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Thank you Dr for the explanation for Group IVA. So here is my summary for Group IVA.

Carbon
-The allotrope are diamond, fullerence and graphite.
- Because of the inert pair effect, the oxidation number +2 become much more stable down the group.
-Carbon show the greatest tendency to catenation.
Silicon
-It is the 2nd most abundant element on earth.
- We can obtain pure Si by reducing SiO2 using Coke.
-3 types of Silicone Disilicone, Chain Silicone, and Branched Silicone.
- It has high melting point
-it dissolve in base only HF which is acid.
- It is thermally stable up to 500-600K and low viscosity.
Tin
-Pure Tin can be extracted from cassitserite,SnO2.
- It is a soft metal, it is melleable but is not very ductile.
-Tin sulfide can exists as mono SnS and disulphide SnS2.
-It can dissolve in water to create a cloudy solution.
-When heated it becomes brittle.
- It is an amphoteric oxide.
Lead
-Has high density, low boiling point.
- It is very soft.
- It is very ductile and highly malleable.
- Lead oxides can exists as PbO, PbO2, and Pb3O4.
-PbO2 is usually use as cathode in lead acid battery.

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Thank you Dr for the whole explaination about group IV. Here is my summary for this group
-Due to the inert pair effect, +2 more stable than +4 as it goes down the group
-Catenation which is the ability of an element to be bonded to another to form a long chain or ring and the catenation decrease as it goes down the group.
-reactivity increase as it goes down the group
CARBON(C)
-the allotropy : diamond, graphite and fullerence (common)
-diamond the hardest one and has very high of melting point
-Oxide of Carbon( CO and CO2)
CO form due to incomplete burning and can be prepare by dehydration of formic acid and reduction of CO2 by hot red. and the uses of CO are hydroformylation and production of pure nikel metal using Mond Process.
CO2 can be prepare by reaction of acid and marble and also heating the marble(CaCO3). the uses of CO2 are fire retartand and one of reactant in producing Na2CO3
-Carbonate and Hydrogen Carbonate(dissolve in water except for group IA)
-Halide of C
did not undergo hydrolysis because C has no d orbital to receive a pair of electron from water and the uses are Freon (refrigating gas) and non stick cooking utensil
-Carbide (ionic, covalent and insterstitial)
SILICON(Si)
-extraction : reducing SiO2 by coke and obtain pure Si by reducing the SiCl4 by Na and zone refining process
-Oxide (silica, SiO2)
can be prepare by hydrolysis of SiCl4 and acidation of water glass(Na2SiO3 disslove in water). silicate can be form when SiO2 react with metal oxide/sulphate/carbonate
-Aluminosilicate (3D silicate and an important in catalyst)
example of it are Feldspor and silicate glass
-Silicone
can be prepare by hydrolysis of alkyl, aryl silicon halide followed by condensation and it has 3 types which is disilicone, chaim silicone and branched silicone
TIN (Sn)
-alpha Sn, beta Sn and gamma Sn can be form depends on the temperature
-the most common alpha Sn(diamond lattice) and beta Sn (tetrogonal)
-Oxide of Si (SnO2 and SnO)
SnO2(+4) can be prepare by direct heating on the metal in air or oxygen
SnO(+2) can be prepare by heating tin oxalette
both of it are amphoteric but SnO more base than SnO2
-Halide of Sn( SnCl4 and SnCl4)
SnCl4(+4) can be prepare by directly heating Sn with chlorine gas and covalent compoind with tetrahedral
SnCl2(+2) has two type: anyhydrous of SnCl2 and hydrated SnCl2.2H2O
-Sulfide of Sn(dark brown)
SnS can be obtained by passing through the H2S gas in the Sn(ii) solution and easily oxidize to SnS2(oxidation of SnS by using ammonium polysulphides)
LEAD(Pb)
-Oxide of Pb: PbO(yellow solid), PbO2(dark brownish black) and Pb3O4(red)
due to the colour of Pb3O4(red) use as pigment in paint which can protect thd iron or steel from rusting
-Halide of Pb( Pb(ii) more stable than Pb(iv) )
PbBr4 and PbI4 do not exist as it not strong oxidizing agent which unable to oxidize to Pb(iv) and for PbX2 is ionic form with white colour except for PbI2 which is yellow.

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Thank you Dr for the lesson . here is my summary for group IVA:

-Normal oxidation number is +4 but due to inert pair effect,  the oxidation number of +2 becomes more stable down the group.
-Reactivity increases down the group.
CARBON(C)
-showing the greatest tendency and forming and forming stable hydrocarbon chains and rings due to good overlapping p pi- p pi orbitals of carbon.
- Able to form allotropy(diamond, graphite and fullerene the most common)
-OXIDE: exist as CO2 & CO
-PREPARATION CO: dehydration of formic acid or oxallic acid by con H2SO4 & reduction of CO2 by hot-red C
PREPARATION CO2: reaction of acid with calcium carbonate (marble) & heating.
HALIDES OF CARBON,CX4: does not undergo hydrolysis because C has no "d" orbital to receive a pair of electron fromwater molecule.
SILICON(Si)
- 2nd most abundant element in the earth.
-exist as SiO2 and as silicate substance.
-having diamond latti
-OXIDE:
->Silicon dioxide,SiO2 (also known as silica)
->Exist as polymeric tetrahedral SiO2.
- PREPARATION: Hydrolysis of SiCl4 & Acidification of water glass
-Silicate (SiO)4- form when SiO2 react with metal oxides/ metal sulphate/ metal carbonate
-Aluminosilicate are 3-dimensional silicate
- Types of Silicone:
1) disilicone
2) chain silicone
3) branched silicone
-Silicon Halides, SiX4 form by using stock's reaction.
Tin(Sn)
-reduction of Tin Ore(pure) with anthracite.
-Transformation temperature between allotropes.
-OXIDE: Exist as SnO2 & SnO
-HALIDES: SnX2 is more stable than SnX4
-SULFIDE: Exist as mono (SnS) and disulphide (SnS2).
Lead (Pb)
- exist as mineral-glass, PbS
OXIDE: Exist as PbO, PbO2, Pb3O4
HALIDES: Pb(II) halides is more stable than Pb(IV) halide

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Thank you Dr for the detailed explanation. Here is my Summary for Group IV:

Carbon
- Due to inert pair effect, the oxidation no.+2 becomes more stable down the group.
- catenation : the ability of an element to be bonded to one another to form long chain or ring.
- carbon shows the greatest tendency to catenation.
-There are 8 allotropes of carbon( diamond, graphite, fullerene)
Silicon
- 2nd most abundant element on earth
- Pure silicon can be extracted by using Coke to reduce sand(SiO2).
-All types of glass have the same key ingredient which is Si.
- There are 3 types of silicones(Disilicone, chain silicone, Branched silicone).
Tin
- Pure Tin is extracted from cassitserite(SnO2)
-SnCi4 is less stable than SnCi2
- Tin sulfide can exsits as SnS and SnS2
Lead
- Lead oxides exists as PbO, PbO2, & Pb3O4
- PbO2 is mainly use as cathode in lead acid battery.
- Trilead tetraoxide is used in the paint industry as a red pigment to protect iron & steel from rusting.

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Thank you for the lesson Dr.Sheela.Here my summary:

CARBON
-Down the group the oxidation no. +2 become more stable due inert pair effect .
-Form allotropy(exist in  more than one physical form).
-Catenation(ability to bonded to another to form long chain or ring)decrease down the the group.
-Allotropy(diamond,graphite,fullerEne)
SILICON
-Extraction(reducing SiO2 by coke,reducing SiCI4)
-Characteristic(increase melting point,does not dissolve inany acid accept HF)
-OXIDE
-polymeric tetrahedral
-dissolved in HF only
-dissolbed in alkali
(SiO4)4
-SiO2 +  metal (oxide/sulphate/carbonate)
-dissoved on water to form water glass
ALUMINOSILICATE
-occur when Al atom substitutes Si in the silicate.
-Zeolite=hydrated aluminosilicate crystal having open structure framework
SILICONES
-Organosilicon silicon compound having heterocatenated Si--O-Si bond in chain ,ring,branches
-Hydrolisis followed by condesation.
-TYPE of SILICON
-disilicone,chair silicone,branched silicone
-USES(as lubricant,in comestic,breast implant)
-HALIDE
-All halide (exceptSiF4)
-are unstable and undergo hydrolisis in H2O.
-HYDRIDES(SILANES)
-Form catenation
-Hydrolisis in water and alkali
TIN
-Tin allotrope
-alfa-Sn,beta-Sn,gama-Sn
-Tin-plague/tin pest
-tin soft metal,not very ductile,crackle when bent.
OXIDE
-Sn + O2----SnO2
-pure ionic oxide
-SnO(black tin,amphoteric oxide(more base than SnO2)
HALIDE
-SnX2 >stable than SnX4
-Sn +CI2----SnX4
-colourless,covalent compund
-SnCI2
-have covalent and ionic character.
-Strong reducing agent(innert pair not strong)
SULPHIDE
-mono(SnS) and disulpahte(SnS2)
-dark brown and yello solid
LEAD(Pb)
-MINERAL GALENA(PbS)
-High density,low boiling point
OXIDE
-Exist (PbO,PbO2,Pb3O4)
-PbO(yellow solid,amphoteric oxide)
-PbO2
-Strong reducing agent,inert pair more strong,used in lead acid batery
-PbO2-----Pb3O4 +O2
-Pb3O4
-Red lead,paint made to protect ion and steel from rusting
HALIDE
-Pb(II)halide > stable Pb(IV) halide
-Br and I2 not strong oxidizing agent to oxidize.

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Thank you dr for your well explainations.My Summary :
CARBON
- Down the group oxidation no. +2 becomes more stable due to inert pair effect.
- Form allotrope which is exists in more than one physical form.
- Strength of covalent bonding which is the existence of polymorph macromolecule.
- Catenation which is bonded to one another to form long chain or ring.
-Reactivity increases down the group.( water,air,acid and base)
SILICON
- Reducing SiO2 by coke and obtain pure Si.
- Dissolve in base and high melting point.
- Types of silicon:
# dissilicone
#chain silicone
# branched silicon
- Thermally stable up to 500-600K and low viscosity with changes with temperature.
-As lubricant, uses in cosmetic and breast implant shell.
TIN
- Soft metal, melleable but not very ductile.
- Becomes brittle on heating and crackles when bent.
- Amphoteric oxide
-Anhydrous salt which is a trasparent crystalline solid.
-Dissolve in water to give cloudy solution.
- Exists as mono (SnS) and disulphide (SnS2)
LEAD
- High density but soft with low boiling point.
- High luster , ductile and high malleable
- Dark brownish solid and black powder.
-Amphoteric oxide and trilead tetraoxide.
-Pigment for paint which is red lead used to protect iron and steel from rusting.

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Thank you for today's lecture. This is my summary of Group IVA.
- Group IVA has a normal oxidation number of +4 and +2 becomes more stable down the group due ti inert pair effect.
- Carbon has 3 allotropes and tin has 2.
- Down the group reactivity increases, size increases, melting and boiling point decreases, tendency to catenation decreases, & IE decreases.
- Strength of covalent bonding decreases if they don't have non-bonding electron. Increases if they have non-bonding electrons.
- Catenation= the ability of an element to bind to itslef to form long chains or rings.
1. Carbon, C
- 3 allotropes; diamond (crystallization of molten magna), graphite (acheson process), & fullerene (lazer vaporization.
- Carbon Monoxide= preparation (reduction of CO2 & dehydration of formic acid); properties (colourless gas, no smell, toxic because binds with hemoglobin in blood), strong reducing agent; & uses.
- Carbon Dioxide= preparation (reaction of acid with calcium carbonate & heating calcium carbonate); properties (colourless gas, no smell); uses.
- Halides of Carbon= CX4
- Carbides
2. Silicon, Si
- Extraction & Characteristics (metallic luster & grayish)
- Silicon Dioxide, SiO2 (silica)= preparation (hydrolysis of silicon tetrachloride & acidification of sodium silicate); characteristics.
- Zeolite is a aluminoscilicate.
- Silicate glass= preparation; characteristics (not true solid, supercooled liquid, no melting point).
- Types of glasses= soft glass, hard glass, flint glass, jena glass, pyrex glass, crooke's glass, quartz glass, ground glass, reinforced glass.
- Types of silicone= disilicone, chain silicone, & branched silicone.
- Silicone properties= thermally stable, low viscosity, water repellent.
- Silicone uses= lubricant, hydraulic fluids, makeup, breast implant, car wax.
- Halides, SiX4.
- Hydrides of silicon (Silanes).
3. Tin, Sn
- Extraction= reduction of tin ore with anthracite.
- Allotropes= a-Sn, B-Sn, y-Sn.
- Properties= soft metal, malleable, brittle on heating.
- Oxides, halides (SnCl4 & SnCl2), sulfide (Sns & SnS2).
4. Lead, Pb
- Extraction= reduction with carbon.
- Properties= high density, soft, low boiling point, high luster, ductile, highly malleable.
- Oxides= PbO, PbO2, Pb3O4.
- Paint pigment= Pb3O4->red.
- Halide of lead= PbX4, PbX2.

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Thank you dr for today's lecture class. Here is my summary for this topic:
-Due to inert pair effect, the oxidation number of +2 becomes more stabe down the group IVA.
-Catenation is the ability of an element to be bonded to one another to form long chain or ring. Tendency to catenation decreases down the group.
-Allotropes of carbon include diamond, graphite, fullerene and so on.
-Properties and structures of each allotrope of carbon.
-Graphite can conduct electricity but diamond cananot.
-Carbon has higher catenation than silicon.
-Preparation, properties and uses of CO and CO2.
-2 ways to extract silicon.
-Types of silica and silicate
-Types of glasses
-Properties and uses of silicone
-Silicon halides, silicon hydrides
-SnCl2 is more stable than SnCl4.
-SnCl2 is predominantly covalent compound but with a little of ionic properties. Hence, it can soluble in both water and organic solvents.
-PbO is more stable than PbO2 due to inert pair effect.
-Pb(II) halide is more stable than Pb(IV) halide.

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Thank you Dr for the explanation on group IVA. This will be my summary for this chapter

Group IVA
- Has normal oxidation number of +4 and +2 as we move down the group which is more stable due to inert pair effect.
- Reactivity increases down the group
Catenation:
- Catenation is an ability for element to be bonded to one another to form long chain or ring
- Carbon shows the greatest tendency to catenation due to good overlapping of p pi-p pi overlapping orbital
- Silicon is low stable to form catenation due to poor overlapping of p pi-p pi orbital
Allotrope of Carbon:
- Diamond
- Graphite
- Fullerene
Compound of Carbon:
- Oxide
- Halide
- Carbonate
- Carbide

Silicon
- Is the second most abundant element metal on earth
Ways to extract Silicon
- Reducing sand with coke
- Reducing Sicl4 with Na
Characteristic of Si
- Has metallic luster and grayish in colour
- Have diamond lattice
- High melting point
- Inert but attacked by halogen
- Dissolve in base but not in acid except HF
Compound of Si
- Oxide
- Halide
- Hydride

Tin
Steps to extract Sn:
- Roasting
- Reduction
- Purification
- Electrolysis
Form allotrope when heated with different temperature:
- <13.2 degree is Alpha Sn
- 13.3 degree - 161 degree is Beta Sn
- 162 degree to 232 degree is Gamma Sn
- >232 is liquid Sn
Compound of Sn:
- Oxide
- Halide
- Sulfide

Lead
Physicochemical properties:
- Resist corrosive
- High malleability
- High density
Compound of Pb
- Oxide
- Halide

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Thank you dr for today’s lesson. This is my summary for group IVA

-Carbon does not affected by inert pair effect

-Inert pair effect is tendency of heavier atoms to form ions (with different charge) & use electron configuration to explain
-Carbon form allotrope which is diamond,graphite,fullerene, nanocarbon.
-Catenation is ability bonded to one another.
-Carbon showed greatest tendency forming stable hydrocarbon chain & rings but Si less stable.
-High energy more stable.
-Down the group, increases reactivity
CARBON
Allotrophy
1) Diamond
-crystallization of molten magna in earth crust
-can synthesized from graphite
-not easy process
-as cutting tool, precious jewelry
2) Graphite
-Acheson process
-stacked of two-dimensional carbon sheets.
-soft , weak bonds between layers
-conducts electricity
-in pencils and lubricant
-oxidizing agent
3) Fullerene
-C60 - icosahedrons = soccer ball
- delocalized in nature of graphite
-carbon nanotube
-very stable
-superconductor wire
Silicon
- 2nd most abundant element
-SiO2 (silica) , silicate substances
-having diamond lattice
-Does not dissolve in any acids (except HF)
-dissolve in base
Compounds
-Oxides
polymeric tetrahedral
-Silicate
polymorph , emerald, diopside, asbestos , mica
-Silicon Halides
-Aluminisilicate
Feldspar, zeolite
Fire work
-Silicate Glass
Soft, hard, flint, jena, pyrex, crookes's , quartz ,ground, reinforces
-Silicones
Tin
Allotrope
- alpha, beta, gamma
-Tin -plague / tin-pest
Oxides - SnO2, SnO
Halides - SnCL4
soluble both water and organic solvent
Sulfide - mono (SnS) , disulphide (SnS2)
Pb
-mineral galena, PbS
-high density but soft with low bp
-high luster, ductile , highly malleable
-resists corrosive
Oxides - PbO, PbO2 , Pb3O4
Halide - Pb (II) more stable than Pb (IV)

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Thank you Dr for the lessons
here are my summary abut gp IVA

-innert pair efffect is non-participation of the outermost ns2 electron in chemical bonding
-stability of +2 oxidatin state is decreases while for +4 is increases.
-catenation decrease down the gp.

CARBON
-allotrope are diamond,fullerence,graphite
-showing the greatest tendency and forming stable hydrocarbon chain and rings.
=oxides exist as co2 and co,preparation  co by dehydration of formic acid or oxalic acid and reduction co2 by hot red.
preparatin co2 by rxn of acid with caco3,uses in carbonate drinking or baking soda.
=carbonate,all carbonates do not dissolves in water except in gp IVA ,have planar structure
=halides,does not go hydrolysis cause c not have d orbital,high stability high bond energy.
=carbides, ionic carbide(saline carbide),easily hydrolize
SILICON
-extraction by reducing SiO2 by coke and to obtain pure substance by reducing SiCl4 by Na or zne refining process.
=oxides known as silica,preparation by hydrolysis of SiCl4 or acidification of water glasss,dissolves in hf only not dissolves in alkali and other acid.
=silicate, structure contains tetrahedral sio4.
=aliminosilicate, 3 dimensional silicate and example is zeolite,have many type glassses like jena,quartz r ground glass
=silicones.preparation by hydrolysis of alkyl or aryl silicon halides,have 3 types-chain,disilicone,branch
=hydrides of silicone prepared by stocks reaction,can burn in air spotaneously.
TIN
-allotrope-alpha,beta,gama
=oxides,SnO2&SnO,amphoteric oxide,pure ionic oxides
=halides,SnCl4 prepared by direct heating the element,SnCl2 prepared by anyhydrous sncl2 or hydrated sncl2
=sulphide,exist as mono and disulphide,SnS obtained by passing through the H2S gas in Sn(ii) solution,SnS2 obtained by oxidation SnS
LEAD
=oxides,exist as PbO,PbO2,Pb3O4
-PbO prepared by direct reaction by elements or thermal decomposition of Pb(NO3)2 or PbCO3,amphoteric oxide
-PbO2 prepared by heating Pb(ii) solution with sodium chlorate or red lead with nitric acids
-Pb3O4(red lead) prepared by heating PbO2 or rxn Pb with oxygen.
=halides,Pb(ii) is more stable tahn Pb (iv),all halides exists in ionic form,PbBr4 and PbI4 does not exist.

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Thank you Dr for today’s class

Summary for Group IVA

-inert pair effect is non-participation of the outer most ns2 electrons in chemical bonding.

-Cartenation is the ability of an element to be bonded to one another to form long chain.

-Carbon show greatest cartenation.

CARBON

-Diamond,Graphite, Fullerene is allotropy of carbon

-Oxides *exist as CO2 and CO

-uses of CO is production of pure Ni, Hydroformylation

-uses of CO2 is fire retardant, reactant in Solvay Process

-All carbonates does not dissolves in water except from Group IA

-Halides of Carbon does not undergo hydrolysis

-Carbides is compund of (C + M)

SILICON

-High melting point boiling point

-Bluish-grey metal sheen

-Does not dissolve in any acid (except HF)

-Silica produce from Si+O2

-Silica is high purity, resistent and transparency

-uses in glass, ceramic

-Silicone produced form reaction between Si,O2,C and H

-Silicone is high thermal resistance

-uses in cosmetic, breast implant shell

TIN

-soft metal, malleable,but not ductile

-Oxides (SnO2, SnO)

-SnO is more basic than SnO2 because it has more electron.

-Halides (SnX2 is more stable than SnX4)

-Sulfide (Exist as mono and disulphide)

LEAD

-Oxide exist as PbO,PbO2,Pb3O4

-Pb3O4 or read lead is commonly used in  in painting to protect iron and steel from rusting

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NUR QISTINA IZZATI BT MOHD FITRINAZRIN POON

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NUR QISTINA IZZATI BT MOHD FITRINAZRIN POON

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Thank you for every lessons in this topic Dr. Sheela.

What I had learnt from this topic are :-
Group IVA elements consists of Carbon ,Silicon ,Germanium, Tin ,Lead.
- Carbon is non-metal
- Si and Ge is metalloid
-Sn and Pb is metal
- Tends to form ionic bonding.
- Normal oxidation number is +4
Oxidation num will become +2 down the group due to inert pair effect.
- Catenation : The tendency to catenation decrease down the group. : C showing greatest tendency .
- Reactivity increases down the group

1. CARBON

Form allotrope

Diamond , graphite, fullerene and nanocarbon.

Carbon cannot form p-pi p-pi bond because 'd' orbital does not exist.

Exist in air , igneous rock, anthracite, bituminous coal, lignite.

Properties of graphite.

Structure of C60

Can exist as CO /CO2 , preparation and uses.

Halides of carbon , CX4

Carbides.

2.  SILICON

Exist as SiO2 ( sand, quartz, flint, agate )

Extract by reducing SiO2 ( sand) by Coke.

To obtain pure Si : reducing SiCl4 by Na then undergoes zone refining process.

Silicon compounds : SiO2 prepared by hydrolysis of SiCl4 or acidification of water glass.

Silicate

Aluminosilicate.

Zeolite and Sodalite

Silicate glass and silicones

3.  TIN ,Sn

Extraction of Sn

Sn allotrope : alfa-Sn (grey) , beta -Sn ( white) , gamma-Sn

Tin-plague or tin-pest

Compounds of Sn : SnO, SnCl2 , Sulfide ( SnS and disulphide SnS2)

4. LEAD, Pb

Exist : mineral-galena, PbS

Exist as PbO, PbO2 and Pb3O4.

Oxidation num of PbO =+2 while PbO2 = +4

PbO yellow acid and is amphoteric oxide.

Preparation of PbO and PbO2

Pb3O4 is trilead tetraoxide : red lead.

Pb3O4 shows properties like PbO and PbO2.

Uses of lead compounds as pigment for paint.

Halide of Pb

Questions:
Dr. Sheela, I want to ask that if we write the chemical equation , do we compulsory to write down the state of reactant and equation ? Thank you in advanced.

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Thank you Dr.Sheela for today's lecture, here's my summary:

C(non-metal); Si, Ge(metalloid); Sn, Pb (metal)

Inert Pair Effect: non participating of outer most ns2 e-s(s orbital- better penetrating power)

Increases descending group

Preference of late p block elements to form ions (oxidation state 2< group valency)

Occurs when e-s pulled closer to nucleus -> more stable, difficult to ionize

C, Si: +4; Ge: +4 (+2); Sn: +4, +2; Pb: (+4) +2

Strength Of Covalent Bonding (decreases from Si – Pb -> tends to form ionic bonding)

M-X

X - no non bonding e-: strength decreases <- poor orbital ppi-ppi overlap orbitals (atomic size increases)

X – has non bonding e-: strength increases <- strong dpi-ppi overlap

Catenation: ability of element bonded to one another -> long chain/ ring

Tendency decreases down group -> larger size -> poor overlapping ppi-ppi orbitals

C

Allotrope: C exist in >1 (bonding)form

Diamond: covalent, sp3(no free e-), high m.p

Production

1.      Crystallization of molten magna

2.      Synthesized from graphite

Graphite: covalent, electrical conductor, acts as both oxidizing & reducing agents(form intercalation compounds)

Production - Archeson Process

Structure- stacked of 2-dimensional C sheets, arranged by layers

C bonded to C(sp3), 4th C connect layers (long -> e-s not bound -> free moving)

Fulllerene: big framework with even #C atoms

C60- bucky ball/buckmisterfullerene: stable(symmetry):

Pore inner diameter ~70A -> can accommodate small ions / molecule

C (sp2) contains C=C retains delocalized nature(graphite)

Oxides

CO: colourless (g), smelless, blue flame, strong reducing agent, acts as ligand(formation of carbonyl complexes)

Preparation

1.      Dehydration of formic acid/oxalic acid by {H2SO4}

2.      Reduction of CO2 by red hot C

Toxic-strongly bonded to hemoglobin than O2

CO2: dry ice (s), dibasic

Dissolves in water -> carbonic acid (anhydride)

React with base -> carbonate (insoluble in water except G1A carbonate)

Act as ligand

Halides

CX4

Not undergo hydrolysis <- no d orbital

CCl4 - organic solvent

CF4(l) – high bond E ->inert, high stability, non-toxic, non-corrosive, insoluble in water alcohols, HF

Carbides: C + metal

Ionic (Gi, ii, iiiA) – easily hydrolyze

Covalent (metalloid) – giant molecules

e.g. SiC(insulator), B4C(metallic): inert, hard

Interstitial (metallic): non-stoichiometric compositions, metallic properties,chemically inert, hydrolysed by steam(>870K)

C + transition metals

C adsorbed into metallic lattice interstices -> occupy holes

Si: inert but can be attacked by halogen, not dissolve in acid except HF, dissolve in base

Extraction

1.      Reducing SiO2(sand) by Coke ( electrical furnace under high temp.; must have excess SiO2 -> prevent SiC formation)

2.      Obtain pure Si

-reducing SiCl4 by Na

-zone refinining

Oxides

SiO2(silica): polymetric tetrahedral, 50% ionic, covalent macromolecule as whole(polymorph)

Zeolite

Regular size, pores, channels -> molecular sieves

Ion exchanger(water softening); if exchange with H+ -> strong acidic solid catalyst, acidic heterogeneous catalysts

Silicate Glass

Sand + metal silicate/aluminosilicate/borosilicate

supercooled liquid with very high viscosity – can’t free flow

amorphous -> no m.p

inert but attacked by F2, HF, alkali

Silicone: thermally stable, low viscosity, alkyl-> water repellent(hydrophobic), inert(chemical attack, oxidation), rubbers remain elastic at low temp.

hydrolysis -> condensation

Depends on type of initial alkyl silicone halide

1.      Disilicone – initial R3SiX

2.      Chain silicone – initial R2SiX2

3.      Branched – initial RSiX3

Silicon Halides: unstable

All SiX4 exist

Undergoes hydrolysis in water through formation of dative bonding (SiX4- O to Si)

SiF4 -> partial hydrolysis

Hydride(Silanes): gas, volatile liquid, burn in air, hydrolysis in water & alkali

Form catention

Preparation

1.      Stock’s reaction

2.      SiCl4 + LiAlH4 -> SiH4 + LiCl + AlCl3

Sn

Extraction

Cassiterite(SnO2) -roasting-> SnO2 -reduction-> Sn -purification-> -electrolysis/melting-> anode:Sn(pure); cathode: SnO2(impure Sn)-reduction with anthracite C-> Sn + 2CO

Allotrope

Tin-plague-pest: changes from beta-Sn to alpha-Sn below 13.2d.c -> increase(volume), metallic appearance becomes pock-marked->powdered

SnS2: yellow

Oxidation of SnS with ammonium polysulfides (NH4)2Sx

Dissolve in excess (NH4)2Sx

Pb

Exist as galena(PbS)

Extraction

2PbS + 2O2 -> 2SO2 + (2PbO -> + C)-> Pb + CO

Oxides

PbO(lead oxide): yellow, amphoteric

Preparation

1.      Direct reaction with O2

2.      Thermal decomposition od Pb(NO3)2 or PbCO3

PbO2(lead dioxide): dark brownish solid / black powder, strong oxidizing agent, ionic, dissolve in acids, amphoeric

Preparation

1.      Heating Pb(ii) soln with NaCl

2.      Red Pb with HNO3

Cathode in lead acid battery

Pb3O4(trilead tetraoxide): red lead

Mixture of 2PbO.PbO2

Preparation

3Pb + O2 -> Pb3O4

PbO2 -heat-> Pb3O4 + O2

Halide: ionic

Pb(ii) more stable than Pb(iv)

PbF4, PbCl4 exists: white

PbBr4, PbI4 not exist <- Br2 & I2 not strong oxidizing agents

PbBr2:white, PbI2:yellow

# data[].attributes.body
Thank you Dr for today's class and here is my summary for Group IVA

- Down the group, oxidation number +2 becomes more stable due to inert pair effect
- Carbon can form allotrope as it exists in more than one physical form

Carbon
- Allotropy: diamond, graphite and fullerene
- Properties: very stable framework due to symmetry structure
Oxides (CO and CO2)
CO
- Prepared by dehydration of formic acid by con H2SO4
- Properties: colorless gas, burned with blue flame
- Uses: production of pure Ni metal
CO2
- Prepared by reaction of acid with CaCO3
- Properties: Colorless, dissolve in H20
- Uses: Fire retardant
Halides
- Properties: inert, volatile
- Uses: Freon for refrigerating gas
Carbides
-  Easily hydrolyze
- Used in making cutting tool, disks

Silicon
Extraction : Reducing Sio2 by Coke, reducing SiCl4 by Na
Properties: high melting point
Oxides
- Prepared by hydrolysis of SiCl4
- Properties: dissolve in alkali
- Silicate, aluminosilicate and silicate glass
- Glasses; soft glass, hard glass, flint glass, jena glass
- Silicone: Disilicone, chain silicone and branched silicone
- Used as lubricants

Tin
- Allotrope: alpha, beta and gamma Sn
- Properties: soft metal, malleable
Oxides
Sno2
- Direct heating of metal in O2
- Does not dissolve in HCl , HNO3 and aqua regia
Sno2
- Prepared by heating tin oxalate
Halides
SnCl4
- Direct heating of elements
- Colorless liquid
Sulfide
SnS
- Obtained by passing through H2S gas in Sn (II) solution
- Dark brown unstable solid
SnS2
- Obtained by oxidation of SnS using (NH4)2Sx
- Yellow solid

Lead
- High density, high lustre
Oxide
PbO
- Direct reaction between elements
- Yellow solid
PbO2
- Heating Pb (II) solutionwith ClO-
- Dark brownish solid
Halide
-Pb (II) halide is more stable than Pb(IV) halide
-PbF4 and PbCl4 exists
- PbBr4 and PbI4 do not exist

# data[].attributes.body
Thank you Dr. for the pre-recorded video and today's class. This is my summary for Group IVA:

-Down the group, the oxidation number of 2+ will become more stable due to the inert pair effect of the s orbital.

-carbon can form allotrope as it can exits  in more than one physical form such as diamond, graphite, fullerene (bucky ball) and nanocarbon, etc.

-the preparation and of carbon monoxide and carbon dioxide.

-extract silicon by reducing sand by coke and reducing silicon tetrachloride by sodium

-different cation in silicate can produce different color of glass

-SnCl2 is more stable than SnCl4 because SnCl2 is in ionic compound but SnCl4 is in covalent compound due to the small size of Sn4+ and the strong polarizability of Sn4+.
However, Sn4+ is more stable than Sn2+.

-SnCl2 also a strong reducing agent (as its stable form of ions is with the oxidation number 4+)

-Pb2+ is more stable than Pb4+ due to the inert pair effect. PbCl4 is a strong oxidizing agent. Pb(II) halide is more stable than Pb(IV) halide

- Pb will form trilead tetraoxide (Pb3O4) which is red in color.

# data[].attributes.body
First of all, thank you dr for the lessons.

For the summary,
Carbon
- have eight allotropy
eg: diamond, graphite, lonsdaleite, fullerene and etc
-  diamond is use for making cutting tool/ jewellery
- graphite as electrode *can be prepared by Acheson Process
-  fullerene or bucky ball, use as absorbent in producing carbon nanotube
- have 4 compounds
- Oxides
* can exist as CO or CO2
* CO
-can be prepared by dehydration of formic acid or oxalic acid by concentrared H2SO4 or reduction of CO2 by hot-red C.
- it is a colourless gas and does not smell, burned with blue flame and a toxic gas, strong reducing agent and acts as ligand
* CO2
- can be prepared by reaction of acid with calcium carbonate or heating limestone
- it is a colourless gass and does not smell, dissolve in water, react with base, also act as ligand
- Carbonate (carbonate and hydrogen carbonate)
* does not dissolve in water, exist as resonance
- Halides
- does not undergo hydrolysis
- uses as refrigirating gas,monomer for plastic, for non sticking cooking utensils, organic solvent
- Carbide
- Salline carbide, mettaloid carbide, metallic carbide
Silicon
- Can obtained pure silicon by reducing SiCl4 by Na, or zone refining process
- does not dissolve in any acids except for HF
- dissolve in base
- Oxides
* SiO2/silica exist as polymeric tetrahedral
* prepared by hydrolysis of SiCl4 and acidification of water glass.
* Silicate, aluminosilicate, zeolite, silicate glass
*silicones
* can be prepared by hydrolysis of alkyl /aryl silicon halides followed by condensation
* have three type , disilicone, chain silicone, branched silicon.
* use as lubricant, breast implant or in cosmetics(primer)
- Halides
* all silicon halides are exist and does not stable and undergo hydrolysis except for SiF4(undergone partial hydrolysis)
- Hydrides
* form catenation
* prepared by Stock's reaction
- Tin
* it allotrope (a-Sn, B-Sn and y-Sn)
* Sn is soft metal, malleable but not very ducktile, crackles when bent, become brittle on heating
- Oxides
* SnO2 can be prepared by direct heating of Sn in air/oxygen
* amphoteric oxides (react with acid and base)
* SnO (black tin) can be prepared by heating tin oxalate
- Halides
* SnX2 is more stable than SnX4, can be prepared by direct heating of elements
- Sulfides
* exist as mono (SnS) and disulphide (SnS2)
* SnS can be obtained by passing through the H2S gas in the Sn(II) solution while SnS2 by oxidation of SnS using ammonium polysulfides
- Lead
- Oxides
* exist as PbO PbO2 and Pb3O4
* PbO can prepared by direct reaction between elements or thermal decomposition of Pb(NO3)2 or PbCO3
* PbO2 by heating Pb(II) solution with sodium chlorate or red lead with nitric acids
* Pb3O4 (trilead tetraoxide) a mixture of 2PbO.PbO2 and show properties like PbO and PbO2
- Halides
* Pb(II) halide is more stable than Pb(IV) halide
* PbF4 and PbCl4 are exist but not the rest
* while Pb(II) halides, all are exist as ionic form

# data[].attributes.body
Thank you dr for the class and this is my summary:

Group 14 elements
- The stability of +4 oxidation state decrease when down the group due to inert pair effect
- When down the group, the size increase, metallic character increase, melting point decrease, electric conductivity increase, IE decrease and catenation increase
- Catenation depends on the size of element
- Strength of covalent bond decrease when down the group

Carbon
- Allotrophy: diamond, graphite and fullerene
- Preparation, properties and use of CO and CO2
- Preparation of carbonate
- Use of halide
- Carbide: Ionic, covalent and interstitial

Silicon
- Extraction and properties
-Silicon oxide (silica)
- Preparation
- Preparation of silicate
- Type, characteristics and use of zeolite
- Silicate glass
- preparation of silicate glass
- Preparation of disilicone, chain silicone and branch silicone
- Silicon halide and silicon hydroxide

- Tin
- Extraction of tin
- Tin Allotrope and properties of Sn
- Tin oxide, tin halide and tin sulfides

- Lead
- Extraction
- oxide, halide, sulfide

# data[].attributes.body
Thnakyou dr for today's lesson.
This is my summary for Group IVA:
-Normal oxidation number is +4
-Oxidation number +2 become more stable due to inert pair effect when down the group
-valence electron is ns2 np2

CARBON
- Allotrope -diamond,graphite,fullerene,nanocarbon
-Oxides -CO & CO2
-Halides does not undergoes hydrolysis because carbon does not have d orbital
-Carbides -ionic,covalent,and interstitial

SILICON
-2nd most abundant element in the earth
-can be prepare by Hydrolysis of SiCl4 and Acidification of water glass
-Oxides -silica,silicate and aluminium silicate(Feldspar & Zeolite)
-Silicate (sand+metal silicate ,aluminosilicate,borosilicate)
-Silicones-having Si-O-Si-O bonds in chains,rings and branches
-Type of silicone is disilicone,branched silicon
-Halides-all halides exist as SiX4 and un dergoes hydrolysis in water except SiF4

TIN(Sn)
-Allotrope-Alpha-Sn,Beta-Sn,gamma-Sn
-Tin plague(change from beta Sn to alpha Sn)
-Oxide(amphoteric oxide)
-Halides (SnX2 is more stable than SnX4)
-SnX2 is strong reducing agent
-Sulfide-exists as mono and disulphide

LEAD(Pb)
-Pb(mineral galena,PbS)
-Oxide(amphoteric oxide)-exist as PbO,PbO2,Pb3O4
-halides(exist as PbX4 which is only PbF4 and PbCl4) but for PbX2 it exist for all halides
-Pb(II) halide is more stable than Pb(IV) halide

# data[].attributes.body
Thank you Dr for today’s lesson and 2 pre-recorded class. This is my summary for group IVA:

-Normal oxidation num is +4.
-Down the group, oxidation num +2 becomes more stable due to inert pair effect

-Si -> Pb tend to form ionic bonding

-Catenation- C showing the greatest tendency to form stable hydrocarbon & Si less stable to catenation due to larger size of Si

Carbon

-C allotrape (diamond, graphite (use as lubricant and act as oxidizing agent), fullerene (“bucky ball”) – truncated icosahedrons

-Oxide (ligand) - CO (toxic gas) & CO2

-Halides- does not undergo hydrolysis (C has no "d" orbital)

-Carbides- (ionic, covalent & interstitial)

Silicon

-Oxides – silica, silicate & aluminosilicate (zeolite)

-Silicate glass (sand + metal silicate, aluminosilicate, borosilicate)

-Silicones – Si-O-Si-O bonds in chains (disilicone), rings & branches

-uses as lubricants, in cosmetics,              breast implant shell and etc

-Halides- all halides exist as SiX4- undergo hydrolysis in water except SiF4

Tin (Sn)

-SnO2 -> roasting -> pure tin ore(SnO2)

-Sn -> electrolysis -> SnO2(anode) &     Sn(cathode)

-Sn allotrape (alpha-Sn, beta-Sn & gamma-Sn)

-Tin-plague (change from beta-Sn to alpha-Sn)

-Oxide (amphoteric oxide)

-SnO2 (white tin) does not dissolve in   HCl, HNO3 & aqua regia

-SnO (black tin) more base than SnO2

-Halides (SnX2 is more stable than SnX4) - SnC2 – strong reducing agent

-Sulfide - exist as mono (SnS- can easily oxidize to SnS2) & disulphide (SnS2)
Lead (Pb)

-Pb (mineral-galena, PbS)

-Oxide (amphoteric oxide) (exists as PbO(yellow) , PbO2(brownish or black) & Pb3O4(red))

-Halides (PbX4- PbF4 & PbCl4 exist) (PbX2- all halides exist) –

-Pb(II) halide is more stable than Pb(IV) halide

# data[].attributes.body
Thank you so much for the lessons, Dr. Sheela. Here is my summary:

C, Si: +4

Ge: +4 (+2 unstable)

Sn: +4, +2

Pb: +2 (+4 unstable)

Oxidation number: +4 —> +2 (inert pair effect)

Strength of covalent bonding (M-X)

- no unpaired e = strength decreases

- has unpaired e = strength increases(C->Si), strength decreases(Sn->Pb)

Catenation

- decreases down the group

- C good overlapping p(pi)-p(pi) orbitals

- Si poor overlapping p(pi)-p(pi) orbitals (larger size than C)

Chemical properties (reactivity increases down the group)

- O2 —> oxides

- S —> sulphide

- Halide

- Acid (cold, no reaction), (hot has reaction)

- Alkali —> [MO3]2- & H2 (except C)

- Metal

- C —> carbide

- Si —> silicides

- Ge, Sn, Pb —> alloy

Carbon

Allotropy

1. Diamond

2. Graphite

3. Fullerene

Oxides

1. Carbon monoxide, CO

2. Carbon dioxide, CO2

Carbonate

1. Carbonate - CO32-

2. Hydrogen carbonate/ bicarbonate - HCO3

Carbide

1. Ionic carbide (saline carbide)

2. Covalent carbide (metalloid carbide)

3. Laterstitial carbide (metallic carbide)

Halide (CX4)

1. CF4 - gas

2. CCl4 & CBr4 - liquid

3. CI4 - solid

Silicon

Allotropy

1. Sand

2. Flint

3. Quartz

4. Agate

Oxides

1. Silicon dioxide / silica (SiO2)

2. Silicate (SiO4)4-

3. Aluminosilicate

Type of glass

- Soft glass

- Hard glass

- Flint glass

- Jena glass

- Pyrex/Corning glass

- Crooke’s glass

- Quartz glass

- Ground glass

- Reinforced glass

Silicones

1. Disilicone

2. Chain silicone

3. Branched silicone

Halides (SiX4) - unstable (except SiF4)

Hydrides (silanes) - form catenation

Tin

Allotropy

1. Alpha-Sn (grey)

2. Beta-Sn (white)

3. Gama-Sn

Oxides

1. SnO2 (+4)

2. SnO (+2)

Halides (SnX2 is more stable than SnX4)

1. SnCl4

2. SnCl2

Sulfide

1. SnS

2. SnS2

Lead

Oxide

1. PbO

2. PbO2

3. Pb3O4

Halide [Pb(II) is more stable than Pb(IV)]

1. PbX4

2. PbX2

QUESTION :
What beaker(component) should we use to handle HF acid?

# data[].attributes.body
Thank you dr for the class and here are summary of group IVA
CARBON
Allotropes:
- diamond, graphite, fullerence
Diamond
-produced from crystallization of molten magma in earth crust
-made up of carbon atoms bonded by covalent bond
- high melting point (4000C)
-  each carbon atom bonded to 4 other carbon having sp3 hybridization
- use as cutting tool and jewelry
Graphite
- prepared by Acheson process
- made up of stacked 2d carbon sheets
- each carbon atom bonded to 3 carbon atoms and arrange in layer
- the 4th bond used tu connect the layer
- soft, conduct electricity and use as lubricant
Fullerene
- also known as bucky ball / buckmisterfullerene
- consist of big carbon framework consisting even number of carbon
- Carbon has sp2 containing 30 C=C
- produce carbon nanotubes
Compounds
- Oxides: CO2 and CO
- preparation: dehydration of formic acid by con H2SO4 or reduction of CO2 by hot-red
-property of CO: colorless gas, burned with blue flames and toxic gas
- usage: production of pure Ni metal, produce higher alcohol, reagent to produce phosgene
- property CO2: colorless gas, solid phase call dry ice, dissolve in water, act as ligand
- usage: fire retardant, produce carbonated drink and baking soda
- preparation CO2: reaction of acid with calcium carbonate, heating limestone
- Halide: not undergo hydrolysis because Carbon has no d orbital
Examples: carbon tetrachloride and perfluoroslkyl
Usage: freon (refrigerating gas), PTFE (non/sticking utensils)
- Carbide: carbon+metal
- ionic carbide: carbon+metal group iA, iiA, iiiA
-covalent carbide: metalloid carbide (SiC, B4C)
- interstitial carbide: metallic carbides
Silicone
- extraction: reducing SiO2, reducing SiCl4 by Na, zone refining process
- characteristic: high melting point, not dissolve in acid except HF, dissolve in base
COMPOUNDS
- Oxides: silicone dioxide(silica)
- exist as polymeric tetrahedral
- Si-O is half ionic due ti difference in electronegativity but covalent as whole molecule
- preparation: hydrolysis of SiCl4, acidification of water glass
- characteristic: inert at low temperature, dissolve in HF and alkali
- Silicate: SiO2 + metal oxide/sulphate/carbonate
-structure: polymorph, contain tetrahedral SiO4 bt Si-O-Si bonds
-samples: diopside, asbestos, mica
- Aluminosilicate: 3 dimensional silicate, occurs when Al substitute with Si in silicate
- examples: feldspar, zeolite
- Silicate glass: sand+ metal silicate alumminosilicate
- characteristic: not true solid, supercool liquid and amorphous
-Type glass: soft glass, hard glass, flint glass, jena glass
- Silicone: organosilicon compounds that have Si-O-Si-O bonds
Preparation: hydrolysis of aryl/alkyl silicone halides and condensation
-type: disilicone(R2SiX), chain silicone (R2SiX2), branched silicone (RSiX3)
-properties: thermally stable, low viscosity
- usage: lubricant, breast implant shell
- Silicon Halides
- all halides except SiF4 sre unstable and undergo hydrolysis in water
- hydrolysis occur through formation dative bonding
- Silanes
- preparation: Stock’s reaction
- properties: exist in the form gas and volatile liquid, burn in air
TIN
- extraction: from roasting cassitserite to get pure tin ore then reduction to get Sn and undergo electrolysis
- type: alpha, beta and gamma Sn
-physicochemical properties: soft metal, malleable but not very ductile
COMPOUNDS
- Oxides: SnO2, SnO
-SnO2: pure ionic oxide, not dissolve in HCl , HNO3, aqua regia. Also amphoteric oxide
- SnO: oxidation no. +2, referred as black tin, amphoteric oxide but more base than SnO2
- Halides: stability SnX2>SnX4
- SnCl4: preparation by direct heating
- properties: covalent liquid, colorless and covalent compounds
- Sulfide: SnS and SnS2
-SnS: dark brown unstable solid, easily oxide to SnS2,
- SnS2: yellow solid, dissolve in excess aluminum polysulfide
LEAD, Pb
- properties: high density, high luster, ductile and highly malleable
COMPOUND
- Oxide: PbO, PbO2, Pb3O4
- PbO: preparation by direct reaction between elements, thermal decomposition
- yellow solid and amphoteric oxide
- PbO2: preparation by heating Pb2+ with ClO- and reaction read lead with HNO3
- dark brownish solid or black powder, strong oxidizing agent, amphoteric oxide
- Pb3O4: red lead, mixture of 2PbO.PbO2
- preparation: excess lead react with oxygen or direct heating
-usage: red paint
* my question is, if we direct heat alpha-Sn with 232C heat, will it directly turn to liquid Sn or it still change from beta, gamma then turn to liquid Sn

# data[].attributes.body
Summary for group IVA :
-normal oxidation number is +4
-down the group oxidation number +2 become more stable due to inert pair effect.
-down the group reactivity increases while the tendency to catenation decrease.

Carbon
-carbon oxides can prepare by dehydration of formic acid by conc. H2SO4 and reduction of CO2 by hot red C.
-all carbonates cannot dissolve in water except carbonate from group IA.
-halides of carbon cannot undergo hydrolysis because C has no d orbital.

Silicon
-the extraction of Si are reducing SiO2 by coke, reducing SiCl4 by Na and process of zone refining.
-silicon dioxide exist as polymeric tetrahedral.
-silicon dioxide can be prepared by hydrolysis of SiCl4 and acidification of water glass.
-Silicate
SiO2 + metal oxides/metal sulphate/metal carbonate
-Silicones
*organo silicon compounds having Si-O-Si bond in chains, branch and rings.
*can prepare by hydrolysis of alkyl/aryl silicon halides.

Tin
-can extract by electrolysis
-SnO2 and SnO is amphoteric oxide.
-SnO2 more base because it is more lewis basic and has more electron.
For halides, SnX2 is more stable than SnX4.

Lead
-exist as mineral-galena, PbS
-PbO is white solid, PbO2 is black powder and Pb3O4 is red lead.
-Pb(II) halide more stable than Pb(IV) halide.
-All halide exist in ionic form.

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

Carbon

Summary Group IVA:
- has valance electron ns2 np2
- oxidation number +2 down the group become more stable due to inert pair effect while for +4 decrease down the group
- Inert pair effect : for oxidation number +4 to +2

-Allotrope:
: C (diamond, graphite, fullerence, nanocarbon)
: Sn (alpha-Sn, beta-Sn)

-Strength of covalent bonding:
: no non-bonding electron-decrease down the group
: has non-bonding electron-increase (C --> Si), decrease (Sn --> Pb)

Catenation
-decrease down the group
-C has greatest tendency and form stable hydrocarbon (good overlapping ppi-ppi orbital)
-Si less stable (poor ppi-ppi overlapping-bcs large size)

Chemical properties
-reactivity increase down the group
-oxygen ( oxides )
-sulphide ( sulphides )
-halides
-Acid (cold, no rxn) (hot, has rxn)
-alkali, OH-  --> (MO3)2- and H2
-metal
C: carbides
Si: silicides
Ge, Sn, Pb: alloy (strong)

Oxides
CO
Preparation:
1. Dehydration formic acid by H2SO4
2. Reduction CO2 by hot-red
CO2
Preparation:
1. Rxn acid with calcium carbonate

Carbonates
- has carbonate and hydrogen carbonates
-does not dissolve in water execpt carbonate from grop IA

Halides
- does not undergo hydrolysis
- CF4: high stability and inertness due to high bond energy
- Freon: refrigerating gas
- Perflurovinilchloride: making plastics
- Polytetrafluoroethene: non stick cooking utensil

Carbides
- C+Metal
: ionic carbides (saline carbides)
: covalent carbides (metalloid carbides)
: interstitial carbides (metallic carbides)

Silicon (Si)

Existance
- SiO2 (sand, quartz, flint, agate)

Extraction
1. Reducing SiO2 (sand)  by Coke
2. To obtain pure Si
: reducing SiCl4 by Na
: refining process

Characteristics
-crystalline -> metallic structure adn grayish color
-diamond lattice
-high melting point
- not dissolve in any acid excpt HF, dissolve in  base

Oxides
-silicon oxcides, SiO2 (silica)
Preparation:
1. Hydrlysis of SiCl4
2. Acidificaton water glass

Silicate, (SiO4)2-
: + metal oxides / metal sulphates / metal carbonates
: structure, polymorph

Auminosilicate
: Al substitute Si in silicate framework
: negatively charge
: eg (feldspar, zeolite)

Silicate glass
- sand + metal silicate / aluminosilicate / borosilicate
Characteristic:
-not  true solid
-supercooled liquid, high viscosity
-no melting point
-inert
Production:
1. mixture calsium silicate and sodium silicate
Type:
- Hard glass
- Soft glass
- Flint glass
- Jena glass
- Pyrex / corning glass
- Crooke's glass
- Quartz glass
- Groung glass
- Reinforced glass

Silicones
- Organo silicon compound contain heterocatenated Si-O-Si-O bonds
Preparation:
1. Hydrolysis of alkyl / aryl silicon halides -> followed by condensation
Types:
- Disilicone, R3SiX
- Chains silicone, R2SiX2
- Branched silicone, RSiX3

Silicon Halides, SiX4
- except SiF4, all halides unstable and undergo hydrolysis in water easily
: SiF4 undergo partial hydolysis
- hydolysis occur -> formation dative bonding from O of water to Si of SiX4
- form catenation
Preparation :
1. Stock's reaction
2. SiCl4 + LiAlH4 ---> SiH +LiCl + AlCl3
Properties:
-exist in gas form
- butn in air spontaneously
-hydrolysis in water and alkali

Tin (Sn) & Lead (Pb)

Tin, Sn
Tin allotrope:
- alpha-Sn (grey) , beta-Sn (white) , gamma-Sn
: transformation temp. between allotropes
- Tin-Plague / tin-pest
: change from white (beta-Sn) to grey (alpha-Sn)

Physicochemical properties
- Soft, melleable, not nery ductile, brittles on heating, crackles when bent

Chemical prop.
1. O2
: form SnO2 on heating
2. Water / steam
: forms little H2 at high temp.
3. Chlorine
: forms SnCl4 on heating
4. Sulphur
: forms SnS / SnS2 depends on temp.
5. Hot conc. / molten alkalis
: forms H2 and Sn(OH)4,2-
6. Diluted acids
: very slow
7. conc. H2SO4
: forms Sn(SO4)2
8. conc. HCl
: forms hydrated SnCl2
9. conc. HNO3
; forms hydrated SnO2

Oxides (SnO2, SnO)
SnO2
- Direct heating in air / oxygen
pure ionic oxides
- not dissolves in HCl, HNO3 / aqua regia
- Amphoteric oxides
: H2So4
: OH-
SnO
- black tin
- Preparation
: Heating tin oxalate
- Amphoteric oxides

Halides
SnCl4
Preparation:
1. direct heating
- Colorless liquid
- Covalent compund
- In moist air, rapidly hydrolyzed and fuming
- rxn with conc. HCl / NH4Cl, form complex SnCl6, 2-
SnCl2
Preparation:
1. Anhydrous SnCl2
2. Hydrated SnCl2.2H2O
- Predominant covalent compound
- Soluble in wates & organic solvents
- Anhydrous salt is transparent crystaline solid
- Dissolved in waater
- Strong reducing agent

Sulfides
- Exist as mono (SnS) & disulphide (SnS2)
SnS
- Obtained by passing through H2S gas in Sn(II) sltn.
- Dark brown unstable solid
- easily oxidized to SnS2
SnS2
- Obtain by oxidation of SnS using ammonium polysulfides
- Yellow solid
- Dissolved in excess of (NH4)2Sx

Lead, Pb
- mineral-galena, PbS

Physicochemical properties
- High density, soft, low boiling point
- High luster, ductile & hugh melleable
- Resist corrosive

Oxides
- PbO, PbO2 & Pb3O4
PbO : Lead oxides
Preparaton:
1. Direct reaction
2. Thermal decomposition Pb(NO3)2 / PbCO3
- Yellow solid
- Amphoteric oxides
PbO2
Preparation:
1. heating Pb(II) sltn with sodium chlorate
2. Red lead with nitric acids
- Dark brownish / black powder
- Strong oxidizing agent
- Ionis compound
- Dissolves in acids
- Decompose when heating
- Amphoteric oxides
Pb3O4
- Red lead
- Mixture of 2PbO.PbO2
- Sjow prperties like PbO and PbO2

Halides
- Pb(II) halides more stable than Pb(IV) halide
PbX4
- PbF4 & PbCl4 exists
- PbBr4 & PbI4 does not exist --> not strong oxidizing agent
PbX2
- All halides exist in ionic form

# data[].attributes.body
Summary of Group IVA
- stability of oxidations states of +4 decrease down the group while stability of oxidations states of +2 increase down the group.

- Catenation: ability of an element atoms to be bonded with each other to form a long chain or a ring.
- C has the highest catenation as I has good overlapping pπ-pπ orbital.

- Allotrope: an element that can exists in more than one physical form.

**Carbon**
- C can react with O2, S, Br2, I2 and acid.

- We studied three physical form of C: diamond, graphite and fullerene and their specific properties

- C compounds: halides, oxide, and carbide and each of them have their specific properties.

**Silicon**
- silicon compounds: oxides, silicate, aluminosilicate, silicones, halides and hydrides and each of them have their own specific properties.

- types of glass: soft glass, hard glass, Pyrex, flint glass, quartz glass and so on

**Tin**
- it has many transformation: alpha, beta, gamma...

- compounds:  oxides, halides and sulfide

**Lead**
- Pb2+ more stable than Pb4+ due to inert pair effect.

- compounds: oxides and halides

# data[].attributes.body
Carbon, C
Allotropy: 1, 2, 3
1. Diamond
-synthesized by graphite
-covalent bond
-very high melting point
-sp3 hybridization

2. Graphite
-prepared by Acheson process with SiO2 + C
-sp2 hybridization
-stacked of 2D carbon sheets
-1 pi bond is free to move through layers & connect the layers (van der waals force)
-soft, conduct electricity
-used in pencils & lubricant (layers can slide over each other)
-reducing & oxidizing agent --> form intercalation compound

3. Fullerene
-even numbers of C
-most symmetry: C60 aka bucky ball
:sp2 hybridization
:contains of 30 C=C bonda
:synthesized by graphite by laser / electrical arc and benzene
:used in carbon nanotube
:very stable
:K3C60 3D superconductor

4. Carbon compound
OXIDES
-CO - toxic gas because can bond to hemoglobin strongly
-strong reducing agent            CO --> CO2
-act as ligand
-CO2 - anhydride acid
-dissociation of H2CO3 in water (dibasic acid)
CARBONATE
-only Group IA carbonate is soluble in water
HALIDES
-no hydrolysis as no d orbital
-CF4: inert, very stable due to high bond energy
CARBIDES
-Ionic carbides (saline carbide)
:C + metal (IA, IIA, IIIA)
-Covalent carbides (metalloid carbides)
:C + Si/C
:giant molecules
:very inert and hard
-Interstitial carbides (metallic carbides)
:non-stoichiometric composition
:very hard but brittle

Silicon, Si
1. Silica, SiO2
-aka silicon dioxide
-covalent but exhibit ionic properties (very different in electronegativity)
-inert at low temp, reactive when temp elavates

2. Silicate, (SiO4)4-
-SiO2 + m oxides / m sulphate / m carbonate
-Aluminosilicate: 3D silicate
-Examples: feldspar, zeolite
:regular pore size
:molecular sieve
:ion exchanger
:acidic heterogenous catalyst
-silicate glass
:soft glass, hard glass, flint glass, jena glass, pyrex / corning glass, crooke's glass, quartz glass, ground glass, reinforced glass

3. Silicone
-S + C/H/O
-heterocatenated SI-O-Si-O bonds in chains, rings and branches
-Disilicone: initial R3SiX
Chain silicone: initial R2SiX2
Branched silicone: initial RSiX3

4. Halides, SiX4
-unstable and undergo hydrolysis in water (except SiF4)
-formation of dative bond

5. Hydrides
-form catenation up to Si6H14
-exist in gas form and volatile liquid

Tin, Sn
1. Oxides
-SnO2 (Sn4+)
:insoluble in HCl, HNO3, aqua regia
:amphoteric oxide
-SnO (Sn2+)
:amphoteric oxide (more base than SnO2
:more lewis basic because having more e-

2. Halides
-SnX2 is more stable than SnX4
-covalent compound but exhibits ionic properties

3. Sulfide
-monosulphide (SnS)
-disulphide (SnS2) more stable

Lead, Pb
1. Oxides (amphoteric)
-PbO (Pb2+) yellow
-PbO2 (Pb4+) dark brownish/black
-Pb3O4 (Pb4+) red
:used in paint

2. Halides
-Pb(II) more stable than Pb(IV)
-only PbF4 & PbCl4 exist

QUESTION:
1.Since SnX2 is more stable than SnX4, does it mean that Sn2+ is more stable than Sn4+?
2. If Sn2+ is more stable than Sn4+, why is Sn halides a reducing agent? Isn't it an oxidizing agent since it tends to exist in the form of Sn2+ rather than Sn4+?

# data[].attributes.body
Group IVA
1)normal oxidation +4
Down gp oxidation no +2 that's mean more stable because inert pair effect.
2)form allotrope
⚪Carbon has diamond, graphite, fullerene and nanocarbon
⚪Tin has a-Sn, B-Sn
2)Strength Covalent bonding M-X
⚪DECREASE
X for No non bonding (no unpaired e)bcs poor orbital p-p
⚪X for has non bonding (has unpaired e)
INCREASE (C-Si) strong d-p overlap
DECREASE(Si-Pb) metallic character
4)Catenation?
Element bonded to one another FORM LONG CHAIN OR RING
⚪decrease down gp
⚪Carbon, great tendency,great P-p
overlap
⚪Silicon, less stable because larger Si, weak p-p overlap
5)REACTIVITY Increase down gp

ELEMENT CARBON

1)Diamond in earth crust from crystallization molten magna.
Synthesized from graphite
(covalent, high mp, sp3, not conduct electric in molten n solid bcs no free e means all valence e used in covalent bond)
2)Graphite (Acheson Process high temp electrical furnace)
Soft, conduct electric, lubricant, oxidising agent /reducing agent
3)Fullerane
C60 : sp2,, from graphite, superconducter wire
4)Compound
⚪Oxides CO2 and CO
⚪Carbonate
⚪Halides

CCl4, CBr4 are liquid

CF4(gas)

Cl4 (solid)

⚪Carbides

ionic carbide (C + M(IA,IIA,IIA))

covalent carbide (SiC and B4C)

Interstitial Carbides

ELEMENT SILICON

A) silicon (Si)

⚪Extract

1)Reducing SiO2 by Coke in     electrical furnace (high temp)
+
excess Si (prevent SiC formed)
2)Obtain Pure Si
i) Reducing SiCl4 by Na
ii) zone refining process
⚪Metallic luster, grayish color, high mp, inert when attacked by halogen, doesn't dissolve in acid but dissolve in HF, dissolve in base
⚪Silicon Oxides = Silica
B) SILICATE (SiO4)4-
⚪SiO2+metal Oxides /sulphate)/carbonate
⚪Polymorph structure
⚪Aluminisilicate(3D silicate, negatively charge, neutralised by cation gp IA, IIA)
-Feldspar
-Zeolite (detergent softener, separate gases,)
⚪Silicate glass [not true solid, supercooled liquid, no mp mean amorphous, heating soften, turn semisolid to clear liquid, inert( when attacked F2, HF, alkali).  ]
Soda glass form mix CaSiO3

C) SILICONES
⚪organosilicon
Si-O-Si-O (chain, rings, branches)
⚪Prepared by
1)Hydrolysis of alkyl /aryl halides followed
2)Condensation
⚪Types of silicone

Dislicone silicone  - R3SiX

Chain silicone - R2SiX2

Branched silicone RSiX3

Uses as lubricant,cosmetic, breast implant, silicone wax for car

⚪Compound
1)Silicon halides  EXC SIF3- unstable, and hydrolysis in water
2)hydride silicon(silanes) form Catenation
-Prepare stock's reaction  then
fractional distillation to separate Silanes

ELEMENT TIN (SN)

⚪Extract
1)roasting SnO2(impurities S,As)
2)reduction of SnO2 by C to Sn
3)purification Of Sn
- by electrolysis or melting
Sn pure in cathode
SnO2 impure in Anode
⚪Tin allotrope

a-Sn greyish diamond lattice, powder  (132.2c)

>B-Sn white, tetragonal, metallic structure (161c)

>y-Sn (232c)

>liquid Sn

⚪Compund of Sn
A) OXIDES
SnO2(+r4)
SnO(+2)
B)HALIDES
SnCl2(+2) more stable than SnCl4(+4)
C)SULPHIDE
SnS - dark brown
SnS2 - yellow

ELEMENT LEAD Pb

⚪Mineral galena, PbS
⚪Extract 1)roast PbS by CO2
2) C added
⚪Compund
A) OXIDE
-PbO (+2), yellow
-PbO2(+4)
brownish solid, black powder
-Pb3O4(mixture 2PbO. PbO2)
Uses of Red lead, red pigment in paint:
protect iron and steel from rusting
B) HALIDE
Pb(II) halide more stable
than Pb(IV) halide

# data[].attributes.body
Summary group IVA
-Oxidation number is +4 but +2 more stable down the group due to Inert pair effect
Catenation - form long chain
-tendency decrease down the group
Carbon
-diamond-graphite-fullerene
Oxides
-CO-colourless, toxic. strong reducing agent
-use in production of pure Ni
-Hydroformylation
CO2
-colorless,
use in fire retardant
use in production of carbonated drinks
Halide-inert, thermally stable liquid, insoluble in water but dissolve in chlorocarbon
CCl4
CF4
Carbides-Lustrous solid, high MP chemically inert
Mn4C,TaC, Cr3C2

Silicon (sand, quartz , flint)
-metallic luster
-high MP not dissolved in acids except HF
Oxides
-SiO2(silica)
inert, but reactive at elevated temperature
(SiO4)4- (silicate)
Aluminosilicate
-Feldspar
-Zeolite -use as water softener and separation of gases
Silicate Glass
-not true solid
-no MP
-inert by most chemical but attack by F2,HF and alkali
Silicone
-silicon compound heterocatenated Si-O-Si-O bond in chains, rings and branches
1)disilicone (R3SiX)
2)chain silicone (R2SiX2)
3) branched silicon (RSiX3)
use as lubricant , low temperature hydraulic fluid and breast implants

silicon Halide SiX4
Hydrides (Silanes)
-volatile liquid
-burn in air spontaneously

Tin ,Sn
Oxide
-SnO2 - ionic, not dissolve HCL, HNO3 and Aqua Regia, Amphoteric
-SnO(black tin) - amphoteric, more base than SnO2

Halide
-SnCl4-colorless, covalent compound , rapid hydrolyzed and fuming in presence of moist air
-SnCl2 -soluble in water and organic solvent , covalent compound

Sulphide
-SnS -dark brown, easily to oxide to SnS2
-SnS2 -yellow solid -dissolve in (NH4)Sx

Lead , Pb

oxide
-PbO -yellow, amphoteric oxide
PbO2 - dark brown/black
- strong oxidizing agent
- ionic compound
- decompose when heated
- dissolved in acids
- amphoteric
Pb3O4- red
- mixture of 2Pbo.PbO2
-uses of pigment for paint

Halide
PbX4
-PbF4 and Pbcl4
PbBr4 and PbI4 not exist as Br and I not strong oxidizing agent
PbX2
-PbBr2, PbI2, PbF2, PbCl2

# data[].attributes.body
Thank you Dr for today's lesson and pre-recorded class. Here are my summary for Group IVA :

- Normal oxidation is +4 but going down the group it will be +2 due to inert pair effect.
- Covalent bonding decrease from Si to Pb as it tends to form ionic bonding due to increase in metallic character.
-Going down the group , the tendency to catenation decrease .

Carbon

Carbon Allotrope :-

Diamond

Graphite

Fullurene

Oxides :
-Exist as CO2 and CO
-CO - Toxic , colourless and does not smell gas .
-CO2-colourless gas and does not smell and an hydride acid when dissolve in water.
Carbonate :
- Structure of C is sp2 and exist as resonance.
Halides :
- Does not undergo hydrolysis due to C has no d-orbital to receive electron from water.
Carbides :

Ionic Carbide- easy to hydrolyze

Covalent carbide - giant molecules

Interstitial carbide -non-stoichiometric composition.

Silicon

- Exists as SiO and silicate substances
- Extraction

1. Reducing SiO2 by Coke

2. To obtain pure Si

Reducing SiCl4 by Na

Zone refining process

- Characteristic - metallic luster and grayish colour, have diamond lattice , high melting point, does not dissolve in acids except HF .
Oxides :
-Exists as polymeric tetrahedral SiO2
-Strong acidic oxide.
- Silicate, Aluminosilicate ( Feldspar and Zeolite) , Silicate glass and silicones.
Halides :
- Unstable and undergo hydrolysis except SiF4.
- Silanes

Tin
-Extraction : Reduction of Tin Ore with anthracite.
-Tin allotrope :-

Alpha-Sn

Beta-Sn

Gamma-Sn

Liquid Sn

Oxides :
-Exist in SnO2 and SnO
SnO2 - pure ionic oxide , does not dissolve in HCl , HNO3 or aqua regia
SnO- referred as black tin , amphoteric oxides but more Lewis basic .
Halides :
- Exist in SnX2 and SnX4 ( SnX2 is more stable than SnX4)
SnCl4- colourless liquid , covalent compound with tetrahedral
SnCl2 - covalent compound , soluble in water and organic solvent.
Sulfides :
-Exist as mono, SnS and disulphate, SnS2.
SnS- dark bown in colour , unstable solid , easily oxidize to SnS2,
SnS2 - yellow solid .

Lead

- Exist as mineral (galena , PbS)
- High density , soft and low boiling point .
Oxides :
- Exist as PbO, PbO2, Pb3O4
PbO - yellow solid
PbO2 - dark brown solid / black poweder , ionic compound , strong oxidizing agent , dissolves in acids.
Pb3O4 - red lead
Halide :
- Pb(II) halide is more stable than Pb(IV)
- Exists in PbF4 and PbCl4
- Ionic form

# data[].attributes.body
Group IVA
- non-metal to metal down the group
- oxidation number changes to +4 to +2 (inert pair effect)
- inert pair effect : preference of late p-block to form ions with oxidation states 2 less than the valence
- Allotrope: element that can exist in more than 1 form
- C = Diamond, graphite, fullerene, nanocarbon
- Catenation: ability to be bonded in a long chain or ring

- C -> great tendency, Si -> less stable. (poor pπ overlapping - large size)
- Increased reactivity going down
- Form compounds: oxides, sulphides, halides.

Carbon
- Many allotropes (eg. diamond, fullerene, graphite)
- Diamond: bonded by covalents, high mp, each C bond with other 4 C, no free e⁻. uses: precious jewelry, cutting tool
- Graphite: prepared by Acheson Process, 2-D C sheets, soft (weak bonds between layers), conducts electricity, oxidizing agent
- Fullerene: big C framework of even numbers, aka. bucky ball, truncated icosahedrons = soccer ball (C₆₀), very stable, similar reaction to alkenes
-Oxides: CO₂ & CO.
CO prep: dehydration of formic acid or oxalic acid by conc. H₂SO₄, reduction of CO₂. Prop.: colorless & scentless, burn with blue flame, toxic, strong reducing agent, ligand. Uses: prod. of pure Ni metal, steam reforming process, reagent to prod. phosgene
CO₂ prep.: react acid with calcium carbonate, heat limestone. Prop.: colorless & scentless, solid = dry ice, dissolve in H₂O = H₂CO₃, react with base = carbonate, ligand. Uses: fire retardant, Solvay process, prod. carbonated drinks & baking soda, carbon cycle-biofuel
CO₃ ²⁻ & HCO₃⁻ : insoluble except group IA, planar C, resonance.
- Halides: not go hydrolysis because no d-orbital. CCl4: organic solvent, CF4: Freon, F₂C=CFCl, PTFE
- Carbides: C + Metal,
ionic: IA, IIA & IIIA, easily hydrolyzed.
covalent: Si & B, giant molecules, inert & hard, cutting tool, SiC insulator B₄C metallic.
interstitial: transition metals, C absorbed into metallic lattices, lustrous solids, high mp, hard but brittle, inert

Silicon
- exist as compound
- extraction: reduce SiO₂, reduce SiCl₄ by Na, zone refining process.
- metallic luster & grayish color, diamond lattice, high mp, inert element except with halogen, dissolves in HF & bases
- oxides: SiO2. Prep.: hydrolysis of SiCl4, acidification of water glass. Char.: inert at low temp., strong acidic oxide at elevated temp., dissolve in alkali
- (SiO₄)⁴⁻: SiO₂ + M oxides/sulphates/carbonates. struc.: polymorph
- Aluminosilicate: 3D silicate, Al subs. Si in silicate framework (becomes -tive, balanced by cations). eg.: feldspar, zeolite.
Zeolite: regular size of pores, molecular sieves, ion exchanger
- Silicate glass: not true solid (supercooled liquid), no mp (amorphous)
Types of glass: flint, pyrex, crooke, quartz, ground, reinforced
- Silicones: organosilicon compounds. Prep.: hydrolysis of alkyl/aryl silicon halides followed by condensation
Types: Disilicone (R₃SiX), Chain (R₂SiX), Branched (RSiX₃).
Prop.: thermally stable, low viscosity, silicone rubbers, hydrophobic (alkyl groups)
Uses: lubricants, low temp. hydraulic fluids, cosmetics, breast implants, wax
- Halides: all SiX₄. all unstable except SiF₄ (partial hydrolysis)
- Hydrides: form catenations. Prep.: Stock's reaction, separated by fractional distillation.
Prop.: exist in gas & volatile liquids, burns spontaneously, hydrolyze in water and alkali

Tin
- Extraction from cassitserite
- Allotrope: alpha, beta, gamma (changes with temp.)
- Prop.: soft metal, malleable, not very ductile, brittle when heated, crackles when bent. reacts with oxygen, water, chlorine, sulphur, hot/conc./molten alkalis, conc. acids.
- Oxides: SnO₂, SnO
SnO₂: prep. direct heat. ionic oxide. does not dissolve in acids, amphoteric.
SnO: prep. heating tin oxalate. more amphoteric than SnO₂.
- Halides: SnX₂ > SnX₄
SnCl₄: prep.: direct heating, colorless, covalent compound, hydrolyze and fumes rapidly in moist air, forms complex SnCl₆ ²⁻ with conc. HCl/NH₄Cl
SnCl2: covalent compound, soluble in both, prep. differs with anhydrous and hydrated.
Anhydrous is transparent crystalline. soluble, strong reducing agent.
- Sulfide: exists as mono or di, mono: prep. pass H₂S in Sn(II) solution, dark brown unstable solid, easily oxidize to SnS2
di: prep.: oxidation of mono, yellow solid, dissolve in excess (NH₄)₂Sx

Lead
- exist as galena, extract by roasting followed by reacting with C, prop.: high density but soft & low bp, high lister, ductile & malleable, resist corrosion
- Oxides: PbO, PbO₂, Pb₃O₄
PbO: prep. direct reaction, thermal decomposition of Pb(NO₃)₂ or PbCO₃. yellow solid. amphoteric.
PbO₂: prep. heat Pb(II) solution with sodium chlorate, red lead with nitric acid. prop.: dark brownish solid or black powder, strong oxidizing agent, ionic compound, decompose when heated, dissolves in acid, amphoteric. uses: cathode in lead acid battery
Pb3O4: red lead, mixture of 2PbO.PbO₂, shows properties of both. Uses: red paint pigments
- Halide: PbF₄ & PbCl₄ exists (others are not strong oxidizing agents). all PbX₂ exists

# data[].attributes.body
My summary for group IV are
-Inert pair effect appearent from chemistry of group II and group IV
-Group IV tend to form oxidation state +4
-Allotrotype
o Carbon -diamond ,graphite, fullerene
o Tin - alpha Sn , beta Sn
-Cantenation
ability element to beb bonded to one another to form long chain
-Trend in chemical properties
1.Reactivity increases down the group
2.Form compound with oxygen, sulphide
3. Reaction with acid
-no reaction if react with hydrochloric acid in cold condition
-Form tin hexachloride when tin react with HCl in hot condition
4. Reaction with alkali
-All react when fused to form anion and evolving H2 except carbon

-Diamond
oProduced from crystallization of molten magna
o have very high melting point
o having sp3 hybridization
o does not conduct electricity
o known precious jewelery and to making cutting tool
-Graphite
o Prepared by acheson process
o soft compared diamond
o conduct electricity
o used in pencil as lubricant
-Fulllerene
o Truncated icosahedral
o used as superconductor wire

-Silicon
Extraction
1. Reducing SiO2
2. Reducing SiCl4 ,zone refining process
-Silicate
SiO2 + metal oxides
-Aluminasilicate
o 3 dimensional silicate
-Silicate glass and type of glass
o sand + metal silicate , alumminosilicate,borosilicate
o Soft glass- bottle / window
o Hard glass - apparatus
o Flint glass
-Silicones
o organosilicon compound having Si-O-Si-O bond
-Type silicone
o Disilicone
o Chain silicone
o Branched silicone
- Tin
i) alpha sn (grey)
ii) beta sn (white)
-SnO2
o oxidaation state +4
o form by direct heating  of metal
o amphoteric oxide
-SnO
o oxidation state +2
o black tin
o prepared by heating tin oxalate
o amphoteric oxide
-SnCl4
o prepared by heating
o colourless compound
o covalent compound
- SnCl2
o predominantly covalent compound
o soluble in water and organic solvent
-SnS
o obtained by passing through gas H2S gas in Sn(II)
-SnS2
o obtained by oxidation SnS
-Lead
o high density
o high luster
o resists corrosive
-PbO
o yellow solid
o PbO + 2HCl ---->PbCl2 + water
o PbO +2OH ------->PbO2 2- + water
-PbO2
o Prepared by heating with sodium chlorate or red lead with nitric acid
o dark brownish solid
-Pb3O4
o Red lead
o mixture of PbO.PbO2

# data[].attributes.body
Group IVA

- normal oxidation number : +4
- down the group, oxidation no becomes +2, more stable due to inert pair effect.
- allotrope : diamond, graphite & fullerene

CARBON

OXIDE - CO ₂ & CO

carbon monoxide,(CO)
- dehydration of formic acid/ oxalic acid by concentration H₂SO₄
- reduction of CO₂ by hot-red
properties
- colourless gas, does not smell
- burned with blue flame
- toxic gas
- strong reducing agent
uses
- production of pure Ni using Mond process
- gas in the synthesis gas, in reforming process to produce fuel
- hydroformylation produce higher alcohol
- reagent to produce phosgene

carbon dioxide,(CO ₂)
- reaction of acid with calcium carbonate
- heating of limestone
properties
- act as ligand
- react with base
- dissolve in water

CARBONATE(CO ₃⁻² ) & HYDROGEN CARBONATE (HCO ₃⁻)

- all carbonate does not dissolve in water except Group IA
- Planar C & exist as resonance

HALIDES OF CARBON(CX ₄)

- does not undergo hydrolysis ( C has no d orbitals to receive a pair of electron from water)
- CCl₄ : organic colvent
- CF₄ : freon

CARBIDES

ionic carbide

- compound of C + M (IA,IIA & IIIA)
- easily hydrolyze
covalent carbide(metalloid carbides)
- giant molecules having covalent bonding
- SiC : tetrahedral lattice
- B₄C : icosahedral B₁₂ units alternating with C3
- both carbides extremely inert & hard substance
- Sic insulator, B₄C metallic
interstitial carbide(metallic carbides)
- atom carbons are adsorbed into metallic lattice interstices
- non stoichiometric composition

SILICON

- 2nd most abundant element  in earth
extraction :
- reducing SiO by coke
pure Si
- reducing SiCl4 by Na
- zone refining process
characteristic:
- high melting point
- inert element but attack by hydrogen
- does not dissolve in acids (except HF)

OXIDES

silicon dioxide, SiO2
- polymeric tetrahedral
- Si-O 50% ionic(diff EN)
# hydrolysis SiCl4
# acidification of water glass
characteristic
- inert  at low temp
- strong acidic oxide at elavated temp
- dissolved in HF
- dissolved in alkali
silicate, (SiO4)4-
- SiO2 + metal (oxides/sulphate/carbonate)
aluminosilicate
- Al atom subs Si in the silicate framework
- framework become -ve charge
- excess charges balanced by cations from group IA & IIA / transition metals
example
1. Feldspar
2. Zeolite
siliicate glass
sand + metal silicate/ aluminosilicate/ borosilicate
silicones
- organosilicon compound having heterocatenated Si-O-Si-O bonds in chains, rings & branches
# hydrolysis of alkyl/ aryl silicon halides
type of silicone
1. Disilicone - initial R3SiX
2. Chain silicone - initial R2SiX2
3. Branched silicone - initail RSiX3
properties
- thermally stable
- silicones water repelent
uses
- cosmetics
- breast implant

HALIDES SiX4

- all SiX4
- all halides (except SiF6)

HYDRIDES (salines)

- form catenation
# stock's reaction
properties
- hydrolysis in water and alkali
- exist in gas
- burn in air spotaneously

TIn,Sn

OXIDES (SnO2, SnO)

SnO2
- pure ionic oxide
- does not dissolve in HCl
- amphoteric oxide
SnO
- oxidation no :  +2
- black tin
- amphoteric oxide

HALIDES

SnX2 > stable SnX4
SnCl4
# direct heating element
- colourless gas
SnCl2
- covalent compound
- soluble in H2O & organic solvent
# anyhdrous SnCl2
# hydarated SnCl2.2H2O

SULFIDES

monosulphide (SnS) & disulphide (SnS2)
SnS
# passing through H2S gas
- dark brown unstable solid
- easily oxidise
SnS2
# oxidation SnS with ammonium polysulfides

LEAD,Pb

mineral galena, PbS
- high density, but soft with low boiling point
- high luster

OXIDES

PbO

# direct reaction
# thermal decomposition Pb(NO3)2/PbCO3
- yellow solid
- amphoteric oxides
PbO2
# heating Pb(II) solution with sodium chlorate
# red lead with nitric acid

Pb3O4
- red lead
- mixture of 2PbO.PbO2

HALIDES

Pb(II) > stable Pb(IV)
PbX4
- PbF4 & PbCl4 exist
- PbBr4 & PbI$ does not exist ( not strong oxidizing agent)
PbX2
- all in ionic form

thankyou Dr for today lesson <3
i've no question so far.

# data[].attributes.body
SUMMARY GROUP IVA

- valence electron, nsnp

- oxidation number of +4

- down the group, +2 is more stable due to inert pair effect

Inert Pair Effect

- describes the preferences of late p-block elements to form ions

whose oxidation state is 2 less than the group valency

- inert pair effect means non-participating of the outer most ns² electrons

in chemical bonding

- occurs when electron are pulled closer to nucleus, making them more stable

And difficult to ionize

- down the group, stability +4 decrease, +2 increase

Catenation

- the ability of electron to be bonded to one another to form long chain

- the tendency decreases down the group

- carbon - have greatest tendency due to good overlapping p(pi)-p(pi) bond

- silicon - less stabled due to poor p(pi)-p(pi) bond overlapping because the

Large size of Si

Reactivity

- increases down the group

CARBON

- exists in air, igneous rock, anthracite, bituminous rock, ignite

Allotropy

- diamond, graphite, fullerene, lonsdaleite, amorphous carbon

Diamond

- can be synthesized from graphite

P=125kbar

Graphite ---------> diamond

Catalyst , Rh/Ni , T =1500-2000k

Structure

- carbon bonded together by covalent bond

- high mp (4000 c)

- carbon bonded to other 4 carbon atoms having sp3 hybrid

The valence e are used up, no free electron, does not conduct electricity

Graphite

- prepared by Archeson process (high temp. Electrical furnace)

Structure

- made up of stacked of two dimensional carbon sheets

- bonded covalently to 3 other carbon (sp2 hybrid)

Properties

- soft

- conduct electricity, have free electron

- pencils and lubricants

- oxidizing/ reducing agents to form intercalation compounds

Fullerene

- consist of big carbon framework consisting even nuimber of carbon

C32 , C₄₄, C50, C₆₀, C₇₀

Structure C₆₀

- truncated icosahedrons

- C₆₀ is essentially a section of graphite curled up

- has sp2 containing 30 c=c bonds and retains the delocalized

Nature of graphite

COMPOUNDS OF CARBON

Oxides

- exist as CO2 and CO

CO

Preparation

- dehydration of formic acid by conc. H2SO4

- reduction of CO2 by hot-red C

Properties

- colourless gas, no smell

- burned with blue flame

- toxic gas, strongly bonded with hemoglobin than O2

- strong reducing agent

- act as ligand in the formation of carbonyl complexes

- CO donates a pair of e to transition metal to form coordinated

Covalent bonding

Uses

- production of pure Ni metal using Mond process

- synthesis gas in steam reforming process

- Hydroformylation (produce higher alcohol)

CO2

- linear molecules, non-polar, sp hybrid

Preparation

- reaction of acid with calcium carbonate

- heating of calcium carbonate

Properties

- colourless gas

- solid CO2=dry ice

- dissolve in water ---> carbonic acid

- react with base ---> carbonate

- act also as ligand (molecule donating e)

Uses

- fire retardant

- reactant in producing Na2CO3

- producing carbonated drink

- carbon cycle-biofuel

Carbonate

- don’t dissolves in water except from group IA

Structure

- planar sp2, exist as resonance

Halide

- doesnt undergo hydrolysis because Carbon has no d

Orbital to receive a pair of electron form water

CCL₄

Preparation

CS₂ + 3Cl₂ ----> CCl₄ + S₂Cl₂

CF₄

Properties

-inert, non-toxic, non-corrosive

-generally volatile

-insoluble

- dissolves in CCl₄, CHCl₃

- the high stability and inertness is due to

Uses

- freon (refrigerating gas), moomer in making plastic,

Non-stciky utensil

Carbide(C + metal)

- ionic carbide ( C + group IA, IIA, IIIA)

- easily hydrolize

-covalent carbide (SiC, B₄C)

- giant molecule having covalent bonding

(B₄C has icosahedral B12 units alternating with C3)

(SiC has tetrahedral lattice and can exist in two forms

corresponding to wurtzite and sphalerite lattices)

- inert and hard substances

- used for making cutting tools

- SiC is an insulator but B4C is metallic in appearance as

well as in properties even though it is covalent carbide

- interstitial carbide

- C are adsorbed into metallic lattice interstices

- have non-stoichiometric composition

- eg (Mn₄C , Mn₅C)

Properties

-lustrous solids with metallic properties

-have high melting points (TaC = 4170 K) and

extremely hard solids but brittle.

-Chemically inert and are hydrolysed by steam only above

870 K

SILICON

- exist as sand / flint

- silicate substances

Extraction

- Reducing SiO2 by coke

- using electric furnace

- excess silica used to prevent formation of Sic

- I) Reducing SiCl4 by Na

- ii) zone refining process

Characteristic

- crystalline Si has metallic luster

- diamond lattice

- High mp

- inert element

- not dissolve in acid except HF

- dissolve in base

COMPOUNDS

Oxides

- SiO2 (silica)

- exist as polymeric tetrahedral

- 50% ionic due to difference in electronegative

- as a molecule, its a covalent macromolecule

Preparation

- Hydrolysis of SiCl4

- acidification of water glass

Characteristic

- inert at low temp

- become strong acidic oxide at elevated temp

- dissolve in HF only and alkali

Silicate

- SiO2 + (m oxides/m sulphate/ m carbonate)

- structure, polymorph

Aluminosilicate

- 3D silicate

- Occur when Al atom substitute Si

- framework become negatively charge

-eg (Felaspar, Zeolite)

Zeolite

- regular size of pores and channels

- act as molecular sieves to separate molecules of different size

- cation balancing framework can be exchangeable

Silicate Glass

- sand + (m silicate/aluminosilicate/borosilicate)

Characteristic

- not a true solid

- has no mp

- heating --> soften ---> semisolid ---> clear liquid

- inert except F2

- produce soda glass

Type Of Glass

- soft glass

- ordinary soda lime

- easily fusible glass

- used for making bottles, windows

- hard glass

- potash lime-glass

- used for apparatus

- resistant in chemicals

- Flint glass

- lead- potash-lime glass

- high refractivity

- used in making lenses

- Jena glass

- zinc-barium-borosilicate glass

- low thermal expansion

- used fro heat shock resistent apparatus

- Pyrex

- sodium-aluminium-borosilicate

- similar to Jena

- Crooke’s glass

- cut off UV ray

- whole CaO replaced by PbO,BaO,ZnO,Mgo

- Quartz glass

- pure silica

- not crack even red hot vessel is plunged straight into water

- Ground glass

- soft glass

- the surface has been grounded by emery

- Reinforced glass

- has net work wires embedded in it

- does not shatter easily

Silicones

- organosilicon having heterocatenated Si-O-Si-O bonds

In chains, rings, branches

- consist Si-O-Si-O with alkyl/aryl bonded to Si

Preparation

- hydrolysis of alkyl/aryl silicon to halides followed by condensation

Types

- Disilicon (R3SiX)

- chain silicon (R2SiX2)

- branched silicon (RSiX3)

Properties

- thermally stable, low viscosity, remain elastic at low temp, inert towards chemical attack

Used

- Lubricant, cosmetic, breast implant, wax on car surface

Halides

- silicone halides, SiX4

- all halides except SiF4 unstable and undergo hydrolysis
- SiF4 undergo partial hydrolysis

Hydrides

- silanes

- form catenation, SiH4,Si2H3….up to Si6H14

Preparation

- stock’s reaction (silanes separated by fractional distillation)

Properties

- exist in gas, volatile liquid

- burn in air

- hydrolysis in water and alkali

TIN (Sn)

Preparation

- extraction of Tin Ore(SnO2)

Tin allotrope

- alpha-Sn (grey)

- beta -Sn (white)

- gamma-Sn

(transformation temperature will change the allotrope)

Physicochemical properties

- soft, malleable, not very ductile, brittle in heationg, crackles when bent

COMPOUND OF TIN

Oxides (SnO, SnO2)

- SnO2

- preparation

- direct heating of metal in O2

- pure ionic oxide

- not dissolve in Hcl, HNO3, aqua regia

- amphoteric acid

-SnO

- black tin

- preparation

- melting of tin oxalate

- amphoteric oxide

Halides

- SnCl4

- preparation

- direct heating of Sn, Cl2

- colourless liquid

- covalent compound

- rapidly hydrolyzed and fuming when in moist air

- form complex with HNO3

- SnCl2

- predominantly covalent compound

- soluble in water, inorganic solvent

- preparation

- anhydrous SnCl2

- Hydrated SnCl2.2H2O

- anhydrous salt is transparent crystalline solid

- dissolved in water to give cloudy solution

- heating SnCl2.2H2O to form basic chloride

- strong reducing agent

Sulfides

-SnS

- obtained by passing through H2S gas in Sn(ii)

- Dark brown unstable solid

- easily oxidized to SnS2

- SnS2

- obtained by oxidation of SnS using ammonium polysulfides

- yellow solid

- dissolve in excess ammonium polysulfides

LEAD (Pb)

- exist as mineral-galena

- extraction - roasting PbS with O2

- PbO + C

- physicochemical properties

- high density, high luster, ductile, malleable

COMPOUND OF LEAD

Oxides

- PbO

- preparation

- direct reation of Pb + O2

- thermal decomposition of PbCO3

- yellow solid

-amphoteric acid

-PbO2

- preparation

- heating of Pb(ii) with sodium chlorate

- read lead with nitric acid

-properties

- dark /  black powder

-strong oxidizing agent

- ionic compound

- decompose when heating

- dissolve in acid

- amphoteric oxides

- uses (as cathode in lead acid battery)

- Pb2O3

- red lead

- preparation

- direct reaction excess 3Pb + O2

- heating of PbO2

- show properties as PbO and PbO2

- uses (as pigment in paint to protect from rusting)

Halides

- PbX4

- PbF4, PbCl4

- Br and I not exist as its not strong reducing agent

- exist in ionic form

# data[].attributes.body
Summary of Group IVA
-Consists of non-metal ,metalloid, metals
-Oxidation number is +4, but as its goes down the group its becomes +2 due to inert pair effect.
-Carbon has 8 allotropes, the main 3 is (Diamond, Graphite, Fullerene)
Diamond
-made of carbon atom bonded together by covalent bonds.
-Has high melting point
Graphite
-prepared by Acheson process
-made up of stacked 2d carbon sheets
-soft, conduct electricity, as an oxidizing agent.
Fullerene
-consist of big C framework consisting even num.
-Compounds of carbon are such as oxides ,halides, carbonate and carbide.
Silicon
-Extraction of silicon by coke, Na and zone refining process.
-Oxides of silicon(Si02) is prepared by hydrolysis of SiCl4 and acidification of water glass
-inert at low temp but reactive at elevated temp, strong acidic at elevated temp, dissolve in HF, and alkali.
-Silicate is formed when Sio2 reacts with metal oxide/sulfate & carbonate.
-Eg of aluminosilicate -feldspar zeolite
-silicate glass=(salt +metal silicate, aluminosilicate & borosilicate
-3 types of silicone are disilicone, chain silicone ,branched silicone
Tin
-Tin allotrope (alpha-Sn , beta-Sn, gamma-Sn)
-compound of Sn such as oxide, halides and sulfide
Lead
-Exist as mineral galena
-Compounds of Pb are oxide(PbO, PbO2&Pb3O4 and halide

Thank you for the lecture dr!

# data[].attributes.body
Group IV Summary
-valence electron: ns2 np2
-normal oxidation number: +4 and down the group oxidation number +2 become more stable due to inert pair effect.
-inert pair effect means non-participation of outer most ns2 electrons in chemical bonding.
-It occurs when electron are pulled closer to nucleus and making them more stable and more difficult to ionize.
-Group IV form allotrope which can exist in more than one physical form.
-Catenation is ability of element to be bonded to one another to form long chain or ring and tendency to catenation decrease down the group.

CARBON
-Diamond;
~produced from crystallization of molten magna in earth crust
~can synthesized from graphite
~structure=
`bonded by covalent bonds
`high melting point
`Each C atom bonded to 4 other C atom having sp3 hybridization
-Fullerene;
~"Bucky ball"
-Compound of carbon;
~Oxides;
1.CO
`dehydration of formic acid or oxalic acid
`colorless,does not smell,blue flame,strongly bonded to hemoglobin than O2
`strong reducing agent, act as ligand, carbonyl complexes
2.CO2
`colorless, dont smell
`solid co2=dry ice
`anhydride acid and act as ligand
3.CO32- & HCO3-
`all didnt dissolve in water except from group IA
4.Halide,CX4
`Chas no "d" orbital
~Carbides
`ionic carbide, covalent carbide & interstitial carbide
`covalent carbide=giant molecules having covalent bonding

SILICON
-Extraction= Reducing SiO2 by coke,Reducing SiCl by Na and zone refining process
-Characteristic=metallic luster,grayish color,high melting point, does not dissolve in any acid except HF
-Silicone Compound;
1.SiO2(Silica):
`Preparation:Hydrolysis of SiCl4 & Acidification of water glass
`characteristic:Inert but become reactive at elevated temperature,strong acid at elevated temp & dissolve in alkali HF only
2.(SiO4)4-(Silicate)
`Structure:polymorph
`Aluminosilicate: 3 dimensional silicate occur when Al Atom subtitute S in SIlicate framework
`Zeolite :regular size of pores and channels
`Silicate glass:not true solid,no melting point(amorphous),cloring glass
`types of glass:Soft glass,Hard glass,flint glass,jena glass,pyrex or corning glass,crooke's glass,quartz glass,grund glass,reinforced glass.
3.Silicones;
`are organosilicon compounds having heterocatenated Si-O-Si-O bonds in chains,rings and branches
`preparation=Hydrolisis of alkyl/aryl silicon halides
4.SiX4(Silicone Halides):
`Hydrolysis occur through formation of dative bond from Oatom of water to Si of SiX4
5.Silanes:
`form catenation
`exist in gas and volatile liquid, burn in air spontaneously, hydrolysis of water and alkali

Tin (Sn)
-tin allotrope: alpha-Sn(grey),   beta-Sn(white),gama-Sn
`soft metal,malleable but not very ductile
1.oxides
-SnO2
`does not dissolve in HCl,HNO3 or aqua regia
`amphoteric oxide
-SnO
`black amphoteric oxide
-Halides
`SnCl4;dirct heating,colorless liquid rapidly hydrolyzed in fuming in moist air
`SnCl2:covalent compound
`SnS:pass through H2Sgas in Sn
`SnS2:obtain by oxidation SnS using ammonium polysulfides,yellow solid

LEAD
1.Oxide
-PbO;yellow solid,amphoteric oxide
-PbO2;dark brownish or black solid powder,strong oxidizing agent
-Pb3O4;red lead
-pigment for paint
2.Halide
-lead(IV) halide,PbX4.

# data[].attributes.body
The summary for today's class.
Tin
- tin can be gain from electrolysis or melting process.
- it is a soft metal, malleable, but not very ductile, become brittle on heating and crackles when bent.
- oxides (SnO2, SnO )
~ SnO2
* can be formed by direct heating of metal in air or oxygen.
* its does not dissolve in HCl, HNO3 or aqua regia.
- its is pure ionic oxide and become amphoteric oxide.
~ SnO
* preparation : heating tin oxalate.
* amphoteric oxide
- halides (SnCl4)
~ preparation : direct heating of the element
~ soluble  in water and organic solvent.
~ strong reducing agent..
- sulfide (SnS, SnS2)
~ SnS obtained by passing through the H2S gas in the Sn(II) solution.
~ SnS is easily oxidize to SnS2.
~ SnS2 obtained by oxidation of SnS using ammonium polysulfides

Lead
- high density but soft with low boiling point.
- high luster, ductile & highly malleable
- oxide (exist as PbO, PbO2, Pb3O4)
* PbO
- preparation : direct reaction between elements or thermal decomposition of Pb(NO3) or PbCO3.
- is an amphoteric oxide
* PbO2
- preparation : heating Pb(II) solution with sodium chlorate or  reaction of red lead with nitric acid.
- is a strong oxidizing agent
- is an amphoteric oxide
* Pb3O4
- is call as red lead
- preparation : Pb react with O2 or PbO is decomposed.
- halide (PbX2, PbX4)
*PbX4
- only PbF4 & PbCl4 exist
- PbBr4 & PbI4  do not exist because Br2 and I2 are not strong oxidizing agents thus unable to oxidize Pb(II) to Pb (IV)

# data[].attributes.body
Thank you dr for the explanation on group 4

Group IVA
CARBON (C)
•	inert pair effect
-non participation of the outermost ns2 electrons in chemical bonding
•	Catenation
-the ability of an element to be bonded to one another to form long chain or ring
Trend in chemical properties
•	Reactivity increase down the group
Exist as
•	Diamond
•	Graphite
•	Fullerene
Compound of Carbon
•	Oxide
-preparation is by dehydration of formic acid or oxalic acid, 
-reduction of CO2 by hot red C
•	Halide
-does not undergo hydrolysis because C has no d orbital to receive a pair of electron from water molecule
•	Carbonate
-also known as hydrogen carbonate @ bicarbonate
-all carbonate do not dissolve in water except for carbonate from group IA 
•	Carbide
-ionic carbide
-covalent carbide
-interstitial carbide

•	SILICON (Si) 
Exist as SiO2 (sand, quartz, flint, agate)
Extraction to obtain Si
•	Reducing SiO2 (sand) by coke
Extraction to obtain pure Si
•	Reducing SiCl4 by Na
•	Zone refining process
Characteristic
•	High melting point
•	Inert element but attack by halogen
•	Does not dissolve in acid accept HF
Silicone compound (OXIDE)
•	Oxides – also known as silica
•	Also exist as poly eric tetrahedral
Preparation
•	Hydrolysis of Sicl4
•	Acidification of water glass
Characteristic of silica
•	Inert at low temperature
•	Become strong acidic oxide at elevated temperature
•	Dissolve in HF only
Silicate
Aluminosilicate
Zeolite
•	Can be ion exchanger
•	It be strong acidic if the cation exchange with H+
Sodalite
Silicate glass
•	Soft glass
•	Hard glass
•	Flint glass
•	Jena glass
•	Pyrex or corning glass
•	Crooke’s glass
•	Quartz glass
•	Ground glass
•	Reinforced glass
Silicones
•	Preparation – hydrolysis of alkyl/aryl silicon halides  followed by condensation
•	Type od silicones – disilicones, chain silicones, branced silicon
•	Uses- in cosmetic (primer), silicone wax, and breast implant

TIN (Sn)
To obtain pure Sn
•	By electrolysis- get impure (anode), pure (cathode)
Tin allotrope
•	Alpha – beta – gamma—liquid stanum
Compound of stanum
•	Oxide
•	Halide
•	Sulphide

PLUMBUM (Pb)

Existence
•	As mineral – galena, PbS
Compound of Pb
•	Oxide
-PbO2 (yellow) uses is as cathode in Lead acid Battery
-Pb3O4 (red pigment) uses as pigment of paint
•	Halide


Question:
Why the gamma-Sn has no color. is it actually colorless?