Question

Write the ground state electron configuration for (a) \(S\) (b) \(\mathrm{Sc}\) (c) Si (d) \(\mathrm{Sr}\) (e) \(\mathrm{Sb}\)

Short answer

Question: Provide the ground state electron configurations for the following elements: (a) Sulfur (S), (b) Scandium (Sc), (c) Silicon (Si), (d) Strontium (Sr), and (e) Antimony (Sb). Answer: (a) S: 1s^2 2s^2 2p^6 3s^2 3p^4, (b) Sc: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1, (c) Si: 1s^2 2s^2 2p^6 3s^2 3p^2, (d) Sr: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2, (e) Sb: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^3.

Step-by-step solution

Find the atomic numbers

Consult the periodic table and find the atomic numbers of each element. The atomic numbers of the elements are as follows: (a) S (Sulfur) - 16 (b) Sc (Scandium) - 21 (c) Si (Silicon) - 14 (d) Sr (Strontium) - 38 (e) Sb (Antimony) - 51

Determine the electron configuration

Follow the Aufbau principle, Hund's rule, and the Pauli Exclusion principle to fill in electrons for each element. (a) Sulfur (S) - Atomic number 16: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^4\) (b) Scandium (Sc) - Atomic number 21: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^1\) (c) Silicon (Si) - Atomic number 14: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^2\) (d) Strontium (Sr) - Atomic number 38: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^{10}\) 4p\(^6\) 5s\(^2\) (e) Antimony (Sb) - Atomic number 51: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^{10}\) 4p\(^6\) 5s\(^2\) 4d\(^{10}\) 5p\(^3\) Now we have the ground state electron configurations for the five elements.