Answer:
The condensed (noble-gas) electron configuration of copper is [Ar] 3d^10 4s^1.
To understand the electron configuration of copper, we need to first look at the periodic table. Copper (Cu) is located in the transition metals section, specifically in Group 11. The atomic number of copper is 29, which means it has 29 electrons.
The electron configuration describes how these electrons are distributed among the energy levels and orbitals of an atom. It follows a specific pattern based on the Aufbau principle, which states that electrons fill the lowest energy levels and orbitals first before moving to higher ones.
In the case of copper, the noble gas that comes before it in the periodic table is argon (Ar), which has an electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6. The noble gas configuration represents a completely filled outermost energy level, making it stable.
To write the condensed (noble-gas) electron configuration of copper, we start with the noble gas configuration of argon and then add the remaining electrons for copper.
Copper has a total of 29 electrons, so we need to add them to the noble gas configuration of argon. The next two electrons go into the 3d orbital, followed by one electron in the 4s orbital.
Therefore, the condensed (noble-gas) electron configuration of copper is [Ar] 3d^10 4s^1.
In summary, the condensed (noble-gas) electron configuration of copper is [Ar] 3d^10 4s^1. This notation indicates that copper has a noble gas core represented by argon's electron configuration and additional electrons occupying the 3d and 4s orbitals.
Step-by-step explanation: