CHEMISTRY BOOT CAMP: REFERENCE TABLES

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1 Name: Date: Hour: CHEMISTRY BOOT CAMP: REFERENCE TABLES Purpose. The science portions of the ACT and MME are designed to test your ability to use scientific reasoning. This generally involves interpreting tables with information that you have little to no prior knowledge about. We will use many of the tables found in Reference Tables for Physical Setting/Chemistry but before we learn about them in detail, you should take this opportunity to see how well you can read a table with little to no prior knowledge. If you have read this, put a check mark in the top right corner of this page. Table C: Selected Prefixes 1. Identify the factor for each of the following prefixes: a) centi- d) micro- b) milli- e) kilo- c) nano- f) pico- 2. Write the symbols for each of the following prefixes: a) deci- d) milli- b) micro- e) pico- c) centi- f) nano- 3. Organize the following prefixes from largest to smallest: centi-, nano-, kilo-, micro-, decilargest,,,, smallest 4. Organize the following prefixes from smallest to largest: milli-, nano-, pico-, micro-, centismallest,,,, largest 5. Why do you suppose most of the selected prefixes have negative exponents? (Hint: Think atoms.) 6. Make a prediction: what prefix do you think is used to describe the size of an atom? Why? Table D: Selected Units 7. What are 2 ways to measure concentration?

2 8. What 3 quantites does joules describe? 9. Identify the symbol for the unit that measures a) length d) pressure b) temperature e) mass c) atomic mass f) volume 10. Identify the name of the unit with the following symbols: a) mol d) ppm b) J e) M c) K f) Pa 11. Organize the unit of time from shortest to longest. shortest,,,, longest 12. Compare the symbol k (found in Table C) with the symbol K (found in Table D). What is the difference? 13. Use Tables C and D to write the following units using prefixes and symbols: Example: centimeter = cm a) milliliter d) microgram b) kilojoule e) picometer c) nanogram f) kilopascal Table E: Selected Polyatomic Ions 14. Identify the polyatomic ions that are cations (positively charged). 15. Identify 3 ions that have the same charge as thiosulfate (S 2 O 2-3 ).

3 16. Identify the elements in each of the following polyatomic ions: a) nitrate b) chlorate c) permanganate d) chromate e) phosphate 17. How are sulfite and sulfate similar? How are they different? 18. Write the chemical formulas for the following compounds (Hint: They all form one-to-one compounds): a) mercury (I) peroxide b) ammonium acetate c) magnesium sulfite d) sodium hypochlorite e) calcium oxalate Table F: Solubility Guidelines for Aqueous Solutions 19. List 3 ions that have no exceptions. 20. List 2 ions that form insoluble compounds with bromide (Br - ). 21. List 2 ions that form soluble compounds with chromate (CrO 2-4 ). 22. Will silver chloride (AgCl) form a soluble compound in water? Why or why not? _ 23. Will calcium carbonate form a soluble compound in water? Why or why not? Table G: Solubility Curves at Standard Pressure 24. What is the independent variable (x-axis)? 25. What is the dependent variable (y-axis)?

4 26. How many solubility curves are displayed on the graph? 27. What is the solubility of NaCl at 90 C? 28. At what temperature is the solubility HCl 72 g solute/100 g H 2 O? 29. At what temperature do KClO 3 and NH 3 have the same solubility? 30. Which compound has the greatest solubility at the lowest temperature? 31. Which compound has the lowest solubility at the highest temperature? 32. Which compounds have the following trend: as temperature increases, solubility decreases? 33. How many more grams of solute can NaNO 3 hold than KCl at 10 C? Table H: Vapor Pressure of Four Liquids 34. What is the independent variable (x-axis)? 35. What is the dependent variable (y-axis)? 36. What are the names of the 4 liquids displayed on the graph? 37. What is the vapor pressure of water at kpa? 38. Which liquid has the highest vapor pressure at the lowest temperature? 39. Which liquid has the lowest vapor pressure at the highest temperature? 40. Why do you suppose there is a dotted line at kpa? (Hint: Look at Table A) 41. If each of these liquids boils at kpa, rank the boiling points of the 4 liquids from lowest to highest. lowest,,, highest Table K: Common Acids 42. What is the chemical formula for nitric acid? 43. What is the name of H 2 CO 3? 44. What is another name for ethanoic acid? 45. What acid does not contain oxygen? 46. What is similar about all of the common acids?

5 47. Develop a rule for determining whether an acid gets ic or ous at the end. Table L: Common Bases 48. What is the chemical formula of aqueous ammonia? _ 49. What is the name of KOH? 50. What is similar about the first 3 common bases? Table P: Organic Prefixes 51. What do the organic prefixes describe? 52. Identify the number of carbon atoms in each of the following organic compounds: a) hexane d) butyne b) octane e) ethanol c) propene f) pentanone Table Q: Homologous Series of Hydrocarbons 53. What are the 3 types of hydrocarbons? 54. What does the note at the bottom of the table tell you? 55. If n=6 what would the chemical formula for each hydrocarbon be? a) alkane b) alkene c) alkyne 56. Classify the following chemical formula as an alkane, alkene or alkyne: a) C 3 H 8 d) C 5 H 8 b) C 4 H 8 e) C 5 H 12 c) C 3 H 4 f) C 2 H 4

Table R: Organic Functional Groups 57. How many classes of compounds are given in the table? 58. What is a similarity between aldehydes, ketones, organic, acids, and esters? 59.

6 Table R: Organic Functional Groups 57. How many classes of compounds are given in the table? 58. What is a similarity between aldehydes, ketones, organic, acids, and esters? 59. What is a similarity between amines and amides? 60. Why do you suppose halides are named halides? (Hint: Think about the name of Group 17 elements) 61. Classify the following compounds by looking at their functional groups: a) d) b) e) c) f) Table S: Properties of Selected Elements 62. What is the source for the information found in the table? 63. Which element has the greatest electronegativity? 64. For elements 76 through 80, which elements have the same size atomic radius? 65. Rank the following elements from greatest to least density: Hg, Ar, O, Y greatest,,, least 66. Rank the following elements from greatest to least ionization energy: F, Na, C, Cu greatest,,, least

7 67. If 298 K is room temperature, list 3 elements that are gases at room temperature? Table T: Important Formulas and Equations 68. What is the density of an object with a mass of 35 grams and a volume of 50 L? 69. Solve for the percent error if the measured value is 1.4 milliliters and the accepted value is 1.5 milliliters. 70. What is the percent composition of oxygen in 1 mole of water? (Hint: 16 g oxygen in 18 g water) 71. If the temperature is 298 K, what is the temperature in Celsius? 72. If the temperature is -40 C, what is the temperature in Kelvin? Periodic Table 73. Color code your periodic table. Metalloids B, Si, Ge, As, Sb, Te, Po Nonmetals everything to the right of the metalloids and hydrogen Metals everything to the left of the metalloids 74. Write the following group names next to their respective groups: Group 1 = alkali metal Group 2 = alkaline earth metal Group 17 = halogens Group 18 = noble gases 75. Write the number of valence electrons above the following groups: Group 1 = 1 Group 15 = 5 Group 2 = 2 Group 16 = 6 Group 13 = 3 Group 17 = 7 Group 14 = 4 Group 18 = 8

4. How much heat does it take to melt 5.0 g of ice? 5. How many grams of water can 10. kj boil into vapor?

4. How much heat does it take to melt 5.0 g of ice? 5. How many grams of water can 10. kj boil into vapor? REFERENCE TABLE REVIEW Since reference table are used so often by scientists and students of science, it is appropriate that high school chemistry students be familiar with them. The tables provided by