Choose an acceptable structure for RbCl(s). Assume that "radius ratio rules" are obeyed and that the ionic radii of Rb+ and Cl− are 148 pm and 181 pm, respectively. Rb+ ions occupy half of the octahedral sites in a face-centred cubic lattice of Cl− ions. Rb+ ions occupy all of the tetrahedral sites in a face-centred cubic lattice of Cl− ions. Rb+ ions occupy all of the cubic sites in a simple cubic lattice of Cl− ions. Rb+ ions occupy half of the tetrahedral sites in a face-centred cubic lattice of Cl− ions. Rb+ ions occupy all of the octahedral sites in a face-centred cubic lattice of Cl− ions.

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Crystal Lattices and Unit Cell

Consider a crystal. The regular and repeating pattern of constituent particles is the most distinguishing feature of crystalline solids. A crystal lattice is formed when these particles are replaced with representative points. The three-dimensional arrangement of constituent particles is known as a crystal lattice. Unit cell is that the smallest portion of a space lattice which when repeated in several directions, generate the whole lattice. Unit cell is a building block of a lattice. It is the smallest unit of cell.