Question

1. describe how the atomic radius(size) and the ionization energy changes
2. within a group(same column)
3. within a period(same row)

sentence starters
from this activity, the models show that as we go down a group, the atomic radius....
for example....
as we go from left to right in the same period, the atomic radius...
one the other hand, as we go down a group, the ionization energy...
finally, as we move from left to right, the ionization energy...
for example....
in conclusion, the atomic radius influences the ionization energy. in general, the larger atoms

Explanation:

• Atomic Radius:
• Within a group: As we go down a group, new electron shells are added. This increases the distance from the nucleus to the outermost electrons, so the atomic radius increases. For example, in Group 1 (alkali metals), lithium (\(Li\)) has a smaller atomic radius than sodium (\(Na\)), which is smaller than potassium (\(K\)).
• Within a period: As we move from left to right in a period, the number of protons in the nucleus increases (increasing the nuclear charge) while the electrons are added to the same shell. The increased nuclear charge pulls the electrons closer, so the atomic radius decreases.
• Ionization Energy:
• Within a group: As we go down a group, the atomic radius increases. The outermost electrons are further from the nucleus and are less tightly held. So, less energy is required to remove an electron, and the ionization energy decreases.
• Within a period: As we move from left to right in a period, the atomic radius decreases (as explained above). The electrons are closer to the nucleus and more tightly held. So, more energy is required to remove an electron, and the ionization energy increases. For example, in Period 3, sodium (\(Na\)) has a lower ionization energy than magnesium (\(Mg\)), which is lower than aluminum (\(Al\)) and so on.

Answer:

• Atomic Radius:
• Within a group: Increases. For example, in Group 1, \(Li < Na < K\).
• Within a period: Decreases.
• Ionization Energy:
• Within a group: Decreases.
• Within a period: Increases. For example, in Period 3, \(Na < Mg < Al\).