Explain bonding Xef6. Pcl5
Answers
Explanation:
PCl
5
: P(G.S)=1s
2
2s
2
2p
6
3s
2
3p
3
P(E.S)=1s
2
2s
2
2p
6
3s
1
3p
3
One s , three p & one d orbitals of same shell participate to give sp
3
d hybridisation.
Shape: Trigonal bipyramidal.
Figure-1 represents the shell diagram.
Figure-2 represents the shape .
NH
3
:N(G.S)=1s
2
2s
2
2p
3
N(E.S)=1s
2
One s , three p participate to give sp
3
hybridisation.
Shape: Pyramidal
Figure-3 represents the shell diagram.
Figure-4 represents the shape .
H
2
O:O(G.S)=1s
2
2s
2
2p
4
O(E.S)=1s
2
2s
2
2p
x
2
2p
y
1
2p
z
1
Two half filled sp
3
hybrid orbital of Oxygen atom & s orbital of 2 Hydrogen atom overlap to form water.
Shape: V-shaped or distorted tetrahedral due to lp−lp,lp−bp,bp−bp repulsion.
Figure-5 represents the shell diagram.
Figure-6 represents the shape .
SF
6
:1s
2
2s
2
2p
6
3s
2
3p
4
Hybridisation- sp
3
d
2
Shape: Octahedral.
Answer:
Formation of PCl
5
(sp
3
d hybridization): The ground state and the excited state outer electronic configurations of phosphorus (Z=15) are represented in Figure 1.
Three P—Cl bond lie in one plane and make an angle of 120
o
with each other; these bonds are termed as equatorial bonds. The remaining two P—Cl bonds—one lying above and the other lying below the equatorial plane, make an angle of 90
o
with the plane. These bonds are called axial bonds. As the axial bond pairs suffer more repulsive interaction than the equatorial bond pairs, therefore axial bonds have been found to be slightly longer and hence slightly weaker than the equatorial bonds; which makes PCl
5
molecule more reactive.
Hope this will help you :)