Periodic Trends Practice

Front

What is ionization energy?

Back

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

Front

Why does ionization energy decrease down a group in the periodic table?

Back

Ionization energy decreases down a group because the valence electrons are farther from the nucleus, reducing the nuclear attraction.

Front

What is the trend of atomic radius as you move down a group?

Back

The atomic radius increases as you move down a group due to the addition of more electron shells.

Front

What is the trend of ionization energy as you move across a period?

Back

Ionization energy generally increases as you move from left to right across a period due to increasing nuclear charge.

Front

Which element has the highest ionization energy in Period 2?

Back

Neon (Ne) has the highest ionization energy in Period 2.

Front

What is the atomic radius of an element?

Back

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

Front

How does the atomic radius change across a period?

Back

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

Front

What is the relationship between atomic mass and atomic radius?

Back

Generally, atomic mass increases down a group, but atomic radius also increases due to additional electron shells.

Front

Which element has a larger atomic radius: Na or Cl?

Back

Sodium (Na) has a larger atomic radius than Chlorine (Cl).

Front

What is the significance of valence electrons in determining chemical properties?

Back

Valence electrons determine how an element reacts chemically and its bonding behavior.