compare the relative stability of the following species? O2, O2+, O2- (super oxide) ; (O2)2- (peroxide) .
Answers
Explanation:
) The electronic configuration of O
2
molecule is
KK(σ2s)
2
(σ
∗
2s)
2
(σ2p
z
)
2
(π2p
x
)
2
(π2p
y
)
2
(π
∗
2p
x
)
1
(π
∗
2p
y
)
1
Its bond order is
2
8−4
=2.
It contains 2 unpaired electrons and is paramagentic.
(2) The electronic configuration of O
2
+
ion is
KK(σ2s)
2
(σ
∗
2s)
2
(σ2p
z
)
2
(π2p
x
)
2
(π2p
y
)
2
(π
∗
2p
x
)
1
Its bond order is
2
8−3
=2.5.
It contains 1 unpaired electron and is paramagnetic.
(3) The electronic configuration of O
2
−
ion is
KK(σ2s)
2
(σ
∗
2s)
2
(σ2p
z
)
2
(π2p
x
)
2
(π2p
y
)
2
(π
∗
2p
x
)
2
(π
∗
2p
y
)
1
Its bond order is
2
8−5
=1.5.
It contains 1 unpaired electron and is paramagnetic.
(4) The electronic configuration of O
2
2−
ion is
KK(σ2s)
2
(σ
∗
2s)
2
(σ2p
z
)
2
(π2p
x
)
2
(π2p
y
)
2
(π
∗
2p
x
)
2
(π
∗
2p
y
)
2
Its bond order is
2
8−6
=1.
It contains all paired electrons and is diamagnetic.
Higher is the bond order, stronger is the bond, and higher is the stability.
The decreasing order of the stability is O
2
+
>O
2
>O
2
−
>O
2
2−
.