Chemistry · Periodic Trends and Ionization Energy
Which statement best explains why sodium (Na) exhibits a much higher difference between its first and second ionization energies (IE2 − IE1) compared to magnesium (Mg) and silicon (Si)?
Verified Solution4 OptionsUpdated: October 2026👁️1 View
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- 1Sodium is a group 1 alkali metal, so metallic bonding completely determines its ionization potential
- 2All Period 3 elements exhibit identical differences between their first and second ionization energies
- 3Magnesium and silicon have significantly more inner shielding electrons, making their second valence electrons easier to remove
- 4Removing the first valence electron from Na leaves a stable noble-gas electron configuration, making the removal of a second electron from an inner closed shell extremely unfavorable energy-wise✓
Correct answer
Removing the first valence electron from Na leaves a stable noble-gas electron configuration, making the removal of a second electron from an inner closed shell extremely unfavorable energy-wise
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