Which one of the following sets of ions represents a collection of isoelectronic species? (Given: Atomic Number: $F: 9, Cl: 17, Na: 11, Mg: 12, Al: 13, K: 19, Ca: 20, Sc: 21$)
- A$Cl^{+}, Na^{+}, Mg^{2+}, Ca^{2+}$
- B$Ba^{2+}, Sr^{2+}, K^{+}, Ca^{2+}$
- C$N^{3-}, O^{2-}, F^{-}, S^{2-}$
- D$K^{+}, Cl^{-}, Ca^{2+}, Sc^{3+}$
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In the neutral state,the element $M$ consists of the isotopes $_{14}M^{28}$,$_{14}M^{29}$,and $_{14}M^{30}$ in the ratio $60 : 30 : 20$ respectively. Correct statements about $M$ in the natural state include that:
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Reason : Number of protons and electrons are different.
Reason : Number of protons and electrons are different.
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