brown liquid

violet solid

Ionic Bonding Group 1 and 17 Gp 1 Metal

2.1

2.8.1

2.8.8.1

2.8.8.18.1

Na

Li

K

Rb

Click here video on NaCI

yellow gas

greenish gas

Ionic bonding between metal and non metal

Metal • Low EN value • Lose electron (cation) • Electropositive ions

Non metal • High EN value • Gain electron (anion) • Electronegative ions

2.8.1 2.8.7

Gp 17 Non metal

transfer electron

2.8 2.8.8

achieve stable octet structure

+ -

Na+ CI- Electrostatic force attraction

bet opposite charge ions

Crystal lattice structure • +/- ion attract/ arranged in orderly manner • arrangement in 3D shape • strong electrostatic forces attraction bet opposite charged ions

Reaction bet sodium with chlorine

Crystal lattice structure

violet solid

brown liquid

Gp 2 Metal 2.2

2.8.2

2.8.8.2

2.8.8.18.2

Mg

Be

Ca

Sr

Click here simulation ionic bonding

yellow gas

greenish gas

Ionic bonding between metal and non metal

Metal • Low EN value • Lose electron (cation) • Electropositive ions

Non metal • High EN value • Gain electron (anion) • Electronegative ions

2.8.2 2.7

Gp 17 Non metal

transfer electron

2.8

achieve stable octet structure

Mg2+ F-

Electrostatic force attraction

bet opposite charge ions Crystal lattice structure

Crystal lattice structure • +/- ion attract/arrange orderly manner • arrangement in 3D shape • strong electrostatic forces attraction bet opposite charged ions

2.8. 8 2.8

F-

Cations/Metals/+ve ions

Gp1 Gp 2 Gp3 Transition metals ions ( variable oxidation states)

Oxidation state

+1

Oxidation

state

+2

Oxidation state

+3

Sc +3

Ti +2 +3

V +2 +3

Cr +2 +3 +6

Mn +2 +3 +6 +7

Fe +2 +3

Co +2 +3

Ni +2

Cu +1 +2

Zn +2

Li 1+ Be2+ Sc 3+ Ti 2+

Ti 3+

V 2+

V 3+

Cr 2+

C r3+

Cr6+

Mn 2+

Mn 3+

Mn 6+

Mn 7+

Fe 2+

Fe 3+

Co2+ Ni2+ Cu1+

Cu2+

Zn2+

Na 1+ Mg2+ Al 3+

K 1+ Ca2+

Anion/Non metal

Gp 5 Gp 6 Gp 7

Oxidation state

Oxidation state

Oxidation state

-3 -2 -1

N3- O2- F-1

P3- S2- CI-1

Br-1

I-1

Metal/Cations/+ve ion

Non Metal/ Anions/ -ve ion

Ionic Compound

Li2O MgCI2 Al2O3 FeO NiO CuO

Li3N Mg3N2 AlN Fe3N2 Ni3N2 Cu3N2

Oxidation state/Charge ion → Li1+ O2-

Formula compound Li

2 O

1

Video on polyatomic ions

Writing Chemical Formula Ionic Compounds

Step 1 : Write Oxidation state/charge

Step 2 : Balance it, (electrically neutral)

by cross multiply – as subscript

Polyatomic ions

Group of non-metals bonded together

Oxidation state

Oxidation state

Oxidation state

-1/+1 -2 -3

(OH)-1

Hydroxide (SO4)2-

Sulphate (PO4)3-

Phosphate

(CN)-1

Cyanide (SO3)

2-

Sulphite

(SCN)-1

Thiocyanate (CO3)

2-

Carbonate

(NO3)-1

Nitrate (S2O3)

2-

Thiosulphate

(NO2)-1

Nitrite (Cr2O7)

2-

Dichromate

(NH4)+1

Ammonium

Polyatomic ions

Li2(CO3) Mg(CO3) Al2(CO3)3 Fe(CO3) Ni(CO3) Cu(CO3)

Li(OH) Mg(OH)2 Al(OH)3 Fe(OH)2 Ni(OH)2 Cu(OH)2

Li2(SO4) Mg(SO4) Al2(SO4)3 FeSO4 Ni(SO4) Cu(SO4) Video on polyatomic ions

Ionic Compound

Metal/Cations/+ve ions

Cations/Metals/+ve ions

Gp1 Gp 2 Gp3 Transition metals ions ( variable oxidation states)

Oxidation state

+1

Oxidation

state

+2

Oxidation state

+3

Sc +3

Ti +2 +3

V +2 +3

Cr +2 +3 +6

Mn +2 +3 +6 +7

Fe +2 +3

Co +2 +3

Ni +2

Cu +1 +2

Li 1+ Be2+ Sc 3+ Ti 2+

Ti 3+

V 2+

V 3+

Cr 2+

C r3+

Cr6+

Mn 2+

Mn 3+

Mn 6+

Mn 7+

Fe 2+

Fe 3+

Co2+ Ni2+ Cu1+

Cu2+

Na 1+ Mg2+ Al 3+

K 1+ Ca2+

Oxidation state/Charge ion → Li1+ (CO3)2-

Formula compound Li

2 (CO

3)1

Step 1 : Write Oxidation state/charge ion

Step 2 : Balance it, (electrically neutral)

by cross multiply – as subscript

Writing Chemical Formula Ionic Compounds

Acids Alkali Metal Hydroxide

Metal oxides Salts Gas

HCI Hydrochloric acid

KOH Potassium hydroxide

CuO Copper(II) oxide

CaCO3

Calcium carbonate CO

Carbon monoxide

HNO3

Nitric acid NaOH

Sodium hydroxide MgO

Magnesium oxide Na2CO3

Sodium carbonate CO2

Carbon dioxide

H2SO3

Sulphurous acid Ca(OH)2

Calcium Hydroxide ZnO

Zinc oxide NaHCO3

Sodium bicarbonate SO2

Sulphur dioxide

HCOOH Methanoic acid

NH3

Ammonia Na2O

Sodium oxide KNO3

Potassium nitrate SO3

Sulphur trioxide

CH3COOH Ethanoic acid

Mg(OH)2

Magnesium hydroxide Al2O3

Aluminium oxide Pb(NO3)2

Lead (II) Nitrate NO2

Nitrogen dioxide

H3PO4

Phosphoric acid Cu(OH)2

Copper (II) hydroxide Fe2O3

Iron(III) oxide NaNO3

Sodium nitrate CH4

Methane

H2CO3

Carbonic acid Al(OH)3

Aluminium hydroxide K2S

Potassium sulphide PbI2

Lead (II) nitrate H2S

Hydrogen sulphide

HNO2

Nitrous acid Fe(OH)2

Iron (II) hydroxide PbS

Lead(II) sulphide AgCI

Silver chloride O2

Oxygen

HF Hydrofluoric acid

Fe(OH)3

Iron (III) hydroxide ZnS

Zinc sulphide MgSO4

Magnesium sulphate N2

Nitrogen

HCIO Hypochlorous acid

Zn(OH)2

Zinc hydroxide AI2S3

Aluminium sulphide Na2S2O3

Sodium thiosulphate CI2

Chlorine

Chemical Formula for common chemicals

Naming chemical compound Writing chemical formula Writing chemical formula

VIDEO TUTORIALS

violet solid

brown liquid

Click here simulation on covalent bond

yellow gas

greenish gas

Covalent bonding between non metals

2.8.7

Gp 17 Non metal

achieve stable octet structure

CI shared pair electron

Covalent Bonding Electrostatic forces attraction between nucleus with shared pair electron

2.8.8

2.8.7

Sharing

electron

Gp 17 Non metal

2.8.8

CI

Non metal • High EN value • Gain electron (anion) • Electronegative ions

Covalent Bond Group 17

CI CI

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

CI CI : x

x

: :

: .

x

x

X

x

x

x

x CI CI

: : x

x

x

x

CI CI

Non metal • High EN value • Gain electron (anion) • Electronegative ions

Single covalent bond – shared pair electron

Covalent bonding between non metals

Covalent Bonding Single covalent bond ONE pair shared e

2.8.8 2.8.8

Covalent Bond

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

CI CI : x

x

: :

:

: .

x

x

X

X

x

x

x

x

x

x

O

CI CI :

: x

x

x

x

x

x

CI CI

Sharing

electron

Bond Strength

2.8 2.8

Sharing

electron

O O : x

x O

N

O O

N :

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

C

: : . N N : N N

:

Covalent Bonding Double covalent bond TWO pair shared e

Covalent Bonding Triple covalent bond THREE pair shared e

O x

x : C O C O O O O

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

Covalent Bonding Double covalent bond TWO pair shared e

:

CI . .

x

Bond Bond order

Bond strength

Bond length/pm

C - C 1 347 154

C = C 2 612 134

C Ξ C 3 820 120

N - N 1 159 145

N = N 2 418 123

N Ξ N 3 914 110

Bond length and Bond strength

Bond length = 0.199nm

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

CI CI : x

x

: :

:

: .

x

x

X

X

x

x

x

x

O

CI CI :

: x

x

x

x

x

x

CI CI

O O : x

x O

N

O O

N :

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

Lewis structure/diagram . Electron cross dot . Valence/bonding pair electron

O

: : .

N N : N N

Triple bond > Double bond > Single bond

Bonding pair e -involve in bonding

Bond length decrease

Bond strength Increase (Double/Triple bond)

Bond length = 0.121nm

Bond length = 0.110nm

Bond order up – Bond strength up – Bond length down

O

Non bonding pair

(Lone pair electron)

Bonding

pair electron

C O : :

Bonding pair electron

Dative bond

(electron pair of oxygen)

Types of bonding

Lone pair e –not involve in bonding

Dative/coordinate bond - pair e come from an atom

Exception to octet rule

All period 2 element - observe octet rule except Be and B

Electron deficient Less than 8 valence e

Expanded octet More than 8 valence e

All period 3 element - observe octet rule except P and S

: Be CI CI

x . :

: :

: :

. X

x .

Be - 4 valence e

B CI CI : : : :

: :

x

: : B - 6 valence e

P S

CI

CI

CI

CI

CI

CI

CI CI

CI CI CI

P - 10 valence e

S – 12 valence e

O

O N O C

N

C Be H N

B

X

x

C S S O

Linear

O C H H N O N O

Trigonal planar

C O O C H N H H Be C N N O O : x

x

X

x

X

x

X

X

X

X

X

X

X

x

X

x

+

+

: :

.

F

F

F

Electron deficient Be

Dative bond from N

N C x

x : Electron deficient N

(7 valence electron)

H

H O O

O O

O O

C

O O

O

O N

O

O

B X F

F

F C

H

H

x

x

O S

O O S

O O : : :

: :

O

C O

x

x

O N

2- -

2-

O

:

: :

x

x

O

:

: :

O

-

Electron deficient B

O

S

O

: :

O : :

: :

Dative bond from S

:

O N

O

O

:

:

-

O X

X

|| ||

Sulphur

expanded octet

(12 valence electron) ✓

BF3 CH2 O SO3 CO3 2- NO3

-

CO2 HCN BeH2

CN - NO2 + NO

::

X

X

X

X

Dative bond from N

O

O O

O

O O

: :

N

:

:

O O

O

N

O

S

O O

O O S

:

S

O O

O O S

: :

N

O O

N O O

-

-

O O N

O O

N

: -

Dative bond from N electron deficient N

(7 valence electron)

S

O O :

:

Sulphur

expanded octet

(10 valence electron)

or

or

Dative bond from S

NO2- NO2 SO2 O3

O

H H

H2O

H H

O

O

F2O

F F

F F

O

S

CI CI

SCI2 SH2

S

H H

S

CI CI

S

H

NH2 -

N

H H

H H

N

-

-

H : : : : :

: : : :

: :

All molecule – octet rule

Bend

Bend

O

O

:

O

Dative bond from O

||

:

S

CI

Sulphur

expanded octet

(12 valence electron)

C

H H

CH4 NH4+

N

BH4- PCI4

+ POCI3

P

CI - +

Tetrahedral

H

H

H

H H

H

B

H

H H H CI

CI CI

+

P

O

CI CI CI

C

H

H H

H

H

N

H H

H

+

H

B H

H H

- CI

P CI

CI CI

+

:

:

:

:

:

: : :

: :

:

:

O

::

P

CI CI :

:

: :

:

: : :

O

SO42-

O O

O

O

S

O

::

O

||

O

H2SO4 H3PO4

CIO4 -

|| O

S O

S

O

O

::

O ||

P

OH

O

::

P

|| O

CI

O O

O

O

CI

::

O O O

-

-

Phosphorus

expanded octet

(10 valence electron)

Chlorine

expanded octet

(14 valence electron)

Tetrahedral

2-

2-

N

H

N

:

:

O

SO32- PH3 NH3

O

H H

H2O

H H

O

O

F2O

F F

F F

O

S

CI CI

SCI2 SH2

S

H H

S

CI CI

S

H

NH2 -

N

H H

H H

N

-

-

H : : : : :

: : : :

: :

Two lone pair

central atom

Bend

CIO3-

H H

P

H H

H

H H

H P

H H

H

:

O O

S

O

S O

: O

2-

2-

CI

O O

O

CI

:

O O

O

-

:

-

SOCI2

S

CI CI

O

S

:

O CI

CI

:

: :

: :

:

One lone pair

central atom

One lone pair

Pyrimidal

Two lone pair

CH4

C

H

NH4+ BH4

- PCI4+ POCI3

H H

H

H

C

H H

H

N

H

H H H

H

N H

H

H

H

B

H H H

H

B

H

H H

CI

CI CI CI

P

CI

CI CI

P

CI

O -

-

+

+

+

+

P

CI CI CI

||

CI CI

CI

O

P

::

Tetrahedral

NO lone pair

:

:

:

:

: :

: :

:

: :

:

: :

: : : :

: :

:

NO lone pair

central atom

P CI CI

CI CI

CI

:

P

CI

CI

CI

CI

Seesaw structure

T structure

S

F

F

F

F

S

F

F

F F

Te

CI

CI

CI

CI

Te CI

CI

CI

CI

:

CI

F

F

F

CI

F

F

F

I

CI

CI

CI

CI

I

CI

CI

I

F

F

F

F

F

I

F

F

F

Xe

F

F

O

O

Xe

F

F

O

O

:

+

+

:

CI

Linear structure

I

I

I

Xe

CI

CI

I

F

F

: : : : : : :

:

:

: :

: :

: :

: : :

: :

: : :

:

: :

:

:

: :

:

:

:

: :

:

: :

: :

:

:

: :

:

: :

:

: :

: :

:

: :

:

: :

: : :

: :

: :

: :

: :

: :

: :

: :

: :

:

: : : NO lone pair

NO lone pair

central atom

ONE lone pair

: ONE lone pair

central atom

TWO lone pair

TWO lone pair

central atom

THREE lone pair

THREE lone pair

central atom

:

Br F

F

F

Br

F

F

F

: :

:

: :

:

: :

:

-

PCI5

SF4 TeCI4 (IF4)+ XeO2F2

CIF3 ICI3 BrF3

(I3)- (ICI2)- XeF2

Trigonal bipyrimidal

Central atom S, Te, I, Xe

- expanded octet

- 10 valence electron

Central atom P

- expanded octet

- 10 valence electron

Central atom CI, I, Br

- expanded octet

- 10 valence electron

Central atom I and Xe

- expanded octet

- 10 valence electron

-

Octahedral

F

S

SF6

F

F

F

F

F

PCI6-

P

CI

CI

CI

CI

CI

CI

IF5O

I

O ||

F

F

F

F

F

F

S

F

F

F

F

F CI

P

CI

CI

CI

CI

CI I

F

F

F

F

F :: O

NO lone pair

Square pyrimidal

CI

Sb

Sb

CI

CI

CI CI

CI

CI

CI CI

CI

(SbCI5)2- BrF5

Xe F

F F

F

Xe F

XeF4

F

F

F

F

Br F

F F

F

F

Br

F

F

O

F

F

Xe

|| F

F F

F

O

::

Xe F

F

F

F

F

Te F

F F

F

F

Te F

F

F

F

XeOF4 (TeF5)-

-

-

CI CI

I

CI CI

(ICI4)- -

I CI

CI

CI

CI

- Square planar

: : : :

: :

:

ONE lone pair

TWO lone pair

:

:

: :

:

:

: : :

: :

:

:

: :

:

: :

: :

: :

:

:

:

:

:

:

:

: :

:

:

:

:

: :

: : : :

:

:

:

: : :

:

: :

:

: :

: :

:

: :

: :

: : :

:

:

:

:

: : : :

:

: :

:

:

: :

: :

: :

: :

:

:

: :

:

: :

: :

: : :

:

:

:

:

:

:

: :

: :

:

: :

: :

:

2-

2-

: :

: :

: :

: :

:

:

:

:

: :

: :

: :

: :

: :

: :

: :

: :

NO lone pair

central atom

Central atom S, P , I

- expanded octet

- 12 valence electron

ONE lone pair

central atom

Central atom Sb, Br, Xe, Te

- expanded octet

- 12 valence electron

TWO lone pair

central atom

Central atom Xe, I

- expanded octet

- 12 valence electron

-

-

Chemical Bonds

Achieve stable electron arrangement of noble gases

Ionic Bonds

Transfer of electron from metal to non metal

Metal donate e Non Metal accept e

Positive ion (cation)

Negative ion (anion)

Ionic compound

Solubility

Covalent Bonds

Sharing of electron bet non metal atoms

Covalent compound/molecules

Non Metal share electrons

Difference in physical property

m/p + b/p conductivity Volatility

+ - electrostatic forces

attraction

Concept Map

Volatility Solubility Conductivity M/p B/p

Ionic compound

Low Soluble in aqueous solvent

High (In aqueous)

High

Covalent compound

High Soluble in organic solvent

Low

Low

0 0.4 4 Difference in electronegativity

difference < 0.4

covalent compound difference > 2

ionic compound

2

CI- Na+

EN - 0.9 EN - 3.0

Diff = 3 – 0.9

= 2.1

C 2.5

H 2.1

EN – 2.5 EN – 2.1

Diff = 2.5 – 2.1

= 0.4