1. Chemical Reactions Chemistry

2. All Chemical Reactions have two parts: 1.Reactants = the substances you start with 2.Products = the substances you end up with The reactants will turn into the products. Reactants Products

3. Chemical Reaction Atoms aren’t created or destroyed (according to the Law of Conservation of Mass) A reaction can be described several ways: #1. In a sentence every item is a word Copper reacts with chlorine to form copper (II) chloride. #2. In a word equation some symbols used copper + chlorine  copper (II) chloride

4. Symbols in Equations t he arrow (→) separates the reactants from the products (arrow points to products) – Read as: “reacts to form” or “yields” The plus sign = “and” (s) after the formula = solid: Fe (s) (g) after the formula = gas: CO 2(g) (l) after the formula = liquid: H 2 O (l)

5. Symbols Used in Equations (aq) after the formula = dissolved in water, an aqueous solution: NaCl (aq) is a salt water solution ↑used after a product indicates a gas has been produced: H 2 ↑ ↓used after a product indicates a solid has been produced: PbI 2 ↓

6. Symbols Used in Equations ■ double arrow 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 is the catalyst)

7. What is a Catalyst? A substance that speeds up a reaction, without being changed or used up by the reaction. Enzymes are biological or protein catalysts in your body.

8. The Skeleton Equation Uses formulas and symbols to describe a reaction – but doesn’t indicate how many; this means they are NOT balanced All chemical equations are a description of the reaction. The equation provides a “balance sheet” to monitor changes in reactants and products and keep track of atoms.

9. Write a Skeleton Equation 1. Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. 1 st - write the basics formulas for reactants and products: Important to write them correctly. Once correctly written, don’t alter them! Fe 2 S 3 (s) + HCl (aq)  FeCl 3 (s) + H 2 S (g) Do you have the same number and type of atoms on both sides?....if not, use COEFFICIENTS! Fe 2 S 3 (s) + 6HCl (aq)  2FeCl 3 (s) + 3H 2 S (g)

10. Write a Skeleton Equation 1. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. HNO 3 (aq) + Na 2 CO 3 (s)  CO 2 (g) + H 2 O (l) + NaNO 3 (aq) BALANCED? 2HNO 3 (aq) +Na 2 CO 3 (s)  CO 2 (g) + H 2 O (l) + 2NaNO 3 (aq)

11. Now, read these equations: 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)

12. Balanced Chemical Equations Atoms can’t be created or destroyed in an ordinary reaction: – All the atoms we start with we must end up with (meaning: balanced!) A balanced equation has the same number of each element on both sides of the equation.

13. Rules for Balancing: 1)Assemble the correct formulas for all the reactants and products, using “+” and “→” 2)Count the number of atoms of each type appearing on both sides 3)Balance the elements one at a time by adding coefficients (the numbers in front) where you need more - save balancing the H and O until last/ balance single atoms last 4) Double-check to make sure it is balanced.

14. NEVER Never change a subscript to balance an equation (only change coefficients) – If you change the subscript (formula) you are describing a different chemical. – H 2 O is a different compound than H 2 O 2 Never put a coefficient in the middle of a formula; they must go only in the front 2 NaCl is okay, but Na 2 Cl is not.

15. Practice Balancing 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

16. Net Ionic Equations Many reactions occur in water- that is, in aqueous solution When dissolved in water, many ionic compounds “dissociate”, or separate, into cations and anions Now we are ready to write an ionic equation

17. Net Ionic Equations AgNO 3 (aq) + NaCl (aq) AgCl (s) + NaNO 3 (aq) this is the full balanced equation next, write it as an ionic equation by splitting the compounds into their ions: Ag + + NO 3 - + Na + + Cl -  AgCl (s) + Na + + NO 3 - Note that the AgCl did not ionize, because it is a “precipitate” (a solid, not aqueous)

18. Net Ionic Equations simplify by crossing out ions not directly involved (called spectator ions, same on both sides) Ag + + Cl - AgCl This is called the net ionic equation Let’s talk about precipitates before we do some other examples

19. Predicting the Precipitate Insoluble salt = a precipitate Always soluble: salts of Na +, K +, NH 4 +, and NO 3 - Usually soluble: salts of Cl - and SO 4 2-, but AgCl, PbCl 2, PbSO 4 and BaSO 4 are insoluble Usually insoluble: salts of OH -, O 2-, CO 3 2-, and PO 4 3- (unless with Na +, K +, or NH 4 + ) Slightly soluble: Ca(OH) 2 and CaSO 4