Class 12 Chemistry · Chapter 2 · Test 1
First-Row Transition Elements
38 MCQs This test covers the definition of a transition element, why Zn and Sc are excluded, the electronic configurations of Ti to Cu and their ions, and the physical properties of the 3d series.
38 questions · 35 min · 38 marks
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Sample questions
The first 5 of 38. Try each one, then tap to see the answer.
Question 1
A transition element is defined as a d-block element that:
- AForms one or more stable ions with incomplete d orbitals
- BHas only s electrons in its outer shell
- CForms ions with completely filled d orbitals only
- DHas a partially filled f subshell
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Answer: A
The definition requires at least one stable ion with an incomplete d subshell.
Question 2
Why is zinc not classified as a transition element?
- AIt has no d electrons
- BIts only ion Zn2+ has a complete 3d10 subshell
- CIt is not in the d-block
- DIt has variable oxidation states
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Answer: B
Zn forms only Zn2+ ([Ar]3d10 4s0) which has a full 3d subshell.
Question 3
The Sc3+ ion is [Ar]3d0 4s0. Why is scandium not classified as a transition element?
- AIt is a non-metal
- BIt is a p-block element
- CIts only stable ion has no d electrons
- DIt has too many oxidation states
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Answer: C
Sc3+ has an empty 3d subshell so it has no stable ion with incomplete d orbitals.
Question 4
How many elements make up the first row of transition elements considered here (Ti to Cu)?
- A5
- B6
- C7
- D8
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Answer: D
Ti V Cr Mn Fe Co Ni and Cu make eight elements.
Question 5
Which groups make up the d-block?
- AGroups 3 to 12
- BGroups 1 and 2
- CGroups 13 to 18
- DGroups 3 to 10
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Answer: A
The d-block is composed of groups 3 to 12.
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