COPY: States of Matter and Intermolecular Forces
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Questions and Answers

What distinguishes the state of a solid from a liquid?

  • A solid can be compressed significantly.
  • A solid has no definite shape.
  • A solid cannot fill a container.
  • A solid has a definite volume and shape. (correct)

Which statement about gases is correct?

  • Gases fill the entire volume of their container. (correct)
  • Gases have a definite volume but no fixed shape.
  • Gases tend to have stronger interparticle attractions than liquids.
  • Gases can be compressed to occupy a larger volume.

How does the kinetic energy of particles in a gas compare to that in a solid?

  • Particles in a gas have lower kinetic energy than those in a solid.
  • Particles in a gas have higher kinetic energy than those in a solid. (correct)
  • Kinetic energy is irrelevant to the states of matter.
  • Particles in a gas have the same kinetic energy as those in a solid.

Which of the following best describes plasma?

<p>Plasma is formed at high temperatures with ionized gases. (B)</p> Signup and view all the answers

Why do liquids have a distinct volume?

<p>Because liquid particles have strong interparticle attractions. (D)</p> Signup and view all the answers

What factor primarily affects the state of matter of a substance?

<p>The temperature and kinetic energy of the particles. (C)</p> Signup and view all the answers

Which state of matter is characterized by particles that are widely spaced and have minimal attraction to each other?

<p>Gas (B)</p> Signup and view all the answers

In what way does a liquid differ from a gas regarding compressibility?

<p>Liquids are not compressible to any appreciable extent. (A)</p> Signup and view all the answers

What typically causes Permanent Dipole-Permanent Dipole interactions?

<p>Differences in electronegativity between bonded atoms (B)</p> Signup and view all the answers

Which pair of substances is influenced by Permanent Dipole-Permanent Dipole interactions?

<p>Bromine fluoride (BrF) and sulfur dioxide (SO2) (A)</p> Signup and view all the answers

How does a polar molecule induce a dipole moment in a nonpolar molecule?

<p>Through the disruption of electron arrangement (D)</p> Signup and view all the answers

Which of the following types of intermolecular forces is stronger than dipole-induced dipole interactions?

<p>Both B and C (D)</p> Signup and view all the answers

What is the characteristic of Induced Dipole - Induced Dipole (Dispersion Forces)?

<p>They are significant only over very short distances (B)</p> Signup and view all the answers

Which of the following statements about dipole-dipole interactions is true?

<p>Attractive forces arise from opposite charges in polar molecules (A)</p> Signup and view all the answers

Which interaction is characterized by very weak forces and present in all types of molecules in condensed phases?

<p>Induced Dipole – Induced Dipole (Dispersion Forces) (B)</p> Signup and view all the answers

What is the average energy associated with a dipole-dipole interaction per mole of bonds?

<p>4 kJ (D)</p> Signup and view all the answers

What primarily accounts for the high melting and boiling points of water compared to similar compounds?

<p>Hydrogen bonding (C)</p> Signup and view all the answers

In the dissolution process, what is a characteristic of a solution?

<p>It is a homogeneous mixture. (C)</p> Signup and view all the answers

Which type of intermolecular forces are present in water?

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

What are the components of a solution?

<p>Solvent and solute (D)</p> Signup and view all the answers

What happens to solids like sodium chloride when water evaporates from their solution?

<p>They yield the original solid. (B)</p> Signup and view all the answers

Which factor does NOT influence the ease of dissolution of a solute?

<p>The color of the solute (D)</p> Signup and view all the answers

In the case of nitrogen dioxide (NO2), what type of intermolecular forces are expected?

<p>Dipole-dipole interactions and London dispersion forces (D)</p> Signup and view all the answers

What defines the solvent in a solution?

<p>It is the most abundant species present. (A)</p> Signup and view all the answers

What is the primary reason that an exothermic dissolution process is favored?

<p>Decrease in the energy of the system (D)</p> Signup and view all the answers

Which of the following statements is true regarding weak attractions in the dissolution process?

<p>Weak solute-solute attractions favor solubility (C)</p> Signup and view all the answers

What does the heat of solution, ΔHsolution, primarily depend on?

<p>The strength of interactions between solute and solvent (C)</p> Signup and view all the answers

Which step in the dissolution process is considered endothermic?

<p>Overcoming solute-solute attractions (C)</p> Signup and view all the answers

For a dissolution process to be considered exothermic overall, what must occur?

<p>Energy released in Step c must exceed the energy absorbed in Steps a and b (B)</p> Signup and view all the answers

How does dissolution contribute to disorder in a solution?

<p>Solute particles gain freedom of motion in the solution (C)</p> Signup and view all the answers

In which of the following scenarios can a solid dissolve in a liquid despite an endothermic process?

<p>If there is a large increase in disorder during dissolution (D)</p> Signup and view all the answers

What role does entropy play in the dissolution process of solids in liquids?

<p>A high disorder in the solute can favor dissolution (A)</p> Signup and view all the answers

What is the main reason that naphthalene does not dissolve in water?

<p>Naphthalene is nonpolar while water is polar. (C)</p> Signup and view all the answers

Which factor increases the magnitude of lattice energy in ionic compounds?

<p>Decreasing size of ions. (B)</p> Signup and view all the answers

What type of process is the dissolution of most ionic solids that release heat?

<p>Always exothermic. (C)</p> Signup and view all the answers

Which of the following statements is true regarding gases dissolving in liquids?

<p>Polar gases are most soluble in polar solvents. (A)</p> Signup and view all the answers

What is the term for the dissolution process when considering liquids mixing with liquids?

<p>Miscibility. (B)</p> Signup and view all the answers

How does the charge-to-size ratio affect the solubility of ionic solids?

<p>As the ratio increases, lattice energy often increases more than hydration energy. (C)</p> Signup and view all the answers

What is the dissolution behavior of ammonium nitrate, NH4NO3?

<p>It dissolves slightly endothermically. (D)</p> Signup and view all the answers

Why does carbon dioxide seem to have higher solubility in water compared to other nonpolar gases?

<p>It chemically reacts with water to form carbonic acid. (B)</p> Signup and view all the answers

Flashcards

Solid

A state of matter with a fixed volume and shape due to strong interparticle attractions, causing particles to be tightly packed and vibrate in fixed positions.

Liquid

A state of matter with a fixed volume but takes the shape of its container due to weaker interparticle attractions compared to solids. Particles can move more freely but remain in contact.

Gas

A state of matter with no fixed volume or shape, particles are far apart and have weak attractions. They move freely and rapidly in all directions.

Plasma

A state of matter characterized by ionized gas with extremely high temperatures, where electrons are stripped from their atoms creating a mix of ions and electrons.

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Kinetic Energy

The energy of motion possessed by particles. It's higher in gases than solids due to greater freedom of movement.

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Intermolecular Forces

Attractive forces between molecules that hold them together in liquids and solids.

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Dipole-Dipole Interactions

A type of intermolecular force that arises from the permanent dipoles of polar molecules, due to unequal sharing of electrons.

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Dipole-Induced Dipole Interactions

A type of intermolecular force that results from temporary dipoles induced in nonpolar molecules by nearby polar molecules or temporary dipoles in other nonpolar molecules.

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London Dispersion Forces

A type of intermolecular force that arises from temporary fluctuations in electron distribution leading to temporary dipoles in all molecules. They are present in all substances but particularly significant in nonpolar molecules and become stronger with increasing size and mass of the molecule.

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Hydrogen Bonding

A strong type of dipole-dipole interaction where a hydrogen atom is bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine) and interacts with a lone pair of electrons on a nearby electronegative atom.

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Dissolution

The process of dissolving a solute in a solvent to form a homogeneous mixture.

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Solvent

The substance that dissolves the solute and is usually present in the larger amount in a solution.

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Solute

The substance that gets dissolved in a solvent. It's the substance being dissolved.

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Solution

A homogeneous mixture formed when a solute dissolves in a solvent, with uniform composition throughout.

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Heat of Solution, ΔHsolution

The energy change associated with dissolving a solute in a solvent. A negative value indicates exothermic dissolution (heat released), and a positive value indicates endothermic dissolution (heat absorbed).

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Solute-Solute Attractions

The attractive forces between solute particles that must be overcome for dissolution to occur.

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Solvent-Solvent Attractions

The attractive forces between solvent particles that must be overcome for dissolution to occur.

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Solute-Solvent Attractions

The attractive forces between solute and solvent particles that drive the dissolution process.

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Solubility

The measure of the tendency of a solid to dissolve in a liquid. It is determined by the balance between attractive and repulsive forces between solute, solvent, and solution particles.

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Lattice Energy

The energy required to break apart the crystal lattice of an ionic compound.

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Hydration Energy

The energy released when ions are surrounded by solvent molecules.

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Miscibility

The process of liquids mixing together in all proportions to form a homogeneous solution.

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Charge-to-Size Ratio

The ratio of charge to the size of an ion.

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Entropy

A measure of the disorder or randomness of a system. It is related to the number of possible arrangements of particles in a system. Higher entropy indicates greater disorder.

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