1. Describing Chemical Change OBJECTIVES: Write equations describing chemical reactions, using appropriate symbols

2. Describing Chemical Change OBJECTIVES: Write balanced chemical equations, when given the names or formulas of the reactants and products in a chemical reaction.

3. All chemical reactions have two parts: Reactants - the substances you start with Products- the substances you end up with The reactants turn into the products. Reactants  Products

4. In a chemical reaction The way atoms are joined is changed Atoms aren’t created or destroyed. Can be described several ways: 1. In a sentence Copper reacts with chlorine to form copper (II) chloride. 2. In a word equation Copper + chlorine  copper (II) chloride

5. Symbols in equations- p.206 the arrow separates the reactants from the products Read “reacts to form” The plus sign = “and” (s) after the formula = solid (g) after the formula = gas (l) after the formula = liquid

6. Symbols used in equations (aq) after the formula - dissolved in water, an aqueous solution.  used after a product indicates a gas (same as (g))  used after a product indicates a solid (same as (s))

7. Symbols used in equations indicates a reversible reaction (more later) shows that heat is supplied to the reaction is used to indicate a catalyst is supplied, in this case, platinum.

8. Skeleton Equation Uses formulas and symbols to describe a reaction doesn’t indicate how many. All chemical equations are sentences that describe reactions.

9. Convert these to equations Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water.

10. Now, read these: Fe(s) + O 2 (g)  Fe 2 O 3 (s) Cu(s) + AgNO 3 (aq)  Ag(s) + Cu(NO 3 ) 2 (aq) NO 2 (g) N 2 (g) + O 2 (g)

11. Balancing Chemical Equations

12. Balanced Equation Atoms can’t be created or destroyed All the atoms we start with we must end up with A balanced equation has the same number of each element on both sides of the equation.

13. C + O 2  CO 2 This equation is already balanced What if it isn’t? C + O O  C O O

14. C + O 2  CO We need one more oxygen in the products. Can’t change the formula, because it describes what it is (carbon monoxide in this example) C + O  C O O

15. Must be used to make another CO But where did the other C come from? C + O  C O O O C

16. Must have started with two C 2 C + O 2  2 CO C + O  C O O O C C

17. Rules for balancing:  Assemble, write the correct formulas for all the reactants and products  Count the number of atoms of each type appearing on both sides  Balance the elements one at a time by adding coefficients (the numbers in front) - save H and O until LAST!  Check to make sure it is balanced.

18. Never change a subscript to balance an equation. If you change the formula you are describing a different reaction. H 2 O is a different compound than H 2 O 2 Never put a coefficient in the middle of a formula 2 NaCl is okay, Na2Cl is not.

19. Example H 2 +H2OH2OO2O2  Make a table to keep track of where you are at

20. Example H 2 +H2OH2OO2O2  Need twice as much O in the product RP H O 2 2 2 1

21. Example H 2 +H2OH2OO2O2  Changes the O RP H O 2 2 2 1 2

22. Example H 2 +H2OH2OO2O2  Also changes the H RP H O 2 2 2 1 2 2

23. Example H 2 +H2OH2OO2O2  Need twice as much H in the reactant RP H O 2 2 2 1 2 2 4

24. Example H 2 +H2OH2OO2O2  Recount RP H O 2 2 2 1 2 2 4 2

25. Example H 2 +H2OH2OO2O2  The equation is balanced, has the same number of each kind of atom on both sides RP H O 2 2 2 1 2 2 4 2 4

26. Example H 2 +H2OH2OO2O2  This is the answer RP H O 2 2 2 1 2 2 4 2 4 Not this

27. dstreib:Stoichiometry,adapted with permission from Dr. Cotton Balancing Examples _ AgNO 3 + _Cu  _Cu(NO 3 ) 2 + _Ag _Mg + _N 2  _Mg 3 N 2 _P + _O 2  _P 4 O 10 _Na + _H 2 O  _H 2 + _NaOH _CH 4 + _O 2  _CO 2 + _H 2 O