, Polonium.

V.e = 6

Metallic character increases down the group

IE decreases down the group due to the decreased shielding effect along Se,Te and Po.

OXYGEN

Types of compounds form : ionic : Group IA and IIA , covalent : most of elements.

Electronegativity is very high (sec highest in periodic table)

Forming strong p-pi p-pi bonds with itself , carbon and nitrogen.

Exist in atmospheric gaseous (21%）， in water ,anionic mineral in CO2,NO3,SO4 and Oxides.

Form 2 allotropes : O2 n O3.

Preparation : Commercial : from fractional distillation of liquid air to separate O2. Lab : Heating of KCLO3 ,decomposition of H2O2 and electrolysis of water uses graphite as electrodes (anode)

Colourless gas and in liquid form: blue liquid

Paramagnetic with 2 unpaired electrons.

Reactive@ elevated temperature n combine directly with most of elements except noble gas.

Producing " fuel cell" ,carbohydrate, respiration, and welding industries.

OZONE

Got resonance structure

FORMATION OF OZONE
1. O (g) + O2 → O 3 (g)
2. Photochemical decomposition of NO 2
NO ₂ (g)  NO (g) + O (g)
O (g) + O ₂ → O 3 (g)
3. Industrial production of O ₃
3O ₂ (g)  2O 3 (g)

CHARACTERISTICS
* Blue gaseous in colour
* Dark blue liquid
* Strong oxidation agent
* Smell

OZONE TEST
Use Mercury, Hg . The bright shining Mercury will become tarnish and starting to stick to the surface of glass in the presence of Ozone.

USES
* Deodorize air, purify water, and treat industrial wastes.
* It atmosphere ,O3 prevent high energy UV frm reaching earth.
* Detergent.
* Preservative.

Compounds of Oxygen : oxide (paramagnetic) ,peroxide(diamagnetic) and superoxide (paramagnetic).

Properties of oxides compounds.

Oxidation increases, acidity increases.

HYDRIDES OF OXYGEN

* H2O-WATER

polar molecule ,act as ligand,amphoteric character

Structure of H2O2 : open book

H2O2 : colourless syrupy liquid strong oxidizing agent also act as reducing agent.

Uses : bleaching agent for wool,hair and teeth , antiseptic.

SULPHUR

Exist as free element ,S (brimstone)

Ores :pyrite (FeS),Galena(PbS) and sphalerite (ZnS)

S8 molecule ( crown shape)

Extraction of S : FRASCH PROCESS

Odourless, tasteless,light yellow,non-metallic solid

Not readily wetted or dissolved by H2O

Flammable and burn in air with blue flame.

Uses : produce H2SO4 , vulcanization of natural rubber , bleaching of dried fruits and paper products.

Reaction with O2 (combustion)

Heating w metal bcomes metal sulfide

Rection w conc acid

Compounds of S

Metallic sulfide (ionic sulfide)

Non-metallic ( covalent sulfide)

Oxides of Sulfur

SO2 & SO3

H2SO3 *H2SO4

Uses of Sulphuric acid , H ₂ SO ₄

* Fertilizers : (NH ₄)₂ SO 4

* Produce conc. HCl

NaCl (s) + H ₂ SO 4 → Na ₂ SO 4 (aq)+ HCl(l)

* Chemicals for detergent, ether and ester
-CONTACT/TOUCH PROCESS

Halides of Sulfur

EXIST

* X= F & Cl

* X= Br (only a few)

NOT EXIST

* X= I

Disulfur dihalide,S ₂ X ₂

* 2S(s) + X ₂ → S ₂ X ₂(l) ; X=F,Cl,Br

* S ₂ F ₂ - gas

*S ₂ Cl ₂ - yellow liquid

*S ₂ Br ₂ - unstable liquid structure

S ₂ X ₂
sp ³ hybridization
Hydrolysis in water
* S ₂ X ₂ + H ₂ O → HX + H ₂ SO ₄ + S↓
*S ₂ Cl ₂
S₂Cl2 react further with Cl₂ to produce SCl2
* S ₂ Cl ₂ + Cl ₂ → 2SCl 2
* SCl₂ reacts with ethane(ethylene, C₂H₄) give mustard gas S(CH₂CH₂Cl)2     *mustard gas used in warfare.
SX ₄
sp ³ d hybridization
Preparation
* S(l) + X ₂ → SX ₄ ; X=Cl
* S(l) + X ₂  SX ₄ ; X=F
Reaction
Hydrolysis in water and alkali
*SX ₄+H ₂ O→ SO ₂(g)+ HX
*SX ₄+OH⁻ →SO ₃ ²⁻(aq) +4X⁻ + 3H ₂ O Able to expend the octet
*SF ₄ + F ₂ →SF ₆
SX ₆
sp ³ d ² hybridization
*Synthesis
S directly react with all halogen except iodine to form SX 6
Properties SF ₆
-Non-toxic
-Colourless,tasteless,Odorless.
-Thermally stable and insoluble in water.
Thiosulfuric acid (H ₂ S ₂ O ₃) & its Salts (S ₂ O ₃ ²⁻)

- H ₂ S ₂ O 3  is not stable

-The important salt is Na ₂ S ₂ O 3 . 5H ₂ O

- sp 3 hybridization

- Uses

-Quantitative analysis in idometry

- In photography :S ₂ O ₃ ²⁻ is used to remove silver(l) salt which is not reduced by Ag.

Thank you very much for the lessons dr .