Question

The factors that influence the ionization energy are:

• A. Size of the atom
• B. Charge of the atom
• C. Size and charge of the atom
• D. Size, charge, and type of electron involved (s, p, d, or f)

Hint:

The factors affecting ionization energy include the nuclear charge, atomic size and the electron type. The ionization energy increases left to right due to nuclear charge, and decreases as you go down a group, because there are more shells that shield the outermost electrons. s-electrons are harder to remove than p-electrons.

Answer 1

The Correct Option is D

Ionization energy, the energy required to remove an electron from a gaseous atom,
depends on the following factors:
• Atomic Size: Smaller atoms have higher ionization energy due to stronger nuclear attraction.
• Nuclear Charge: Higher nuclear charge increases the attraction between the nucleus and electrons, raising ionization energy.
• Type of Electron: Electrons in the s-orbital experience less shielding than those in p, d, or f orbitals, making them harder to remove.
For example, elements in the same period show increasing ionization energy as nuclear charge increases.