1. Chemical Reactions and Equations Reactants →Products Reactants are starting materials and are shown at left of arrow Products are final materials and are shown on right of arrow

2. Phase Labels Phase labels show state of materials written as subscript in parentheses after formula (s) = solid (l)= liquid (g) = gas (aq) = aqueous (dissolved in water)

3. Greek Letter Delta Δ indicates that heat must be added to make reaction go Δ shown over arrow

4. Evidence for a Chemical Reaction Formation of a gas (Fizzes) Formation of a solid (precipitate) when liquids are mixed Change in color (not just dilution of color) Change in heat (released or absorbed)

5. Equations must be BALANCED According to Law of Conservation of Matter (Mass), matter cannot be created or destroyed in a chemical reaction Thus equations must have same number of each kind of atom on left and right sides

6. Rules for Balancing Equations 1.Write correct formula for each reactant and product. 2.Do NOT change formula----ever! 3.Change the number of each kind of atom in equation by writing coefficients in front of the formula.

7. 4.Keep changing coefficients until the equation is balanced and there are the same number of atoms of each kind on both sides. 5.Double check your equation.

8. Balance the following equation H 2 + N 2  NH 3

9. 3 H 2 + N 2  2 NH 3

10. Avogadro’s Number and the Mole Atomic mass unit (amu) - unit of measure for the mass of atoms. –carbon-12 assigned the mass of exactly 12 amu –1 amu = 1.66 x 10 -24 g –periodic table gives atomic weights in amu.

11. What is atomic weight of one F atom? Atomic weight of one F atom (from periodic table) is 19.00 amu What is mass of one F atom in grams?

12. More convenient to work with grams than amu, but mass of one atom is VERY SMALL Therefore, we use a new unit: mole (mol)

13. Mole 1 mole = 6.022 x 10 23 (of anything) Unit similar to other common units dozen (12) gross (12 dozen or 144)

14. Avogadro’s number = 6.022 x 10 23 Number of atoms of C found in 12.01 grams of Carbon

16. Molar Mass of element Mass in grams of one mole of atoms Can convert between atoms, moles and mass

17. Mass ↔ Moles Use molar mass1 mol = “x” g How many grams are there in 0.20 mol of H? 0.20 mol H x 1.008 g H = 0.20 g H 1 mol H How many mol of C are there in 4.0 g of C?

18. Molar Mass Mass of one mole of compound Molar mass has same numerical value as formula weight, but different units (g/mol) 1 formula weight of NaCl = 58.5 amu 1 mole of NaCl= 58.5 g

19. Compounds Formula mass (formula weight): Mass of one molecule or formula unit Given in amu Add up atomic mass of all atoms in compound

20. Calculation of Formula Weight NaCl 1 Na @ 23.0 amu= 23.0 amu 1 Cl @ 35.45 amu= 35.45 “ 1 formula weight of NaCl = 58.5 amu

21. What do the coefficients in a balanced equation mean? 3 H 2 + 1 N 2  2 NH 3 Moles 312 Molecules 312 Coefficients do not give mass relationship

22. Conversions between moles and atoms 1 mol = 6.02 x 10 23

24. Need to convert moles to mass in order to get mass relationships (not coefficients) 3 H 2 + 1 N 2  2 NH 3 3 mol H 2 + 1 mol N 2 → 2 mol NH 3 3 mol H 2 x 1 mol N 2 x 2 mol NH 3 x 2 g H 2 /mol H 2 28 g N 2 /mol N 2 17 g NH 3 /mol NH 3 6 g H 2 + 28 g N 2 = 34 g NH 3

25. 2 Mg + O 2  2 MgO How much MgO can be made if you start with 6.07 g of Mg? Convert g Mg to mol Mg Convert mol Mg to mol MgO (Use equation) Convert mol MgO to g Mg 1 mol Mg = 24.3 g 1 mol MgO = 40.3 g 1 mol O 2 = 32 g

26. 2 Mg + O 2  2 MgO How much MgO can be made if you start with 6.08 g of Mg?

27. 2 Mg + O 2  2 MgO How much MgO can be made if you start with 6.08 g of Mg?

28. Limiting Reagent May run out of one compound before you use up all of the other compound. If you start with 6.08 g Mg and 32 g O 2 which will be used up first?

29. Limiting Reagent May run out of one compound before you use up all of the other compound. If you start with 6.08 g Mg and 32 g O 2 which will be used up first?