Question

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

Explanation:

• Atomic radius within a group: As we go down a group, the atomic radius increases. This is because each subsequent element has an additional electron shell. For example, in Group 1 (the alkali metals), lithium (\(Li\)) has an atomic radius of approximately \(152\) pm, sodium (\(Na\)) has \(186\) pm, and potassium (\(K\)) has \(227\) pm.
• Atomic radius within a period: As we go from left to right in the same period, the atomic radius decreases. This is due to the increasing nuclear charge (number of protons) which attracts the electrons more strongly, pulling them closer to the nucleus.
• Ionization energy within a group: As we go down a group, the ionization energy decreases. The outermost electrons are in higher - energy shells, farther from the nucleus, and are thus easier to remove.
• Ionization energy within a period: As we move from left to right, the ionization energy generally increases. The increased nuclear charge makes it more difficult to remove an electron. For example, in Period 3, sodium (\(Na\)) has an ionization energy of \(496\) kJ/mol, and chlorine (\(Cl\)) has \(1251\) kJ/mol.

Answer:

• Atomic radius:
• Within a group: Increases.
• Within a period: Decreases.
• Ionization energy:
• Within a group: Decreases.
• Within a period: Increases.