1. Chemical Equations & Reactions Chapter 8 Lesson 1

2. Chemical Reactions You should be able to  Classify reactions by type.  Write a balanced molecular equation, complete ionic equation, and a net ionic equation.  Balance oxidation-reduction reactions.  Predict if a precipitate will form using the solubility rules.  Predict products of reactions given the chemical names of the reactants.

3. Organize Your Thoughts Chemical reactions Chemical equations Chemical equations Balancing equations Predicting products from reactants Synthesis Decomposition Single replacement Double replacement Combustion Packard, Jacobs, Marshall, Chemistry Pearson AGS Globe, page 175

4. Describing a Chemical Reaction Indications of a Chemical Reaction –Evolution of heat, light, and/or sound –Production of a gas –Formation of a precipitate –Color change

5. Signs of Chemical Reactions There are five main signs that indicate a chemical reaction has taken place: change in colorchange in odorproduction of new gases or vapor input or release of energy difficult to reverse release input

6. Chemical Equations reactantsproducts Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al(s) + 3 O 2 (g) 2 Al 2 O 3 (s) The numbers in the front are called stoichiometric coefficients stoichiometric coefficients. The letters (s), (g), and (l) are the physical states of compounds. reactants product aluminum oxide

7. Chemical Equations This equation means: 4 Al(s) + 3 O 2 (g) 2 Al 2 O 3 (s) 4 Al atoms + 3 O 2 molecules yield 2 molecules of Al 2 O 3 4 Al moles + 3 O 2 moles yield 2 moles of Al 2 O 3 or 4 g Al + 3 g O 2 yield 2 g Al 2 O 3 4 mol Al@27g/mol 3 mol O 2 @32g/mol 2 mol Al 2 O 3 @102g/mol 108 g + 96 g = 204 g aluminum oxide sandpaper

8. Chemical Equations Because the same atoms are present in a reaction at the beginning (reactants) and at the end (products), the amount of matter in a system does not change. Law of Conservation of Matter The Law of Conservation of Matter Kotz web ChemicalFactory 100% 80% 20%

9. Chemical Equations conservation of matter Because of the principle of the conservation of matter, equation must be balanced An equation must be balanced. It must have the same number of atoms of the same kind on both sides. Lavoisier, 1788

10. 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.

11. Chemical Equations Reactants – the substances that exist before a chemical change (or reaction) takes place. Products – the new substance(s) that are formed during the chemical changes. CHEMICAL EQUATION indicates the reactants and products of a reaction. REACTANTS  PRODUCTS

12. Word Equations A WORD EQUATION describes chemical change using the names of the reactants and products. Write the word equation for the reaction of methane gas with oxygen gas to form carbon dioxide and water. methane + oxygen Reactant Product CH 4 O2O2 CO 2 H2OH2O + + 2 2 carbon dioxide + water

13. Cl H H H HH H H H 2 + Cl 2  HCl H 2 + Cl 2  2 HCl reactants products H Cl reactants products H Cl 2 2 22 2 2 1 1 (unbalanced) (balanced) Unbalanced and Balanced Equations

14. ? Visualizing a Chemical Reaction Na + Cl 2 NaCl ___ mole Cl 2 ___ mole NaCl___ mole Na 2 105 2 5

15. Visualizing a Chemical Reaction Na + Cl 2 NaCl 2 2

16. Meaning of Chemical Formula Chemical Symbol Meaning Composition H 2 O One molecule of water: Two H atoms and one O atom 2 H 2 O Two molecules of water: Four H atoms and two O atoms H 2 O 2 One molecule of hydrogen peroxide: Two H atoms and two O atoms

17. Balancing Chemical Equations Balanced Equation – one in which the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product What is the relationship between conservation of mass and the fact that a balanced equation will always have the same number of atoms of each element on both sides of an equation? Determine whether the following equation is balanced. 2 Na + H 2 O  2 NaOH + H 2 2 Na + 2 H 2 O  2 NaOH + H 2

18. Balancing Chemical Equations Write a word equation for the reaction. Write the correct formulas for all reactants and products. Determine the coefficients that make the equation balance.

19. Balancing Chemical Equations An important point to remember 2 NO(g) + O 2 (g)  2NO 2 (g) The 2 to the left of NO(g) and NO 2 (g) refers to the number of molecules present in the balanced equation. It is a “multiplier” for every atom in the molecule. The subscript 2 in O 2 (g) and NO 2 (g) refers to the number of atoms of this type that are present in each molecules (or ionic compound).

20. Showing Phases in Chemical Equations Solid Phase – the substance is relatively rigid and has a definite volume and shape. NaCl(s) Liquid Phase – the substance has a definite volume, but is able to change shape by flowing. H 2 O(l) Gaseous Phase – the substance has no definite volume or shape, and it shows little response to gravity. Cl 2 (g) H 2 O(s) H 2 O(l) H 2 O(g)

21. Additional Symbols Used in Chemical Equations “Yields”; indicates result of reaction Used to indicate a reversible reaction A reactant or product in the solid state; also used to indicate a precipitate Alternative to (s), but used only to indicate a precipitate A reactant or product in the liquid state A reactant or product in an aqueous solution (dissolved in water) A reactant or product in the gaseous state (s)(s) (l)(l) (aq) (g)(g)

22. Additional Symbols Used in Chemical Equations Alternative to (g), but used only to indicate a gaseous product Reactants are heated Pressure at which reaction is carried out, in this case 2 atm Pressure at which reaction is carried out exceeds normal atmospheric pressure Temperature at which reaction is carried out, in this case 0 o C Formula of catalyst, in this case manganese (IV) oxide, used to alter the rate of the reaction 2 atm pressure 0 o C MnO 2 

23. Solubility Ionic Equations Cover the answers, work the problem, then check the answer. 1. Dissolve ammonium nitrate: 2. Precipitate cupric hydroxide: 3. Dissolve chromium thiocyanate: 4. Precipitate lead arsenate: 5. Dissolve silicon permanganate: 6. Precipitate zinc phosphate: NH 4 NO 3 (s) ---> NH 4 +1 (aq) + NO 3 -1 (aq) Cu +2 (aq) + 2OH -1 (aq) ---> Cu(OH) 2 (s) Cr(SCN) 3 (s) ---> Cr +3 (aq) + 3SCN -1 (aq) 3Pb +2 (aq) + 2AsO 4 -3 (aq) ---> Pb 3 (AsO 4 ) 2 (s) Si(MnO 4 ) 4 (s) ---> Si +4 (aq) + 4MnO 4 -1 (aq) 3Zn +2 (aq) + 2PO 4 -3 (aq) ---> Zn 3 (PO 4 ) 2 (s)