CHM101 Quiz - Xirius

1. Which type of bonding involves the sharing of electron pairs between atoms?

A. Ionic bonding B. Metallic bonding C. Covalent bonding D. Van der Waal’s forces

2. Which bonding type results from electrostatic attraction between positive and negative ions?

A. Covalent B. Ionic C. Metallic D. Hydrogen

3. At the same temperature, heavier particles compared to lighter particles:

A. Move faster B. Move slower C. Move at the same speed D. Have zero velocity

4. Which of the following elements is NOT commonly involved in hydrogen bonding?

A. Oxygen B. Fluorine C. Nitrogen D. Sodium

5. Dipole-dipole interactions occur between:

A. Two non-polar molecules B. Two polar molecules C. A polar and a non-polar molecule D. Charged ions only

6. Which intermolecular force is stronger than van der Waal’s forces but weaker than covalent bonding?

A. Ionic bonds B. Metallic bonds C. Hydrogen bonding D. Dipole-induced dipole

7. Which force is responsible for the condensation of water vapour?

A. Covalent bonds B. Ionic bonds C. Intermolecular hydrogen bonding D. Metallic bonding

8. Instantaneous dipoles are caused by:

A. Permanent polarity in molecules B. Fluctuations in electron cloud density C. Ionic charges D. External electric fields only

9. Which type of bonding involves the electrostatic attraction between a delocalized electron cloud and metal ions?

A. Covalent bonding B. Metallic bonding C. Ionic bonding D. Hydrogen bonding

10. Ionic compounds conduct electricity only when:

A. Solid B. Molten or dissolved in water C. Frozen D. Evaporated

11. Which property is characteristic of gases but not solids or liquids?

A. Fixed volume and shape B. High density C. Particles closely packed in a fixed pattern D. Particles are far apart and can be compressed

12. Which statement correctly describes van der Waal’s forces?

A. They include only ionic bonds B. They include dipole-dipole, dipole-induced dipole, and London dispersion forces C. They are stronger than covalent bonds D. They exist only in metals

13. Which phase change involves the transition from gas to liquid?

A. Melting B. Evaporation C. Condensation D. Sublimation

14. What determines the state of matter according to the kinetic theory?

A. Pressure alone B. The motion and arrangement of particles C. The number of electrons only D. Whether the substance contains metals

15. According to the kinetic theory of matter, temperature measures the:

A. Speed of light B. Average kinetic energy of particles C. Mass of particles D. Potential energy of particles

16. Why do substances with stronger intermolecular forces have higher boiling points?

A. Because particles move faster with stronger forces B. Because more energy is required to break the intermolecular forces C. Because they have more electrons D. Because they have larger molecular size

17. During melting, particles:

A. Lose energy and stop moving B. Gain energy and move more freely C. Have no change in energy D. Form ionic bonds

18. What primarily determines the phase of matter according to the kinetic theory of matter?

A. The color of the substance B. The motion and arrangement of particles influenced by temperature C. The chemical composition only D. The pressure applied to the substance

19. During a phase change, such as melting, the temperature:

A. Increases continuously B. Decreases continuously C. Remains constant until the phase change is complete D. Changes randomly

20. Covalent compounds generally have:

A. High melting and boiling points B. Poor electrical conductivity C. High density compared to solids D. Made from metal and non-metal combinations

21. What distinguishes a coordinate covalent bond from a regular covalent bond?

A. It involves transfer of electrons from one atom to another B. The shared pair of electrons is donated by only one of the bonded atoms C. It only exists in metals D. It involves only ionic interactions

22. In solids, particles:

A. Move freely and randomly B. Vibrate in fixed positions without changing location C. Slide past each other easily D. Have indefinite shape and volume

23. What is the primary difference between intermolecular and intramolecular hydrogen bonding?

A. Intermolecular occurs within the same molecule; intramolecular occurs between molecules B. Intermolecular occurs between molecules; intramolecular occurs within the same molecule C. Both occur only between ions D. Both occur between metals

24. In dipole-induced dipole interactions, what causes the induced dipole?

A. Electron transfer B. Permanent dipole on polar molecule C. Hydrogen bonding D. Covalent bond formation

25. What happens to particles in a solid when temperature increases but remains below melting point?

A. They move freely B. They vibrate more vigorously in fixed positions C. They break bonds and liquefy D. They gain infinite kinetic energy

26. What happens to kinetic energy (K.E.) of particles during phase changes?

A. K.E. increases steadily B. K.E. decreases steadily C. K.E. remains constant during phase change D. K.E. becomes zero during phase change

27. Hydrogen bonding requires that hydrogen be directly bonded to which atoms?

A. Carbon, hydrogen, or oxygen B. Hydrogen and any other atom C. Highly electronegative atoms like F, O, N, or Cl D. Metals only

28. Which of these phase changes skips the liquid state entirely?

A. Freezing B. Sublimation C. Condensation D. Melting

29. Which of the following interactions is included in Van der Waal’s forces?

A. Ionic bonding B. Covalent bonding C. Dipole-induced dipole interactions D. Metallic bonding

30. Which property is NOT typical of ionic compounds?

A. High melting point B. Conduct electricity in molten state C. Soft and flexible nature D. Made of metal and non-metal elements

31. The ability of a gas to be compressed is mainly due to:

A. Large spaces between particles B. High particle density C. Fixed volume D. Strong intermolecular forces

32. What is the name of the force of attraction between two temporary dipoles?

A. Hydrogen bonding B. Ionic bonding C. London dispersion forces D. Metallic bonding

33. Hydrogen bonding occurs only when hydrogen is directly bonded to which type of atom?

A. Alkali metals B. Highly electronegative atoms such as F, O, N, or Cl C. Any metal atoms D. Noble gases

34. During evaporation, particles leaving the liquid have:

A. Less kinetic energy than average B. Same kinetic energy as average C. More kinetic energy than average D. No kinetic energy

35. What causes evaporation to occur even below the boiling point temperature?

A. All particles gain kinetic energy equally B. Some particles gain enough kinetic energy to overcome intermolecular forces C. The temperature dramatically increases locally D. The liquid freezes

36. Which factor increases the strength of metallic bonding?

A. Larger size of metal ion B. More valence electrons C. Decrease in number of valence electrons D. Increase in gas pressure

37. The difference in electronegativity between atoms in a molecule causes:

A. Ionic bonding B. Permanent dipoles C. Instantaneous dipoles D. No polarity

38. Evaporation differs from boiling because:

A. Evaporation happens at boiling point B. Evaporation happens on the surface at any temperature C. Boiling happens on the surface only D. Both occur only at standard atmospheric pressure

39. The stronger the intermolecular forces (IF’s), the:

A. Lower the boiling point B. Higher the boiling point C. No effect on boiling point D. Lower the melting point

40. Coordinate covalent bonding is characterized by:

A. Both atoms share electrons equally B. Electrons are transferred from one atom to another C. The shared electron pair is donated by only one atom D. Atoms bonded by hydrogen bonding

41. Gases have which of the following characteristics?

A. Fixed volume and shape B. High density and incompressible C. Indefinite shape and volume and low density D. Arranged in fixed regular patterns

42. For hydrogen bonding to occur, an unshared pair of electrons must be present on:

A. Hydrogen atom B. Any atom C. Highly electronegative atom bonded to hydrogen D. Metal atoms

43. Metallic bonding is mainly the electrostatic attraction between:

A. Metal ions and shared electrons B. Metal ions and delocalized electron cloud C. Non-metal ions and electrons D. Positive ions and negative ions

44. Which statement about liquids is TRUE?

A. They have fixed shape but no fixed volume B. Their particles are packed very loosely C. They have fixed volume but take the shape of the container D. They cannot flow freely

45. The physical state with fixed volume but indefinite shape is:

A. Solid B. Liquid C. Gas D. Plasma

46. What type of bonding is found in metals that explains their high melting points and conductivity?