Al(3+)<Mg(2+)<Na+<F−<O(2−)<N(3−)...
Explanation:
1. Isoelectronic Species:
Isoelectronic species are those which have the same number of electrons. In the given sequence of elements, Al, Mg, Na, FO, and N are present. To determine if they are isoelectronic, we need to compare the number of electrons in each species.
2. Electron Configuration:
To find the number of electrons in each species, we need to determine their electron configurations. The electron configurations of the given elements are as follows:
- Al: 1s² 2s² 2p⁶ 3s² 3p¹
- Mg: 1s² 2s² 2p⁶ 3s²
- Na: 1s² 2s² 2p⁶ 3s¹
- FO: 1s² 2s² 2p⁶
- N: 1s² 2s² 2p³
3. Counting Electrons:
By counting the number of electrons in each species, we get:
- Al: 13 electrons
- Mg: 12 electrons
- Na: 11 electrons
- FO: 10 electrons
- N: 7 electrons
4. Conclusion:
From the above count, we can see that Al, Mg, and Na do not have the same number of electrons. However, FO and N have the same number of electrons, i.e., 10 electrons. Therefore, the given sequence can be described as isoelectronic species.
5. Answer:
Hence, the correct answer is option 'B' - isoelectronic species.
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