Why does the reactivity of metals increase from right to left on the periodic table?(1 point)

Question

Responses

Metals 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 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.

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.

Answer 1

The best response to explain 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, metals generally have more protons in their nucleus, which increases the positive charge that attracts the negatively charged electrons. This stronger attraction makes the valence electrons harder to remove, thus decreasing metallic reactivity. In contrast, metals on the left side have fewer protons, so their valence electrons are held less tightly and can be removed more easily, making them more reactive.