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Standard XII
Chemistry
Introduction of VSEPR
40.Why AB3L3 ...
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40.Why AB3L3 types are not possible in nature where A is central atom and B is Bonded atoms and L is lone pair. Note:consider every bond as single bond
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Q.
A central atom in a molecule has two lone pairs of electrons and forms three single bonds. The shape of this molecule is,
Q.
Which of the following statement is correct regarding
I
−
3
ion?
Q.
The
I
−
3
ion has
Q.
In
C
O
2
,
I
−
3
,
N
O
−
2
and
N
O
+
2
,
if the sum of bond pairs (single bond) on the central atom of all the molecules given is
x
and the sum of all lone pairs on the central atom of all the molecules given is
y
then,
(
x
+
y
)
is:
Q.
Consider the following statements;
(I) The hybridlsation found in cation of solid
P
C
l
5
is
s
p
3
.
(II) In
A
B
2
L
2
type the
B
−
A
−
B
bond angle is always greater than the normal tetrahedral bond angle.
(III) In
C
I
O
−
3
,
N
H
3
and
X
e
O
3
the hybridisation and the number of lone pairs on the central atoms are same.
(IV) In
P
4
molecule, there are six
P
−
P
bonds and four lone pairs of electrons.
of these statements :
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