NEET UG - Kossel Lewis approach, ionic and covalent bonds, factors affecting ionic bond formation, lattice enthalpy Question Bank with Options

1. Which of the following elements would require the least energy to form a stable cation?

A) Neon

B) Argon

C) Krypton

D) Xenon

2. The Kossel-Lewis approach is also known as the:

A) Valence Bond Theory

B) Molecular Orbital Theory

C) Octet Rule approach

D) Crystal Field Theory

3. Which of the following compounds exhibits significant covalent character in its bonds?

A) CsF

B) MgO

C) AlCl3

D) NaCl

4. In the formation of an ionic bond, energy is required for ionization and dissociation, but energy is released during:

A) Electron affinity

B) Lattice formation

C) Atomization

D) Sublimation

5. The driving force behind the formation of ionic bonds is the tendency of atoms to achieve:

A) A full d-subshell

B) An unpaired electron

C) A stable electron configuration like a noble gas

D) Maximum kinetic energy

6. Which of the following factors would contribute to a higher lattice enthalpy?

A) Larger ionic radii

B) Smaller ionic radii

C) Lower ionic charges

D) Greater distance between ions

7. The Lewis dot structure for the oxygen molecule (O2) shows:

A) A single bond and two lone pairs on each oxygen atom

B) A double bond and two lone pairs on each oxygen atom

C) A triple bond and one lone pair on each oxygen atom

D) A double bond and one lone pair on each oxygen atom

8. A covalent bond is generally formed between atoms with:

A) A large difference in electronegativity

B) A small difference in electronegativity

C) Very low ionization energies

D) Very high electron affinities

9. The term 'octet rule' is most directly related to:

A) The number of neutrons in an atom's nucleus

B) The number of protons in an atom's nucleus

C) The number of electrons in an atom's valence shell

D) The total number of electrons in an atom

10. Which of the following ionic compounds would have a lattice enthalpy that is less negative (weaker) than NaCl?

A) LiF

B) MgO

C) CaCl2

D) KBr

11. Lattice enthalpy is defined for the process of forming:

A) One mole of gaseous ions from their constituent elements in their standard states

B) One mole of a solid ionic compound from its constituent gaseous ions

C) One mole of a solid ionic compound from its constituent elements in their standard states

D) One mole of gaseous ions from one mole of a solid ionic compound

12. Which factor favors the formation of an ionic bond?

A) High ionization energy of the metal and high electron affinity of the non-metal

B) Low ionization energy of the metal and high electron affinity of the non-metal

C) Low ionization energy of the metal and low electron affinity of the non-metal

D) High ionization energy of the metal and low electron affinity of the non-metal

13. The Lewis structure for ammonia (NH3) shows:

A) Three single covalent bonds and one lone pair on nitrogen

B) One single and one double covalent bond on nitrogen

C) Three double covalent bonds on nitrogen

D) Three single covalent bonds and no lone pairs on nitrogen

14. Which of the following is a characteristic of covalent compounds?

A) They are typically good conductors of electricity in solid state.

B) They usually have high melting and boiling points.

C) They exist as discrete molecules held together by weak intermolecular forces.

D) They are formed between metals and non-metals.

15. When an atom gains electrons to form an anion, its size generally:

A) Increases

B) Decreases

C) Remains the same

D) Becomes undefined

16. When an atom loses electrons to form a cation, its size generally:

A) Increases

B) Decreases

C) Remains the same

D) Becomes undefined

17. Which of the following factors LEAST affects the lattice enthalpy of an ionic compound?

A) The charges of the ions

B) The size of the ions

C) The number of electrons in the ions

D) The distance between the ions

18. The Kossel-Lewis approach emphasizes the role of electrons in achieving:

A) Nuclear stability

B) Chemical inertness

C) A stable noble gas electron configuration

D) Paramagnetism

19. Which of the following represents a polar covalent bond?

A) H-H bond in H2

B) O=O bond in O2

C) H-Cl bond in HCl

D) C-C bond in ethane

20. In the ionic compound formed between a Group 1 metal and a Group 17 halogen, what is the typical charge on the cation and anion, respectively?

A) +1 and -1

B) +1 and -2

C) +2 and -1

D) +1 and +1

21. The Born-Haber cycle is used to calculate:

A) Ionization energy

B) Electron affinity

C) Lattice enthalpy

D) Enthalpy of formation

22. Which of the following elements has the most negative electron affinity?

A) Oxygen

B) Sulfur

C) Selenium

D) Tellurium

23. Which of the following elements has the highest ionization energy?

A) Lithium

B) Sodium

C) Potassium

D) Cesium

24. What is the primary reason for the difference in melting points between NaCl and CH4?

A) NaCl has stronger covalent bonds than CH4.

B) CH4 has a higher lattice enthalpy than NaCl.

C) NaCl is an ionic compound with strong electrostatic forces, while CH4 is a covalent molecule with weak intermolecular forces.

D) CH4 has a more stable electron configuration than NaCl.

25. Which of the following is the most stable Lewis structure for the carbonate ion (CO3^2-)?

A) One C=O double bond and two C-O single bonds, with appropriate formal charges

B) Three C-O single bonds, with appropriate formal charges

C) One C-O single bond and two C=O double bonds, with appropriate formal charges

D) Two C=O double bonds and one C-O single bond, with appropriate formal charges

26. The formation of an anion involves:

A) Gain of electrons

B) Loss of electrons

C) Sharing of electrons

D) Donation of electrons

27. The formation of a cation involves:

A) Gain of electrons

B) Loss of electrons

C) Sharing of electrons

D) Dipping of electrons

28. Which factor, when increased, generally leads to a more exothermic (more negative) lattice enthalpy?

A) Interionic distance

B) Ionic radius

C) Magnitude of ionic charges

D) Number of ions in the compound

29. A large negative lattice enthalpy indicates:

A) Weak attractive forces between ions

B) Strong attractive forces between ions

C) High solubility in water

D) Low melting point

30. Which of the following is an example of a molecule with a covalent bond?

A) KCl

B) CaO

C) CH4

D) Na2O

31. The Lewis structure of water (H2O) shows:

A) Two single covalent bonds and two lone pairs on oxygen

B) One double covalent bond and one lone pair on oxygen

C) Two single covalent bonds and no lone pairs on oxygen

D) One single and one double covalent bond

32. Which type of bond is formed between two non-metal atoms with similar electronegativities?

A) Ionic bond

B) Covalent bond

C) Metallic bond

D) Hydrogen bond

33. In the formation of MgO, what is the charge on the magnesium ion?

A) +1

B) +2

C) +3

D) -2

34. In the formation of NaCl, which ion is formed by losing an electron?

A) Cl-

B) Na+

C) Both Na+ and Cl-

D) Neither Na+ nor Cl-

35. The octet rule, as proposed by Kossel and Lewis, states that atoms tend to gain, lose, or share electrons to achieve:

A) A stable electron configuration with two electrons in the outermost shell

B) A stable electron configuration with eight electrons in the outermost shell

C) A half-filled outermost electron shell

D) A completely empty outermost electron shell

36. Which of the following ionic compounds has the highest lattice enthalpy?

A) NaCl

B) MgO

C) AlN

D) LiF

37. Lattice enthalpy is generally a/an ________ process.

A) Endothermic

B) Exothermic

C) Isothermal

D) Adiabatic

38. Which of the following is NOT a factor affecting ionic bond formation?

A) Ionization energy of the metal

B) Electron affinity of the non-metal

C) Lattice enthalpy of the ionic compound

D) Electronegativity of the metal

39. A covalent bond is formed by:

A) Complete transfer of electrons

B) Sharing of electrons

C) Electrostatic attraction between oppositely charged ions

D) Formation of a metallic lattice

40. The Lewis structure of an atom uses dots to represent:

A) Protons

B) Neutrons

C) Valence electrons

D) Core electrons

41. Which of the following pairs of elements is most likely to form an ionic compound?

A) Carbon and Oxygen

B) Hydrogen and Chlorine

C) Sodium and Fluorine

D) Nitrogen and Phosphorus

42. Ionic compounds typically have high melting and boiling points due to:

A) Weak intermolecular forces

B) Strong electrostatic forces between ions

C) Covalent character in their bonds

D) Low lattice enthalpy

43. Which factor primarily influences the strength of an ionic bond according to Coulomb's law?

A) Size of the ions

B) Number of electrons transferred

C) Distance between the ions and the magnitude of charges

D) Polarizability of the ions

44. What is the term used for the energy released when one mole of an ionic compound is formed from its gaseous ions?

A) Ionization energy

B) Electron affinity

C) Lattice enthalpy

D) Enthalpy of atomization

45. The Kossel-Lewis approach explains chemical bonding based on:

A) Electronegativity differences

B) Atomic orbital overlap

C) Achieving a stable electron configuration, typically resembling noble gases

D) Magnetic properties of atoms

46. Which of the following elements is most likely to form a covalent bond?

A) Potassium

B) Magnesium

C) Sulfur

D) Calcium

47. Which of the following elements is most likely to form an ionic bond?

A) Chlorine

B) Sodium

C) Carbon

D) Nitrogen

48. What is the primary characteristic of an ionic bond?

A) Sharing of electrons between atoms

B) Transfer of electrons between atoms

C) Formation of a sea of electrons

D) Delocalization of pi electrons

49. Who introduced the concept of electron sharing to explain chemical bonding?

A) Dmitri Mendeleev

B) G.N. Lewis

C) J.H. van 't Hoff

D) Svante Arrhenius

Kossel Lewis approach, ionic and covalent bonds, factors affecting ionic bond formation, lattice enthalpy - Question Bank