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Step 1:I'll solve this problem step by step:
Step 2:: Identify the Copper Ion
Copper typically forms two common ions in aqueous solutions: - Copper(I) ion: Cu⁺ - Copper(II) ion: Cu²⁺
Step 3:: Determine the Most Common Oxidation State
In most water solutions, copper forms the Cu²⁺ (copper(II)) ion. This is the more stable and prevalent form of copper in aqueous environments.
Step 4:: Explain the Charge
The Cu²⁺ ion has a charge of + 2, which means it has lost two electrons from its neutral atomic state.
Step 5:: Verify the Oxidation State
- Neutral copper atom has electron configuration: $$[Ar] 3d^{10} 4s^{1}
- When forming Cu²⁺, it loses two electrons: [Ar] 3d^{9}
Final Answer
In water solutions, copper ions typically have a charge of + 2 (Cu²⁺), forming the copper(II) ion.
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