Question

correct order regarding second ionisation potential is 1)N>C>B>Be 2) N>C>Be>B 3)N>B>C>Be 4)Be >N >C >B​

Answer 1

Answer:

Option 3rd is correct

Because the first opinion is decrease in ionic size of the atom. But the question is why B having more ionisation enthalpy than carbon.

Reason is B is 2s2 where as C is 2s2 2p1 hence we know the stability of the S orbital is much more than P orbital. Hence due to this extra stability of the S orbital in B is having more ionisation enthalpy

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Answer 2

The correct order regarding the second ionization potential is Option (3) N > B > C > Be.

Explanation:

The second ionization energy (IE₂) is the amount of energy required to remove an electron from a monovalent cation such as X⁺.

                                     X⁺(g) →X²⁺(g) + e⁻

Like the first ionization energy (IE₁), the second ionization energy (IE₂) is also affected by various factors such as nuclear size, effective nuclear charge, and electronic configuration. The second ionization energies are expected to increase from left to right because the ionic size decreases.

∴ Expected Order of Ionization Potential: Be⁺ < B⁺ < C⁺ < N⁺

→ The electronic configuration of monovalent cation species is as follows:

Be⁺ = 1s², 2s¹

B⁺ = 1s², 2s²

C⁺ = 1s², 2s², 2p¹

N⁺ = 1s², 2s², 2p²

→ After losing an electron Be⁺ is going to attain a noble gas configuration therefore Be⁺ will have the lowest ionization energy.

→ As the 2s subshell of B⁺ is fulfilled therefore its ionization potential will have a higher value. Therefore B⁺ will have a higher value of the ionization potential as compared to C⁺.

∴ Correct Order of Ionization Potential: Be⁺ < C⁺ < B⁺ < N⁺

Therefore the correct order regarding the second ionization potential is Option (3) N > B > C > Be.

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