Why does the reactivity of metals increase from right to left on the periodic table?(1 point)ResponsesMetals on the right have fewer protons, making it harder to attract electrons from other atoms.Metals on the right have fewer protons, making it harder to attract electrons from other atoms.Metals on the right have more valence energy levels, so the ability of the nucleus to attract electrons is reduced.Metals on the right have more valence energy levels, so the ability of the nucleus to attract electrons is reduced.Metals on the right have more protons, causing valence electrons to be held more strongly.Metals on the right have more protons, causing valence electrons to be held more strongly.Metals on the right have fewer valence energy levels, so electrons are closer to the nucleus and harder to pull away.Metals on the right have fewer valence energy levels, so electrons are closer to the nucleus and harder to pull away.

Answer 1

The correct response explaining why the reactivity of metals increases from right to left on the periodic table is:

Metals on the right have more protons, causing valence electrons to be held more strongly.

As you move from right to left on the periodic table, the number of protons in the nucleus decreases. This results in a weaker positive charge in the nucleus, making it easier for these metals to lose their valence electrons and increase their reactivity. Conversely, metals on the right end of the periodic table, which have more protons, hold their valence electrons more tightly, making them less reactive.