Which of the following correctly describes the Lewis dot structure for the copper(II) chloride ion, CuCl2?

• A. Cu^{2+} is surrounded by two Cl^{-} ions, each with three lone pairs, and no lone pairs on Cu^{2+}.
• B. Cu^{2+} shares a double bond with each Cl atom, and each Cl has two lone pairs.
• C. Cu^{2+} forms a linear structure with Cl_{2}^{2-}, and each Cl atom has one lone pair.
• D. Cu^{2+} is surrounded by two Cl atoms, each with four lone pairs, and Cu^{2+} has two lone pairs.

Answer: (A)

Verified step by step guidance

1. Identify the species involved: CuCl2 consists of a copper ion with a +2 charge (Cu^{2+}) and two chloride ions (Cl^{-}).
2. Recall that chloride ions (Cl^{-}) typically have a full octet with three lone pairs of electrons around each chlorine atom.
3. Consider the electron configuration of Cu^{2+}: as a metal cation, it usually does not have lone pairs in its valence shell when bonded in ionic compounds.
4. Understand that Cu^{2+} and Cl^{-} ions interact primarily through ionic bonds rather than covalent bonds with shared electron pairs, so no double bonds are expected.
5. Conclude that the Lewis structure should show Cu^{2+} surrounded by two Cl^{-} ions, each Cl having three lone pairs, and no lone pairs on Cu^{2+}.