shape of compounds due hybridisation
1.Shape of sncl2 (stannois chloride)
Ground state
Sn
(50) 5s^2 5px^1 5py^1 5pz^0
since sp^2 hybridisation takes place so sncl2 molecule should be triangular or triginal planar but actually sncl2 molecule is Bent because ane position of triangle is occupied by lone pair of electron.
2 shape of ClO4(perchlorate)
Ground state
Cl
(17) 3s^2 3px^2 3py^2 3pz^1 3d^0
excited state
3s^2 3px^1 3py^1 3pz^1 3d^3
{ sp3 hybridisation } {π bond}
orbital formed π bond don't take part in hybridisation .since sp3 hybridisation take place . so ClO4 is tetrahedral.
3.Shape of ClO3^-(chlorate ion)
Ground state
Cl
(17) 3s^2 3px^2 3py^2 3pz^1 3d^0
excited state
3s^2 3px^1 3py^1 3pz^1 3d^2
{ sp3 hybridisation} {2π bond}
since sp3 hybridisation takes place .so clo3^-should be tetrahedral. but actually clo3^-
is pyramidal .because one position of tetrahedral occupied by lone pair of electron.
4.Shape of So4^2-(sulphate ion)
ground state
S
(16) 3s^2 3px^2 3py^1 3pz^1 3d^0
excited state
3s^1 3px^1 3py^1 3pz^1 3d^2
(sp3 hybridisation) (2πbond)
since sp3 hybridisation takes place. so So4^2-
is tetrahedral.
5.Shape of No3^-(nitrate ion)
ground state
N
(7) 1s^2 2s^2 2px^1 2py^1 3pz^1
( sp hybridisation) ( form c-o-b)
since sp^2 hybridisation takes place NO3^- is triangular planar. bond angle 120°
6.Shape of Icl2^-(Inter halogen)
ground state
I
(53) 5s^2 5px^2 5py^2 5pz^1 5d^0
{sp3d hybridisation} ( form c-o-b)
since sp3d hybridisation takes place so Icl2^- ion should be trigonal bypyramidal but actually Icl2^- is linear. because three positions of triangle occupied by lone pair of electron.
Direct Determine Hybridisation
formula
1/2[V+X-C+A]
here
V- no. of electron in valence shell of central atom.
X-no. of monovalent atom
C- charge on cation(+)
A- charge on anion(-)
1.Shape of sncl2 (stannois chloride)
Ground state
Sn
(50) 5s^2 5px^1 5py^1 5pz^0
since sp^2 hybridisation takes place so sncl2 molecule should be triangular or triginal planar but actually sncl2 molecule is Bent because ane position of triangle is occupied by lone pair of electron.
2 shape of ClO4(perchlorate)
Ground state
Cl
(17) 3s^2 3px^2 3py^2 3pz^1 3d^0
excited state
3s^2 3px^1 3py^1 3pz^1 3d^3
{ sp3 hybridisation } {π bond}
orbital formed π bond don't take part in hybridisation .since sp3 hybridisation take place . so ClO4 is tetrahedral.
3.Shape of ClO3^-(chlorate ion)
Ground state
Cl
(17) 3s^2 3px^2 3py^2 3pz^1 3d^0
excited state
3s^2 3px^1 3py^1 3pz^1 3d^2
{ sp3 hybridisation} {2π bond}
since sp3 hybridisation takes place .so clo3^-should be tetrahedral. but actually clo3^-
is pyramidal .because one position of tetrahedral occupied by lone pair of electron.
4.Shape of So4^2-(sulphate ion)
ground state
S
(16) 3s^2 3px^2 3py^1 3pz^1 3d^0
excited state
3s^1 3px^1 3py^1 3pz^1 3d^2
(sp3 hybridisation) (2πbond)
since sp3 hybridisation takes place. so So4^2-
is tetrahedral.
5.Shape of No3^-(nitrate ion)
ground state
N
(7) 1s^2 2s^2 2px^1 2py^1 3pz^1
( sp hybridisation) ( form c-o-b)
since sp^2 hybridisation takes place NO3^- is triangular planar. bond angle 120°
6.Shape of Icl2^-(Inter halogen)
ground state
I
(53) 5s^2 5px^2 5py^2 5pz^1 5d^0
{sp3d hybridisation} ( form c-o-b)
since sp3d hybridisation takes place so Icl2^- ion should be trigonal bypyramidal but actually Icl2^- is linear. because three positions of triangle occupied by lone pair of electron.
Direct Determine Hybridisation
formula
1/2[V+X-C+A]
here
V- no. of electron in valence shell of central atom.
X-no. of monovalent atom
C- charge on cation(+)
A- charge on anion(-)
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