Final Answer:
The correct electronic configuration of Cu²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹ because it has lost two electrons from its neutral state (Cu). This results in the removal of electrons from the 4s orbital before the 3d orbital.Therefore, the correct option is B) The electronic configuration of Cu²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹.
Step-by-step explanation:
Copper (Cu) is a transition metal with an atomic number of 29. The electronic configuration of a neutral copper atom is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹. This is derived by filling the electron orbitals in order of increasing energy levels and following the Pauli exclusion principle and Hund's rule. The 4s orbital is filled before the 3d orbital.
Now, let's consider the copper ions mentioned in the options:
A) Cu⁺ has lost one electron, so its electronic configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰.
B) Cu²⁺ has lost two electrons, so its electronic configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹. (Correct)
C) The electronic configuration of copper atoms is given correctly as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰.
D) The electronic configuration of copper atoms is incorrect as it suggests 4s² 3d⁹, but the correct configuration is 4s¹ 3d¹⁰.
In conclusion, option B is the incorrect statement about copper because the electronic configuration of Cu²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹, not 3d¹⁰ as stated in option B.
Therefore, the correct option is B) The electronic configuration of Cu²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁹.