Questions and Answers
What explains the higher first ionization energy of sulfur compared to phosphorus?
From which orbital is the first valence electron removed in the sulfur atom?
Why is a half-filled 3p orbital more stable than a partially filled 3p orbital in 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?
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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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Description
This quiz explores the differences in first ionization energies between sulfur (S) and phosphorus (P) atoms. It examines how the stability of half-filled orbitals affects the ionization process, highlighting why S has a higher ionization energy compared to P. Test your understanding of atomic structure and ionization processes!
