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Questions and Answers

Which of the following observations suggest that a chemical reaction has taken place? (Select all that apply)

  • Production of a gas (correct)
  • Color change (correct)
  • Evolution of energy as heat and light (correct)
  • Formation of a precipitate (correct)

    • List three requirements for a correctly written chemical equation.

    1. The equation must represent known facts. 2. The equation must contain the correct formulas for the reactants and products. 3. The law of conservation of mass must be satisfied.

    Write a word equation and a formula equation for the reaction of solid sodium oxide with water to form sodium hydroxide.

    Word equation: sodium oxide + water ⎯→ sodium hydroxide; Formula equation: Na2O(s) + H2O(l) ⎯→ 2NaOH(aq)

    List three types of synthesis reactions.

    <ol> <li>Reactions of elements with oxygen and sulfur 2. Reactions of metals with halogens 3. Synthesis reactions with oxides</li> </ol> Signup and view all the answers

    List five types of decomposition reactions.

    <ol> <li>Decomposition of binary compounds 2. Metal carbonates 3. Metal hydroxides 4. Metal chlorates 5. Acids</li> </ol> Signup and view all the answers

    List four types of single-replacement reactions.

    <ol> <li>Replacement of a metal in a compound by another metal 2. Replacement of hydrogen in water by a metal 3. Replacement of hydrogen in an acid by a metal 4. Replacement of halogens</li> </ol> Signup and view all the answers

    List three types of double-replacement reactions.

    <ol> <li>Formation of a precipitate 2. Formation of a gas 3. Formation of water</li> </ol> Signup and view all the answers

    Explain the significance of an activity series.

    <p>The more active the element, the higher up on the activity list they are. Elements lower than others on the activity series cannot replace other elements in a single-replacement reaction.</p> Signup and view all the answers

    What is a combustion reaction?

    <p>A reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat.</p> Signup and view all the answers

    What is a decomposition reaction?

    <p>A reaction in which a single compound produces two or more simpler substances.</p> Signup and view all the answers

    What is a displacement reaction?

    <p>A reaction in which one element replaces a similar element in a compound.</p> Signup and view all the answers

    What is a double-replacement reaction?

    <p>A reaction in which the ions of two compounds exchange places in an aqueous solution to form two new compounds.</p> Signup and view all the answers

    What is electrolysis?

    <p>The decomposition of a substance by an electric current.</p> Signup and view all the answers

    What is a precipitate?

    <p>A solid that is produced as a result of a chemical reaction in solution and that separates from the solution.</p> Signup and view all the answers

    What is a reversible reaction?

    <p>A chemical reaction in which the products re-form the original reactants.</p> Signup and view all the answers

    What is a single-replacement reaction?

    <p>A reaction in which one element replaces a similar element in a compound.</p> Signup and view all the answers

    What is a synthesis reaction?

    <p>A reaction in which two or more substances combine to form a new compound.</p> Signup and view all the answers

    Knowledge about what products are produced in a chemical reaction is obtained by?

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

    To balance a chemical equation, it may be necessary to adjust the?

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

    A chemical equation is balanced when the?

    <p>Same number of each kind of atom appears in the reactants and in the products (C)</p> Signup and view all the answers

    When the equation Fe3O4 + Al → Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?

    <p>9 (D)</p> Signup and view all the answers

    The reaction 2Mg(s) + O2(g) → 2MgO(s) is a?

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

    The reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is a?

    <p>Single-replacement reaction (A)</p> Signup and view all the answers

    The reaction 2HgO(s) → 2Hg(l) + O2(g) is a(n)?

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

    The reaction Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) is a?

    <p>Double-replacement reaction (D)</p> Signup and view all the answers

    The decomposition of a substance by an electric current is called?

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

    When heated, a metal carbonate decomposes into a metal oxide and?

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

    An active metal and a halogen react to form a(n)?

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

    If chlorine gas is produced by halogen replacement, the other halogen in the reaction must be?

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

    An element in the activity series can replace any element?

    <p>Below it on the list (D)</p> Signup and view all the answers

    Predict what happens when lead is added to nitric acid.

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

    Study Notes

    Observations of Chemical Reactions

    • Energy can be released during a reaction in forms such as heat and light.
    • The production of gas is a common indication of a chemical reaction.
    • Formation of a precipitate signals a transformation in the solution.
    • A noticeable color change often accompanies a chemical reaction.

    Requirements for Chemical Equations

    • Must accurately represent known facts regarding the reaction.
    • Correct formulas for all reactants and products are necessary.
    • Must adhere to the law of conservation of mass.

    Writing Chemical Equations

    • A word equation expresses reactants and products in descriptive terms.
    • Example: Sodium oxide + Water ⎯→ Sodium hydroxide.
    • A formula equation uses chemical symbols, e.g., Na2O(s) + H2O(l) ⎯→ 2NaOH(aq).

    Types of Reactions

    • Synthesis Reactions: Include reactions with oxygen/sulfur, metal and halogen combinations, and oxides.
    • Decomposition Reactions: Types involve binary compounds, metal carbonates, hydroxides, chlorates, and acids.
    • Single-Replacement Reactions: Involve a metal displacing another metal, hydrogen replacement in water or acids, and halogen substitutions.
    • Double-Replacement Reactions: Result in products such as precipitates, gases, or water.

    Activity Series Significance

    • Elements higher on an activity series can replace those below them in reactions.
    • This series helps predict the occurrence of single-replacement reactions based on the activity level of elements.

    Definitions of Reaction Types

    • Combustion Reaction: Substance combines with oxygen, releasing energy as light and heat.
    • Decomposition Reaction: A single compound breaks down into simpler substances.
    • Displacement Reaction: One element replaces a similar element in a compound.
    • Double-Replacement Reaction: Ions from two compounds exchange positions to form new compounds.
    • Electrolysis: Decomposition caused by passing an electric current through a substance.
    • Precipitate: A solid formed from a solution during a chemical reaction.
    • Reversible Reaction: Reactants can reform from products in chemical reactions.

    Balancing Chemical Equations

    • Coefficients can be adjusted to achieve balance in a chemical equation.
    • A balanced equation has the same number of each type of atom on both sides.

    Specific Reaction Types

    • Synthesis Example: 2Mg(s) + O2(g) ⎯→ 2MgO(s).
    • Single-Replacement Example: Mg(s) + 2HCl(aq) ⎯→ H2(g) + MgCl2(aq).
    • Decomposition Example: 2HgO(s) ⎯→ 2Hg(l) + O2(g).
    • Double-Replacement Example: Pb(NO3)2(aq) + 2KI(aq) ⎯→ PbI2(s) + 2KNO3(aq).

    Metal and Halogen Reactions

    • Metal carbonates decompose into metal oxides and carbon dioxide upon heating.
    • Active metals react with halogens to form salts; the most active halogen can be determined.

    Predictive Outcomes of Reactions

    • Lead reacts with nitric acid producing hydrogen gas.
    • Elements in an activity series can replace those below them, influencing reaction outcomes and product formation.

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