Quiz 7: States Of Matter And Intermolecular Forces
This quiz will test your knowledge of states of matter, changing states of matter, and intermolecular forces among molecules.
Questions and Answers
- 1.
A ___________ has a definite shape and a definite volume.
- A.
Solid
- B.
Liquid
- C.
Gas
- D.
Molecule
Correct Answer
A. SolidExplanation
A solid has a definite shape and a definite volume because its particles are closely packed together and have strong intermolecular forces. This arrangement restricts the movement of the particles, causing them to vibrate in fixed positions. As a result, solids maintain their shape and volume.Rate this question:
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- 2.
A __________ has no definite shape and no definite volume.
- A.
Solid
- B.
Liquid
- C.
Gas
- D.
Molecule
Correct Answer
C. GasExplanation
A gas is a state of matter that does not have a definite shape or volume. Unlike solids and liquids, which have distinct boundaries and occupy a fixed amount of space, gases can expand to fill any container they are placed in. The particles in a gas are loosely packed and move freely, allowing them to spread out and fill the available space. This lack of definite shape and volume is a defining characteristic of gases.Rate this question:
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- 3.
A ____________ has no definite shape, but a definite volume.
- A.
Solid
- B.
Liquid
- C.
Gas
- D.
Molecule
Correct Answer
B. LiquidExplanation
A liquid is a state of matter that has no definite shape, meaning it can take the shape of its container, but it does have a definite volume, meaning it maintains a specific amount of space. Unlike solids, which have both a definite shape and volume, and gases, which have neither a definite shape nor volume, liquids have the ability to flow and are characterized by their ability to pour and be poured. Therefore, a liquid fits the description of having no definite shape, but a definite volume.Rate this question:
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- 4.
The change in state from a solid to a liquid is called __________.
- A.
Freezing
- B.
Condensation
- C.
Evaporation
- D.
Melting
Correct Answer
D. MeltingExplanation
The change in state from a solid to a liquid is called melting. This occurs when heat is applied to a solid substance, causing the particles to gain energy and vibrate more rapidly, eventually breaking the bonds that hold them in a fixed position. As a result, the solid substance transitions into a liquid state, where the particles are able to move more freely while still maintaining their cohesive properties.Rate this question:
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- 5.
The change in state from gas to liquid is called ____________.
- A.
Condensation
- B.
Freezing
- C.
Melting
- D.
Evaporation
Correct Answer
A. CondensationExplanation
Condensation refers to the process of a gas changing into a liquid state. This occurs when the temperature of the gas decreases, causing the gas particles to lose energy and come closer together, forming a liquid. This change in state is commonly observed when water vapor in the air cools down and forms water droplets on a cold surface, such as dew forming on grass in the morning or water droplets forming on the outside of a cold glass.Rate this question:
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- 6.
_____________ is the change in state from liquid to solid.
- A.
Melting
- B.
Freezing
- C.
Evaporation
- D.
Condensation
Correct Answer
B. FreezingExplanation
Freezing is the process in which a substance changes its state from liquid to solid. During freezing, the particles in a liquid slow down and come closer together, forming a rigid structure. This results in the formation of a solid.Rate this question:
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- 7.
______________ is the change in state from liquid to gas.
- A.
Freezing
- B.
Melting
- C.
Condensation
- D.
Evaporation
Correct Answer
D. EvaporationExplanation
Evaporation is the process by which a substance changes from a liquid state to a gaseous state. This occurs when the molecules of the liquid gain enough energy to overcome the attractive forces holding them together, allowing them to escape into the surrounding environment as gas. This process is commonly observed when water or other liquids are heated, causing them to evaporate and form water vapor or gas. Therefore, evaporation is the correct answer for the given question.Rate this question:
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- 8.
What causes matter to change from one state to another?
- A.
Light
- B.
Heat
- C.
Sound
- D.
Gasoline
Correct Answer
B. HeatExplanation
Heat is the correct answer because it is the primary factor that causes matter to change from one state to another. When heat is applied to a substance, it increases the kinetic energy of its particles, causing them to move faster and break the intermolecular forces holding them together. This results in a change of state, such as solid to liquid (melting) or liquid to gas (evaporation). Heat is essential in the process of changing the physical state of matter.Rate this question:
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- 9.
The molecules in a liquid spread out to fill the entire container.
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
Molecules in a liquid do not spread out to fill the entire container. Unlike gases, liquids have a definite volume and take the shape of the container they are in, but the molecules still remain close together. The movement of liquid molecules is more restricted compared to gases, as they have stronger intermolecular forces holding them together.Rate this question:
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- 10.
Water in its gas state is called __________.
- A.
Clouds
- B.
Gas water
- C.
Water
- D.
Water vapor (steam)
Correct Answer
D. Water vapor (steam)Explanation
Water in its gas state is called water vapor or steam. When water evaporates, it turns into a gas and becomes water vapor. This is commonly seen when water boils, and steam is produced. Water vapor is invisible, but it can condense into visible water droplets when it cools down, forming clouds or fog. Therefore, the correct answer is water vapor (steam).Rate this question:
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- 11.
The molecules in a solid stay closely and vibrate against each other.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
In a solid, the molecules are tightly packed together and have strong intermolecular forces holding them in place. Due to this close proximity, the molecules are able to vibrate against each other. This vibration is responsible for the solid's rigidity and ability to maintain its shape. Therefore, the statement that the molecules in a solid stay closely and vibrate against each other is true.Rate this question:
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- 12.
The molecules in a gas move fast and spread out to fill the entire container.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
In a gas, the molecules are in constant motion and have high kinetic energy. This causes them to move rapidly and randomly, colliding with each other and the walls of the container. As a result, they spread out to fill the entire available space within the container. Therefore, the statement "The molecules in a gas move fast and spread out to fill the entire container" is true.Rate this question:
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- 13.
Determine the main type of intermolecular forces in ethanol C2H5OH.
- A.
London dispersion forces
- B.
Dipole-depole forces
- C.
Hydrogen bonding
- D.
Ion-ion oposite attractions
Correct Answer
C. Hydrogen bondingExplanation
It is hydrogen bonding because there is attraction between a hydrogen from one molecule with an oxygen from another molecule. Hydrogen bonding is a strong IMF, causing ethanol exist as a liquid at room temperature.Rate this question:
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- 14.
Determine the main type of intermolecular forces in PH3.
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
Correct Answer
C. Dipole-Dipole ForcesExplanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding; Saltwater (ionic compound and water)=Ion-Dipole Forces. Since PH3 is a polar molecule (it's asymmetrical overall, in terms of charge distribution) without H-F, H-O, or H-N, this qualifies as having dipole-dipole forces.Rate this question:
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- 15.
Determine the main type of intermolecular forces in CCl4.
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
Correct Answer
A. London Dispersion ForcesExplanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding;
Saltwater (ionic compound and water)=Ion-Dipole Forces. Since CCl4 is nonpolar (symmetrical distribution of charge overall), this qualifies as having London Dispersion Forces.Rate this question:
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- 16.
Rank the following molecules in order of increasing boiling point: NaF (salt), H2S, HF, CO2.
- A.
NaF < H2S < HF < CO2
- B.
H2S < CO2 < HF < NaF
- C.
CO2 < H2S < HF < NaF
- D.
CO2 < HF < H2S < NaF
Correct Answer
C. CO2 < H2S < HF < NaFExplanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest IMF's, lowest boiling point); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding; Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest IMF's, highest boiling point). CO2 is nonpolar (symmetrical distribution of charge), so it has London forces. H2S is a polar molecule (asymmetrical distribution of charge) without H-F, H-O, or H-N, so it has dipole-dipole forces. HF has F-H in its structure, so it has hydrogen bonding. NaF is an ionic compound, so it has ion-ion opposite attractions. In order, London forces are weakest, dipole-dipole forces are stronger, hydrogen bonds are even stronger than dipole-dipole, and ion-ion forces are strongest.Rate this question:
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- 17.
Rank the following molecules in order of increasing boiling point: CH3Cl, CH3OH, Na2O (aq), CF4.
- A.
CF4 < CH3OH < CH3Cl < Na2O (aq)
- B.
CF4 < CH3Cl < CH3OH < Na2O (aq)
- C.
CF4 < Na2O (aq) < CH3Cl < CH3OH
- D.
CF4 < Na2O (aq) < CH3OH < CH3Cl
Correct Answer
B. CF4 < CH3Cl < CH3OH < Na2O (aq)Explanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest IMF's, lowest boiling point); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding; Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest IMF's, highest boiling point). CF4 is nonpolar (symmetrical distribution of charge), so it has London forces. CH3Cl is a polar molecule (asymmetrical distribution of charge) without H-F, H-O, or H-N, so it has dipole-dipole forces. CH3OH has O-H in its structure, so it has hydrogen bonding. Na2O (aq) has an ionic compound, Na2O, dissolved in water (aq), so it has ion-dipole forces. In order, London forces are weakest, dipole-dipole forces are stronger, hydrogen bonds are even stronger than dipole-dipole, and ion-dipole forces are strongest.Rate this question:
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- 18.
At standard pressure, NH3 has a boiling point of 240 K, AsH3 has a boiling point of 211 K, and PH3 has a boiling point of 186 K. What accounts for the higher boiling point of NH3?
- A.
NH3 has a higher boiling point, because it contains London forces.
- B.
NH3 has a higher boiling point, because it contains hydrogen bonds.
- C.
NH3 has a higher boiling point, because it contains dipole-dipole forces.
- D.
NH3 has a higher boiling point, because it contains ion-dipole forces.
Correct Answer
B. NH3 has a higher boiling point, because it contains hydrogen bonds.Explanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding; Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest). NH3 has H-N, so it has hydrogen bonding. AsH3 and PH3 are polar molecules (asymmetrical distribution of charge) without H-O, N-H, and H-F, so they have dipole-dipole forces. Hydrogen bonding is stronger than dipole-dipole forces are, so NH3 has the highest boiling point, because it has the strongest IMF's out of the three molecules.Rate this question:
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- 19.
At standard pressure, HF has a higher boiling point than HCl, HBr, or H2 does. What accounts for the higher boiling point of HF?
- A.
HF has a higher boiling point, because it contains London forces.
- B.
HF has a higher boiling point, because it contains hydrogen bonds.
- C.
HF has a higher boiling point, because it contains dipole-dipole forces.
- D.
HF has a higher boiling point, because it contains ion-dipole forces.
Correct Answer
B. HF has a higher boiling point, because it contains hydrogen bonds.Explanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding;
Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest). HF has H-F, so it has hydrogen bonding. HCl and HBr are polar molecules (asymmetrical distribution of charge) without H-F, H-N, or H-O, so they have dipole-dipole forces. H2 is a nonpolar molecule (symmetrical distribution of charge), so it has London forces. Hydrogen bonding in H-F is the strongest IMF (stronger than dipole-dipole and London forces), so HF will have the highest boiling point, because it has the strongest IMF's of the four molecules.Rate this question:
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- 20.
At standard pressure, HF and NH3 have higher boiling points than HBr and CH4 do. What accounts for the higher boiling point of HF?
- A.
NH3 and HF have higher boiling points, because they contain London Forces.
- B.
NH3 and HF have higher boiling points, because they contain hydrogen bonds.
- C.
NH3 and HF have higher boiling points, because they contain dipole-dipole forces.
- D.
NH3 and HF have higher boiling points, because they contain ion-dipole forces.
Correct Answer
B. NH3 and HF have higher boiling points, because they contain hydrogen bonds.Explanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding;
Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest). NH3 and HF have hydrogen bonding because they have H-F/H-O/H-N bonded. HBr is polar, so it's just dipole-dipole. CH4 is nonpolar, so it's London Dispersion Forces. Hydrogen Bonds are stronger IMF's than dipole-dipole and London Forces are, so NH3 and HF have higher boiling points as a result.Rate this question:
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- 21.
At standard pressure, H2Se and CO have higher boiling points than CF4 and CO2 do. What accounts for the higher boiling point of H2Se and CO?
- A.
H2Se and CO have higher boiling points, because they contain London Forces.
- B.
H2Se and CO have higher boiling points, because they contain hydrogen bonds.
- C.
H2Se and CO have higher boiling points, because they contain dipole-dipole forces.
- D.
H2Se and CO have higher boiling points, because they contain ion-dipole forces.
Correct Answer
C. H2Se and CO have higher boiling points, because they contain dipole-dipole forces.Explanation
Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big ∆EN)=Hydrogen Bonding
Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest). H2Se and CO have dipole-dipole forces because they are polar molecules without H-F/H-O/H-N. CF4 and CO2 are both nonpolar, so they have London Dispersion Forces. Dipole-Dipole Forces are stronger IMF's than London Forces are, so H2Se and CO have higher boiling points as a result.Rate this question:
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- 22.
Compounds like CuO and NaHCO3 are soluble in water. Compare the boiling point of a solution of CuO to the boiling point of water at standard pressure.
- A.
The solution of CuO has a higher boiling point than water does.
- B.
Water has a higher boiling point than the CuO solution does.
Correct Answer
A. The solution of CuO has a higher boiling point than water does.Explanation
Ionic Compound + Water=Ion-Dipole Forces (strongest IMF's); H-O, H-N, H-F=Hydrogen Bonds (Weaker than Ion-dipole forces); CuO in water is an ionic compound in water, so it has ion-dipole forces. On the other hand, water has H-O, so it has hydrogen bonding. Ion-dipole has stronger IMF's and, therefore, a higher boiling point.Rate this question:
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- 23.
A mixture contains hydrogen fluoride and ammonia. Identify a strong intermolecular force of attraction between hydrogen fluoride and ammonia.
- A.
Dipole-Dipole Forces
- B.
Hydrogen Bonding
- C.
Ion-Dipole Forces
- D.
London Dispersion Forces
Correct Answer
B. Hydrogen BondingExplanation
H-O, H-N, H-F=Hydrogen Bonds (Weaker than Ion-dipole forces). Both hydrogen fluoride (HF) and ammonia (NH3) contain H-F, H-O, or H-N bonds, so the IMF's between them are hydrogen bonds.Rate this question:
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- 24.
Which element combines with hydrogen to form a compound with the strongest hydrogen bonding between its molecules?
- A.
Sulfur
- B.
Tellurium
- C.
Selenium
- D.
Oxygen
Correct Answer
D. OxygenExplanation
H-O, H-N, H-F=Hydrogen Bonds (Weaker than Ion-dipole forces). H and O makes an H-O bond, so the IMF's between the molecules are hydrogen bonding.Rate this question:
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- 25.
Substance A has a boiling point of 13 degrees Celsius, Substance B has a boiling point of 20 degrees Celsius, Substance C has a boiling point of 23 degrees Celsius, Substance D has a boiling point of 12 degrees Celsius. Which substance has the strongest intermolecular forces?
- A.
Substance A
- B.
Substance B
- C.
Substance C
- D.
Substance D
Correct Answer
C. Substance CExplanation
Higher Boiling Point=Stronger Intermolecular Forces.Rate this question:
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Mar 21, 2023Quiz Edited by
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Nov 14, 2016Quiz Created by
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