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Answer 1 · 2015-09-19T03:21:11

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You may want to draw the bonds between them. Just remember that the cation will be attracted to the anion.

Answer 2 · 2016-01-15T21:09:03

It is difficult to draw the lattice structures of ionic compounds without a computer.

It is more important that you be able to recognize the unit cells in the lattice structures.

The positive and negative ions are often in a cubic array. Here are two examples.

$"CsCl"$ , a simple cubic structure

The $"Cl"^-$ ions are the blue atoms at the corners of the cube.

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The $"Cs"^+$ ions are at the centre of the cube.

The unit cell extends through the whole crystal.

This animation shows the $"CsCl"$ lattice, the $"Cs"$ sublattice in blue, and the $"Cl"$ sublattice in brown.

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$"NaCl"$ , a face centred cube

The green $"Cl"^-$ ions occupy each corner and the centre of each face of the cube.

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In the picture below, the $"Na"^+$ ions also occupy a face-centred cubic unit cell.

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These unit cells extend through the whole crystal.

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