Group 13 to Group 18 elements, electronic configuration and general trends across periods and down groups - One Line Questions

1. What is the most common oxidation state of elements in Group 17 (Halogens)? — -1
2. What is the electronic configuration of Gallium (Ga)? — [Ar] 3d¹⁰ 4s² 4p¹
3. What is the electronic configuration of Iodine (I)? — [Kr] 4d¹⁰ 5s² 5p⁵
4. What is the electronic configuration of Tin (Sn)? — [Kr] 4d¹⁰ 5s² 5p²
5. What is the electronic configuration of Sulfur (S)? — [Ne] 3s² 3p⁴
6. What is the common oxidation state for most Group 14 elements? — +2 and +4
7. What is the electronic configuration of Neon (Ne)? — 1s² 2s² 2p⁶
8. The trend of decreasing atomic radius across a period is primarily due to: — Both A and B
9. The first ionization enthalpy of Aluminum (Al) is lower than that of Magnesium (Mg) because: — Mg has a stable 3s² configuration.
10. Which element in Group 13 is used in the production of borosilicate glass? — Boron
11. Which element is the lightest p-block metal? — Aluminum
12. Which of the following is a characteristic trend in Group 13 elements moving down the group? — Metallic character increases
13. Which of the following trends is observed across a period in the p-block elements (left to right)? — Metallic character decreases
14. The tendency to exhibit +3 oxidation state in Group 13 elements is strongest for: — Aluminum
15. Which element is the first member of Group 13 in the periodic table? — Boron
16. Which element in Group 13 has a melting point of approximately 29.76 °C, making it a liquid at slightly above room temperature? — Gallium
17. Which element in Group 13 is a crucial component of semiconductors like silicon? — Boron
18. Why does Boron have a higher first ionization enthalpy than Beryllium, despite Beryllium being to its left in the same period? — Beryllium has a stable 2s² configuration.
19. Why are Boron compounds generally covalent? — Boron has a high electronegativity and a small size, making it difficult to form B³⁺ ion.
20. Which is the most abundant p-block element in the Earth's crust? — Aluminum
21. Which element in Group 14 exhibits allotropy? — Carbon
22. Which of the following elements is a metalloid in Group 14? — Silicon
23. Which of the following is the most electronegative element in the entire periodic table? — Fluorine
24. Which is the most reactive non-metal in the periodic table? — Fluorine
25. Which of the following halogens is a pale yellow-green gas at room temperature? — Chlorine
26. The electronic configuration of Helium (He) is 1s². What is its group in the periodic table? — Group 18
27. The inert pair effect is most prominent in which group of p-block elements? — Group 14
28. The relative stability of +3 oxidation state over +5 oxidation state increases down which group? — Group 14
29. Which element in Group 18 is used in lighting, specifically in fluorescent lamps and neon signs? — Neon
30. The trend of increasing atomic radius down a group is mainly due to: — Addition of new electron shells
31. What is the reason for the decreasing ionization enthalpy down Group 13? — Increase in atomic size and shielding effect
32. The electronegativity of elements generally decreases down a group in the p-block due to: — Decreasing atomic size and increasing shielding effect
33. The ability of an atom to attract the shared pair of electrons towards itself is known as: — Electronegativity
34. Which of the following is NOT a characteristic of Boron, the first element of Group 13? — Its atomic radius is larger than Aluminum.
35. The maximum oxidation state of an element in Group 16 generally corresponds to: — Its group number
36. The anomalous behavior of Nitrogen (first element of Group 15) is due to: — Its small size, high electronegativity, and absence of d-orbitals.
37. What is the anomalous behavior of the first element in each p-block group attributed to? — Smaller size, higher electronegativity, and absence of d-orbitals in the valence shell
38. Which element is the heaviest known stable isotope in the p-block? — Bismuth
39. Which oxide of Nitrogen is a neutral oxide? — N₂O
40. Which element in Group 15 is a vital component of nucleic acids and ATP? — Phosphorus
41. Which element in Group 15 is known for its allotropy? — Phosphorus
42. Which element in Group 15 exhibits the least tendency to form covalent compounds? — Bismuth
43. Which element in Group 15 has the electronic configuration [Ar] 3d¹⁰ 4s² 4p³? — Arsenic
44. Which element in Group 15 exhibits amphoteric behavior in its oxides? — Arsenic
45. What is the general electronic configuration of Group 18 elements (Noble Gases)? — ns²np⁶
46. Which element in Group 16 forms the most stable hydrides? — Oxygen
47. Which element in Group 16 has the highest electronegativity? — Oxygen
48. Which element in Group 16 is a gas at room temperature and is essential for respiration? — Oxygen
49. The ionization enthalpy generally increases across a period because: — The nuclear charge increases while the shielding effect remains relatively constant.
50. Which of the following is a characteristic of Group 17 elements (Halogens)? — They readily gain electrons to form halide ions.
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