Question

Oxygen has lower first ionization enthalpy than nitrogen and fluorine why

Answer 1

Answer:

Explanation:

Oxygen has outer electronic configuration:

2s2 2p4

removal of ine electron from the 2p subshell will make its configuration

2s2 2p3

thus it attains a half filled configuration

thus lesser energy is required to remove an elecron from oxygen

whereas in Nitrogen

the electronic configuration is

2s2 2p3

it has a stable half filled configuration

and thus more energy is required to remove an electron from nitrogen

in case of Flourine

the electronic configuration is

2s2 2p5

it has to gain one more electron to attain noble gas configuration and become stable

thus more energy is required to remove an electron from flourine

thus ionisation enthalpy of oxygen is lesser than nitrogen or flourine