Tuesday May 25, 2010 (Review for Semester Final) (Day 1)

1. TuesdayMay 25, 2010(Review for Semester Final)(Day 1)

2. Bell Ringer Tuesday, 5/25/10 No Bell Ringer Today.

3. Semester Exam Information • If your score is higher on the EOC than on the semester exam, your may take your EOC grade as your semester exam grade. • Semester Exam Exemptions • If you passed the Science TAKS test, you may choose to be exempt from the semester final exam. You may take your second semester average as your exam grade, but only if by doing so you pass the course. If you choose to go ahead and take the exam, you will receive the higher of the two grades. You must report to class during the exam period. This option applies to sophomores and juniors only. • If you have a spring semester average of 85 or higher at the end of the fifth week of the final six-weeks and have been absent 2 or fewer days this semester, you may take your second semester average as your exam grade. This option applies to juniors and seniors only.

5. Review for Final Exam(Day 1)

6. 1 The Kinetic-Molecular Theory of Matter is based upon what idea? Particles of matter are always in motion.

7. 2 The average kinetic energy of gas particles depends upon the _________________ of the gas. temperature

8. 3 Which of the common phases of matter has the lowest density? gases

9. 4 Which of the common phases of matter is the most compressible? gases

10. 5 Give an example of the diffusion of a gas. smelling breakfast cooking in the next room

11. 6 The force of the collisions of gas particles against the inside walls of their container is called _______. pressure

12. 7 86.34 kilopascals of pressure is how many atmospheres? 1 atm = 101.325 kPa 0.8521 atm

13. 8 The pressure exerted on a 650. mL sample of oxygen gas at constant temperature is increased from 0.285 atm to 0.785 atm. What will the final volume of the sample be? Law?Formula? Boyle’s Law • P1V1 = P2V2 • P1V1 /P2 = V2 • 236 mL • 0.285 x 650./0.785= V2

14. 9 A sample of fluorine gas at 22oC and 3.03 atm occupies a volume of 5.12 L. What volume would this gas occupy at 66oC and 0.650 atm? Law? Formula? • P1V1/T1 = P2V2/T2 Combined Law • P1V1T2 = P2V2T1 • P1V1T2/P2T1 = V2 • 27.4 L • 3.03x5.12x339/0.650x295 = V2

15. 10 How many moles of oxygen gas are there if the gas has a volume of 4.50 L, a pressure of 2.50 atm, and a temperature of 40oC? Law? Formula? Ideal Gas Law • PV= nRT • PV / RT= n • 0.440 mol • 2.50x4.50 / 0.0821x313= n

16. 11 The insect in this picture is able to stand on the surface of the water because the force of the surface tension on the water’s surface is stronger than the pull of gravity on the insect.

17. 12 If the attractive forces between water molecules in the liquid phase become much stronger, the liquid water will freeze into ice.

18. 13 • cork According to the density column in the picture, which of the materials is the most dense? glycerin the least dense?

19. 14 A student discovers that the sample of matter she is working with is incompressible, has an extremely low rate of diffusion, and has a high density. What is most likely the identity of her material? a solid

20. 15 Water normally boils at 100°C at sea level and at 97°C on a North American mountaintop. This difference in boiling points can be explained by the difference between the locations’ air pressure.

21. 16 The picture shows the results of pouring a blue liquid into a clear liquid and allowing the mixture to settle for 25 minutes. Compared to the clear liquid, the blue liquid is more dense.

22. 17 Clouds are formed when water vapor in the atmosphere changes into tiny droplets of liquid water. This is the process of Condensation.

23. 18 According to the diagram, if water boils at 1000C, the pressure will be 1.00 atm

24. 19 Water is a very effective solvent because it is a polar molecule. + + -

25. 20 Name a common instance that proves that solid water is less dense than liquid water. Ice floats in liquid water.

26. 21 If a student is trying to determine the saturation point of a solid solute in a liquid solvent, what factors would he most be concerned with? the nature (identity) of the solute and solvent and the temperature of the solvent.

27. 22 According to the chart, how many grams of sodium nitrate (NaNO3) will dissolve in 100 grams of water when the water is at a temperature of 57oC? about 120 grams

28. 23 What factor will most directly affect the solubility of a solid in a liquid? the temperature of the solvent

29. 24 A fish is living in a small pond. One night in November the air temperature falls from 74oF to 43oF. The water temperature decreases as a result. What is a major change that will most likely occur in the fish’s life? The colder water will now hold more oxygen gas and the fish will not have to work as hard to get enough.

30. 25 List the factors that would increase the amount of solid solute that will dissolve in a liquid solvent. increase the temperature of the solvent • add more solvent

31. 26 What is the main difference between the three types of mixtures: solutions, colloids and suspensions? the size the solute particles are broken down to in the dissolving process

32. 27 The table shows properties of four liquids that are insoluble in water. If the four liquids are poured into a beaker containing water, which liquid will form a layer below the water? Liquid Q

33. 28 Why will gasoline not dissolve in water? Gasoline is a non-polar solute and water is a polar solvent.

34. 29 Why does saltwater conduct electrical current? water breaks the salt into charged ions, which conduct current.

35. 30 If a student dissolves 1.5 moles of NaCl in water and makes 4.0 liters of a saltwater solution, what is the molarity of the solution? M = 0.38 M = mol solute / L solution

36. 31 What is occurring in the equation below? HCl æ H+ + Cl- HCl is being ionized by water. H2O

37. 32 In the equation below, Compound X is Compound X æ H+ + an anion- an acid. H2O

38. 33 What is true of an acid in regards to ion concentration? [H+] > [OH-]

39. 34 List three common household items that can be classified as acids. Battery acid Lemon juice Vinegar

40. 35 Name the following acid: H2SO4 sulfuric acid

41. 36 When the indicator bromthymol blue is added to HCl, it changes color from blue to yellow. When it is added to NaOH it remains blue. What does this indicate? Bromthymol blue is an acid-only indicator.

42. 37 A student has a solution that tastes bitter, feels slippery, and is a weak electrolyte. What is most likely the identity of her solution? a base

43. 38 Which ion, H+ or OH-, is present in greater number in vinegar at a pH of 5, and how many more ions of this type are there than the other type? H+ is present in greater number. There are 100x more H + ions than OH- ions at a pH of 5.

44. 39 Which of the following statements is the most accurate? • Soap and shampoo are acidic, while oranges and lemons are basic. • The foods we eat can contain many different types of acids, whereas household cleaning supplies can contain bases. • Acids are always safe to taste as long as you don’t taste too much. • All bases are harmful and should never be touched.

45. 40 List three environmental problems caused by acid rain. the deterioration of buildings and statues. the killing of plants and animals in a forest. the killing of plants and animals in rivers and streams.

46. 41 Can you make an element (like gold) from other elements? Explain. Yes, you can make gold atoms from other atoms, but only in vary small amounts.

47. 42 Name a pair of elements that could undergo nuclear fusion to produce gold. Any elements that have atomic numbers that total 79, like iridium and helium

48. 43 List two examples each of nuclear fission and nuclear fusion. Fission a submarine using a nuclear reactor for power the explosion of an atomic-bomb Fusion the Sun generating heat and light the explosion of a hydrogen-bomb

49. 44 What parts of the atom participate directly in a nuclear reaction? protons and neutrons

50. 45 Which one of the following is not a result of a nuclear reaction? • the generation of x-rays for cancer treatment • the Sun generating radiation • hydrogen gas and oxygen gas combining to make water • radioactivity produced from the detonation of an atom bomb