An ionic crystalline solid, MX2, has cubic unit cell. Which of the following arrangements of the ions is consistent with the stoichiometry of the compound?
I know the answer is M2+ ions at the corners and at each face, 8 X- ions at the body centers. but can someone plane why and how why it is the answer
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I don't know what other choices were presented, so I can't eliminate them, but I can explain why the one you describe is consistent with the requirement that there are twice as many X's as M's.
In the cube, there are 8 corners, but each corner is shared by 8 different cells, so only 1/8 of the M ion at a corner is inside the cube. Therefore, the 8 corners together give you only 1 ion of M. The "face" ions are shared between the cube we are looking at and its facing neighbors, so each face ion lies only half inside the cube; the 6 faces together give you only 3 ions of M. That makes 4 ions of M all told. The "body" ions of X are positioned at coordinates (1/4,1/4,1/4), (1/4,1/4,3/4), (1/4,3/4,3/4), (3/4,3/4,3/4), (3/4,3/4,1/4), (3/4,1/4,1/4), (3/4,1/4,3/4), and (1/4,3/4,1/4). Each of them lies entirely inside the cube, so the cube contains 8 ions of X and 4 ions of M, which is the correct ratio for "MX2".