Chemistry Homework Help

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Unit Cell

Q. What is the length of the line (labeled c) that runs diagonally across one of the faces of the cube in terms of r (the atomic radius)?

Solved • Aug 28, 2019

Unit Cell

Q. Identify the three types of unit cells shown. Drag the item to the appropriate bin.

Solved • Aug 28, 2019

Unit Cell

Q. A representation of a unit cell for a compound of formula AuxCuy is shown below. (a) Identify the type of units cell shown boy-centered cubic face-centered cubic simple cubic (b) Determine the number of Au atoms (blue spheres) and Cu atoms (yellow spheres) in a unit cell. Au atoms Cu atoms (c) Determine the empirical formula for AuxCuy. (omit states-of-matter from your answer.)

Solved • Jun 24, 2019

Unit Cell

Q. Determine the fraction of an atom in (a) and (b) at the center, and at a single face, edge, or corner of the unit cells pictured below. (a) cesium chloride (Cs+ is green, Cl- is gold.) (b) sodium chloride (Cl- is grey, Na+ is green.)

Solved • Jun 24, 2019

Unit Cell

Q. Determine the empirical formula from the number of atoms in the following unit cells.

Solved • Jun 24, 2019

Unit Cell

Q. Describe the different types of cubic lattices In a primitive cubic unit cell, the lattice points lie at the corners of the cube and at the center of the cube. The cube has 8 corners, and each corner contains _____ of an atom. In a body-centered cubic unit cell, the lattice points at the corners of the cube and at the center of the cube. This means that at different locations This means that at different locations within the unit cell, there exist different fractions of carbon atoms. At the center, we find _____ atoms(s). There is also _____ of an atom at each of the 8 corners. In a face-centered cubic unit cell, the lattice points lie at the corners of the cube and at the centers of the faces of the cube. There is _____ of an atom on each of the 6 faces, and ______ of an atom at each of the 8 corners.

Solved • Jun 24, 2019

Unit Cell

Q. Gold follows a face-centered cubic structure. Calculate the density of gold. (Atomic radius = 166 pm; Molar Mass = 196.97 g/mol)

Solved • Jun 12, 2019