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.

where is the following

explanation: