# data[].attributes.body
Thank you Dr for the explanation in the videos. Here's my summary
- Group VA is also known as the Pnictides Group
- Atomic & ionic radii increases as going down the group
- Electronegativity & Ionization energy decrease as going down the group
- 3 ways to complete the octet( accepting electrons, sharing electrons & releasing electrons)
Nitrogen
-Physical properties(exists as gas in room temperature, odorless & colourless,  inert gas)
- Ammonia is used as fertilizer &  explosion(TNT)
-Physical properties of N2O( unreactive, soluble in water , decomposed upon heating & reacts with alkali & organic compound)
Phosphorus
- 3 types of phosphorus(red, white & black phosphorous)
-Red phosphorous has no smell, non- toxic & non- phosphorescence
-phosphorescence- glows in air
Trihalides of phosphorous can be prepared by direct halogenation of P4 except PF3
- White phosphorous is also called 'Willie Peter' in the military & used as incendiary  bombs, smoke screening and in tracer ammunition.

# data[].attributes.body
Thank you for the lectures, Dr. Below is my summary about Group VA.
- N & P (non-metal), As (metalloid), Sb & Bi (metal)
- Density, boiling point, atomic radius, & ionic radius increases down the group.
- IE, electronegativity decreases.
- oxidation number -3, +3, +5 (+3 becomes more stable down the group)
- 3 ways to complete octet; accepting eectron (anion), sharing valence eletrons, releasing electrons.
- Bi only shows coordination 3 & 6= more metallic properties.
1. Nitrogen
- Preparation; heating ammonium nitrite solution, oxidation of ammonia with copper(II) oxide, oxidation of ammonia with oxychlorate.
- Physical properties; colourless, odorless, inert.
- Chemical properties; reaction at hiigh temperature & room temperature.
- Ammonia, NH3; preparation (reaction of base on ammonium halide salt, hydrolysis of an azide, HABER Process), physical properties (choking smell, colourless, H-bond formed, dielectric constant low), chemical properties (reaction with metals, burn in oxygen with light green colour, dissolved in water to form ammonium hydroxide, aid-base neutralization, cation hydrolysis of ammonium salt, acting as reducing agent, ammonium salts decomposed on heating), uses (fertilizer, formation of organic chemicals, explosive, production of plastic & fiber, clean, bleach, & deodorize)
- N2O; preparation (decomposition of liquid ammonium nitrate0, properties (not reactive, inert to halogen, alkali metals & ozone at room temperature, assists combustion, very soluble in water), uses (anesthetic (laughing gas), aerosol propellant, colourless, very soft smell).
- NO; preparation (OSTWALD PROCESS, Cu + HNO3, birkeland-eyde reaction, dry reaction), properties (colourless gas, solid/liquid), uses (preparting nitric acid).
- NO2; preparation (NH3 oxidation, heat 2Pb(NO3)2, Cu + 4HNO3).
- Nitrogen oxoacid (H2N2O2, HNO2, HNO3); O, H, N, acid properties.
- Application of nitrogen compounds; preserve the freshness of packaged or bulk foods, pressurize kegs of some beers, cryopreservation of biological samples, laughing gas, drugs.
2. Phosphorus
- White phosphorus, red phosphorus, & black phosphorus.
- WP; soft solid, white, solid/liquid (P4), gas (P2), flammable to air, glows, smell of garlic, very toxic, disolve in CS2.
- RP; physical properties depenging on preparation, amorphous, dark red, stable in air (moderate reactivity compared to WP), no smell, non-toxic, doesn't glow in air, make matches, flame retardant materials.
- BP; sheet form, good conductor of electricity, most stable P allotrope, structure resembles graphite lattice.
- Phosphine (PH3); toxic gas, colourless, smelly, less soluble in water, alcohol, & ether, trigonal pyramid.
- PX3; prepared by direct halogenation of P4 (except PF3).
- PF3; colourless gas, acts as ligand, toxic, weak base, dissolve in water, prepared by fuorination of PCL3.
- PCL3; colourless liquid.
- PF5; catalyst for polymerization, very strong lewis acid.
- PCL5; yellow solid, prepared by direct chlorination, dissolve in polar solvent, chlorination agent.
- Phosphorus oxide; basic unit id P2O3 but stable as dimer P4O6, preparation by quantitative combustion.
- P4O6; white solid, stable towards O2 at room temperature, dissolves in water.
- P4O10; preparation by burning WP or P(III) oxide in excess oxygen, white powder, react vigorously with water.
- Oxoacid; lower acid (P(I) & P(III), reducing agent), higher acid (P(V), oxidizing agent), ionization occurs in all acids.
- Hypophosphorus acid, H3PO2; preparation (boiling white phosphorus in alkali/hydroxide of alkaline earth metals), properties (colourless crystal, monobasic acid, free acid & its anion are strong reducing agent.
- Phosphoric(III) acid (H3PO3 & H4P2O5); reaction of PCL3 or P4O6 with water, pure solid, colourless, deliquescence, dibasic acid, strong reducing agent in alkali/acid.
- Phosphoric acid (H3PO4 & H4P2O7); treating phosphate rock with sulfuric acid, reacting phosphorus(V) oxide with hot water, oxidizing phosphorus with conc. nitric(V) acid, colourless solid (pure), very soluble in water, tribasic acid.
- Application of phosphorus compounds; holme's signals, smoke screens.

# data[].attributes.body
Thank you for the detailed explanation for Group VA dr. Here is my summary for Group VA, for Nitrogen and Phosphorus

Nitrogen
-  It can be prepared by,
i)heating ammonium nitrate
ii) oxidation of ammonia with copper(ii) oxide
iii) oxidation of ammonia with oxychlorate
Hydride, Ammonia, NH3
-prepare in lab using reaction of base on ammonium halide salt, -hydrolysis of azide
-Use haber process for industry method.
- When react with mteal it create azide.
- It burns in oxygen with light green colour.
- It is soluble in water
Oxide
-tons of oxide, N2O, NO, NO2,
N2O3, N2O5
-Colouless gas
Oxoacid
- It is a compound containing OHN, ex:HNO3.
-  It is an oxidation agent,
Ammonium Salt
-all of it is soluble except NH4CLO4, NH4CO3
-it is obtained from strong acid.

Phosphorus
-Three types of phosphorus, red, black and white.
- Very good conductor for electricity.
Hydride, Phosphine, PH3
-it is a toxic gas
-colourless gas and smelly.
Halide, Phosphorus Trihalide, PX3
-some example is PF3, PCL3 PF5, PCL5.
Oxide
-some example is P4O6, P4O7, P4O8, P4O9, P4O10
Oxoacid
-it has two types
i) P(I), lower acid and P(II) as an oxidizing agent,
-some example is H3PO2, H3PO3, H3PO4.

# data[].attributes.body
group VA summary
Nitrogen
prep-lab
1)heating ammonium nitrite
2)oxidation ammonia with copper(II)oxide
3)oxidation ammonia with oxychlorate
-industry-fractional distillation of liquid air
properties-colourless, odourless
*Hydrides- NH3
lab prep-reaction of base on ammonium halide salt
-hydrolysis of an azide
industry prep-Haber process
*Oxide
1)N2O
prep-decompose of liquid ammonium nitrate
property- not reactive, inert
2)NO
industry-prep-ostwald process
lab prep-reaction of Cu/HNO3
property-colourless gas
3)NO2-form dimer N2O4
toxic
*Oxoacid
i)H2N2O2
ii)HNO2
iii)HNO3
*Ammonium salt
-soluble except NH4ClO4 and NH4CO3
used to preserve freshness of packaged food

Phosphorus
1)White
soft solid, flammable when exposed to air, toxic. dissolve in CS2 & organic solvent
2)Red
amorphous, stable in air, non-toxic, insoluble in CS2
3)Black
sheet form like graphite, good conductor of electric

*Hydride-phosphine, PH3
-toxic, colourless, smelly
-less soluble in water

* Halide
-direct halogenation except PF3
PF3- act as ligand, toxic, weak base , dissolve in water
PF5- catalyst for polymerization, very strong lewis acid. dissolve in polar solvent

*Oxide
Phosphorus(III)oxide, P4O6
Phosphorus(V)oxide, P4O10

*Oxoacid
Lower acid(reducing agent)
1)Phosphoric(I)acid, H3PO2
2)Phosphoric(III)acid, H3PO3

Higher acid(oxidizing agent)-
Phosphoric acid
H3PO4-phosphoric(V)acid
H4P2O7-diphosphoric(V)acid

# data[].attributes.body
 For Valency, Coordination Number & Hybridization
Bi only shows coordination 3 and 6 -> more metallic pro

# data[].attributes.body
Thank you for the lesson about group VA.Here is my summary.
GENERAL
-density, boiling point, atomic and ionic radius increase and for ionization energy and electronegativity decrease as it goes down the group
-oxidation number : +3,-3 and +5 but most stable is +3
-achieve octet by gain 3 electrons to form anion, lose electron to form cation with +3 charge not +5 charge due to the inert pair effect and sharing electrons (covalent)
-N cannot increase valency due to no d orbital
NITROGEN
-can be prepare by laboratory(heating ammonium nitrite solution, oxidation of ammonia with CuO and oxidation of ammonia with oxychlorate) and industry by fractional distillation of liquid air
-Hydrides
can be prepare by industry(Haber Process which need N2(by steam reforming or water gas shift process) and H2 (by compress air distillation) and laboratory by reaction of base on ammonium halide salt anc hydrolysis of an azide
chemical properties:
-react with metal form azide
-burn in O2 with light green colour
-dissolved in water
-act as reducing agent
application: fertilizer, production of fibre and plastic and explosive
-OXIDE(N2O, NO, NO2,N2O3, N2O5)
N2O
can be prepare by decomposition of liquid ammnonium nitrate
inert toward halogen, alkali metal and ozone at room temperature
can assist combustion and dissolve in water
can be used in anesthetic as it easily soluble in water
NO
can be prepare by industrially which is Ostwald Process or laboratory which is reaction of Cu/HNO3 and preparation for pure NO
diamagnetic if solid or liquid but paramagnetic if gas
NO2(paramagnetic, brown orange), N2O4(diamagnetic, colourless)
can be prepare by laboratory and industrially which is NH3 oxidation
-OXOACID (H2N2O2, HNO2)
HNO2
-weak acid, oxidizing agent(reduce to NO, N2O, N2) and reducing agent (oxidize to HNO3)
HNO2 can be use in Brown Ring Test to test the presence of nitrate
-AMMONIUM SALT (all soluble except NH4ClO4, NH4CO3)
apply in preserve thd freshness of package/bulk food and pressurize kegs of some beers
PHOSPHORUS
-White Phosphorus (solid/liquid= P4, gas=P2
-flammable so keep it water( vey toxic and smell like a garlic)
-held by weak Van Der Waals
-Red Phosphorus(physical properties depend on method of preparation)
-no toxic or smelly like white phosphorus
-held by covalent bonds
-Black Phosphorus
-has free electron so good conductor
-Hydride
very toxic, colourless and smelly
-similar to NH3
-act as ligand but weaker than NH3
-Halides
can be prepare by direct halogenation of P4 except PF3(prepare by flourination of PCll3)
PCl5 can be chlorination agent
-Oxide
basic unit: P4O6, stable dimer: P2O3, can be prepare by quatitative combustion
-P4O10 can be prepare by burning white phosphorus or phosphorus(III) oxide in excess O2
-Oxoacid(higher acid: P(I) and P(III), reducing agent and lower acid: P(V), oxidizing agent)
-H3PO2 can be prepare by boiling white phosphorus in alkali/hydroxide of alkalime earth metal. monobasic acid
-H3PO3 can be prepare by reaction of PCl3/P4O6 with water. dibasic acid
-H3PO4 can be prepare by industry (treating phsphorate rock with H2SO4 and laboratory ( reacting phosphoric(V) oxide with hot water and oxidizing phosphorus with concentrated nitric (V) acid. tribasic acid
-Phosphine used as Holme's signals and smoke screen(need to wear mask as it toxic)

# data[].attributes.body
Thank you Dr. for the pre- recorded videos. Here is my summary about group VA :-
-Going down the group ,

Metallic characteristic, density , boiling point, atomic radius & ionic radius increases.

IE and electronegativity decreases

- Oxidation number : -3 , +3 ,+5 or { +5, +4,+3, -3 } but going down the group +3 becomes more stable.
- 3 ways to complete octet :-

Accepting electron

Sharing valance electrons

Releasing electrons

Nitrogen
-Preparation
In laboratory

Heating ammonium nitrite solution

Oxidation of ammonia with copper(II) oxide

Oxidation of ammonia with oxychlorate

In industry

Fractional distillation of liquid air.

Hydrides - Ammonia (NH3)
Laboratory preparation

Reaction of base on ammonium halide salt

Hydrolysis of an azide

Industrial preparation - Haber Process
Properties - Chocking smell and colourless and dielectric constant low.
Applications - As fertilizer , bleach and used as an explosive and production of plastic and fiber.
Oxides - Dinitrogen oxide, Nitrogen monoxide, Nitric dioxide .
Oxoacid - Hyponitrous acid , Nitrous acid, Nictric acid.
Ammonium Salt - Soluble except NH4ClO4

Phosphorus

White phosphorus

Red phosphorus

Black phosphorus

Hydride - Phosphine (PH3)
Properties
-Toxic , colourless and smelly
-Less soluble in water, alcohol and ether.
Halide
- Phosphorus trihalide
Preparation : Direct halogenation (except PF3)
-Phosphorus pentahalide
Oxides
Preparation - Quantitative combustion
- Phosphorus(III) oxide
-Phosphorus(V) oxide
Oxoacid
- Lower acid- reducing agent

Phosphoric(I) acid, H3PO2

Preparation : Boiling white phosphorus in alkali or hydroxide of alkaline earth metals

Phosphoric(III) acid , H3PO3

Preparation : Reaction of PCl3 or P4O6 with water.

-Higher acid -oxidizing agent

Phosphoric acid, H3PO4

Preparation

Industry

- Treating phosphate rock with sulfuric acid

Laboratory

-Reacting Phosphorus(V) with hot water
-Oxidizing phosphorus with conc. nitric(V) acid.

# data[].attributes.body
Thank you dr for the lesson. Here is my summary on group VA

When down the group VA element:
metallic properties increase
density increase
boiling point increase
atomic/ionic radius increase
IE / EN decrease
stability of +3 increase

- There are 3 ways to complete octet which is accepting e, sharing e, releasing e

-Nitrogen: preparation in lab & industry, physical properties and chemical properties

- Oxide includes N2O, NO, NO2, N2O3 and N2O5 but focus on NO2 , NO and N2O (preparation and properties)

- NH3: preparation in lab and industry, application and 7 types of chemical rxn

- Ammonium salt: properties and uses

- Nitrogen Oxoacid: HNO2 and HNO3 (preparation and properties)

Phosphorus: white P , red P and black P

- Hydride: PH3 ; Halide PX3

- Halides including PF3 PCl3 PF5 PCl5

- Oxide: P4O6, P4O7, P4O8, P4O9, P4O10

- 2 types of oxoacid: lower acid and higher acid

# data[].attributes.body
Group VA ( The Pnictides Group)

Thank you dr for the class!  ♡♡♡

Nitrogen

·         Non metal element (gas)

Preparation

·         In laboratory

-heating ammonium nitrate solution

-oxidation of ammonia with copper (II) oxide

-oxydation with ammonia with oxychlorate(chlorate(I)ion)

·         In industry

-by fractional distillation

Physical properties

·         Colorless and odourless gas

·         Inert (not easy to react)

Nitrogen compound

·         Hydride

- ammonia

·         Oxide

-nitrous oxide

-nitric oxide

-Nitric dioxide

-dinitrogen dioxide

-dinitrogen pentoxide

·         Oxoacid

-nitric (I) acid

-nitric (III) acid

-nitric (V) acid

Application of nitrogen compound

·         To preserve the freshness of food

·         To pressurize the kegs of some beers

·         Used in cryopreservation of blood

·         To be a partial anesthetic

Phosphorus

White phosphorus, P4

·         Soft solid

·         Flammable when exposed to air

·         Smell of garlic, very toxic

Red phosphorus

·         Amorphous, dark red

·         Stable in air

·         No smell, Non toxic

Black phosphorus

·         Good conductor of electric

·         Most stable P allotropes

·         The structure resembles graphite lattice

Phosphorus compounds

·         Hydrides

-toxic gas

-smelly

-colorless

-Less soluble in water

-melting point less than NH3

·         Halides

-Xà F, Cl

-PX3

-PX5

·         Oxides

-P4O6

-P4O10

·         Oxoacids

-lower acid- P(I) and P(III) as reducing agent

-higher acid –P(V) as oxidizing agent

Consist of – H3PO2, H3PO3, H3PO4

Application of phosphorous compound

·         Used in military application

·         Used in Holme’s signal

·         Used in smoke screens

# data[].attributes.body
Thank you Dr fr the lessson
here are my summary about gp VA

-element for group VA  become metallic as we go down the group
-boiling point,density,atomic and ionic radius increase down the group.
-ionization energy and elegtronegativity decrease down the group
-the most stable oxidatin number +3 as go down the droup due to innert pair effect
-3 ways to cmplete octet(accept,sharing and release electron)

NITROGEN
preparation in labratory
-heating ammonium nitrates slution
-oxidatin of ammonia with copper(ii)oxide
-oxidation of ammonia with oxychlorate
in idustry
-frictional distillation of liquid air
i)HYDRIDES(ammonia, NH3)
-preparation in lab (the reaction of base on ammonium halide salt,hydrolysis of an azide)
-preparatuin in industry (haber process)
-chemical properties (reaction with metals azide (N3-),acid base neutralization,dissolved in water form ammonium hydroxide,acting as reducing agent,decomposed when heating)
ii) OXIDES
-N2O (preparation by the decomposition of liquid ammonium nitrate,properties not reactives,very soluble,decomposed to N2 and O2 when heating,uses as anesthetic because soluble in body)
-NO (preparatin in industry by ostwald process,laboratory by reaction of Cu/HNO3,aqueous slution,dry reaction and birkeland eyde reaction)
-NO2 (preparation in industry by NH3 oxidation,laboratory by thermal decomposition 2Pb(NO3)2
iii)OXOACID
-nitric (i) acid (stable solution,known as hyponitrous acid)
-nitric (iii) acid (weak acid ,stable in solution ,known as nitrous acid,an oxidizing and reducing agent salts derivatives)
-nitric (v) acid (preparatin industry by ostwald process,known as nitric acid ,colourless liquid but when exposed to light turn to yellow,act as oxidizing agent)
iv)ammonium salt
-all soluble except NH4ClO4
-salt decomposed when heating

PHOSPHOROUS
-white phosphorous (flammable when expsed to air,very reactive and toxic)
-red phosphorous (amarphous,dark red,non toxic,odourless)
-black phosphorous (most stable p allotrope,good conductor electric,sheet form like graphite)

i)HYDRIDES
-phosphine,PH3 (toxic gas,colurless ,smelly,less soluble in water,less electronegative than N)
ii)HALIDES
phosphorous trihalide PX3
-prepared by direct halogenation of P4 except PF3
-PF3 (colourless gas,formed complexes transition with metal,weak base,dissolves in water,prepared by fluorination of PCl3)
PCl3 (colourless liquid)
-pentahalide (PF5)
-catalyst for polymerazation.strong lewis acid
PCl5 (prepared by direct chlorination,easily hydrolized inwater ,chlorination agent)
iii) OXIDES
-phosphorous (III) oxides (prepared by quantitative combustion,white solid,dissolved in water)
-phosphorous (v) oxide (prepared by burning white phsphorous or phosphorous (iii)oxide ,white powder,react vigorously with water)
iv) OXOACID
-have 2 types (lower acid P(I),P(III)-reducing agent
-higher acid P(v)-oxidizing agent )
-phosphoric (i) acid (H3PO2) (preparation by boiling white phosphorous in alkali or hydroxide of alkaline earth metal,monobasic acid,strong reducing agent)
-phosphoric (iii) acid (H3PO3) (preparation by reaction of PCl3 or P4O6 with water ,strong reducing agent)
-phosphoric(v) acid (H3PO4) (preparatin in industry by treating phosphate rock with sulphuric acid, in lab by reacting phosphorous (v) oxide with hot water ,very soluble in water,tribasic acid)

# data[].attributes.body
Thank you dr for today's lesson. Here is my summary about this topic:
-N&P-->non metal
As-->metalloid
Sb&Bi-->metal
- +3 oxidation number becomes more stable down the group.
-N forms multiple bonds while the others do not.
-Bi only shows coordination 3 and 6 (more metallic properties)

NITROGEN
-3 ways to be extracted in laboratory (heating NH4NO2, oxidation of NH3 and CuO, oxidation of NH3 and Ca(OCl)2 )
-Fractional distillation of liquid air can produce nitrogen gas in industry.
Nitrogen hydrides (Ammonia, NH3)
- can be extracted through HABER Process in industry.
-choking smell
-physical properties similar with water
-chemical properties
⁘form amide
⁘Ostwald process
⁘form ammonium hydroxide
⁘Acid –base neutralization reaction
⁘Cation hydrolysis of ammonium salt
⁘reducing agent
⁘ligand
⁘Ammonium salts decomposed on heating
-Nessler's Agent is used to test for ammonia.
Nitrogen Oxides (NO)x
Dinitrogen oxide, N2O (Nitrous oxide)

Not reactive

Very soluble in water

An anesthetic

Nitric Oxide, NO(nitrogen monoxide)

OSWALD PROCESS

Important for preparing nitric acid from oxidation of ammonia

Nitric Dioxide, NO2(nitrogen dioxide)

Form a dimer, N2O4

Very Toxic

Nitrogen Oxoacid

H2N2O2 (nitric(I) acid): hyponitrous acid

HNO2  (nitric(III) acid) :  nitrous acid

HNO3  (nitric(V) acid): nitric acid

Brown Ring Test
-test the for presence of nitrates

PHOSPORUS
White Phosphorus

-Soft solid
-Kept in water (flammable when exposed to air)
-Smell of garlic, very toxic
Red Phosphorus
-Stable in air
-No smell, non-toxic

Black Phosphorus
-Sheet form like graphite/metals
-most stable P allotrope
Phosphine, PH3
-Toxic gas
-Less soluble in water, alcohol and ether (no formation of hydrogen bond)
-Complexing agent
Phosphorus Oxides
-Phosphorus(III) oxide, P4O6(P2O3)

White solid

Dissolves in water form phosphorus acid, H3PO3

-Phosphorus(v) oxide, P4O10

White powder

React vigorously with water to form mixture of acids

Oxoacid of Phosphorus
-Lower acid, P(I) and P(III) – reducing agent

-Higher acid, P(V) – oxidizing agent
-Phosphoric(I) acid, H3PO2

hypophosphorous acid

colourless crystal

monobasic acid

-Phosphoric(III) acid, H3PO2

pure solid

dibasic acid

strong reducing agent in alkali or acid

-Phosphoric acid, H3PO4

Colourless solid

Very soluble in water

Tribasic acid

# data[].attributes.body
Thank you Dr for the video .Here my summary.

NITROGEN
-Physical properties
i)density,boiling point,ionic radius increase
ii)IE,electronegativity decrease
-Preparation
i)heating NH3
ii)oxidation NH3 with CuO
iii)Oxidation of NH3 with oxychlorate
iv)industry(fractionally distillation of liquid air
HYDRIDE
-haber process
-N2 +H2-----2NH3
colourless
-dielectric constant low
OXIDE
-N2O=very soluble in water
-NO=OSWALD process,colourless gas
-NO2=form dimer,very toxic,poisonous gas
OXOACID
-H2N2O2 (basic acid,stable)
-HNO2(weak acid,oxidizing agent)
-HNO3(OSWALD process ,turn yellow
HALIDE
i)PF3= colourless gas ,weak base
ii)PCI3=colourless liquid
-P4 + CI2------PCI3
iii)PCI5(very strong lewis acid can accept a pair of electron suing empty orbital)
iv)PCI5(yellow solid,pepared by direct chlorination
PHOSPHORUS
P4(white phosphorus)
-flammable when exposed to air it glow
-RED phosphorus,BLACK phosphorus
-HYDRIDE
-toxic gas,smelly,acting as ligand
-OXIDE
-P4O6(Preparation:quantitative combustion)
-P4O10(white powder)
-OXOACID
-consist P,O,H
-H3PO2=monobasic acid
-H3PO3=with H4P2O5,dibasic acid
-H3PO4=with H4P2O7
-solve in H2O due to hydrogen bond
-tribasic acid

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

N , P (non-metal); As (metalloid); Sb, Bi(metal)

To complete octet:

Accept 3 e- -> anion (-3); with electropositive metal (GIA & IIA) - ionic compound

Sharing valence e-; with less reactive metals/non-metal-covalent compound (except Bi: metal -> ionic)

Release 3 e- -> cation (+3 inert pair effect/+5 rare due to high IE); ionization only occurs for Bi->Bi3+ & Sn->Sn3+

N: More reactive at high temp, more inert at room temp.

Preparation:

Lab

Heat NH4NO2

Oxidize NH3 by CuO

Oxidize NH3 by Ca(OCl)2

Industry

Fractional distillation of liquid air

Compounds

Hydrides

Ammonia NH3: low dielectric constant, explosive

Preparation:

Lab

base + ammonium halide salt

Hydrolysis of azide (N3-)

Industry

Haber Process

Oxides

Dinitrogen oxide,N2O: inert(halogen, alkali metals, ozone at RT), react w alkali compounds & organic compounds (elevated temp.), assist combustion, anesthetic. Laughing gas

Preparation:

Decomposition ammonium nitrate (l)

Decomposed -> N2 + 1/2O2

Nitric oxide,NO:
Preparation:

Industry

Ostwald Process

Lab

Cu + HNO3

Pure NO

Aqueous – 2NaNO2 + 2NaI + 4H2SO4 -> I2 + 2NO + NaHSO4; 2NaNO2+2FeSO4+3H2SO4->2H2O+2NO+Fe2(SO4)3+NaHSO4

Dry – KNO2 +KNO3 + Cr2O3-> 2K2CrO4 + 4NO

Birkeland-Eyde rxn

Nitric dioxide, NO2: monomer brow-orange, paramagnetic (dimer-N2O4 colourless, diamagnetic), toxic gas

Preparation:

Industry

Oxidation NH3

NO + O2

Lab

Heat Pb(NO3)2

Cu + HNO3

Oxoacid

Nitric(I) acid, H2N2O2: Hyponitrous acid, basic acid

Nitric(III) acid, HNO2: Nitrous acid, weak acid (oxidizing / reducing agent)

Nitric(IV) acid, HNO3: colourless (turns yellow when decomposed by light in prescence of NO2), acid oxidizing catalyst
Preparation:

Industry

Ostwald Process – oxidation of NH3

KNO3+H2SO4

1. Only Cu(NO3)2 insoluble in water

2. Brown Ring Test -Fe2+ reduce NO32- to HNO3 (+ Fe3+ -> brown coloured complex)

Ammonium Salt

1. Only NH4ClO4 insoluble

2. Salts obtained from oxidation of strong acid

3. Soln acidic – hydrolysis NH4+

4. NH4+ decomposed when heating

P

White P: P4 (solid/liquid at RT), P2 (gas), flammable when exposed to air (kept in water), toxic, garlic smell, phosphorescence

Red P: amorphous, dark red, non-toxic, odourless, non-phosphorescence

Black P: sheet, conduct electric, most stable P, toxic, low m.p (no H bond), ligand

Hydride

Phosphine, PH3: toxic, less soluble (water alcohol, ether)

Halide

Phosphorus Trihalide, PX3
Preparation:

Direct halogenation P4 (except PF3)

PF3: ligand, toxic (forms complex w hemoglobin -> disturb O2 transportation

Preparation – fluorination

PCl5: yellow(s), (l) and (g) phase, easily hydrolysed in water, easily attack by compound (w OH), dissolved in polar solv

Oxide
Preparation:

Quantitative combustion

Phosphoric(I) acid, H3PO2: monobasic

Preparation:

Boil white P in alkali/hydroxide/alkaline earth metals

P(III) oxide, P4O6: dimer, stable towards O2 (RT), P(III)->P(V) (high temp.),dissolved in water

1. Basic unit – P2O3 (less stable)

Preparation:

P(V) oxide, P4O10: react vigorously w water

Oxoacid

Lower acid: reducing agent

Phosphoric(I) acid, H3PO2: hypophosphorous acid, colourless crystal, monobasic

Preparation:

Burn white P/P4O6 in excess O2

Phosphoric(III) acid, H3PO3: phosphoric acid, pure colourless solid, deliquescene,dibasic acid

1. Hydration -> diphosphoric acid, H4P2O5

Preparation:

PCl3/P4O6 + water

Higher acid: oxidizing agent

Phosphoric(V) acid, H3PO4: soluble in water(H boding btwn H-O), tribasic acid

1. Hydrolysis -> Diphosphoric(V) acid, H4P5O7

Preparation

Industry

Treating Ca3(PO4)2(phosphate rock) w H2SO4

Lab

P4O10 + hot water

Oxidized P with conc.H3PO4

Question:
1.

For Part 1: 3 ways to complete octet
3. releasing electrons
ionization only occurs for:
Bi->Bi³⁺ & Sn->Sn³⁺

Is it mean other elements in GV do not form cation3+ or relatively less?

# data[].attributes.body
Thank You Dr  for the lecture. here are my summary for group VA:
- Density, b.p, atomic radius and ionic radius increase down the group.
- ionization energy, electronegativity decrease as go down the group.
-oxidation number of +3 becomes stable as it goes down the group .
-only N forms multiple bonds
- 3 ways to complete octet:
- accepting e-
- sharing valence e-
- releasing e-
NITROGEN
-preparation by :
1)Heating ammonium nitrite solution
2) oxadation of ammonia with copper(II) oxide
3) Oxidation of ammonia with oxychlorate
-physical properties:
- colourless, odourless gas
- inert
-chemical properties
- Reaction at high temp
- reaction at room temp
-Hydrides:
-preparation  in lab by the reaction of base on ammonium halide salt and hydrolysis of an azide
-peparation in industrial by the Haber process.
-Oxide:
-N2O, NO and NO2 the most popular
-Nitrogen Oxoacid has H2N202,HNO2,HNO3

PHOSPHORUS
-PH3:
- toxic gas, colourless, smelly
-mp lower than NH3 because P less electronegative than N
-PX3:
- prepared by direct halogenation of P4 except PF3
-PX5:
- very strong lewis acid
-OXIDES:
- P4O6 & P4O10 are the most important.
-OXOACID OF PHOSPHORUS:
- lower acid & higher acid
-H3P02,H3PO3,H3PO4

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

Summary for pnictides group:
* Stable oxidation no : -3 +3 +5
* As go down the group, increase atomic radius, atomic radius and metallic properties while ionization energy and electronegativity decreases.
*3 ways to complete octet : accepting electron, sharing electrons and releasing electrons

NITROGEN
Preparation in laboratory
1.Heating ammonium nitrite solution
2.Oxidation of ammonia with copper(II) Oxide
3.Oxidation of ammonia with oxychlorate
Preparation in  industry
Fractional distillation of liquid air

Ammonia (NH3)
* Preparation in laboratory
The reaction of base on ammonium halide salt
Hydrolysis of an azide
* In industry by Haber process.
* Ammonia has choking smell and colorless
* Physical properties similar to water
* Dielectric constant low

Oxides of nitrogen
* N2O is prepared by the decomposition of liquid ammonium nitrate. Not reactive, inert to halogens, and very soluble in water.
* NO is prepared in industry by Ostwald process. Colourless gas and important for preparing nitric acid.
* NO2 is very toxic gas  an prepared by NH3 oxidation.

Nitrogen Oxaacid
* Nitric(III) acid is weak acid. HNO2 is oxdizing agent and reducing agent.
* Nitric Acid, HNO3 prepared by oxidation of ammonia. Volatile colourless liquid.

PHOSPHORUS
* White Phosphorus is soft solid , white and very toxic. * Red phosphorus is stable in air and non-toxic.
* Black phosphorus is sheet form like graphite and good conductor electric.
* Phosphine,PH3 is toxic , less soluble in water, alcohol ether because the absence of hydrogen bond. Melting point lower than NH3 because P less electronegative than N.
* Phosphorus Trihalide, PX3 is prepared by direct halogenation except PF3. PF3 form complexes with transition metal (act as a ligand), it toxic and weak base. PCl is colourless liquid.
* Phosphorus Pentahalide,  PX5 is catalyst for polymerazation and very strong lewis acid. PCl5 is yellow solid, trioganal bipyramidal in liquid and gas phase and dissolves in polar solvent.
* Oxides of Phosphorus. P4O6 is white solid , stable towards oxygen at room temperatures. P4O10 is white powder and react vigorously with water.
* Oxaacid of phosphorus. H3PO2 is colourless crystal and monobasic acid. It free acid. H3PO3 is pure solid, colourless and dibasic acid. H3PO4  is colourless solid and very soluble in water. Tribasic acid.
Uses of Phosphorus :
1. White phosphorus in the military.
2. Combustion of phosphine used in Holme’s signals.
3. Phosphine used in smoke screens.

# data[].attributes.body
Group VA  (Pnictides Group)

properties
N : non metal (g)
P : no metal (s)
As : metalloid (s)
Sb : metal (s)
Bi : metal (s)

- density, boiling point, atomic radius & ionic radius increases
- ionization & electronegativity decreases
- only N form multiple bonds

3 ways to complete octet
1. accepting electron
2. sharing valence electron
3. releasing electron

NITROGEN

laboratory
# Heating ammonium nitrate solution
# Oxidation of ammonia with copper(II) oxide
# Oxidation of ammonia with oxychlorate (chlorate(I))

industry
# Fractional distillation of liquid in air

physical & chemical properties
- colourless, odourless gas
- inert
- low melting & boiling point (liquid N2 as coolant)
- reaction at hgh temp
- reaction at room temp

Compounds of Nitrogen
1) Hydride
laboratory
# Reaction of base on ammonium halide salt
# Hydrolysis of azide
industry
# Haber Process

physical properties
- colourless, chooking smell
- similar to H2O ( can form Hydrogen bond)
- dielectric constant low (less ionic than H2O & good solvent in organic compoung)

chemical properties
- reaction with metals
- burn in oxygen with light green colour
- dissolve in H2O to form ammonium hydroxide
- acid-base neutralization reaction
- cation hydrolysis of ammonium salt
- reducing agent
- ammonium salt decomposed on heating

applications
- fertilizer
- formation organic chemicals
- bleach

2) Oxides
1. Dinitrogen Oxide. N2O (nitrous oxide)
# decomposition of liquid ammonim sulphate
- not reactive metals
- decomposed to N2 & O2 on heating
- very soluble in H2O
- reacts with alkali metals & organic compounds
- anesthetic, laughing gas, aerosol propellent

2. Nitric Oxide, NO (nitrogen monoxide)
# Ostwald Process (industry)
# reaction of Cu/HNO3
# Bikeland-Eyde reaction

3. Nitric Dioxide, NO2
- form dimer, N2O4
# NH3 oxidation (industry)
# Themal decomposition

3) Oxoacid
1. Nitric (I) Acid , H2N2O2
- basic acid
- stable in solution
- hyponitrous acid

2. Nitric (II) Acid, HNO2 (nitrous acid)
- weak acid
-  oxidizing agent
- reducing agent
- salts derivatives
- isoelectric to O3 & F,O,N

3. Nitric (V) Acid, HNO3 (nitric acid)
# Ostwald Process
- colourless but turn yellow under light
- white solid, keep in dark bottle
- self ionization
- oxidation agent
- Brown Ring Test (reduce nitrates to nitric oxides)

4) Ammonium salt
- all soluble except (NH4ClO4, NH4CO3)
- salts obtained from strong acid
- NH4+ salt decomposed when heating
- oxidizing anion
- preserve freshness

PHOSPHORUS

white phosphorus
- soft solid , white
- solid/liquid : P4 , gas : P2
- flammable, when exposed to air it glow > presence phosphorescence
- kept in water
- smell of garlic, very toxic
- dissolve in CS2 & organic solvent
red phosphorus
- amorphous, dark red
- stable in air
- no smell
- makes matches head, flame retardant materials
black phosphorus
- sheet form like graphite
- conduct electricity
- most stable P allotrope

Compounds of Phosphorus
1. Hydride
Phosphine, PH3
- toxic gas, colourless, smelly
- less soluble in H2O, alcohol & ether (does not form  hydrogen bond)
- melting point lower than NH3 (P < electrinegativity than N)
- structure similar to ammonia (trigonal pyramid)
- complexing agent (act as ligand but weaker than NH3, P-H bond less polar)

2. Halide
1. Phosphorus Trihalide, PX3
- all PX3 exist
# direct halogenation of P4 (except PF3)

PF3
- colourless gas
- form complexes with transition metal (ligand)
- toxic
# fluorination of PCl3

PCl3
- colourless liquid

2. Phosphorus Pentahalide, PX5

PF5
- catalyst for polymerization

PCl5
- yellow solid
# direct chlorination

3. Oxide
1. Phosphorus(II) Oxide, P4O6 (P2O3)
- stable dimer, P4O6
# Quantitive combustion
- white solid
- stable towards O2 at room temperature
- dissolves in water

2. Phosphorus(V) Oxide, P4O10
# Burning white phosphorus/phosphorus(II) oxide in excess oxygen
- white powder
- react vigorously with H2O

4. Oxoacid
- lower acid , P(I) & P(III) > reducing agent
- higher acid, P(V) > oxidising agent
1. Phosphoric(I) Acid, H3PO2
- hypophosphorus acid
# boiling white phosphorus in alkali/hydroxide of Group IIA
- colourless crystal
- monobasic acid

2. Phosphoric(II) Acid, H3PO3
# Reaction of PCl3/P4O6 with H2O
- pure solid, colourless
- dibasic acid
- strong reducing agent in alkali/acid
H2P2O5
# elimination of H20 from H3PO3 (dehydration)

3. Phosphoric Acid, H3PO4
# Treating phosphate with sulfuric acid
# Reacting Phosphorous(V) oxide with hot water
# Oxidizing phosphorous with conc. nitric (V) acid
- colourless solid
- very soluble in H2O
- tribasic acid

Applications
- WP for military application
- Holme's signals
- Phosphine, smoke screens

Thankyou Dr for today class. I've no question so far.

# data[].attributes.body
Thank you Dr for today's lesson. Here is my summary for group VA

- Density, boiling point, atomic radius and ionic radius increase going down the group
- IE and electronegativity decrease going down the group
- Oxidation number of +3 becomes stable as goes down the group
- 3 ways to complete octet: accepting electron, sharing electron and releasing electron

NITROGEN
- Prepared in lab by heating NH4NO2 solution, oxidation of NH3 with CuO
- Prepared in industry by fractional distillation of liquid air
- Physical properties: colourless, odourless gas and inert

NH3
- Prepared in lab by the reaction of base on ammonium halide salt
- Prepared in industry by Haber Process
- Physical properties: choking smell, colourless
- Chemical properties: burn in O2 with light green colour, act as reducing agent

- Oxides include N2O, NO, NO2, N2O3 and N2O5
N2O
- Prepared by decomposition of liquid NH4NO3
- very soluble in water
NO
- Prepared by Ostwald process
NO2
- Form a dimer
- Prepared by NH3 oxidation

- Nitrogen Oxoacid: H2N2O2, HNO2 and HNO3

- Ammonium salt: all soluble except NH4CIO4 and NH4CO3, decomposed when heating

PHOSPHORUS

White Phosphorus
- soft solid, white
- kept in water
- smell of garlic, very toxic
Red Phosphorus
- amorphous, dark red
- stable in air
- no smell, non toxic
Black Phosphorus
- sheet form like graphite
- good conductor of electricity
- most stable P allotrope
Phosphine
- toxic gas, colourless
- less soluble in water, alcohol and ether
Phosphorous Trihalide
- prepared by direct halogenation of P4 except PF3
PF3: colourless gas, weak base and dissolve in water
PF5: catalyst for polymerization
PCl5: yellow solid, prepared by direct chlorination
- Oxides of phosphorus: P406, P4O7, P4O8, P4O9 and P4O10
- 2 types of oxoacid: lower acid (reducing agent) and higher acid (oxidizing agent)

# data[].attributes.body
Thank you dr for the good explaination in the pre-recorded video :) Here is the summary in Group VA

NITROGEN

Physical properties:
N : non-metal (gas)
P : non-metal (solid)
As : metalloid (solid)
Sb : metal (solid)
Bi : metal (solid)

3 ways to complete octet
1) Accepting electron --> become anion
: X3- ion occur with very  electropositive metal ( Group IA & IIA ) --> form ionic compound
2) Sharing valence electron
: bonding with less reactive metals or non-metal --> covalent compound
3) Releasing electrons --> becomes cation
: X5+ ion does not form (high IE to remove e-)
: inert pair effect occur --> forming X³⁺
: ionization ONLY occur for Bi-->Bi³⁺ and Sb-->Sb³⁺

Nitrogen
- Preparation:

Laboratory

1) Heating ammonium nitrate solution
2) Oxidation of ammonia with copper (II) oxide
3) Oxidation of ammonia with oxychlorate ( Chlorate (I) ion )

Industry

1) Fractional distillation of liquid air
- Physical properties:

colourless, odourless gas

inert atmosphere

liquid N₂ as coolent

- Chemical properties:
1) Reaction at high temperature
: with H ₂ --> ammonia
: with O ₂ --> nitrogen oxide
2) Reaction at room temperature
: with Li --> lithium nitride

Hydride
Ammonia, NH ₃

Laboratory

1) Reaction of base on ammonium halide salt
2) Hydrolysis of an azide

Industrial

1) Harber Process
- Physical properties:

choking smell, colourless

bp low

similar to water

dielectric constant low

: less ionic than water
: good solvent for organic
- chemical properties:
1) With metal --> azide (N³⁻)
2) Burn in O2 with light green colour
: without catalyst  --> get N ₂
: with catalyst (Ostwald Process)
3) Dissolved in water to form ammonium hydroxide
4) Acid-base neutralization
5) Cation hydrolysis of ammonium salt
6) Acting as reducing agent
7) Ammonium salts decompose on heating
- Application:

fertilizer

formation of organic chemical

as an explosive

Oxides
1) Dinitrogen oxides, N2O (Nitrous oxide)
Preparation:
- Decomposition of liquid ammonium nitrate
Properties:

Not reactive, inert towards halogen, alkali metals and ozone at RT

Decompose to N2 and O2 on heating

Assists combustion

Very soluble in water

Reacts with alkali metalk and organic compound

Uses:

Anesthetics, easily soluble in water/body liquid

Aerosol propellant

Aolourless and very soft smell

As laughing gas

2) Nitric oxide, NO (nitrogen monoxide)
Preparation:
- Industry : Ostwald Process
- Laboratory
a) Cu/HNO3
b) For pure NO
: aqueous solution
: dry reaction
c) Birkeland-Eyde Reaction
3) Nitric oxide, NO2 (nitrogen dioxide)
- Form dimer, N2O4
- Very toxic
Preparation:
- Industry
: NH3 Oxidation

Oxoacid
- Acid properties
-Contain O, H, N
- Consists of:
: H2N2O2 -> hyponitrous acid
: HNO2 -> nitrous acid
: HNO3 -> nitric acid
1) Nitric (I) acid, H2N2O2
- Basic acid
- Stable in solution
2) Nitric (III) acid, HNO2
- Waek acid
- Stable in solution
- Properties:

Oxidizing agent --> reduce to NO, N2O and N2

Reducing agent --> oxidized to HNO3

Salts derivatives

3) Nitric (V) acid, HNO3
Preparation
- Industry (Ostwald Process) - oxidation of ammonia
Properties:
- oxidizing agent
: to form salt
- acid oxidizing catalyst
- nitrate salts soluble in water/hydrated except Cu(NO3)2

Phosphorus

White phosphorus
Physicochemical properties:
- soft solid, white
- solid/liquid - P4 paint
- gas - P2
- flammable when exposed to air it glow
- kept in water
- smell of garlic, very toxic
- dissolve in CS2 & organic solvent

Red phosphorus
- physical properties depend on preparation method
- amorphous, dark red
- stable in air: moderate reactivity
- no smell / non-toxic / non-phosphorescence
- make matches head & flame terardant

Black phosphorus
- sheet form like graphite/metals
- a good conductro of electricity
- most stable P allotrope
- structure resembles graphite latttice

Hydrides
Phosphine, PH3
Properties:
- toxic gas, colourless, smelly
- less soluble in water, alcohol, ether
-  structure similar to ammonia
- mp lower than NH3 bcs P less electronegative than N

Halides
PF3
- colourless gas
- form complexes with transition metal
- toxic
- waek base
- dissolve in water
Preparation:
- by fluorination of PCl3
PF5
- catalyst for polymerization
- very strong lewis acid
--> accept e- using d⁰ orbital
- yellow solid, trigonal bipyramidal
- prepared by direct chlorination
- dissolve in polear solvent
- easily attacked with OH group
- chlorination agent

Oxides

Phosphorus (III) oxide, P4O6

Properties:
- white solid
- stable towards O2 at RT
- dissolves in water

Phosphorus (V) oxide, P4O10

Preparation:
1) Burning white P / P4O6 in excess O2
Properties:
- white powder
- reacts vigorously with water --> mixture of acid

Oxoacid
- 2 types
: Lower acid, P(I) and P(III) - reducing agent
: Higher acid, P(V) - oxidizing agent
Properties:
- ionization occured at P-O-H
- P atom form tetrahedral unit

Phosphoric (I) acid, H3PO2

-known as hypophosphorus acid
Preparation
- Boiling white P in alkali/hydroxide of alkaline esrth metal
Properties:
- colourless crystal
- monobasic acid
- free acid and its anoin are strong reducing agent

Phosphoric (III) acid, H3PO3

Preparation:
- Reaction of PCl3/P4O6 with water
Properties:
- pure solid, colourless
- deliquescene
- dibasic acid
- 2 types of phosphite salts
- strong reducing agent in alkali/acid

Phosphoric acid, H3PO4

- 2 types:
: H3PO4
-  phosphoric (V) acid
: H4P2O7
- diphosphoric(V) acid
Preparation:
- Industry
1) Treating phosphate rock with sulfuric acid
- Laboratory
1) Reacting phosphorus(V)axide with hot water
2) Oxidizing phosphorus with conc. nitric(V)acid
Properties:
- colourless solid (pure)
- very soluble in water -> syrupy solution
- tribasic acid
Applications:
- used in military application -> incendiary bomb
- used in Holme's signal
- used in smoke screens

# data[].attributes.body
Thank you dr for this topic videos. here are my summary

1) Group VA also known as Pnictides group
- down the group, the metallic properties, atomic radius and ionic radius increases. however, ionization energy, and electronegativity decreases down the group.
- N can form multiple bond
- there are 3 ways to complete the octet for this group
* accepting electron to become anion
* sharing valence electron
* releasing electron

NITROGEN
- In laboratory , can be prepared by heating ammonium nitrite solution, oxidation of ammonia with copper(II) oxide and oxidation of ammonia with oxychlorate
- In industry, prepared by fractional distillation of liquid air
- Nitrogen is colourless and odourless gass and inert. Nitrogen can react in both high and room temperature
*AMMONIA
- can be prepared by reaction of base on ammonium halide salt or hydrolysis of an azide. in industry, by haber process
- it chemical properties are have choking smell and colourless gas and have similar physical properties with water
- Ammonia can react with metals (form azide), burn in oxygen with light green colour (without catalyst form dinitrogen, and with catalyst form nitrogen oxide). it also can dissolved in water (form ammonium hydroxide) and involve in acid-base neutralization reaction. then, involve in cation hydrolysis of ammonium salt also act as reducing agent and will decomposed on heating
- oxide of nitrogen have 5, which are dinitrogen oxide (N2O), nitric acid(NO), nitric dioxide (NO2), dinitrogen trioxide (N2O3) and dinitrogen pentoxide (N2O5)

PHOSPHORUS
- red and white phosphorus is more famous then black phosphorous.
-  compound of phosphorous are hydride (phosphine, PH3), halide (phosphorous trihalide, PX3, phosphorous pentahalide, PX5), oxides (phosphorous(III) oxide, P4O6, phosphorous(V) oxide, P4O10).
- next is oxoacid (for lower acid, P(I) and P(III), and for higher acid P(V))(the oxoacid are H3PO2 or phosphoric(I) acid, H3PO3, phosphoric(III) acid and phosphoric acid, H3PO4)

the application are
1) white phosphorous- in military application (incendiary bombs or smoke-screening)
2) spontaneous combustion of phosphine- used in Holme's signal

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

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

# data[].attributes.body
THANK YOU DR SHEELA FOR THE LESSONS AND IM VERY SORRY FOR BEING LATE TO POST THIS SUMMARY..

Group VA consists of nitrogen,phsphorus,arsenic,antimony and bismuth.
- They have 5 velance electrons.
-Density and size of atomic are increasing down the group
- IE and electronegativity decreasing down the group
- most satble oxidation number is +3 because of inert pair
3 ways to complete octet
* Accepting electrons
*Sharing electrons
*Releasing electrons

NItrogen
-Nitrogen is an important element in world because of 78% of air contain of it.
-Can be prepared in lab : 1. by heating NH4NO2 ,2.oxidation of NH3 with CuO , 3. Oxidation of NH3 with osychlorate.
-Prepared in industry : Fractional distillation of liquid air
- Nitrogen is colourless and odourless gas.
-Nitrogen can form hydrides,oxides,oxacid
HYDRIDES
-AMMONIA ,NH3
-Industrial manufacture of ammonia is through the HABER PROCESS which the ammonia gas obtained as liquid (NH3)
-chocking smell,colorless.
-dielectric constant low: less ionic than water and good solvent for organic compounds.
-Chemicals properties for ammonia : 1. reaction with metals , 2. Burn in oxygen with light green colour, 3. Dissolved in H2O to form NH4OH. , 4. Acid-base neutralization reaction , 5. Cation hydrolysis of NH4CL ( acid-base dimer process) , 6. Acting as reducing agent.( reduce chlorine to chloride.) , 7. Ammonium salt decomposed on heating.
-Applications : fertilizer,explosive,production of plastic and fiber, NH3 solution : clean,bleach and dedorize.
OXIDES : N20,NO,NO2,N2O3,N2O5.
-N2O : dinitrogen oxide/nitrous oxide
-can be prepared by decomposition of liquid ammonium nitrate.
-Not reactive,decomposed to N2 and O2 on heationg.
-very soluble in H2O
-Uses : an anesthetic,aerosol propellent , known as laughing gas.
-NO : nitric oxide ( nitogen monoxide)
- prepared by OSTWALD PROCESS (industry)
-LAB : reaction of Cu/HNO3 , preparation for pure NO : aqueous solution and dry reaction , Bikerland-Eyde Reaction.
-NO2 ,NITRIC DIOXIDE
-Form dimer ,N204
-Very toxic
-NO2 : paramagnetic ,N2O4 : Diamagnetic
PREPARATION:
-Industry : NH3 OXIDATION
-LAB: THERMAL DECOMPOSITION OF Pb (NO3)2
NITROGEN OXACID (H2N2O2,HNO2 AND HNO3)
Nitric (I) acid , H2N2O2
-hyponitrous acid
Nitric (III) acid ,HNO2 = NITROUS ACID
- (weak acid）
-oxidizing agent : reduced to NO,N2O and N2.
-As reducing agent : oxidized to HNO3.
-Isoeletronic
Nitric (V) acid ,HNO3 = NITRIC ACID
- OSTWALD PROCESS : OXIDATION OF NH3 (INDUSTRY)
-volite colourless liquid
-turn to yellow due to presences of NO2
-white solid
-Oxidation agent
-HNO3 is sp2 hybrid
-BROWN RING SALT
ALL SOLUBLE EXCEPT NH4ClO4 ( AMMONIUM SALT)
-USES : preserve the freshness of packaged or bulk food, liquid nitogen used in cryopreservation of blood, reproductive cells and other biological samples.
, N2O : laughing gas

PHOSPHORUS
- Contains 3 allotropes : white , black and red
White phosphorus ,P4
-soft solid,white
-solid/liquid: P4
-gas : p2
-smell of garlic;very toxic
dissolve in CS2 and organic solvent
-tetrahedral P4 molecule
Red phosphorus
-amorphous ,dark red.
]-stable in air
no smell and non toxic
-used to make matches head and flames retardant materials.
-Comparisons of white/yellow P and Red P.
Black Phosphorus
-good conductor of electricity
-most stable P allotrope.
-Sheet form graphite /metals

PHOSPHORUS COMPOUNDS : HYDRIDES,HALIDES ,OXIDES AND OXACID
HYDRIDES
-Phosphine ,PH3 .
-Toxic gas,colourless and can cause death if breathing continuously in 10 ppm
-less solube in water and alcohol and ether cause no H bond
trigonal planar structure
HALIDES
-All PX3 EXIST (x = F--->I)
-prepared by direct halogenation of P4 exist PF3.
-trigonal planar
-PF3/PCL3
-PF5/PCL5
OXIDES
-EXIST : P4O6,P4O7,P4O9 AND P4O10
OXACID
- 2 TYPES OF OXACID : LOWER AND HIGHER
-lower acid P(I) AND P(III) -REDUCING AGENT
-higher acid P(V) : oxidizing agent.
-H3PO2 ( PHOSPHORIC (I) ACID  , H3PO3 ( PHOSPHORIC (III) ACID AND H3PO4(PHOSPHORIC ACID)
-USES : smoke-screening (phosphine), Holmes signals (phosphine) , military applications as smoke bombs and smoke pots (white phosphorus ,P4)
Thats all my summary for this topics.
So far i have no any question for this topics.Thank you Dr sheela.

# data[].attributes.body
Group VA  pnictides group
🔴N, P :non metal
As :metalloid
Sb, Bi : metal
🔴 Increase down gp : density, atomic radius, ionic radius
🔴Decrease IE, electronegativity
🔴+3 become stable down the group
🔴Only N form Multiple bonds
🔴Complete octet by
1)accept electron (anion - 3)
2)sharing electron(form covalent exc for Bi, bcs form ionic)
3) releasing electron (cation)
+5❌very high IE
+3✅  innet pair eff.
IE occur for  Bi and Sb
🔴Valency, coordination no, hybridization
N :sp3, 4 coordination no
P-Bi : has d orbital, can hybrid

Only Bi  shows coordination 3-6 (metallic properties)

ELEMENT NITROGEN  (78% in air)
Preparation
In lab
1)Heating NH4NO2 solution
2)Oxidation NH3 + CuO
3)Oxidation NH3+Ca(OCl) 2
In industry
Fractional distillation of liquid air

🔴Compund
1)Hydride : ammonia NH3
Industrial preparation :Haber process.
2)Oxide : N2O, No, NO2, N2O3 N2O5
3)Oxoacid : Compound contain OHN : H2N2O2, HNO2, HNO3
*brown ring test for nitrates
Fe2+ reduces Nitrates to nitric oxide, form brown coloured compound *
4)Ammonium salt soluble, exc NH4CLO4, NH4CO3

ELEMENT PHOSPHORUS
✅Allotropic form : white, black red.
⚪WHITE P4,
Exposed in air so Glow in the dark->P4O6  tetraphosphorus hexoxide. Kept in water.
Smell of garlic
Very toxic
Dissolve in CS2, organic solvent
🔴RED
Stable in air, no smell, non toxic, not glow in dark.
Used to matches head&fkame retardent material
⚫Black (sheet form like graphite)
Good conductor electricity

✅Compound
1)hydride PH3, phosphine
2)halide
PX3 phosphorus trihalide
PX5 phosphorus pentahalide
3)oxide :
P4O6
P4O10
4) Oxoacid
- lower acid, reducing agent.
P(I), H3PO2
P(II)-H3PO3 phosponic acid To    H4P2O5 diphosponic acid by dehydration

-higher acid  oxidatizing agentH3
P(V) H3PO4 phosphoric acid to
H4P2O7 diphosphoric acid by dehydration

APPLICATIONS OF  PHOSPHORUS
1)WP in military, bombs, smoke screening(White phosphorus)
2)Holme's signal (calcium carbide&calcium phosphine thrown to sea)

# data[].attributes.body
anomalous properties of bi:

does not form covalent bond but ionic.

only show +3 and +6 coordination as it  shows more metallic properties

Nitrogen

exists in air(78%) and amino acids

colorless and odorless gas

Preparation of N

heating ammonium nitrate solution

oxidation of ammonia with CuO

oxidation of NH₃ with oxychlorate, OCl⁻

fractional distillation of liquid air

- N can form 3 compounds: hydrides, oxides, oxoacid and each of them have their own specific preparation and properties

- Use brown ring test to test the presence of nitrate ion.

Phosphorus

has 3 types: white, red and black

red is more safety than white as it is more stable compared to white at room temperature

P can forms hydrides (phosphine), halide (trihalides and pentahalides), oxide (3 types refer to the oxidation state of P), oxoacid (also 3 types)

# data[].attributes.body
Thankyou dr for today and other pre-recorded class. This is my summary for group VA

-Most stable oxidation num: -3,+3,+5 (+3 become stable as we go down a group)

-3 ways to complete octet

-Accepting electron -> anion

-Sharing valence electron

-Releasing electron

-Valency- P->Bi – ns2np3nd0

-Bi only show coordination 3 & 6 (more metallic properties)

-N- NCl3 only valency of 3:sp3 (no d orbital)

Nitrogen

-Hydrides- NH3 (haber process), (dielectric constant low). (contrast to water)

-application: fertilizer, an explosive, bleach, deodorize

-Oxides- N2O(+1)- uses as an anesthetic & laughing gas, NO(+2)- Ostwald process, NO2(+4)- form a dimer & very toxic gas, N2O3(+3), N2O5(+5)

-Oxoacid- H2N2O2 (basic acid), HNO2 (weak acid), HNO3 (Ostwald process) (oxidation agent)

-Brown ring test (test for nitrates)

-Ammonium salt- all soluble except NH4ClO4

Phosphorus

-Allotropic forms – white (very toxic & reactive), red (moderate reactivity) & black (most stable P allotrope-sheet form like graphite)

-Hydrides- PH3- toxic gas, acting as ligand

-Halides- PX3- All PX3 exist from F to I

- PX5- PF5 (very strong lewis acid) & PCl5 (chlorination agent)

-Oxides- P4O6 (basic unit is P2O3)  & P4O10

-Oxoacid- lower acid- (H3PO2 & H3PO3) & higher acid- (H3PO4-H4P2O7) -(ionization occurred at -P-O- + H+)

-Application: P4 used as incendiary bombs, PH3- Holme’s signals & smoke screens

# data[].attributes.body
Thank you Dr. for the class for Group VA.

Summary of Group VA:
-nitrogen is non-metal and in gas form when it is in Room Temperature

-phosphorus is non-metal and in solid form when it is in Room Temperature

-will form X3- with only very electropositive compound.

-tends to share electrons with other element which is less reactive (covalent compound).

-will not form X5+ due to its very high IE and only occurs for Bi3+ and also Sb3+.

-In lab, nitrogen can be prepared by three different ways: heating ammonium nitrate, oxidation of ammonia with copper(II)oxide and also oxidation ammonia  with oxychlorate.

-In industry, nitrogen can be prepared by distillation of liquid air

- there is a few oxides for nitrogen such  as  N2O, NO,NO2,N2O3 and N2O5.

-we can prepare N2O by the decomposition of liquid ammonium nitrate

-we also can prepare NO by undergoing the OSTWALD PROCESS in industry. But for lab, we can prepare it by reaction between Cu and HNO3, Birkeland-Edye Reaction and also using NaNO3,Nal and H2SO4 to prepare a aqueous solution and using KNO3.KNO2 and Cr2O3 to prepare a dry solution.

-NO2 can be prepared by oxidizing NH3 in industry, and in lab heating Pb(NO3)2 and using Cu react with HNO3 also can get the NO2.

-also learnt about the different pH for different oxoacid of nitrogen such as H2N2O2, HNO2 and HNO3.

-nitrate can be tested out by brown ring test.

-ammonium salt are all soluble except for ammonium chlorate and ammonium carbonate.

-also learnt about the application of nitrogen gas such as used to preserve the freshness of the food etc.

-phosphorus got allotropy which is white, black and red.

-white phosphorus are solid/liquid if it is P4 and it is  gaseous when P2. It is a soft solid and flammable when exposed to air. So it usually kept in water. And it is poisonous and smells like garlic.

-red phosphorus is stable in air. It has no smell and no toxic. Used to make matches head.

-black phosphorus  is a good conductor of electricity. It is the most stable allotropy compare to the others. Its structure resembles graphite lattice.

- and also learnt about the halides which got trihalide and pentahalide, hydrides and also the oxides.

-there is two type of oxoacids for phosphorus which is lower acid, P(I) and P(III) which is reducing agent and also the higher acid, P(V) which is a oxidizing agent.

-also learnt about the application of phosphorus compound such as white phosphorus is used in military as an application in bombs which can actually burn the skin right through the bone.

# data[].attributes.body
-consist of non-metal,metalloid and metal element.
-3 ways to complete oc

# data[].attributes.body
Thank you Dr for your well explaination . Here are my summary :
GROUP VA
# nitrogen and phosphorus are non metal
# IE and electronegativity decrease as it goes down the group
# density, b.p and atomic/ionic radius increases down the group
# 3 ways to complete octet ( accepting e, sharing e and release e)

NITROGEN
# Can be prepared in lab ( heating NH4NO2, oxidation NH3 with CuO, oxidation NH3 with 3Ca(OCl)2)
#Physical properties ( colourless, odourless gas, as inert atmoshere)
# Chemical properties ( reacts at high temp and room temp)
# Can be form as ammonia using HABER process
# OXIDES ( dinitrogen oxide N2O)
- can be prepared by decomposition of liquid ammonium nitrate
- not reactive, alkali metals, ozone at room temp
- as anesthetic , aerosol propellant, Laughing gas
# Other N2O we have other oxides such as NO, NO2, N2O3, N2O5)
# NITROGEN OXOACID which are
- H2N2O2
- HNO2
- HNO3
# Application of N
- modified atmosphere
- pressurize kegs of some beers
- cryopreservation of blood

PHOSPHORUS
# Allotropic forms ( white, black, red)
# WHITE
- solid or liquid (P4) and gas(P2)
- flammable when exposed to air
- kept in water
- very toxic
- dissolve in CS2
# RED
- amorphous , dark red
- stable in air
- non toxic
- can make matches head
#BLACK
- sheet form like graphite
- good conductor
# PHOSPHORUS COMPOUND
- PH3
> toxic gas , colourless and smelly
> less soluble in water
> complexing agent
- PX3
> prepared by direct halogenation of P4 except PF3
> dissolve in water (PF3)
> weak base (PF3)
> colourless
- PX5
> catalyst for polymerization (PF5)
> very strong Lewis acid (PF5)
> dissolve in polar solvent (PCl5)
> easily attacked by OH compound  (PCl5)
# OXIDES OF P
- P4O6
> white solid
> dissolve in water
> stable towards O2 at room temp
- P4O10
.> prepared by burning white P in excess O2
.> react virgously with water
#OXOACID OF P
- 2 types ( lower and higher acid)
- form tetrahedral unit
- H3PO2
> known as hypophosphorus acid
> prepared by boiling white P in alkali
> monobasic acid
- H3PO3
> 2 types ( H3PO3 and H4P2O5)
> prepared by reacts with PCl3 or P4O6 with water
>pure solid and colourless
> strong reducing agent
-H3PO4
> 2 types (H3PO4 and H4P2O7)
> prepared in industry and lab
>tribasic acid
> very soluble in water
# Application of P
- used in military application
- used in Holme's signals
- used in smoke screens

# data[].attributes.body
Thankyou Dr for this topic videos.Here is my summary for group VA,
🌺As we go down the group +3 is more stable oxidation number
🌺3 ways to complete octet:
-accepting electron
-sharing valence electron
-releasing electron
NITROGEN
🦋forms multiple bonds while others do not
🦋Compounds of Nitrogen
1.HYDRIDE
-Ammonia,NH3
-Lab preparation (the reaction of base on ammonium halide salt,hydrolysis of an azide)
-In industry(Haber Process)
>Physical properties
-H bond formed in the molecule (FON)
>Chemical properties
-Reaction with metals➡azide
-Burn in oxygen with light green colour(without and with catalyst(Ostwald Process))
-Dissolved in water
2.OXIDE
-(N2O,NO,NO2,N2O3,N2O5)
-different in oxidation number
-colourless gas
-Liquid n2 as coolant
3.OXOACID
-H2N2O2,HNO2,HNO3
>H2N2O2
-Hyponitrous acid
-basic acid
>HNO2
-nitrous acid
-weak acid
>HNO3
-nitric acid
-In industry (Ostwald Process)
-Oxidation agent
4.AMMONIUM SALT
-all soluble except NH4CLO4,NH4CO3
-obtained from strong acid such as HCl etc

PHOSPHORUS
-[Ne]3s23p3
-There are 3 types of allotropes which is:
⚪White Phosphorus
-soft solid
-very reactive in air
-very toxic
-gas-P2
🔴Red Phosphorus
-Amorphous,dark red
-non-toxic
-Not glow in air
⚫Black Phosphorus
-Sheet form like graphite/metals
-A good conductor of electricity
-The most stable P allotrope
1.HYDRIDES
-Phosphine,PH3
-toxic gas,colourless,smelly
-10ppm,continuously breathing-die
-Trigonal pyramidal
2.HALIDES
-Phosphorus Trihalide,PX3
>PF3
-colourless gas
-toxic
-weak base
>PCl3
-colourless liquid
>PF5
-catalyst for polymerization
-very strong Lewis acid
>PCl5
-yellow solid
-dissolve in polar solvent
3.OXIDES
-P4O6,P4O7,P4O8,P4O9,P4O10
>P4O6
-white solid
-dissolve in water
>P4O10
-white powder
-react with water ➡ mixture of acids
4.OXOACID
-2 types
i.lower acid ,P(I) & P(II) as reducing agent
ii.higher acid,P(V)-oxidizing agent
-Ionization occured at P-O-H
>H3PO2
-colourless crystal
-monobasic acid ,pKa =1.2
>H3PO3(H3PO3,H4P2O5)
-pure solid
-deliquescence (absorb moisture from the atmosphere)
-dibasic acid
>H3PO4(H3PO4,H4P2O7)
-colourless solid
-tribasic acid

# data[].attributes.body
SUMMARY GROUP VA

- density, boiling point, atomic and ionic radii increase down the group

- IE and electronegativity decrease

- various oxidation number, +3 becomes stable down the group

- N can form multiple bonds

3 ways to complete octet

- accept electron, sharing electron, release electron

NITROGEN

- exist in air (78%), nitrate compound, amino acid

Preparation
- heating ammonium nitrate

-  oxidation ammonia with oxychlorate

- oxidation ammonia with copper (II) oxide

- fractional distillation of liquid air

Physical Properties
- Colourless gas, odourless

- inert (not easy to react with other element)

- liquid N₂ as coolant

COMPOUNDS

Hydrides

- Ammonia (NH₃)

Preparation
- base on aluminium halide salt

- hydrolysis of azide

- haber process

Physical Properties
- choking smell, colourless
- similar to water (H-bond form)

- low dielectric constant

- less ionic than water

- good solvent for organic compound

Chemical Properties
- Reaction with metals --> azide
- burn in oxygen --> light green colour

- dissolve in water to form ammonium hydroxide

- acid-base neutralization reaction

- cation hydrolysis of ammonium salt

- as reducing agent

Application
- Nitrogen fertilizer

- explosive material

- fibre and plastic

- bleach, deodorize

Oxides

N₂O (Nitrous acid)

Preparation - decomposition of liquid ammonium nitrate,

Properties
- Not reactive, inert towards halogen/alkali metals, ozone at room temperature

- decomposed to N₂ and O₂ on heating

- Assist on combustion

- very soluble in water

- React with alkali metals and organic compound

Uses
- anesthetics, easily soluble in water/body liquid

- aerosol propellant

- laughing gas

NO (Nitric oxide)

Preparation
- ostwald process

- reaction of Cu/HNO₃

- Birkeland-Eyde reaction

Properties
- Colourless gas (paramagnetic)

- solid/ liquid (dimagnetic)

- important for preparing nitric acid

NO₂ (Nitric dioxide)

- form a dimer , N₂O₄

- very toxic

- NO2 (paramagnetic)

- N₂O₄(dimagnetic)

Preparation - oxidation of ammonia

- thermal decomposition

Oxoacid

- contain O, H, N

- acid properties

- H₂N₂O₂, HNO₂, HNO3
H₂N₂O₂

- weak acid, stable in solution

Properties
- an oxidizing and reducing agent

- salt derivatives

- isoelectronic to ozone

HNO₃

Preparation - ostwald process

Properties
- volatile colourless liquid
- turn yellow due to presence of NO₂

- white solid

- undergo self-ionization

- oxidizing agent

- acid oxidizing catalyst

- nitrate salts soluble in water

Ammonium Salt

- All soluble in water except NH₄ClO, NH₄CO₃

- obtained from strong acid

- NH₄⁺ decomposed when heating

Application of Nitrogen

- as a modified atmosphere to preserve the freshness

- to pressurize kegs of some beers

- cryopreservation of blood to remove cyst

- laughing gas

- drugs

PHOSPHOROUS

Allotrope - white, red, black phosphorous

White Phosphorous
- soft solid, white

- solid / liquid, P₄ unit

- gas , P₂ unit

- flammable when exposed to air

- smell of garlic, very toxic

- dissolve in CS₄ and organic solvent

Red Phosphorous
- Physical properties depend on preparation method

- amorphous

- stable in air

- no smell/ non toxic

- used to make matching head

Black Phosphorous
- sheet form like graphite

- a good conductor of electric

- most stable allotrope

- resemble graphite lattice

COMPOUNDS

Hydrides (PH₃)

Preparation - pyrolysis of H₃PO₃

- heating of H₃PO₂/H₃PO₃

Properties
- toxic gas, colourless, smelly

- 10 ppm, continuously breathing cause to die

- less soluble in water, alcohol, ether

- act as ligand

Halides

- all PX₃ exist

- prepared by direct halogenation except PF₃

PF₃ - colourless gas

- form complexes with transition metal

- toxic, weak base, dissolve in water

- prepared by fluorination of PCl₃

PCl3 - colourless liquid

- prepared by direct halogenation

PF₅ - preparation by PCl₅ with calcium fluoride

- catalyst for polymerization

- very strong lewis acid

PCl5 - yellow solid

- prepared by direct chlorination

- dissolve in polar solvent

- easily hydrolyzed in water

- easily attacked by compound with OH group

- as chlorination agent

Oxide

Phosphorous (III) oxide, P₄O₆

- basic unit is P₂O₃ but stable as dimer

Preparation - Quantitative combustion

Properties - white solid, stable toward O₂ at room temperature, dissolve in water

Phosphorous (V) Oxide

Preparation - Burning white/ phosphorous (III) oxide in excess oxygen

Properties - white powder, react vigorously with water

Oxoacid

Types
- lower acid, P(I) & P (III) - reducing agent

- higher acid P(V) - oxidizing agent

Properties
- ionization occurred at P-O-H
- P atom form tetrahedral unit with p(pi)-d(pi) back bonding at P=O

Phosphoric (I) acid

Preparation - boiling white phosphorous in alkali or hydroxide alkali metal

Properties - colourless crystal, monobasic acid, free acid and its anion are strong reducing agent due to direct P-H bond

Phosphorous (III) acid (H₃PO₃, H₄P₂O₅)

Preparation - reaction of PCl3 or P₄O₆ with water

Properties - pure solid, deliquscence, dibasic acid, strong reducing agent in alkali/acid

Phosphorous (V) acid (H₃PO₄, H₄P₂O₇)

Preparation
- treating phosphate rock with sulfuric acid

- reacting phosphorous (V) oxide with hot water

Properties - Colourless solid, very soluble in water, tribasic acid

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

N, P - non-metal
As - metalloid
Sb, Bi - metal

Down the group:
- density increases
- size increases
- ionization energy decreases
- -3, +4, +5 (down the group +3 is more stable)

Ways to complete octet
- accept electron
- share valence electron
- release electron

NITROGEN
Preparation (Laboratory)
1. heat ammonium nitrate
2. oxidation ammonia with copper(II) oxide
3. oxidation ammonia with oxychlorate
Preparation(Industry)
1. Fractional distillation of liquid air

Hydride
NH3

Oxide
N2O
NO
NO2
N2O3
N2O5

Oxoacid
H2N2O2
HNO2
HNO3

Ammonium salt

Uses of N
- preserve the freshness of food
- pressurize kegs of some beer
- cryoperservation of blood, reproductive cells
- anesthetic (laughing gas)
- drug

PHOSPHORUS
Allotrope
- White
- Red
- Black

Hydride
PH3

Halide
PX3
PX5

Oxide
P4O6
P4O7
P4O8
P4O9
P4O10

Oxoacid
H3PO2
H3PO3
H3PO4

Uses of P
- incendiary bomb
- smoke-screening
- smoke bomb
- tracer ammunition
- Holme's signal

# data[].attributes.body
Thank you Dr for today’s lesson. This is my summary for GroupVA (The Pnictides Group)
-Metallic character,density boiling point,atomic and ionic radius increases down the group
3 ways to complete octet : Accepting electron, sharing valence electron, releasing electron.
NITROGEN
Preparation- Heating ammonium nitrite solution, oxidation of ammonia with copper (II) oxide, oxidation of ammonia with oxychlorate (chlorate(I) ion), fractional distillation of liquid air (industry)
COMPOUNDS OF NITROGEN
Hydrides (Ammonia, NH3)
Lab preparation - Reaction of base on ammonium halide salt, hydrolysis of an azide
Industry – Haber process
Physical properties - similar to water (H-bond formed in molecule),dielectric constant low (less ionic than water , good solvent for organic)
Applications – nitrogen fertilizer, organic chemicals, an explosive for plastic and fiber, bleach and deodorize
Oxides (NO)X
N₂O
-not reactive, decompose to N₂ and O2 on heating, very soluble in water, reacts with alkali metals and organic compounds
Application – an anesthetic , aerosol propellent , laughing gas
NO

-OSTWALD PROCESS (industry)
- colourless gass(paramagnetic), solid/liquid(diamagnetic), importand for preparing nitric acid from oxidation of ammonia.

Nitrogen oxoacid

-Nitric(I) acid , Nitric(III) acid, nitric(IV) acid
Applications of nitrogen compounds
modified atmosphere of packaged or bulk foods, pressurize kegs of some beers, cropreservation of blood, reproductive cells, laughing gas , antibiotics.

PHOSPHORUS
Allotrophic
1)White phosphorus
-P₄ , glow when exposed to air. Kept in water. Very toxic
2)Red Phosphorus
-Stable in air,non-toxic
3) Black phosphorus
-Good conductor of electricity
COMPOUNDS
1)Hydride
-phosphine
Toxic gas, smelly, less soluble in water bsc no hydrogen bond, melting point lower than NH₃,
-acting as ligand but weaker than NH₃
-PX3
-act as ligand, toxic because forms complex with iron (Fe) in hemoglobin which is disturb the O2
-PX5
2)Halide
-trihalide- prepared by direct halogenation of P₄
-pentahalide – very strong lewis acid
3)Oxide
Prepared by quantitative combustion
4)Oxoacid
2 types – Lower (reducing agent) and higher (oxidizing agent)
Applications
-white phosphorus , as incendiary bomb
-phosphine , smoke screens
-holme’s signals

# data[].attributes.body
Summary for Group VA:
NITROGEN
1. 3 ways to complete octet :
i) accepting electron (occurs with very electropositive metal)
ii) sharing valence electron
iii) releasing electron
2. Preparation :
i) heating ammonium nitrite solution.
ii) oxidation ammonia with copper(II) oxide.
iii) oxidation of ammonia with chlorate(I)
iv) fractional distillation of liquid air.
3. Nitrogen Compounds-HYDRIDES
-Preparation :
i) The reaction of base on ammonium halide salts
ii) hydrolysis of an azide
iii) Haber Process(industrial manufacture of NH3)
4. Nitrogen Compounds-OXIDES
i) Dinitrogen oxide
ii) Nitrogen monoxide
iii) Nitrogen dioxide
iv) Dinitrogen trioxide
v)Dinitrogen pentoxide
5. Nitrogen Compounds-OXOACID
i) Nitric(I) acid
ii) Nitric(III) acid
iii) Nitric(V) acid
-Using brown ring test (depends on the ability of Fe2+ to reduce nitrates to nitric oxide)
6. Nitrogen Compounds-AMMONIUM SALT
-all soluble except NH4ClO4
-salts obtained from strong acid
7. Application :
-preserve freshness
-pressurize kegs of some beers
-laughing gas
-cryopreservation blood

PHOSPHORUS
1. Allotropes of phosphorus are white, red and black.
2. Phosphorus Compounds-HYDRIDES
-PH3 is extremely dangerous gas
-All PX3 prepare by direct halogenation of PF4 except PF3
-PF5 is strong Lewis acid
-PCl5 prepare by direct chlorination
3. Phosphorus Compounds-OXIDES
- Exist : P4O6, P4O7, P4O8, P4O9, P4O10
- H4P2O5 is formed when H3PO3 and H3PO4 undergoes dehydration
4. Application :
-WP used in military applications
-Holme's signals
-Phosphine used in smoke screens

# data[].attributes.body
Group VA
- Non-metal to metal down the group
- most stable oxidation numbers: -3, +3, +5 (+3 most stable down the group)
- 3 ways to complete octet:
1. Accept e⁻ (with very electropositive metal)
2. Sharing val. e⁻ (with less reactive metals/non-metals, except Bi)
3. Release e⁻ (only X³⁺, Bi & Sb)
- N = sp3 (no d-orbital), others can expand.

Nitrogen
- Lab Prep: heat NH₄NO₂ sol., oxidation of NH₃ with CuO, oxidation of NH₃ with Ca(OCl)₂
Ind. Prep: Fractional distillation of air
- Phys. Prop.: colourless, odourless, inert
- Chem. Prop.: react with H₂ & O₂ at high temp, react with Li at room temp.
- Hydrides
Lab Prep.: react base on ammonium halide salt, hydrolysis of an azide
Ind. Prep.: Haber Process (by Fritz Haber for bombs in WWII)
Phys. Prop.: choking smell, colourless, low BP, similar phys. prop. to H₂O, low dielectric constant (less ionic than H₂O, good solvent for organic comp.)
Chem. Prop.: react with metals, burn in O₂ with light green colour, dissolves in water forms ammonium hydroxide, acid-base neutralization, cation hydrolysis of ammonium salt, reducing agent, decomposes on heating
App.: fertilizer, form organic chemicals, explosive, clean, bleach, deodorize, etch aluminium, saponify oils & fats
- Oxides
N ₂ O
Prep.: decomposition of liquid ammonium nitrate
Prop.: not reactive. inert to halogen, alkali metals & ozone at rtp. decomposed on heating. assist combustion. very soluble in H₂O. reacts with alkali metals & organic comp.
Uses: anesthetic, aerosol propellant, laughing gas
NO
Ind. Prep: Ostwald Process
Lab Prep: reaction of Cu/HNO₃, preparation for pure NO (aqueous or dry), Birkeland-Eyde Reaction (not suitable for commercialization)
Reacts with multiple chemicals
Prop.: colourless gas = paramagentic, solid/liquid = diamagnetic, important for preparing nitric acid
NO ₂
Forms dimer = N₂O₄, at low temps., changes brown-orange to colourless
Very toxic
Monomer = paramagnetic, Dimer = diamagnetic
Ind. Prep.: NH₃ Oxidation
Lab Prep.: heat Pb(NO₃)₂, react HNO₃ with Cu
Reacts with multiple chemicals
Nitrogen Oxoacid (H ₂ N ₂ O ₂, HNO ₂, HNO ₃)
Acid prop.
H₂N₂O₂: basic acid, stable in sol., aka. hyponitrous acid
HNO₂: weak acid, stable in sol., aka. nitrous acid, oxidizing & reducing agent, isoelectronic to O₃ & FNO
HNO3: aka. nitric acid, Ostwald Process, volatile, turns yellow under the light, oxidizing agent, acid oxidizing catalyst, nitrate salts soluble in water except anhydrous Cu(NO₃)₂
- Brown Ring Test for nitrates
- Ammonium salt: all soluble except NH₄ClO₄, NH₄CO₃, salts obtained by reacting with strong acids, decomposed when heating
-App: modified atmosphere for preservation, pressurize kegs, LN₂ - cryogenation, N₂O - aneshetic, drugs & antibiotics.

Phosphorus
- White, Black, Red.
- White: soft white solid, P₄ - solid/liquid, P₂ - gas, flammable & glows (phosphorescence), toxic, garlic odour, dissolves in CS₂, P₄ reacts with multiple chemicals
- Red: phys. prop. depend on prep., amorphous, stable in air, no smell, non-toxic, non-phosphorescence, made into match heads and flame retardant materials
- Black: sheet form like graphite, good conductor of electricity, most stable
- PH ₃: reacts with multiple chemicals, toxic (fatal), colourless, smelly, less soluble in water, alcohol & ether, low MP, similar struc. to ammonia, acts as ligand but weaker than NH3
- PX3 (halide)
All exist
Direct halogenation (Cl -> I)
Fluorination of PCl₃ (F)
PF ₃
colourless gas, form complex with trans. metal, toxic, weka base, dissolves in water,
PCl ₃
colourless liquid
PF ₅
Prep.: react PCl₅ with CaF₂
Catalyst for polymerization
Very strong Lewis Acid
PCl ₅
Yellow solid, trigonal bipyramid (liquid & gas state)
Prep.: direct chlorination
Dissolves in polar solvent
Easily hydrolysed
Easily attacked by comp. with OH group
Chlorination agent
- Oxides
Exist: P₄O₆, P₄O₇, P₄O₈, P₄O₉ & P₄O₁₀
P ₄ O ₆ (P ₂ O ₃)
Stable as dimer
Prep.: Quantitative combustion
Prop.: White solid, stable towards O₂ at room temp., dissolves in water
P₄O₁₀
Prep.: Burn white phosphorus or phosphorus (III) oxide
Prop.: white powder, react vigorously with H₂O
- Oxoacid
2 tyes: lower (P(I) & P(III) - red. agent) & higher (P(V) - oxi. agent)
Prop.: ionization occurs at ~P-O-H
H ₃ PO ₂
aka. hypophosphorous acid
prep.: boil white phosphorus in alkali or hydroxide of Group IIA
prop.: colourless crystal, monobasic acid, free acid & anion - strong red. agent
H ₃ PO ₃
2 types: H₃PO₃ aka. phosphoric acid & H₄P₂O₅ aka. diphosphoric acid
Prep.: react PCl₃ or P₄O₆ with H₂O
Prop.: pure solid, colourless, deliquescence, 2 type of phosphite salts, strong red. agent.
H ₃ PO ₄
2 types: H₃PO₄ aka. phosphoric(V) acid & H₄P₂O₇ aka. diphosphoric(V) acid
Ind. Prep.: treating phosphate rock with sulfuric acid
Lab Prep.: react phosphorus(V) oxide with hot water, oxidizing phosphorus with conc. nitric(V) acid
Prop.: colourless solid, very soluble in water, tribasic acid
- Application
White phsophorus - military application (bombs)
Holme's signals

# data[].attributes.body
Summary of Group AV
Nitrogen
1)Exist in two state of elements in RT(gas, solid)
2)Density decreases going down the group
3)IE, Electronegativity decreases down the group
4)3 ways to achieve complete octet are accepting electrons, sharing valence electron and releasing electrons
5)Preparations of nitrogen(In Laboratory)
-heating ammonium nitrite solution
-oxidation of ammonia with copper(II) oxide
-oxidation of ammonia with oxychlorate( chlorate(I) ion)
Industry
-Fractional distillation
6)Ammonia is prepared by
-reaction of base on ammonium halide salt
-hydrolysis of azide
Industrial(Haber process)
7) Chemical properties are such as it reacts with metal, burn in oxygen and dissolves water to form ammonium hydroxide.
8)Oxides of nitrogen are (N20, NO,NO2,N2O3&N2O5)
9)Three nitrogen oxoacids are (H2N2O2, HNO2,HNO3)

Phosphorus
1)3 types of phosphorus which are white, red and black
White phosphorus
-soft solid, white gas at P2
Solid/Phosphorus-P4 unit
-Flammable when exposed to air it glows
Red Phosphorus
-Physical properties depends on preparation methods
-Amorphous, dark red
-Stable in air
Black Phosphorus
-Sheet form like graphite
-A good conductor of electricity
The most stable P allotrope
2) Hydride of phosphorus is phosphine(PH3)
3)Halides of phosphorus are such as phosphorus trihalide, pentahalide (PX3, PX5)
4)Oxides of phosphorus are phosphorus(III) oxide, phosphorus(V) oxide(P4O6,P4O10)
5)For oxoacids there are two types which is lower (reducing agent) and higher(oxidizing agent)

Thank your for the lecture dr!

# data[].attributes.body
Thanks Dr. for  the videos of Group VA. Here are some summary for group VA
Group IV
- physical properties: density increases, while IE, electronegativity decreases as go down the group
-3 ways to get octet: accepting electron, sharing valence electron, releasing electron

NITROGEN
- preparation: heating ammonium nitrite, oxidation of NH3 with CuO, oxidation of NH3 with Ca(OCl) or fractional distillation of liquid air in industrial
-physical properties: colourless, odourless gas
COMPOUND
• hydride
- NH3
- preparation: reaction of base on ammonium halide, hydrolysis of an azide and haber process
-physical properties: choking smell, colourless, similar to water
-chemical properties: react with metal form azide, burn in O2 with light green color, dissolve in water
- application: fertilizer, used as an explosives,
• oxides
1. N2O
- preparation: decomposition of NH4NO3
- properties: not reactive, soluble in water
-use: anesthetic, aerosol propellant, laughing gas
2. NO
- preparation: ostwald process in industrial
- properties: colourless gas (paramagnetic), solid/liquid (diamagnetic)
3. NO2
- form a dimer, very toxic gas
-preparation: NH3 oxidation in industrial
• oxoacid
- contain O,H,N and acid properties
1. H2N2O2
- bacis acid, stable in solution
2. HNO3
- weak acid, stable in solution
-properties: oxidizing agent, reducing agent
3. HNO3
-preparation: ostwald process in industrial
- properties: volatile colourless liquid, turn to yellow when NO2 presence
Application: pressurize kegs of beer, cryopreservation of blood, laughing gas

Phosphorus
-physicochemical properties: soft solid, white, flammable when exposed to air
-physical properties: amorphous, dark red, stable in air
-Reaction: react with H2O to form phosphoric acid, with O2 to form phosphorus trioxide
Black phosphorus
- sheet form like graphite, good conductor, most stable P
COMPOUND
• phosphine
- preparation: phosphorus acid (pyrolysis), also can react with H3PO2
-properties: toxic gas, colourless, smelly
-reaction: react with O2 or N2O can form explosion
• phosphorus trihalide
- can exist from F to I
-prepared by direct halogenation of P4 except PF3
- colourless gas, toxic, weak base
•phosphorus pentahalide
- preparation: PCl5 react with CaF2
- very strong lewis acid
• oxides
- P4O6
- preparation: quantitative combustion
-properties: white solid, dissolve in water
-P4O10
- preparation: burning P4 in excess O2
-properties: white powder, react with water
• oxoacid
-2 types: lower acid, higher acid
- general properties: form tetrahedral unit
- H3PO2: prepared by boiling P4 in alkali/hydroxide of alkaline earth metal
- H3PO3: prepared by reaction of PCl3/ P4O6 with water
-H3PO4: prepared in industry by treating phosphate rock eith H2SO4

# data[].attributes.body
Summary Group VA
-consist of non-metal,metalloid and metal element.
-3 ways to complete octet:
`accepting elctron and become anion
`sharing valance electron
`releasing electrons and become cation

NITROGEN
-preparation:
`heating ammonium nitrite solution
`oxidation ammonia w copper(II)oxide
`oxidation of ammonia with oxychlorate
`in industry= fractional distillation of liquid air
-physical property:
cololess,odourledd,inert,very low boiling and melting point
-hydrides: ammonia
laboratory preparation:
`reaction of base on ammonium halide salt
`hydrolysis of an azide
industrial manufacture of ammonia : haber process
-physical properties of ammonia:
choking smell,colorless,low b.p.,physical properties similar to water,less ionic than water,good solvent for organic compounds
-chemical properties:
`reaction with metals form azide
`burn in oxygen w light green color
`dissolve in water form ammonium hydroxide
`acid-base neutralization reaction
`cation hydrolysis of ammonium salt
`acting as reducing agent
`ammonium salts decomposed on heating
-oxides of notrogen:
`dinitrogen oxide,N2O
-preparation :by decomposition of liquid ammonium nitrate
-properties:not reactive,inerts towerds halogen,alkali metals and ozone at room temperature,assist combustion,very soluble in water,react w alkali metals and organic compound
`nitric oxide,NO:
-preparation:
-industry:ostwald process
-lab:reaction of Cu/HNO3,preparation for pure NO,Birkeland-eyde reaction
`nitric dioxide,NO2:
-form dimer,N2O4
-veru toxic
-preparation,
`industry:NH3 oxidation
`Nitrogen oxoacid:
-compound containing O,H,N
-acid properties
*nitric acid:stable in solution,hyponitrous acid
*Nitric (III)acid,HNO2:
-nitrous acid,weak acid,stable in solution
-properties:oxidizing agent,reducing agent,salt derivatives
*nitric (V)acid,HNO3:nitri acid
-preparation:industry:ostwald process
-properties:volatile colorless liquid,white solid,self-ionization process,oxidation agent,acid oxidizing catalyst
-brown ring test
`ammonium salt
-all soluble except NH4ClO4,
-salt obtained from strong acid
-NH4 decompose when heating

PHOSPHORUS
-allotropic forms
`white phosphorus:
*soft solid,white,solid/liquid-P4,gas-P2,flammable when exposed to air it glow become P4O6,toxic
`red phosphorus
-physical properties depend on method
-amorphous,dark red
-stable in air,no smell,nontoxic,non-phosphorescence
`black phosphorus:
-sheet form like graphite/metal
-good conductor of electricity,most stable P allitrope
`phosphine,PH3
-properties:toxic gas,colorless,smelly,less soluboe in water ,alcohol an ether,low melting point than NH3,structure similar to ammonia
`phosphorus trihalide,PX3
-all PX3 exist
-prepaired by direct halogenation of P4 except PF3
`phosphorus pentahalide,PX5
-catalyst for polyrization
`oxide phosphorus
-phosphorus (III) oxide,P2O3
*properties:white solid,stable toward O2,dissolve in water
-phosphorus (V)oxide:
*preparation:burning white phosphorus or phosphorus (III)oxide in excess oxygen
*prperties:white powder,react vigorously with water
`oxoacid of phosphorus
-lower acid;P(I) and P(III)-reducing agent
-higher acid,P(V)-oxidizing agent
-general property:all acid,ionized occured at ~P-O-H
-P atom form tetrehedral unit
-phos phosphoric (I) acid,H3PO2
`known as hypophosphorus in alkali or hydroxide of alkaline earth metal
`properties:colorless crystal,monobasic acid,free acid and its anion are strong reducing agent due to direct P-H BOND
-PHOSPORUS (III) acid,H3PO3
`H3PO3 and H4P2O5
`properties :pure solid,dibasic acid
-phosphoric acid,H3PO4:W
`H3PO4 and H4P2O7
`properties:colorless,soluble in water,tribasic acid.

thank you dr!

# data[].attributes.body
Summary for group VA
~NITROGEN~
1. There are 3  ways to complete octet:
i) accepting electron become anion (X3-) but only occur with electropositive metal from group 1A, IIA
ii) sharing valence electron
iii) releasing electron become cation (X3+)

2. only N has hybridization on sp3 while P to Bi has hybridization of sp3d because they has d orbital.

3. preparation on N :
i) in laboratory
- heating ammonium nitrate solution
- oxidation of ammonia with copper(II) oxide
- oxidation of ammonia with oxychlorate
ii) in industry
- fractional distillation of liquid air

4. nitrogen compound
- hydride ( ammonia)
- oxide ( N20, NO, NO2)
- oxoacid (H2N2O2, HNO2, HNO3)

5. application
- preserve the freshness of packaged or bulk food
- preserve kegs of beer
- used in clinical setting in cryotherapy
- anesthetic

~PHOSPHORUS~
1. there are 3 type of phosphorus
i) white phosphorus (P4)
- has odour
- poisonous
- highly reactive
- show phosphorescene
- soluble in CS2
ii) red phosphorus
- odourless
- non poisonous
- less reactive
- does not show phosphorescene
- insoluble in CS2
iii) black phosphorus
- good  conductor of electricity
- the most stable P allotrope

2. phosphorus compound
i) hydride ( phosphine, PH3)
ii) halide ( phosphorus trihalide, PX3 and phosphorus pentahalide, PX5)
iii) oxide ( phosphorus (III) oxide, P4O6 and phosphorus (V) oxide, P4O10)
iv) oxoacid ( phosphoric(I) acid, H3PO2 / phosphoric (III) acid, H3PO3 / phosphoric acid, H3PO4.

3. application of phosphorus compound
- white phosphorus used in military application as incendiary bomb
- spontaneous combustion of phosphine is used in Holme's signals
- phosphine used in smoke screen

# data[].attributes.body
Thankyou dr for today's explanation. Here are my summary for group VA
NITROGEN
Preparation
1.Heating ammonium nitrite solution
2.Oxidation of ammonia with copper(II) oxide
3.Oxidation of ammonia with oxychlorate
4. Fractional distillation of liquid water
Physical properties
-colourless , odourless
-inert
Hydrides
1. Preparation
- Reaction of base on ammonium halide salt
- Hydrolysis of an azide
2. Ammonia
-chocking smell , colourless
-physical properties similar to water
3. Reaction
o Reaction with metals to form azide
o Burn in oxygen with light green colour
o Dissolved in water to form ammonium hydroxide
4. Application Ammonia
-produced fertilizer
-formation of organic chemicals
-used as an explosive
Oxides of Nitrogen
1. Dinitrogen oxide
2. Nitric oxide
3. Nitric dioxide
4. Dinitrogen trioxide
5. Dinitrogen pentoxide
Nitrogen Oxoacid
1. Nitric acid
2. Nitric(III) acid
3. Nitric (IV) acid
Brown Ring test
-depends on ability of Fe2+ to reduce nitrates to nitric oxide
Application Nitrogen
-preserved freshness
- to pressurize kegs of some beers
- used in cryopreservation of blood
- used in laughing gas
PHOSPHOROUS
1. White Phosphorous (P4)
- Flammable when exposed to air
-smell in garlic , very toxic
2. Red Phosphorous
- Stable in air
- Non toxic
3. Black Phosphorous
- Most stable
- Good conductor of electricity
4. Phosphine (PH3)
- Toxic gas
-colourless , smelly
5. Phosphorus trihalide(PX3)
- prepared by directed halogenation
-colourless
-toxic gas
6. Phosphorous pentahalide (PX5)
-PCl5
o yellow solid
o prepared by direct chorination
o easily hydrolysed in water
o easily attacked by compound OH group
7 . Oxide Phosphorus
a) Phosphorus(III) oxide
-white solid
- dissolves in water
b) Phosphorus (V) oxide
-white powder
-react fast with water
8. Oxoacid phosphorus
a) Phosphoric (I) acid (H3PO2)
-colourless
-monobasic acid
b) Phosphoric (III) acid ( H3PO3)
-pure solid
-dibasic acid
c) Phosphoric acid (H3PO4)
-colouless basic
-tribasic acid