Questions and Answers
What is the term for a substance that is capable of being dissolved?
What is a homogeneous mixture of two or more substances in a single phase called?
solution
The dissolving medium in a solution is called the ___
solvent
The substance dissolved in a solution is called the ___
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If particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated, the mixture is called a ___
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Particles that are intermediate in size between those in solutions and suspensions form mixtures known as ___
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What happens when an ionic compound dissolves?
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Solutions that can conduct electric current are known as ____
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What are three ways to increase the rate of dissolution?
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What governs solubility?
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What are the types of intermolecular forces?
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Non-polar molecules dissolve in ___ solvents
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Polar molecules dissolve ___ and ___
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Two liquids that dissolve in each other are called ___
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Two liquids that do not dissolve into each other are called ___
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The solubility of a gas in a liquid is ____ proportional to the partial pressure of that gas on the surface of the liquid.
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What is the rapid escape of a gas from a liquid in which it is dissolved called?
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The solubility of gases in water usually ___ with ___ temperature.
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A ___ is heat that can either be released or absorbed when a compound is dissolved.
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What is the net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent called?
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What is amount of solute dissolved per a given amount of solvent known as?
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In the chemistry world, the most common unit of concentration is _()
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What is the concentration of a solution expressed in moles of solute per kilogram of solvent?
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What are characteristics of ionic compounds?
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What are characteristics of covalent compounds?
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What are electrostatic interactions?
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What are the three types of compounds?
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Anions are __ or __
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__ can change state
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Molecules means ___
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Two solutes, ionic salt, polar molecule, are called ___
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One solute, nonpolar molecule is called ___
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What are some examples of polar covalent molecules?
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What are some examples of non-polar covalent molecules?
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In enthalpy of solution, a solution gets colder, energy is a reactant required/absorbed, 'take', is classified as ___
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In enthalpy of solution, a solution gets warmer, energy is a product or released, 'make', is classified as ___
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What are the three steps to dissolve?
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What are strong electrolytes?
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What is considered a weak electrolyte?
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What produces ions when dissolved?
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What allows solutions to conduct electric current?
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When dissolving gases in water, you should __ pressure and __ in temperature.
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What are the three steps to make a molarity solution?
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What is the density of water?
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You don't need a volumetric flask in ___
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What are the three steps to make a molality solution?
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Study Notes
Solutions and Mixtures
- Soluble: Capable of being dissolved.
- Solution: A homogeneous mixture of two or more substances in a single phase.
- Solvent: The dissolving medium in a solution.
- Solute: The substance dissolved in a solution.
- Suspension: Mixture with large particles that settle unless stirred.
- Colloids: Intermediate-sized particles between solutions and suspensions.
Properties of Solutions
- Electrolytes: Solutions that can conduct electric current.
- Increasing dissolution rate: Achieved by increasing surface area, agitating the solution, or heating it.
Molecular Interactions
- Intermolecular forces: Attractions between molecules that influence solubility.
- Intramolecular forces: Attractions within a molecule, such as covalent bonds.
- Types of intermolecular forces: Ion-dipole, dipole-dipole, hydrogen bonding, and London dispersion forces.
Solubility Concepts
- Polar molecules dissolve in polar solvents and ionic compounds.
- Non-polar molecules dissolve in non-polar solvents.
- Miscible: Two liquids that dissolve in each other.
- Immiscible: Two liquids that do not dissolve into each other.
- Gas solubility in liquids is directly proportional to the gas's partial pressure.
Thermodynamics of Solutions
- Effervescence: Rapid escape of gas from a liquid.
- Gas solubility decreases with increasing temperature.
- Enthalpy: Heat absorbed or released during dissolution.
- Enthalpy of solution: Net energy absorbed by the solution when a solute dissolves.
Concentration Metrics
- Concentration: Amount of solute per given solvent.
- Molarity (M): Common concentration unit expressed as moles of solute per liter of solution.
- Molality: Concentration expressed in moles of solute per kilogram of solvent.
Compound Characteristics
- Ionic compounds: Typically involve electron transfer, have high electronegativity (>1.7), and form crystals.
- Covalent compounds: Involve electron sharing, have lower electronegativity (<1.7), and primarily consist of nonmetals.
Types of Compounds
- Types include ionic salts, polar covalent molecules, and non-polar covalent molecules.
- Anions can be single elements or polyatomic ions.
- Molecules can change state and are defined by covalent bonding.
Solution Preparation
- Process of dissolving involves breaking solute and solvent interactions, followed by forming solute-solvent interactions.
- Strong electrolytes include ionic salts; weak electrolytes generally refer to acids.
- Steps to prepare molarity solutions: Mass out moles, place in a volumetric flask, and add solvent to the mark.
- Density of water is 1 kg/L; molality preparation does not require volumetric flasks.
Overall Summary
- Important principles of solubility, thermodynamics, and preparation of solutions; distinctions between electrolytes, types of molecular interactions, and methods to calculate concentration are foundational in chemistry.
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Description
Test your understanding of key terms from Chemistry Chapter 12. This quiz covers important concepts such as solutions, solutes, and solvents. Use these flashcards to reinforce your knowledge and prepare for your chemistry exams.
