Atomic Radius and Ionization Energy - Chemistry

Front

What is atomic radius?

Back

The atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons.

Front

How does atomic radius change across a period in the periodic table?

Back

Atomic radius decreases from left to right across a period due to increased nuclear charge pulling electrons closer.

Front

How does atomic radius change down a group in the periodic table?

Back

Atomic radius increases down a group because additional energy levels are added, making the atom larger.

Front

What is ionization energy?

Back

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

Front

How does ionization energy change across a period?

Back

Ionization energy increases across a period due to increased nuclear charge and decreased atomic radius.

Front

How does ionization energy change down a group?

Back

Ionization energy decreases down a group because the outer electrons are further from the nucleus and experience more shielding.

Front

What is the trend of ionization energy for noble gases?

Back

Noble gases have the highest ionization energies in their respective periods due to their stable electron configurations.

Front

What is the relationship between atomic radius and ionization energy?

Back

Generally, as atomic radius increases, ionization energy decreases because the outer electrons are further from the nucleus.

Front

What is effective nuclear charge?

Back

Effective nuclear charge is the net positive charge experienced by an electron in a multi-electron atom, accounting for shielding by other electrons.

Front

How does effective nuclear charge affect atomic radius?

Back

Higher effective nuclear charge pulls electrons closer to the nucleus, resulting in a smaller atomic radius.