Which statement best describes the effect of low ionization energies and low electronegativities on metallic bonding?

a)the valence electrons are easily delocalized.
b)the valence electrons stay in a single orbital.
c)the valence electrons break free of the crystals.
d)the valence electrons move closer to the nuclei.

The statement "The valence electrons are easily delocalized" best describes the effect of low ionization energies and low electronegativities on metallic bonding. Electronegativity is defined as the atom's ability to attract electrons. In a metallic bond the positive nucleus is surrounded by electrons that are free to move. This delocalized electrons create electrostatic interaction between positive and negative charge, which keeps the metal together. Delocalization makes it difficult for the nucleus to attract electrons towards itself hence low ionization energy and low electronegativity.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.