JEE Main - Group-wise behaviour and unique features of first elements in groups Online Test (MCQ Quiz)

1. Which of the following is a characteristic property of the first element in Group 1 (alkali metals)?

A) High melting point B) Formation of ionic hydrides C) Large atomic radius D) Low ionization enthalpy

2. The first element of Group 14, Carbon, exhibits unique properties compared to other elements in the group. Which of these is NOT a unique property of Carbon?

A) Ability to form multiple bonds with itself (catenation) B) Formation of stable oxides like CO and CO2 C) Existence in allotropic forms like diamond and graphite D) Formation of ionic compounds with electronegative elements

3. Why does Lithium (Li), the first element of Group 1, show diagonal relationship with Magnesium (Mg) of Group 2?

A) Similar electronegativity and polarizing power B) Similar atomic and ionic radii C) Similar ionization energies D) Similar chemical reactivity

4. Fluorine (F), the first element of Group 17 (halogens), is the most electronegative element. What is a direct consequence of this high electronegativity?

A) It readily forms positive ions B) It forms covalent bonds with most non-metals C) It acts as a reducing agent D) It has a low boiling point

5. Which of the following is a unique characteristic of Boron (B), the first element of Group 13?

A) Forms stable +3 oxidation state B) Forms a large number of alloys C) Forms hydrides that are electron-deficient D) Has a high melting point

6. The first element of Group 16, Oxygen (O), exhibits anomalous behavior. Which of these is an example of its unique property?

A) Forms a stable -2 oxidation state B) Has a higher ionization enthalpy than Nitrogen C) Forms O2 molecule with a double bond D) Forms allotropes like O2 and O3

7. Why does Lithium (Li) form Li3N (lithium nitride) while other alkali metals form nitrides with different stoichiometry (e.g., Na3N is unstable)?

A) Lithium has a higher ionization enthalpy B) Lithium has a smaller ionic radius and higher polarizing power C) Lithium has a lower electronegativity D) Lithium is less reactive

8. Nitrogen (N), the first element of Group 15, shows remarkable differences from other elements in the group. Which of these is a direct consequence of the small size and high electronegativity of Nitrogen?

A) It forms stable pentavalent compounds B) It readily forms N³⁻ ion C) It forms multiple bonds with itself (N≡N) D) It has a high boiling point

9. Which property of Fluorine (F) is responsible for its inability to form F₂⁻ ion and its strong oxidizing nature?

A) Very low electron gain enthalpy B) Very high electronegativity and weak F-F bond C) Large atomic radius D) High ionization enthalpy

10. The diagonal relationship between Beryllium (Be) and Aluminum (Al) is attributed to:

A) Similar electronegativity and polarizing power B) Similar atomic and ionic radii C) Similar ionization energies D) Similar chemical reactivity

11. Why does Carbon (C) predominantly form covalent compounds, whereas other Group 14 elements like Silicon (Si) and Germanium (Ge) also form ionic compounds?

A) Carbon has a higher ionization enthalpy B) Carbon has a very small size and high electronegativity, making it difficult to form C⁴⁺ or C⁴⁻ ions C) Carbon has a lower tendency for catenation D) Carbon has a higher atomic radius

12. Which of the following is a unique characteristic of Hydrogen (H) as the first element of Group 1?

A) It is a metal B) It forms ionic compounds with halogens C) It can exhibit +1 and -1 oxidation states D) It has a high boiling point

13. The first element of Group 2, Beryllium (Be), shows deviation from the general trend. Which property is unique to Beryllium compared to other alkaline earth metals?

A) Forms Be²⁺ ion readily B) Has a high melting point C) Forms stable covalent compounds and shows diagonal relationship with Aluminum D) Has a low ionization enthalpy

14. Why does Fluorine (F) exist as a diatomic molecule (F₂) with a single bond, while Oxygen (O) exists as O₂ with a double bond and Nitrogen (N) as N₂ with a triple bond?

A) Fluorine has a larger atomic radius B) The F-F single bond is exceptionally weak C) Fluorine has a lower electronegativity D) Fluorine readily forms ionic bonds

15. Which unique property of Boron (B) allows it to form complex borohydrides with unusual bonding?

A) High ionization enthalpy B) Formation of electron-deficient compounds C) Tendency to form ionic bonds D) Large atomic radius

16. The first element of Group 15, Nitrogen (N), differs significantly from Phosphorus (P) and other elements in the group primarily due to:

A) Its larger atomic size B) Its inability to form pπ-pπ multiple bonds C) Its higher ionization enthalpy D) Its lower electronegativity

17. Which characteristic of Lithium (Li) is responsible for its low solubility in organic solvents compared to other alkali metal salts?

A) High ionic character of its salts B) Strong hydration of Li⁺ ion due to its small size C) Low polarizing power of Li⁺ ion D) High tendency to form metallic bonds

18. Why is Silicon (Si) tetrafluoride (SiF₄) a gas, while Carbon tetrachloride (CCl₄) is a liquid at room temperature, despite both being Group 14 elements?

A) SiF₄ has stronger intermolecular forces B) SiF₄ is a covalent molecule with weak intermolecular forces, while CCl₄ has stronger dipole-dipole interactions due to bond polarity differences C) SiF₄ has a lower molecular weight D) SiF₄ forms ionic bonds, while CCl₄ forms covalent bonds

19. The anomalous behavior of Fluorine (F) is NOT attributed to:

A) Small size B) High electronegativity C) Presence of d-orbitals in the valence shell D) Weak F-F bond

20. Which property of Oxygen (O) is responsible for its ability to form O₃ (ozone), a property not exhibited by other elements in Group 16?

A) High ionization enthalpy B) Small size and ability to form pπ-pπ multiple bonds C) Low electronegativity D) Tendency to form ionic bonds

21. Why does Beryllium (Be) form a stable oxide BeO, which is amphoteric, while other alkaline earth metal oxides are basic?

A) Beryllium has a higher ionization enthalpy B) Beryllium has a small ionic radius and high charge density, leading to significant covalent character in BeO C) Beryllium readily forms Be²⁺ ions D) Beryllium has a high melting point

22. The diagonal relationship between Lithium (Li) and Magnesium (Mg) is primarily due to:

A) Similar electronegativity and polarizing power B) Similar atomic radius C) Similar ionization enthalpies D) Similar chemical reactivity

23. Which unique characteristic of Carbon (C) allows it to form an enormous number of organic compounds?

A) High melting point B) Ability to form multiple bonds with itself (catenation) C) Formation of ionic carbides D) Low ionization enthalpy

24. Why does Hydrogen (H) resemble halogens in some aspects?

A) It has a high ionization enthalpy B) It can gain an electron to form H⁻ ion C) It is a non-metal D) It has a high boiling point

25. The first element of Group 13, Boron (B), exhibits anomalous behavior. Which of these is NOT a consequence of its small size and high electronegativity?

A) It forms BH₃ which is unstable and dimerizes to B₂H₆ B) It forms compounds with significant covalent character C) It exhibits +3 oxidation state readily D) It forms a very stable oxide B₂O₃

26. Which property of Nitrogen (N) is responsible for the inertness of N₂ gas at room temperature?

A) Low ionization enthalpy B) High electronegativity C) Presence of a strong triple bond D) Small atomic radius

27. The diagonal relationship between Beryllium (Be) and Aluminum (Al) is observed because they have similar:

A) Number of valence electrons B) Charge density (charge/radius ratio) C) Ionization enthalpies D) Electronegativity values only

28. Why does Fluorine (F) not form oxyacids like other halogens (e.g., HClO, HBrO)?

A) Fluorine has a very high electronegativity B) Fluorine is too small to accommodate oxygen atoms C) Fluorine cannot expand its octet D) Fluorine readily forms ionic bonds

29. Which of the following is a unique characteristic of Lithium (Li) among alkali metals?

A) Forms a stable nitride B) Reacts vigorously with water C) Has a low melting point D) Forms soluble salts

30. Carbon's ability to form stable multiple bonds with itself (catenation) is significantly greater than that of Silicon (Si). This is primarily due to:

A) Higher ionization enthalpy of Carbon B) Stronger C-C single bond compared to Si-Si single bond C) Smaller size and better orbital overlap in Carbon D) Higher electronegativity of Carbon

31. Why does Oxygen (O) form O₂ with a double bond, whereas Sulfur (S) forms S₈ rings?

A) Oxygen has a higher ionization enthalpy B) Oxygen's small size allows effective pπ-pπ overlap for double bond formation, which is less effective for Sulfur C) Oxygen has a lower electronegativity D) Oxygen readily forms ionic bonds

32. The first element of Group 1, Lithium (Li), is unique due to its:

A) High reactivity B) Low melting point C) Diagonal relationship with Magnesium D) Formation of strongly ionic compounds

33. Which property of Beryllium (Be) makes it form covalent compounds and exhibit a diagonal relationship with Aluminum (Al)?

A) High ionization enthalpy B) Low electronegativity C) Small ionic radius and high charge density D) Tendency to form Be²⁺ ions

34. The anomalous behavior of Boron (B) compared to other Group 13 elements is mainly due to:

A) Its large atomic radius B) Its inability to form multiple bonds C) Its high electronegativity and small size D) Its low ionization enthalpy

35. Why does Nitrogen (N) form N₂ with a triple bond, while Phosphorus (P) exists as P₄ tetrahedra?

A) Nitrogen has a smaller atomic radius and can form stable pπ-pπ multiple bonds B) Nitrogen has a lower ionization enthalpy C) Nitrogen has a higher electronegativity D) Nitrogen readily forms ionic bonds

36. Which factor contributes most to the unique chemistry of Fluorine (F) as the first element of Group 17?

A) Low electronegativity B) Large atomic radius C) Weak F-F bond and high electronegativity D) High electron gain enthalpy

37. The diagonal relationship between Boron (B) and Silicon (Si) is observed due to:

A) Similar electronegativity and polarizing power B) Similar atomic and ionic radii C) Similar ionization energies D) Similar chemical reactivity

38. Why does Oxygen (O) form O²⁻ ion readily, but other Group 16 elements like Sulfur (S) can form S²⁻, S₂²⁻, etc.?

A) Oxygen has a lower ionization enthalpy B) Oxygen's small size leads to high lattice energy for its oxide, stabilizing O²⁻ C) Oxygen has a higher electronegativity D) Oxygen cannot expand its octet

39. Which property of Hydrogen (H) allows it to form compounds like NaH, which are called hydrides?

A) Its high ionization enthalpy B) Its ability to accept an electron to form H⁻ ion C) Its metallic character D) Its low boiling point

40. The first element of Group 2, Beryllium (Be), shows covalent bonding tendencies. This is primarily due to:

A) Its low ionization enthalpy B) Its high electronegativity C) Its small size and high charge density D) Its tendency to form ionic compounds

41. Why does Lithium (Li) form Li₂CO₃ which decomposes at high temperature, while other alkali metal carbonates are very stable?

A) Li⁺ ion has a higher polarizing power B) Li⁺ ion has a smaller ionic radius C) Li⁺ ion has a higher charge density D) All of the above

42. Which unique feature of Carbon (C) distinguishes it from other Group 14 elements regarding its bonding?

A) Forms ionic carbides B) Forms multiple bonds with itself extensively C) Has a higher atomic radius D) Has a lower ionization enthalpy

43. The anomalous behavior of Nitrogen (N) is NOT due to:

A) Small atomic size B) High electronegativity C) Presence of d-orbitals in the valence shell D) Ability to form pπ-pπ multiple bonds

44. Why is Fluorine (F) the strongest oxidizing agent?

A) High electron affinity B) Weak F-F bond, high electronegativity, and stable F⁻ ion C) Low ionization enthalpy D) Large atomic radius

45. Which property of Boron (B) leads to its diagonal relationship with Silicon (Si)?

A) Similar atomic radii B) Similar electronegativity and polarizing power C) Similar ionization enthalpies D) Similar chemical reactivity

46. Why does Oxygen (O) form O₂ with a double bond, while Sulfur (S) forms S₈ rings and exhibits allotropy like O₂ and O₃?

A) Oxygen has a higher ionization enthalpy B) Oxygen's small size allows effective pπ-pπ overlap for double bond formation, while Sulfur prefers sπ-pπ or single bonds and forms larger rings C) Oxygen has a lower electronegativity D) Oxygen readily forms ionic bonds

47. Hydrogen (H) can be considered an alkali metal due to:

A) Its tendency to lose one electron to form H⁺ B) Its high ionization enthalpy C) Its non-metallic character D) Its low boiling point

48. The anomalous behavior of Beryllium (Be) compared to other alkaline earth metals is primarily due to:

A) Its low ionization enthalpy B) Its high electronegativity and small size C) Its tendency to form ionic compounds D) Its large atomic radius

49. Which of the following is a unique characteristic of Lithium (Li) among alkali metals concerning its compounds?

A) Forms Li₂O₂ and LiO₂ B) Forms soluble carbonates C) Forms strongly ionic chlorides D) Has a high melting point

50. The ability of Carbon (C) to form stable C-C single bonds and C=C double bonds is significantly greater than that of Silicon (Si). This is primarily due to:

A) Higher ionization enthalpy of Carbon B) Stronger C-C single bond and better pπ-pπ overlap for double bonds C) Smaller size and better orbital overlap in Carbon D) Higher electronegativity of Carbon

Group-wise behaviour and unique features of first elements in groups - Online Test

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