Electronic configurations of Mg+2 ion and Cl– ion are
- 2, 8 and 2, 8, 8
- 2, 8, 2 and 2, 8, 8
- 2, 8, 8 and 2, 8
2, 8, 2 and 2, 8, 7
The Correct Option is A
Approach Solution - 1
To determine the electronic configurations of Mg+2 and Cl– ions, we start by understanding their neutral atoms:
1. Magnesium (Mg): A neutral magnesium atom has an atomic number of 12, so its electronic configuration is 2, 8, 2. When it loses 2 electrons to form Mg+2, it loses its two outermost electrons, resulting in the configuration 2, 8.
2. Chlorine (Cl): A neutral chlorine atom has an atomic number of 17, making its electronic configuration 2, 8, 7. When it gains one electron to become Cl–, it adds one electron to its outer shell, resulting in the configuration 2, 8, 8.
Hence, the electronic configurations of Mg+2 and Cl– ions are 2, 8 and 2, 8, 8, respectively.
Approach Solution -2
Explanation:
- Magnesium (Mg) → Atomic number = 12 → Neutral atom configuration: 2, 8, 2
- Mg2+ means it has lost 2 electrons → New configuration = 2, 8
- Chlorine (Cl) → Atomic number = 17 → Neutral atom configuration: 2, 8, 7
- Cl– means it has gained 1 electron → New configuration = 2, 8, 8
Correct Answer: 2, 8 and 2, 8, 8
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