The electron configuration: [Kr] 4d10 , corresponds to which of the following atom/ ion: Sn2 Inj+
The Correct Answer and Explanation is:
The correct answer is Sn²⁺ (Tin (II) ion).
Explanation:
The electron configuration given is:
[Kr] 4d¹⁰
This means the element or ion has:
- The same electron configuration as krypton (Kr), which is the noble gas with atomic number 36
- Plus 10 electrons in the 4d subshell
Let us identify what neutral atom would have this configuration after ionization.
Step 1: Understand the full configuration of neutral tin (Sn)
Tin (Sn) has atomic number 50, meaning a neutral tin atom has 50 electrons. Its ground-state electron configuration is:
[Kr] 5s² 4d¹⁰ 5p²
So, the outermost electrons are:
- 2 electrons in the 5s orbital
- 2 electrons in the 5p orbital
Step 2: What happens when Sn loses electrons to form Sn²⁺
When Sn loses 2 electrons, it forms Sn²⁺. The electrons are removed from the outermost energy level first (which is the 5p and 5s orbitals).
- First, the 2 electrons from the 5p² are removed
- That leaves the configuration: [Kr] 4d¹⁰
So Sn²⁺ has the configuration [Kr] 4d¹⁰.
Step 3: Consider Inj⁺
“Inj⁺” does not correspond to any known chemical symbol or ion. It might be a typo or an undefined species, so we discard it.
Conclusion:
The electron configuration [Kr] 4d¹⁰ corresponds to Sn²⁺, the tin ion with a +2 charge. This ion has lost the two electrons from the 5p orbital, leaving a stable, filled 4d subshell and no electrons in the 5th energy level. This configuration gives the ion some extra stability due to the completely filled 4d subshell.
