This document summarizes different types of chemical reactions and equations. It describes reactants and products, chemical equations, and indicators of chemical reactions like heat evolution and color changes. It also discusses balancing chemical equations, types of reactions like synthesis, decomposition, and displacement reactions, and using activity series to predict reaction outcomes.

1. Chemical Equations and Reactions Chapter 8

2. Describing Chemical Reactions Chemical reaction the process by which one or more substances are changed into one or more different substances Reactants the original substances Products the resulting substances Chemical Equation an equation that represents, with symbols and formulas, the identities and relative amounts of the reactants and products in a chemical reaction

3. Indications of A Chemical Reaction Evolution of heat and light Production of a gas Formation of a precipitate Precipitate – a solid that is produced as a result of a chemical reaction in solution and that separates from the solution Color change

4. Characteristics of Chemical Equations The equation must represent known facts The equation must contain the correct formulas for the reactants and products The law of conservation of mass must be satisfied Coefficient – a small whole number that appears in front of a formula in a chemical equation.

5. Word Equation – an equation in which the reactants and products in a chemical reaction are represented by words. Ex. methane + oxygen  carbon dioxide + water means yield Formula Equation – represents the reactants and products of a chemical reaction by their symbols or formulas. Ex. CH4(g) + O2(g)  CO2(g) + H2O(g) (unbalanced)

6. Significance of a Chemical Equation The coefficients of a chemical reaction indicate relative, not absolute, amounts of reactants and products. The relative masses of the reactants and products of a chemical reaction can be determined from the reaction’s coefficients. The reverse reaction for a chemical equation has the same relative amounts of substances as the forward reaction.

7. 4 1 1 2 2 1 2 4 1 2 4 2 1 2 4 1 2 4 2 1 4 Balancing Equations CH4(g) + O2(g)  CO2(g) + H2O(g) CH4(g) + O2(g)  CO2(g) + 2H2O(g) CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

8. Types of Chemical Reactions Synthesis reaction (composition reaction) – a reaction where two or more substances combine to form a new compound. A + X  AX where A and X are elements of compounds Ex. 2Mg(s) + O2(g) 2MgO(s)

9. Reactions of Metals with Halogens M + X  MX where M is a metal and X is a halogen. Ex. 2Na(s) + Cl2(g) 2NaCl(s)

10. Decomposition Reactions Decomposition reaction – a single reaction that undergoes a reaction that produces two or more simpler substances. AX  A + X where AX is the compound and A and X are the simpler elements or compounds Ex. 2H2O(l) 2H2(g) + O2(g) Electrolysis – the decomposition of a substance by an electric current. electricity

11. Δ Δ 2HgO(s) 2Hg(l) + O2(g) The means heat is needed to make the reaction happen

12. Single Replacement Reaction (displacement) a reaction where one element replaces a similar element in a compound. A + BX  AX + B where A, B, and X are elements and AX and BX are compounds Ex. 2Al(s) + 3Pb(NO3)2(aq)  3Pb(s) + 2Al(NO3)3(aq)

13. Double-Replacement Reaction Double-Replacement reactions – a reaction where the ions of two compounds exchange places in an aqueous solution to form a new compound. AX + BY  AY + BX where A, B, X, and Y represent ions and AY and BX represent ionic or molecular compounds Ex. 2KI(aq) + Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq)

14. Combustion reaction – a reaction where a substance combines with oxygen, releasing a large amount of energy in the form of light and heat. Ex. 2H2(g) + O2(g)  2H2O(g)

15. Activity Series of the Elements Activity series – a list of elements organized according to the ease with which the elements undergo certain chemical reactions.