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Ionization Energy Comparison: S vs P

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Questions and Answers

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?

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?

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?

<p>Sulfur's half-filled 3p orbital is more stable.</p> Signup and view all the answers

Which statement about the ionization energies of sulfur and phosphorus is accurate?

<p>Sulfur has a higher ionization energy than phosphorus.</p> Signup and view all the answers

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!