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 (C), Melting point increases (D)</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 (A)</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 (B), Liquids that do not vaporize easily (D)</p> Signup and view all the answers

Is vaporization endothermic?

<p>True (A)</p> Signup and view all the answers

Is condensation endothermic?

<p>False (B)</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 (A), Transition from solid to gas (C), Transition from liquid to gas (D)</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

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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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