2. Law of Conservation of Matter The Law of Conservation of Matter states that matter can neither be created nor destroyed.The Law of Conservation of Matter states that matter can neither be created nor destroyed. Because the same atoms are present in a reaction at the beginning and at the end, the amount of matter in a system does not changeBecause the same atoms are present in a reaction at the beginning and at the end, the amount of matter in a system does not change Antoine Lavoisier, (1788)

3. –Chemical reactions involve changes in matter, the making of new materials with new properties, and energy changes. –Symbols represent elements, formulas describe compounds, chemical equations describe a chemical reaction. 4 Al(s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) 4 Al(s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) Chemical Reactions

4. 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 units 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

5. CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2

6. Diatomic Molecules Diatomic Molecules are elements that are not found by themselves freely in nature, they are found as 2 atoms bonded together. There are 7 total diatomic molecules. Element PresentElemental State at 25 o C Molecule hydrogen colorless gas H 2 nitrogen colorless gas N 2 oxygen pale blue gas O 2 fluorine pale yellow gas F 2 chlorine pale green gas Cl 2 bromine reddish-brown liquid Br 2 iodine lustrous, dark purple solid I 2

8. Reactant(s) Product(s) 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.

9. reactantsproducts. Chemical equations show the conversion of reactants into products. A (+) sign separates molecules on the same side The arrow is read as “yields” or “produces” Example C + O 2  CO 2 This reads “carbon plus oxygen react to yield carbon dioxide” Parts of a Chemical Reaction Equation

10. Symbols Used in Chemical Equations “Yields”; indicates result of reaction Used to indicate a reversible reaction, equilibrium A reactant or product in the solid state; also used 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)

11. Chemical Equations Chemical equations show correct chemical formulas and “coefficients” (if more than 1) to show the amounts (mole) of reactant and products! REACTANTS (starting materials) PRODUCTS (ending materials) which “yield” (…come together and make…) CaCO 3 + 2 HCl CaCl 2 + H 2 O + CO 2 Chemical equations use formulas and coefficients to describe both what reacts and forms,and how much!

12. Writing Chemical Equations To convert a word equation into a chemical equation… Three steps must be kept in mind: 1.From reading the reaction, decide which substances are reactants and which are products reactant words: “__combines with__” “__reacts with___” “___decomposes into” product words: “___is formed” “produces ____” “___is obtained by”

13. Writing Chemical Equations 2. Be sure the FORMULAS of all substances are written CORRECTLY! Be sure you know how to use your oxidation table of ions and their charges! (If the wrong formula is used for ANY reactant or product, the chemical equation will never be correct!)

14. Writing Chemical Equations 3.Write the reactant formulas to the left of the “yields” sign, and… write the product formulas to the right of the “yields” sign. (It doesn’t matter what order the reactants are written, so long as they are all on the left side of the “yields” sign…) (The same is true for products, but on the right side of the “yields” sign.) (Note: the reaction written with just the correct formulas is called a “skeleton equation”).

15. Na + Cl 2 22 Write the word equation for the reaction of 2 atoms sodium reacting with chlorine gas to form 2 units of sodium chloride. NaCl

16. Writing Chemical Equations Example 1: Iron(II) sulfide is formed from the reaction of iron metal and sulfur. Step 1: iron and sulfur are the reactants iron(II) sulfide is the product Step 2: iron = Fe, sulfur = S, and… iron(II) sulfide = Fe +2 and S -2, written “FeS” Step 3: Fe + S  FeS

17. Writing Chemical Equations Example 2: Carbon combines with oxygen to form carbon dioxide. Step 1: carbon and oxygen are the reactants carbon dioxide is the product Step 2: carbon = C, oxygen = O 2 (diatomic), and… Carbon dioxide = C +4 and O -2, written “CO 2 ” Step 3: C + O 2  CO 2

18. Writing Chemical Equations Example 3: 4 atoms of zinc reacts with 2 units of aluminum phosphate to yield 2 atoms of aluminum and zinc phosphate Step 1: zinc and aluminum phosphate are the reactants aluminum and zinc phosphate are the products Step 2: zinc = Zn, aluminum phosphate = AlPO 4, and… aluminum = Al and zinc phosphate = Zn 3 (PO 4 ) 2 Step 3: 3Zn + 2AlPO 4  2Al + Zn 3 (PO 4 ) 2

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

20. 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

21. 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

22. 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

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

24. 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

25. 1) Write a word equation for the reaction. Write a balanced equation for the reaction between chlorine and sodium bromide to produce bromine and sodium chloride. 2) Write the correct formulas for all reactants and products. 3) Determine the coefficients that make the equation balance. chlorine + sodium bromide  bromine + sodium chloride Cl 2 + NaBr  Br 2 + NaCl Cl 2 + 2 NaBr  Br 2 + 2 NaCl

26. 1) Write a word equation for the reaction. 2) Write the correct formulas for all reactants and products. 3) Determine the coefficients that make the equation balance. aluminum sulfate + calcium chloride  calcium sulfate Al 2 (SO 4 ) 3 + CaCl 2  CaSO 4 + AlCl 3 Write the balanced equation for the reaction between aluminum sulfate and calcium chloride to form a white precipitate of calcium sulfate. Al 2 (SO 4 ) 3 + 3 CaCl 2  3 CaSO 4 + 2 AlCl 3 + aluminum chloride ? ?