Periodic Trends: Atomic Radius and Ionization Energy

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What is the atomic radius?

The atomic radius is the distance from the nucleus of an atom to the outermost electron cloud.

How does atomic radius change across a period?

Atomic radius decreases across a period from left to right.

Why does atomic radius decrease across a period?

Atomic radius decreases across a period due to increased nuclear charge pulling electrons closer to the nucleus.

How does atomic radius change down a group?

Atomic radius increases down a group.

Why does atomic radius increase down a group?

Atomic radius increases down a group because additional electron shells are added, which outweighs the increased nuclear charge effect.

What is ionization energy?

Ionization energy is the energy required to remove an electron from an atom in its gaseous state.

How does ionization energy change across a period?

Ionization energy generally increases across a period.

Why does ionization energy increase across a period?

Ionization energy increases across a period due to greater nuclear charge, making it harder to remove an electron.

How does ionization energy change down a group?

Ionization energy decreases down a group.

Why does ionization energy decrease down a group?

Ionization energy decreases down a group because electrons are farther away from the nucleus, and the increased distance reduces nuclear attraction.

What trend is observed in ionization energy for noble gases?

Noble gases have high ionization energies because they have full valence shells, making electron removal more difficult.

Explain the relationship between atomic radius and ionization energy.

Generally, as atomic radius decreases, ionization energy increases due to the stronger attraction between the nucleus and electrons.

Which element has the smallest atomic radius in the periodic table?

Helium has the smallest atomic radius in the periodic table.

How does shielding affect atomic radius?

Increased shielding from inner electrons allows the outer electrons to be less attracted to the nucleus, increasing atomic radius.

How does effective nuclear charge influence periodic trends?

Effective nuclear charge increases across a period, reducing atomic radius and increasing ionization energy.