JEE Main - Kossel-Lewis approach ionic and covalent bonding concepts One Line Questions & Answers

1. Consider the formation of MgCl2. Magnesium (Mg) loses 2 electrons to form Mg2+. Chlorine (Cl) gains 1 electron to form Cl-. How many Cl atoms are needed to react with one Mg atom? — 2

2. How many valence electrons does an atom of Oxygen typically have? — 6

3. In a covalent bond, each atom contributes electrons to form: — A shared pair of electrons

4. The Lewis structure for the cyanide ion (CN-) has: — A triple bond and 2 lone pair electrons

5. According to the Kossel-Lewis approach, what do atoms tend to achieve during chemical bonding? — A stable electron configuration like that of noble gases

6. The Lewis structure of N2 shows a triple bond. This implies: — A strong attraction between the nitrogen atoms

7. Which of the following species can act as a Lewis base (electron pair donor)? — NH3

8. What is the 'octet rule' in the context of the Kossel-Lewis approach? — Atoms tend to gain, lose, or share electrons to achieve eight valence electrons

9. The compound BCl3 exhibits which of the following bonding characteristics? — Boron has an incomplete octet.

10. In the formation of a coordinate covalent bond (or dative bond), one atom provides: — Both electrons for the shared pair

11. Which element's Lewis symbol consists of a single letter 'C' surrounded by four dots? — Carbon

12. Which element is an exception to the octet rule and typically forms compounds with less than eight valence electrons? — Boron

13. Which of the following molecules exhibits a polar covalent bond? — HCl

14. The formation of a covalent bond involves: — Sharing of electrons between atoms

15. When sodium (Na) reacts with chlorine (Cl), what type of bond is primarily formed? — Ionic bond

16. What is the electrostatic force of attraction between oppositely charged ions called? — Ionic bond

17. When an atom of a highly electropositive element reacts with an atom of a highly electronegative element, what type of bond is predominantly formed? — Ionic bond

18. The concept of 'formal charge' in Lewis structures is used to: — Assign charges to atoms in a molecule or polyatomic ion to minimize overall charge.

19. Which of the following is an example of a compound with extensive ionic bonding? — Potassium Iodide (KI)

20. What are valence electrons according to the Kossel-Lewis concept? — Electrons involved in chemical bonding

21. Which of the following elements readily forms ionic bonds by losing one electron to achieve a stable octet? — Sodium

22. Who proposed the Kossel-Lewis approach for explaining chemical bonding? — Gilbert N. Lewis and Walther Kossel

23. Which of the following molecules contains a double covalent bond? — O2

24. Which of the following molecules contains only nonpolar covalent bonds? — N2

25. Which of the following is an example of a Lewis acid that does not have an octet of electrons around the central atom and is often involved in covalent bond formation? — AlCl3

26. Which of the following is NOT a characteristic of ionic compounds? — Electrical conductivity in solid state

27. The ammonium ion (NH4+) is formed when ammonia (NH3) reacts with a proton (H+). The bond formed between NH3 and H+ is a: — Coordinate covalent bond

28. What is the Lewis structure of a water molecule (H2O) primarily based on? — Covalent bonding

29. What is the primary limitation of the Kossel-Lewis approach? — It does not explain the shapes of molecules.

30. In the formation of NaCl, Sodium (Na) loses an electron to become Na+. What does Chlorine (Cl) do? — Gains an electron to become Cl-

31. Which of the following is NOT a characteristic of covalent compounds? — Formation of ionic lattices

32. The Kossel-Lewis approach primarily explains the formation of which types of chemical bonds? — Ionic and Covalent bonds

33. Covalent bonds are typically formed between: — Nonmetals and nonmetals

34. Which of the following compounds would be expected to have the highest melting point due to strong ionic bonding? — Sodium Chloride (NaCl)

35. Which of the following ions would have a Lewis structure with a single negative charge and eight valence electrons around the central atom? — Cl-

36. Which of the following species can act as a Lewis acid (electron pair acceptor)? — BF3

37. What is the term used to describe a covalent bond where electrons are shared unequally? — Polar covalent bond

38. How many covalent bonds are formed between a carbon atom and four hydrogen atoms in methane (CH4)? — Four

39. The Lewis symbol for Sodium (Na) would typically show: — One dot

40. In a triple covalent bond, how many pairs of electrons are shared between two atoms? — Three pairs

41. The formation of an ionic bond involves: — Transfer of electrons

42. What is the central idea of the Kossel-Lewis approach to chemical bonding? — Interaction of atomic orbitals

43. Which of the following is an example of a compound with extensive covalent bonding? — Carbon Tetrachloride (CCl4)

44. In the Kossel-Lewis model, the formation of a bond between two atoms is driven by: — The achievement of a stable electron configuration

45. The Kossel-Lewis approach helps to explain the formation of compounds by considering: — The transfer or sharing of valence electrons

46. The Lewis structure of ozone (O3) involves resonance. Which statement best describes this? — The actual structure is an average of two contributing Lewis structures, with bond lengths intermediate between single and double bonds.

47. What is a Lewis dot symbol used to represent? — The valence electrons of an atom

48. Which of the following is a limitation of representing bonding using only Lewis structures? — They do not predict molecular geometry or bond energies accurately.

49. Ionic bonds are typically formed between: — A metal and a nonmetal

50. The Lewis structure of CO2 shows: — Two double bonds between C and O

Kossel-Lewis approach ionic and covalent bonding concepts - One Line Questions