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Question

Consider the following reactions :
O(g)+eO(g),ΔH1
F(g)+eF(g),ΔH2
Cl(g)+eCl(g),ΔH3
O(g)+eO2(g),ΔH4
The correct statement(s) is/are

A
ΔH3 and ΔH2 both are negative
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B
ΔH1 and ΔH4 both are positive
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C
ΔH1, ΔH2 and ΔH3 are negative
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D
ΔH4 is negative
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Solution

The correct option is C ΔH1, ΔH2 and ΔH3 are negative
a) ΔH3 and ΔH2 both are negative because both F and Cl is getting a stable electronic configuration by accepting an electron. So energy will release.
b) ΔH1 will have a negative value since due to the effective nuclear charge of O atom, electron will receive an attractive force and electron will release energy to occupy a lower energy orbital. But ΔH4 is positive because here we are adding an electron to an ion which is already negatively charged, so to overcome the repulsion we need to provide energy.
c) For the already mentioned reasons we can say that ΔH1, ΔH2 and ΔH3 are negative.
d) ΔH4 is positive as it is a endothermic reaction as mentioned above.

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