1. Read pages 346-349, define chemical equation and skeleton equation, AND complete #s 1 and 2 on page 349. Assignment Day 1 4-25

2. 1. Locate your Chapter # 7 test. 2. Calculate and record your % grade. 3. I studied for this test by… 4. Next time I will study by… 5. Set a goal for next time: If you did not meet your goal it stays the same. If you did meet your goal your new goal must be an improvement of at least one point. Day 2 4-26

3. Describing Chemical Reactions Chemical Reactions – a process in which one or more substances are converted into new substances with different physical and chemical properties Bonds break, and/or form, and/or rearrange!!!

4. H 2(g) + F 2(g) 2HF (g) Chemical equation reactantsproducts Describing Chemical Reactions Reactions are represented by chemical equations

5. H 2(g) + F 2(g) 2HF (g) reactantsproducts Describing Chemical Reactions State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

6. H 2(g) + F 2(g) 2HF (g) reactantsproducts Describing Chemical Reactions Coefficients – how many mols of each element react with each other – mol ratio

7. H 2(g) + F 2(g) 2HF (g) Describing Chemical Reactions 1 mol of hydrogen gas reacts with 1 mol of fluorine gas to produce 2 mols of hydrogen fluoride gas For now think of a mol as a piece: 1 piece of hydrogen gas reacts with 1 piece of fluorine gas to produce 2 pieces of hydrogen fluoride gas

8. Atoms are neither created nor destroyed in ordinary chem. rxns. Describing Chemical Reactions Conservation of matter -

9. Describing Chemical Reactions A heads-up on diatomic gases: If the natural state of an element is gas, assume it is always a diatomic molecule (Example: Nitrogen = N 2 ) – NOT including the noble gases

10. Chemical Reactions – What’d We Just Do? Bonds … a process in which one or more substances are converted into new substances with different physical and chemical properties

11. H 2(g) + F 2(g) 2HF (g) Chemical equation reactantsproducts What’d We Just Do?

12. H 2(g) + F 2(g) 2HF (g) reactantsproducts State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution What’d We Just Do?

13. H 2(g) + F 2(g) 2HF (g) reactantsproducts Coefficients – how many mols of each element react with each other – mol ratio What’d We Just Do?

14. Balancing Equations Writing a chemical equation: Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid. Hydrogen gas = Chlorine = Liquid Hydrochloric acid =

15. Balancing Equations Writing a chemical equation: Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid. Reactants = Product = H 2(g) + Cl 2(g)  HCl (l)

16. Balancing Equations Atoms are neither created nor destroyed in ordinary chem. rxns. - Sum of atoms on each side must be equal - Use coefficients to help

17. Balancing Equations H 2(g) + Cl 2(g)  HCl (l)

18. Read pages 346-349, define chemical equation and skeleton equation, AND complete #s 1 and 2 on page 349. Assignment Day 1 4-25

19. Balance the following chemical reaction: Li 2 O (s) + H 2 O (l)  LiOH (aq) Q Of The Day Day 4 4-24

20. Balance the following chemical reaction: HCl (aq) + Mg(OH) 2(aq)  MgCl 2(aq) + H 2 O (l) Q Of The Day Day 5 4-25

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22. 1. Define chemical reaction (using your own brain – doesn’t have to be perfect today). Day 2 4-20

23. 1. Define chemical reaction (use your notes if needed). Day 2 4-20

24. Use the following chemical reaction to answer the questions below: 4Li (s) + O 2(g)  2Li 2 O (s) a. lithium oxide = what state of matter b. What does the 4 in front of Li tell you? c. What is produced? Q Of The Day Day 3 4-23

26. Chemical Reactions – Last time Bonds … a process in which one or more substances are converted into new substances with different physical and chemical properties

27. Last time Atoms are neither created nor destroyed in ordinary chem. rxns. Conservation of matter -

28. H 2(g) + F 2(g) 2HF (g) Chemical equation reactantsproducts Last time

29. H 2(g) + F 2(g) 2HF (g) reactantsproducts State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution Last time

30. 2H 2(g) + O 2(g) 2H 2 O (l) reactantsproducts Coefficients – how many mols of each element react with each other – mol ratio Last time

31. Liquid water breaks apart into hydrogen gas and oxygen gas (electrolysis). Equation: Build:

32. Solid sodium reacts with chlorine gas to produce solid sodium chloride. Equation: Build:

33. Solid magnesium reacts with fluorine gas to produce solid magnesium fluoride. Equation: Build:

34. Review section 11.1 and complete #s 8, 10, 11a (skip 11b and 11c) on page 354

35. Balancing Equations Writing a chemical equation: Solid aluminum reacts with oxygen gas to produce solid aluminum oxide (Al 2 O 3 ). Equation =

36. Review section 11.1 and complete #s 7-9 (9a only) AND 10-11 (do 11a, skip 11b and 11c) on page 354

37. H 2(g) + F 2(g) 2HF (g) ____________________ _______________ Reactions are represented by ___________________ _______________

38. H 2(g) + F 2(g) 2HF (g) State of matter: g = _______, l = __________, s = _________, aq = _________________________

39. H 2(g) + F 2(g) 2HF (g) Coefficients – _______________________________ _____________________________________ – mol ratio