What are the principle geometrical consequences of ionic, covalent and metallic bonding

What are the principle geometrical consequences of ionic, covalent and metallic bonding  

Ionic bonding is long-range in operation, and the electrostatic force that controls the attraction or repulsion is the same in all directions. Thus, the most important geometrical feature of ionic bonding is that it is nondirectional. Atoms linked by ionic forces pack together to minimise the various attractive and repulsive forces so that cations are surrounded mainly by anions, and anions by cations. 

Atoms that are linked by electron-pair bonds are positioned so that orbital overlap is maximised. The orbitals used are also sensitive to bond overlap and hybridisation, so that atomic orbitals frequently mix to give hybrid orbitals with greater overlapping power. The shapes of atomic orbitals and hybrid orbitals are quite definite and point in fixed directions. This leads to the fact that covalent bonding is directional. From a geometrical point of view, the array of covalent bonds in a solid resembles a net. 

The formation of metallic bonds requires that the atoms lose outer electrons to a common electron band that runs throughout the solid. This means that atoms lose a large part of their chemical identity and resemble round spheres. The geometrical consequence of this is that atoms pack together like spheres and the bonding is nondirectional. Atoms simply pack together to minimise the space occupied. 

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