Question

Across the periodic table, atomic radius continues to decrease through Group 17. How does this fact help explain why the metals in Group 3 through 13 are less reactive than the metals in Group 1 and 2

Answer 1

The atomic radius decreasing across the periodic table explains why Group 3-13 metals are less reactive than Group 1 and 2 metals.

Step-by-step explanation:

The fact that the atomic radius decreases as you go across the periodic table helps explain why the metals in Group 3 through 13 are less reactive than the metals in Group 1 and 2.

Metals in Group 1 and 2 have larger atomic radii, which means that their outer electrons are further away from the nucleus and are less attracted by the nucleus. This makes it easier for these metals to lose electrons and become more reactive.

Answer 2

valance electrons are being added to the same energy level at the same time the nucleus is increasing in protons. The increase in nuclear charge attracts the electrons more strongly, pulling them closer to the nucleus.