Periodic trends atomic and ionic radii ionization enthalpy electron gain enthalpy - One Line Questions

1. The ionization enthalpy of Argon is significantly higher than that of Chlorine. This is due to: — Both A and B
2. Which statement about atomic radii is INCORRECT? — Noble gases have larger atomic radii than halogens in the same period.
3. What is isoelectronic species? — Atoms with the same number of electrons
4. Which of the following is an exception to the general trend of ionization enthalpy in Group 13? — B > Al
5. How does electron gain enthalpy generally change across a period? — Becomes more negative (or less positive) from left to right
6. How does electron gain enthalpy generally change down a group? — Becomes less negative (or more positive) down the group
7. The ionization enthalpy of Boron (atomic number 5) is lower than that of Beryllium (atomic number 4). What is the reason? — The electron removed from Boron is from a 2p orbital which is higher in energy than the 2s orbital of Beryllium
8. Which of the following elements has a positive electron gain enthalpy? — Noble gases
9. What is the primary reason for the trend in electron gain enthalpy across a period? — Increase in effective nuclear charge
10. What is the main reason for the increase in atomic radius down a group? — Addition of new electron shells
11. How does atomic radius generally change down a group in the periodic table? — Increases down the group
12. Which statement about electron gain enthalpy is INCORRECT? — Alkaline earth metals have highly negative electron gain enthalpies.
13. What is electron gain enthalpy? — Energy released when an electron is added to a neutral gaseous atom to form an anion
14. What is ionization enthalpy? — Energy required to remove an electron from a neutral gaseous atom
15. The electron gain enthalpies of Group 17 elements (halogens) generally become less negative in the order: — Cl > F > Br > I
16. The electron gain enthalpy of Fluorine is less negative than that of Chlorine. What is the reason? — Fluorine has a smaller atomic radius, leading to interelectronic repulsion in the compact 2p subshell
17. What is the trend in ionic radii down a group? — Generally increases
18. The electronic configuration of an element is 1s²2s²2p⁶3s²3p³. What is the trend of its ionization enthalpy compared to the element with configuration 1s²2s²2p⁶3s¹? — Higher than the element with 3s¹
19. Which symbol represents the first ionization enthalpy? — IE₁
20. What is the primary reason for the increase in ionization enthalpy across a period? — Increase in effective nuclear charge
21. What is the main reason for the decrease in ionization enthalpy down a group? — Increase in shielding effect of inner electrons
22. What is the primary reason for the decrease in atomic radius across a period? — Increase in effective nuclear charge
23. In an isoelectronic series, how does the ionic radius change with increasing nuclear charge? — Decreases
24. How does the first ionization enthalpy generally change down a group? — Decreases down the group
25. How does the first ionization enthalpy generally change across a period? — Increases from left to right
26. How does atomic radius generally change across a period in the periodic table? — Decreases from left to right
27. Which statement about ionization enthalpy is CORRECT? — Noble gases have very low ionization enthalpies.
28. Which of the following ions is smallest in size: K⁺, Cl⁻, S²⁻, P³⁻? — K⁺
29. How does the ionic radius of a cation compare to its parent atom? — Smaller than the parent atom
30. The second ionization enthalpy (IE₂) is always __________ the first ionization enthalpy (IE₁). — greater than
31. Which element is expected to have the smallest atomic radius among Li, Be, B, and C? — C
32. Which element has the highest first ionization enthalpy in the second period? — Ne
33. Which element has the most negative electron gain enthalpy in the second period? — F
34. Which of the following sets of elements shows increasing order of atomic radii? — Li < Be < B < C
35. Which of the following sets of elements shows decreasing order of first ionization enthalpy? — Ne > F > O > N
36. The first ionization enthalpies of Group 1 elements (alkali metals) generally decrease in the order: — Li > Na > K > Rb > Cs
37. Which ion is expected to have the smallest radius: Li⁺, Na⁺, K⁺, or Rb⁺? — Li⁺
38. Which element is expected to have the largest atomic radius among Na, Mg, K, and Ca? — K
39. Which element has the lowest first ionization enthalpy in the third period? — Na
40. The anomaly in the atomic radii trend in the third period is observed between: — Mg and Al
41. The electron gain enthalpy of Nitrogen is positive. This is because: — Nitrogen has a very stable half-filled p-subshell
42. Which factor has the least effect on the ionization enthalpy of an element? — Number of neutrons
43. Which of the following factors primarily determines the atomic radius of an atom? — Distance of the outermost electron from the nucleus
44. Which of the following species is diamagnetic? — O₂²⁻
45. Consider the isoelectronic series: O²⁻, F⁻, Na⁺, Mg²⁺. Which species has the largest ionic radius? — O²⁻
46. A negative electron gain enthalpy indicates that the atom __________. — readily accepts an electron
47. Which of the following has the highest electron affinity (most negative electron gain enthalpy)? — S
48. Which ion is expected to have the largest radius: S²⁻, Cl⁻, K⁺, or Ca²⁺? — S²⁻
49. How does the ionic radius of an anion compare to its parent atom? — Larger than the parent atom
50. Consider the elements X, Y, and Z with atomic numbers 11, 12, and 13 respectively. The correct order of their atomic radii is: — X > Y > Z
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