Questions on Water: Structure and the Physical Properties
Structure of Water and Ice, Physical Properties of Water – Multiple Choice Questions
1. What is the molecular shape of a water molecule?
A) Linear
B) Tetrahedral
C) Trigonal planar
D) Bent (angular)
E) Pyramidal
2. What type of bond connects the hydrogen and oxygen atoms within a water molecule?
A) Ionic bond
B) Metallic bond
C) Nonpolar covalent bond
D) Polar covalent bond
E) Hydrogen bond
3. What type of intermolecular force is most responsible for water's high boiling point?
A) London dispersion forces
B) Dipole-dipole interactions
C) Ion-dipole forces
D) Covalent bonds
E) Hydrogen bonding
4. Which statement best describes the arrangement of water molecules in ice?
A) Molecules are tightly packed and disordered
B) Molecules are in random motion
C) Molecules form a rigid hexagonal lattice
D) Molecules slide past each other freely
E) Molecules break apart into ions
5. Why is ice less dense than liquid water?
A) Hydrogen bonding in liquid is stronger
B) Water molecules are more spread out in ice
C) Ice contains dissolved gases
D) Water loses mass upon freezing
E) Ice has more kinetic energy
6. The angle between hydrogen atoms in a water molecule is approximately:
A) 90°
B) 104.5°
C) 120°
D) 180°
E) 60°
7. What is the main reason water is called the "universal solvent"?
A) It's a nonpolar molecule
B) It can dissolve lipids
C) It has strong London forces
D) It forms hydrogen bonds with many substances
E) It has high viscosity
8. Which of the following best explains water's high surface tension?
A) Ionic bonding
B) Polarizability
C) Hydrogen bonding among surface molecules
D) Weak dispersion forces
E) Cohesion between air molecules
9. What is the specific heat capacity of water?
A) 2.01 J/g·°C
B) 0.90 J/g·°C
C) 1.00 J/g·°C
D) 4.18 J/g·°C
E) 9.10 J/g·°C
10. Which of the following properties of water allows for temperature regulation in living organisms?
A) High compressibility
B) High reactivity
C) Low heat of vaporization
D) High specific heat capacity
E) High electrical conductivity
11. Why does water have a relatively high boiling point for a small molecule?
A) Strong ionic bonds
B) Large molar mass
C) Presence of hydrogen bonding
D) Weak dipole interactions
E) High density
12. Which of these properties is greater in water than in most other common liquids?
A) Compressibility
B) Viscosity
C) Boiling point
D) Density
E) Transparency
13. What happens to the volume of water when it freezes?
A) It decreases
B) It stays the same
C) It increases
D) It first decreases, then increases
E) It becomes zero
14. Which temperature represents the maximum density of water?
A) 0°C
B) 4°C
C) 25°C
D) 50°C
E) 100°C
15. The structure of ice results in:
A) Low surface tension
B) High density
C) Expansion upon freezing
D) Increased molecular mass
E) Decrease in boiling point
16. Why is ice effective in insulating lakes in the winter?
A) It absorbs sunlight
B) It is a poor conductor of heat
C) It is highly dense
D) It allows convection
E) It releases oxygen
17. Which characteristic makes water essential for metabolic reactions?
A) It’s nonpolar
B) It’s unreactive
C) It dissolves ionic and polar substances
D) It’s transparent
E) It has low boiling point
18. In the solid phase (ice), each water molecule is hydrogen bonded to:
A) 2 other water molecules
B) 3 other water molecules
C) 4 other water molecules
D) 5 other water molecules
E) 6 other water molecules
19. What phase change occurs at 0°C under normal pressure?
A) Condensation
B) Freezing or melting
C) Vaporization
D) Sublimation
E) Evaporation
20. What is the dominant force responsible for cohesion in liquid water?
A) Ion-dipole interactions
B) Dipole-dipole forces
C) Covalent bonding
D) Hydrogen bonding
E) Dispersion forces
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Answers with Full Explanations
1. D – Water has a bent or angular molecular shape due to its two lone electron pairs.
2. D – The O–H bonds in water are polar covalent, creating partial charges.
3. E – Hydrogen bonds between water molecules are responsible for its high boiling point.
4. C – In ice, water molecules form a hexagonal crystalline lattice.
5. B – Ice is less dense because water molecules in ice are more spread out due to hydrogen bonding.
6. B – The bond angle in a water molecule is approximately 104.5°.
7. D – Water dissolves many substances due to its ability to form hydrogen bonds.
8. C – Hydrogen bonding among surface molecules creates high surface tension.
9. D – Water has a specific heat capacity of 4.18 J/g·°C, very high for a liquid.
10. D – Water’s high specific heat allows it to absorb and release heat slowly, regulating temperature.
11. C – Hydrogen bonds require extra energy to break, causing a high boiling point.
12. C – Water has a higher boiling point than most small molecular compounds due to hydrogen bonding.
13. C – Water expands upon freezing.
14. B – Water reaches its maximum density at 4°C.
15. C – The open structure of ice causes expansion and lower density.
16. B – Ice is a poor conductor of heat, providing insulation for aquatic life.
17. C – Water is a polar solvent, essential for dissolving ionic and polar molecules in metabolism.
18. C – In ice, each molecule is hydrogen-bonded to 4 others.
19. B – At 0°C, water undergoes melting or freezing, depending on direction of heat flow.
20. D – Hydrogen bonding is the main cohesive force in liquid water.
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