Question

Metals are good conductor of heat because:
A. they do not have free electrons
B. they gain electrons easily
C. their particles are very closely packed so the vibrations are passed on very quickly
D. all of the above.

Answer 1

Hint: In metals there are no completely paired electrons in the outermost shell which means the electrons leave up the outer shell of the certain atom and further form positive ions and a sea of electrons that are de localised.

Complete step by step solution:
> Talking about the structure of the metal it consists of very enclosed that is closely packed ions of the metals which are arranged in some specific metal lattice. Whereas a pure metal has a very giant structure and the atoms of the pure metal are arranged in the layers when we apply some force to the atom there are chances that the layer could slide over one another. As much as force needed by the atom harder and stronger the metal will be.
Taking an example of sodium having the electronic configuration as\[1{s^2}2{s^2}2{p^6}3{s^1} \]. So, the electronic configuration of the outermost electron in sodium \[3{s^1} \]is which tends to be the free electron and other orbitals are filled so the free electrons work for the heat transmission as the vibration of the electron helps in the transmission of heat.
So basically, all metals contain free electrons which in turn helps in heat transfer running as free electrons do not associate themselves with any atom and are considered to be the valence electrons of metals and are bound loosely. So, this particular electron helps in the formation of a charged fluid which travels from some place to the other in any conductor and helps in the conduction of heat and electricity.

The correct answer is C.

Note: The metal has a loose packed metal lattice which gives the metal an ease to transfer the heat from one atom to the other. Also, the free electron availability of the metal atom makes it efficient to transfer the heat and makes it a good conductor of heat.