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Standard XII

Chemistry

Introduction to Le Chatelier's Principle

A salt AB cry...

Question

A salt AB crystallises in the CsCl structure. The anions at the corners and the cation in the centre, hence radius ratio $(\frac{r_{t}}{r})$ is

0.225

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0.441

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0.625

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0.732

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Solution

The correct option is D 0.732
For BCC, $\frac{r_{+}}{r_{-}} = 0.732$ or above.

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Similar questions

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 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 :

Q. If the length of body diagonal for

CsCl

, which crystallises into a cubic structure with

{Cl}^{-}

ions at the corners and

{Cs}^{+}

ions at the centre of unit cell is

7 ˚ A

and the radius of

{Cs}^{+}

ion is

1.69 ˚ A

. The radius of

{Cl}^{-}

ion?

Q. If the length of the body diagonal for CsCl which crystallises into a cubic structure with

C l^{-}

ions at the corners and

C s^{+}

ions at the centre of the unit cells is

7 ˚ A

and the radius of the

C s^{+}

ion is

1.69 ˚ A

. What is the radii (in

˚ A

) for

C l^{-}

ion?

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 ?

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

The correct option is D 0.732For BCC, r+r−=0.732 or above.

A salt AB crystallises in the CsCl structure. The anions at the corners and the cation in the centre, hence radius ratio $(\frac{r_{t}}{r})$ is

The correct option is D 0.732
For BCC, $\frac{r_{+}}{r_{-}} = 0.732$ or above.