Question

write the ground - state electron configuration for each element. part 1 of 2 s: part 2 of 2 au:

Explanation:

Step1: Recall electron - filling rules

Electrons fill orbitals in the order of increasing energy: 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p. Also, s - orbitals can hold 2 electrons, p - orbitals can hold 6 electrons, d - orbitals can hold 10 electrons, and f - orbitals can hold 14 electrons.

Step2: Determine electron configuration of S

Sulfur (S) has an atomic number of 16. Filling electrons: 1s²2s²2p⁶3s²3p⁴.

Step3: Determine electron configuration of Au

Gold (Au) has an atomic number of 79. The electron - configuration is [Xe]4f¹⁴5d¹⁰6s¹. The [Xe] represents the electron configuration of xenon (atomic number 54), and then we fill the remaining 25 electrons following the energy - level order. However, due to the stability of a full d - subshell and a half - filled s - subshell, the actual configuration of Au has a 6s¹ electron instead of 6s²5d⁹.

Answer:

Part 1 of 2: 1s²2s²2p⁶3s²3p⁴
Part 2 of 2: [Xe]4f¹⁴5d¹⁰6s¹