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**Hint:**Find the valency of copper ions by taking other atoms in their general form. Follow the principles of electronic configuration. Copper belongs to the d-block in the periodic table. By considering the number of electrons in the d-subshell calculate the group number. By the electronic configuration of copper, we can decide to which period it belongs.

**Complete answer:**

We know that copper exhibits more than one oxidation state. The total charge on compound CuCl is 0. And the general valency of copper is -1. The number of chlorine atoms is 1. So the charge of copper will be +1. It is the lower oxidation state of copper so the compound will be called cuprous chloride. Valency of copper in CuCl is +1.

The total charge on $CuCl_{ 2 }$ is 0. And the general valency of copper is -1. The number of chlorine atoms is 2. So the charge of copper will be +2. It is the higher oxidation state of copper. The compound is called cupric chloride. Cupric ions form a precipitate when reacted with hydrogen sulfide. It forms a blue color complex in the presence of aqueous ammonia.

Copper has 29 electrons in its neutral form. It has d subshell electrons. Electronic configuration of copper is $1s^{ 2 }2s^{ 2 }2p^{ 6 }3s^{ 2 }3p^{ 6 }3d^{ 10 }4s^{ 1 }$.

Configuration $Cu^{ + }$ ion is $1s^{ 2 }2s^{ 2 }2p^{ 6 }3s^{ 2 }3p^{ 6 }3d^{ 10 }$. Electrons are lost from the 4s subshell.

Configuration $Cu^{ +2 }$ ion is $1s^{ 2 }2s^{ 2 }2p^{ 6 }3s^{ 2 }3p^{ 6 }3d^{ 9 }$. Electrons are lost from the 3d subshell.

Copper belongs to the fourth period. It belongs to the eleventh group.

**Note:**Cupric ion is more stable than cuprous ion so copper exists in the +2 oxidation state. In copper, electronic configuration copper has 3d subshell filled before 4s because when inner shells are completely filled they attain more stability.

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