Back
- What is the name and formula of the compound commonly used in the manufacture of glass to increase the index of refraction?
Problem 6
Problem 27
An X-ray beam with λ = 154 pm incident on the surface of a crystal produced a maximum reflection at an angle of θ = 28.3°. Assuming n = 1, calculate the separation between layers of atoms in the crystal.
- An X-ray beam of unknown wavelength is diffracted from a NaCl surface. If the interplanar distance in the crystal is 286 pm, and the angle of maximum reflection is found to be 7.23°, what is the wavelength of the X-ray beam? (Assume n = 1.)
Problem 29
Problem 31a
Determine the number of atoms per unit cell for each metal.
(a) Polonium
Problem 31b
Determine the number of atoms per unit cell for each metal.
(b) Tungsten
Problem 31c
Determine the number of atoms per unit cell for each metal.
(c) Nickel
- What is the packing efficiency of a body-centered cubic unit cell?
Problem 33
- What is the packing efficiency of a face-centered cubic unit cell? Please show your work.
Problem 34
Problem 35
Platinum crystallizes with the face-centered cubic unit cell. The radius of a platinum atom is 139 pm. Calculate the edge length of the unit cell and the density of platinum in g/cm3.
Problem 36
Molybdenum crystallizes with the body-centered unit cell. The radius of a molybdenum atom is 136 pm. Calculate the edge length of the unit cell and the density of molybdenum
Problem 39
Rhodium has a density of 12.41 g/cm3 and crystallizes with the face-centered cubic unit cell. Calculate the radius of a rhodium atom.
Problem 40
Barium has a density of 3.59 g/cm3 and crystallizes with the body-centered cubic unit cell. Calculate the radius of a barium atom.
Problem 41
Plonium crystallizes with a simple cubic structure. It has a density of 9.3 g/cm3, a radius of 167 pm, and a molar mass of 209 g/mol. Use these data to calculate Avogadro's number (the number of atoms in one mole).
- Palladium crystallizes with a face-centered cubic structure. It has a density of 12.0 g/cm³, a radius of 138 pm, and a molar mass of 106.42 g/mol. Use these data to calculate Avogadro's number.
Problem 42
Problem 44a
Identify each solid as molecular, ionic, or atomic. a. Ru(s)
Problem 44b
Identify each solid as molecular, ionic, or atomic. b. H2O(s)
Problem 44d
Identify each solid as molecular, ionic, or atomic. d. Xe(s)