Question

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

Explanation:

• Across a period (left - to - right in the periodic table), the atomic number (number of protons) increases.
• For metals, the reactivity is related to the ease of losing valence electrons.
• As the number of protons (nuclear charge) increases from left to right in a period, the attraction of the nucleus for the valence electrons increases.
• Metals on the right side of a period have a higher nuclear charge (more protons) compared to metals on the left side of the same period.
• This stronger nuclear - electron attraction makes it more difficult for the metal atoms on the right to lose their valence electrons (less reactive), while metal atoms on the left, with a lower nuclear charge (fewer protons in the same period), can lose valence electrons more easily (more reactive). So, the reactivity of metals increases from right to left in a period because metals on the right have more protons, causing valence electrons to be held more strongly.

Answer:

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