Assume that at 298 K and 789 mmHg pressure, 8.4634 g of an alkali metal completely reacts with gaseous halogen in a 0.750 L container. 12.9 kJ are released during the reaction (ΔH = −12.9 kJ). The end product, a binary ionic compound, crystallizes in a unit cell with cations aligned along each edge between anions and anions in a face-centered cubic arrangement. The edge length of the unit cell is 696 pm. Additionally, the cube's center contains a cation. Draw a detailed illustration of the unit cell from above, labeling the ions. Are the anions in contact with each other?

Consider a primitive cubic lattice. If you pull the top straight up keeping all the angles at 90°, determine the primitive lattice that formed.

A hypothetical element has a radius of 156 pm, a molar mass of 196 g/mol, and a density of 10.7 g/cm³. Based on the information given, estimate the value of the Avogadro's number.

The diameter of a K atom is 235 pm Shown below are 2 different ways to pack the atoms.  

Identify which arrangement would lead to a greater density for K if the packing is extended to three dimensions.