Question

Atoms of elements at the top of a group on the periodic table are smaller than the atoms of elements at the bottom of the group. How does this help explain the difference in the reactivity of metals within a group?

A. The valence electrons of the larger atoms are farther from the nucleus and are easier to remove, so the metals near the top are more reactive than those at the bottom.
B. The valence electrons of the larger atoms are farther from the nucleus and are harder to remove, so the metals near the bottom are more reactive than those at the top.
C. The valence electrons of the larger atoms are farther from the nucleus and are harder to remove, so the metals near the top are more reactive than those at the bottom.
D. The valence electrons of the larger atoms are farther from the nucleus and are easier to remove, so the metals near the bottom are more reactive than those at the top.

Answer 1

Answer:

The answer is D.

Explanation:

Hope this helps.

Answer 2

The difference in the reactivity of metals within a group is explained by D. The valence electrons of the larger atoms are farther from the nucleus and are easier to remove, so the metals near the bottom are more reactive than those at the top.

• As said in the statement, the atoms of elements at the top of a group on the periodic table are smaller than the atoms of elements at the bottom of the group.
• Metals will lose electrons to form anions.
• If an atom is smaller, then the distance of the valence electrons from the nucleus will be less.
• Lesser the distance means the electrostatic force between proton and electron is more.
• Hence, the electron of smaller atoms is not lost easily as compared to that of the larger atoms.
• Hence, the reactivity of the metals near the top is less and that of the metals near the bottom is more.