Which of the following order of ionization energy is correct?

Question

Which of the following order of ionization energy is correct? (A) B < Be < N < C (B) Be > B > C > N (C) B < Be < C < N (D) Be < B < C < N

Tardigrade Admin · Accepted Answer

Ionisation energy generally increase in a period from left to right. But due to comparatively stabler configuration of Be (1 s2, 2 s2), it has more ionisation energy than Boron (1 s2, 2 s2, 2 p1). Hence, the correct order is: B < Be < C < N

Q. Which of the following order of ionization energy is correct?

B < Be < N < C

Be > B > C > N

B < Be < C < N

Be < B < C < N

Ionisation energy generally increase in a period from left to right. But due to comparatively stabler configuration of Be $(1 s^{2}, 2 s^{2})$ , it has more ionisation energy than Boron $(1 s^{2}, 2 s^{2}, 2 p^{1})$ . Hence, the correct order is : $B < B e < C < N$

Q. Which of the following order of ionization energy is correct?

B < Be < N < C

Be > B > C > N

B < Be < C < N

Be < B < C < N

Ionisation energy generally increase in a period from left to right. But due to comparatively stabler configuration of Be (1s2,2s2), it has more ionisation energy than Boron (1s2,2s2,2p1). Hence, the correct order is : B<Be<C<N

Ionisation energy generally increase in a period from left to right. But due to comparatively stabler configuration of Be $(1 s^{2}, 2 s^{2})$ , it has more ionisation energy than Boron $(1 s^{2}, 2 s^{2}, 2 p^{1})$ . Hence, the correct order is : $B < B e < C < N$