Transition elements electronic configuration occurrence and general characteristics - One Line Questions

1. What is the general electronic configuration of transition elements? — (n-1)d¹⁻¹⁰ ns¹⁻²
2. The general electronic configuration of the f-block elements is: — (n-2)f¹⁻¹⁴ (n-1)d⁰⁻¹ ns²
3. Which of the following is a common oxidation state for Manganese (Mn)? — All of the above
4. What is the most common oxidation state of Iron (Fe)? — +2
5. The most stable oxidation state of Copper (Cu) is: — +1
6. The tendency of transition metals to form alloys is similar to: — Alkaline earth metals
7. Which of the following is a common ore of Iron? — Haematite
8. Which of the following is NOT found in elemental form in nature? — Iron (Fe)
9. Which transition metal is known for its use in alloys like stainless steel? — Iron (Fe)
10. Which of the following transition metals is used in galvanization? — Zinc (Zn)
11. Which of the following transition metal ions is colorless in aqueous solution? — Zn²⁺
12. The color of transition metal compounds is generally explained by: — All of the above
13. The magnetic behavior of transition metals is generally: — Paramagnetic
14. Which of the following transition metal ions is diamagnetic? — Zn²⁺
15. Which of the following is NOT a characteristic property of transition metals? — High ionization enthalpies
16. Which of the following is a characteristic property of transition metals that is NOT shared by zinc, cadmium, and mercury? — All of the above
17. Which of the following is a characteristic of the f-block elements (inner transition elements)? — All of the above
18. The occurrence of transition metals in nature is primarily as: — Oxides and sulfides
19. The atomic radii of transition elements generally: — Decrease across the period
20. The stability of transition metal ions generally increases with: — Increase in nuclear charge
21. Which of the following transition metals has the electronic configuration [Ar] 3d⁵ 4s¹? — Manganese (Mn)
22. Which of the following transition metals exhibits the highest oxidation state? — Manganese (Mn)
23. Which of the following transition metals is liquid at room temperature? — Mercury (Hg)
24. The electron configuration of Copper (Cu) is an exception to the general rule because: — It achieves a more stable completely filled d-subshell
25. The electronic configuration of Chromium (Cr) is [Ar] 3d⁵ 4s¹ because: — It achieves a more stable half-filled d-subshell and a half-filled s-subshell
26. The electronic configuration of Nickel (Ni) is [Ar] 3d⁸ 4s². — It readily forms Ni²⁺ ions.
27. Which series of elements are known as the first transition series? — 3d series
28. The high density of transition metals is due to: — Large atomic mass and relatively small atomic volume
29. Which of the following is a characteristic property of the d-block elements? — Formation of colored ions
30. Which element has the electronic configuration [Ar] 3d¹⁰ 4s²? — Zinc (Zn)
31. Which of the following transition metals has the electronic configuration [Ar] 3d¹⁰ 4s¹? — Copper (Cu)
32. Which element marks the beginning of the transition elements in the first period? — Scandium (Sc)
33. The characteristic property of transition metals that leads to the formation of colored compounds is: — Presence of unpaired electrons in d-orbitals
34. The reason for the existence of interstitial compounds formed by transition metals is: — Presence of vacant d-orbitals and relatively large interstitial spaces in their crystal lattices
35. Transition elements belong to which block of the periodic table? — d-block
36. Which of the following is an exception to the general electronic configuration of transition elements? — Chromium (Cr)
37. The stability of the half-filled (d⁵) and fully-filled (d¹⁰) subshells influences the electronic configuration of which transition elements? — Chromium (Cr) and Copper (Cu)
38. The general trend in ionization enthalpy of transition elements is: — Gradual increase
39. The lanthanide contraction results in: — Similar ionic radii of elements in the 3rd transition series to those in the 2nd transition series
40. The tendency to form complex compounds is a characteristic of transition metals due to: — Small ionic radii and high charge density
41. The formation of interstitial compounds is favored by: — Small non-metal atoms like H, C, N
42. Why do transition metals generally have high melting and boiling points? — Strong metallic bonding due to delocalized electrons and large number of unpaired electrons
43. The variable oxidation states of transition metals are due to: — The involvement of both (n-1)d and ns electrons in bonding
44. Transition metals form alloys because: — They have similar atomic radii and crystal structures
45. The electronic configuration of Manganese (Mn) is [Ar] 3d⁵ 4s². — This configuration explains its common +2 oxidation state.
46. The lanthanides and actinides are collectively known as: — Inner transition elements
47. The paramagnetic property arises from the presence of: — Unpaired electrons
48. The catalytic activity of transition metals is attributed to: — Variable oxidation states and ability to form complexes
49. Which of the following is an exception to the electronic configuration rule for transition elements in the second series (4d)? — Molybdenum (Mo)
50. Which of the following transition metal ions is paramagnetic? — Zn²⁺ ([Ar] 3d¹⁰)
All One Line Questions
E-Book Transition elements electronic configuration occurrence and general characteristics Online Test Transition elements electronic configuration occurrence and general characteristics Question Bank Transition elements electronic configuration occurrence and general characteristics