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

1 Answer
Nov 8, 2015

Answer:

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

Explanation:

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.