Question

Write the ground state electron configuration for (a) \(\mathrm{C}\) (b) \(\mathrm{Cl}\) (c) Co (d) \(\mathrm{Cs}\) (e) Cd

Short answer

Answer: The ground state electron configurations for the given elements are as follows: - Carbon (C): 1s² 2s² 2p⁴ - Chlorine (Cl): 1s² 2s² 2p⁶ 3s² 3p⁵ - Cobalt (Co): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷ - Cesium (Cs): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s¹ - Cadmium (Cd): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰

Step-by-step solution

Determine Atomic Number (number of electrons)

Carbon has an atomic number of 6, meaning it has 6 electrons in its ground state.

Fill electron orbitals following Aufbau principle, Pauli Exclusion principle, and Hund's rule

Following the Aufbau principle (filling orbitals in order of increasing energy levels), we will put the electrons in the following orbitals: 1s, 2s, and 2p. 1s can hold 2 electrons, 2s can hold 2 electrons, and 2p can hold 6 electrons. We place the 6 electrons as follows: 1s² (2 electrons) → 2s² (2 electrons) → 2p⁴ (4 electrons)

Write ground state electron configuration

The ground state electron configuration for Carbon is: \(\mathrm{1s^2\:2s^2\:2p^4}\). (b) \(\mathrm{Cl}\)

Determine Atomic Number (number of electrons)

Chlorine has an atomic number of 17, meaning it has 17 electrons in its ground state.

Fill electron orbitals following Aufbau principle, Pauli Exclusion principle, and Hund's rule

Following the Aufbau principle, we will put the electrons in the following orbitals: 1s, 2s, 2p, 3s, and 3p. We place the 17 electrons as follows: 1s² (2 electrons) → 2s² (2 electrons) → 2p⁶ (6 electrons) → 3s² (2 electrons) → 3p⁵ (5 electrons)

Write ground state electron configuration

The ground state electron configuration for Chlorine is: \(\mathrm{1s^2\:2s^2\:2p^6\:3s^2\:3p^5}\). (c) Co

Determine Atomic Number (number of electrons)

Cobalt has an atomic number of 27, meaning it has 27 electrons in its ground state.

Fill electron orbitals following Aufbau principle, Pauli Exclusion principle, and Hund's rule

Following the Aufbau principle, we will put the electrons in the following orbitals: 1s, 2s, 2p, 3s, 3p, 4s, 3d, and 4p. We place the 27 electrons as follows: 1s² (2 electrons) → 2s² (2 electrons) → 2p⁶ (6 electrons) → 3s² (2 electrons) → 3p⁶ (6 electrons) → 4s² (2 electrons) → 3d⁷ (7 electrons)

Write ground state electron configuration

The ground state electron configuration for Cobalt is: \(\mathrm{1s^2\:2s^2\:2p^6\:3s^2\:3p^6\:4s^2\:3d^7}\). (d) \(\mathrm{Cs}\)

Determine Atomic Number (number of electrons)

Cesium has an atomic number of 55, meaning it has 55 electrons in its ground state.

Fill electron orbitals following Aufbau principle, Pauli Exclusion principle, and Hund's rule

Following the Aufbau principle, we will put the electrons in the following orbitals: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, and 6s. We place the 55 electrons as follows: 1s² (2 electrons) → 2s² (2 electrons) → 2p⁶ (6 electrons) → 3s² (2 electrons) → 3p⁶ (6 electrons) → 4s² (2 electrons) → 3d¹⁰ (10 electrons) → 4p⁶ (6 electrons) → 5s² (2 electrons) → 4d¹⁰ (10 electrons) → 5p⁶ (6 electrons) → 6s¹ (1 electron)

Write ground state electron configuration

The ground state electron configuration for Cesium is: \(\mathrm{1s^2\:2s^2\:2p^6\:3s^2\:3p^6\:4s^2\:3d^{10}\:4p^6\:5s^2\:4d^{10}\:5p^6\:6s^1}\). (e) Cd

Determine Atomic Number (number of electrons)

Cadmium has an atomic number of 48, meaning it has 48 electrons in its ground state.

Fill electron orbitals following Aufbau principle, Pauli Exclusion principle, and Hund's rule

Following the Aufbau principle, we will put the electrons in the following orbitals: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, and 4d. We place the 48 electrons as follows: 1s² (2 electrons) → 2s² (2 electrons) → 2p⁶ (6 electrons) → 3s² (2 electrons) → 3p⁶ (6 electrons) → 4s² (2 electrons) → 3d¹⁰ (10 electrons) → 4p⁶ (6 electrons) → 5s² (2 electrons) → 4d¹⁰ (10 electrons)

Write ground state electron configuration

The ground state electron configuration for Cadmium is: \(\mathrm{1s^2\:2s^2\:2p^6\:3s^2\:3p^6\:4s^2\:3d^{10}\:4p^6\:5s^2\:4d^{10}}\).