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Questions and Answers
What explains the higher first ionization energy of sulfur compared to phosphorus?
What explains the higher first ionization energy of sulfur compared to phosphorus?
- The presence of a full outer orbital in sulfur
- The stability of a half-filled orbital in sulfur (correct)
- Sulfur has a higher atomic mass than phosphorus
- Phosphorus has more protons, attracting the electron more strongly
From which orbital is the first valence electron removed in the sulfur atom?
From which orbital is the first valence electron removed in the sulfur atom?
- 3s orbital
- 2p orbital
- 3p orbital (correct)
- 1s orbital
Why is a half-filled 3p orbital more stable than a partially filled 3p orbital in phosphorus?
Why is a half-filled 3p orbital more stable than a partially filled 3p orbital in phosphorus?
- It leads to a larger atomic radius.
- It allows for greater electron repulsion.
- It has lower energy due to symmetry and exchange energy. (correct)
- It results in maximum electron pairing.
What is the primary reason more energy is needed to remove the first electron from sulfur compared to phosphorus?
What is the primary reason more energy is needed to remove the first electron from sulfur compared to phosphorus?
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Which statement about the ionization energies of sulfur and phosphorus is accurate?
Which statement about the ionization energies of sulfur and phosphorus is accurate?
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Study Notes
Ionization Energies of Sulfur and Phosphorus
- Sulfur (S) has a higher first ionization energy compared to phosphorus (P).
- The difference in ionization energy can be attributed to the stability of electron configurations.
- The first valence electron from sulfur is extracted from a half-filled 3p orbital.
- In contrast, the first valence electron from phosphorus is removed from a partially filled 3p orbital.
- A half-filled orbital, such as that of sulfur, exhibits greater stability due to electron pairing effects and symmetry.
- This enhanced stability of sulfur's half-filled 3p orbital necessitates greater energy to remove its first valence electron.
- Consequently, removing an electron from sulfur requires more energy than from phosphorus due to these stability differences.
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