Chemical Bonding

Bent

Tetrahedral

Trigonal planer

Diagonal

Oxygen

Nitrogen

Fluorine

Chlorine

they are inert

they are unstable

they are mono-atomic gas

they have high tendency to combine with their own atoms.

lp-lp repulsion is more than lp-bp repulsion.

lp-bp repulsion is more than lp-lp repulsion.

lp-lp repulsion is equal to lp-bp repulsion.

Presence of lone pair does not affect the bond angle

hybrid structures

isomeric structures

canonical structures

dipole structures.

Bp-Bp > Lp-Bp > Lp-Lp

Lp-Lp > Lp-Bp > Bp-Bp

Lp-Bp > Bp-Bp > Lp-Lp

Lp-Lp > Bp-Bp > Lp-Bp

(I)- direct (II)- inverse

(I)- direct (II)- direct

(I)-inverse (II)-direct

(I)-inverse (II)-inverse

square planar structure

triangular structure

tetrahedral structure

octahedral structure.

the difference between the number of electrons in bonding and antibonding orbitals

total number of electrons in bonding and antibonding orbitals

twice the difference between the number of electrons in bonding and antibonding orbitals

half the difference between the number of electrons in bonding and antibonding orbitals.

$AlCl_{3}<MgCl_{2}<NaCl$

$MgCl_{2}<NaCl<AlCl_{3}$

$NaCl<MgCl_{2}<AlCl_{3}$

$NaCl<AlCl_{3}<MgCl_{2}$

HF

NH3

BF 3

CHCl3

Three

Four

Eight

Six

bond pair - bond pair > lone pair - bond pair > lone pair - lone pair

lone pair - bond pair > bond pair - bond pair > lone pair - lone pair

lone pair - lone pair > lone pair - bond pair > bond pair - bond pair

lone pair - lone pair > bond pair - bond pair > lone pair - bond pair

$sp^{3}>sp^{2}>sp$

$sp>sp^{2}>sp^{3}$

$sp=sp^{2}>sp^{3}$

$sp=sp^{2}=sp^{3}$