Name: ________________________ Class: ___________________ Date: __________
ID: A
2010 Take Home Final Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What SI unit is used to measure the number of representative particles in a substance? a. kilogram b. kelvin c. mole d. ampere 2. Which group of measurements is the most precise? (Each group of measurements is for a different object.) a. 1 g, 3 g, 5 g b. 2 g, 2.5 g, 3 g c. 2.0 g, 3.0 g, 4.0 g d. 2 g, 3 g, 4 g 3. A bond formed between a silicon atom and an oxygen atom is likely to be ____. a. nonpolar covalent b. ionic c. polar covalent d. coordinate covalent 4. What is the approximate frequency of a photon having an energy 5 × 10 −24 J? (h = 6.6 × 10 −34 J⋅s) a. 3 × 10 −58 Hz b. 8 × 10 9 Hz c. 3 × 10 −57 Hz d. 1 × 10 −10 Hz 5. Which of the following theories provides information concerning both molecular shape and molecular bonding? a. Bohr atomic theory b. orbital hybridization theory c. VSEPR theory d. molecular orbital theory 6. What is the volume, in liters, of 0.500 mol of C 3 H 8 gas at STP? a. 0.0335 L b. 22.4 L c. 16.8 L d. 11.2 L 7. Which action changes the identity of the substance referenced? a. melting gold b. running an electric current through copper c. corroding iron d. breaking an ice cube 8. What is the number of moles in 9.63 L of H 2 S gas at STP? a. 0.104 mol b. 3.54 mol c. 0.430 mol d. 14.7 mol 9. The sum of the protons and neutrons in an atom equals the ____. a. mass number b. nucleus number c. atomic mass d. atomic number 10. What is the formula unit of aluminum oxide? a. Al 2 O 3 b. AlO 3 c. AlO d. Al 3 O 11. Elements that are characterized by the filling of p orbitals are classified as ____. a. groups 3A through 8A b. inner transition metals c. transition metals d. groups 1A and 2A 12. How many significant figures are in the measurement 40,500 mg? a. two b. five c. four d. three 13. What is the temperature –34°C expressed in kelvins? a. 339 K b. 139 K c. 207 K d. 239 K 14. Suppose you encounter a chemical formula with H as the cation. What do you know about this compound immediately? a. It is an acid. b. It is a base. c. It is a polyatomic ionic compound. d. It has a +1 charge. 15. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____. a. 38 protons and 38 electrons b. 152 protons and 76 electrons c. 76 protons and 0 electrons d. 76 protons and 76 electrons
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Name: ________________________
ID: A
16. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible? a. mobile electrons b. inner shell electrons c. the electrons closest to the nuclei d. pairs of valence electrons 17. When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____. a. -ite b. -ic c. -ide d. -ate 18. What is the number of moles in 500 L of He gas at STP? a. 90 mol b. 22 mol c. 0.2 mol d. 0.05 mol 19. The smallest particle of an element that retains the properties of that element is a(n) ____. a. neutron b. atom c. proton d. electron 20. A compound held together by ionic bonds is called a ____. a. polar compound b. diatomic molecule c. salt d. covalent molecule 21. For which of the following conversions does the value of the conversion factor depend upon the formula of the substance? a. moles of any substance to number of particles b. mass of any substance to moles c. density of gas (STP) to molar mass d. volume of gas (STP) to moles 22. What is the electron configuration of the iodide ion? a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 d. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 6 23. The quantum mechanical model of the atom ____. a. was proposed by Niels Bohr b. involves the probability of finding an electron in a certain position c. has many analogies in the visible world d. defines the exact path of an electron around the nucleus 24. What is the formula for hydrosulfuric acid? a. HSO 2 b. H 2 S c. H 2 SO 2 d. H 2 S 2 25. Which of the following shows both the correct formula and correct name of an acid? a. HI, iodic acid b. HClO 2 , chloric acid c. HNO 2 , hydronitrous acid d. H 3 PO 4 , phosphoric acid 26. An example of an extensive property of matter is ____. a. hardness b. mass c. pressure d. temperature 27. Which type of solid has the highest melting point? a. network solid b. nonmetallic solid c. metal d. ionic solid 28. Which of the following is NOT a true about atomic mass? a. The atomic mass is the mass of one mole of atoms. b. The atomic mass is 12 g for magnesium. c. The atomic mass is found by checking the periodic table. d. The atomic mass is the number of grams of an element that is numerically equal to the mass in amu. 29. The octet rule states that, in chemical compounds, atoms tend to have ____. a. eight electrons in their principal energy level b. the electron configuration of a noble gas c. more protons than electrons d. more electrons than protons 30. Which of the following measurements (of different masses) is the most accurate? a. 3.122 22 g b. 3.000 000 g c. 3.100 00 g d. 3.1000 g 31. What is the temperature of absolute zero measured in °C? a. –273°C b. –173°C c. –73°C d. –373°C
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Name: ________________________
ID: A
32. Each period in the periodic table corresponds to ____. a. a principal energy level b. a suborbital c. an energy sublevel d. an orbital 33. How many atoms are in 0.075 mol of titanium? a. 4.5 × 10 22 b. 6.4 × 10 2 c. 1.2 × 10-25 d. 2.2 × 10 24 34. What is the correct formula for calcium dihydrogen phosphate? a. Ca(H 2 PO 4 ) 2 b. CaH 2 PO 4 c. Ca 2 H 2 PO 4 d. Ca(H 2 HPO 4 ) 2 35. How many molecules are in 2.10 mol CO 2 ? a. 3.49 × 10 −24 molecules b. 3.79 × 10 24 molecules c. 1.26 × 10 24 molecules d. 2.53 × 10 24 molecules 36. How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration? a. 4 b. 3 c. 2 d. 1 37. The electron configuration of a fluoride ion, F − , is ____. a. 1s 2 2s 2 2p 6 3s 1 b. the same as that of a potassium ion c. the same as that of a neon atom d. 1s 2 2s 2 2p 5 38. What is the correct formula for barium chlorate? a. BaCl 2 b. Ba(ClO) 2 c. Ba(ClO 2 ) 2 d. Ba(ClO 3 ) 2 39. Which set of chemical name and chemical formula for the same compound is correct? a. ammonium sulfite, (NH 4 ) 2 S b. iron(III) phosphate, FePO 4 c. lithium carbonate, LiCO 3 d. magnesium dichromate, MgCrO 4 40. Which of the following CANNOT be classified as a substance? a. gold b. air c. table salt d. nitrogen 41. What is the molar mass of (NH 4 ) 2 CO3? a. 96 g b. 78 g c. 144 g d. 132 g 42. What is the molar mass of AuCl3? a. 303.6 g b. 96 g c. 232.5 g d. 130 g 43. Which of the following is the correct name for N 2 O 5 ? a. nitrous oxide b. dinitrogen pentoxide c. nitrate oxide d. nitrogen dioxide 44. Which of the following is NOT an example of matter? a. water vapor b. air c. heat d. smoke 45. Which of the following shows correctly an ion pair and the ionic compound the two ions form? a. Fe 3 + , O 2 − ; Fe 2 O 3 b. Cr 3 + , I − ; CrI c. Sn 4 + , N 3 − ; Sn 4 N 3 d. Cu 2 + , O 2 − ; Cu 2 O 2 46. What type of hybrid orbital exists in the methane molecule? a. sp b. sp 2 c. sp 3 d. sp 3 d 2 47. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____. a. lower b. unpredictable c. the same d. higher
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Name: ________________________
ID: A
48. Which of the following elements has the smallest atomic radius? a. sulfur b. bromine c. selenium d. chlorine 49. In which of the following sets are the charges given correctly for all the ions? a. K + , Sr 2 + , O 2 − b. Na + , Mg + , Al + c. Rb − , Ba 2 − , P 3 + d. N − , O 2 − , F 3 − 50. The shape of the methane molecule is called ____. a. square b. tetrahedral c. four-cornered d. planar 51. Which type of electromagnetic radiation includes the wavelength 10 −7 m? a. microwave b. gamma ray c. visible light d. radio wave 52. A theory is a ____. a. well-tested explanation for a broad set of observations b. procedure used to test a proposed explanation c. summary of the results of many observations d. proposed explanation for an observation 53. What is the number of moles in 432 g Ba(NO 3 ) 2 ? a. 0.237 mol b. 1.65 mol c. 0.605 mol d. 3.66 mol 54. The expression of 5008 km in scientific notation is ____. a. 5.008 × 10 4 km b. 5.008 × 10 −3 km c. 5.008 × 10 3 km d. 50.08× 10 −4 km 55. Which of the following are considered physical properties of a substance? a. malleability and hardness b. color and odor c. melting and boiling points d. all of the above 56. The light given off by an electric discharge through sodium vapor is ____. a. a continuous spectrum b. an emission spectrum c. of a single wavelength d. white light
Prefix mega (M) kilo (k) deci (d) centi (c) milli (m) micro (μ) nano (n) pico (p)
Commonly Used Metric Prefixes Meaning 1 million times larger than the unit it precedes 1000 times larger than the unit it precedes 10 times smaller than the unit it precedes 100 times smaller than the unit it precedes 1000 times smaller than the unit it precedes 1 million times smaller than the unit it precedes 1000 million times smaller than the unit it precedes 1 trillion times smaller than the unit it precedes
Factor 10 6 10 3 10 −1 10 −2 10 −3 10 −6 10 −9 10 −12
57. What is the quantity 0.0075 meters expressed in centimeters? Use the table above to help you. a. 0.75 cm b. 0.075 cm c. 70.5 cm d. 7.5 cm 58. How many moles of CaBr 2 are in 5.0 grams of CaBr 2 ? a. 4.0 × 10 1 mol b. 1.0 × 10 3 mol c. 4.2 × 10 −2 mol d. 2.5 × 10 −2 mol 59. When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the number of significant figures in ____. a. the most precise measurement b. the least precise measurement c. the least and most precise measurements d. all of the measurements
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Name: ________________________
ID: A
60. The atomic masses of any two elements contain the same number of ____. a. milliliters b. ions c. grams d. atoms 61. The shape (not the size) of an electron cloud is determined by the electron's ____. a. energy sublevel b. position c. speed d. principal quantum number 62. To what category of elements does an element belong if it is a poor conductor of electricity? a. metals b. nonmetals c. metalloids d. transition elements 63. Isotopes of the same element have different ____. a. atomic numbers b. numbers of neutrons c. numbers of electrons d. numbers of protons 64. When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the ____. a. hydrogen region of the molecule b. oxygen region of the molecule c. H—O—H plane of the molecule d. geometric center of the molecule 65. In any chemical compound, the elements are always combined in the same proportion by ____. a. charge b. volume c. mass d. density 66. All atoms of the same element have the same ____. a. mass numbers b. number of neutrons c. number of protons d. mass 67. Once formed, how are coordinate covalent bonds different from other covalent bonds? a. They are weaker. b. They are stronger. c. They are more ionic in character. d. There is no difference. 68. Which of the following statements is false? a. Chemistry explains many aspects of nature. b. Studying chemistry ensures that officials make correct choices in funding technology. c. Knowledge of chemistry allows the public to make informed decisions. d. Knowledge of chemistry helps prepare people for careers in soil science. 69. Which of the following elements exists as a diatomic molecule? a. sulfur b. nitrogen c. lithium d. neon 70. In the Bohr model of the atom, an electron in an orbit has a fixed ____. a. color b. size c. position d. energy 71. What is the mass in grams of 5.90 mol C 8 H 18 ? a. 673 g b. 0.0512 g c. 389 g d. 19.4 g 72. Which of the following is NOT a characteristic of most ionic compounds? a. They are composed of metallic and nonmetallic elements. b. They have low melting points. c. When melted, they conduct an electric current. d. They are solids. 73. Which combination of temperature and pressure correctly describes standard temperature and pressure, STP? a. 0°C and 22.4 kPa b. 100°C and 100 kPa c. 1°C and 0 kPa d. 0°C and 101 kPa 74. What is true about the molar mass of chlorine gas? a. The molar mass is 71.0 g. b. The molar mass is 35.5 g. c. The molar mass is equal to the mass of one mole of chlorine atoms. d. none of the above 75. What does an -ite or -ate ending in a polyatomic ion mean? a. Oxygen is in the formula. b. Sulfur is in the formula. c. Nitrogen is in the formula. d. Bromine is in the formula.
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Name: ________________________
ID: A
76. All of the following are physical properties of matter EXCEPT ____. a. ability to rust b. color c. melting point d. mass 77. The particles that are found in the nucleus of an atom are ____. a. protons and electrons b. electrons only c. neutrons and electrons d. protons and neutrons 78. What is the density at STP of the gas sulfur hexafluoride, SF 6 ? a. 0.153 g/L b. 3270 g/L c. 6.52 g/L d. 3.93 × 10 24 g/L 79. All of the following are equal to Avogadro's number EXCEPT ____. a. the number of atoms of bromine in 1 mol Br 2 b. the number of atoms of gold in 1 mol Au c. the number of molecules of carbon monoxide in 1 mol CO d. the number of molecules of nitrogen in 1 mol N 2 80. The atomic mass of an element is the ____. a. weighted average of the masses of the isotopes of the element b. average of the mass number and the atomic number for the element c. total number of subatomic particles in its nucleus d. total mass of the isotopes of the element 81. An ionic bond is a bond between ____. a. a cation and an anion b. the ions of two different metals c. valence electrons and cations d. the ions of two different nonmetals 82. When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____. a. ionic covalent bond b. coordinate covalent bond c. unequal covalent bond d. one-sided covalent bond 83. Which of the following elements has the smallest first ionization energy? a. sodium b. calcium c. potassium d. magnesium 84. Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen? a. S b. O c. C d. Na 85. The modern periodic table is arranged in order of increasing atomic ____. a. number b. charge c. mass d. radius 86. The letter "p" in the symbol 4p 3 indicates the ____. a. spin of an electron b. orbital shape c. speed of an electron d. principle energy level 87. Which state of matter is characterized by having an indefinite shape, but a definite volume? a. liquid b. gas c. solid d. none of the above 88. Which of the following is a heterogeneous mixture? a. soil b. air c. steel d. salt water 89. A substance that can be separated into two or more substances only by a chemical change is a(n) ____. a. compound b. solution c. element d. mixture 90. What are quanta of light called? a. excitons b. charms c. muons d. photons 91. How are bases named? a. like monatomic elements b. like polyatomic ions c. like molecular compounds d. like ionic compounds 92. What is the correct name for Sn 3 (PO 4 ) 2 ? a. tin(IV) phosphate b. tritin diphosphate c. tin(III) phosphate d. tin(II) phosphate
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Name: ________________________
ID: A
93. The volume of one mole of a substance is 22.4 L at STP for all ____. a. liquids b. compounds c. solids d. gases 94. How many moles of tungsten atoms are in 4.8 × 10 25 atoms of tungsten? a. 8.0 × 10 1 moles b. 1.3 × 10 −1 moles c. 1.3 × 10 −2 moles d. 8.0 × 10 2 moles 95. The molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____. a. liquid b. solid c. element d. gas at STP 96. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? 1. 20 E 2. 20 E 3. 219 E 4. 21 E 10 11 10 a. 1 and 2 b. 2 and 3 c. 1 and 4 d. 3 and 4 97. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C 3 H 7 O? a. 5 b. 5 × (6.02 × 10 23 ) c. 35 d. 35 × (6.02 × 10 23 ) 98. Which step in the scientific method requires you to use your senses to obtain information? a. designing an experiment b. stating a theory c. making an observation d. revising a hypothesis 99. Avogadro's number of representative particles is equal to one ____. a. kelvin b. kilogram c. gram d. mole Multiple Response Identify one or more choices that best complete the statement or answer the question. 100. 9.0 grams of Beryllium contains the same number of representative particles as a. 44.0 grams of CO2. b. 16.0 grams of O2. c. 32.0 grams of CH3OH. d. 4.0 grams of elemental Hydrogen.
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