Consider the following species -Ndisplaystyle -3- - Odisplaystyle -2- -Fdisplaystyle - Nadisplaystyle - - Mgdisplaystyle -2-and Aldisplaystyle -3-a- What is common in them-b- Arrange them in the order of increasing ionic radii-

Question

Toppr Admin · Accepted Answer

-a- All the given species contain same number of electrons -10- Hence- they are isoelectronic species- With increase in the nuclear charge- the ionic size decreases-b- The increasing order of ionic radii is Al3-lt-Mg2-lt-Na-lt-F-x2212-lt-O2-x2212-lt-N3-x2212-

Consider the following species :

N $^{3 -}$ , O $^{2 -}$ ,F $^{-}$ , Na $^{+}$ , Mg $^{2 +}$ and Al $^{3 +}$

(a) What is common in them?

(b) Arrange them in the order of increasing ionic radii.

(a) All the given species contain same number of electrons (10). Hence, they are isoelectronic species. With increase in the nuclear charge, the ionic size decreases.

(b) The increasing order of ionic radii is $A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} < O^{2 -} < N^{3 -}$ .

Consider the following species :N3− , O2− ,F−, Na+ , Mg2+and Al3+(a) What is common in them?(b) Arrange them in the order of increasing ionic radii.

(a) All the given species contain same number of electrons (10). Hence, they are isoelectronic species. With increase in the nuclear charge, the ionic size decreases.(b) The increasing order of ionic radii is Al3+<Mg2+<Na+<F−<O2−<N3−.

Consider the following species :

N $^{3 -}$ , O $^{2 -}$ ,F $^{-}$ , Na $^{+}$ , Mg $^{2 +}$ and Al $^{3 +}$

(a) What is common in them?

(b) Arrange them in the order of increasing ionic radii.

(a) All the given species contain same number of electrons (10). Hence, they are isoelectronic species. With increase in the nuclear charge, the ionic size decreases.

(b) The increasing order of ionic radii is $A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} < O^{2 -} < N^{3 -}$ .