Question

the atomic radii of the elements in the nitrogen group in the periodic table are given in the table above. which of the following best helps explain the trend of increasing atomic radius from n to bi?

Answer 1

The atomic radius increases from nitrogen to bismuth in the nitrogen group due to the addition of principal energy levels and the larger size of orbitals in these levels, outweighing the increased nuclear charge.

Step-by-step explanation:

The trend of increasing atomic radius from nitrogen (N) to bismuth (Bi) in the nitrogen group can be explained by the Group Trend in the periodic table. As you go down a group, the atomic number increases, which introduces more occupied principal energy levels. Although there is an increase in positive nuclear charge, the impact of additional electron shells is greater, leading to an expansion of the atom's radius with each subsequent element down the group.

Higher principal energy levels have orbitals larger in size compared to those in the lower energy levels. Consequently, as electrons occupy these higher-energy orbitals or shells with each descending element, the atomic radius increases. This effect is due to the increase in the distance of the outermost electrons from the nucleus as we scan down the group.

Answer 2

The increasing atomic radius from nitrogen (N) to bismuth (Bi) in the nitrogen group is attributed to the addition of energy levels or shells as one descends the group. With each successive element, more electron shells are added, causing the outermost electrons to be farther from the nucleus and resulting in larger atomic radii. This trend aligns with the general pattern observed within a group on the periodic table.

Step-by-step explanation:

In a group (or column) of the periodic table, elements have the same number of valence electrons, which are the electrons in the outermost energy level. As you move down a group from nitrogen (N) to bismuth (Bi), you are adding more energy levels or shells.

The key factor influencing atomic radius within a group is the increasing number of electron shells. As you move down the nitrogen group, each subsequent element has an additional electron shell. The outermost electrons are farther away from the nucleus because they are located in a higher energy level, and this results in an increase in atomic radius.

Therefore, the trend of increasing atomic radius from nitrogen (N) to bismuth (Bi) in the nitrogen group can be explained by the addition of energy levels or shells as you go down the group. The outermost electrons are located farther from the nucleus, leading to larger atomic radii for the elements further down the group.