12-17-24 Exit Ticket (Chemistry)

Front

What is atomic size?

Back

Atomic size refers to the distance from the nucleus of an atom to the outermost shell of electrons. It is typically measured in picometers (pm) or angstroms (Å).

Front

Which has a larger atomic size: Na or Na⁺?

Back

Na has a larger atomic size than Na⁺ because the removal of an electron from Na reduces electron-electron repulsion, resulting in a smaller ionic radius.

Front

What is ionization energy?

Back

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is measured in kilojoules per mole (kJ/mol).

Front

Which has a higher ionization energy: Al or Cl?

Back

Cl has a higher ionization energy than Al because Cl has a greater effective nuclear charge, attracting its electrons more strongly.

Front

Which has a larger ionic size: O⁻¹ or O⁻²?

Back

O⁻² has a larger ionic size than O⁻¹ because the addition of an extra electron increases electron-electron repulsion, causing the ion to expand.

Front

Which has a larger ionic size: Cu⁺¹ or Cu⁺²?

Back

Cu⁺¹ has a larger ionic size than Cu⁺² because the loss of an additional electron in Cu⁺² increases the effective nuclear charge on the remaining electrons, pulling them closer to the nucleus.

Front

What is the trend of atomic size in the periodic table?

Back

Atomic size increases down a group and decreases across a period from left to right due to increasing nuclear charge and electron shielding.

Front

What is the trend of ionization energy in the periodic table?

Back

Ionization energy increases across a period from left to right and decreases down a group due to increased distance from the nucleus and electron shielding.

Front

What is the relationship between atomic size and ionization energy?

Back

Generally, as atomic size increases, ionization energy decreases because the outer electrons are further from the nucleus and experience less attraction.

Front

Define 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.