1. Released Questions Chemistry CA Standards Test Released Questions

2. Measure temperature Measure heat Measure color of light

5. Observation  Hypothesis  Theory  Law

6. (The Atomic Theory) A well-accepted idea.

8. Refer to your Periodic Table

9. Chemical Families act the same.

10. Alkali metals (Li, Na, K…) are the easiest atoms to pull an electron off of. Noble gases are the hardest to pull an electron off of.

11. Family 6 has 6 valence electrons.

13. Most particles missed the nucleus A few alpha particles hit something small and very dense!

16. single-atom Cl 2 F 2 He N 2 The Diatomic Elements: HONClBrIF or BrINClHOF

18. The examples contain C, N, H, & O nonmetals with nonmetals

21. Use your Periodic Table Same family as Silicon

27. Volume decreases x2 Pressure increases x2

29. At STP, 1.0 mole = 22.4 L So, half a mole = 11.2 L The answer is STP (T=273 K & P=1.00 atm)

30. K -273 = ºC 423 - 273 Remember, no calculator… The answer is NOT negative. And 423 – 273  696!

31. These mix very well so you can dissolve alcohol in water or water in alcohol! Hint: Read the question before looking at the table of information…

33. “Like Dissolves Like” Polar solutes dissolve in polar solvents. Nonpolar solutes dissolve in nonpolar solvents. Polar and nonpolar do not mix (e.g. oil & H 2 O).

34. A Proportion! If 36.2 g dissolves in 100 g of H 2 O, How much dissolves in 50 g of H 2 O?

35. Hint: If the math confuses you, try each answer until you find the right one.

36. ppm is related to %

39. Heat = mass x (change in Temp) x specific heat = 30 g (40.0ºC) (0.4 J/g ºC) = 30 (4)(4) J = 120 x 4 = 480 J From the formula sheet:

40. HCl + NaOH  H 2 O + NaCl (salt water) Salt water is neutral!

41. Our’s looked more like this: Which answer is NOT an electrolyte?

42. Nope… bases are slippery. Nope… acids + bases form salts. Nope… they become less acidic… they get neutralized!

44. Acidic = Low pH Basic = High pH

48. Le Châtelier's Principle Reactants  Products

49. Increase pressure = decrease in volume Not enough room… switch to the side that takes up less room (fewer moles of gas) 2121

50. Add heat… shift left Add liquid… no change Shift left… make O 2 Fewer moles of gas on the right. 5  2

51. Shift right… use up CO No change… 2  2 Shift right… make CO 2 Shift left: use up NO

52. H 2 O(l)  H 2 O(g)

53. 4

54. CH 3 CH 2 OH is C 2 H 6 O C 2 H 6 O + 3O 2  2CO 2 + 3H 2 O

55. Molar mass of carbon-12: 12.00 g/mole Or… 12 grams = 1 mole so… 6 grams =.5 moles

56. Approximate: 195 g = 1 mole… so 97.6 g =.5 mole 1 mole = 6.02 x 10 23 atoms… so.5 mole = 3.01 x 10 23 atoms! Look up Pt on the Periodic Table

57. 1 mole CO 2 and 2 moles H 2 O are formed. Translate: 6.02 x 10 23 = 1 mole 1.2 x 10 24 = 2 moles Use P.O.E. Process OfOf Elimination

58. Molar Mass of CH 4 12.0 + 4.0 = 16.0 g/mole Hint: Again… if the math is too much… try each answer out.

59. 52 g Cr = 6.02 x 10 23 atoms 13 g Cr = ¼ x 6.02 x 10 23 atoms = 1.5 x 10 23 atoms

60. 1 Fe 2 O 3 = 2(55.85) + 3(16.00) = 112 + 48 = 160 grams 3 CO = 3(12.0 + 16.0) = 3(28) = 84 grams So… 160 grams Fe 2 O 3 is needed to react with 84 grams of CO!

61. 6(2+16) = 6(18) = 60 + 48 = 108 grams 2(14+3) = 2(17) = 34 grams 108 g H 2 O  34 g NH 3 so… 54 g H 2 O  17 g NH 3 Hint: The numbers have to be simple because you won’t have a calculator.