Question

The 1st ionization potential (ev) of N and O respectively are
(A)8.29,8.29. (B)11.32,11.32
(C)8.29,11.32. (D)11.32,8.32

Answer 1

Answer:

the answer is option d

Explanation:

nitrogen electronic configuration is

$1 { {s}^{2 \:} } \: 2 {s}^{2} \: 2 {p}^{3}$

oxygen electronic configuration is

$1 {s}^{2} \: 2 {s}^{2} \: 2 {p}^{4}$

nitrogen has half filled configuration in outermost subshell. it is stable than oxygen due to half filled subshell.

hence it becomes difficult to remove electron from nitrogen than oxygen.

difficulty is overcome by supplying more energy to remove electron in nitrogen.

so nitrogen has higher ionisation enthalpy than oxygen.

d option suits it.