IONIC/ELECTROVALENT
BOND
. Strong electro static
force of attraction
between positive and
negative ions.
. Crystalline in nature
. High M.P and B.P
. Soluble in Polar Solvents.
Eg: NaCl, MgCl2 etc.
IONIC/
ELECTROVALENT
BOND
CO-VALENT
BOND
HYDROGEN BOND
. Bond formed when the -ve
end of one molecule
attracts the +ve end of
other
1. Intermolecular: H- Bonding
occur within one single
molecule.
2. Intermolecular: H Bonding
between two different
molecules of same or
diff. compounds.
. Bond formed by mutual
sharing of e-.
. Low M.P. and B.P.
. Bad conductor of
electricityv
. Insoluble in Polar Solvents
but soluble in non-polar
solvent.
Ex: CH4, H2, Cl2.
. Strong electro static
force of attraction
between positive and
negative ions.
. Crystalline in nature
. High M.P and B.P
. Soluble in Polar Solvents.
Eg: NaCl, MgCl2 etc.
VALENCE BOND THEORY
VBT
KOSEL LEWIS APPROCH
THEORIES OF CO-VALENT BOND
TYPES OF BONDS
KOSSEL LEWIS APPROACH
A covalent bond is formed by the
overlapping of two half filled atomic
orbitals.
Atoms can combine either by
transfer of e- or by sharing
of valence e- in order to have
an octet in their valence shell.
Type of overLapping
Octet Rule
LEWIS SYMBOLS
Sigma(σ)
Sidewise overlapping
Valence e- are represented by
dots around the element.
: :
: :
. s-s overlapping
H; Na; : Cl ; O , : N :
TYPE OF CO-VALENT
BOND
+
. Polar covalent bond
Eg: NH3, CHCl3
. Non-polar covalent bond
Eg: Cl2, CO2.
s
s
FAJAN'S RULE
: :
H
+
s+
+
p
C
s
H
CHEMICAL BONDING
AND
MOLECULAR STRUCTURE
s+
s
FORMAL
CHARGE
. Bond length:
Equilibrium distance
between the nuclei
of two bonded atom
1
bod length ∝
bond order
No. of Bond
BOND ORDER between the two
atoms
p
VSEPR THEORY
HYBRIDISATION
Type of
No. of
No. of Arrangement
Molecule Bonding pair Lone Pair of e- pair
Shape
Example
AB2E
2
1
Bent
SO2O3
AB3E
3
1
Trigonal
Pyramidal
NH3
AB3E2
Angle between the
BOND ANGLE orbitals containing
bonding e- pair around
central atom.
BOND
ENTHALPY
2
2
Bent
Concept of mixing
atomic orbital to
form new hybrid
MOLECULAR ORBITAL
THEORY
Formation of Molecular Orbitals
H2O
Molecular orbitals
+
DIPOLE
MOMENT
M = charge × Distance of
seperation
anand_mani16
No. of
nodal plane
. MOT are formed the combinate of atomic orbitals.
. No. of molecular orbitals = no. of atomic orbital
combined.
MOT
0
AB4E
4
1
+
See saw
σ∗
SF4
+
AB3E2
3
2
T-Shape
ClF5
px
AB5E
5
1
Square
Pyramid
XeF5
px
DR. Anand Mani
4
2
square
Planner
XeF4
https://www.anandmani.com/
Bonding molecular
orbitals
Anti bonding atomic
orbitals
π
ELECTRONIC CONFIGURATION
px
px
pz
pz
π
pz
π∗
-
pz
2
<
(σ1s < σ*1s < σ2s < σ*2s < σ2pz < (π2px = π2px)
< (π*2px = π*2py) < σ*2pz
[For O2, F2, Ne2]
2
(σ1s < σ*1s < σ2s < σ*2s < [π2px = π2py] < σ2pz)
< (π*2px = π*2py) < σ*2pz
[For B2, C2, N2]
π∗
+
AB4E2
1
1
-
Product of the magnitude
of the
charge and distance
between centres
of positive and negative
charge.
The shape of a molecule
depends upon the numbers
of valence shell e- (B.P or
l.p) surrounding in the
central atom
σ
Amount of enrgy
required to break
one mole of bonds.
Decreasing order of repulsive
interaction:
lp - lp > lp - bp > bp . bp
Polarized anion
Atomic orbitals
&
p-p overlap
s-p overlap
p-p overlap
Polarization of anion by cation
BOND
PARAMETERS
p
+
p
1
F.C. = r - L - B
2
+
. s-p overlapping
C
Cation
s-s overlap
H
H
No compounds is 100% ionic or 100%
covalent
. Covalent nature ∝ size of anion
1
. Covalent nature ∝
size of cation
Pi(π)
Sidewise overlapping
3
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