Question

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 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.

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.
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Answer 1

The correct response is:

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

This is because, as you move from left to right across a period on the periodic table, the number of protons in the nucleus increases. This means that the positive charge of the nucleus becomes greater, which pulls the valence electrons closer, making it harder for them to be lost and thus decreasing reactivity. Conversely, metals on the left side have fewer protons and their valence electrons are more easily lost, leading to higher reactivity.