Quiz 10: Solids and Liquids

Dipole-dipole interactions are generally weaker than dispersion forces.

Polar molecules have a significantly higher boiling point than nonpolar molecules.

H₂O molecules experience hydrogen bonding.

Hydrocarbons such as CH₄ experience strong hydrogen bonding.

The strongest intermolecular forces present in a H₂S molecule are dispersion forces.

Melting is always an endothermic reaction.

ΔH will be negative for a solidification reaction.

A substance stays at the same temperature during melting.

The process of a liquid becoming a solid is called solidification.

The process of a solid-to-gas change is called deposition.

The energy change when 24 g of H₂O(g) condenses to a liquid at 100°C is 40.68 kJ. (ΔH_vap of H₂O = 40.68 kJ/mol; molar mass of H₂O = 18 g/mol)

Enthalpy of vaporization is the amount of energy needed to change from a liquid to a gas or from a gas to a liquid.

The formation of a gas from a liquid at temperatures below the boiling point is called evaporation.

The partial pressure of the vapor at equilibrium is called the vapor pressure of the liquid.

Vapor pressures of solids are typically much higher than that of liquids.

The vapor pressure for a substance is inversely proportional to the temperature.

Surface tension is an effect caused by an imbalance of forces on the atoms at the surface of a liquid.

Adhesion is the tendency of a substance to interact with itself.

Mercury has stronger adhesive forces than cohesive forces.

Solids can be easily compressed.

An amorphous solid has no long-term structure or repetition.

A crystalline solid has a regular, repeating three-dimensional structure.

Ionic solids are conductors of electricity in their solid state.

Carbon in its diamond form is a covalent network solid.

The element Ag will exist as a metallic solid in the solid state.

The preferred phase of a substance at a given set of conditions is a balance between the _____ of the particles and intermolecular forces between the particles. A) magnetic properties B) energy C) flammability D) wavelength E) frequency

_____ is caused by the instantaneous position of an electron in a molecule, which temporarily makes that point of the molecule negatively charged and the rest of the molecule positively charged. A) Dipole-dipole interaction B) Hydrogen bonding C) Ionic bonding D) Covalent bonding E) Dispersion force

Considering the dispersion force, which of the following molecules is least likely to be a gas? A) calcium B) neon C) nitrogen D) oxygen E) neon

By looking at the periodic table, identify the atom that would experience the strongest dispersion force. A) N B) O C) Al D) C E) Cl

Identify the substance where the most significant intermolecular force would be the dispersion force. A) HCl B) HBr C) C₂H₆ D) NaOH E) NH₃

Which of the following substances experience hydrogen bonding? A) H₂O B) HCl C) CH₄ D) H₂S E) C₆H₆

Identify the substance for which the most significant intermolecular force will be the dispersion force. A) NaCl B) NH₃ C) HCl D) C₃H₈ E) (CH₃)₂CO

For which of the following products will the most significant intermolecular force NOT be the dipole-dipole interaction? A) HF B) C₆H₅OH C) HI D) NH₃ E) CH₄

Hydrogen bonds are formed when hydrogen is bonded to a(n) _____ atom. A) sodium B) chlorine C) bromine D) oxygen E) iodine

The process of a solid becoming a liquid is called _____. A) boiling B) normalization C) solidification D) freezing E) melting

The temperature at which a substance in the solid state becomes a liquid is called the_____. A) heat of formation B) latent point C) melting point D) boiling point E) entropy of fusion

Which of the following at best describes the enthalpy of fusion? A) Energy needed to change from a liquid to gas B) Temperature at which melting occurs C) Temperature at which boiling occurs D) Energy needed to change from a solid to liquid E) Temperature at which a solid becomes conductive

A reaction where the substance remains at the same temperature is called a(n) _____. A) adiabatic process B) isothermal process C) isobaric process D) polytrophic process E) isochoric process

What will happen to liquids when stored in zero gravity environments? A) Liquids take the shape of the container. B) Liquids Harden and become solid particles. C) Liquids float in such environments. D) Liquids expand to become a larger mass. E) Liquids evaporate to become gases.

Which of the following refers to the amount of energy required to convert a liquid to a gas? A) Enthalpy of formation B) Heat of fusion C) Enthalpy of fusion D) Heat of liquidation E) Enthalpy of vaporization

What is the energy change when 72 g of H₂O (g) condense to a liquid at 373 K? (ΔH_vap of water = 40.68 kJ/mol; molar mass of H₂O = 18 g/mol) A) 81 kJ B) 41 kJ C) 160 kJ D) 210 kJ E) 240 kJ

The energy change occurring is 2.10 kJ when_____ of H₂O (g) condenses to a liquid at 100°C. (ΔH_vap of water = 40.68 kJ/mol; molar mass of H₂O = 18 g/mol). A) 12.6 g B) 8.56 g C) 1.63 g D) 17.6 g E) 0.929 g

What is the energy change when 565 g of C₂H₅OH boil at its normal boiling point of 78.3°C? (ΔH_vap for ethanol = 38.6 kJ/mol; molar mass of C₂H₅OH = 46.0 g/mol) A) 396 kJ B) 302 kJ C) 119 kJ D) 474 kJ E) 124 kJ

Which of the following terms refer to the solid-to-gas change of compounds? A) Boiling B) Normalization C) Solidification D) Deposition E) Sublimation

Identify the term that refers to the gas-to-solid change of compounds. A) Deposition B) Normalization C) Solidification D) Sublimation E) Boiling

The ΔH_vap for water is 40.68 kJ/mol and the ΔH_fus is 6.010 kJ/mol. Calculate the ΔH_sub. A) 34.67 kJ/mol B) 46.69 kJ/mol C) 244.5 kJ/mol D) 69.34 kJ/mol E) 93.38 kJ/mol

The formation of a gas from a liquid at temperatures below the boiling point is called _____. A) sublimation B) deposition C) evaporation D) melting E) under-boiling

Which of the following is considered the reverse process of vaporization? A) osmosis B) solidification C) melting D) sublimation E) condensation

The temperature at which the vapor pressure of a liquid equals the surrounding environmental pressure is called the _____. A) enthalpy of fusion B) boiling point C) melting point D) enthalpy of vaporization E) freezing point

The normal vapor pressure is the temperature at which the vapor pressure is _____ torr. A) 460 B) 500 C) 600 D) 760 E) 800

By referring to the plots of vapor pressure versus temperature provided in the text, identify the likely boiling point of water at 600 torr vapor pressure. A) 92°C B) 98°C C) 56°C D) 69°C E) 78°C

_____ is responsible for the fact that small insects can "walk" on water. A) Vapor pressure B) Surface tension C) Change in enthalpy D) Density E) Viscosity

Certain liquids tend to bead up when present in small amounts. What is the reason for this? A) low surface tension B) high vapor pressure C) low vapor pressure D) high surface tension E) low density

Liquids form spheres in free fall or zero gravity. Which of the following is the reason for this behavior? A) liquid vapor pressure B) surface tension C) viscosity D) low density E) entropy

_____ is the tendency of a substance to interact with other substances because of intermolecular forces. A) Adhesion B) Viscosity C) Osmosis D) Capillary action E) Cohesion

_____ is the tendency of a substance to interact with itself. A) Surface tension B) Adhesion C) Osmosis D) Cohesion E) Viscosity

When a liquid is introduced to a small-diameter tube of another substance, the liquid moves up or down in the tube, as if ignoring gravity. Which of the following terms specifically refers to this action? A) adhesion B) capillary action C) surface tension D) cohesion E) viscosity

Which of the following is a major similarity between solids and liquids? A) Strength of the intermolecular forces is the same in both the phases B) Covalent bonds are not common in both the phases C) The particles are in contact with each other in both the phases D) Hydrogen bonds are not common in both the phases E) They can take the shape of the container in which they are stored

A(n) _____ solid is a solid with no long-term structure or repetition. A) amorphous B) crystalline C) molecular D) ionic E) covalent network

A(n) _____ solid is a solid that has a regular, repeating three-dimensional structure. A) amorphous B) molecular C) ionic D) covalent network E) crystalline

Which of the following is an example of an amorphous solid? A) metals B) biological molecules C) glasses D) salt crystals E) semiconductors

An NaCl crystal is an example of a(n) _____ solid A) crystalline B) ionic C) molecular D) amorphous E) covalent network

Which of the following is an ionic solid? A) NaBr B) I₂ C) C₆H₆ D) S₅ E) C₆Cl₆

Which of the following types of bonding is commonly seen in molecular solids? A) hydrogen bond B) ionic bond C) ion-dipole bond D) covalent bond E) dipole interaction

Which of the following is a molecular solid? A) CuCl B) AuCl C) NaCl D) CuCl₂ E) CCl₄

What kind of crystal would CH₄ form in its solid state? A) ionic B) molecular C) amorphous D) crystalline E) covalent network

Which of the following elements will form a metallic solid in its solid state? A) O B) S C) Se D) Cu E) C

A shiny and silvery solid substance stored in the form of a sheet is a(n) _____ solid. A) amorphous B) ionic C) metallic D) crystalline E) covalent network

Why does a substance have the phase it does? How does the temperature affect the existence in various phases?

What is dispersion force? Explain.

What are dipole-dipole interactions?

Does hydrogen bonding exist in both H₂S and NH₃? Explain your answer.

Explain the terms melting, solidification, and melting point.

What is enthalpy of fusion? Provide an example.

Explain how boiling point changes with changes in pressure.

What are sublimation and deposition? What is enthalpy of sublimation?

Explain the process of evaporation.

What is surface tension? List some of its effects on liquids.

What are adhesion and cohesion? What are their impacts?

Explain the concept of capillary action.

What are amorphous solids? Provide examples.

What are ionic solids? Explain with an example.

What are molecular solids? Explain their behavior. Provide an example.

_____ is an intermolecular force caused by the instantaneous position of an electron in a molecule.

_____ is an intermolecular force caused by molecules with a permanent dipole.

The process of a solid becoming a liquid is called _____.

The characteristic temperature at which a solid becomes a liquid is called the _____.

_____ refers to the amount of energy needed to change from a solid to a liquid or from a liquid to a solid.

The process of a gas becoming a liquid is called _____.

The amount of energy needed to change from a liquid to a gas or from a gas to a liquid is referred to as _____.

The process of a gas becoming a solid is called _____.

The formation of a gas phase from a liquid at temperatures below the boiling point is called _____.

_____ refers to a situation in which a process still occurs but the opposite process also occurs at the same rate so that there is no net change in the system.

_____ refers to an effect caused by an imbalance of forces on the atoms at the surface of a liquid.

The tendency of a substance to interact with other substances because of intermolecular forces is called _____.

A solid with a regular, repeating three-dimensional structure is known as a(n) _____ solid.

_____ are crystalline solids whose components are covalently bonded molecules.

A solid with the characteristic properties of a metal is called a(n) _____ solid.