To determine the correct formula for copper(II) chloride, we need to consider the charges of the ions involved. Copper(II) indicates that the copper ion has a +2 charge, denoted as [tex]\( \text{Cu}^{2+} \)[/tex]. Chloride, which is derived from chlorine, has a -1 charge and is denoted as [tex]\( \text{Cl}^- \)[/tex].
To form a neutral compound (one without any net charge), the positive and negative charges must balance each other out.
Given:
- Copper ion: [tex]\( \text{Cu}^{2+} \)[/tex]
- Chloride ion: [tex]\( \text{Cl}^- \)[/tex]
We know that:
- One copper ion has a charge of +2.
- One chloride ion has a charge of -1.
To balance the +2 charge from the copper ion, we need two chloride ions because two chloride ions together will have a total charge of -2.
Therefore, one copper ion (Cu) will combine with two chloride ions (Cl) to form the compound.
Thus, the correct chemical formula for copper(II) chloride is [tex]\( \text{CuCl}_2 \)[/tex].
So, the correct answer is:
D. [tex]\( \text{CuCl}_2 \)[/tex]
