The ionic radii of A- and B- ions are 0-98-10-10 m and 1-81-10-10 m- The coordination number of each ion in AB is-

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Structural Isomerism

The ionic rad...

Question

The ionic radii of $A^{+}$ and $B^{-}$ ions are $0.98 \times 10^{- 10} m$ and $1.81 \times 10^{- 10} m .$ The coordination number of each ion in $A B$ is:

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Solution

The correct option is C 6
$Radius ratio = \frac{Radius of Cation}{Radius of Anion}$
Radius-Ratio Rule:
Size and type of void occupied by an ion is determined by knowing relative size of cations and anions.

$\frac{r_{+}}{r_{-}} = \frac{0.98 \times 10^{- 10}}{1.81 \times 10^{- 10}} = 0.541$

It lies in the range $0.414 - 0.732.$ Hence coordination number of each ion will be 6

Radius Ratio Type of void occupied Coordination Number Examples

< 0.155 Linear Void 2

0.155 to 0.225 Planar Triangular void 3 Boron Oxide

0.225 to 0.414 Tetrahedral Void 4 Zinc Sulphide

0.414 to 0.732 Octahedral Void 6 Sodium Chloride

0.732 to 1 Body Centred Cubic Void 8 Caesium Chloride

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The ionic radii of $A^{+}$ and $B^{-}$ ions are $0.98 \times 10^{- 10} m$ and $1.81 \times 10^{- 10} m$ . The coordination number of each ion in AB is

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Ionic radii of $M g^{2 +}$ and $O^{2 -}$ ions are 66 pm and 140 pm respectively. The type of interstitial void and coordination number of $M g^{2 +}$ ion respectively are

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Structural Isomerism

Standard X Chemistry

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Radius Ratio	Type of void occupied	Coordination Number	Examples
< 0.155	Linear Void	2
0.155 to 0.225	Planar Triangular void	3	Boron Oxide
0.225 to 0.414	Tetrahedral Void	4	Zinc Sulphide
0.414 to 0.732	Octahedral Void	6	Sodium Chloride
0.732 to 1	Body Centred Cubic Void	8	Caesium Chloride

The ionic radii of A+ and B− ions are 0.98×10−10m and 1.81×10−10m. The coordination number of each ion in AB is:

The ionic radii of $A^{+}$ and $B^{-}$ ions are $0.98 \times 10^{- 10} m$ and $1.81 \times 10^{- 10} m .$ The coordination number of each ion in $A B$ is: