Which characteristics of metal atoms explain why valence electrons in a metal are delocalized? metal atoms are large and have high electronegativities. metal atoms are small and have low electronegativities. metal atoms are large and have low electronegativities. metal atoms are small and have high electronegativities.

Option C

Metals are known for their electropositive nature, as they can easily donate electrons to get stable electronic configuration. In the periodic table, in group I there are alkali metals which can give 1 electron and form ions and group II elements are alkaline earth metals, they can give 2 electrons to form ions.

Due to the tendency of losing electrons, they are less electronegative in nature.  Also, due to low ionization enthalpy the outermost electrons are delocalized (they can be easily removed).

Also, they can easily lose electrons that means the electrons are far away from the positive charge nucleus (bigger size of atom) as compared to the non-metals which have tendency to gain electrons.

Thus, the best characteristic is metal atoms are large and have low electronegativies.

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).