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

Question

Metals on the right have fewer protons, making it harder to attract electrons from other atoms.
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 valence energy levels, so the ability of the nucleus to attract electrons is
reduced.

Answer 1

The correct statement is: "Metals on the right have more protons, causing valence electrons to be held more strongly."

As you move from right to left across a period in the periodic table, the number of protons in the nucleus decreases, resulting in a weaker positive charge that can attract and hold onto the valence electrons. Consequently, metals on the left side of the periodic table (such as alkali metals) tend to lose their valence electrons more easily, making them more reactive compared to metals on the right (such as transition metals or other post-transition metals).