sign in sign up
<<
Home , Potassium sulfide

Worksheet 1 – Matter & Measurement MCQ Name: ______

1. The element chromium has as its chemical symbol A. C B. Co C. Cr D. Cu

2. The symbol “S” is used to represent the element: A. silicon B. sodium C. sulfur D. tin

3. An example of a chemical compound is A. air B. brass C. granite D. table salt

4. The two major types of pure substances are: A. compounds and solutions B. compounds and elements C. solutions and elements D. solutions and mixtures

5. A sample cannot be separated into two or more substances by physical means. It must be, A. a compound B. an element C. either a compound or an element D. a mixture

6. All of the following properties of a sample of a pure substance can be used for identification except its A. mass B. density C. melting point D. in 100 g of water

7. A chemical reaction is used to separate A. a compound into its elements B. a mixture into its components C. gases from liquidsD. solids from liquids

8. Distillation can readily be used to separate A. the elements in a compound B. a dissolved solid in a liquid C. a heterogeneous mixture of two solids D. a homogeneous solution of two solids

9. The mass of a sample is 0.00158 g. The number of significant figures in this measurement is A. 1 B. 3 C. 5 D. 6

10. The mathematical operation, [(6.075 - 5.12) + 14.4661 g, yields A. 15 g B. 15.4 g C. 15.42 g D. 15.421 g

11. The mathematical operation, [(13.76 + 1.0078)(0.0155)] g, yields A. 0.23 g B. 0.229 g C. 0.2289 g D. 0.22890 g

12. A beaker's mass is 21.05 g, while the mass of this beaker containing a sample of water is 22.15 g. The mass of the water sample is A. 1 g B. 1.1 g C. 1.10 g D. 1.100 g

13. The number of millimeters (mm) in one kilometer (km) is A. 10 B. 10 3 C. 10 6 D. 10 9

14. Another way to express the volume 0.0087 L is with A. 8.7 x 10 -3 L B. 8.7 x 10 -2L C. 8.7 x 10 2 L D. 8.7 x 10 3 L

15. A car travels a distance of 638 kilometers. This distance in feet is A. 0.0751 B. 0.194 C. 2.09 x 10 6 D. 5.42 x 10 6

16. Another way to express a mass of 25.3 mg is by A. 2.53 x 10 -2 g B. 2.53 x 10 -1 kg C. 253 lb D. 2530 cg

AP Chemistry Chapters 1&2 Worksheets Page 1 17. Some units of pressure and their relations are: 1 atm = 1.01325 x 10 5 Pa = 760 torr. If a gas cylinder is pressurized to 542 atm, it could be recorded as A. 0.713 torr B. 4.12 x 10 5 torr C. 5.49 x 10 4 Pa D. 5.35 x 10 -3 Pa

18. Determine the combined length of a 10.12 inch rod and a 6.0 x 10 2 inch rod A. 7.13 x 10 2cm B. 15.49 x 10 2 cm C. 1.5 x 10 3 cm D. 4.6 x 10 3cm

19. As units of energy 1 calorie equals 4.184 joules; convert 8.522 calories to joules. A. 2.497 x 10 -3 joules B. 2.037 joules C. 35.66 joules D. 9.770 joules

20. An individual weighs 92.3 kg; this person's weight in pounds is A. 36 B. 42 C. 98 D. 203

21. The amount of milliliters in 2.5 gallons is, A. 0.0106 B. 2.4 x 10 3 C. 9.5 x 10 3 D. 1.06 x 10 4

22. A certain chemical procedure requires 52.6 cm of iron wire. How many feet of iron wire are required? A. 1.73 B. 11.1 C. 249 D. 1.60 x 10 2

23. There are 4047 m 2 in one acre; determine the area of a 254 acre tract of land in square kilometers. A. 6.28 x 10 -3 B. 1.03 C. 62.8 D. 1.03 x 10 3

24. Several units of mass which are specific to precious metals and gems are provided: 1 carat = 0.200 gram, 1 grain = 0.0648 gram, 24 grains = 1 pennyweight. Determine the difference in mass (in grams) between 24.56 pennyweight of silver and 18.9 carats of diamond. A. 34.42 g B. 52.8 g C. 78.7 g D. 9092 g

25. A pool is filled with water by a hose that delivers water at a flow rate of 1.0 gal/sec. The equivalent flow rate in units of L/min is A. 14 B. 16 C. 57 D. 2.3 x 10 2

26. If pollution due to oxides of nitrogen is at the level of 1.5 x 10 -9 kg/L, how many grams of nitrogen oxides are inhaled with one hundred in 3 of air? A. 2.5 x 10 -6 g B. 4.2 x 10 5 g C. 9.5 x 10 -9 g D. 1.1 x 10 12 g

27. A 58.7 gram sample of an alloy containing 55% copper by mass is prepared. The amount of copper used in this preparation is A. 26 g B. 32 g C. 107 g D. 114 g

28. A 1.28 g sample of copper is heated with sulfur to produce 1.60 g of a compound containing both copper and sulfur. The mass percentage of sulfur in this compound is A. 20% B. 40% C. 60% D. 80%

29. If a steel rod is 1.50% (by mass) carbon and has a mass of 2.50 kg per meter of rod, how many grams of carbon would be found in a 10.0 meter length of rod? A. 375 g B. 167 g C. 150 g D. 0.0600 kg

30. The LD 50 for a chemical is the dose expected to be lethal for 50% of the population. The LD 50 , for sodium cyclamate is 17.0 g per kg of body weight. If an average can of diet soda contains 96 mg of sodium cyclamate and an average adult human weighs 7.0 x 10 1 kg; determine the number of cans of diet soda that must be consumed to achieve the LD 50 . A. 0.40 B. 43 C. 1.14 x 10 3 D. 1.2 x 10 4

AP Chemistry Chapters 1&2 Worksheets Page 2

31. A swimming pool is 60.0 feet long by 25.0 feet wide and is 8.0 feet deep. The water in this pool is treated with chlorine as a disinfectant. If the concentration of chlorine is 0.070% chorine by mass and the density of the water is 1.0 g/cm 3, how many grams of chlorine must be used to treat the pool? A. 2.8 x 10 1 B. 2.6 x 10 2 C. 2.6 x 10 4 D. 2.4 x 10 5

32. The temperature of a system is measured to be 75.4°F. An equivalent temperature would be A. 59.6°C B. 78.1°C C. 297.2K D. 332.7K

33. The boiling point of chlorine is -34.6°C. This temperature expressed in K is A. -30.3 B. 177.4 C. 238.5 D. 307.6

34. The melting point of methanol is -98°C, and its boiling point is 65°C. At room temperature, 70°F, this compound exists as a A. solid B. liquid C. gas D. solid-liquid mixture

35. The mass of a metal cylinder is 21.97 g, and its volume is 11.2 mL. The density of this metal is A. 0.510 g/mL B. 0.542 g/mL C. 1.00 g/mL D. 1.96 g/mL

36. Which would occupy the largest volume? A. 500 g of carbon tetrachloride; density = 1.6 g/mL B. 500 g of benzene; density 0.88 giml C. 500 g of n-heptane; density = 0.68 g/mL D. They will all be the same.

37. The density of lead metal is 11.3 g/mL. The volume of a 53.45 g piece of this metal is A. 4.73 mL B. 211 mL C. 603 mL D. 274 mL

38. The density of aluminum is 2.699 g/mL. If a block of pure aluminum occupies 25.6 mL, its mass in pounds is A. 0.152 B. 69.1 C. 4.31 x 10 3 D. 3.14 x 10 4

39. The density of methanol is 0.8127 g/mL. An equivalent expression of this density in pounds per cubic inch is A. 0.02963 B. 0.1493 C. 4.228 D. 13.32

40. How much water (density = 1.0 g/mL) will be lost from a full container if 52.5 grams of silver (density = 10.5 g/mL) are placed in the container? A. 0.2 g B. 5.0 g C. 62.7 g D. 551 g

41. A student collects the following data on a piece of metal by weighing it on a piece of paper and measuring the volume of water displaced in a graduated cylinder. mass paper = 0.452 g, mass paper + metal = 72.943 g, volume water = 15.2 mL, volume water + metal = 19.0 mL. The density of this metal is A. 2.15 g/mL B. 3.84 g/mL C. 4.80 g/mL D. 19 g/mL

42. The solubility of calcium chloride is 74.5 g per 100.0 g of water at 20°C. The amount of water needed to dissolve 271 g of calcium chloride at 20°C is A. 202 g B. 345 g C. 364 g D. 446 g

43. The solubility of nickel chloride is 64.2 grams in 100 cm 3 of water at 20°C. Determine the gallons of water needed to dissolve 3.0 pounds of nickel chloride at this temperature A. 0.56 B. 2.2 C. 23 D. 1105

AP Chemistry Chapters 1&2 Worksheets Page 3 AP Chemistry Chapters 1&2 Worksheets Page 4 Worksheet 2 –Atoms, Molecules & Ions MCQ Name: ______

1. One element that might be expected to have chemical properties similar to arsenic would be A. Germanium, Ge B. Selenium, Se C. Antimony, Sb D. Krypton, Kr

2. One isotope with 24 neutrons is A. B. C. D.

3. An ion of possesses A. 15 electrons B. 18 electrons C. 19 electrons D. 20 electrons

4. The number of protons in 37 Cl - is A. 1 B. 17 C. 18 D. 37

5. The proper name for P 4010 is A. phosphorus oxide B. tetraphosphorus decaoxide C. quantraphosphorus octaoxide D. phosphorus(IV) oxide

6. The compound copper (II) nitrate would have the formula A. CuNO 3 B. Cu 2NO 3 C. Cu(NO 3)2 D. Cu 2NO 2

7. Predict the formula of the ionic compound formed by magnesium and oxygen. A. MgO B. MgO 2 C. Mg 2O D. Mg 2O2

8. An estimate of the size. of atoms can be given by diameters of A. 10 -10 m (0.1 nm) B. 10 -7 m (0.1 mm) C. 10 -4 m (0.1 cm) D. 10 -1 m

9. The smallest unit of a compound that still maintains the chemical properties of that compound is the A. electron B. nucleus C. atom D. molecule

10. The relative number of atoms of each element in a particular compound, A. is always 1:1 B. is definite and constant C. is the same as the weight ratio D. cannot be determined experimentally

11. The following set of data for a compound best illustrates what law? Expt Mg Cl Mg/Cl 1 24.0 g 71.0 g 0.338 2 12.0 g 35.5 g 0.338 A. multiple proportions B. definite composition C. conservation of mass D. polyatomic ions

12. The law of multiple proportions is illustrated by the following pair of substances: A. PCl 3, PCl 5 B. KCl, CaCl 2 C. CH 2O, C 6H12 O6 D. H2O, D 2O (where D is an isotope of hydrogen)

13. Which of the following contribute charge but NOT significant mass to an atom? A. protons B. neutrons C. electrons D. nuclei

14. The atomic particles found in the nucleus of an atom are A. electrons and protons B. neutrons and isotopes C. neutrons and electrons D. neutrons and protons

15. Most of the volume of an atom is occupied by the space required for the A. electrons B. protons C. nucleus D. neutrons

16. Lithium, sodium, potassium, and rubidium are all members of the A. alkali metals B. alkaline earth metals D. transition metals D. halogens

17. Sodium, magnesium, aluminum, and chlorine are all elements in the same A. family B. group C. alkali metals D. period

18. Argon is a member of the A. alkaline earths B. halogens C. metals D. noble gases

AP Chemistry Chapters 1&2 Worksheets Page 5 19. An example of an element that can be classified as a metalloid is A. arsenic B. cobalt C. sodium D. sulfur

20. All atoms of a given isotope of the same element A. possess the same mass B. possess the same chemical properties C. have the same atomic number D. all the above

21. Uranium exists in several isotopes; the different isotopes have different numbers of A. protons B. neutrons C. electrons D. atomic numbers

22. An atom with 35 protons and 45 neutrons would be an isotope of the element A. rhodium, Rh B. neon, Ne C. mercury, Hg D. bromine, Br

23. Atoms of mercury possess A. 2 electrons B. 80 electrons C. 120 electrons D. 200 electrons

24. The atomic number of an element is 68; this means the atoms of this element possess A. 68 neutrons B. 68 isotopes C. 68 protons D. 68 neutrons and protons

25. The isotope has A. 26 protons, 26 electrons, 26 neutrons B. 26 protons, 29 electrons, 26 neutrons C. 26 protons, 26 electrons, 29 neutrons B. 29 protons, 26 electrons, 26 neutrons

26. The isotope has in its nucleus A. 24 neutrons B. 28 neutrons C. 28 protons D. 52 neutrons

27. A molecule of fluorine gas is typically written as, A. F B. F 2 C. F 4 D. F 8

28. An example of an anion is A. F - B. Na + C. Ca D. O

29. The isotope + contains how many electrons? A. 0 B. 1 C. 2 D. 3

30. Magnesium typically forms ions of this charge: A. -2 B. -1 C. +1 D. +2

31. The oxide ion possesses A. 6 electrons B. 8 electrons C. 10 electrons D. 16 electrons

32. Both + and - have the same number of A. protons B. neutrons C. electrons D. protons + neutrons

33. The number of atoms in the formula (NH 4)3PO 4 is A. 2 B. 4 C. 10 D. 20

34. The simplest formula of the molecule P 4O10 is A. PO B. P 2O5 C. P 4O10 D. P8O20

35. Hydrazine has NH 2 as its simplest formula. Each molecule contains four hydrogen atoms; accordingly its molecular formula is A. NH 2 B. 2NH 2 C. (NH 2)4 D. N 2H4

36. The proper name for the compound with the formula K 2S is A. potassium B. dipotassium monosulfide C. D. potassium(II) sulfite

AP Chemistry Chapters 1&2 Worksheets Page 6 37. The for calcium nitride is, A. CaN B. Ca 2N C. CaN 2 D. Ca 3N2

38. The chemical formula for dinitrogen pentoxide is A. NO B. N 2O5 C. N 5O2 D. N 3O4

39. The chemical formula of methane is A. CH 4 B. NH 3 C. H 2O2 D. Cl 2

40. All of the following anions carry a -2 charge except A. sulfate B. nitrate C. carbonate D. chromate

41. The acetate ion is 2- - + - A. CO 3 B. CN C. NH 4 D. C 2H3O2

42. Aqueous solutions of HCl, HNO 3, H 2SO 4, and HClO are all A. acids B. alkalis C. binary ionic compounds D. oxoanions

43. Sodium carbonate has the chemical formula A. SCO 3 B. S 2CO 3 C. Na 4C D. Na 2CO 3

44. The chemical formula for ammonium sulfate is A. AmSO 4 B. (NH 4)2S C. (NH 4)2SO 4 D. NH 4SO 4

45. The number of oxygen atoms in two hydroxide ions is A. 0 B. 1 C. 2 D. 4

46. The proper name for the compound with the formula Fe(NO 3)2 is, A. iron nitride B. iron dinitrate C. iron(I) nitrate D. iron(II) nitrate

47. The correct name for the compound Co(OH) 3 is A. cobalt hydrate B. cobalt(I) oxyhydride C. cobalt(III) trioxyhydride D. cobalt(III) hydroxide

48. An aqueous solution of HNO 3 is referred to as A. nitric acid B. nitrogen hydroxide C. hydrogen nitride D. hydronitrate acid

49. The chemical formula for hydroiodic acid is A. HI B. HIO C. HIO 2 D. HIO 3

50. CaSO 4·1/2H 2O is in a general class of compounds called A. hydrates B. acids C. clathrates D. oxoacids

AP Chemistry Chapters 1&2 Worksheets Page 7 AP Chemistry Chapters 1&2 Worksheets Page 8 Worksheet 3 – Stoichiometery MCQ Name: ______

1. The element rhenium consists of atoms of two isotopes: 185 Re of mass 184.953 amu and 187 Re of mass 186.956 amu. If the average atomic mass of rhenium is 186.207 amu, what is the percent natural abundance of the heavier rhenium isotope? A. 37.39% B. 50.00% C. 62.61% D. 99.60%

2. The number of grams of Co(NO 3)2 in 0.456 mole of this compound is, A. 7.57 x 10 25 B. 0.00249 C. 83.4 D. 2.75 x 10 23

3. What is the mass percent of sodium in sodium sulfate, Na 2SO 4? A. 16.19% B. 19.33% C. 28.57% D. 32.37%

4. If 1.54 grams of an oxide of osmium (Os) are analyzed and found to contain 1.15 grams of osmium, the simplest formula of this compound is A. OsO B. OsO 2 C. Os 2O D. OsO 4

5. The atomic mass of Al on the carbon-12 stale is 27.0 amu. If a new scale were established with carbon-12 assigned an atomic mass of 4.00 amu, the atomic mass of Al on the new scale would be, in atomic mass units, A. 3.00 B. 9.00 C. 27.0 D. 81.0

6. Suppose a hypothetical element (symbol = Z, atomic number = 107) is suggested to exist as two isotopes: 86.95% as 264 Z of mass 263.992 amu and 13.05% as 266 Z of mass 265.990 amu. Determine the atomic mass of Z. A. 264.253 amu B. 264.261 amu C. 264.562 amu D. 265.000 amu

7. Antimony (Sb) occurs naturally in two major isotopic forms: 121 Sb with 120.9038 amu and 123 Sb with mass 122.9041 amu. Determine the percentage natural abundance of the 121 Sb isotope, if the weighted average atomic mass is 121.75 amu for antimony. A. 42.3% B. 50.0% C. 57.7% D. 99.3%

8. One mole of atomic He contains A. 4.002 neutrons B. 2 molecules C. 8 grams D. 6.02 x 1023 atoms

9. Determine the number of atoms of sulfur in 2.5 moles of sulfur. A. 4.2 x 10 24 B. 2.5 C. 4.7 x 10 22 D. 1.5 x 10 24

10. How many atoms of carbon are there in 0.80 moles of C 6H12 O6? A. 4.8 x 10 23 atoms B. 6.02 x 10 23 atoms C. 2.9 x 10 24 atoms D. 3.6 x 10 24 atoms

11. Determine the formula mass of calcium phosphate, Ca 3(PO 4)2. A. 87.05 amu B. 134.99 amu C. 279.21 amu D. 310.18 amu

12. A sample of molecular hydrogen massing 1.008 g contains the same number of atoms as A. 16.00 g of oxygen gas B. 12.00 g of 12 C C. both of the above D. none of the above

13. Determine the number of moles of NaC1 in 454 grams of sodium chloride. A. 7.77 B. 2.65 x 10 4 C. 4.68 x 10 24 D. 2.73 x 10 26

2 14. Determine the number of molecules of sucrose in 2.00 x 10 grams of sucrose, C 12 H22 O11. A. 0.585 B. 6.84 x 10 6 C. 3.52 x 10 23 D. 1.20 x 10 6

15. Determine the mass in grams of one molecule of iodine, I 2 A. 1.66 x 10 -26 B. 4.22 x 10 -22 C. 253.81 D. 2.37 x 10 21

16. Calculate the number of molecules of vitamin A, C 20 H30 O, in 1.5 milligrams of this compound. A. 3.2 x 10 18 B. 9.0 x 10 26 C. 3.2 x 10 21 D. 2.6 x 10 23

17. The molar mass of ammonium chromate is A. 78 g/mole B. 102 g/mole C. 134 g/mole D. 152 g/mole

AP Chemistry Chapters 1&2 Worksheets Page 9 18. How many moles of zinc (Zn) are in a cube of the metal (density = 7.14 g/cm 3) with dimensions of 5.00 x 10 -3 cm by 10.0 cm by 10.0 cm? A. 2.29 x 10 -4 moles B. 5.46 x 10 -2 moles C. 0.109 moles D. 18.3 moles

19. Calculate the mass percent chlorine in the compound CC1 2F2, a compound that may nave detrimental effects on the ozone layer in the upper atmosphere, A. 33.33% B. 40.00% C. 53.34% D. 58.64%

20. Consider the three compounds: sodium carbonate {Na 2CO 3}, calcium carbonate {CaCO 3} and iron (II) carbonate (FeCO 3). With respect to the mass percent oxygen in each compound, A. all have the same mass% oxygen B. Na 2CO 3 has the greater mass% oxygen C. CaCO 3 has the greater mass% oxygen D. FeCO 3 has the greater mass% oxygen

21. Of the compounds listed, which has the highest percentage of nitrogen by mass A. NH 3 B. Cu(NH 3)4SO 4 C. Fe(NO 3)2 D. NH 4NO 3

22. Metallic sodium can be obtained by high temperature electrolysis of sodium chloride. How many pounds of sodium can be produced from 5.00 x 10 2 pounds of NaCI? A. 197 B. 250 C. 303 D. 500

23. Tungsten metal {W} can be produced by the reaction of tungsten (VI) oxide {WO 3} with hydrogen. How many grams of tungsten can be obtained from 4.52 kilograms of tungsten (VI) oxide? A. 19.5 B. 79.3 C. 936 D. 3.58 x10 3

24. A 0.500 gram sample of citric acid containing only carbon, hydrogen and oxygen is burned to produce 0.687 g of CO 2 and 0.187 g of H2O. These data can be used to calculate the mass percent, A. carbon to be 72.8% B. oxygen to be 69.7% C. oxygen to be 58.3% D. hydrogen to be 37.5%

25. Combustion of a 0.4000 g sample of a compound composed only of carbon, hydrogen, and oxygen produced 0.5996 g of CO 2 and 0.1638 g of H 2O. Determine the weight percent of carbon in this compound. A. 40.91% B. 54.52% C. 66.71% D. 78.54%

26. Determine the simplest formula for a compound that contains the following composition by mass: 32.79% sodium, 13.02% aluminum, and 54.19% fluorine. A. Na 5AlF 8 B. Na 4Al 2F7 C. Na 3AlF 6 D. Na 2AlF 3

27. A compound containing only carbon, nitrogen, and hydrogen is analyzed to contain 58.82% carbon, 27.45% nitrogen, and 13.73% hydrogen (by mass). Its simplest formula is A. C 5N2H14 B. C 4N2H C. C 5NH 7 D. C4NH 10

28. When a 1.50 g sample of a compound containing only carbon and sulfur is burned, 0.87 g of CO 2 and 2.53 g of SO 2 are produced. Determine the simplest formula of this compound. A. CS B. C 2S C. CS 2 D. CS 3

29. A compound has a simplest formula of CH 2N and a molar mass of 84 g/mole. Its molecular formula is, A. CH 2N B. C 2H4N4 C. C 3H6N3 D. C4H8N2

30. A certain compound contains 78.2% boron and 21.8% hydrogen by mass. The molar mass of this compound is about 25±5 g/mole. The molecular formula is A. BH 3 B. B 2H2 C. B 2H6 D. B 2H8

AP Chemistry Chapters 1&2 Worksheets Page 10