Which of the following represents the change in electronic configuration that is

Question

Which of the following represents the change in electronic configuration that is associated with the first ionization energy of Aluminum? A) [Ne]3s^13p^1 rightarrow [Ne]3s^1 + e^- B) [Ne]3s^23p^1 rightarrow [Ne]3s^1 3P^1 C) [Ne]3s^23p^1 rightarrow [Ne]3s^2 + e^- D) [Ne]3s^2 + e^- rightarrow [Ne]3s^23p^1 What is the general trend in ionization energy and electron affinity values? A) Both decrease as one traverses a period from left to right and both decrease as one descends a group. B) Both decrease as one traverses a period from left to right and both increase as one descends a group. C) Both increase as one traverses a period from left to right and both decrease as one descends a group. D) Both increase as one traverses a period from left to right and both increase as one descends a group.

Explanation / Answer

11. The energy which is needed to remove an electron from an atom is called the ionization energy. The following equation of the first ionization energy of Al.:

Al (g) ----> Al+ (g) + e –

The electronic configuration of aluminum is [Ne] 3s23p1. When the one electron to be removed in the 3p orbital then the electronic configuration of aluminum ion should be, [Ne] 3s2

thus the option C is correct answer.

[Ne] 3s23p1----> [Ne] 3s2 + e-

12. Option C is correct answer.

Because of increasing effective nuclear charge, the first ionization energy and electron affinity both increases as move left to right transverse a row (period) of the periodic table while it decreases as move down a column (group) of the periodic table.

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