Question

Given this image and the ionic radii rCu + = 0.74 ? and rO 2- = 1.26 ?, Cu=63g/mol and O=16g/mol a. Determine how many of each type of ion there are per unit cell? In this structure the ions touch along the body diagonal (large diagonal) of the unit cell. This is shown more clearly in the following Figure C 2.2., where the atoms in the front half of the unit cell have been removed for clarity. Cell edge, a Face diagonal, x Figure C 2.2. Structure of a binary compound Copper Oxygen b. Estimate the length of the edge of the cubic unit cell. c. Estimate the density of the compound. Avogadro’s number is 6.02 x 10^23 atoms per mole.

          Given this image and the ionic radii rCu + = 0.74 ? and rO 2- = 1.26 ?, Cu=63g/mol and O=16g/mol

a. Determine how many of each type of ion there are per unit cell?
In this structure the ions touch along the body diagonal (large diagonal) of the unit cell. This is shown more clearly in the following Figure C 2.2., where the atoms in the front half of the unit cell have been removed for clarity.
Cell edge, a
Face diagonal, x
Figure C 2.2. Structure of a binary compound Copper Oxygen

b. Estimate the length of the edge of the cubic unit cell.
c. Estimate the density of the compound.
Avogadro’s number is 6.02 x 10^23 atoms per mole.

Given this image and the ionic radii rCu + = 0.74 ? and rO 2- = 1.26 ?, Cu=63g/mol and O=16g/mol

a. Determine how many of each type of ion there are per unit cell?
In this structure the ions touch along the body diagonal (large diagonal) of the unit cell. This is shown more clearly in the following Figure C 2.2., where the atoms in the front half of the unit cell have been removed for clarity.
Cell edge, a
Face diagonal, x
Figure C 2.2. Structure of a binary compound Copper Oxygen

b. Estimate the length of the edge of the cubic unit cell.
c. Estimate the density of the compound.
Avogadro’s number is 6.02 x 10^23 atoms per mole.

Added by Marcus S.

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