Question

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

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.

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 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.
Skip to navigation

Answer 1

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

Explanation: Across a period nuclear charge increases, so valence electrons are held more tightly (smaller radius, higher effective nuclear charge). Metals react by losing electrons, so those that hold their electrons more weakly (on the left) are more reactive.