Question

Part A

Give the ground-state electron configurationfor silicon ( $\rm Si$ ).

Express the complete electronconfiguration using superscripts where appropriate. For example,the configuration for Li would be entered as1s^22s^1.

Part B

Give the actual ground-stateelectron configuration for copper ( $\rm Cu$ ).

Express the electron configurationusing superscripts where appropriate. For example, theconfiguration for Li would be entered as 1s^22s^1.

Answer 1

Concepts and reason

The problem is based on the concept of electronic configuration of elements.

The distribution of electrons in an orbital is represented by the electronic configuration. The electrons are filled in increasing order of energy.

Fundamentals

Electronic configuration represents the distribution of electrons in the orbital shells and subshells. The electrons are arranged in the increasing order of principal quantum number. While filling the electrons in an orbital they follow Pauli’s Exclusion principle, Hund’s Rule and Aufbau’s Principle. As per Pauli’s Exclusion principle, no two electrons can have the same quantum number. Hund’s rule states that electron will singly occupy the orbital in the subshell with the same spin. Aufbau’s principle state that electrons are filled in the increasing order of energy.

Part A

Silicon atom, Si has 14 electrons. Therefore, the electronic configuration of Silicon is

Part B

Copper atom has 29 electrons. Therefore, the electronic configuration of is .

Ans: Part A

The ground state electronic configuration of Silicon is .

Part B

‎The ground state electronic configuration of is.