MCQ
Which of the order for ionization energy is correct?
- A$Be < B < C < N < O$
- ✓$B < Be < C < O < N$
- C$Be > B > C > N > O$
- D$B < Be < N < C < O$
✓
Answer
Correct option: B.
$B < Be < C < O < N$
b
The correct order for ionization energy is $B \,<\, Be\, <\, C \,< \,O \,< \,N$.
The correct order for ionization energy is $B \,<\, Be\, <\, C \,< \,O \,< \,N$.
On moving from left to right in a period, with increase in the atomic number, the ionisation enthalpy increases.
However there are few exceptions
$(1)$ Ionization energy of $B\,<\,$ ionization energy of $B e$. This is because less amount of energy is required to remove a p electron than s electron from the same principal quantum shell.
$(2)$ Ionization energy of $O\, <\,$ ionization energy of $N$.
Nitrogen has half filled $2 p$ subshell which is very stable. More energy is required for removal of electron from half filled, stable subshell.
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