Answer:
Ions of different elements which have
same number of electrons but differ from one another in magnitude of nuclear
charge are known as isoelectronic species.
(i) \[{{F}^{-}}\]
has 10 electrons. Isoelectronic species:
\[N{{a}^{+}},M{{g}^{2+}},A{{l}^{3+}},{{N}^{3-}},{{O}^{2-}}\]
(ii) Ar has
18 electrons. Isoelectronic species:
\[{{K}^{+}},C{{a}^{2+}},{{P}^{3-}},{{S}^{2-}},C{{l}^{2-}}\]
(iii) \[M{{g}^{2+}}\]
has 10 electrons. Isoelectronic species:
\[N{{a}^{+}},A{{l}^{3+}},{{N}^{3-}},{{O}^{2-}},{{F}^{-}}\]
(iv) \[R{{b}^{+}}\]
has 36 electrons. Isoelectronic species:
\[S{{r}^{2+}},Kr,B{{r}^{-}}S{{e}^{2-}},A{{s}^{3-}}\]
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