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I'm not 100% sure what you mean by 'common elements' but I will just try to explain trends in bonding across the periodic table.

So, groups 1,2, and Al, Ga, In, Tl, Ge, Sn, Pb, Sb, Bi and Po are all metal so all form metallic bonds the strength of these bond increase as we move across the groups as there are not only more delocalised electrons but also a greater positive nuclear charge. so, the electrons are more attracted to the nucleus.

The other group 3 and 4 elements (B, C and Si) form macromolecular or giant covalent structures and covalent bonds as they 3 or 4 outer electrons to share and form a covalent bond with another atom. The many of these strong covalent bonds make these structures strong with high boiling points.

From group 5, 6 and 7 the elements form simple a covalent structures as they do not have enough outer electrons to form many bonds. For example take iodine, iodine forms I2. Between the I2 molecules are forces of attraction called van der walls (IMFs). These are weak and are easy to break giving iodine and the other simple covalent molecules low boiling points.

Lastly there is, group 0, the noble gases which do not bond (except Xe which can actually bond) so they form simple atomic structures with no covalent bonds and these have very very low boiling points.

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Q: The type of bonding formed by common elements can be related to their position in the periodic table including bulk properties of their components explain this theory?
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