A) s-electrons in \[Mg(Z=12)\]
B) p-electrons in \[Cl\text{ }(Z=17)\]
C) d-electrons in \[Fe(Z=26)\]
D) p-electrons in \[Ne(Z=10)\]
Correct Answer: B
Solution :
Electronic configuration of \[F{{e}^{2+}}\] is \[[Ar]3{{d}^{6}}4{{s}^{0}}\].| \[\therefore \] Number of electrons = 6 |
| \[Mg-1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}\](6d electrons) |
| It matches with the 6d electrons of \[F{{e}^{2+}}\] |
| \[Cl-1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\,3{{s}^{2}}3{{p}^{5}}\](11p elections) |
| It does not match with the 6d electrons of \[F{{e}^{2+}}\]. |
| \[Fe-[Ar]3{{d}^{6}}4{{s}^{2}}\] (6d electrons) |
| It matches with the 6d electrons of \[F{{e}^{2+}}\] |
| \[Ne-1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\] (6p electrons) |
| It matches with the 6d electrons of \[F{{e}^{2+}}\] |
| Hence, \[Cl\] has 11p electrons which does not matches in number with 6d electrons of \[F{{e}^{2+}}\]. |
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