Questions and Answers
What represents a chemical reaction?
What do necessary conditions in a chemical equation indicate?
Conditions such as heat, catalysts, or a spark.
Matter can be created or destroyed in a chemical reaction.
False
What are stoichiometric coefficients?
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In a chemical equation, reactants are on the ______ of the arrow.
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Which of the following is NOT a class of chemical reactions?
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What is the general form of an acid-base neutralization reaction?
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Reduction involves the loss of electrons.
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What is the general form of a combustion reaction?
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What do net ionic equations represent?
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Which of the following statements about solubility is true?
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Study Notes
Chemical Equations
- A chemical equation symbolizes a reaction, showing reactants on the left and products on the right.
- Example: Hydrogen + Oxygen → Water.
Necessary Conditions
- Conditions like heat, catalysts, or a spark are noted above the reaction arrow.
Law of Conservation of Mass
- Matter is not created or destroyed during chemical reactions; atoms are merely rearranged.
Stoichiometry
- The study of relationships between reactant quantities in chemical reactions.
Stoichiometric Coefficients
- Numeric prefixes used in balanced chemical equations represent the amount of substances involved.
Balancing Chemical Equations
- Start with an unbalanced equation, ensuring correct formulas for all substances.
- Begin balancing with unique elements, leaving pure elements until the end, and treat polyatomic ions as whole units.
Classes of Chemical Reactions
- Types include:
- Precipitation reactions (formation of solids)
- Acid-base neutralization reactions
- Oxidation-reduction (redox) reactions (electron transfer)
- Combustion reactions
Precipitation Reactions
- Typically double displacement reactions, following the general pattern: AB + CD → AD + CB.
Precipitation and Solubility Guidelines
- Solubility refers to how much of a compound dissolves in a solvent at a specific temperature.
- Compounds that dissolve significantly are labeled (aq) for aqueous, while insoluble ones marked (s) indicate solids.
Acids, Bases, and Neutralization Reactions
- General Reaction Format: HA + MOH → H2O + MA (Acid + Base → Water + Salt).
- Bases can include hydroxides and others like NH3.
Redox Reactions
- Involves the transfer of electrons, according to oxidation and reduction processes.
Oxidation
- Defined by the loss of electrons.
Reduction
- Characterized by the gain of electrons.
Oxidizing Agent
- A substance that oxidizes another and gets reduced in the process.
Reducing Agent
- Reduces another substance while itself being oxidized, identifiable on the reactant side.
Single Replacement Reactions
- Example: Fe(s) + Cu^2+(aq) → Fe^2+(aq) + Cu(s) showcasing redox behavior.
Combustion Reaction
- General format: Fuel + O2 → CO2 + H2O.
Recognizing Redox
- Requires a bookkeeping system to track electron transfer, using oxidation numbers (not true charges).
Activity Series
- A prediction tool for element reactivity, indicating which element prefers to be a cation.
Driving Forces for Reactions
- Reactions occur due to:
- Formation of a precipitate
- Gas formation
- Formation of molecular compounds (e.g., H2O)
- Generation of weak acids or bases
- Redox processes
Net Ionic Equations
- Focus on the components that dissociate in solution.
Components That Break Apart (NET)
- Soluble salts, strong acids (e.g., HCl, HBr), and strong bases (e.g., Group 1 hydroxides).
Components That Stay Together
- Includes solids, liquids, gases, weak acids/bases, and insoluble salts.
Solubility Rules
- Salts of Li+, Na+, K+, Rb+, Cs+, and NH4+ are always soluble.
- Nitrates (NO3-), acetates (C2H3O2-), and chlorates (ClO3-) are also generally soluble.
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Description
Test your knowledge with these flashcards focused on the classification and balancing of chemical reactions from Chapter 5. Each card features key terms and their definitions, allowing you to reinforce your understanding of chemical equations and necessary conditions for reactions.
