Why are metals malleable, and ductile, and conductive of heat and electricity?

Question

Olivia Anton · Accepted Answer

Because of #"metallic bonding."#

#"Metallic bonding"# results from the close packing of metal atoms, such that the atoms contribute a few of their valence electrons to the overall lattice. These valence electrons are delocalized, and not associated with any particular atom.

Metallic bonding is thus often described as #"positive ions in a sea of electrons"#, in which the metal nuclei can move with respect to each other, without disrupting the metallic bond.

And since #"metallic bonding"# is thus non-molecular, the individual metal atoms can move with respect to each other without disrupting the metallic bond. As a consequence metals are (i) #"malleable"#, capable of being hammered out into a sheet, and (ii) #"ductile"#, capable of being drawn into a wire. These properties make metals the premier material for making tools.

Most metals also have electrical conductivity due to the delocalization of electrons in metallic bonds.

Wyatt Adkins · Answer

undefined Metals can be easily hammered or drawn into various shapes without breaking apart due to their metallic bonding, which allows metal atoms to slide past one another without breaking bonds. Metals are also conductive of heat and electricity due to the free electrons within their structure, known as delocalized electrons, which can move freely throughout the metal lattice and effectively carry both heat and electric charge.