Atomic Radius, Forces of Attraction, and Ionization Energy

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

What is the trend of atomic radius down a group in the periodic table?

Back

Atomic radius increases down a group because additional electron shells are added.

Front

Define 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 generally increases across a period due to increased nuclear charge.

Front

What is the trend of ionization energy 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 force of attraction between the nucleus and valence electrons?

Back

It is the electrostatic force that holds the electrons in their orbitals around the nucleus.

Front

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

Back

Na (Sodium) has a larger atomic radius than Cl (Chlorine) because it is located further left on the periodic table.

Front

What is a cation?

Back

A cation is a positively charged ion formed when an atom loses one or more electrons.

Front

What is an anion?

Back

An anion is a negatively charged ion formed when an atom gains one or more electrons.