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Atomic Radius:  Increases across a period and a down a group that is because a number of shells increase down a group and distance in between electrons and nucleus increases atomic radius increases
Ionization energy: Increases across a period decreases down a group because number of shells increases down a group shielding effect increases down a group and distance between electron and nucleus increases and nuclear force attraction decreases

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The atomic radius of atoms generally decreases from left to right across a period,  because energy levels are added and this makes the atom bigger.

Moving left to right within a period or upward within a group, the first ionization energy generally increases. The energy required to remove the highest-energy electron from a neutral atom, therefore explaining the decreased

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Atomic Radius - increases as you move down a group and decrease down moving left to right across a period.
Ionization energy - increases as you move across a period and decrease while moving down a group. When moving to the right of a period, the number of electrons increases, and the strength of shielding increases.

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Atomic radius increases when we go down a group because the energy levels increases, but it decrease when we go across a period.
Ionization energy increases when we go across the period put it decreases when we go down a group because because the electrons are held in lower energy orbitals, closer to the nucleus and therefore are more tightly bound (harder to remove)

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Atomic radius- Across a period the atomic radius decreases because of the distance between the energy levels and the nucleus grow father apart. When you move down a group the atomic radius increases.
Ionization energy-  Across a period the ionization energy increases because of of the electromagnetic charge. Down a group it decreases, because the number of electrons increase.

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Atomic Radius: The number of energy level increases as you move down as the group as the number of electrons increases and it decreases across a period.
Ionization Energy: As you move down a group ionization energy decreases while moving across a period it increases.

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Yousif AJ
Atomic Radius: The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons.

Ionization Energy: The minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule.

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Atomic Radius:  Generally, it decreases from left to right across a period. However, as you move down it increases.
Ionization Energy:  ionization energy decreases from moving top to bottom down a periodic table group. Moving down a group, a valence shell is consistently added.

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the atomic radius increases as you go down the group and the energy levels increases
and the ionization energy increases across the period

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Atomic radius increases down a group as energy levels increase. However, atomic radius decreases across a period as electrons are closer to the nucleus.
Ionization energy increases across periods as valence electrons are added to the same energy level. However, ionization energy decreases down a group because as we move down a group, a valence shell is added.

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- Atomic radius decreases across a period and increases down a group, because the size of the atom is smaller and the outer electrons are closer to the neucleus.
- Ionization energy: First Ionization generally increases across the period, because valence shell increases.

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Period: The ionization energy increases across a period as electrons are added in the same energy level and valence electrons increase. The ionization energy decreases down a group because there are more energy shells and the valence electrons are farther from the nucleus, and the atomic radius increases.

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Atomic Radius:  Increases across a period and a down a group that is because a number of shells increase down a group and distance in between electrons and nucleus increases atomic radius increases
Ionization energy: Increases across a period decreases down a group because number of shells increases down a group shielding effect increases down a group and distance between electron and nucleus increases and nuclear force attraction decreases

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Ionization increases across a period and decreases down a group. it is easier for valence electrons to ionize across the period.
Atomic radius increases down a group and decreases across a period. every energy level is gets further away as we move down a group meaning the atomic radius will increase.

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Atomic radius: increases down a group because each energy level is further than the last which makes the radius increase in size, and decreases down a period because electrons are added to the same energy level and protons to the nucleus, this causes a stronger force of attraction which causes the radius to decrease in size.

Ionization energy:
Down a period- increasing nuclear charge, electrons added to the same level.

Down a group: increasing energy levels, screening/shielding effect.

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Ionization energy increases from left to right in a period and decreases from top to bottom in a group, because there will be more electrons blocking the way of the attraction with the outer electrons and across a period the attraction gets stronger since the atomic radius increases.
Atomic radius increases as you move down a group and decreases as it goes across a period, because the attraction gets weaker as it goes across the period and the attraction gets stronger as you go down a group.

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- The atomic radius increases as you move down a group because the energy levels also increase which means each energy level is further away from the nucleus than the last. However, as you move across the period, the atomic radius decreases because the electrons are being added to the same energy level which creates a stronger attraction pulling the electrons to the nucleus.

- Ionization Energy increases across the period as the valence electrons of the atom are increasing. The ionization energy also increases down the group due to the screening effect.