Which element has the larger ionization energy? a. Li,N
b. Kr, Ne
c.
Li
The Correct Answer and Explanation is:
Correct Answers:
a. N (Nitrogen) has a larger ionization energy than Li (Lithium)
b. Ne (Neon) has a larger ionization energy than Kr (Krypton)
c. Incomplete — Option “c. Li” appears to be a fragment and cannot be answered without more context.
Explanation
Ionization energy is the amount of energy required to remove the outermost electron from a gaseous atom or ion in its ground state. It reflects how tightly an atom holds onto its electrons. A higher ionization energy means the electron is more difficult to remove. Ionization energy depends on several factors, primarily:
- Atomic radius – Smaller atoms hold electrons more tightly due to stronger electrostatic attraction between the nucleus and electrons.
- Nuclear charge (Z) – More protons mean a stronger pull on electrons.
- Electron shielding – Inner-shell electrons repel outer electrons, making them easier to remove.
a. Li vs. N
Lithium (Li) is in Group 1, Period 2, and has one valence electron. Nitrogen (N) is in Group 15, Period 2, and has five valence electrons. Both are in the same period, but nitrogen has a higher nuclear charge and smaller atomic radius. Therefore, nitrogen’s electrons are held more tightly, giving it a higher ionization energy than lithium.
b. Kr vs. Ne
Krypton (Kr) is a noble gas in Period 4, while neon (Ne) is a noble gas in Period 2. Although both are stable with full outer shells, krypton has more electron shells and thus a larger atomic radius. The outer electrons in Kr experience more shielding and are further from the nucleus compared to Ne. As a result, Ne has a significantly higher ionization energy than Kr.
c. Li
This option seems incomplete. If it intended to compare Li to another element, the comparison is missing. If it’s asking whether Li has a high or low ionization energy, the answer is that Li has a relatively low ionization energy due to its single valence electron, which is loosely held.
