[Cu(H2O)6]2+ is known to exhibit a blue color due to d-d transitions in the presence of water ligands.
Questions & Step-by-step Solutions
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Q
Q: What is the color of the complex [Cu(H2O)6]2+?
Solution: [Cu(H2O)6]2+ is known to exhibit a blue color due to d-d transitions in the presence of water ligands.
Steps: 6
Step 1: Identify the complex ion, which is [Cu(H2O)6]2+. This means it has a copper (Cu) ion surrounded by six water (H2O) molecules.
Step 2: Understand that the copper ion in this complex is in a +2 oxidation state (Cu2+).
Step 3: Recognize that the water molecules act as ligands, which means they are attached to the copper ion and influence its properties.
Step 4: Learn that the color of a complex ion is often due to electronic transitions, specifically d-d transitions, which occur when electrons move between different energy levels in the metal ion.
Step 5: Note that for [Cu(H2O)6]2+, these d-d transitions result in the absorption of certain wavelengths of light.
Step 6: Determine that the specific wavelengths absorbed by [Cu(H2O)6]2+ correspond to the color blue, which is why the complex appears blue.
