The oxidation state of cu which are expected to be diamagnetic
Correct answer: C. Cu+1
- A. Cu+2
- B. Cu+4
- C. Cu+1
- D. Cu+3
Explanation
Copper has the configuration [Ar] 3d10 4s1, so Cu+ loses the 4s electron and becomes [Ar] 3d10. All electrons are then paired, making Cu+ diamagnetic. Option a, Cu2+, is the likely mistake because it is a common copper ion, but Cu2+ has a 3d9 configuration with one unpaired electron and is paramagnetic.
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About Electronic Structure of d-Block Elements
The electronic structure of d-block elements covers the filling of the (n-1)d and ns orbitals, general electronic configurations, and the exceptions shown by chromium and copper. It explains how partially filled d orbitals produce variable oxidation states, coloured ions, magnetic behaviour and complex formation, while distinguishing transition elements from elements with completely filled d subshells.
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