Ionization Energy

What is ionization energy and why is it important?

• Ionization energy is the energy released when an electron is added to an atom.

• Ionization energy is the mass of an atom measured in atomic units.

• Ionization energy is the temperature at which an atom becomes a gas.

• Ionization energy is the energy needed to remove an electron from an atom, and it is important for understanding chemical reactivity and bonding.

Describe the general trend of ionization energy across a period in the periodic table.

• Ionization energy increases across a period.

• Ionization energy remains constant across a period.

• Ionization energy decreases across a period.

• Ionization energy fluctuates randomly across a period.

How does ionization energy change down a group in the periodic table?

• Ionization energy increases down a group.

• Ionization energy decreases down a group.

• Ionization energy remains constant down a group.

• Ionization energy fluctuates randomly down a group.

What factors influence the ionization energy of an element?

• Chemical reactivity and phase state

• Temperature and pressure

• Atomic size, nuclear charge, electron shielding, and subshell configuration.

• Atomic weight and density

What role does nuclear charge play in determining ionization energy?

• Nuclear charge increases ionization energy by enhancing the attraction between the nucleus and electrons.

• Nuclear charge has no effect on ionization energy as it is solely determined by electron affinity.

• Higher nuclear charge leads to a decrease in ionization energy due to increased electron repulsion.

• Nuclear charge decreases ionization energy by weakening the attraction between the nucleus and electrons.

Differentiate between first ionization energy and successive ionization energy.

• First ionization energy is the energy required to remove all electrons from an atom.

• Successive ionization energies are always lower than the first ionization energy.

• First ionization energy applies to all elements, while successive ionization energy only applies to metals.

• First ionization energy is for the first electron; successive ionization energies are for subsequent electrons.

Why is the second ionization energy usually higher than the first?

• The second ionization energy is lower due to decreased nuclear charge.

• The first electron removal makes the atom more stable, reducing energy needed for the second.

• The second ionization energy is higher due to increased effective nuclear charge after the first electron is removed.

• The second ionization energy is the same as the first because both involve similar energy levels.

Provide an example of an element with a high first ionization energy and explain why.

• Sodium

• Lithium

• Barium

• Helium

Compare the first ionization energies of sodium and chlorine. Which is higher and why?

• Both sodium and chlorine have the same ionization energy.

• Chlorine has a higher ionization energy than sodium.

• Sodium has a higher ionization energy than chlorine.

• Chlorine has a lower ionization energy than sodium.

How does electron shielding affect ionization energy?

• Electron shielding only affects electron affinity.

• Electron shielding increases ionization energy.

• Electron shielding has no effect on ionization energy.

• Electron shielding decreases ionization energy.