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Question
Assertion (A) : Copper is a non-transition element.
Reason (R) : Copper has completely filled d-orbitals in its ground state.
Options
Both (A) and (R) are true and (R) is the correct explanation of (A).
Both (A) and (R) are true, but (R) is not the correct explanation of (A).
(A) is true, but (R) is false.
(A) is false, but (R) is true.
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Solution
(A) is false, but (R) is true.
Explanation:
Copper is a transition metal due to the presence of incompletely filled d-orbital in its common oxidation state Cu+2 (3d9) while in its ground state the electronic configuration of Copper is (3d104s1).
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Silver atom has completely filled d orbitals (4d10) in its ground state. How can you say that it is a transition element?
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Zn2+ ion is iso – electronic with
Explain the observation, at the end of each period, there is a slight increase in the atomic radius of d-block elements.
Name the element of 3d series which exhibits the largest number of oxidation states. Give reason.
Match the properties with the elements of 3d series:
| (i) | lowest enthalpy of atomisation | (p) | Sc |
| (ii) | shows maximum number of oxidation states | (q) | Mn |
| (iii) | transition metal that does not form coloured compounds |
(r) | Zn |
| (s) | Ti |
