Question

1. explain the trend for ionization energy as you move down a group on the periodic table (from top to bottom). make sure to explain why this trend occurs.
2. explain why sodium (na) has a smaller radius than cesium (cs)
3. explain why chlorine (cl) has a higher electronegativity value than iodine (i).

Explanation:

Question 4

As you move down a group on the periodic table, ionization energy decreases. This is because the out - ermost electrons are in higher energy levels, farther from the nucleus, and are shielded by more inner - shell electrons. So, it takes less energy to remove an electron.

Question 5

Sodium has a smaller radius than cesium because cesium has more electron shells. As you move down a group, the addition of electron shells increases the atomic radius. Sodium is in the third period and cesium in the sixth period, so cesium's outer electrons are in a much larger, more extended shell.

Question 6

Chlorine has a higher electronegativity than iodine because chlorine has a smaller atomic radius and less shielding of its outer electrons. The nucleus of chlorine can attract bonding electrons more strongly. As you move down a group, atomic size increases and electronegativity decreases due to increased shielding and larger atomic radii.

Answer:

Question 4

Ionization energy decreases down a group because outer - electrons are farther from the nucleus and more shielded.

Question 5

Sodium has fewer electron shells than cesium, so its radius is smaller.

Question 6

Chlorine has a smaller radius and less shielding, so it has higher electronegativity than iodine.