Questions: Why is the ionization energy of Cl lower than F, but higher than that of S?

Why is the ionization energy of Cl lower than F, but higher than that of S?

Solution

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Solution Steps

Step 1: Understanding Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It is influenced by the nuclear charge, electron shielding, and the distance of the outermost electron from the nucleus.

Step 2: Comparing Cl and F

Fluorine (F) has a higher ionization energy than chlorine (Cl) because F is smaller in size, meaning its valence electrons are closer to the nucleus and more strongly attracted to it. This results in a higher ionization energy for F compared to Cl.

Step 3: Comparing Cl and S

Chlorine (Cl) has a higher ionization energy than sulfur (S) because Cl has a higher nuclear charge and a similar level of electron shielding. This results in a stronger attraction between the nucleus and the valence electrons in Cl, making it harder to remove an electron compared to S.

Final Answer

The ionization energy of Cl is lower than F because F is smaller and has a stronger attraction to its electrons. Cl has a higher ionization energy than S because Cl has a higher nuclear charge with similar shielding, leading to a stronger attraction to its electrons.

\[ \boxed{\text{Cl has lower ionization energy than F, but higher than S.}} \]

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