ib chemistry on lewis structure, ionic and covalent bonding

http://lawrencekok.blogspot.com

Prepared by Lawrence Kok

Tutorial on Lewis Structure, Ionic and Covalent bonding.

brown liquid

Ionic Bonding Group 1 and 17 Gp 1 Metal2.1

2.8.1

2.8.8.1

2.8.8.18.1

Na

Li

K

Rb

yellow gas

greenish gas

violet solid

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

Gp 17 Non metal

brown liquid


2.8.1

2.8.8.1

2.8.8.18.1

Na

Li

K

Rb

yellow gas

greenish gas

violet solid




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

brown liquid


2.8.1

2.8.8.1

2.8.8.18.1

Na

Li

K

Rb

Click here video 0n NaCI

yellow gas

greenish gas

violet solid




2.8.1 2.8.7

Gp 17 Non metal

transfer electron

2.8 2.8.8


+ -

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

brown liquid

Gp 2 Metal2.2

2.8.2

2.8.8.2

2.8.8.18.2

Mg

Be

Ca

Sr

yellow gas

greenish gas

violet solid




Gp 17 Non metal

brown liquid

Gp 2 Metal2.2

2.8.2

2.8.8.2

2.8.8.18.2

Mg

Be

Ca

Sr

yellow gas

greenish gas

violet solid




2.8.2 2.7

Gp 17 Non metal

transfer electron

2.8


Mg2+ F-

Electrostatic force attraction bet opposite charge ions

2.8. 82.8

F-

brown liquid

Gp 2 Metal2.2

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

violet solid




2.8.2 2.7

Gp 17 Non metal

transfer electron

2.8


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. 82.8

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

Writing Chemical Formula Ionic Compounds



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



Ionic Compound

Li2O MgCI2 Al2O3 FeO NiO CuO

Li3N Mg3N2 AlN Fe3N2 Ni3N2 Cu3N2




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



Ionic Compound

Li2O MgCI2 Al2O3 FeO NiO CuO

Li3N Mg3N2 AlN Fe3N2 Ni3N2 Cu3N2

Oxidation state/Charge ion→ Li1+ O2-

Formula compound Li2

O1

Video on polyatomic ions


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 ionsMetal/Cations/+ve ions



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+


Polyatomic ions


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)

Ionic Compound

Metal/Cations/+ve ions



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+


Polyatomic ions


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



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 Li2

(CO3)1

Step 1 : Write Oxidation state/charge ion

Step 2 : Balance it, (electrically neutral) by cross multiply – as subscript


Acids AlkaliMetal Hydroxide

Metal oxides Salts Gas

HCIHydrochloric acid

KOHPotassium hydroxide

CuOCopper(II) oxide

CaCO3

Calcium carbonate

COCarbon monoxide

HNO3

Nitric acidNaOH

Sodium hydroxideMgO

Magnesium oxideNa2CO3

Sodium carbonate

CO2

Carbon dioxide

H2SO3

Sulphurous acidCa(OH)2

Calcium HydroxideZnO

Zinc oxideNaHCO3

Sodium bicarbonate

SO2

Sulphur dioxide

HCOOHMethanoic acid

NH3

AmmoniaNa2O

Sodium oxideKNO3

Potassium nitrateSO3

Sulphur trioxide

CH3COOHEthanoic acid

Mg(OH)2

Magnesium hydroxide

Al2O3

Aluminium oxidePb(NO3)2

Lead (II) NitrateNO2

Nitrogen dioxide

H3PO4

Phosphoric acidCu(OH)2

Copper (II) hydroxide

Fe2O3

Iron(III) oxideNaNO3

Sodium nitrateCH4

Methane

H2CO3

Carbonic acidAl(OH)3

Aluminium hydroxide

K2SPotassium sulphide

PbI2

Lead (II) nitrateH2S

Hydrogen sulphide

HNO2

Nitrous acidFe(OH)2

Iron (II) hydroxidePbS

Lead(II) sulphideAgCI

Silver chlorideO2

Oxygen

HFHydrofluoric acid

Fe(OH)3

Iron (III) hydroxideZnS

Zinc sulphideMgSO4

Magnesium sulphate

N2

Nitrogen

HCIOHypochlorous acid

Zn(OH)2

Zinc hydroxideAI2S3

Aluminium sulphide

Na2S2O3

Sodium thiosulphate

CI2

Chlorine

Chemical Formula for common chemicals

Naming chemical compound

Writing chemical formula

Writing chemical formula

VIDEO TUTORIALS

brown liquid

yellow gas

greenish gas

violet solid

Covalent bonding between non metals

Gp 17 Non metalGp 17 Non metal


Covalent Bond Group 17


brown liquid

yellow gas

greenish gas

violet solid


2.8.7

Gp 17 Non metal


CI shared pair electron

Covalent BondingElectrostatic forces attraction between nucleus with shared pair electron

2.8.8

2.8.7 Sharing electron

Gp 17 Non metal

2.8.8

CI



CICI


brown liquid

Click here simulation on covalent bond

yellow gas

greenish gas

violet solid


2.8.7

Gp 17 Non metal


CI shared pair electron

Covalent BondingElectrostatic forces attraction between nucleus with shared pair electron

2.8.8

2.8.7 Sharing electron

Gp 17 Non metal

2.8.8

CI



CICI

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

CI CI: xx:

:

:.

xx

X

xx

xx CI CI

:: xx

xx

CI CI


Single covalent bond – shared pair electron


Covalent BondingSingle covalent bond ONE pair shared e

2.8.8 2.8.8

Covalent Bond


CI CI: xx

::

:.

xx

X

xx

xx CI CI

:: xx

xx

CI CI

Sharing electron

Bond Strength



2.8.8 2.8.8

Covalent Bond


CI CI: xx

::

:.

xx

X

xx

xx

O

CI CI:

: xxxx

CI CI

Sharing electron

Bond Strength

2.8 2.8

Sharing electron

:O O: : x

x

xx

xx

O:

: xx

xx

O O


Covalent BondingDouble covalent bond TWO pair shared e



2.8.8 2.8.8

Covalent Bond


CI CI: xx

::

:

:.

xx

X

X

xx

xx

xx

O

CI CI:

: xxxx

xx

CI CI

Sharing electron

Bond Strength

2.8 2.8

Sharing electron

:O O: : x

x

xx

xx

O:

: xx

xx

N

O O

N:



C

: :. N N: N N

:

Covalent BondingDouble covalent bond TWO pair shared e

Covalent BondingTriple covalent bondTHREE pair shared e

O:

: xx: CO:

:

C :O:

: O

:

O O


Covalent BondingDouble covalent bondTWO pair shared e

Bond length and Bond strength

Bond length = 0.199nm


CI CI: xx

::

:

:.

xx

X

X

xx

xx

O

CI CI:

: xxxx

xx

CI CI

:O O: : x

x

xx

xx

O:

: xx

xx

N

O O

N:



: :.N N: N N



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




CI CI: xx

::

:

:.

xx

X

X

xx

xx

O

CI CI:

: xxxx

xx

CI CI

:O O: : x

x

xx

xx

O:

: xx

xx

N

O O

N:



: :.N N: N N

Triple bond > Double bond > Single bond

Bond length decrease

Bond strength Increase

(Double/Triple bond)



Bond order up – Bond strength up – Bond length down

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




CI CI: xx

::

:

:.

xx

X

X

xx

xx

O

CI CI:

: xxxx

xx

CI CI

:O O: : x

x

xx

xx

O:

: xx

xx

N

O O

N:



O

: :.N N: N N

:Triple bond > Double bond > Single

bond

Bonding pair e -involve in

bonding







O

:

Non bonding pair (Lone pair electron)

Bonding pair electron

C O: :


Dative bond (electron pair of oxy)

Types of bonding

Lone pair e –not involve in bonding

Dative/coordinate bond

- pair e come from an atom

: :

:

.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




CI CI: xx

::

:

:.

xx

X

X

xx

xx

O

CI CI:

: xxxx

xx

CI CI

:O O: : x

x

xx

xx

O:

: xx

xx

N

O O

N:



O

: :.N N: N N

:Triple bond > Double bond > Single

bond

Bonding pair e -involve in

bonding







O

:

Non bonding pair (Lone pair electron)


C O: :


Dative bond (electron pair of oxy)

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 deficientLess than 8 valence e

Expanded octetMore than 8 valence e

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

: BeCI CIx. :

::

::

x

x.

Be - 4 valence e

BCI CI: :::

:: x

: :B - 6 valence e

P S

CI

CI

CI

CI

CI

CI

CICI

CICICI

P - 10 valence e

S – 12 valence e

: :

O:

ONO C

N

C BeH N X x:Linear

O C H H NO N O

C OO CH N HH Be C N N O O:xx

:::

X x

X x

XX X X

X

X

X x

:

X x

:

:

+

+: :

:

:.

Electron deficient Be

Dative bond from N

NCxx :

Electron deficient N(7 valence electron)

CO2 HCN BeH2

CN - NO2 + NO

::

O:

ONO C

N

C BeH N

:

B

:

X x:

:

:

C SSO

Linear

O C H H NO N O

Trigonal

planar

C OO CH N HH Be C N N O O:xx

:::

X x

X x

XX X X

X

X

X x

:

X x

:

:

+

+: :

:

:.

F

F

F

Electron deficient Be

Dative bond from N

NCxx :

Electron deficient N(7 valence electron)

H

H O O

O O

O O

CO O

O

O N

O

O

BXF

X

X F

X

FC

H

H

X

x x

O

:

S

x

x

O OS

O:

xx

xx

O:::

: :

x x

O:

CO:

: :

X

O:::

X

x x

O :

: N

2- -

2-

O:

: :

X

x x

xx

O

:

: :

O:

:

-

Electron deficient B

O

x x

S

O

: : O: : ::

::

Dative bond from S

:

:

ON

O

O

:

:

: :

: :

-

O

x

x

x x

: :

::

||||

|| ||

Sulphur expanded octet (12 valence electron) ✓

BF3 CH2 O SO3 CO3 2- NO3

-

CO2 HCN BeH2

CN - NO2 + NO

::

:

O

HH

H2O

H H

O: :

O

F2O

F F

F F

O

S

CICI

SCI2 SH2

S

H H

S

CI CI

S

H

: : :: : :

NH2 -

N

HH

HH

N: :

-

-. .

.. . .. . . .

.. . . ... .

.. . . . . .H: : : : :

: : : :: :

All molecule – octet rule

Bend

:

O

O O

O

O O

||

::

:

:

::

: ::

N

:

:

:

O O

||

O

NO

:: :

:

:

: ::

SO O

||

OOS :::

:

SO O

||||

OOS ::

:: :::

:

:: ::

N

O O

||

N ::

OO

::

:::

:

-

-

O ON

::

:

::

:

:

O O:

::N

::

::

:

-

Dative bond from Nelectron deficient N(7 valence electron)

SO O

::

:

:

:

:::

Sulphur expanded octet (10 valence electron)

or

or

Dative bond from S

NO2- NO2 SO2 O3

O

HH

H2O

H H

O: :

O

F2O

F F

F F

O

S

CICI

SCI2 SH2

S

H H

S

CI CI

S

H

: : :: : :

NH2 -

N

HH

HH

N: :

-

-. .

.. . .. . . .

.. . . ... .

.. . . . . .H: : : : :

: : : :: :

All molecule – octet rule

Bend

Bend

:O::

O

:

::

O

:

:Dative bond from O

||

:CI

C

HH

CH4 NH4+

N

BH4- PCI4

+ POCI3

P

CI-+

Tetrahedral

H

H

H

HH

H

B

H

HHH CI

CICI

+

P

O

CICICI

C

H

H

HH

H

N

H

H

H

+

H

B H

H

H

-CI

PCI

CI

CI

+

:

:

:

:

:

:::

: :

:

:

O

::

P

CI

CI ::

: ::

:

::

: :

||

:

S

CI

Sulphur expanded octet (12 valence electron)

C

HH

CH4 NH4+

N

BH4- PCI4

+ POCI3

P

CI-+

Tetrahedral

H

H

H

HH

H

B

H

HHH CI

CICI

+

P

O

CICICI

C

H

H

HH

H

N

H

H

H

+

H

B H

H

H

-CI

PCI

CI

CI

+

:

:

:

:

:

:::

: :

:

:

O

::

P

CI

CI ::

: ::

:

::

: :

OSO4

2-

O

|| ||

OO

O

S

O

::

O

::

||

O

H2SO4 H3PO4

CIO4 -

||O

S ||O

OHHO

S

O

O

::

::

O

O:

O||

POH

OHHO

O

::O

P

OO

||O

CIO

||

OO

O

CI

::

:: O

::

O

O

: :

:

:

: :

:

:

:

::

:

::

: H : :

H

: :

:

: :

H HH

:

:::::

-

-

Phosphorus expanded octet (10 valence electron)

:: :

:

:

:

Chlorine expanded octet (14 valence electron)

Tetrahedral

2-

2-

:

O

HH

H2O

H H

O: :

O

F2O

F F

F F

O

S

CICI

SCI2 SH2

S

H H

S

CI CI

S

H

: : :: : :

NH2 -

N

HH

HH

N: :

-

-. .

.. . .. . . .

.. . . ... .

.. . . . . .H: : : : :

: : : :: :

Two lone pair central atom

Bend

Two lone pair

N

H

N

:

:

O

SO32- PH3 NH3

O

HH

H2O

H H

O: :

O

F2O

F F

F F

O

S

CICI

SCI2 SH2

S

H H

S

CI CI

S

H

: : :: : :

NH2 -

N

HH

HH

N: :

-

-. .

.. . .. . . .

.. . . ... .

.. . . . . .H: : : : :

: : : :: :


Bend

CIO3-

HH

PH

HH

H. .

HH

PH

H. .

H

:

O O

S||

O

SO

:

::

O

2-

2-

CIO

OO

CI

:

OOO

-

:

:

:

: : : :

: :

:

:

: : :

:

::

-

SOCI2

SCI

CIO||

S:::

OCI

CI

:

: :

::

::

:

One lone pair central atom

One lone pair

Pyrimidal

Two lone pair

N

H

N

:

:

O

SO32- PH3 NH3

O

HH

H2O

H H

O: :

O

F2O

F F

F F

O

S

CICI

SCI2 SH2

S

H H

S

CI CI

S

H

: : :: : :

NH2 -

N

HH

HH

N: :

-

-. .

.. . .. . . .

.. . . ... .

.. . . . . .H: : : : :

: : : :: :


Bend

CIO3-

HH

PH

HH

H. .

HH

PH

H. .

H

:

O O

S||

O

SO

:

::

O

2-

2-

CIO

OO

CI

:

OOO

-

:

:

:

: : : :

: :

:

:

: : :

:

::

-

SOCI2

SCI

CIO||

S:::

OCI

CI

:

: :

::

::

:

One lone pair central atom

One lone pair

Pyrimidal

Two lone pair

CH4

C

H

NH4+ BH4

- PCI4+ POCI3

HH

H

H

CH

HH

N

H

H HH

H

NH

HH

H

BHH H

H

BH

HH

CI

CI CI CI

P

CI

CICI

P

CI

O-

-

+

+

+

+

P

CI CICI

||

CI CICI

O

P

::

Tetrahedral

NO lone pair

:

::

:

::

::

:

:

:

::

:

::

::: :

::

:

NO lone pair central atom

P CICI

CICI

CI

P

CI

CI

CI

CI

CI

NO lone pair


PCI5

Trigonal bipyrimid

al

Central atom P- expanded octet - 10 valence electron

P CICI

CICI

CI

:

P

CI

CI

CI

CI

Seesawstructur

e

S

F

F

F

F

S

F

F

FF

Te

CI

CI

CI

CI

Te

CI

CI

CICI

:

I

FF

F

F

F

I

F

F

F

Xe

F

F

O

O

Xe

F

F

O ::

O

:

+

+

:

CI

:::::::

:

:

::

::

:::

:

::

::

:: :

::

:::

:

::

:

:

: :

:

:

:

::

:

::

::

:

:

NO lone pair


ONE lone pair

:ONE lone pair central atom

PCI5

SF4 TeCI4 (IF4)+ XeO2F2

Trigonal bipyrimid

al

Central atom S, Te, I and Xe - expanded octet - 10 valence electron


P CICI

CICI

CI

:

P

CI

CI

CI

CI

Seesawstructur

e

Tstructur

e

S

F

F

F

F

S

F

F

FF

Te

CI

CI

CI

CI

Te

CI

CI

CICI

:

CI

F

F

F

CI

F

F

F

I

CI

CI

CI

CI

I

CI CI

I

FF

F

F

F

I

F

F

F

Xe

F

F

O

O

Xe

F

F

O ::

O

:

+

+

:

CI

:::::::

:

:

::

::

:::

:

::

::

:: :

::

:::

:

::

:

:

: :

:

:

:

::

:

::

::

:

:

::

:

::

:

::

::

:

::

:

::

:

:

::

:

:

NO lone pair


ONE lone pair


TWO lone pair

::

TWO lone pair central atom

BrF

F

F

Br

F

F

F

: :

:

: :

:

::

:

:

:

PCI5


CIF3

ICI3 BrF3

Trigonal bipyrimid

al



Central atom CI, I and Br - expanded octet - 10 valence electron

P CICI

CICI

CI

:

P

CI

CI

CI

CI

Seesawstructur

e

Tstructur

e

S

F

F

F

F

S

F

F

FF

Te

CI

CI

CI

CI

Te

CI

CI

CICI

:

CI

F

F

F

CI

F

F

F

I

CI

CI

CI

CI

I

CI CI

I

FF

F

F

F

I

F

F

F

Xe

F

F

O

O

Xe

F

F

O ::

O

:

+

+

:

CI

Linearstructur

e

I

I

I

Xe

CI

CI

I

F

F

:::::::

:

:

::

::

:::

:

::

::

:: :

::

:::

:

::

:

:

: :

:

:

:

::

:

::

::

:

:

::

:

::

:

::

::

:

::

:

::

:

::

::

::

::

::

::

::

::

::

:

::

:

:

: : :: : :: : :

NO lone pair


ONE lone pair


TWO lone pair

::


THREE lone pair

THREE lone pair central atom

:::

BrF

F

F

Br

F

F

F

: :

:

: :

:

::

:

:

:

-

PCI5


CIF3

ICI3 BrF3

(I3)- (ICI2)- XeF2

Trigonal bipyrimid

al



Central atom CI, I and Br - expanded octet - 10 valence electron

Central atom I and Xe - expanded octet - 10 valence electron

-

Octahedral

F

S

SF6

F

FF

F

F

PCI6-

P

CICI

CI

CI

CI

CI

IF5O

I

O||

F

F

F

F

F

F

SF

FF

F

FCI

PCI

CI

CI

CI

CII

F F

F

F

F ::

O

NO lone pair

:

:

:::

:

::: :

::

:

::

:

::

::

::

::

:

:

:

::

:

:

:

:::

: ::::

:

:

:

::

:

::

:

::

::


Central atom S, P and I- expanded octet - 12 valence electron

-

-

Octahedral

F

S

SF6

F

FF

F

F

PCI6-

P

CICI

CI

CI

CI

CI

IF5O

I

O||

F

F

F

F

F

F

SF

FF

F

FCI

PCI

CI

CI

CI

CII

F F

F

F

F ::

O

NO lone pair

Square pyrimidal

CI

Sb

Sb

CI

CI

CICI

CI

CI

CICI

CI

(SbCI5)2- BrF5

F

BrF

FF

F

F

Br

F

F

O

F

F

Xe||

F

FF

F

O

::

Xe

F

F

F

F

F

Te F

FF

F

F

Te F

F

F

F

XeOF4 (TeF5)-

-

-: : : :

:

ONE lone pair

:

:

:::

:

::: :

::

:

::

:

::

::

::

:

:

:

:

:

:

:

::

:

:

:

:::

: ::::

:

:

:

::

:

::

:

::

::

:

::

::

::

::

:

:

:

::::

:

::

:

:

::

::

::

::

:

:

::

:

::

::

:::

:

:

:

:

:

:

::

::

:

::

::

:

2-

2-



ONE lone pair central atom

Central atom Sb, Br, Xe, Te- expanded octet - 12 valence electron

-

-

Octahedral

F

S

SF6

F

FF

F

F

PCI6-

P

CICI

CI

CI

CI

CI

IF5O

I

O||

F

F

F

F

F

F

SF

FF

F

FCI

PCI

CI

CI

CI

CII

F F

F

F

F ::

O

NO lone pair

Square pyrimidal

CI

Sb

Sb

CI

CI

CICI

CI

CI

CICI

CI

(SbCI5)2- BrF5

XeF

FF

F

Xe

F

XeF4

F

F

F

F

BrF

FF

F

F

Br

F

F

O

F

F

Xe||

F

FF

F

O

::

Xe

F

F

F

F

F

Te F

FF

F

F

Te F

F

F

F

XeOF4 (TeF5)-

-

-

CICII

CICI

(ICI4)--

ICICI

CI

CI

-Square planar

: : : :

::

:

ONE lone pair

TWO lone pair

:

:

:::

:

::: :

::

:

::

:

::

::

::

:

:

:

:

:

:

:

::

:

:

:

:::

: ::::

:

:

:

::

:

::

:

::

::

:

::

::

::

::

:

:

:

::::

:

::

:

:

::

::

::

::

:

:

::

:

::

::

:::

:

:

:

:

:

:

::

::

:

::

::

:

2-

2-

::

::

::

::

:

:

:

:

::

::

::

::

::

::

::

::



ONE lone pair central atom

Central atom Sb, Br, Xe, Te- expanded octet - 12 valence electron


Central atom Xe and 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/pconductivityVolatility

+ -electrostatic forces attraction

Volatility

Solubility Conductivity

M/p B/p

Ionic compoun

d

Low Soluble in aqueoussolvent

High (In aqueous)

High

Covalent compoun

d

High Soluble in organicsolvent

Low Low

0 0.4 4

Difference in electronegativity

difference < 0.4covalent compound

difference > 2ionic compound

2

CI-Na+

EN - 0.9 EN - 3.0

Diff = 3 – 0.9 = 2.1

C2.5

H2.1

EN – 2.5 EN – 2.1

Diff = 2.5 – 2.1 = 0.4

Acknowledgements

Thanks to source of pictures and video used in this presentation

Thanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/

Prepared by Lawrence Kok

Check out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com

ib chemistry on lewis structure, ionic and covalent bonding

Education

anionnon metal gp

metal metal low en value

metal transfer electron

ve ions gp1 gp

ions reaction

brown liquid gp

oxidation statecharge

covalent bonding