Which of the following statements is incorrect:a)The second ionization energy of sulphur is greater than that of chlorineb)The third ionization energy of phosphorus is greater than that of aluminiumc)The first ionization energy of aluminium is approximately the same as that of galliumd)The second ionization energy of boron is greater than that of carbon.Correct answer is option 'B'. Can you explain this answer?

Question

Answer

Incorrect Statement:

The third ionization energy of phosphorus is greater than that of aluminium.

Explanation:

Ionization energy is defined as the amount of energy required to remove an electron from a gaseous atom or ion. The ionization energy increases across a period and decreases down a group in the periodic table.

(a) The second ionization energy of sulphur is greater than that of chlorine:

Sulphur has a higher atomic number than chlorine. Therefore, the second ionization energy of sulphur is greater than that of chlorine.

(b) The third ionization energy of phosphorus is greater than that of aluminium:

This statement is incorrect. Phosphorus has five valence electrons, and its electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^3. When one electron is removed from phosphorus, it becomes P+. The electronic configuration of P+ is 1s^2 2s^2 2p^6 3s^2 3p^2. To remove another electron from P+, more energy is required, which results in a higher third ionization energy.

On the other hand, aluminium has three valence electrons, and its electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^1. When one electron is removed from aluminium, it becomes Al+. The electronic configuration of Al+ is 1s^2 2s^2 2p^6 3s^2 3p^0. To remove another electron from Al+, less energy is required, which results in a lower third ionization energy.

(c) The first ionization energy of aluminium is approximately the same as that of gallium:

Aluminium and gallium are in the same group of the periodic table, and they have similar electron configurations. Therefore, the first ionization energy of aluminium is approximately the same as that of gallium.

(d) The second ionization energy of boron is greater than that of carbon:

Boron has three valence electrons, and its electronic configuration is 1s^2 2s^2 2p^1. When one electron is removed from boron, it becomes B+. The electronic configuration of B+ is 1s^2 2s^2 2p^0. To remove another electron from B+, more energy is required, which results in a higher second ionization energy.

On the other hand, carbon has four valence electrons, and its electronic configuration is 1s^2 2s^2 2p^2. When one electron is removed from carbon, it becomes C+. The electronic configuration of C+ is 1s^2 2s^2 2p^1. To remove another electron from C+, less energy is required, which results in a lower second ionization energy.

Answer

Third ionization energy of Aluminium is greater than Phosphorus

because in phosphorus the electron at the time of third ionization is removed from 3p orbital which contains one electron

while in aluminium third ionization electron is removed from 3S orbital which contains one electron

now considering the stability of half filled 3S having one electron is more stable than 3p orbital having one electron

thus the amount of energy required to remove electron is more in case of aluminium than that of phosphorus

so correct answer is B because the statement is incorrect hope it would help

Answer

Option B because in third I.A e- release from 3p1 in phosphorus, and in aluminium it release from 3s1 (which more stable bcz half fill) so Al I.A. Greater than phosphorus

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