Bond type
|
sp3
|
sp2
|
sp
|
Bond angle
|
109º28¢
|
120°
|
180°
|
(iii) By increasing lone pair of electron, bond angle decreases approximately by 2.5%.
CH4
|
NH3
|
H2O
|
|
Bond angle
|
109º
|
107o
|
105o
|
(iv) If the electronegativity of the central atom decreases, bond angle decreases.
In case the central atom remains the same, bond angle increases with the decrease in electroneativity of the surrounding atom.
Bond Energy
Definition of Bond Energy
“The amount of energy required to break one mole of bondsof a particular type so as to
separate them into gaseous atoms is called bond dissociation energy or simply bond energy”.
Greater is the bond energy,stronger is the bond. Bond energy is usually expressed in kJ mol–.
Factors affecting bond energy
(i) Greater the size of the atom, greater is the bond length and less is the bond dissociation energy i.e. less is the bond strength.
(ii) For the bond between the two similar atoms, greater is the multiplicity of the bond, greater is the bond dissociation energy.
(iii) Greater the number of lone pairs of electrons present on the bonded atoms, greater is the repulsion between the atoms and hence less is the bond dissociation energy.
(iv)The bond energy increases as the hybrid orbitals have greater amount of s orbital contribution. Thus, bond energy decreases in the following order, sp > sp2 > sp3
(v) Greater the electronegativity difference, greater is the bond polarity and hence greater will be the bond strength i.e., bond energy, H – F > H – Cl > H – Br > H – I,
(vi) Among halogens Cl – Cl > F – F > Br – Br > I – I, (Decreasing order of bond energy) Resonance increases bond energy.
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