1. Question of the Day Name for H 3 PO 4 = Formula for magnesium hydroxide = Day 1 9-12

2. How do I name chemicals? How do I determine a chemical’s formula? Day 6 9-11

3. Practicing formulas: Barium Sulfide Ferric Chloride Cobalt II oxide

4. Ionic Compounds & Polyatomic Ions Oxyanions – polyatomic ions that contain oxygen ate = ending for most common ion (ClO 3 - Chlorate) ite = ending for one less oxygen (ClO 2 - Chlorite) hypo = prefix for another less oxygen (ClO - Hypochlorite) per = prefix for one more than most common (ClO 4 - Perchlorate)

5. Binary Molecular Compounds Based on Prefixes 1. Less electronegative first – prefix only if more than one atom 2. Second element – prefix, root of name, ending ide (if only two elements) 3.o or a @ the end of prefix is dropped if name begins with a vowel (monooxide, monoxide)

6. PAGE 281 Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10 Binary Molecular Compounds – prefix system

7. Write the Formula: Germanium tetraiodide diphosphorous trioxide Write the Name: N 2 O 5 SbF 3 GeI 4 P2O3P2O3 Dinitrogen pentoxide Antimony trifluoride Binary Molecular Compounds

8. Write the Formula: carbon tetraiodide dinitrogen trioxide Write the Name: As 2 O 5 ICl 3 CI 4 N 2 O 3 diarsenic pentoxide iodine trichloride

9. Molecular Element – molecule of atoms of same element – NOT a compound -like O 2, Cl 2, O 3 allotrope – single element, different structure

12. Day 2 9-13 1.Name Cu 2 CO 3 2.What are the formulas for sulfurous acid and Ferric nitrite?

13. 1. How do I use an equation to represent a chemical reaction?

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

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

16. 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

17. 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

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

19. 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

20. 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)

21. 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

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

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

24. Balancing Equations Chemicals equations are not always balanced, sometimes we will have to balance them … 1. Balance different types of atoms one at a time 2. Start with atoms that appear only once on each side

25. 1. Balance different types of atoms one at a time 2. Start with atoms that appear only once on each side 3. Balance polyatomic ions that appear on both sides of the equation as a single unit 4. Balance H and O atoms last Balancing Equations

26. If it’s not working… 1. Deep breathe 2. Check your chemical formulas 3. NEVER change subscripts this changes the compounds!!! 4. It’s ok to start over if you get frustrated Balancing Equations

27. Al (s) + O 2(g)  Al 2 O 3(s)

28. Balancing Equations Na + Mg 3 (PO 4 ) 2 → Mg + Na 3 PO 4 Polyatomic Example:

31. 1. Name the following: CoPO 4 and HC 2 H 3 O 2. 2. What are the formulas for the following: cadmium borate and chloric acid? Day 3 9-16

32. 1. How do I prepare solutions? 2. How do I balance chemical equations?

33. C 6 H 14 + O 2 CO 2 + H 2 O COHCOH COHCOH 6 2 142 3 1 C’s First 6 12 13 O’s Second 14219 26 28 38 12 38 6 Balancing Equations

34. C 3 H 8(g) + O 2(g)  CO 2(g) + H 2 O (g)

35. Molarity = desired concentration moles/liter so a 1M solution contains 1 mole for every 1 liter Desired concentration X volume (L) X molar mass of solid = needed mass

36. Moles Liters grams Moles gramsX X=

37. Molarity = desired concentration moles/liter so a 1M solution contains 1 mole for every 1 liter Desired conc. X Desired vol. (L) = Starting conc. X Starting vol. of acid (L)

38. Moles Liters Moles Liters XX Desired conc. X Desired vol. (L) = Starting conc. X Starting vol. of acid (L) =

39. 350 mL 0.5 M CuCl 2 50 mL 0.5 M KOH 300 mL 1 M CuCl 2 200 mL 2 M H 3 PO 4 Period 1 9-14

40. 50 mL 0.5 M CuCl 2 50 mL 1 M CuCl 2 200 mL 4 M H 2 SO 4 200 mL 1 M HCl Period 3 9-17

41. Read and/or review section 11.1 AND complete #s 9 (part b only), 10, and 11 on the bottom of page 354 # 11 p. 273, # 13 p. 275, # 14 p. 277, #s 21, 23- 26 p. 279 Due tomorrow (Day 3 9-14)

42. Day 3 9-14 Liquid water breaks apart into hydrogen gas and oxygen gas (electrolysis). Equation: Balance: Reaction Type:

43. – solid formed when two aqueous solutions react – product that comes out of solution

44. 4. Balance H 2 SO 4 + NaOH  Na 2 SO 4 + H 2 O Na SO 4 H O Na SO 4 H O

45. Types of Chemical Reactions Synthesis reaction – composition reaction – 2 or more substances combine to form a new compound A + B AB A and B = eles. Or cmpds. AB = cmpd. Example # 1: 2H 2 (g) + O 2 (g) 2H 2 O(g) A B AB Synthesis Reactions

46. A and B = eles. Or cmpds. AB = cmpd. Example # 2: 2H 2 SO 3 (aq) + O 2 (g) 2H 2 SO 4 (aq) A B AB Example # 3: CaO(s) + SO 2 (g) CaSO 3 (s) A B AB Types of Chemical EquationsSynthesis Reactions

47. Types of Chemical EquationsSynthesis Reactions Examples: - an element reacts with oxygen to form an oxide - most metals react with halogens to form cmpds. - oxides of active metals react with water to produce metal hydroxides - certain metal oxides and nonmetal oxides react to form salts

48. Types of Chemical EquationsSynthesis Reactions

49. Types of Chemical EquationsDecompostion Reactions decomposition reaction – single compound undergoes a reaction that produces 2 or more simpler subs. – usually require add. of energy (heat or electricity) AB A + B A and B = eles. Or cmpds. AB = cmpd. Example: 2H 2 O(l) 2H 2 (g) + O 2 (g) AB A B electricity

50. Types of Chemical EquationsDecompostion Reactions Examples: - electric current to a binary compound producing its elements - heating the oxides of less active metals - Metal carbonates produce metal oxide + CO 2

51. Types of Chemical EquationsDecompostion Reactions Electrolysis – decpomposition of a substance by an electrical current

52. Types of Chemical EquationsDecompostion Reactions