Asked by julie
What is the predicted order of first ionization energies from highest to lowest for aluminum, phosphorus, silicon, and sulfur?
Al > P > Si > S
Al > Si > P > S
S > P > Si > Al
P > S > Si > Al
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P > S > Si > Al
Explanation: Ionization energy generally increases across a period, but phosphorus (p3, half-filled p subshell) is especially stable so it has the highest IE. Sulfur (p4) is slightly lower than P because of electron pairing repulsion. Silicon and aluminum follow with Si > Al. (Approx. 1st IEs: P ≈ 10.49 eV, S ≈ 10.36 eV, Si ≈ 8.15 eV, Al ≈ 5.99 eV.)
Explanation: Ionization energy generally increases across a period, but phosphorus (p3, half-filled p subshell) is especially stable so it has the highest IE. Sulfur (p4) is slightly lower than P because of electron pairing repulsion. Silicon and aluminum follow with Si > Al. (Approx. 1st IEs: P ≈ 10.49 eV, S ≈ 10.36 eV, Si ≈ 8.15 eV, Al ≈ 5.99 eV.)
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