In comparison of metals to nonmetals, metals tend to have (choose 3)
A. higher electronegativity values
B. lower ionization energy values
C. negative charges
D. greater conductivity
E. higher ionization energy values
F. lower electronegativity values
G. lower conductivity

B.

D.

F.

Explanation:

Metals tend to me elements of groups I and II

These atoms have low ionization energy, meaning they can easily lose electrons because of their lower mass number – compared to elements in the same period – meaning their valence electrons are loosely held by the nucleus.  This also means that they have low electronegativity – the tendency of the atoms to attract electrons clouds to itself such as in a bond. These metals atoms also form metallic bonds with themselves (unlike nonmetals have preferred covalent bonds) hence they have delocalized electrons that make them good conductors of electricity and heat.

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.