Explain why the metallic bonds in some metals are stronger than bonds in other metals?

1 Answer
Nov 8, 2015

The physical properties of different metals may be rationalized on the basis of intrinsic nuclear charge and number of valence electrons.


Metallic bonding accounts for the physical properties of metals: malleability; ductility; electrical and thermal conductivity; lustre.

Some metals have more valence electrons to contribute to the metallic network. The alkali metals have only the 1 valence electron to the metallic lattice, and these are low melting solids and liquids.

The #d#-block metals have more valence electrons to contribute, and thus the positive ions in a sea of electrons, become more positive (because they have lost more electrons), and there is a greater density of electron "sea". This is an area where simple chemical considerations lead on to band structure, which I am reluctant (and incompetent!) to discuss.