Single Choice

Which one of the following groups represents a collection of isoelectronic species? (At. nos.: Cs-55, Br-35)

A$$Na^{+}, Ca^{2+}, Mg^{2+}$$
B$$N^{3-}, F^{-}, Na^{+}$$
Correct Answer
C$$Be, Al^{3+}, Cl^{-}$$
D$$Ca^{2+}, Cs^{+}, Br$$

Solution

$$N^{3-}, F^{-}, Na^{+}$$ represents a collection of iso-electronic species. They have 10 electrons each. Iso-electronic species have the same number of electrons. The atomic numbers of N, F and Na are 7,9 and 11 respectively.
Number of electrons in $$N^{3-}=7+3=10$$.
Number of electrons in $$F^{-}=9+1=10$$.
Number of electrons in $$Na^+=11-1=10$$.

SIMILAR QUESTIONS

Chemical Bonding

Which of the following arrangements represents the increasing order (smallest to largest) of ionic radii of the given species $$O^{2-}, S^{2-}, N^{3-}, P^{3-}$$?

Chemical Bonding

The ionic radii (in $$\mathring{A}$$) of $$N^{3-}$$, $$O^{2-}$$ and $$F^{-}$$ are respectively :

Chemical Bonding

The increasing order of the ionic radii of the given isoelectronic species is:

Chemical Bonding

The correct order of decreasing ionic radius among the following anions would be:

Chemical Bonding

Which of the following have the largest ionic size?

Chemical Bonding

The species $$Ar, K^+$$ and $$Ca^{2+}$$ contain the same number of electrons. In which order do their radii increase?

Chemical Bonding

What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions. (i) F$$\displaystyle ^{-}$$ (ii) Ar (iii) Mg$$\displaystyle ^{2+}$$ (iii) Rb$$\displaystyle ^{+}$$

Chemical Bonding

The size of isoelectronic species $$F\displaystyle ^{-}$$, $$Ne$$ and $$Na\displaystyle ^{+}$$ is affected by :

Chemical Bonding

$$K^{+}$$ and $$Cl^{-}$$ ions are isoelectronic. Which of the following statements is not correct?

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