MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

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1 Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Elements in Group 8A are known as the. A) alkali metals B) alkaline earth metals C) noble gases D) chalcogens E) halogens 1) 2) and reside in the atomic nucleus. A) Electrons, neutrons B) Protons, neutrons C) Protons, electrons D) none of the above E) Neutrons, only neutrons 2) 3) Potassium is a and chlorine is a. A) metal, nonmetal B) metalloid, nonmetal C) metal, metalloid D) metal, metal E) nonmetal, metal 3) 4) In the periodic table, the rows are called and the columns are called. A) staffs, families B) periods, groups C) rows, groups D) cogeners, families E) octaves, groups 4) 5) Elements in Group 1A are known as the. A) alkali metals B) halogens C) alkaline earth metals D) chalcogens E) noble gases 5) 1

2 6) The atomic number indicates. A) the total number of neutrons and protons in a nucleus B) the number of neutrons in a nucleus C) the number of protons or electrons in a neutral atom D) the number of atoms in 1 g of an element E) the number of different isotopes of an element 6) 7) The nucleus of an atom contains. A) electrons B) protons and electrons C) protons and neutrons D) protons E) protons, neutrons, and electrons 7) 8) What is the formula for perchloric acid? 8) A) HClO B) HCl C) HClO4 D) HClO2 E) HClO3 9) Elements in Group 7A are known as the. A) alkali metals B) noble gases C) chalcogens D) alkaline earth metals E) halogens 9) 10) When a metal and a nonmetal react, the tends to lose electrons and the tends to gain electrons. 10) A) nonmetal, nonmetal B) nonmetal, metal C) metal, nonmetal D) metal, metal E) None of the above, these elements share electrons. 11) The correct name for HIO2 is. 11) A) hydriodic acid B) periodous acid C) iodous acid D) hypoiodic acid E) periodic acid 2

3 12) typically form ions with a 2+ charge. A) Alkaline earth metals B) Chalcogens C) Transition metals D) Halogens E) Alkali metals 12) 13) The charge on the manganese in the salt MnF3 is. 13) A) -2 B) +1 C) +3 D) -1 E) +2 14) Of the following, only is not a metalloid. A) Si B) As C) Al D) B E) Ge 14) 15) The formula of bromic acid is. A) HBrO3 B) HBr C) HBrO2 D) HBrO4 E) HBrO 15) 16) Potassium forms an ion with a charge of. A) -2 B) 0 C) -1 D) +2 E) +1 16) 17) Aluminum forms an ion with a charge of. A) +2 B) -1 C) +3 D) -3 E) +1 17) 18) Iodine forms an ion with a charge of. A) +1 B) -1 C) +2 D) -2 E) -7 18) 19) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? 19) A) Cs, Ba B) H, Li C) Ca, Sr D) C, O E) Ga, Ge 20) The formula for aluminum hydroxide is. 20) A) Al3OH B) Al(OH)3 C) AlOH D) Al2O3 E) Al2(OH)3 21) An element that appears in the lower left corner of the periodic table is. A) definitely a non-metal B) definitely a metalloid C) either a metal or metalloid D) either a metalloid or a non-metal E) definitely a metal 21) 3

4 22) In the periodic table, the elements are arranged in. A) reverse alphabetical order B) order of increasing metallic properties C) order of increasing atomic number D) order of increasing neutron content E) alphabetical order 22) 23) Of the choices below, which one is not an ionic compound? 23) A) RbCl B) PbCl2 C) NaCl D) MoCl6 E) PCl5 24) Which pair of elements is most apt to form an ionic compound with each other? A) barium, bromine B) nitrogen, hydrogen C) sulfur, fluorine D) calcium, sodium E) oxygen, fluorine 24) 25) The value of H for the reaction below is -72 kj. kj of heat are released when 1.0 mol of HBr is formed in this reaction. 25) H2 (g) + Br2 (g) 2HBr (g) A) 144 B) 72 C) 36 D) -72 E) ) The value of H for the reaction below is -126 kj. The amount of heat that is released by the reaction of 25.0 g of Na2O2 with water is kj. 26) 2Na2O2 (s) + 2H2O (l) 4NaOH (s) + O2 (g) A) 40.4 B) 67.5 C) 80.8 D) -126 E) ) The value of H for the reaction below is kj. kj of heat are released in the combustion of 16.0 g of C6H6 (l)? 27) 2C6H6 (l) + 15O2 (g) 12CO2 (g) + 6H2O (l) A) B) C) D) E) ) A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2 C to 30.5 C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is g. 28) A) 8.1 B) 1.5 C) 6.6 D) 72 E) 65 4

5 29) The value of H for the reaction below is -186 kj. Calculate the heat (kj) released from the reaction of 25 g of Cl2. 29) H2 (g) + Cl2 (g) 2HCl (g) A) -186 B) C) 47 D) 66 E) 33 30) The value of H for the reaction below is kj: 30) CH3OH (l) CO (g) + 2H2 (g) How many kj of heat are consumed when 5.75 g of CO (g) reacts completely with hydrogen to form CH3OH (l)? A) 162 B) 23.3 C) 8.3 D) 62.0 E) ) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 C to 37 C? 31) A) B) 2.0 C) 0.13 D) E) 29 32) The temperature of a 15-g sample of lead metal increases from 22 C to 37 C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is J/g-K. 32) A) 7.8 B) -29 C) 1.9 D) 0.13 E) 29 33) H for the reaction 33) IF5 (g) IF3 (g) + F2 (g) is kj, give the data below. IF (g) + F2 (g) IF3 (g) IF (g) + 2 F2 (g) IF5 (g) H = -390 kj H = -745 kj A) B) -35 C) D) +355 E) +35 5

6 34) Given the following reactions 34) Fe2O3 (s) + 3CO (s) 2Fe (s) + 3CO2 (g) 3Fe (s) + 4CO2 (s) 4CO (g) + Fe3O4 (s) H = kj H = kj the enthalpy of the reaction of Fe2O3 with CO 3Fe2O3 (s) + CO (g) CO2 (g) + 2Fe3O4 (s) is kj. A) 40.5 B) -109 C) +109 D) E) ) Given the following reactions 35) (1) 2NO N2 + O2 H = -180 kj (2) 2NO + O2 2NO2 H = -112 kj the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide N2 + 2O2 2NO2 is kj. A) 68 B) -68 C) 292 D) -146 E) ) Calculate H (in kj) for reaction 3. 36) 2S (s) + 3O2 (g) 2SO3 (g) S (s) + O2 (g) SO2 (g) H = -790 kj H = -297 kj the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide 2SO2 (g) + O2 (g) 2SO3 (g) is kj. A) 1087 B) -543 C) -196 D) E) ) A H corresponds to an process. A) negative, endothermic B) negative, exothermic C) positive, exothermic D) zero, exothermic E) zero, endothermic 37) 6

7 38) H for an endothermic process is while H for an exothermic process is. A) zero, negative B) zero, positive C) positive, zero D) negative, positive E) positive, negative 38) 39) The units of of specific heat are. A) J/K or J/ C B) K/J or C/J C) g-k/j or g- C/J D) J/mol E) J/g-K or J/g- C 39) 40) How many p-orbitals are occupied in a Ne atom? A) 0 B) 6 C) 1 D) 2 E) 3 40) 41) How many quantum numbers are necessary to designate a particular electron in an atom? 41) A) 2 B) 1 C) 5 D) 3 E) 4 42) [Ar]4s23d104p3 is the electron configuration of a(n) atom. A) Sn B) As C) P D) Sb E) V 42) 43) The second energy level of atomic argon contains electrons. A) 2 B) 6 C) 8 D) 18 E) 36 43) 44) Each p-sublevel can accommodate a maximum of electrons. A) 6 B) 3 C) 2 D) 5 E) 10 44) 45) The largest principal quantum number in the electron configuration of iodine is. A) 1 B) 4 C) 5 D) 6 E) 7 45) 46) The electron configuration for Zn is. A) [Ar]4s23d10 B) [Kr]4s23d10 C) [Ar]4s13d10 D) [Ar]3s23d10 E) [Kr]3s23d10 46) 7

8 47) The largest principal quantum number in the electron configuration of cobalt is. A) 2 B) 3 C) 4 D) 7 E) 9 47) 48) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the of an electron. 48) A) velocity B) color C) speed D) shape E) mass 49) There are unpaired valence electrons in a fluorine atom. A) 0 B) 1 C) 2 D) 3 E) 4 49) 50) Which of the subshells below do not exist? A) 2d B) 2p C) 2s D) all of the above E) none of the above 50) 51) Which electron configuration represents a violation of the Pauli exclusion principle? A) 51) B) C) D) E) 8

9 52) Which of the subshells below do not exist? A) 4p B) 4d C) 4f D) 4s E) none of the above 52) 53) Which one of the following orbitals can hold two electrons? A) 3s B) 2p C) 4d D) all of the above E) none of the above 53) 54) The electron configuration of Fe is. A) 1s22s23s23p63d6 B) 1s22s22p63s23p64s23d 6 C) 1s22s23s23p10 D) 1s22s22p63s23p64s24d6 E) 1s22s22p63s23p64s2 54) 9

10 55) Which electron configuration represents a violation of Hund's rule for an atom? A) 55) B) C) D) E) 56) Which of the following elements has an electron configuration different from the predicted one? A) Xe B) Cu C) Cl D) Ti E) Ca 56) 57) is credited with developing the concept of atomic numbers. A) Ernest Rutherford B) Dmitri Mendeleev C) Lothar Meyer D) Henry Moseley E) Michael Faraday 57) 58) Which two elements have the same electron configuration? A) Cl and Ar B) Cu and Ag C) Fe and Cu D) Pd and Pt E) No two elements have the same ground-state electron configuration. 58) 10

11 59) The ionization energies of the elements as you go from left to right across a period of the periodic table, and as you go from the bottom to the top of a group in the table. 59) A) increase, increase B) increase, decrease C) decrease, increase D) decrease, decrease E) are completely unpredictable 60) The have the most negative electron affinities. A) chalcogens B) alkali metals C) alkaline earth metals D) transition metals E) halogens 60) 61) In general, as you go across a period in the periodic table from left to right: (1) the atomic radius ; (2) the electron affinity becomes negative; and (3) the first ionization energy. A) increases, increasingly, decreases B) decreases, increasingly, decreases C) increases, increasingly, increases D) decreases, increasingly, increases E) decreases, decreasingly, increases 61) 62) Of the hydrogen halides, only is a weak acid. A) HF (aq) B) HCl (aq) C) HI (aq) D) HBr (aq) E) They are all weak acids. 62) 63) Which one of the following atoms has the largest radius? A) Ba B) Ca C) Sr D) Co E) I 63) 64) Which one of the following atoms has the largest radius? A) O B) Ne C) S D) Cl E) F 64) 65) Which one of the following has the smallest radius? A) Na B) Br C) Cl D) Fe E) P 65) 11

12 66) Of the following atoms, which has the largest first ionization energy? A) P B) O C) Br D) I E) C 66) 67) Of the following elements, which has the largest first ionization energy? A) Rb B) Ca C) Sr D) K E) Ba 67) 68) Of the following elements, which has the largest first ionization energy? A) P B) Si C) N D) C E) B 68) 69) have the lowest first ionization energies of the groups listed. A) Alkaline earth metals B) Alkali metals C) Halogens D) Noble gases E) Transition elements 69) 70) Which one of the following compounds produces a basic solution when dissolved in water? 70) A) O2 B) SO2 C) Na2O D) OF2 E) CO2 71) Which ion below has the largest radius? A) F- B) Br- C) K+ D) Cl- E) Na+ 71) 72) All of the following are ionic compounds except. 72) A) Na2SO4 B) NaCl C) Li3N D) K2O E) SiO2 73) Based on the octet rule, phosphorus most likely forms a ion. A) P3- B) P+ C) P5+ D) P5- E) P3+ 73) 74) What is the maximum number of double bonds that a carbon atom can form? A) 1 B) 3 C) 0 D) 4 E) 2 74) 75) Based on the octet rule, magnesium most likely forms a ion. A) Mg6+ B) Mg2- C) Mg- D) Mg2+ E) Mg6-75) 76) A double bond consists of pairs of electrons shared between two atoms. A) 1 B) 2 C) 3 D) 4 E) 6 76) 77) How many single covalent bonds must a carbon atom form to have a complete octet in its outer level? 77) A) 4 B) 1 C) 3 D) 0 E) 2 12

13 78) A Br nsted-lowry acid is defined as a substance that. A) acts as a proton acceptor B) acts as a proton donor C) decreases [H+] when placed in H2O 78) D) increases [OH-] when placed in H2O E) increases [H+] when placed in H2O 79) In the molecule below, which atom has the largest partial negative charge? 79) Cl F C Br I A) Cl B) F C) C D) I E) Br 80) A substance that is capable of acting as both an acid and as a base is. A) miscible B) conjugated C) saturated D) amphoteric E) autosomal 80) 81) A nonpolar bond will form between two atoms of electronegativity. A) identical, equal B) identical, different C) different, opposite D) different, different E) similar, different 81) 82) Of the atoms below, is the most electronegative. A) O B) Br C) Cl D) F E) N 82) 83) What is the maximum number of double bonds that a hydrogen atom can form? A) 0 B) 1 C) 2 D) 3 E) 4 83) 84) Given the electronegativities below, which covalent single bond is most polar? 84) Element: H C N O Electronegativity: A) O-H B) O-C C) N-H D) O-N E) C-H 13

14 85) Of the bonds below, is the least polar. A) C, F B) Na, S C) Na, Cl D) P, S E) Si, Cl 85) 86) A sample of gas initially at 4.00 kpa was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was kpa. 86) A) 2.00 B) 1.00 C) 16.0 D) 4.00 E) ) Which of the following has eight valence electrons? A) Kr B) Ti4+ C) Cl- D) Na+ E) all of the above 87) 88) A sample of a gas at kpa is expanded at constant temperature from 10 L to 15 L. The final pressure is kpa. 88) A) 7.5 B) 67 C) 3.3 D) 1.5 E) 15 89) A gas originally at 27 C in a 3.9 L flask is cooled at constant pressure until the temperature is 11 C. The new volume of the gas is L. 89) A) 3.9 B) 0.24 C) 4.1 D) 3.7 E) ) A sample of a gas originally at 25 C and 102.3kPa pressure in a 2.5 L container is allowed to expand until the pressure is kpa and the temperature is 15 C. The final volume of the gas is L. 90) A) 0.38 B) 3.0 C) 2.6 D) 2.1 E) ) The first person to investigate the relationship between the pressure of a gas and its volume was. 91) A) Joseph Louis Gay-Lussac B) Jacques Charles C) Robert Boyle D) Lord Kelvin E) Amadeo Avogadro 92) A sample of He gas occupies 57.9 L at K and 1.00 kpa. The volume of this sample is L at 423 K and 1.00 kpa. 92) A) 41.1 B) 81.6 C) 57.9 D) 1.41 E)

15 93) Standard temperature and pressure (STP), in the context of gases, refers to. A) 0 K & 100 kpa B) 0 Celsius & kpa C) 273 K and 1 torr D) 0 K and kpa E) 298 K and 1 atm 93) 94) Of the following, is a correct statement of Boyle's law. A) PV = constant B) V T = constant 94) C) P V = constant D) n P = constant E) V P = constant 95) A gas is and assumes of its container whereas a liquid is and assumes of its container. 95) A) compressible, the shape, not compressible, the volume and shape B) compressible, the volume and shape, compressible, the volume C) condensed, the volume and shape, condensed, the volume and shape D) compressible, the volume and shape, not compressible, the shape of a portion E) condensed, the shape, compressible, the volume and shape 96) Of the following gases, will have the greatest rate of diffusion at a given temperature. A) HCl B) CH4 C) HBr D) NH3 E) Ar 96) 97) Of the following, is a valid statement of Charles' law. A) V = constant P B) P T = constant 97) C) V T = constant D) PV = constant E) V = constant n 98) The volume of an gas is zero at. A) -363 K B) -273 K C) -45 F D) -273 C E) 0 C 98) 15

16 99) A Br nsted-lowry base is defined as a substance that. A) decreases [H+] when placed in H2O 99) B) increases [OH-] when placed in H2O C) acts as a proton acceptor D) acts as a proton donor E) increases [H+] when placed in H2O 100) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H+ B) causes an increase in the concentration of H+ in aqueous solutions C) can accept a pair of electrons to form a coordinate covalent bond D) tastes bitter E) reacts with the solvent to form the cation formed by autoionization of that solvent 100) 101) What is the ph of an aqueous solution at 25.0 C that contains M hydronium ion? A) 7.00 B) 8.40 C) 9.00 D) 3.98 E) ) 102) What is the ph of an aqueous solution at 25.0 C in which [OH-] is M? A) B) C) D) E) ) 103) What is the concentration (in M) of hydronium ions in a solution at 25.0 C with ph = 4.282? A) 4.28 B) C) 9.71 D) E) ) 104) Which solution below has the highest concentration of hydroxide ions? A) ph = 12.6 B) ph = 7.00 C) ph = 3.21 D) ph = 9.82 E) ph = ) 105) Of the following acids, is not a strong acid. 105) A) HCl B) HNO2 C) H2SO4 D) HNO3 E) HClO4 106) Classify the following compounds as weak acids (W) or strong acids (S): 106) nitrous acid hydrochloric acid hydrofluoric acid A) S S S B) S W W C) W W W D) W S W E) W S S 16

17 107) Ammonia is a. A) strong acid B) weak acid C) salt D) strong base E) weak base 107) 108) The gain of electrons by an element is called. A) oxidation B) disproportionation C) reduction D) fractionation E) sublimation 109) What is the oxidation number of chromium in Cr2 O 2-7 ion? 108) 109) A) +14 B) +12 C) +3 D) +7 E) ) What is the oxidation number of manganese in MnO2? 110) A) +4 B) +2 C) +3 D) +7 E) ) What is the oxidation number of potassium in KMnO4? 111) A) -1 B) +1 C) 0 D) +2 E) ) Which substance is serving as the reducing agent in the following reaction? 112) 14H+ + Cr2O Ni 3Ni2+ + 2Cr3+ + 7H2O A) Ni2+ B) H+ C) Ni D) H2O E) Cr2O7 2-17

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In nature, sulfur is most commonly found in. 1) A) pure elemental sulfur B) H2S C) sulfuric