Chemistry Chapter 11 Flashcards
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Questions and Answers

What are the main properties of liquids in contrast to gases and solids?

  • Easily compressed
  • Definite volume (correct)
  • High density compared to gases (correct)
  • Indefinite shape and assumes the shape of their container (correct)

    • What are the main properties of solids in contrast to liquids and gases?

  • Easily compressed
  • Higher density compared to gases (correct)
  • Definite volume (correct)
  • Definite shape (correct)

    • What factors cause changes between the solid and liquid state?

    Cooling converts a liquid to a solid; heating converts a solid to a liquid.

    What factors cause changes between the liquid and gas state?

    <p>Increasing pressure or cooling converts gas to liquid; heating converts liquid to gas.</p> Signup and view all the answers

    What happens to physical properties as the strength of intermolecular forces increases?

    <p>Boiling point increases</p> Signup and view all the answers

    What intermolecular force is present in all molecules and atoms?

    <p>Dispersion forces</p> Signup and view all the answers

    The dispersion force increases with increasing molar mass.

    <p>True</p> Signup and view all the answers

    Where do dipole-dipole forces exist?

    <p>In all polar molecules.</p> Signup and view all the answers

    Which atoms bond with hydrogen in hydrogen bonding?

    <p>Fluorine, Oxygen, and Nitrogen.</p> Signup and view all the answers

    What is the strongest intermolecular force?

    <p>Hydrogen bonds.</p> Signup and view all the answers

    When does the ion-dipole force occur?

    <p>When an ionic compound is mixed with a polar compound.</p> Signup and view all the answers

    What is surface tension of a liquid?

    <p>The energy required to increase surface area by a unit amount.</p> Signup and view all the answers

    What is viscosity?

    <p>The resistance of a liquid to flow.</p> Signup and view all the answers

    What is capillary action?

    <p>The ability of a liquid to flow against gravity up a narrow tube.</p> Signup and view all the answers

    What are cohesive forces versus adhesive forces?

    <p>Cohesive forces are attractions between molecules in a liquid; adhesive forces are attractions between molecules and the surface of a tube.</p> Signup and view all the answers

    What is vaporization?

    <p>The process by which thermal energy overcomes intermolecular forces to produce a state change from liquid to gas.</p> Signup and view all the answers

    What is the transition from gas to liquid called?

    <p>Condensation.</p> Signup and view all the answers

    What are volatile and non-volatile liquids?

    <p>Liquids that vaporize easily</p> Signup and view all the answers

    Is vaporization endothermic?

    <p>True</p> Signup and view all the answers

    Is condensation endothermic?

    <p>False</p> Signup and view all the answers

    What is the heat of vaporization?

    <p>The amount of heat required to vaporize one mole of a liquid to gas.</p> Signup and view all the answers

    What is dynamic equilibrium?

    <p>When the rate of condensation equals the rate of vaporization.</p> Signup and view all the answers

    What is vapor pressure?

    <p>The pressure of gas in dynamic equilibrium with its liquid.</p> Signup and view all the answers

    What is the boiling point of a liquid?

    <p>The temperature at which the liquid's vapor pressure equals the external pressure.</p> Signup and view all the answers

    What is the normal boiling point of a liquid?

    <p>The temperature at which its vapor pressure equals 1 atm.</p> Signup and view all the answers

    What is sublimation?

    <p>The transition directly from solid to gas phase.</p> Signup and view all the answers

    What is a phase diagram?

    <p>A map of the state or phase of a substance as a function of pressure.</p> Signup and view all the answers

    What is the triple point on a phase diagram?

    <p>The unique set of conditions at which the three states are equally stable and in equilibrium.</p> Signup and view all the answers

    What is the critical point on a phase diagram?

    <p>The temperature and pressure above which a supercritical fluid exists.</p> Signup and view all the answers

    What is the fusion curve, sublimation curve, and vaporization curve?

    <p>Requires transition from solid to liquid</p> Signup and view all the answers

    What are molecular solids?

    <p>Solids whose composite units are molecules.</p> Signup and view all the answers

    What are ionic solids?

    <p>Solids with composite units that are ions.</p> Signup and view all the answers

    What are atomic solids?

    <p>Solids whose composite units are individual atoms.</p> Signup and view all the answers

    What are nonbonding atomic solids?

    <p>Solids held together by relatively weak dispersion forces.</p> Signup and view all the answers

    What are metallic atomic solids?

    <p>Solids held together by metallic bonds.</p> Signup and view all the answers

    What are covalent atomic solids?

    <p>Solids held together by covalent bonds.</p> Signup and view all the answers

    What is a solution?

    <p>A homogeneous mixture of two or more substances.</p> Signup and view all the answers

    What is a solvent?

    <p>The majority component in a solution.</p> Signup and view all the answers

    What is a solute?

    <p>The minority component in a solution.</p> Signup and view all the answers

    What is the solubility of a substance?

    <p>The amount of the substance that will dissolve in a given amount of solvent.</p> Signup and view all the answers

    What is entropy?

    <p>A measure of energy randomization or energy dispersal in a system.</p> Signup and view all the answers

    When heat is evolved, the solution process is...

    <p>Exothermic.</p> Signup and view all the answers

    When heat is absorbed, the solution process is...

    <p>Endothermic.</p> Signup and view all the answers

    What is a saturated solution?

    <p>A solution in which the dissolved solute is in dynamic equilibrium with the solid solute.</p> Signup and view all the answers

    What is an unsaturated solution?

    <p>A solution containing less than the equilibrium amount of solute.</p> Signup and view all the answers

    What is a supersaturated solution?

    <p>One containing more than the equilibrium amount of solute.</p> Signup and view all the answers

    How does temperature affect the solubility of solids and gases?

    <p>Solubility of solids increases with temperature; solubility of gases decreases.</p> Signup and view all the answers

    What is osmosis?

    <p>The flow of a solvent from a solution of lower solute concentration to one of higher solute concentration.</p> Signup and view all the answers

    Study Notes

    Properties of States of Matter

    • Liquids have a definite volume and higher density compared to gases; they take the shape of their container and are not easily compressed.
    • Solids possess a definite shape and volume, are dense, resistant to compression, and can be classified as crystalline (ordered) or amorphous (disordered).

    State Changes

    • A liquid transforms into a solid through cooling, while heating converts a solid into a liquid.
    • The interconversion between liquid and gas states is influenced by pressure increases or cooling for gas to liquid, and heating for liquid to gas.

    Intermolecular Forces

    • Increasing intermolecular forces raise melting point, boiling point, viscosity, and surface tension, while lowering vapor pressure.
    • Dispersion forces exist in all molecules and atoms, with strength increasing alongside molar mass.
    • Dipole-dipole forces occur in polar molecules, while hydrogen bonds form between hydrogen and F, O, or N.

    Phase Transition Processes

    • Ion-dipole forces arise when ionic compounds mix with polar compounds, representing the strongest intermolecular force.
    • Surface tension is the energy needed to increase a liquid's surface area, while viscosity measures a liquid's resistance to flow.
    • Capillary action refers to a liquid's ability to rise against gravity in a narrow tube.

    Vaporization and Condensation

    • Vaporization is an endothermic process where thermal energy allows liquid to convert to gas.
    • Condensation, an exothermic process, occurs when gas transitions to a liquid, releasing heat.
    • Heat of vaporization represents the heat required to vaporize one mole of liquid, increasing with stronger intermolecular forces.

    Equilibrium and Phase Diagrams

    • Dynamic equilibrium refers to equal rates of vaporization and condensation.
    • Vapor pressure is the pressure exerted by a gas in equilibrium with its liquid.
    • The boiling point is when a liquid's vapor pressure matches the external pressure; normal boiling point occurs at 1 atm.

    Sublimation and Phase Diagrams

    • Sublimation is the direct transition from solid to gas.
    • A phase diagram displays the states of matter versus pressure, with key points like the triple point (where all states are stable) and the critical point (above which a supercritical fluid exists).
    • Fusion, sublimation, and vaporization curves indicate the transitions between solid, gas, and liquid phases.

    Types of Solids

    • Molecular solids consist of molecules and have lower melting points.
    • Ionic solids are made of ions, exhibiting high melting points.
    • Atomic solids consist of individual atoms and can be further categorized into nonbonding, metallic, and covalent atomic solids based on bonding types.

    Solutions and Solubility

    • Solutions are homogeneous mixtures comprised of a solvent (majority component) and solute (minority component).
    • Solubility defines how much substance dissolves in a given solvent; solid solubility generally increases with temperature, whereas gas solubility decreases.
    • The solution process can be exothermic (heat evolved) or endothermic (heat absorbed), influencing solute dynamic equilibria.

    Saturation States

    • A saturated solution contains solute in dynamic equilibrium with solid solute, while an unsaturated solution holds less than the equilibrium amount.
    • A supersaturated solution contains more solute than equilibrium allows, demonstrating unique chemical behavior.

    Osmosis

    • Osmosis describes solvent movement from lower to higher solute concentration solutions, highlighting the natural tendency for mixtures to equilibrate.

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    Description

    Explore the key properties of liquids and solids in this Chemistry Chapter 11 flashcard quiz. Understand how these states of matter compare to gases, highlighting their unique characteristics. Perfect for reinforcing your chemistry knowledge and preparing for exams.

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