Question

which of the following is incorrect a)IE1of Li >IE1 of Be b)IE1 of Be > IE1 of B c)IE1 of Li>IE1 of Na d)IE1 of He >IE1 of Ne

Answer 1

Answer:

option A is correct ans

Explanation:

As we go from left to right in period the ionization potential increases but for Be and B exception.

As the Be has 1s 2 2s 2and boron has 1s 2 2s 2p1

so its easy to remove electron from boron than beryllium.

So, option A is correct.

Answer 2

The incorrect statement among the given options is IE₁ of Li> Be.

• Ionization energy indicates the energy required to remove an electron from the outermost shell of an atom.
• The Ionization energy increases from left to right in a period whereas it decreases down a group.
• Lithium(Li), beryllium(Be), and boron(B) belong to the same period that is the second period.
• So the ionization energy order must be Li<Be<B. But the actual order is Li<Be>B.
• This deviation in order of ionization energy is attributed to the $1s^{2} 2s^{2} 2p^{1}$ configuration of the boron atom. The loss of one electron in the $2p$ orbital results in a stable configuration of the boron. So it readily loses the electron resulting in low ionization energy.
• The ionization energy of lithium is greater than sodium due to the large size of sodium.
• Neon is large in size than helium and has less ionization energy.