Exam Review - Chemistry
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1 Exam Review - Chemistry Part A: Matching Identify the symbol that best matches the description given. a. e. b. f. c. g. d. h. 1. Oxidizing Material 2. Biohazardous Infectious Material 3. Poisonous and Infectious Material Causing Immediate and Serious Toxic Effects 4. Dangerously Reactive Material 5. Corrosive Material 1 P a g e
2 6. Poisonous and Infectious Material Causing Other Toxic Effects 7. Compressed Gas 8. Flammable and Combustible Material Identify the term that best matches the definition or description given. a. viscosity f. density b. melting point g. odour c. solubility h. lustre d. hardness i. malleable e. conductivity j. state 9. ability to conduct electricity or heat 10. soft and pliable 11. ratio of mass to volume 12. sweet or pungent 13. how easily a liquid flows 14. liquid 15. temperature of melting 16. ability to dissolve in another substance 17. shininess 18. ability to scratch other materials 2 P a g e
3 Identify the name that matches the chemical formula in the question. a. hydrogen monoxide e. silicon dioxide b. carbon dioxide f. sulphur hexafluoride c. nitrogen trihydride (ammonia) g. nitrogen tribromide d. fluorine dioxide h. carbon monoxide 19. SF SiO HO 22. CO 23. CO NBr FO NH 3 3 P a g e
4 Part B: Short Answer 27. List three things that the particle theory of matter tells us. 28. List three qualitative physical properties. 29. Identify three physical properties that would be useful in identifying an unknown liquid. 30. Label each of the arrows on the diagram below. 4 P a g e
5 31. Draw diagrams to show the behaviour of particles in each of the three states of matter. 32. Classify each of the following as a solution, mixture, or pure substance. A. a cup of coffee B. a glass of distilled water C. a pizza D. gasoline 33. Compare the density of a gas to the density of a liquid. Your answer may include an illustration to explain the density differences. 34. What is at the centre of an atom? 35. How is the mass number for an atom calculated? 36. Describe the experimental evidence obtained by J. J. Thomson that made it necessary to revise John Dalton s model of the atom. 37. How would Rutherford s conclusions change if all of the alpha particles went straight though the gold foil? 5 P a g e
6 38. Construct a chart outlining the parts of an atom as well as their location and charge, if any. 39. Fill in the Name of element column based on the information provided. Name of element Atomic number 24 Mass number 2 Number of protons 13 Number of neutrons Fill in the Atomic number column based on the information provided. Name of element Magnesium Atomic number Mass number 48 Number of protons Number of neutrons Draw a Bohr-Rutherford model of a magnesium atom. 6 P a g e
7 42. Draw a Bohr-Rutherford model of a fluorine atom. 43. Draw a Bohr-Rutherford model of a sodium atom. 44. Draw a Bohr-Rutherford model of an oxygen atom. 45. Label the following diagram. 7 P a g e
8 46. On the periodic table above, draw in the staircase that separates the metals from the non-metals. 47. If an atom gains an electron, why does it become negative? Explain fully, using an example. 48. What does the 2+ in Mg 2+ represent? 49. Construct a diagram illustrating the formation of magnesium chloride from magnesium and chlorine. Use complete Bohr diagrams. 50. Distinguish between elements and compounds. 8 P a g e
9 Part C: Problem 51. A sample of silver has a density of 10.5 g/cm 3. Determine the volume of a sample if the mass is 38.0 g. 52. A sample of an unknown material has a volume of 24.4 cm 3. Determine the density of the sample if the mass is 36.0 g. 53. Complete the following table. Type of element State at room temperature Appearance Conductivity may conduct electricity; poor conductors of heat Malleability and ductility brittle; not ductile all but one are solids 9 P a g e
10 Answer Section Part A: MATCHING 1. ANS: B PTS: 1 2. ANS: D PTS: 1 3. ANS: C PTS: 1 4. ANS: H PTS: 1 5. ANS: F PTS: 1 6. ANS: G PTS: 1 7. ANS: A PTS: 1 8. ANS: E PTS: 1 9. ANS: E PTS: ANS: I PTS: ANS: F PTS: ANS: G PTS: ANS: A PTS: ANS: J PTS: ANS: B PTS: ANS: C PTS: ANS: H PTS: ANS: D PTS: ANS: F PTS: ANS: E PTS: ANS: A PTS: 1 10 P a g e
11 22. ANS: H PTS: ANS: B PTS: ANS: G PTS: ANS: D PTS: ANS: C PTS: 1 Part B: SHORT ANSWER 27. ANS: Answers can be any three of the following: All matter is made up of tiny particles. Each pure substance has its own type of particle. Particles attract each other. Particles are always moving. Particles at a higher temperature move faster, on average, than particles at a lower temperature. 28. ANS: Answers will vary but may include three of these properties: colour, odour, state, texture, lustre, and malleability. 29. ANS: Answers will vary. The most common physical properties used to describe liquids are viscosity, boiling point, conductivity, and density. 11 P a g e
12 30. ANS: 31. ANS: The particles in a solid are tightly packed in a regular pattern; the particles in a liquid are close together but randomly spaced; and the particles in a gas are well spaced out and with no regular arrangement. For example, 12 P a g e
13 32. ANS: A. solution (Coffee is a solution of sugar, water, and bean distillate.) B. pure substance (Distilled water contains only one type of particle.) C. mixture D. pure substance (Gasoline is a pure substance in grade 9. Although it is a mixture of a variety of hydrocarbons, students are not expected to know this yet. Should a student suggest that it is a mixture, ask them to explain their answer upon return of the paper.) 33. ANS: The density of a gas is lower than that of a liquid since the particles are spread out over a greater area. For example, 34. ANS: At the centre of the atom there are protons and neutrons. 35. ANS: mass number = number of protons in the atom + number of neutrons in the atom 36. ANS: Experimentation with gas discharge tubes gave evidence of small negatively charged particles (electrons) that were common to all elements. 37. ANS: Rutherford s work in this case would have supported J. J. Thomson s model of the atom. It would have proved that there was not a localization of positive charges in one place. 38. ANS: 13 P a g e
14 39. ANS: Name of element Atomic number Mass number Number of protons Number of neutrons chromium 24 does not exist 2 aluminum 13 fluorine ANS: Name of element Atomic number Mass number Number of protons Number of neutrons Magnesium ANS: Marking: 1 point for correct number of neutrons in the nucleus, 1 point for correct number of protons in the nucleus, and 1 point for correct electron configuration 42. ANS: 14 P a g e
15 43. ANS: 44. ANS: 45. ANS: 46. ANS: 47. ANS: When an atom gains an electron, there are more negative charges than positive charges. Since the negative charges and positive no longer balance, the end result is a charged atom. Examples will vary but should include totalling of positive and negative charges. 15 P a g e
16 48. ANS: The 2+ represents the loss of two electrons that occurred to make the atom stable (having a full outer valence shell). 49. ANS: 50. ANS: Elements are individual atoms (or atoms of the same type), whereas compounds are groups of different atoms joined together. PROBLEM 51. ANS: 16 P a g e
17 52. ANS: 53. ANS: Type of element State at room temperature Appearance Conductivity may conduct electricity; metalloids solids shiny or dull poor conductors of heat some gases; poor non-metals some solids; conductors of dull only bromine heat and is a liquid electricity metals all but one are solids shiny good conductors of heat and electricity Malleability and ductility brittle; not ductile brittle; not ductile malleable; ductile 17 P a g e
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