General Chemistry 2 - First Semester (1st Quarter)

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Questions and Answers

Which of the following is NOT one of the four types of intermolecular forces?

  • Dipole-dipole forces
  • Covalent forces (correct)
  • Ion-dipole forces
  • London dispersion forces

Which type of intermolecular force is responsible for the attraction between polar molecules?

  • London dispersion forces
  • Dipole-dipole forces (correct)
  • Hydrogen bonds
  • Ion-dipole forces

Which type of intermolecular force involves the attraction between polar molecules and ions?

  • Ion-dipole forces (correct)
  • London dispersion forces
  • Hydrogen bonds
  • Dipole-dipole forces

Which type of intermolecular force is a special type of dipole-dipole force involving hydrogen and either nitrogen, oxygen, or fluorine?

<p>Hydrogen bonds (D)</p> Signup and view all the answers

Which type of bonding involves the sharing of electrons between a nonmetal and nonmetal?

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

Which of the following is NOT one of the four types of intermolecular forces?

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

Which type of intermolecular force is responsible for the attraction between polar molecules?

<p>Dipole-dipole forces (A)</p> Signup and view all the answers

Which type of intermolecular force involves the attraction between polar molecules and ions?

<p>Ion-dipole forces (D)</p> Signup and view all the answers

Which of the following is NOT a type of intermolecular force?

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

Which of the following compounds is likely to exhibit hydrogen bonding?

<p>H₂O (B)</p> Signup and view all the answers

What determines a matter's characteristics?

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

Which of the following is a physical property of liquids?

<p>Surface tension (C)</p> Signup and view all the answers

What is the purpose of determining the melting point of a solid substance?

<p>To identify the substance (A)</p> Signup and view all the answers

Which type of crystal is held together by metallic bonds?

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

What physical property can help distinguish a crystalline from an amorphous solid?

<p>Regular repeating pattern (C)</p> Signup and view all the answers

What forces bind the structure units in ionic crystals?

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

Which of the following is NOT a physical property of liquids?

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

What determines the melting point of a solid substance?

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

Which type of crystal is held together by covalent network bonds?

<p>Covalent network crystals (B)</p> Signup and view all the answers

Which of the following is a physical property of liquids?

<p>Surface tension (C)</p> Signup and view all the answers

What determines the melting point of a solid substance?

<p>Intermolecular forces (C)</p> Signup and view all the answers

What physical property can help distinguish a crystalline from an amorphous solid?

<p>Long-range order (D)</p> Signup and view all the answers

Which of the following statements about solubility is correct?

<p>Solubility refers to the maximum quantity of solute that can be dissolved in a given quantity of solvent at a given temperature. (D)</p> Signup and view all the answers

Which of the following is true about phase changes?

<p>Phase changes involve the absorption and release of heat energy. (A)</p> Signup and view all the answers

What is the triple point?

<p>The intersection of the liquid-vapor and solid-liquid curves on a phase diagram. (D)</p> Signup and view all the answers

How does temperature affect solubility?

<p>Increasing temperature generally increases solubility for most substances. (B)</p> Signup and view all the answers

What is the purpose of determining the melting point of a solid substance?

<p>To identify the substance. (A)</p> Signup and view all the answers

During hot days, fish stay at the deeper cooler part of a body of water. Can you explain this behavior using what you know about the solubility of gas?

<p>Fish stay at the deeper cooler part of a body of water because the solubility of gas decreases with increasing temperature. (C)</p> Signup and view all the answers

How would you convince people that using compressors to breathe under mine shafts and during deep-sea diving is dangerous?

<p>Using compressors to breathe under mine shafts and during deep-sea diving is dangerous because it increases the pressure of the gas, leading to decompression sickness. (C)</p> Signup and view all the answers

Explain why sugar crystals form on a string when a hot sugar solution is left to cool to room temperature.

<p>Sugar crystals form on a string when a hot sugar solution is left to cool to room temperature because the solubility of sugar decreases with decreasing temperature. (A)</p> Signup and view all the answers

According to the text, what is the molar concentration of molecules in a mountain at a temperature of 25°C?

<p>2.4 mol/L (B)</p> Signup and view all the answers

Based on the text, what is the molar concentration constant of oxygen at a temperature of 25°C?

<p>1.3x10⁻³ mol/L atm (D)</p> Signup and view all the answers

According to the text, what are the two substances involved in the solution process?

<p>Paint thinner and water (B)</p> Signup and view all the answers

Which set of concentration readings showed a discrepancy: the concentration readings expressed in molarity or the concentration readings expressed in molality?

<p>The concentration readings expressed in molarity (D)</p> Signup and view all the answers

Which expression of concentration uses the number of moles of solute per liter of solution?

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

Which expression of concentration uses the number of moles of solute per 1000 g or 1 kg of solvent?

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

What can be used to determine the concentration of a solution?

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

At the end of titration, what is equal?

<p>The number of moles of the reactants (D)</p> Signup and view all the answers

Which expression of concentration uses the number of moles of solute per liter of solution?

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

What is the difference between molarity and molality?

<p>Molarity is expressed in terms of moles of solute per liter of solution, while molality is expressed in terms of moles of solute per 1000 g or 1 kg of solvent. (C)</p> Signup and view all the answers

Which set of concentration reading was not equal when compared: the concentration readings expressed in molarity or the concentration readings expressed in molality?

<p>Concentration readings expressed in molality (B)</p> Signup and view all the answers

Which expression of concentration uses the number of moles of solute per liter of solution?

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

What is the difference between molarity and molality?

<p>Molarity is expressed in moles per liter of solvent, while molality is expressed in moles per 1000 grams of solvent. (A)</p> Signup and view all the answers

Which set of concentration readings showed a discrepancy: the concentration readings expressed in molarity or the concentration readings expressed in molality?

<p>Both sets of concentration readings showed a discrepancy (D)</p> Signup and view all the answers

According to Raoult’s law, how is the vapor pressure of a solution affected by the amount of solute?

<p>The vapor pressure decreases with the amount of solute. (D)</p> Signup and view all the answers

How are the freezing point and boiling point of a solution affected by the solute?

<p>The freezing point is elevated and the boiling point is lowered. (C)</p> Signup and view all the answers

What is osmosis?

<p>The process in which the solvent moves through a semi-permeable membrane from a lower concentration of solute to a higher concentration. (A)</p> Signup and view all the answers

What is equilibrium in osmosis?

<p>Equilibrium is established if the concentration is equal. (C)</p> Signup and view all the answers

What is osmotic pressure?

<p>The pressure exerted by the solute on the solvent in osmosis. (B)</p> Signup and view all the answers

According to Raoult’s law, how are the freezing point and boiling point of the solution affected by the solute?

<p>The freezing point is lowered and the boiling point is elevated. (D)</p> Signup and view all the answers

According to Raoult’s law, how are the freezing point and boiling point of the solution affected by the solute?

<p>The freezing point is lowered and the boiling point is elevated (A)</p> Signup and view all the answers

What is osmosis?

<p>The movement of solvent through a semi-permeable membrane (A)</p> Signup and view all the answers

What is osmotic pressure?

<p>The pressure exerted by the solute on the solvent (A)</p> Signup and view all the answers

Which of the following is true about thermochemical equations?

<p>They are balanced chemical equations that include the enthalpy change (D)</p> Signup and view all the answers

What is the purpose of writing thermochemical equations?

<p>To represent the enthalpy change of a chemical reaction (B)</p> Signup and view all the answers

What does the enthalpy change in a thermochemical equation represent?

<p>The heat energy absorbed or released during a chemical reaction (C)</p> Signup and view all the answers

How are thermochemical equations different from regular balanced chemical equations?

<p>Thermochemical equations include the enthalpy change (C)</p> Signup and view all the answers

What is the significance of the enthalpy change in a thermochemical equation?

<p>It indicates the direction and magnitude of the heat flow during a chemical reaction (A)</p> Signup and view all the answers

Which of the following is true about thermochemical equations?

<p>Thermochemical equations represent the enthalpy change of a chemical reaction. (B)</p> Signup and view all the answers

According to the text, what are the two substances involved in the solution process?

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

Which set of concentration readings showed a discrepancy: the concentration readings expressed in molarity or the concentration readings expressed in molality?

<p>The concentration readings expressed in molarity (C)</p> Signup and view all the answers

Which of the following is NOT a characteristic of thermochemical equations?

<p>They represent the physical states of reactants and products (C)</p> Signup and view all the answers

According to the text, what is the purpose of writing thermochemical equations?

<p>To show the molar ratios of reactants and products (B)</p> Signup and view all the answers

According to Raoult’s law, how are the boiling point and freezing point of the solution affected by the solute?

<p>The boiling point decreases and the freezing point increases (A)</p> Signup and view all the answers

Flashcards

Intermolecular Forces

Attractive forces between molecules

Dipole-Dipole Forces

Attraction between polar molecules

Hydrogen Bonding

Strong dipole-dipole force in molecules with H, N, O, or F

London Dispersion Forces

Weak forces between all molecules due to temporary dipoles

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Ion-Dipole Forces

Attraction between ions and polar molecules

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Covalent Bonding

Sharing of electrons between nonmetals

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Ionic Bonding

Electrostatic attraction between ions

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Viscosity

Liquid's resistance to flow

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Surface Tension

Force holding liquid surface together

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Crystalline Solid

Solid with well-organized structure

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Amorphous Solid

Solid with no ordered structure

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Solubility

Ability of one substance to dissolve in another

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Triple Point

Temperature and pressure where solid, liquid, and gas phases coexist

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Molarity

Moles of solute per liter of solution

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Molality

Moles of solute per 1000g of solvent

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Titration Endpoint

Point where moles of acid equals moles of base

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Raoult's Law

Vapor pressure of a solution depends on solute concentration

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Osmosis

Solvent movement through a membrane

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Melting Point

Temperature where a solid turns into a liquid

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Freezing Point

Temperature where a liquid turns into a solid

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Boiling Point

Temperature where a liquid turns into a gas

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Thermochemical Equation

Chemical equation with the enthalpy change

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Study Notes

Intermolecular Forces

  • Four types of intermolecular forces include dipole-dipole, hydrogen bonding, London dispersion forces, and ion-dipole forces.
  • Dipole-dipole forces are responsible for attraction between polar molecules.
  • Ion-dipole forces occur between polar molecules and ions.
  • Hydrogen bonding is a special dipole-dipole interaction involving hydrogen and nitrogen, oxygen, or fluorine.

Types of Bonding

  • Covalent bonding involves sharing electrons, typically between nonmetals.
  • Ionic bonds result from the electrostatic attraction between ions.

Properties of Liquids and Solvents

  • Physical properties of liquids include viscosity, surface tension, and density.
  • Melting point determination is important for identifying a solid substance.
  • The crystalline structure is distinct from amorphous solids, often characterized by sharp melting points.

Crystalline and Amorphous Solids

  • Crystalline solids have well-defined geometric arrangements, while amorphous solids lack such structure.
  • Forces in ionic crystals are held together by strong ionic bonds.
  • Covalent network solids are held by extensive covalent bonds throughout the structure.

Solubility and Phase Changes

  • Solubility is impacted by temperature; generally, higher temperatures increase gas solubility in liquids.
  • The triple point refers to the temperature and pressure at which a substance can coexist in solid, liquid, and gas phases.
  • Phase changes involve transitions such as melting, freezing, and boiling.

Concentration and Titration

  • Molarity is expressed in moles of solute per liter of solution, whereas molality is moles of solute per 1000 g of solvent.
  • Discrepancies may arise between molarity and molality readings during experiments.
  • At the endpoint of a titration, the moles of acid equal the moles of base.

Raoult's Law

  • Raoult’s law states that the vapor pressure of a solution is directly affected by the concentration of solute.
  • Adding a solute generally lowers the freezing point and raises the boiling point of the solvent.

Osmosis and Equilibrium

  • Osmosis is the movement of solvent molecules through a semi-permeable membrane from a less concentrated to a more concentrated solution.
  • Osmotic pressure is the pressure required to stop the osmotic flow of solvent.
  • Equilibrium in osmosis occurs when the rate of solute movement is equal in both directions across the membrane.

Thermochemical Equations

  • Thermochemical equations indicate energy changes, specifically enthalpy changes during chemical reactions.
  • These equations differ from regular balanced equations because they include the heat exchange associated with the reaction.
  • Writing thermochemical equations helps to understand energy changes during chemical processes.

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