Question

❤❤❤Hey❤❤❤
(i) Write two conditions required for the linear combination of atomic orbitals to
form molecular orbitals.
(ii)Draw the shapes of the following molecules on the basis of VSEPR theory
XeF4 and SF4.
(iii) What is the change in hybridization (if any) of the Al atom in the following
reaction? AICl3 + Cl^- → AICI4^-

Carries 3 Marks
Class 11 CBSE

Answer 1

• Answer 1 :

=> A bond is formed between two atoms when the new forces of attraction are greater than forces of repulsion.

=> Atomic orbitals should be lies on axis so that maximum overlapping can take place..

First i want to tell you that how to find hybridisation of any compound..

Formula : n = 1/2 [v + s + (-ve charge) - (+ve charge) ]

Here, v = valence electron of central atom

s = no. of single bonded atoms with central atom

-ve = total negative charge on compound

+ve = total positive charge on compound

if n = 2 -----> sp

n = 3 -----> sp2

n = 4 ------> sp3

n = 5 ------> sp3d

n = 6 ------> sp3d2

n = 7 ------> sp3d3

now,

• Answer 2)

XeF4 : n = 1/2 [ 8 + 4 + 0 - 0 ] = 6

hybridisation of XeF4 = sp3d2

shape = squar planner

SF4 : n = 1/2 [ 6 + 4 + 0 - 0 ] = 5

hybridisation of SF4 = sp3d

shape = trigonal bipiramidal

• Answer 3)

AlCl3 + Cl^- ---------> AlCl4^-

=> hybridisation of AlCl3

n = 1/2 [ 3 + 3 +0 - 0 ] = 3

sp2

=> hybridisation of AlCl4^-

n = 1/2 [ 3 + 4 + 1 - 0 ] = 4

sp3

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