Questions and Answers
What is defined as the amount of substance containing as many particles as there are atoms in 12g of ¹²C?
Which term refers to a substance that dissociates in solution to produce hydrogen ions?
What is the term for the minimum energy required for a reaction to take place?
Which process describes when the product of a reaction also serves as a catalyst for that same reaction?
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Which type of isotope has the same atomic number but different mass numbers?
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What defines the time taken for half of the atoms in a sample of an isotope to decay?
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What is the term for the average mass of an atom of an element relative to 1/12 the mass of a Carbon-12 atom?
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Which type of catalysis involves a catalyst in a different physical phase than the reactants?
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What is a characteristic of structural isomers?
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Which of the following describes a primary alcohol?
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What does Hess's Law state about chemical reactions?
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Which statement best defines an endothermic reaction?
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What does the octane number indicate about a fuel?
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What is the heat of combustion of a substance?
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What is the law of conservation of energy?
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What is bond energy?
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What is hydrolysis?
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What does Le Chatelier’s Principle state?
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What is the dissociation constant of water (Kᵥᵥ)?
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Which type of water is characterized by the inability to easily form lather with soap?
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How is the pH of a solution defined?
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What does biochemical oxygen demand (BOD) indicate?
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What is the process of electrolysis primarily used for?
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What defines an inert electrode?
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Which statement accurately describes reduction in terms of oxidation number?
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How does Gay-Lussac’s Law relate to gas reactions?
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What characterizes an ideal gas?
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What does the empirical formula of a compound indicate?
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Which law states that, at constant temperature, the volume of a gas is inversely proportional to its pressure?
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What characteristic defines a volatile liquid?
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What defines an atomic orbital?
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Which of the following best describes electronegativity?
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Which statement about ionization energy is correct?
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What is true about a covalent bond?
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How is the atomic radius of an element determined?
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What does the Heisenberg’s Uncertainty Principle state?
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Which of the following defines a reducing agent?
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What characterizes dipole-dipole interactions?
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What does hydrolysis involve in its process?
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Which principle states that a system at equilibrium will adjust to minimize stress?
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What defines the pH of a solution?
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What is indicated by a high Biochemical Oxygen Demand (BOD)?
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Which term refers to hardness in water that can be removed by boiling?
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What is flocculation in the context of water treatment?
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Permanent hardness in water requires what type of treatment?
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Which expression correctly defines the nature of a reversible reaction?
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Study Notes
Gas Laws and Concepts
- Avogadro’s Law: Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
- Boyle’s Law: At constant temperature, the volume of a gas is inversely proportional to its pressure.
- Charles’ Law: At constant pressure, the volume of a gas is directly proportional to its Kelvin temperature.
- Gay-Lussac’s Law: Volumes of gases in reactions bear simple whole number ratios when measured under identical conditions.
Chemical Terms and Definitions
- Mole: Amount of a substance that contains as many particles as there are atoms in 12g of carbon-12.
- Primary Standard: Stable, water-soluble substance available in pure form.
- Standard Solution: A solution with an accurately known concentration.
Acids and Bases
- Arrhenius Acid: Dissociates in solution to form hydrogen ions.
- Arrhenius Base: Dissociates in solution to form hydroxide ions.
- Bronsted-Lowry Acid: Proton donor.
- Bronsted-Lowry Base: Proton acceptor.
- Conjugate Acid-Base Pairs: Differ by presence or absence of a proton.
Reaction Dynamics
- Activation Energy: Minimum energy needed for a reaction to occur.
- Catalyst: Substance that alters reaction rate without being consumed.
- Autocatalysis: Reaction product acts as a catalyst.
- Effective Collision: Collision with sufficient energy that results in product formation.
Particle and Atomic Concepts
- Isotopes: Elements with the same atomic number but different mass numbers.
- Atomic Number: Number of protons in an atom's nucleus.
- Mass Number: Sum of protons and neutrons in the nucleus.
- Relative Atomic Mass: Average mass relative to 1/12 of a carbon-12 atom.
Chemical Bonding
- Covalent Bond: Formed by sharing pairs of electrons between nonmetals.
- Ionic Bond: Electrostatic attraction between oppositely charged ions.
- Electronegativity: An atom’s attraction for shared electrons in a covalent bond.
Energy and Thermodynamics
- Endothermic Reaction: Reaction that absorbs heat.
- Exothermic Reaction: Reaction that releases heat.
- Heat of Combustion: Heat change when one mole of a substance is burned in excess oxygen.
- Hess’s Law: Total heat change is independent of the number of steps in a reaction process.
Solution Properties
- Electrolyte: Conducts electricity when dissolved in water or molten.
- Hard Water: Does not easily form lather with soap.
- Soft Water: Easily forms lather with soap.
Reaction Types
- Oxidation: Loss of electrons (OIL - oxidation is loss).
- Reduction: Gain of electrons (RIG - reduction is gain).
- Reversible Reaction: Can proceed in both directions.
Equilibria
- Chemical Equilibrium: Rate of forward reaction equals rate of reverse reaction.
- Le Chatelier’s Principle: System shifts to minimize the effect of stress applied to it.
Additional Concepts
- Hydrolysis: Decomposition by water.
- Volatile Liquid: Easily evaporates, characterized by lower boiling points.
- Empirical Formula: Simplest whole number ratio of elements in a compound.
- Molecular Formula: Actual number of atoms of each element in a compound.
Environmental and Biological Factors
- Biochemical Oxygen Demand (BOD): Measure of dissolved oxygen consumed by biological action over five days at 20°C in the dark.
Gas Laws and Concepts
- Avogadro’s Law: Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
- Boyle’s Law: At constant temperature, the volume of a gas is inversely proportional to its pressure.
- Charles’ Law: At constant pressure, the volume of a gas is directly proportional to its Kelvin temperature.
- Gay-Lussac’s Law: Volumes of gases in reactions bear simple whole number ratios when measured under identical conditions.
Chemical Terms and Definitions
- Mole: Amount of a substance that contains as many particles as there are atoms in 12g of carbon-12.
- Primary Standard: Stable, water-soluble substance available in pure form.
- Standard Solution: A solution with an accurately known concentration.
Acids and Bases
- Arrhenius Acid: Dissociates in solution to form hydrogen ions.
- Arrhenius Base: Dissociates in solution to form hydroxide ions.
- Bronsted-Lowry Acid: Proton donor.
- Bronsted-Lowry Base: Proton acceptor.
- Conjugate Acid-Base Pairs: Differ by presence or absence of a proton.
Reaction Dynamics
- Activation Energy: Minimum energy needed for a reaction to occur.
- Catalyst: Substance that alters reaction rate without being consumed.
- Autocatalysis: Reaction product acts as a catalyst.
- Effective Collision: Collision with sufficient energy that results in product formation.
Particle and Atomic Concepts
- Isotopes: Elements with the same atomic number but different mass numbers.
- Atomic Number: Number of protons in an atom's nucleus.
- Mass Number: Sum of protons and neutrons in the nucleus.
- Relative Atomic Mass: Average mass relative to 1/12 of a carbon-12 atom.
Chemical Bonding
- Covalent Bond: Formed by sharing pairs of electrons between nonmetals.
- Ionic Bond: Electrostatic attraction between oppositely charged ions.
- Electronegativity: An atom’s attraction for shared electrons in a covalent bond.
Energy and Thermodynamics
- Endothermic Reaction: Reaction that absorbs heat.
- Exothermic Reaction: Reaction that releases heat.
- Heat of Combustion: Heat change when one mole of a substance is burned in excess oxygen.
- Hess’s Law: Total heat change is independent of the number of steps in a reaction process.
Solution Properties
- Electrolyte: Conducts electricity when dissolved in water or molten.
- Hard Water: Does not easily form lather with soap.
- Soft Water: Easily forms lather with soap.
Reaction Types
- Oxidation: Loss of electrons (OIL - oxidation is loss).
- Reduction: Gain of electrons (RIG - reduction is gain).
- Reversible Reaction: Can proceed in both directions.
Equilibria
- Chemical Equilibrium: Rate of forward reaction equals rate of reverse reaction.
- Le Chatelier’s Principle: System shifts to minimize the effect of stress applied to it.
Additional Concepts
- Hydrolysis: Decomposition by water.
- Volatile Liquid: Easily evaporates, characterized by lower boiling points.
- Empirical Formula: Simplest whole number ratio of elements in a compound.
- Molecular Formula: Actual number of atoms of each element in a compound.
Environmental and Biological Factors
- Biochemical Oxygen Demand (BOD): Measure of dissolved oxygen consumed by biological action over five days at 20°C in the dark.
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Description
This quiz covers key concepts in chemistry, including hydrolysis, chemical equilibrium, and reversible reactions. Understand Le Chatelier’s Principle and the dissociation constant of water as you test your knowledge on these important topics.
