Solid RbI has the so-called NaCl structure. The shortest distance between the centre of a rubidium cation and the centre of an iodide anion is 367.0 pm.
Calculate the length of the edge of the conventional face-centred cubic unit cell of RbI.
Calculate the density of solid RbI.
Calculate the shortest distance (centre to centre) between two iodide anions in solid RbI.
2007-02-11 06:10:18 · 1 answers · asked by kyro292 1 in Science & Mathematics ➔ Physics
The length of a side is twice the distance between ions or a = 2*d(Rb-I) = 734.0 pm.
The volume of the unit cell is a^3 and the mass is 4*(Rb+I), so the density is 4*(Rb+I)/a^3
The primitive translation vector to a face is a/2X + a/2Y and the distance is d=sqrt((a/2)^2+(a/2)^2) = a/sqrt(2)
You can plug in the numbers to get the final results.
2007-02-12 17:52:50 · answer #1 · answered by d/dx+d/dy+d/dz 6 · 0⤊ 0⤋