Modern periodic law and periodicity in properties - One Line Questions

1. The ionic radius of $F^-$ is larger than that of $O^{2-}$ because: — $O^{2-}$ has a lower ratio of electrons to protons
2. Which of the following oxides is amphoteric? — $Al_2O_3$
3. The first ionization enthalpy is the energy required to remove the most loosely bound electron from: — A neutral gaseous atom
4. Electron gain enthalpy is the energy change when an electron is added to: — A neutral gaseous atom
5. The ionization enthalpies of transition metals show: — A gradual increase
6. Lanthanides and actinides are collectively known as: — Inner transition metals
7. The modern periodic law states that the physical and chemical properties of elements are periodic functions of their: — Atomic number
8. Which property generally increases down a group in the periodic table? — Atomic radius
9. The blocking of d-orbitals in transition metals affects which property significantly? — Color of compounds
10. Non-metallic character generally increases down a group because: — Electronegativity decreases, making it harder to attract electrons
11. Which of the following statements about periodic trends is INCORRECT? — Ionization enthalpy increases down a group.
12. The atomic radii of the elements in the second period show a general decrease from Li to Ne. Which pair of elements deviates from this trend? — Be and B
13. The ionization enthalpy generally increases across a period. Which element is an exception to this trend and has a lower value than the preceding element? — Oxygen
14. Which element is the most electronegative? — Fluorine
15. Who is credited with developing the first modern periodic table based on atomic number? — Henry Moseley
16. Which element has the lowest first ionization enthalpy? — Cesium
17. Which element is the least electronegative among halogens? — Iodine
18. Which of the following is a characteristic property of transition metals? — Variable oxidation states
19. The element with the electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1$ belongs to which group? — Group 1
20. The element with electronic configuration $[Ar] 3d^5 4s^1$ belongs to: — Group 6
21. The element with the electronic configuration $[Kr] 4d^{10} 5s^2$ belongs to: — Group 12
22. The element with the electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^5$ belongs to which group? — Group 17
23. The deviation from the expected trend in electron gain enthalpy for elements like Nitrogen is due to: — Increased electron-electron repulsion in a smaller atom
24. Which element has the highest first ionization enthalpy? — Helium
25. The alkali metals (Group 1) are characterized by: — Low ionization enthalpy and high reactivity
26. The halogens (Group 17) are characterized by: — High electronegativity and tendency to gain one electron
27. Noble gases (Group 18) are characterized by: — Full valence electron shells and very low reactivity
28. Which of the following is a consequence of the lanthanide contraction? — Similar chemical properties between second and third transition series elements
29. Down a group, atomic radius increases primarily because of: — Increase in the number of electron shells
30. Atomic radius generally decreases across a period due to: — Increase in nuclear charge and constant shielding effect
31. The trend in the basicity of oxides across a period is: — Decreases
32. The trend in the basicity of oxides down a group is: — Increases
33. Which of the following properties generally decreases across a period from left to right? — Atomic radius
34. Metallic character generally decreases across a period because: — Nuclear charge increases, making it harder to lose electrons
35. Which of the following is a metalloid? — Silicon
36. Oxidation state refers to the hypothetical charge that an atom would have if: — All its bonds were to atoms of greater electronegativity and the electrons were assigned to the more electronegative atom
37. Which of the following elements has the largest atomic radius? — Li
38. Which of the following pairs of elements have similar chemical properties? — Li and Na
39. The highest ionization enthalpy for the second period elements is observed for: — Neon
40. Elements with a negative electron gain enthalpy tend to: — Gain electrons easily
41. Which of the following elements exhibits the most pronounced metallic character? — Potassium
42. The element that exhibits the highest oxidation state is: — Manganese (Mn)
43. Which property is most affected by the shielding of d-electrons in transition metals? — Ionization enthalpy
44. Which of the following is an exception to the general trend in ionization enthalpy across a period? — Nitrogen ($Z=7$) and Oxygen ($Z=8$)
45. Groups in the modern periodic table represent elements with the same: — Number of valence electrons
46. Electronegativity is the tendency of an atom to attract: — Electrons towards its nucleus in a chemical bond
47. Which element has the most negative electron gain enthalpy? — Chlorine
48. Which of the following ions is isoelectronic with Neon ($Ne^{10+}$)? — All of the above
49. Which of the following elements would have the most positive electron gain enthalpy? — Argon
50. In the modern periodic table, periods correspond to: — The principal quantum number (n)
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