Cesium chloride forms a simple cubic lattice in which Cs+ ions are at the corners and a Cl+ ion is...

Question

Cesium chloride forms a simple cubic lattice in which Cs⁺ ions are at the corners and a Cl⁺ ion is in the center (see Figure XXXXXXXXXXThe cation–anion contact occurs along the body diagonal of the unit cell. (The body diagonal start at one corner and then runs through the center of the cell to the opposite corner.) The length of the edge of the unit cell is 412.3 pm. The Cl⁺ ion has a radius of 181 pm. Calculate the radius of the Cs⁺ ion.

Figure 11.34 The unit cell for cesium chloride, CsCl. The chloride ion is located in the center of the unit cell. The ions are not shown full-size to make it easier to see their locations in the unit cell.

Robert · Accepted Answer

According to the Pythagores theorem, 
=  a 2 + b2 = c2 for a right triangle.  
 Firstly  
we have  to find the length of a diagonal on a face of the unit cell. 
 Since a = b here 
, we may write this as 2l2 = c2  
, where l = length of the edge of the unit cell and c = the diagonal length.

Cesium chloride forms a simple cubic lattice in which Cs + ions are at the corners and a Cl + ion is in the center (see Figure XXXXXXXXXXThe cation–anion contact occurs along the body diagonal of the...

Solution

Answer To This Question Is Available To Download

Related Questions & Answers

Submit New Assignment