JEE Main - Transition elements electronic configuration occurrence and general characteristics Online Test (MCQ Quiz)

1. What is the general electronic configuration of transition elements?

A) (n-1)d¹⁻¹⁰ ns¹⁻² B) (n-1)d⁰⁻¹⁰ ns² C) (n-1)d¹⁻¹⁰ ns⁰ D) (n-1)d¹⁻⁷ ns¹⁻²

2. Which of the following is NOT a characteristic property of transition metals?

A) Formation of colored compounds B) Exhibition of variable oxidation states C) Paramagnetic behavior D) High ionization enthalpies

3. Transition elements belong to which block of the periodic table?

A) s-block B) p-block C) d-block D) f-block

4. The characteristic property of transition metals that leads to the formation of colored compounds is:

A) Presence of unpaired electrons in d-orbitals B) High melting and boiling points C) Metallic bonding D) Ability to form alloys

5. Which of the following transition metals has the electronic configuration [Ar] 3d⁵ 4s¹?

A) Iron (Fe) B) Chromium (Cr) C) Manganese (Mn) D) Copper (Cu)

6. The variable oxidation states of transition metals are due to:

A) The involvement of both (n-1)d and ns electrons in bonding B) The stability of a completely filled d-subshell C) The large difference in energy between (n-1)d and ns orbitals D) The absence of unpaired electrons

7. Which of the following is an exception to the general electronic configuration of transition elements?

A) Scandium (Sc) B) Titanium (Ti) C) Vanadium (V) D) Chromium (Cr)

8. The catalytic activity of transition metals is attributed to:

A) Variable oxidation states and ability to form complexes B) High density and metallic character C) Paramagnetic nature D) Formation of colored ions

9. Which of the following transition metal ions is colorless in aqueous solution?

A) Cu²⁺ B) Ni²⁺ C) Zn²⁺ D) Fe³⁺

10. The tendency to form complex compounds is a characteristic of transition metals due to:

A) Small ionic radii and high charge density B) Large atomic radii C) Low ionization energy D) Diamagnetic nature

11. Which series of elements are known as the first transition series?

A) Lanthanoids B) Actinoids C) 3d series D) 4d series

12. The magnetic behavior of transition metals is generally:

A) Diamagnetic B) Paramagnetic C) Ferromagnetic D) Antiferromagnetic

13. Why do transition metals generally have high melting and boiling points?

A) Strong metallic bonding due to delocalized electrons and large number of unpaired electrons B) Weak interatomic forces C) Low density D) Presence of only ns electrons

14. Which element marks the beginning of the transition elements in the first period?

A) Potassium (K) B) Calcium (Ca) C) Scandium (Sc) D) Titanium (Ti)

15. The electron configuration of Copper (Cu) is an exception to the general rule because:

A) It achieves a more stable half-filled d-subshell B) It achieves a more stable completely filled d-subshell C) It has a higher ionization energy D) It has a lower electronegativity

16. Which of the following is a common oxidation state for Manganese (Mn)?

A) +1 B) +2 C) +7 D) All of the above

17. Transition metals form alloys because:

A) They have similar atomic radii and crystal structures B) They have very different atomic radii C) They are highly reactive D) They have low melting points

18. The reason for the existence of interstitial compounds formed by transition metals is:

A) Presence of vacant d-orbitals and relatively large interstitial spaces in their crystal lattices B) Small atomic size C) High electronegativity D) Formation of ionic bonds

19. Which of the following is NOT found in elemental form in nature?

A) Copper (Cu) B) Gold (Au) C) Silver (Ag) D) Iron (Fe)

20. The stability of the half-filled (d⁵) and fully-filled (d¹⁰) subshells influences the electronic configuration of which transition elements?

A) Scandium (Sc) and Titanium (Ti) B) Chromium (Cr) and Copper (Cu) C) Vanadium (V) and Iron (Fe) D) Cobalt (Co) and Nickel (Ni)

21. Which of the following transition metals exhibits the highest oxidation state?

A) Iron (Fe) B) Manganese (Mn) C) Cobalt (Co) D) Nickel (Ni)

22. The paramagnetic property arises from the presence of:

A) Unpaired electrons B) Paired electrons C) Completely filled orbitals D) Empty orbitals

23. Which of the following transition metal ions is paramagnetic?

A) Zn²⁺ ([Ar] 3d¹⁰) B) Sc³⁺ ([Ar]) C) Ti⁴⁺ ([Ar]) D) Cu⁺ ([Ar] 3d¹⁰)

24. The atomic radii of transition elements generally:

A) Increase across the period B) Decrease across the period C) Remain constant across the period D) Initially decrease then increase across the period

25. What is the most common oxidation state of Iron (Fe)?

A) +1 B) +2 C) +3 D) +4

26. The lanthanides and actinides are collectively known as:

A) Transition elements B) Inner transition elements C) Main group elements D) Noble gases

27. Which of the following is a characteristic property of the d-block elements?

A) Low melting points B) Formation of colored ions C) High ionization energies D) Tendency to gain electrons

28. The electronic configuration of Chromium (Cr) is [Ar] 3d⁵ 4s¹ because:

A) It achieves a more stable half-filled d-subshell and a half-filled s-subshell B) It achieves a more stable completely filled d-subshell C) The energy difference between 3d and 4s orbitals is minimized D) It forms a more stable +1 oxidation state

29. Which transition metal is known for its use in alloys like stainless steel?

A) Copper (Cu) B) Zinc (Zn) C) Iron (Fe) D) Nickel (Ni)

30. The high density of transition metals is due to:

A) Large atomic mass and relatively small atomic volume B) Small atomic mass and large atomic volume C) Weak metallic bonds D) Low ionization energies

31. Which element has the electronic configuration [Ar] 3d¹⁰ 4s²?

A) Nickel (Ni) B) Copper (Cu) C) Zinc (Zn) D) Gallium (Ga)

32. The tendency of transition metals to form alloys is similar to:

A) Alkali metals B) Alkaline earth metals C) Non-metals D) Halogens

33. Which of the following is a characteristic of the f-block elements (inner transition elements)?

A) Formation of colored ions B) Variable oxidation states C) Lanthanide contraction D) All of the above

34. The color of transition metal compounds is generally explained by:

A) d-d transitions B) Charge transfer transitions C) Ligand field theory D) All of the above

35. Which of the following is an exception to the electronic configuration rule for transition elements in the second series (4d)?

A) Yttrium (Y) B) Zirconium (Zr) C) Niobium (Nb) D) Molybdenum (Mo)

36. The occurrence of transition metals in nature is primarily as:

A) Free elements B) Oxides and sulfides C) Halides D) Carbonates

37. Which of the following transition metal ions is diamagnetic?

A) Fe²⁺ B) Co²⁺ C) Ni²⁺ D) Zn²⁺

38. The general trend in ionization enthalpy of transition elements is:

A) Sharp increase B) Gradual increase C) Sharp decrease D) Gradual decrease

39. The electronic configuration of Manganese (Mn) is [Ar] 3d⁵ 4s².

A) This configuration explains its common +2 oxidation state. B) This configuration explains its common +7 oxidation state. C) This configuration is an exception to the general rule. D) This configuration is similar to Iron (Fe).

40. Which of the following transition metals is liquid at room temperature?

A) Iron (Fe) B) Copper (Cu) C) Mercury (Hg) D) Silver (Ag)

41. The formation of interstitial compounds is favored by:

A) Small non-metal atoms like H, C, N B) Large non-metal atoms C) Metal atoms with large interstitial spaces D) Low coordination numbers

42. Which of the following is a common ore of Iron?

A) Bauxite B) Haematite C) Cinnabar D) Malachite

43. The stability of transition metal ions generally increases with:

A) Increase in nuclear charge B) Decrease in nuclear charge C) Increase in atomic size D) Decrease in ionization energy

44. The electronic configuration of Nickel (Ni) is [Ar] 3d⁸ 4s².

A) It readily forms Ni²⁺ ions. B) It readily forms Ni³⁺ ions. C) It is diamagnetic. D) It exhibits only +2 oxidation state.

45. Which of the following transition metals is used in galvanization?

A) Copper (Cu) B) Zinc (Zn) C) Iron (Fe) D) Nickel (Ni)

46. The lanthanide contraction results in:

A) Similar ionic radii of elements in the 3rd transition series to those in the 2nd transition series B) Larger ionic radii of elements in the 3rd transition series C) Smaller ionic radii of elements in the 2nd transition series D) Increased reactivity of the 3rd transition series elements

47. The most stable oxidation state of Copper (Cu) is:

A) +1 B) +2 C) +3 D) +4

48. Which of the following is a characteristic property of transition metals that is NOT shared by zinc, cadmium, and mercury?

A) Formation of colored compounds B) Variable oxidation states C) Paramagnetic behavior D) All of the above

49. The general electronic configuration of the f-block elements is:

A) (n-2)f¹⁻¹⁴ (n-1)d⁰⁻¹ ns² B) (n-1)d¹⁻¹⁰ ns¹⁻² C) (n-1)f⁰⁻¹⁴ ns² D) (n-2)f¹⁻¹⁴ (n-1)d¹⁻¹⁰ ns¹⁻²

50. Which of the following transition metals has the electronic configuration [Ar] 3d¹⁰ 4s¹?

A) Nickel (Ni) B) Copper (Cu) C) Zinc (Zn) D) Gold (Au)

Transition elements electronic configuration occurrence and general characteristics - Online Test

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