Chemistry: Principles And Reactions, 7th Edition Test Bank

Chapter 2–Atoms, Molecules, and Ions Student: Which of the following statements is/are postulates of Dalton’s atomic theory? 1. Elements are composed of tiny particles called atoms. 2. No atom is changed into another element in an ordinary chemical reaction. 3. Compounds are formed when two or more atoms combine. A. 1 only B. 2 only C. 3 only D. l and 3 E. 1,2 and 3 J.J. Thomson determined that electrons are small, negatively charged particles by A. bombarding gold foil with alpha particles. B. exposing photographic plates to radioactive uranium. C. deflecting cathode rays with electric and magnetic fields. D. converting cathode rays to electron particles using a fluorescent screen. E. decomposing neutrons into protons and electrons. Which of the following statements is/are CORRECT? l. A neutron is an uncharged particle with a mass slightly greater than a proton. 2. The nucleus of an atom has a negative charge. 3. More than 99.9% of an atom’s mass is concentrated in the electron cloud surrounding the nucleus. A. 1 only B. 2 only C. 3 only D. l and 3 E. 1,2 and 3 Rank the subatomic particles from least to greatest mass. . electrons = neutrons = protons . electrons = protons < neutrons . electrons < neutrons = protons . electrons < protons < neutrons . electrons < neutrons 10. All ofthe following statements are true EXCEPT A. all atoms of a given element have the same mass number. B. for any neutral element, the number of electrons is equal to the number ofprotons. C. the mass number is the sum of the number ofprotons and neutrons. D. isotopes of atoms contain the same number ofprotons but a different number of neutrons. E. the atomic number equals the number of protons in an atom. All atoms of the same element have the same number of . A. neutrons B. protons C. protons and neutrons D. electrons and neutrons E. protons, neutrons, and electrons What is the mass number of an argon atom with 22 neutrons? A. 2 B. 18 C. 22 D. 40 E. 39.95 Which of the following atoms contains the fewest protons? 232Th ‘ 231 Pa 245Pu . 238U 232 meow> Pa How many protons, neutrons, and electrons are in a silver atom with a mass number of 108? A. 47 protons, 47 neutrons, 61 electrons B. 47 protons, 61 neutrons, 47 electrons C. 61 protons, 47 neutrons, 47 electrons D. 47 protons, 108 neutrons, 47 electrons E. 61 protons, 108 neutrons, 61 electrons F-20, a radioactive isotope of fluorine, has A. 9 protons, 10 neutrons, and l electron. B. 9 protons, 10 neutrons, and 9 electrons. C. 9 protons, ll neutrons, and 9 electrons. D. 10 protons, 9 neutrons, and l electron. E. 10 protons, 10 neutrons, and 10 electrons. 11. Which two atoms below have the same number of neutrons? 15 1:5 2U 20 E 30’ ED’ QF’ IUHE’ 11 HE A. 1SDand 1:0 B. 1Egandfima C. EElrand fig HE D. EEFandfiHa E. 3’3 and22 1:: He 11 Ma 12. What is the atomic symbol for an element with 39 protons and 50 neutrons? A. ”511: Ha B. $11? 0- :3 v D- $511 37″ E. 35′ Al: 13. Which two of the ions below have the same number of electrons? 132′ -112 2+ 225′ 2+ 2|]? 4+132′ 2+ 53195,1,511 9331313 9321313 95533 A. 13? —and135′ – 3+ 53 5|)” can? “and”? 2+ 3213b 5533 D. 1:3 SI12+ and 1:: 2+ 633 E. 225′ 2+ d2ll’l’ 4+ 33 121:. an E; 121:. 14. Two isotopes of a given element Will have the same number of , but a different number of in their nucleus. A. protons, electrons B. electrons, protons C. protons, neutrons D. neutrons, protons E. electrons, neutrons 15. Which of the following are a pair of isotopes? A. :3 Far and :3 K B. :3 [:3 and :3 K C. 1331. and :3 Er D. 4U 35′ EU [:3 and 15′ K E. :3 [:3 andgfi [:3 16. Which species has 63 neutrons? 112 A. 431321 112 B’ 45, In C. ‘3 3&1 D. 1:: Ell E. none of the above 17. Two isotopes of chlorine are found in nature, Cl-35 and Cl-37. The average mass of chlorine is 35.45 amu. The more abundant isotope of Cl has A. 17 protons, l7 electrons, and 18 neutrons. B. 17 protons, l7 electrons, and 18.45 neutrons. C. 17 protons, l7 electrons, and 20 neutrons. D. 18 protons, 18 electrons, and 17 neutrons. E. 19 protons, l9 electrons, and 16 neutrons. 18. 19. 20. 21. What is the identity of55 E? 25 . zinc . silver . iridium . cesium . manganese mUOUUD> What is the symbol for an element which contains 57 neutrons and has a mass number of 101? A. Er B. Ru C. Md D. La E. Os Rubidium has two naturally occurring isotopes. The average mass of Rb is 85.4678 amu. If 72.15% of Rb is found as Rb-85 (84.9117 amu), what is the mass of the other isotope? A. 0.56 amu B. 85.68 amu C. 86.91 amu D. 86.02 amu E. 83.47 amu Silver has two stable isotopes with masses of 106.90509 amu and 108.9047 amu. The average molar mass of silver is 107.868 amu. What is the percent abundance of each isotope? A. 50.0% Ag-107 and 50.0% Ag-109 B. 51.8% Ag-107 and 48.2% Ag-109 C. 55.4% Ag-107 and 44.6% Ag-109 D. 48.2% Ag-107 and 51.8% Ag-109 E. 44.6% Ag-107 and 55.4% Ag-109 22. Gallium has an average atomic mass of 69.7 amu. In a typical sample, 60.4% of Ga exists as Ga-69 (68.9257 amu). What is the identity and the atomic mass of the other isotope? A. :‘i [33; 70.9 amu B. :‘i [33; 70.9 amu C. :1 [33; 70.9 amu D. 7″1 G ;71.9 amu 31 a E. 3 [33; 71.9 amu 23. An element has three naturally occurring isotopes with the following abundances and masses: amu 8.99% .985042 0.00% 4.985837 1.01% .982593 Determine the molar mass of the element. A. 24.31 g/mol B. 24.98 g/mol C. 74.95 g/mol D. 2431 g/mol E. none of the above 24. The average molar mass of lithium is 6.941. A sample of lithium consists of two isotopes with masses of 6.01512 amu and 7.01600 amu. Determine the percent abundance of each isotope. A. 7.49% Li-6 and 92.51% Li—7 B. 8.45% Li-6 and 91.55% Li—7 C. 12.49% Li-6 and 87.51% Li—7 D. 91.55% Li-6 and 8.45% Li—7 E. 92.51% Li-6 and 7.49% Li-7 25. What is the mass (in grams) of a boron atom? A. 10.8 g _23 B. 1.80 ‘1024 g C. 1.66 ‘1022 g D. 5.57 ‘ 10_ g E. 1.54’1025g 26. 27. 28. 29. 30. 31. Group 1 elements are also known as A. alkaline earth metals. B. alkali metals. C. chalcogens. D. halogens. E. noble gases. How many nonmetallic elements are there in group 13? WUOW? AmNr—O Identify the halogen from period 4. A. Br B. I C. Kr D. Ar E. K What element is in the fourth period in Group 3A? A. Sb B. Ga C. In D. Si E. Tl Which group ofthree elements contains a nonmetal, a metal, and a metalloid? A. Li, Al, Si B. Na, Hg, I C. I, Hg, Si D. K, 0, Br E. H, Al, N Which three elements are likely to have similar chemical and physical properties? A. boron, silicon, and germanium B. sodium, magnesium, and aluminum C. sodium, potassium, and rubidium D. oxygen, sulfur, and chlorine E. carbon, nitrogen, and oxygen . Which group ofthree elements contains a transition metal, a halogen, and a noble gas? A. S, 1, Cu B. Br, Kr, Ba C. Ar, Hg, Rn D. Ce, N, He E. Cu, 1, Xe . How many elements are contained in period 2? A. 3 B. 8 C. 10 D. 18 E. 32 . Of the naturally occurring elements in group 14, how many are nonmetals, metalloids, and metals? A. O nonmetals, 3 metalloids, and 2 metals B. l nonmetal, 2 metalloids, and 2 metals C. 2 nonmetals, 2 metalloids, and 1 metal D. 2 nonmetals, l metalloid, and 2 metals E. 3 nonmetals, O metalloids, and 2 metals . Which two of the following elements are abundant in the Earth’s crust, but missing from the human body: 0, Al, Si, Fe, C, N? A. O and Fe B. Si and C C. Al and Si D. O and N E. Fe and N . The formula of ethanol, CH3CH2OH, is an example of a(n) . condensed formula. . empirical formula. . structural formula. . ionic compound formula. . mass spectrum. mUOUUD> . Which element is most likely to form an ion With a -2 charge? A.K E g 1‘ WUQW map-u 38. 39. 40. 41. 42. 43. Which atom is most likely to form an ion with a +2 charge? A. scandium B. calcium C. aluminum D. oxygen E. fluorine A strontium ion has electrons. A. 35 B. 36 C. 37 D. 38 E. 39 For a nonmetal in Group 16 of the periodic table, the most common monatomic ion Will have a charge of —3 —2 —1 +1 +2 meow» Identify the ions and their charges in NaZSO4. A. Na: so4’2_ B. Na+, SO4_ C. NaHSO 4_ D. Na2+, SO 2_ E. Na , SO4 Identify the ions and their charges in KH2P04. What is the correct formula for an ionic compound that contains magnesium ions and phosphide ions? A. MgP B. MgP C. Mg3E D. Mg (1304)2 E. Mg2 3 44. 45. 46. 47. 48. 49. What is the correct formula for an ionic compound that contains aluminum ions and chloride ions? A. AlCl B. AlCl c. A1C12 D. A1 Cl E. A12C13 3 2 What are the values for X and y, respectively, in Ca H P04? X Y A. 1 and2 B. 2and1 C. 1and3 D.2and2 E. l andl Sodium sulfate has the chemical formula Na2804. Based on this information, the formula for chromium(III) sulfate is A. CrSO B. Cr(sd) c. cgsdfi3 D. Cr SO E. Cr2(so‘ ) 3 4 2 What is the correct name for MnS? A. manganese sulfide B. dimanganese sulfate C. dimanganese sulf1de D. manganese(II) sulfate E. manganese(II) sulflde What is the correct name for K3PO4? A. tripotassium phosphate B. potassium(l) monophosphorus tetraoxide C. potassium(l) phosphate D. potassium phosphate E. potassium phosphide What is the correct name for TiCl4? A. monotitanium tetrachloride B. tetrachlorine titanate C. titanium tetrachlorine D. titanium(IV) tetrachloride E. titanium(IV) chloride 10 50. 51. 52. 53. 54. 55. What is the correct name for A1203? . alum aluminum trioxide aluminum ozinide . aluminum oxide E. dialuminum trioxide cow> What is the correct formula for aluminum selenide? A. AlSe B. AlSe c. A1 s% D. A128e E. A128e3 3 2 What is the correct formula for iron(II) nitrate? A. Fe2(NO3)2 B. Fe NO C. FetNo3) D. Fe N 3 E. FeliIO2 3 What is the correct formula for barium perchlorate? A. BaClO B. BaClO4 c. 1331((31d4)2 D. Ba(ClO ) E. Ba(ClO3)2 3 3 What is the correct name for N203? A. nitrogen oxide B. nitrogen(ll) oxide C. nitrogen(lll) oxide D. trioxygen dinitride E. dinitrogen trioxide What is the correct name for PFS? A. phosphorus pentafluoride B. phosphorus(V) fluoride C. phosphorofluoride D. pentafluorophosphorus E. pentafluorophosphate ll 56. 57. 58. 59. 60. What is the correct name for CCl4? A. carbon chlorine B. tetracarbon chloride C. carbon tetrachloride D. carbon(IV) chloride E. tetrachlorocarbide What is the correct formula for sulfur dichloride? A. sc1 B. sc1 c. s D. s c1 E. s2(:12 4 2 [\.) What is the correct formula for potassium dichromate? A. KZCrzO B. K2(Cr d7)2 c. KZCrd D. K (Crd ) E. K6104 4 2 What is the formula for hypochlorous acid? A. HCl B. HClO C. HClO D. HCIO2 E. HCIO: What is the correct name for HZSO4(aq)? A. sulfuric acid B. sulfide acid C. sulfurous acid D. hydrogen sulfate acid E. hydrogen sulfide acid 12 61. Using the laws of constant composition and the conservation of mass, complete the molecular picture of hydrogen molecules (circles) reacting with oxygen molecules (squares) to give water. on an. + —- Cir-Cf l3 62. Using the laws of constant composition and the conservation of mass, complete the molecular picture of hydrogen molecules (circles) reacting with chlorine molecules (squares) to give hydrogen chloride (HCl). CH3 M |:I-|:I EH3 63. BAC stands for: A. Breath Alcohol Concentration B. Blood Alcohol Concentration C. Brain Alcohol Concentration D. Blood Alcohol Consumption E. Bad Alcohol Correlation 14 64. Which of the following is a non-electrolyte in water? A. NaCl B. SF C. Kixio D. MgS 3 E. NH4C1 15 Chapter 2–Atoms, Molecules, and Ions Key Which of the following statements is/are postulates of Dalton’s atomic theory? 1. Elements are composed of tiny particles called atoms. 2. No atom is changed into another element in an ordinary chemical reaction. 3. Compounds are formed when two or more atoms combine. 1 only 2 only 3 only 1 and 3 L l, 2 and 3 J.J. Thomson determined that electrons are small, negatively charged particles by bombarding gold foil with alpha particles. exposing photographic plates to radioactive uranium. Q deflecting cathode rays with electric and magnetic fields. converting cathode rays to electron particles using a fluorescent screen. decomposing neutrons into protons and electrons. Which of the following statements is/are CORRECT? l. A neutron is an uncharged particle with a mass slightly greater than a proton. 2. The nucleus of an atom has a negative charge. 3. More than 99.9% of an atom’s mass is concentrated in the electron cloud surrounding the nucleus. A 1 only 2 only 3 only 1 and 3 l, 2 and 3 Rank the subatomic particles from least to greatest mass. electrons = neutrons = protons electrons = protons < neutrons electrons < neutrons = protons Q electrons < protons < neutrons electrons < neutrons < protons 10. All of the following statements are true EXCEPT A all atoms of a given element have the same mass number. for any neutral element, the number of electrons is equal to the number ofprotons. the mass number is the sum of the number ofprotons and neutrons. isotopes of atoms contain the same number ofprotons but a different number of neutrons. the atomic number equals the number of protons in an atom. All atoms of the same element have the same number of . neutrons L protons protons and neutrons electrons and neutrons protons, neutrons, and electrons What is the mass number of an argon atom with 22 neutrons? 2 18 22 Q 40 39.95 Which of the following atoms contains the fewest protons? A 232Th 231Pa 245Pu 23 8U 232Pa How many protons, neutrons, and electrons are in a silver atom with a mass number of 108? 47 protons, 47 neutrons, 61 electrons L 47 protons, 61 neutrons, 47 electrons 61 protons, 47 neutrons, 47 electrons 47 protons, 108 neutrons, 47 electrons 61 protons, 108 neutrons, 61 electrons F-20, a radioactive isotope of fluorine, has 9 protons, 10 neutrons, and 1 electron. 9 protons, 10 neutrons, and 9 electrons. Q 9 protons, ll neutrons, and 9 electrons. 10 protons, 9 neutrons, and 1 electron. 10 protons, 10 neutrons, and 10 electrons. ll. 12. 13. Which two atoms below have the same number ofneutrons? 15 115 2U 2U 22 20’ 2D” 21411111‘1'3’111q 13031101 1:0 1Egandfima EEFandi‘EHe QEEFandfiHa 2:1 and 22 12 He 11 Ha What is the atomic symbol for an element with 39 protons and 50 neutrons? 2:: 11 Na 3] Sn 222' 22 4'5": Which two of the ions below have the same number of electrons? 122 -112? 2+ 222 2+ 222 4+122 2+ 531’5fl1-Jfl ’Eflph ’Eflph ’ ESE-El A. "9'1— and133 3+ — 53 J‘fiE-a 53I 511511 21:12 2+ and 132 2+ 212 Pb 5532 112 2+ and 122 2+ 511511 2533 2|]? 2+ (1202' 4+ 2+ 121:. an 22 121:. 14. 15. 16. 17. Two isotopes of a given element Will have the same number of , but a different number of in their nucleus. protons, electrons electrons, protons Q protons, neutrons neutrons, protons electrons, neutrons Which of the following are a pair of isotopes? 13 Far “‘13 H 33 Ca and 13 H 13m and :3 Hr 4t: and 39 an [:3 19 I": L :3 Ca andg Ca Which species has 63 neutrons? 112 43Cd 112 h 45, In :3 Elfin 152 53 Eu none of the above Two isotopes of chlorine are found in nature, Cl-35 and Cl-37. The average mass of chlorine is 35.45 amu. The more abundant isotope of Cl has A 17 protons, l7 electrons, and 18 neutrons. 17 protons, l7 electrons, and 18.45 neutrons. 17 protons, l7 electrons, and 20 neutrons. 18 protons, l8 electrons, and 17 neutrons. 19 protons, l9 electrons, and 16 neutrons. 18. 19. 20. 21. What is the identity of5'5 E? 25 zinc silver iridium cesium L manganese What is the symbol for an element which contains 57 neutrons and has a mass number of 101? Er h Ru Md La Os Rubidium has two naturally occurring isotopes. The average mass of Rb is 85.4678 amu. If72.15% of Rb is found as Rb-85 (84.9117 amu), what is the mass of the other isotope? 0.56 amu 85.68 amu Q 86.91 amu 86.02 amu 83.47 amu Silver has two stable isotopes with masses of 106.90509 amu and 108.9047 amu. The average molar mass of silver is 107.868 amu. What is the percent abundance of each isotope? 50.0% Ag-107 and 50.0% Ag-109 h 51.8% Ag-107 and 48.2% Ag-109 55.4% Ag-107 and 44.6% Ag-109 48.2% Ag-107 and 51.8% Ag-109 44.6% Ag-107 and 55.4% Ag-109 22. 23. 24. 25. Gallium has an average atomic mass of 69.7 amu. In a typical sample, 60.4% of Ga exists as Ga-69 (68.9257 amu). What is the identity and the atomic mass of the other isotope? :‘i [33; 70.9 amu :‘i [33; 70.9 amu Q :i [33; 70.9 amu :1 [33; 71.9 amu 3 3371.9 amu An element has three naturally occurring isotopes with the following abundances and masses: amu 8.99% .985042 0.00% 4.985837 1.01% .982593 Determine the molar mass of the element. A 24.31 g/mol 24.98 g/mol 74.95 g/mol 2431 g/mol none of the above The average molar mass of lithium is 6.941. A sample of lithium consists of two isotopes with masses of 6.01512 amu and 7.01600 amu. Determine the percent abundance of each isotope. A 7.49% Li-6 and 92.51% Li-7 8.45% Li-6 and 91.55% Li-7 12.49% Li-6 and 87.51% Li-7 91.55% Li-6 and 8.45% Li-7 92.51% Li-6 and 7.49% Li-7 What is the mass (in grams) of a boron atom? n 1.80 ' 103: g 1.66 ' 1022 g 5.57 ' 10_ g 1.54'1025g 26. 27. 28. 29. 30. 31. Group 1 elements are also known as alkaline earth metals. L alkali metals. chalcogens. halogens. noble gases. How many nonmetallic elements are there in group 13? E Awwr—‘O Identify the halogen from period 4. A Br I Kr Ar K What element is in the fourth period in Group 3A? Sb L Ga In Si Tl Which group of three elements contains a nonmetal, a metal, and a metalloid? Li, Al, Si Na, Hg, 1 Q I, Hg, Si K, 0, Br H, Al, N Which three elements are likely to have similar chemical and physical properties? boron, silicon, and germanium sodium, magnesium, and aluminum Q sodium, potassium, and rubidium oxygen, sulfur, and chlorine carbon, nitrogen, and oxygen 32. 33. 34. 35. 36. 37. Which group of three elements contains a transition metal, a halogen, and a noble gas? S, 1, Cu Br, Kr, Ba Ar, Hg, Rn Ce, N, He L Cu, 1, Xe How many elements are contained in period 2? 3 g 8 10 18 32 Of the naturally occurring elements in group 14, how many are nonmetals, metalloids, and metals? 0 nonmetals, 3 metalloids, and 2 metals L 1 nonmetal, 2 metalloids, and 2 metals 2 nonmetals, 2 metalloids, and 1 metal 2 nonmetals, l metalloid, and 2 metals 3 nonmetals, 0 metalloids, and 2 metals Which two of the following elements are abundant in the Earth's crust, but missing from the human body: 0, Al, Si, Fe, C, N? O and Fe Si and C Q Al and Si O and N Fe and N The formula of ethanol, CH3CHZOH, is an example of a(n) A condensed formula. empirical formula. structural formula. ionic compound formula. mass spectrum. Which element is most likely to form an ion with a -2 charge? K Mg P Br L S 38. 39. 40. 41. 42. 43. Which atom is most likely to form an ion with a +2 charge? scandium L calcium aluminum oxygen fluorine A strontium ion has electrons. 35 g 36 37 38 39 For a nonmetal in Group 16 of the periodic table, the most common monatomic ion will have a charge of . —3 g —2 —1 +1 +2 Identify the ions and their charges in NaZSO4. Na: so4‘2_ ;Na+, SO4_ Na SO 24 4- Na2+, SO 2_ Na , SO4 Identify the ions and their charges in KH2PO4. What is the correct formula for an ionic compound that contains magnesium ions and phosphide ions? MgP MgP o Mg313lg Mg3( O4)2 Mg2P3 44. 45. 46. 47. 48. 49. What is the correct formula for an ionic compound that contains aluminum ions and chloride ions? AlCl AlCl ;AlC12 Al Cl A12C13 3 2 What are the values for X and y, respectively, in Ca H P04? X y land2 2andl land3 2and2 L landl Sodium sulfate has the chemical formula NaZSO4. Based on this information, the formula for chromium(IlI) sulfate is CrSO What is the correct name for MnS? manganese sulfide dimanganese sulfate dimanganese sulfide manganesefll) sulfate L manganesefll) sulfide What is the correct name for K3PO4? tripotassium phosphate potassium(l) monophosphorus tetraoxide potassium(l) phosphate L potassium phosphate potassium phosphide What is the correct name for TiCl4? monotitanium tetrachloride tetrachlorine titanate titanium tetrachlorine titanium(IV) tetrachloride L titanium(IV) chloride 10 50. 51. 52. 53. 54. 55. What is the correct name for A1203? alum aluminum trioxide aluminum ozinide Q aluminum oxide dialuminum trioxide What is the correct formula for aluminum selenide? AlSe AlSe What is the correct formula for iron(II) nitrate? Fe2(NO3)2 Fe NO Q FefNO§)2 Fe N FeliIC; 3 What is the correct formula for barium perchlorate? BaClO BaClo4 ;Ba((:1d4)2 Ba(ClO ) 3 2 331((3103)3 What is the correct name for N203? nitrogen oxide nitrogen(II) oxide nitrogen(III) oxide trioxygen dinitride L dinitrogen trioxide What is the correct name for PFS? A phosphorus pentafluoride phosphorus(V) fluoride phosphorofluoride pentafluorophosphorus pentafluorophosphate ll 56. 57. 58. 59. 60. What is the correct name for CCl4? carbon chlorine tetracarbon chloride Q carbon tetrachloride carbon(IV) chloride tetrachlorocarbide What is the correct formula for sulfur dichloride? SCI n SCI s Ci s (:1 2 s (:12 #NN What is the correct formula for potassium dichromate? A KzCrzO K2(Cr d7)2 KzCré K (Crd1 ) K€r04 4 2 What is the formula for hypochlorous acid? HCl ;HClO HClO Holo2 H0034 What is the correct name for HZSO4(aq)? A sulfuric acid sulfide acid sulfurous acid hydrogen sulfate acid hydrogen sulfide acid 12 61. Using the laws of constant composition and the conservation of mass, complete the molecular picture ofhydrogen molecules (circles) reacting with oxygen molecules (squares) to give water. W m: CH: + '"' Eli-El Cir-Cf i, l3 62. Using the laws of constant composition and the conservation of mass, complete the molecular picture ofhydrogen molecules (circles) reacting with chlorine molecules (squares) to give hydrogen chloride (HCl). CH:- IEHJ I:I-I:I EH3 |fi E 63. BAC stands for: Breath Alcohol Concentration L Blood Alcohol Concentration Brain Alcohol Concentration Blood Alcohol Consumption Bad Alcohol Correlation 14 64. Which of the following is a non-electrolyte in water? NaCl E SF K1\?O MgS 3 NH4C1 15