A salt MY crystallizes in the CsCl structure. The anions at the coners touch each other and cation is at the centre. The radius ratio, $\frac{r_{\oplus}}{r_{⊝}}$ for this structure is :

0.225

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0.414

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0.732

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1.0

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Solution

The correct option is D $0.732$
Limitting radius
ratio $= r / R$ Coordination
Number of cation Structural
Arrangement
(Geometry of voids) Example
$0.155 - 0.225$ $3$ Plane Trigonal Boron Oxide
$0.225 - 0.414$ $4$ Tetrahedral $Z n S, S i O_{2}$
$0.414 - 0.732$ $4$ Square planer $-$
$0.414 - 0.732$ $6$ Octahedral $N a C l, M g O_{2}$
$0.732 - 1.000$ $8$ Cubic $C a C l$

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Similar questions

Q. A salt AB crystallises in the CsCl structure. The anions at the corners and the cation in the centre, hence radius ratio

(\frac{r_{t}}{r})

Q. A salt XY crystallises in the CsCl structure. If the anions are located at the corners and the cation in the centre, the radius ratio

\frac{r_{+}}{r_{-}}

is:

Q. A crystalline structure has radius ratio (

r_{+} / r_{-}

) in the range of

0.225 - 0.414

. The coordination number and arrangement of anions around the cations are:

The CsCl type structure is exhibited by alkali halides only when the radius of the cation is large enough to keep touching its eight nearest neighbour anions. Below what minimum ratio of cation to anion radii $(\frac{r_{+}}{r_{-}})$ this contact is prevented ?

A compound having radius ratio,

(\frac{r^{+}}{r^{-}})

in the range of

0.732 - 1

generally has

C s C l

structure.

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Limitting radius ratio $= r / R$	Coordination Number of cation	Structural Arrangement (Geometry of voids)	Example
$0.155 - 0.225$	$3$	Plane Trigonal	Boron Oxide
$0.225 - 0.414$	$4$	Tetrahedral	$Z n S, S i O_{2}$
$0.414 - 0.732$	$4$	Square planer	$-$
$0.414 - 0.732$	$6$	Octahedral	$N a C l, M g O_{2}$
$0.732 - 1.000$	$8$	Cubic	$C a C l$

A salt MY crystallizes in the CsCl structure. The anions at the coners touch each other and cation is at the centre. The radius ratio, r⊕r⊝ for this structure is :

A salt MY crystallizes in the CsCl structure. The anions at the coners touch each other and cation is at the centre. The radius ratio, $\frac{r_{\oplus}}{r_{⊝}}$ for this structure is :