Group 13 to Group 18 elements, electronic configuration and general trends across periods and down groups - Question Bank

1. Which element in Group 15 is a vital component of nucleic acids and ATP?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Antimony
2. The tendency to exhibit +3 oxidation state in Group 13 elements is strongest for:
A) Boron
B) Aluminum
C) Gallium
D) Thallium
3. Which is the most reactive non-metal in the periodic table?
A) Chlorine
B) Oxygen
C) Fluorine
D) Bromine
4. What is the electronic configuration of Sulfur (S)?
A) [Ne] 3s² 3p⁴
B) [Ne] 3s² 3p³
C) [Ne] 3s¹ 3p⁵
D) [Ar] 3s² 3p⁴
5. Which element in Group 13 is used in the production of borosilicate glass?
A) Aluminum
B) Boron
C) Gallium
D) Indium
6. The ionization enthalpy generally increases across a period because:
A) The number of electron shells increases.
B) The nuclear charge increases while the shielding effect remains relatively constant.
C) The atomic radius increases.
D) The effective nuclear charge decreases.
7. Which element is the heaviest known stable isotope in the p-block?
A) Lead
B) Bismuth
C) Polonium
D) Astatine
8. Which of the following is a characteristic of Group 17 elements (Halogens)?
A) They are highly electropositive.
B) They readily lose electrons.
C) They readily gain electrons to form halide ions.
D) They have low ionization enthalpies.
9. What is the electronic configuration of Iodine (I)?
A) [Ar] 3d¹⁰ 4s² 4p⁵
B) [Kr] 4d¹⁰ 5s² 5p⁵
C) [Xe] 5d¹⁰ 6s² 6p⁵
D) [Kr] 5s² 5p⁶ 4d¹⁰
10. Which element in Group 14 exhibits allotropy?
A) Carbon
B) Silicon
C) Germanium
D) Tin
11. The trend of increasing atomic radius down a group is mainly due to:
A) Increase in nuclear charge
B) Addition of new electron shells
C) Decrease in effective nuclear charge
D) Increased shielding effect
12. Which is the most abundant p-block element in the Earth's crust?
A) Carbon
B) Silicon
C) Aluminum
D) Oxygen
13. Which element in Group 16 forms the most stable hydrides?
A) Oxygen
B) Sulfur
C) Selenium
D) Tellurium
14. Which oxide of Nitrogen is a neutral oxide?
A) N₂O₅
B) NO₂
C) N₂O
D) NO
15. The first ionization enthalpy of Aluminum (Al) is lower than that of Magnesium (Mg) because:
A) Al has a larger atomic radius.
B) Al has a p-electron which is easier to remove than an s-electron.
C) Mg has a stable 3s² configuration.
D) Al has a greater effective nuclear charge.
16. Why are Boron compounds generally covalent?
A) Boron has a very low ionization enthalpy.
B) Boron has a high electronegativity and a small size, making it difficult to form B³⁺ ion.
C) Boron readily forms ionic bonds.
D) Boron has available d-orbitals in its valence shell.
17. Which element in Group 18 is used in lighting, specifically in fluorescent lamps and neon signs?
A) Helium
B) Neon
C) Argon
D) Krypton
18. Which of the following is the most electronegative element in the entire periodic table?
A) Chlorine
B) Oxygen
C) Fluorine
D) Nitrogen
19. What is the electronic configuration of Tin (Sn)?
A) [Ar] 3d¹⁰ 4s² 4p⁶
B) [Kr] 4d¹⁰ 5s² 5p²
C) [Ar] 4s² 4p⁶ 3d¹⁰
D) [Kr] 5s² 5p⁶ 4d¹⁰
20. The anomalous behavior of Nitrogen (first element of Group 15) is due to:
A) Its small size, high electronegativity, and absence of d-orbitals.
B) Its large size and low ionization enthalpy.
C) Its tendency to form ionic compounds.
D) Its ability to form extensive pi-bonds.
21. Which element in Group 16 has the highest electronegativity?
A) Oxygen
B) Sulfur
C) Selenium
D) Tellurium
22. Which element in Group 15 exhibits amphoteric behavior in its oxides?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Bismuth
23. The trend of decreasing atomic radius across a period is primarily due to:
A) Addition of electrons in the same shell
B) Increased nuclear charge
C) Decreased shielding effect
D) Both A and B
24. Which element in Group 13 is a crucial component of semiconductors like silicon?
A) Boron
B) Aluminum
C) Gallium
D) Indium
25. What is the electronic configuration of Neon (Ne)?
A) 1s² 2s² 2p⁶
B) 1s² 2s² 2p⁵
C) 1s² 2s¹
D) 1s² 2s²
26. Which of the following halogens is a pale yellow-green gas at room temperature?
A) Fluorine
B) Chlorine
C) Bromine
D) Iodine
27. Which allotrope of Phosphorus is the most stable under normal conditions?
A) White Phosphorus
B) Red Phosphorus
C) Black Phosphorus
D) Violet Phosphorus
28. The ability of an atom to attract the shared pair of electrons towards itself is known as:
A) Ionization enthalpy
B) Electron gain enthalpy
C) Electronegativity
D) Atomic radius
29. Which element in Group 15 has the electronic configuration [Ar] 3d¹⁰ 4s² 4p³?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Arsenic
30. The relative stability of +3 oxidation state over +5 oxidation state increases down which group?
A) Group 13
B) Group 14
C) Group 15
D) Group 16
31. Which element in Group 13 has a melting point of approximately 29.76 °C, making it a liquid at slightly above room temperature?
A) Boron
B) Aluminum
C) Gallium
D) Indium
32. The electronic configuration of Helium (He) is 1s². What is its group in the periodic table?
A) Group 1
B) Group 2
C) Group 18
D) Group 17
33. What is the most common oxidation state of elements in Group 17 (Halogens)?
A) -1
B) 0
C) +1
D) +3
34. Which element in Group 16 is a gas at room temperature and is essential for respiration?
A) Sulfur
B) Selenium
C) Oxygen
D) Tellurium
35. The electronegativity of elements generally decreases down a group in the p-block due to:
A) Increasing nuclear charge
B) Decreasing atomic size and increasing shielding effect
C) Increasing effective nuclear charge
D) D-orbital participation
36. Which of the following elements is a metalloid in Group 14?
A) Carbon
B) Silicon
C) Germanium
D) Tin
37. What is the anomalous behavior of the first element in each p-block group attributed to?
A) Larger size and higher ionization enthalpy
B) Presence of d-orbitals in the valence shell
C) Smaller size, higher electronegativity, and absence of d-orbitals in the valence shell
D) Greater tendency to form ionic compounds
38. Which element in Group 15 exhibits the least tendency to form covalent compounds?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Bismuth
39. Why does Boron have a higher first ionization enthalpy than Beryllium, despite Beryllium being to its left in the same period?
A) Boron has a larger atomic radius.
B) Boron's valence electrons are in a 2p orbital, which is higher in energy than the 2s orbital of Beryllium.
C) Beryllium has a stable 2s² configuration.
D) Boron has a greater effective nuclear charge.
40. What is the electronic configuration of Gallium (Ga)?
A) [Ar] 3d¹⁰ 4s² 4p¹
B) [Ne] 3d¹⁰ 4s² 4p¹
C) [Ar] 4s² 4p⁶ 3d¹⁰
D) [Ar] 3d¹⁰ 4s¹ 4p²
41. Which of the following trends is observed across a period in the p-block elements (left to right)?
A) Atomic radius increases
B) Ionization enthalpy decreases
C) Metallic character decreases
D) Electronegativity decreases
42. The maximum oxidation state of an element in Group 16 generally corresponds to:
A) Its group number
B) Its group number minus 10
C) Its group number minus 2
D) Its group number minus 18
43. Which element in Group 15 is known for its allotropy?
A) Nitrogen
B) Phosphorus
C) Arsenic
D) Bismuth
44. What is the reason for the decreasing ionization enthalpy down Group 13?
A) Increase in nuclear charge only
B) Increase in atomic size and shielding effect
C) Decrease in electron-electron repulsion
D) Increase in effective nuclear charge
45. Which of the following is NOT a characteristic of Boron, the first element of Group 13?
A) It is a metalloid.
B) It forms covalent compounds.
C) It exhibits +3 oxidation state predominantly.
D) Its atomic radius is larger than Aluminum.
46. The inert pair effect is most prominent in which group of p-block elements?
A) Group 13
B) Group 14
C) Group 15
D) Group 16
47. Which element is the lightest p-block metal?
A) Aluminum
B) Gallium
C) Boron
D) Indium
48. What is the common oxidation state for most Group 14 elements?
A) +2 and +4
B) +1 and +3
C) +3 and +5
D) +4 and +6
49. Which of the following is a characteristic trend in Group 13 elements moving down the group?
A) Atomic radius decreases
B) Ionization enthalpy increases
C) Metallic character increases
D) Electronegativity increases
50. What is the general electronic configuration of Group 18 elements (Noble Gases)?
A) ns²np⁶
B) ns²np⁵
C) ns²np¹
D) ns²np²
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