MCQ on d and f block element for class 12th NEET | pdf

Hello students, NEET  Chemistry is the scoring paper in the medical entrance examination. Here, you will discover the d and f block elements MCQs for NEET Chemistry. MCQ Questions for all Concepts as per the latest syllabus. Practice more on a regular basis with these d and f block elements for class 12th NEET Chemistry chemistry objective questions bank, improve your subject knowledge & problem-solving skills along with time management.

The d-block and f-block elements are two groups of elements in the periodic table that have partially filled d or f subshells in their common oxidation states.

Elements of d block: The d-block elements are often referred to as transition metals. They are located in groups 3-12 of the periodic table. The d-block is the central block of elements. It is called the ‘d-block’ because the electrons of these elements are in the d orbital. These elements include elements such as iron (Fe), copper (Cu), silver (Ag), and gold (Au), among others.

Elements of f block: The f-block elements, also known as inner transition metals, are located at the bottom of the periodic table, in the lanthanide and actinide series. The f-block is not actually a block of the periodic table, but is part of the d-block. It is called the f-block because it is where the f orbitals begin to fill. The lanthanides are elements 57–71 (La through Lu), and the actinides are elements 89–103 (Ac through Lr).

MCQs on d and f block element for class 12th NEET | PDF

To support NEET aspirants in their preparation, Vedantu provides a curated list of important questions for the D and F Block Elements, expertly solved by subject matter experts. Students can access the free PDF by following the links provided toward the end of the article. This chapter is particularly important for NEET 2025, and students are advised to focus on it thoroughly. The PDF includes key questions along with detailed, step-by-step solutions designed to enhance conceptual understanding. If you’re aiming to score higher in the NEET exam, we strongly recommend practising these essential questions provided by Vedantu.

D and f Block elements MCQ PDF Download

1) The d-block elements start with ____ Period.
a) 4
b) 3
c) 5
d) 6
Answer: a
Explanation: The d-block elements begin from the 4th period. The first d-block element is Scandium (Sc), which belongs to period 4.

2) The d-block belongs to ___ groups to _____ groups.
a) 2 to 12
b) 3 to 11
c) 4 to 12
d) 3 to 12
Answer: d
Explanation: The d-block elements lie between group 3 and group 12 of the periodic table.

3) The anomalous electronic configuration in 3d-series is shown by ______
a) Cr, Cu
b) Sc, Cr
c) Cr, Zn
d) Cr, Mn
Answer: a
Explanation: Chromium (Cr) and Copper (Cu) have unusual electronic configurations due to extra stability of half-filled and fully filled d-orbitals.

4) The abnormal low melting points are shown by
a) Sc, Zn
b) Cr, Fe
c) Mn, Tc
d) Ir, Pt
Answer: c
Explanation: Manganese (Mn) and Technetium (Tc) show low melting points due to irregular atomic structures and weak metallic bonding.

5) In 1st transition series which has low melting point
a) Os
b) Pt
c) Cu
d) Zn
Answer: d
Explanation: Zinc (Zn) has the lowest melting point in the first transition series because of completely filled orbitals and weak metallic bonding.

6) In d-block which has highest density
a) Os
b) Ru
c) Zn
d) Pt
Answer: a
Explanation: Osmium (Os) has the highest density among all d-block elements due to its high atomic mass and tightly packed atoms.

7) The lowest density d-block element is ______
a) Zn
b) Y
c) Sc
d) Cu
Answer: c
Explanation: Scandium (Sc) has the lowest density among d-block elements because it has low atomic mass and larger atomic size.

8) The +1 oxidation state is shown by _______
a) Ru
b) Zn
c) Cu
d) Pt
Answer: c
Explanation: Copper (Cu) shows a +1 oxidation state in compounds like Cu₂O due to the stable 3d¹⁰ configuration after losing one electron.

9) In 5d series, +8 oxidation state is shown by __________
a) Zn
b) Hf
c) Os
d) Mn
Answer: c
Explanation: Osmium (Os) in the 5d series shows +8 oxidation state in compounds like OsO₄, which is the highest known oxidation state.

10) In [Ti(H₂O)₆]³⁺ will absorb yellow-green light but its transmitted colour is _______
a) blue
b) yellow
c) purple
d) red
Answer: c
Explanation: The complex absorbs yellow-green light and shows its complementary colour, which is purple.

11) The colour of transition metal is due to________
a) presence of unpaired d-electron
b) d-d transition
c) nature of ligands and geometry of complex
d) All the above
Answer: d
Explanation: Transition metal compounds show colour because of d-d electronic transitions, unpaired d-electrons, and also the influence of ligands and complex shape on energy levels.

12) Transition elements that show anomalous configurations in first series are_______
a) Cr and Ni
b) Cu and Co
c) Fe and Ni
d) Cr and Cu
Answer: d
Explanation: Chromium and Copper have abnormal configurations for extra stability. Cr is [Ar] 3d⁵4s¹ and Cu is [Ar] 3d¹⁰4s¹.

13) The outer electronic configuration of an atom is 3d⁶ 4s². The atom belongs to________
a) copper family
b) iron family
c) zinc family
d) manganese family
Answer: b
Explanation: The electronic configuration 3d⁶ 4s² matches with Iron (Fe), which is in the iron family.

14) In the first transition series, the incoming electrons enter_______
a) 3d orbitals
b) 4d orbitals
c) 5d orbitals
d) 6d orbitals
Answer: a
Explanation: In the first transition series (period 4), electrons are added to the 3d orbitals.

15) Zinc, cadmium and mercury are
a) d-block elements
b) s-block elements
c) p-block elements
d) f-block elements
Answer: a
Explanation: Zn, Cd, and Hg are in group 12 and have filled d-orbitals, so they are d-block elements even though they show limited transition properties.

16) In the transition elements, the incoming electron occupies (n – 1) d-orbital in preference to
a) ns
b) (n-1)p
c) np
d) (n-1)s
Answer: a
Explanation: Electrons in transition elements fill the (n-1)d orbital before the outermost ns orbital due to lower energy.

17) Among the following outermost configurations of transition metals, which shows the highest oxidation state?
a) 3d³ 4s²
b) 3d⁵ 4s¹
c) 3d⁵ 4s²
d) 3d⁶ 4s²
Answer: c
Explanation: 3d⁵ 4s² corresponds to Manganese (Mn), which can show a maximum oxidation state of +7.

18) Manganese achieves its highest oxidation state in its compound______
a) MnO₂
b) KMnO₄
c) Mn₂O₄
d) KMnO₄
Answer: d
Explanation: In KMnO₄ (potassium permanganate), manganese has an oxidation state of +7, which is its highest possible oxidation state.

19) Transition metals
a) exhibit diamagnetism
b) undergo inert pair effect
c) do not form alloys
d) show variable oxidation states
Answer: d
Explanation: Transition metals show variable oxidation states due to the involvement of both (n-1)d and ns electrons in bonding.

20) The most stable oxidation state of iron is _______
a) -3
b) +3
c) +2
d) -2
Answer: b
Explanation: Iron commonly forms +2 and +3 oxidation states, but +3 is more stable in most of its compounds.

21) FeSO₄ has colour ______
a) green
b) blue
c) violet
d) yellow
Answer: a
Explanation: FeSO₄ appears green due to the presence of Fe²⁺ ions, which cause d-d transitions resulting in a pale green colour.

22) Complexation is shown by__________
a) Au
b) Ag
c) Cu
d) all
Answer: d
Explanation: All these transition metals (Au, Ag, Cu) can form complex compounds due to the availability of d-orbitals for bonding.

23) The spin-only magnetic moment of Mn⁴⁺ ion is nearly
a) 4BM
b) 3BM
c) 6BM
d) 5BM
Answer: a
Explanation: Mn⁴⁺ has 3 unpaired electrons (3d³), and using the formula √(n(n+2)) BM, we get √15 ≈ 3.87 ≈ 4BM.

24) Which of the following statements about the interstitial compounds is incorrect?
a) interstitial compounds are much harder
b) transition metallic carbides are chemically reactive
c) transition metal hydrides are powerful reducing agent
d) interstitial compounds have higher melting points than the pure metal
Answer: b
Explanation: Transition metallic carbides are generally chemically stable, not highly reactive. Hence, this statement is incorrect.

25) Which is not the correct statement about the chemistry of 3d and 4f series elements?
a) 3d elements show more oxidation states than 4f series elements
b) the energy difference between 3d and 4s orbitals is very little
c) Europium (II) is more stable than Ce(II)
d) the paramagnetic character in 3d series elements increases from scandium to copper
Answer: d
Explanation: Paramagnetism depends on unpaired electrons. It does not increase steadily from Sc to Cu; it increases then decreases.

26) Alkaline KMnO₄ is called
a) Schiff’s reagent
b) Baeyer’s reagent
c) Benedict’s reagent
d) Tollen’s reagent
Answer: b
Explanation: Alkaline KMnO₄ is known as Baeyer’s reagent. It is used to test for unsaturation (double or triple bonds) in organic compounds.

27) When potassium dichromate is heated with potassium hydroxide and the solution obtained is acidified, colour becomes_____
a) yellow
b) green
c) orange
d) blue
Answer: c
Explanation: Upon acidification of the solution, orange-coloured dichromate ions (Cr₂O₇²⁻) are formed.

28) The purple colour of permanganate ion (MnO₄⁻) arises due to_______
a) 3d-3d transition of electrons
b) 4f-4f transition of electrons
c) charge transfer
d) 5f-5f transition of electrons
Answer: c
Explanation: The intense purple colour of MnO₄⁻ is due to charge transfer transition between Mn and oxygen, not d-d transitions.

29) Potassium permanganate is used
a) as Baeyer’s reagent
b) in dyeing
c) in the tanning of leather
d) in the manufacture of pigment
Answer: a
Explanation: Potassium permanganate is commonly used as Baeyer’s reagent to test for unsaturation in alkenes and alkynes.

30) The 3d block element that exhibits maximum number of oxidation states is______
a) Mn
b) Ti
c) Sc
d) Zn
Answer: a
Explanation: Manganese (Mn) shows oxidation states from +2 to +7, which is the highest range among 3d elements.

31) The most common lanthanide is_____
a) samarium
b) lanthanum
c) plutonium
d) cerium
Answer: d
Explanation: Cerium (Ce) is the most abundant and commonly used lanthanide in various applications like glass polishing and catalysts.

32) Usually lanthanides form______
a) ionic bond
b) covalent bond
c) co-ordinate bond
d) hydrogen bond
Answer: a
Explanation: Lanthanides typically form ionic bonds due to their large size and +3 oxidation state, which promotes ionic character.

33) The atomic numbers of 4f-series range from_____
a) 57 to 71
b) 58 to 72
c) 58 to 71
d) 57 to 72
Answer: c
Explanation: The 4f series starts from cerium (Z=58) to lutetium (Z=71). Lanthanum (Z=57) is not included in the 4f block.

34) The atomic numbers of 5f-series range from______
a) 89 to 72
b) 89 to 112
c) 90 to 103
d) 90 to 112
Answer: c
Explanation: The 5f block, or actinide series, includes elements from thorium (Z=90) to lawrencium (Z=103).

35) The f-block elements are characterized by_________
a) filling of 4f-subshell
b) filling of (n-2) f-subshell
c) filling of 5f
d) both ‘b’ and ‘c’ above
Answer: b
Explanation: f-block elements involve filling of the (n-2)f orbital. For lanthanides (n=6), (n-2)=4 ⇒ 4f orbital; for actinides (n=7), (n-2)=5 ⇒ 5f orbital.

36) In lanthanides the last electron enters (n-2)f subshell where n is equal to______
a) 6
b) 4
c) 5
d) 7
Answer: a
Explanation: In lanthanides, n = 6 (period 6), so (n-2) = 4. Thus, the last electron enters the 4f subshell.

37) Number of electrons present in f-orbital in antepenultimate shell of Ho (Z=67) is______
a) 11
b) 8
c) 7
d) 9
Answer: a
Explanation: Holmium (Z=67) has 11 electrons in the 4f orbital, which is the antepenultimate shell.

38) f-block elements are also called
a) transition elements
b) coinage elements
c) rare earth elements
d) inner transition elements
Answer: d
Explanation: f-block elements are called inner transition elements because their f-orbitals are filled after d and s orbitals.

39) How many unpaired electrons are present in Ce²⁺
a) 2
b) 3
c) 4
d) 5
Answer: a
Explanation: Ce²⁺ has electronic configuration [Xe] 4f², so it has 2 unpaired electrons.

40) The actual value of lanthanide contraction is equal to about (La to Lu)
a) 21 pm
b) 85 pm
c) 42 pm
d) 106 pm
Answer: a
Explanation: The decrease in ionic radius from La³⁺ to Lu³⁺ is about 21 picometers, which is known as lanthanide contraction.

41) The lanthanide contraction is due to_________
a) increase in atomic number
b) decrease in ionic radii
c) poor shielding effect of 4f-electron
d) both a and c above
Answer: d
Explanation: Lanthanide contraction is caused by the increase in atomic number and the poor shielding effect of 4f electrons, which results in a gradual decrease in atomic and ionic sizes.

42) Some statements are given below,
The lanthanide contraction affects the_______
A) densities
B) post lanthanide element
C) colours
D) basic nature of hydroxides of lanthanides.
Among the above, the false statement is/are
a) A, B and C
b) A and D
c) C only
d) A and C
Answer: c
Explanation: Lanthanide contraction does not significantly affect the color of elements; it affects density, properties of post-lanthanides, and basicity of hydroxides.

43) The normal increase in atomic size i.e. Sc-Y-La, in the periodic table, disappears after La, due to
a) increase in atomic number of lanthanides
b) lanthanide contraction
c) decrease in atomic radii of 4d-elements
d) decrease in number of energy shells in the atoms
Answer: b
Explanation: After lanthanum, the atomic size does not increase as expected due to lanthanide contraction, which results from poor shielding by 4f electrons.

44) In lanthanides Lu(OH)3 is less basic than La(OH)3. This is the effect of (M stands for a lanthanide element).
a) increase in ionic character of M–OH bond
b) decrease in electropositive nature of M
c) decrease in ionic character of M–OH bond
d) lanthanide contraction and decrease in ionic character
Answer: d
Explanation: Lanthanide contraction causes a decrease in ionic radius, which increases covalent character in M–OH bonds, making hydroxides less basic down the group.

45) Identify the correct statement among the following.
a) d-block elements show irregular and erratic chemical properties among themselves
b) La and Lu have partially filled d-orbitals and no other partially filled orbitals
c) the chemistry of various lanthanoids is very similar
d) 4f and 5f orbitals are equally shielded
Answer: c
Explanation: Lanthanides have similar chemistry due to the similar size and common +3 oxidation state; other statements are incorrect or misleading.

46) Which of the following belongs to actinide series of elements?
a) Nd
b) U
c) Sm
d) Pr
Answer: b
Explanation: Uranium (U) is part of the actinide series. The other options are lanthanides.

47) Which of the following actinides does not occur in nature?
a) Th
b) Am
c) U
d) Pa
Answer: b
Explanation: Americium (Am) is synthetic and not found naturally; other actinides like Th, U, and Pa occur in nature.

48) The main reason for more number of oxidation states of the actinides than the corresponding lanthanides.
a) more energy difference between 5f and 6d orbitals than 4f and 5d orbitals
b) less energy difference between 5f and 6d orbitals than 4f and 5d orbitals
c) larger atomic size of actinides
d) more reactive nature of actinides than lanthanides
Answer: b
Explanation: The 5f and 6d orbitals in actinides have smaller energy differences, allowing more oxidation states compared to the 4f and 5d orbitals in lanthanides.

49) Which of the following statement is incorrect regarding lanthanides and actinides?
a) oxidation state of +3 is most common in both the series
b) In both series f-orbitals are progressively filled
c) the elements of these series are radioactive
d) both series show contraction effect
Answer: c
Explanation: Not all lanthanides are radioactive. Most actinides are radioactive, but only a few lanthanides like promethium are radioactive.

50) Most of the ions of lanthanide and actinide series have unpaired electrons in (n-2) f orbitals and hence they are___________
a) diamagnetic
b) paramagnetic
c) ferromagnetic
d) non-magnetic
Answer: b
Explanation: Due to unpaired electrons in f orbitals, most ions of lanthanide and actinide series exhibit paramagnetism.

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