test questions 2009

7/29/2019 Test Questions 2009

1/69

1. Give the names of the following ions:CO3

2!, HCO3!, CN!, OCN!, SCN!, NO2

!, NO3!, PO4

3!, HPO42!, H2PO4

!, SO32!, HSO3

!, SO42!,

HSO4!, S2O3

2!, HS2O3!, ClO!, ClO2

!, ClO3!, ClO4

!, BrO3!, IO3

!, O2!, OH!, H3O+, NH4

+, S2!, HS!,MnO4

!, CrO42!, HCrO4

!, Cr2O72!, HCr2O7

!, CH3COO!

2. Give the names of the following compounds:H

2CO

3, CH

3COOH, H

2Cr

2O

7, H

2CrO

4, HMnO

4, H

2S, NH

3, H

2O, H

2O

2, HIO

3, HClO

4, HBrO

3, HClO

3,

HClO2, H2SO4, HClO, HI, HBr, HF, HCl, H2S2O3, H2SO3, HOCN, HCN, HSCN, HNO2, HNO3,H3PO4, NH4Cl, NH4Br, NH4F, NH4I, NH4NO3, (NH4)2SO4, (NH4)3PO4, (NH4)2CO3, NH4CH3COO,LiCl, LiBr, LiF, LiI, Li2O, LiNO3, Li2SO4, Li3PO4, Li2CO3, LiOH, LiCH3COO, NaCl, NaBr, NaF,NaI, NaCN, NaOCN, NaSCN, NaNO3, NaNO2, Na2SO4, NaHSO4, Na2SO3, NaHSO3, Na2S, NaHS,Na2S2O3, Na3PO4, Na2HPO4, NaH2PO4, Na2CO3, NaHCO3, NaOH, NaClO, NaClO2, NaClO3,NaClO4, NaBrO3, NaIO3, NaCH3COO, KCl, KBr, KF, KI, KCN, KOCN, KSCN, KNO3, KNO2,K2SO4, KHSO4, K2SO3, KHSO3, K2S, KHS, K2S2O3, K3PO4, K2HPO4, KH2PO4, K2CO3, KHCO3,KOH, KClO, KClO2, KClO3, KClO4, KBrO3, KIO3, K2CrO4, K2Cr2O7, KMnO4, KCH3COO, RbCl,RbBr, RbF, RbI, RbNO3, Rb2SO4, Rb3PO4, Rb2CO3, RbOH, RbCH3COO, CsCl, CsBr, CsF, CsI,CsNO3, Cs2SO4, Cs3PO4, Cs2CO3, CsOH, CsCH3COO, MgF2, MgCl2, MgBr2, MgI2, MgO, MgSO4,

MgCO3, Mg(HCO3)2, Mg(OH)2, Mg(NO3)2, CaF2, CaCl2, CaBr2, CaI2, CaO, CaSO4, CaCO3,Ca(HCO3)2, Ca(OH)2, Ca(NO3)2, SrF2, SrCl2, SrBr2, SrI2, SrO, SrSO4, SrCO3, Sr(HCO3)2, Sr(OH)2,Sr(NO3)2, BaF2, BaCl2, BaBr2, BaI2, BaO, BaSO4, BaCO3, Ba(HCO3)2, Ba(OH)2, Ba(NO3)2, BeF2,BeCl2, BeBr2, BeO, Be(OH)2, BF3, BCl3, BBr3, BI3, B2O3, AlF3, AlCl3, AlBr3, AlI3, Al2O3, Al(NO3)3,Al2(SO4)3, Al(OH)3, AlPO4, GaF3, GaCl3, GaBr3, GaI3, Ga2O3, Ga(NO3)3, Ga2(SO4)3, Ga(OH)3,GaPO4, InF3, InCl3, InBr3, InI3, In2O3, In(NO3)3, In2(SO4)3, In(OH)3, InPO4, TlF3, TlCl3, Tl2O3,Tl(NO3)3, Tl2(SO4)3, Tl(OH)3, TlCN, TlF, TlCl, TlBr, TlI, Tl2O, Tl2CO3, Tl2SO4, CO2, CO, CCl4, CF4,SiO2, SiCl4, SiBr4, GeO2, GeF4, GeBr4, GeCl4, GeI4, Sn(CH3COO)2, Sn(CH3COO)4, SnBr2, SnBr4,SnCl2, SnCl4, SnF2, SnF4, SnI2, SnI4, SnO, SnO2, SnSO4, Sn(SO4)2, SnS, Pb(CH3COO)2,Pb(CH3COO)4, PbBr2, PbCO3, PbCl2, PbCrO4, PbF2, PbI2, PbO, PbO2, Pb(ClO4)2, PbSO4, PbS, NF3,NCl3, N2O, NO, N2O3, NO2, N2O4, N2O5, P2O5, P2O3, PBr5, PCl5, P2S5, PBr3, PCl3, P2S3, AsBr3,

AsCl3, AsI3, As2O3, As2O5, As2S3, SbBr3, SbCl3, SbCl5, SbF3, SbF5, SbI3, Sb2O3, Sb2O5, Sb2S3, Sb2S5,Bi(CH3COO)3, BiBr3, BiCl3, BiF3, BiI3, Bi(NO3)3, Bi2O3, Bi2S3, OF2, SO2, SO3, SCl2, SF6, SeO2,SeS2, SeBr4, SeCl4, TeO2, TeBr4, TeCl4, TeI4, Po(NO3)2, ClF, ClF3, ClF5, Cl2O, ClO2, BrCl, BrF,BrF3, BrF5, Br2O, Br2O3, IF, IF3, IF5, ICl, IBr, I2O5, AtI, AtBr, XeF2, XeF4, XeF6, XeO3, XeO4, KrF2,Sc(CH3COO)3, ScCl3, Sc(NO3)3, Sc2O3, Sc(ClO4)3, YBr3, Y2(CO3)3, YCl3, YF3, YI3, Y(NO3)3, Y2O3,Y(ClO4)3, La(CH3COO)3, LaBr3, La2(CO3)3, LaCl3, LaF3, La(OH)3, LaI3, La(NO3)3, La2O3,La(ClO4)3, La2(SO4)3, TiBr4, TiCl2, TiCl3, TiCl4, TiF3, TiF4, TiI4, TiO2, TiS2, ZrBr4, ZrCl4, ZrF4, ZrI4,ZrO2, Zr(SO4)2, HfCl4, HfF4, HfO2, Hf(SO4)2, VBr3, VCl2, VCl3, VCl4, VF3, VF4, VI3, V2O3, V2O5,NbBr5, NbCl5, NbF5, NbO, NbO2, Nb2O5, TaBr5, TaCl5, TaF5, Ta2O5, CrCl2, CrCl3, CrF2, CrF3,Cr(NO3)3, Cr2O3, CrO2, CrO3, MoBr3, MoCl3, MoCl4, MoCl5, MoF4, MoO2, MoO3, MoS2, WBr5,WCl4, WCl6, WF6, WO2, WO3, WS2, Mn(CH3COO)2, Mn(CH3COO)3, MnBr2, MnCO3, MnCl2, MnF2,

MnF3, MnI2, Mn(NO3)2, MnO, Mn2O3, MnO2, Mn2O7, Mn(ClO4)2, MnSO4, MnS, TcCl4, TcCl6, TcF5,TcF6, TcO2, Tc2O7, ReCl3, ReCl5, ReF6, ReO2, ReO3, Re2O7, Re2S7, Fe(CH3COO)2, FeBr2, FeCl2,FeCl3, FeF2, FeF3, FeI2, Fe(NO3)3, FeO, Fe2O3, Fe(ClO4)2, Fe(ClO4)3, FePO4, FeSO4, FeS, RuBr3,RuCl3, RuI3, RuO2, OsCl3, OsO4, Co(CH3COO)2, CoBr2, CoCO3, CoCl2, CoF2, Co(OH)2, CoI2,Co(NO3)2, CoO, Co(ClO4)2, CoSO4, Co(SCN)2, RhBr3, RhCl3, RhI3, Rh(NO3)3, Rh2O3, RhPO4,Rh2(SO4)3, IrBr3, IrCl3, IrCl4, IrO2, Ni(CH3COO)2, NiBr2, NiCl2, NiF2, Ni(OH)2, NiI2, Ni(NO3)2, NiO,Ni(ClO4)2, NiSO4, NiS, Pd(CH3COO)2, PdBr2, PdCl2, Pd(CN)2, PdI2, Pd(NO3)2, PdO, PdSO4, PdS,PtBr2, PtBr4, PtCl2, PtCl4, Pt(CN)2, PtI2, Pd(NO3)2, PtO2, PtS2, Cu(CH3COO)2, CuBr, CuBr2, CuCl,CuCl2, CuCN, CuF2, Cu(OH)2, CuI, Cu(NO3)2, Cu2O, CuO, Cu(ClO4)2, CuSO4, Cu2S, CuS, CuSCN,AgCH3COO, AgBrO3, AgBr, Ag2CO3, AgCl, Ag2CrO2, AgOCN, AgCN, AgF, AgIO3, AgI, AgNO3,AgNO2, Ag2O, AgO, AgClO4, AgMnO4, Ag3PO4, Ag2SO4, Ag2S, AgSCN, AuBr3, AuCl3, AuCN,Au(OH)3, AuI, AuI3, Au2O3, Au2S, Au2S3, Zn(CH3COO)2, ZnBr2, ZnCO3, ZnCl2, Zn(CN)2, ZnF2,Zn(OH)2, ZnI2, Zn(NO3)2, ZnO, Zn(ClO4)2, ZnSO4, ZnS, Cd(CH3COO)2, CdBr2, CdCO3, CdCl2, CdF2,Cd(OH)2, CdI2, Cd(NO3)2, CdO, Cd(ClO4)2, CdSO4, CdS, Hg(CH3COO)2, HgBr2, Hg2Cl2, HgCl2,


2/69

Hg(CN)2, Hg2F2, HgF2, Hg2I2, HgI2, Hg2(NO3)2, Hg(NO3)2, HgO, Hg(ClO4)2, Hg2SO4, HgSO4, HgS,Hg(SCN)2, Ce(CH3COO)3, CeBr3, Ce2(CO3)3, CeCl3, CeF3, CeF4, Ce(OH)4, CeI3, Ce(NO3)3, CeO2,Ce(ClO4)3, Ce2(SO4)3, Ce(SO4)2, Pr(CH3COO)3, PrBr3, PrCl3, PrF3, Pr(NO3)3, Pr(ClO4)3, Pr2(SO4)3,Nd(CH3COO)3, NdBr3, Nd2(CO3)3, NdCl3, NdF3, NdI3, Nd(NO3)3, NdO, Nd2O3, Nd(ClO4)3,Nd2(SO4)3, PmF3, Pm(OH)3, Pm2(SO4)3, Sm(CH3COO)3, SmBr3, SmCl3, SmF3, SmI2, Sm(NO3)3,SmO, Sm2O3, Sm(ClO4)3, Sm2(SO4)3, Eu(CH3COO)3, Eu2(CO3)3, EuCl2, EuCl3, EuF3, Eu(NO3)3,EuO, Eu2O3, Eu(ClO4)3, Eu2(SO4)3, Gd(CH3COO)3, GdBr3, Gd2(CO3)3, GdCl3, GdF3, Gd(NO3)3,Gd2O3, Gd(ClO4)3, Gd2(SO4)3, Tb(CH3COO)3, TbBr3, Tb2(CO3)3, TbCl3, TbF3, TbI3, Tb(NO3)3,Tb(ClO4)3, Tb2(SO4)3, Dy(CH3COO)3, DyBr3, DyCl3, DyF3, DyI3, Dy(NO3)3, Dy2O3, Dy(ClO4)3,Dy2(SO4)3, HoBr3, Ho2(CO3)3, HoCl3, HoF3, HoI3, Ho(NO3)3, Ho2O3, Ho(ClO4)3, Ho2(SO4)3,Er(CH3COO)3, ErBr3, Er2(CO3)3, ErCl3, ErF3, ErI3, Er(NO3)3, Er2O3, Er(ClO4)3, Er2(SO4)3,Tm(CH3COO)3, TmBr3, Tm2(CO3)3, TmCl3, TmF3, TmI3, Tm(NO3)3, Tm2O3, Tm(ClO4)3, Tm2(SO4)3,Yb(CH3COO)3, YbBr3, YbCl3, YbF3, Yb(NO3)3, YbO, Yb2O3, Yb2(SO4)3, Lu(CH3COO)3, LuCl3,LuF3, Lu(NO3)3, Lu2O3, Lu(ClO4)3, Lu2(SO4)3, ThO2, PaO2, Pa2O5, PaI5, UF3, UF6, UO2, U2O5, UO3,NpF3, NpO2, PuF3, Pu2O3, PuO2, AmF3, AmI2, Am2O3, AmO2, CmF3, Cm2O3, CmO2, BkF3, Bk2O3,BkO2, CfF3, CfI2, Cf2O3, CfO2, EsCl3, Es2O3

3. Give the formulas of the following compounds: (see complete list in question 2).4. Give the formulas of the chemicals for the following Latin namesnatrium chloratum, natrium hypochlorosum, natrium chlorosum, natrium chloricum, natriumperchloricum, natrium hydroxydatum, natrium sulfuricum, natrium sulfurosum, natrium nitricum,natrium nitrosum, natrium carbonicum, natrium flouratum, natrium bromatum, natrium iodatum,kalium chloratum, kalium hypochlorosum, kalium chlorosum, kalium chloricum, kaliumperchloricum, kalium hydroxydatum, kalium sulfuricum, kalium sulfurosum, kalium nitricum, kaliumnitrosum, kalium carbonicum, kalium flouratum, kalium bromatum, kalium iodatum, magnesiumchloratum, magnesium perchloricum, magnesium hydroxydatum, magnesium sulfuricum, magnesiumcarbonicum, magnesium flouratum, magnesium bromatum, magnesium oxydatum, acidum

perchloricum, acidum sulfuricum, acidum nitricum, acidum carbonicum

5. Give the oxidation numbers of all atoms in the following compounds:H2CO3 , H2Cr2O7, H2CrO4, HMnO4, H2S, NH3, H2O, H2O2, HIO3, HClO4, HBrO3, HClO3, HClO2,H2SO4, HClO, HI, HBr, HF, HCl, H2S2O3, H2SO3, HNO2, HNO3, H3PO4, NH4Cl, NH4Br, NH4F,NH4I, NH4NO3, (NH4)2SO4, (NH4)3PO4, (NH4)2CO3, LiCl, LiBr, LiF, LiI, Li2O, LiNO3, Li2SO4,Li3PO4, Li2CO3, LiOH, NaCl, NaBr, NaF, NaI, NaNO3, NaNO2, Na2SO4, NaHSO4, Na2SO3, NaHSO3,Na2S, NaHS, Na2S2O3, Na3PO4, Na2HPO4, NaH2PO4, Na2CO3, NaHCO3, NaOH, NaClO, NaClO2,NaClO3, NaClO4, NaBrO3, NaIO3, KCl, KBr, KF, KI, KNO3, KNO2, K2SO4, KHSO4, K2SO3, KHSO3,K2S, KHS, K2S2O3, K3PO4, K2HPO4, KH2PO4, K2CO3, KHCO3, KOH, KClO, KClO2, KClO3, KClO4,KBrO3, KIO3, K2CrO4, K2Cr2O7, KMnO4, RbCl, RbBr, RbF, RbI, RbNO3, Rb2SO4, Rb3PO4, Rb2CO3,

RbOH, CsCl, CsBr, CsF, CsI, CsNO3, Cs2SO4, Cs3PO4, Cs2CO3, CsOH, MgF2, MgCl2, MgBr2, MgI2,MgO, MgSO4, MgCO3, Mg(HCO3)2, Mg(OH)2, Mg(NO3)2, CaF2, CaCl2, CaBr2, CaI2, CaO, CaSO4,CaCO3, Ca(HCO3)2, Ca(OH)2, Ca(NO3)2, SrF2, SrCl2, SrBr2, SrI2, SrO, SrSO4, SrCO3, Sr(HCO3)2,Sr(OH)2, Sr(NO3)2, BaF2, BaCl2, BaBr2, BaI2, BaO, BaSO4, BaCO3, Ba(HCO3)2, Ba(OH)2, Ba(NO3)2,BeF2, BeCl2, BeBr2, BeO, Be(OH)2, BF3, BCl3, BBr3, BI3, B2O3, AlF3, AlCl3, AlBr3, AlI3, Al2O3,Al(NO3)3, Al2(SO4)3, Al(OH)3, AlPO4, GaF3, GaCl3, GaBr3, GaI3, Ga2O3, Ga(NO3)3, Ga2(SO4)3,Ga(OH)3, GaPO4, InF3, In2O3, In(NO3)3, In2(SO4)3, In(OH)3, InPO4, TlF3, Tl2O3, Tl(NO3)3, Tl2(SO4)3,Tl(OH)3, TlF, Tl2O, CO2, CO, CF4, SiO2, GeO2, GeF4, SnF2, SnF4, SnO, SnO2, PbF2, PbO, PbO2, NF3,N2O, NO, N2O3, NO2, N2O4, N2O5, P2O5, P2O3, As2O3, As2O5, SbF3, SbF5, Sb2O3, Sb2O5, BiF3, Bi2O3,SO2, SO3, SF6, SeO2, TeO2, ClF, ClF3,ClF5, Cl2O, ClO2, BrF, BrF3, BrF5, Br2O, Br2O3, IF, IF3, IF5,I2O5, XeF2, XeF4, XeF6, XeO3, XeO4, KrF2, Sc2O3, YF3, Y2O3, LaF3, La(OH)3, La2O3, TiF3, TiF4,TiO2, ZrF4, ZrO2, HfF4, HfO2, VF3, VF4, V2O3, V2O5, NbF5, NbO, NbO2, Nb2O5, TaF5, Ta2O5, CrF2,CrF3, Cr2O3, CrO2, CrO3, MoF4, MoO2, MoO3, WF6, WO2, WO3, MnF2, MnF3, MnO, Mn2O3, MnO2,Mn2O7, TcF5, TcF6, TcO2, Tc2O7, ReF6, ReO2, ReO3, Re2O7, FeF2, FeF3, FeO, Fe2O3, RuO2, OsO4,


3/69

CoF2, Co(OH)2, CoO, Rh2O3, IrO2, NiF2, Ni(OH)2, NiO, PdO, PtO2, CuF2, Cu(OH)2, Cu2O, CuO,AgF, Ag2O, AgO, Au(OH)3, Au2O3, ZnF2, Zn(OH)2, ZnO, CdF2, Cd(OH)2, CdO, Hg2F2, HgF2, HgO,CeF3, CeF4, Ce(OH)4, CeO2, PrF3, NdF3, NdO, Nd2O3, PmF3, Pm(OH)3, SmF3, SmO, Sm2O3, EuF3,EuO, Eu2O3, GdF3, Gd2O3, TbF3, DyF3, Dy2O3, HoF3, Ho2O3, ErF3, Er2O3, TmF3, Tm2O3, YbF3, YbO,Yb2O3, LuF3, Lu2O3, ThO2, PaO2, Pa2O5, UF3, UF6, UO2, U2O5, UO3, NpF3, NpO2, PuF3, Pu2O3,PuO2, AmF3, Am2O3, AmO2, CmF3, Cm2O3, CmO2, BkF3, Bk2O3, BkO2, CfF3, Cf2O3, CfO2, Es2O3

6. Balance the following chemical equations.....CaO + ....H2O = ....Ca(OH)2....N2O4 = ....NO2....Ca(OH)2 + ....H3PO4 = ....Ca3(PO4)2 + ....H2O....Al(OH)3 + ....HCl = ....AlCl3+ ....H2O....AgNO3 + ....H2SO4 = ....Ag2SO4+ ....HNO3....N2 + ....H2 = ....NH3....HgO = ....Hg + ....O2....NaCl + ....H2SO4 = ....Na2SO4 + ....HCl....H2 + ....Cl2 = ....HCl

....NaHCO3 + ....C6H8O7 = ....CO2 + ....Na3C6H5O7 + ....H2O....HNO3 + ....P4O10 = ....(HPO3)3 + ....N2O5

....CO2 + ....H2O = ....C6H12O6 + ....O2

....NaHCO3 = ....Na2CO3 + ....H2O + ....CO2

....Fe + ....O2 = ....Fe2O3

....FeO + ....O2 = ....Fe2O3

....FeS2 + ....O2 = ....Fe3O4 + ....SO2

....CuFeS2 + ....O2 = ....Fe3O4 + ....CuO + ....SO2

....C8H18 + ....O2 = ....CO2 + ....H2O

....NH3 + ....O2 = ....HNO3 + ....H2O

....Fe2O3 + ....CO = ....Fe3O4 + ....CO2

....Fe3O4 + ....CO = ....FeO + ....CO2....Au2S3 + ....H2 = ....Au + ....H2S

....Ce + ....HCl = ....CeCl3 + ....H2

....Eu + ....HF = ....EuF3 + ....H2

....Ca + ....H2O = ....Ca(OH)2 + ....H2

....Al + ....H2O + ....NaOH = ....Na[Al(OH)4] + ....H2

....Zn + ....H2O + ....NaOH = ....Na2[Zn(OH)4] + ....H2

....Cu + ....AgNO3 = ....Cu(NO3)2 + ....Ag

....Cu + ....HNO3 = ....Cu(NO3)2 + ....NO + ....H2O

....P + ....HNO3 = ....H3PO4 + ....NO2 + ....H2O

....Ag + ....H2SO4 = ....Ag2SO4 + ....SO2 + ....H2O

....CS2 + ....NH3 = ....H2S + ....NH4SCN

....Cu(OH)2 + ....NH3 = ....[Cu(NH3)4](OH)2

....Na[Cr(OH)4] + ....H2O2 + ....NaOH = ....Na2CrO4 + ....H2O

....KI + ....H2O2 = ....I2 + ....KOH

....H2S + ....H2SO3 = ....S + ....H2O

....Hg2I2 + ....KI = ....K2[HgI4] + ....Hg

....CuCl2 + ....NaCN = ....Na[Cu(CN)2] + ....(CN)2 + ....NaCl

....NO2 + ....NaOH = ....NaNO2 + ....NaNO3 + ....H2O

....NO + ....CsOH = ....CsNO2 + ....N2 + ....H2O

....NH4NO3 = ....N2O + ....H2O

....CaH2 + ....H2O = ....Ca(OH)2 + ....H2

....NaBH4 + ....H2O = ....NaB(OH)4 + ....H2

....C6H4O2 + ....H2O = ....C6H6O2 + ....O2

....MnO4 + ....(COOH)2 + ....H

+ = ....Mn2+ + ....CO2 + ....H2O


4/69

....Cr2O72 + ....NH2Cl + ....H

+ = ....Cr3+ + ....N2 + ....Cl + ....H2O

....MnO4 + ....NH2OH + ....H

+ = ....Mn2+ + ....N2 + ....H2O....KMnO4 + ....Na2SO3 + ....H2O = ....MnO2 + ....Na2SO4 + ....KOH....CH3CHO + ....[Cu(NH3)4](OH)2 = ....CH3COOH + ....Cu2O + ....H2O +....NH3

7. Give the usual letter used to refer to the following physical properties or constants:

amount of substance, mass, length, temperature, volume, pressure, density, energy, internal energy,enthalpy, entropy, free energy, rate constant, equilibrium constant, degree of dissociation, stabilityproduct, concentration, mole fraction, gas constant, molar weight, osmotic pressure, heat, heatcapacity, specific heat, principal quantum number, angular-momentum quantum number, magneticquantum number, spin quantum number, speed of light, Plancks constant, wavelength, frequency,atomic number, mass number, effective nuclear charge, half-life

8. Give the definition of the following physical or chemical terms:percent yield, molarity, molality, mole fraction, atomic number, mass number, pressure, density,average molar weight of a mixture, weight percent, ppm, ppb

9. Decide if the following compounds are non-electrolytes, weak electrolytes, or strong electrolytes:HCl, HBr, HI, HF, HClO4, CH3COOH, CH3OH, HNO3, HCOOH, C2H5OH, H2SO4, H3PO4, C12H22O11(common sugar), KBr, NaCl, NaOH, KOH

10. Select the properties the precise absolute value of which can be determined by measurements.temperature, internal energy, heat, pressure, enthalpy, electric potential, entropy, specific heat, freeenergy, viscosity

11. Select the properties for which only changes, but not the precise absolute values can be determinedby measurements.temperature, internal energy, heat, pressure, enthalpy, electric potential, entropy, specific heat, free

energy, viscosity


5/69

12. How many of the following numbers have 4 significant figures?3.0156 16.00 0.004 1.35 104 0.001405

a) 5 b) 2 c) 1 d) 4 e) 3

13. How many of the following numbers have 4 significant figures?4.009 21.00 0.4023 2.160 104 0.001409

a) 3 b) 1 c) 4 d) 2 e) 514. How many significant figures are in the number 3.0 10-6?a) four b) three c) two d) six e) five

15. Calculate the following to the correct number of significant figures.2123.1 + 1.2340 = _____

a) 2124 b) 2124.3340 c) 2124.3 d) 2124.33 e) 2124.334

16. Calculate the following to the correct number of significant figures.4.302 0.0122 = _____

a) 4.2898 b) 4.289 c) 4.290 d) 4.29 e) 4.30

17. Calculate the following to the correct number of significant figures.10.23 + 4.355 = _____

a) 15 b) 14.59 c) 14.585 d) 14.6 e) 14.58

18. Calculate the following to the correct number of significant figures.4.32 / 0.2432 = _____

a) 18 b) 17.8 c) 17.76 d) 17.763 e) 17.76315789

19. Calculate the following to the correct number of significant figures.

2.34 / 0.12 = _____a) 0.281 b) 19.5 c) 2.0 101 d) 0.28 e) 2 101

20. Calculate the following to the correct number of significant figures.23.1 x 0.0012 = _____

a) 0.03 b) 2.77 102 c) 0.028 d) 0.0277 e) 0.2772

21. Calculate the following to the correct number of significant figures.( 42.7 + 0.259 ) / 28.4445 = _____

a) 1.5103 b) 1.510 c) 1.51 d) 1.5 e) 2

22. Do the indicated arithmetic and give the answer to the correct number of significant figures.(0.00015 x 54.6) + 1.0020 = _____

a) 1.010 b) 1.0102 c) 1.01019 d) 1.01 e) 1.0

23. The correct value of the following expression is:(1050 x 10-20)2 / (10-60)1/3 = _____

a) 1090 b) 1060 c) 1040 d) 1080 e) 1070

24. Round off the quantity 785.4 g to the nearest 0.1 kg.a) 1.0 kg b) 0.79 kg c) 0.785 kg d) 0.8 kg e) 7.8 kg

25. Express the quantity 956 mL in L rounded to the nearest 0.1 L.a) 1 L b) 0.9 L c) 0.95 L d) 0.96 L e) 1.0 L


6/69

26. Round off the quantity 10.256 m to the nearest 0.1 m.a) 10.2 m b) 10.3 m c) 10.25 m d) 10.26 e) 10.256

27. Which of the following metric relationships is incorrect?a) 1 kilogram = 104 decigrams b) 1 nanogram = 103 micrograms c) 1 microliter = 10-6 litersd) 1 kilogram = 106 milligrams e) 100 centimeters = 1 meter

28. In which of the following sequences are the prefixes of the metric system listed in order ofincreasing size?a) nano, milli, micro b) deci, mega, kilo c) deci, micro, kilod) micro, deci, centi e) nano, milli, centi

29. A frog's egg is about 1.5 103 micrometers in diameter. What is the equivalent diameter isnanometers?a) 1.5 103 b) 1.5 c) 1.5 106 d) 1.5 10-3 e) 1.5 101

30. How many 0.1-g doses of tetracycline can be supplied from 1 kg of tetracycline?

a) 1 107

b) 1 102

c) 1 105

d) 1 104

e) 1 103

31. How many 50 cg tablets of aspirin can be produced from 5 kg of aspirin?a) 1 102 b) 1 106 c) 1 105 d) 1 104 e) 1 103

32. A cigarette contains 2.5 102 milligrams of nickel. How many micrograms of nickel are in thecigarette?a) 0.0025 g b) 0.25 g c) 2.5 g d) 25 g e) 0.025 g

33. During a severe pollution period in a European city, the concentration of lead in the air was 3.0 x10-6 g per cubic meter. What was the concentration expressed in milligrams per liter?

a) 3.0 10-12 mg/L b) 3.0 10-9 mg/L c) 3.0 10-3 mg/L d) 3.0 10-6 mg/L e) 3.0 mg/L

34. The melting point of methane is -182oC. What is the equivalent temperature on the Kelvin scale?a) 123 K b) -230 K c) -91 K d) 230 K e) 91 K

35. A sample of 6 g of lead at 20oC and a sample of 8 g of zinc at 30oC are placed in contact with eachother. We can conclude that:a) the lead will cool b) heat will flow from lead to zincc) the temperature of the lead will decrease d) the temperature of the zinc will decrease

36. A brand of gasoline can be shown to be a mixture by:a) reacting it with oxygen b) burning it c) smelling itd) determining its density e) separating it into its components

37. The best way to determine whether a sample of a white solid is table sugar would be to:a) taste it b) dissolve it in water c) burn it d) weigh it e) determine its melting point

38. Which of the following contains the largest number of neutrons?a) 19482Pb b)

19080Hg c)

19281Tl d)

20680Hg e)

19682Pb

39. Which of the following pairs of subatomic particles have essentially the same mass?

a) neutron and nucleus b) proton and electron c) proton and neutrond) anion and cation e) neutron and electron


7/69

40. A cation has a positive charge because:a) there are more protons than neutrons b) there are fewer electrons than protonsc) the neutrons in the nucleus are charged d) it has a positively charged nucleuse) there are more electrons than protons

41. Gain of two electrons by a neutral atom results in the formation of:a) a cation b) a polyatomic ion c) a neutron d) an anion e) an isotope

42. The total number of atoms represented by UO2 (ClO4)2 is:a) 9 b) 13 c) 10 d) 11 e) 12

43. The total number of atoms represented by Ca(C2H3O2)2 is:a) 17 b) 15 c) 14 d) 13 e) 11

44. The total number of atoms represented by Cd(MnO4)2 is:a) 12 b) 9 c) 10 d) 11 e) 8

45. A reaction mechanism is composed of the following two gas-phase elementary steps:N2O N2 + ON2O + O N2 + O2

45.1. What is the overall reaction? (1 correct answer)a) N2 + O N2O b) N2O N2 + Oc) N2O + O N2 + O2 d) 2N2O 2N2 + O2e) N2 + O2 N2O + O

45.2. What is the reactant? (1 correct answer)a) N2 b) O2 c) N2O d) O e) none of these species

45.3. What is the intermediate? (1 correct answer)a) N2 b) O2 c) N2O d) O e) none of these species

45.4. What is the catalyst? (1 correct answer)a) N2 b) O2 c) N2O d) O e) none of these species

45.5. What are the products? (2 correct answers)a) N2 b) O2 c) N2O d) O e) none of these species

46. A reaction mechanism is composed of the following two solution-phase elementary steps:H2O2 + I

H2O + IOH2O2 + IO

H2O + O2 + I46.1. What is the overall reaction? (1 correct answer)

a) 2 H2O2 2 H2O + O2 b) IO + H2O H2O2 + IO

c) IO

+ I

+ 2H+

I2 + H2O d) H2O2 + IO

H2O + O2 + IO

e) H2O2 + I

H2O + IO46.2. What is the reactant? (1 correct answer)

a) H2O b) O2 c) H2O2 d) I e) IO

46.3. What is the intermediate? (1 correct answer)a) none of these species b) O2 c) H2O2 d) I

e) IO46.4. What is the catalyst? (1 correct answer)

a) H2O b) none of these species c) H2O2 d) I e) IO

46.5. What are the products? (2 correct answers)a) H2O b) O2 c) H2O2 d) I

e) IO


8/69

47. A reaction mechanism is composed of the following three gas-phase elementary steps:O2 + NO NO2 +ONO2 NO + OO + O2 O3

47.1. What is the overall reaction? (1 correct answer)a) O2 + NO NO2 +O b) O + O2 O3

c) NO2 NO + O d) 2NO + O2 2 NO2e) 3O2 2O347.2. What is the reactant? (1 correct answer)

a) O2 b) NO c) NO2 d)O e) O347.3. What are the intermediates? (2 correct answers)

a) O2 b) NO c) NO2 d)O e) O347.4. What is the catalyst? (1 correct answer)

a) O2 b) NO c) none of these species d)O e) O347.5. What is the product? (1 correct answer)

a) O2 b) NO c) NO2 d)O e) O3

48. Which is an INCORRECT statement regarding the SI system of units?a) The basic unit of mass in the SI system is the gram.b) The basic unit of length in the SI system is the meter.c) The basic unit of time in the SI system is the second.d) The basic unit of volume in the SI system is the cubic meter.e) The basic unit for amount of substance in the SI system is the mole.

49. Which distance is the largest? (Given: 1 ngstrom = 1 10-10 m)a) 5 ngstroms b) 1 nm c) 10-7 mm d) 100 pm e) all are the same

50. Which of the following property is an intensive property of a material?a) energy b) volume c) density d) mass e) amount of substance

51. Which state of matter does not completely fill its container and has no definite shape of its own?a) gas b) liquid c) solid d) none of these

52. Which state of matter is most easily compressed?a) gas b) liquid c) solid d) all are the same

53. Which of the following substance classifications isNOT CORRECT?a) air = homogeneous mixture b) chlorine = element

c) sodium chloride = compound d) ice-cream with chocolate = homogeneous mixture54. Below are five properties concerning a sample of elemental gallium. Which of the followinganswers specifies all the intensive properties?

I. The temperature of the sample is 18oC.II. The mass of the sample is 16.2 grams.III. The volume of the sample is 2.74 cm3.IV. The density of the sample is 5.9 g/cm3.V. The sample reacts readily with fluorine.

a) I and IV b) IV and V c) II and III d) I, IV, and V

55. Which of the following is an example of a compound?a) aluminum b) sodium bicarbonate c) air d) mud


9/69

56. Which of the following processes are exothermic?I. Combustion of natural gas. II. Freezing water. III. Melting ice.IV. Boiling water. V. Condensing steam.a) III, IV and V b) I, II, and III c) III and IV d) I, II and V e) all ofthem

57. Which of the following statements is FALSE?a) Different mixtures of the same two substances can have different compositions.b) Compounds are composed of two or more elements in fixed proportions.c) A solution is a homogeneous mixture.d) Elements cannot be decomposed into simpler substances by chemical means.e) A heterogeneous mixture has a constant composition throughout.

58. Which of the following materials is NOT a pure substance?a) ethyl alcohol b) salt c) aspirin d) iron e) cheese

59. The statement that the total mass does not change in a chemical reaction is the law of:

a) Conservation of Mass b) Definite Proportions c) Evolutiond) Greatest Simplicity e) Thermodynamics

60. From the decomposition of an unknown solid, one obtains a gas and a new solid, both of which arepure substances. From just this information it can be said, without a doubt, that:a) one of the products is an element b) neither product is an elementc) both products are elements d) the original solid is not an element

61. Which of the following properties do liquids and gases have in common?a) they expand slightly on heating b) they will flow c) they are rigidd) they are easily compressed e) they expand to fill their container

62. The fact that compound calcium carbonate is made up of 40% calcium, 12% carbon, and 48%oxygen is an illustration of the law of:a) Definite Proportions b) Conservation of Mass and Energy c) the Jungled) Multiple Proportions e) Transmutation

63. Which of the following properties is an example of an EXTENSIVE property of a material?a) density b) mass c) reactivity with oxygen d) temperature e) boiling point

64. Which of the following materials has NOT been properly classified?a) filtered air = heterogeneous mixture b) hot tea (with no cream or sugar) = homogeneous

mixturec) diamond = element d) wood = heterogeneous mixture e) pure table salt = compound

65. Which number below is INCORRECTLY converted to or from scientific notation?a) 0.0037 = 3.7 x 103 b) 1.862 x 10-2 = 0.01862 c) 32,656 = 3.2656 x 104d) 96.4 x 103 = 96,400 e) all are converted correctly

66. In which item below is the result expressedINCORRECTLY in terms of number of significantfigures?a) 3.14 x 2.584 = 8.11 b) 0.003/0.0015 = 2 c) 1.314 + 189.71 = 191.0d) 96.4 x 103 = 96,400 e) all results are expressed to the appropriate number of significantfigures


10/69

67. Which of the following materials is NOT a pure substance?a) ethyl alcohol, CH3CH2OH b) salt, NaCl c) CaCO3 (calcium carbonate)d) milk e) diamond

68. Which of the following properties do liquids and solids have in common?a) they expand contract slightly upon heating b) they are both fluidsc) they are rigid d) they are difficult to compress e) they expand to fill all available volume

69. Which of the following is NOT an SI unit of that measured quantity?a) Length is expressed in meters b) Energy is expressed in caloriesc) Time is expressed in seconds d) Mass is expressed in kilogramse) Temperature is expressed in Kelvin

70. Which of the following is the biggest length? (1 Angstrom = 10-10m)a) 10 nm b) 0.1 m c) 104 pm d) 100 Angstroms e) all are equal lengths

71. A braking automobile converts kinetic energy into heat energy in the brake pads. This is an

example of the:a) law of conservation of energy b) law of constant compositionc) law of conservation of mass d) law of gravity

72. One of the following does NOT describe gases. Which one is it?a) particles far apart b) rigid shape c) easily compressed d) relatively low densities

73. Which of the following is a compound and NOT an element or mixture?a) ethyl alcohol b) crude oil c) neon d) sulfur

74. Which of the following is NOT a mixture?

a) air b) milk c) oxygen d) seawater

75. Which of the following numbers has 4 significant figures?a) 0.04309 b) 0.0430 c) 0.043090 d) 0.43980

76. Which of the following is an intensive property of matter?a) mass b) density c) volume d) weight e) heat capacity

77. Which of the following are heterogeneous mixtures?I. sugarII. sugar dissolved in water

III. an aqueous suspension of magnesium hydroxide (milk of magnesia)IV. samples of nitrogen and oxygen in the same containerV. samples of argon and iron in the same container

a) III only b) I, II, and IV c) III and V d) III and IV e) II, IV, and V

78. Liquid propane boils at 231K. What is its boiling point in C ?a) 42C b) 315C c) -42C d) 504C e) -231C

79. Identify the compound below which is an ionic compound.a) CH4 b) H2O2 c) Na2CO3 d) NH3 e) SO2


11/69

80. Identify the INCORRECT statement below:a) The atomic weight is the number of atoms in one mole of the element.b) The electron and proton have charges of equal magnitude and opposite sign.c) The atomic number is the number of protons in the nucleus.d) An atom is the smallest particle of an element that maintains the chemical identity of that element.e) The number above the element symbol on the periodic chart is the atomic number.

81. Identify the INCORRECT statement below:a) Atoms cannot be created, destroyed, or transformed into atoms of another element except bynuclear reactions.b) Some elements exist in pure form as polyatomic molecules.c) All atoms of a given element have identical properties, which differ from those of other elements.d) Compounds form when masses of different elements combine in small whole-number ratios.e) The relative numbers and kinds of atoms are constant in a given compound.

82. Identify the compound below which is a molecular compound:a) CaF2 b) NaCl c) Na2CO3 d) NH4NO3 e) SO3

83. Which has a greater mass?a) 1 atom of iron b) 1 atom of Neon c) 1 molecule of carbon dioxide d) 1 molecule ofwater

84. The fact that water is always found to be 89% Oxygen and 11% Hydrogen by mass is an exampleof:a) The Law of Conservation of Matter b) The Law of Conservation of Energyc) The Law of Multiple Proportions d) The Law of Definite Proportionse) Daltons theory of atoms

85. Which of the following species DOES NOT represent an element in its most stable form?a) H2 b) Br c) S8 d) P4 e) Ne

86. Which of the following is NOT an ionic compound?a) LiF b) CCl4 c) NH4Cl d) FeSO4

87. A doubly negative ion, symbolized by X2-, forms a compound with a metal M, of the formulaM2X. What is the charge on the metal, M?a) +1 b) +2 c) +3 d) +4

88. Which of the following statements is incorrect?

a) A molecule is the smallest part of a compound that can have a stable independent existence.b) Molecules that consist of more than one atom are called polyatomic molecules.c) The atomic number of an element is defined as the number of neutrons in the nucleus.d) Molecules of compounds are composed of more than one kind of atom.

89. Which of the following statements is not an idea from Daltons Atomic Theory?a) An element is composed of extremely small indivisible particles called atoms.b) All atoms of a given element have identical properties which differ from those of all other elements.c) Atoms can only be transformed into atoms of another element by nuclear reactions.d) Compounds are formed when atoms of different elements combine with each other in small whole-number ratios.e) The relative numbers and kind of atoms are consistent in a given compound.


12/69

90. Identify the compound below which is an ionic compound.a) CO2 b) H2O2 c) CaSO4 d) H2O e) SO3

91. Identify the compound formula that is INCORRECT.a) Mg3(PO4)2 for magnesium phosphate b) Fe(NO3)2 for iron(II) nitratec) NaCO3 for sodium carbonate d) CuCl for cuprous chloridee) AgBr for silver bromide

92. Identify the INCORRECT statement below:a) The atomic weight of an element is the mass in grams of 6.022 x 1023 atoms of the element.b) Avogadro's number is the number of atoms in exactly 1 gram of Carbon-12.c) The electron and proton have charges of equal magnitude and opposite sign.d) The atomic number is the number of protons in the nucleus.e) The number above the element symbol on the periodic chart is the atomic number.

93. Which of the following species DOES NOT represent an element in its most stable form?a) N2 b) Cl c) S8 d) P4 e) He

94. Which of the following statements is INCORRECT?a) A molecule is the smallest part of a compound that can have a stable independent existence.b) The molar mass can be expressed in grams/mol.c) An amu is 1/12 the mass of one Carbon-12 atom.d) The atomic weight scale is based on the mass of an atom of Carbon (isotope 12).e) A gram of each different element consists of the same number of atoms.

95. Which of the following ions does NOT have a 1 charge?a) oxide b) fluoride c) hydroxide d) nitrate e) acetate

96. Which of the following elements in its pure stable form exists as a diatomic molecule?a) Carbon b) Nitrogen c) Sulfur d) Phosphorus e) Iron

97. Which of the following compounds is INCORRECTLY classified as ionic versus molecular?a) H2O is a molecular compound b) NO2 is an ionic compoundc) HCl is a molecular compound d) CaO is an ionic compounde) NH4Cl is an ionic compound

98. Which of the following statements is INCORRECT?a) A molecule is the smallest particle of a compound that can have a stable independent existence.b) Molecules that consist of more than one atom are called polyatomic molecules.

c) The atomic number of an element is defined as the number of neutrons in the nucleus.d) Molecules of compounds are composed of more than one kind of atom.e) The charge on an electron is negative, and the charge on a proton is positive.

99. Which of the following statements is INCORRECT?a) A molecule of potassium chloride, KCl, consists of one K+ ion and one Clion.b) Ions that possess a positive charge are called cations.c) Polyatomic ions are groups of atoms that have an electric charge.d) It is acceptable to use a formula to refer to either an ionic compound or a molecular compound.e) Ions that possess a negative charge are called anions.


13/69

100. Each response below lists an ion by name and by chemical symbol or formula. Also each ion isclassified as monatonic or polyatomic and as a cation or anion. Which response contains anERROR?a) phosphate; PO4

3- ; polyatomic; anion b) sulfite; SO32- ; polyatomic; anion

c) nitrite; NO3- ; polyatomic; anion d) iron(II); Fe2+ ; monatomic; cation

e) bromide; Br - ; monatomic; anion

101. Atoms are composed of:a) protons, neutrons, electrons b) protons, neutrinos, electionsc) positrons, neutrons, electrons d) positrons, neutrons, negatrons

102. Which of the following sets illustrates the Law of Multiple Proportions?a) Li2O, Na2O, K2O b) KCl, CaCl2, ScCl3 c) O, O2, O3 d) BrF, BrF2, BrF3

103. How many atoms are in a sulfuric acid molecule?a) 1 b) 7 c) 5 d) 6

104. Choose the correct answer:

a) cations have a positive charge, anions have a negative chargeb) anions have a positive charge, cations have a negative chargec) the opposite of a cat ion is a dog iond) ions cannot form in chemical reactions

105. Identify the INCORRECT statement below concerning an aqueous solution which is 0.1 M HClsolution:a) This solution is a homogeneous mixture of ionized HCl and H2O.b) In this solution water is the solute.c) The solvent is the dispersing medium, which is the substance present in greatest abundance.d) In this solution there are essentially no non-ionized HCl molecules present.

e) This solution has a high electrical conductivity.

106. Identify the INCORRECT statement below:a) Many properties of the elements are periodic functions of their atomic weight.b) The periodic law of the elements was first noted by Mendeleev in the mid-1800's.c) The vertical columns of the periodic chart are called groups, sharing similar properties.d) Elements with atomic numbers of 9, 17, 35, and 53 are the alkali metals.e) Elements Li, B, N and F are all in the same period.

107. Which of the following substances is a strong electrolyte?a) glucose b) acetic acid c) methyl alcohol d) water e) sodium hydroxide

108. Identify which substance below is NOT a strong acid in aqueous solution:a) HBr b) HCl c) HNO3 d) H2SO4 e) HF

109. Identify the strong base (in aqueous solution) from among the following compounds:a) Na2S b) Cu(NO3)2 c) NH3 d) NH4Cl e) KOH

110. Identify the substance below which is INSOLUBLE in water.a) Na2S b) Ca3(PO4)2 c) MgCl2 d) AgNO3 e) CaCl2

111. Which substance when dissolved in water would give rise to a solution which isHIGHLYconductive?a) sucrose b) sodium carbonate c) methyl alcohol d) acetic acid e) glucose


14/69

112. Which of the following reactions is not balanced?a) P4 + 3O2 P4O6 b) Cu(NO3)2 CuO + 2NO2 + O2c) 2Al2O3 + 3C + 6Cl2 4AlCl3 + 3CO2 d) 3PbO + 2NH3 3Pb + N2 + 3H2O

113. Which of the following is an alkaline earth metal?a) Zr b) Sn c) Ca d) Li e) Th

114. Which one of the following is a strong acid?a) HF b) HNO3 c) CH3COOH d) H2SO3 e) H2CO3

115. Which response includes all of the following that are redox reactions and no others?I. BaSO3 BaO + SO2 II. 2K + Br2 2KBrIII. H2CO3 + Ca(OH)2 CaCO3 + 2H2O IV. SnS2 + HCl H2SnCl6 + 2H2SV. 3Cl2 + 6KOH 5KCl + KClO3 + 3H2O

a) II, III, and IV b) I and III c) II and V d) I and IV e) another one or anothercombination

116. Which of the following equations is not balanced?a) Zn + 2HCl ZnCl2 + H2 b) 2Na + 2H2O 2NaOH + H2c) CH4 + 2O2 CO2 + 2H2O d) 2H2 + O2 2H2Oe) SO2 + O2 SO3

117. Stoichiometry deals with:a) primarily combustion reactions. b) mass or mole combining relationships in a chemical reaction.c) heat evolved by a chemical reaction. d) rates of chemical reactions.

118. Molarity is defined as:a) moles of solute per kilogram of solvent. b) moles of solute per moles of solution.c) grams of solute per liter of solution. d) moles of solvent per liter of solute.e) moles of solute per liter of solution.

119. Identify the CORRECT relationship below:a) Moles of solute present in solution equals concentration in molarity times the volume of solution inmilliliters.b) Moles of solute present in solution equals concentration in molarity times the volume of solution inLiters.c) Moles of solute present in solution equals % solute times the grams of solution.d) Grams of solute present in solution equals % solute times the grams of solution.

120. Which of the following equations is not balanced?a) BaO + 2 HCl BaCl2 + H2O b) Ca + 2 H2O Ca(OH)2 + 2 H2c) 2 C2H6 + 7 O2 4 CO2 + 6 H2O d) 2 SO2 + O2 2 SO3

121. What scientific law serves as the basis for balancing chemical equations by requiring that there beno observable change in the quantity of matter during a chemical reaction?a) Law of Conservation of Energy b) Law of Constant Compositionc) Law of Conservation of Mass d) Law of Definite Proportions

122. Two solutions are poured together. Which mixture of solutions produces a precipitate?

a) a solution of Na2S and a solution Cu(NO3)2 b) a solution of Na3PO4 and a solution of KClc) a solution of KNO3 and a solution of FeCl3 d) none of these produce a precipitate


15/69

123. Which of the following is the correct net ionic equation for the neutralization of HCl with KOHin aqueous solution?a) H+(aq) + OH-(aq) H2O(l)b) HCl(aq) + KOH(aq) KCl(aq) + H2Oc) H+(aq) + Cl-(aq) + K+(aq) + OH- (aq) K+(aq) + Cl-(aq) + H2Od) H+(aq) + KOH(aq) K+(aq) + H2O

124. In which of the following compounds is the oxidation number assignedINCORRECTLY?a) in KMnO4, the oxidation number of Mn is +7b) in H2CO3, the oxidation number of C is +1c) in Na2S, the oxidation number of S is 2d) in NaH, sodium hydride, the oxidation number of H is 1

125. Which of the following statements is INCORRECT?a) Reduction is an algebraic decrease in the oxidation number of an element with a corresponding gainof electrons.b) Combustion of methane is an example of an oxidation/reduction reaction.

c) Oxidation is an algebraic increase in the oxidation number of an element with a corresponding lossof electrons.d) In a redox reaction the oxidizing agent is the species that is oxidized.e) One cannot ever have an oxidation without also having a reduction simultaneously.

126. In the following reaction, which species is being reduced? FeBr3 + 3Cl2 2FeCl3 + 3Br2a) the Cl in Cl2 b) the Fe in FeBr3 c) the Br in FeBr3 d) this is not a redoxreaction

127. Which of the following reactions will NOT occur?a) CuSO4(aq) + Zn(s) Cu(s) + ZnSO4(aq) b) 2NaNO3(aq) + Zn(s) 2Na(s) + Zn(NO3)2(aq)c) 2AgNO2(aq) + Zn(s) 2Ag(s) + Zn(NO3)2(aq) d) 2HCl(aq) + Zn(s) H2(g) + ZnCl2(aq)

128. Which of the following matched pairs of name and formula has an error?a) CaF2 is calcium fluoride b) Na2S is sodium sulfatec) HCN is hydrogen cyanide d) KBr is potassium bromide

129. Which of the following matched pairs of name and formula has an error?a) SnBr2 is tin(II) bromide b) FeCl3 is ferric chloridec) Mn2O3 is manganese(II) oxide d) CuS is copper(II) sulfide

130. In which compound is nitrogen in the +1 oxidation state?a) N2O4 b) HNO3 c) N2 d) N2O e) none of these

131. Which reaction is NOT a redox reaction?a) CaCl2(aq) + Na2CO3(aq) CaCO3(s) + 2 NaCl(aq)b) 2 Na(s) + 2 H2O 2 NaOH + H2(g)c) 2 H2 + O2 2 H2Od) Zn(s) + Cu(NO3)2(aq) Zn(NO3)2(aq) + Cu(s)

132. In the following reaction identify the oxidizing agent: 2 Na(s) + H2 2 NaH(s)a) Na(s) b) NaH(s) c) H2(g) d) this is not a redox reaction


16/69

133. Which of the following is the correct NET IONIC reaction for the neutralization of acetic acid(CH3COOH) with Ca(OH)2?a) 2 CH3COOH + Ca(OH)2 Ca(CH3COO)2 + 2 H2Ob) H+ + OH H2Oc) CH3COOH + OH

CH3COO + H2Od) 2 H+ + Ca(OH)2 Ca2+ + 2 H2O

134. Which of the following is INCORRECTLY classified?a) CH3COOH / weak electrolyte b) HCl / strong electrolyte c) NaCl / strong electrolyted) NaOH / weak electrolyte e) H2O / nonelectrolyte

135. Which of the following compounds are INCORRECTLY classified (solubility refers to water)?a) NaBr / soluble b) KCrO4 / insoluble c) MgCl2 / solubled) AgCl / insoluble e) PbS / insoluble

136. Which of these is a weak acid?a) HNO3 b) H2SO4 c) HBr d) HI e) H2S

137. Solutions of BaCl2(aq), Na2SO4(aq) and KNO3(aq) are mixed together. What is the likelyprecipitate?a) NaNO3 b) Ba(NO3)2 c) BaSO4 d) KCl e) K2SO4

138. Which of the following mixtures would NOT lead to the evolution of hydrogen gas from anaqueous solution?a) Zn + 2 HCl b) Cu + 2 HCl c) K + H2O d) Na + H2SO4

139. Identify the INCORRECT statement regarding the periodic table.a) The properties of the elements are periodic function of their atomic number.

b) The periodic law was first noted by Mendeleev in the mid- 1800's.c) Elements with z = 2 and 10 have similar properties.d) Elements in horizontal rows have similar properties.e) The element magnesium is an alkaline earth metal.

140. Which is the net ionic reaction for the reaction of AgNO3(aq) with NaCl(aq)?a) AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)b) Ag+(aq) + Cl(aq) AgCl(s)c) AgNO3(aq) + Cl

(aq) AgCl(s) + NO3(aq)d) Ag+(aq) + NO3(aq) + Na

+(aq) + Cl(aq) AgCl(s) + Na+(aq) + NO3(aq)

141. Which is the net ionic reaction for the neutralization of acetic acid with sodium hydroxide?a) H+(aq) + OH(aq) H2Ob) H+(aq) + CH3COO

(aq) + Na+(aq) + OH- (aq) Na+(aq) + CH3COO(aq) + H2Oc) CH3COOH(aq) + OH

(aq) CH3COO(aq) + H2Od) H+(aq) + OH(aq) H2O + NaCH3COO(aq)

142. In the following reaction which species is being oxidized? Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s)a) Zn b) Cu2+ c) Zn2+ d) Cu e) this is not a redox reaction

143. Which below is the MOST active metal?

a) Sn b) Zn c) Cu d) Ag e) Li


17/69

144. Which metal below will NOT displace hydrogen gas from a solution of HCl(aq)?a) Na b) Zn c) Mg d) Cu e) Cs

145. How many of the three types of elementary particles are present in a neutral atom of14C?a) 12 protons, 14 neutrons, 12 electrons b) 6 protons, 8 neutrons, 6 electronsc) 6 protons, 6 neutrons, 6 electrons d) 12 protons, 8 neutrons, 12 electronse) 14 protons, 6 neutrons, 14 electrons

146. Identify the INCORRECT statement below:a) Light can be viewed as an electromagnetic wave.b) Light exists in particles called photons having energies directly proportional to their frequencies.c) The photoelectric effect led to the discovery of the particle-like nature of light.d) In the photoelectric effect, photons of high energy eject electrons from a metal.e) Red light (= 700 nm) has photons of greater energy than blue light (= 400 nm).

147. Which of the following are the formulas for the principle species in aqueous solution for(NH4)3PO4?

a) NH3 and H3PO4 b) NH2-

and H6PO4+3

c) NH4+

and PO4-3

d) This compound isinsoluble.

148. For the following reaction, which ions are the "spectator" (unreactive) ions?Pb(NO3)2(aq) + K2SO4(aq) PbSO4(s) + 2 KNO3(aq)

a) Pb+2 and SO42 b) K+ and NO3

c) K+ and SO42 d) Pb+2 and NO3

149. For the following acid/base reaction, the net ionic equation is: HBr + KOH KBr + H2Oa) K+ + OH KOH b) K+ + Br KBr c) Br + OH+ BrOH d) H+ + OH H2O

150. Which of the following compounds is soluble in water?

a) BaCO3 b) FeS c) CaSO4 d) AgNO3 e) PbCl2

151. Which one of the following salts is SOLUBLE in water?a) KClO3 b) BaSO4 c) Ag3PO4 d) CuS e) FeCO3

152. Which one of the following salts is INSOLUBLE in water?a) MgSO4 b) KNO3 c) AgBr d) FeCl3 e) NaBr

153. Which one of the following salts is soluble in water?a) FeS b) Ag2CO3 c) NH4F d) CrPO4 e) Hg2Cl2

154. Which one of the following salts is INSOLUBLE in water?a) K2S b) NaClO c) Mg(NO3)2 d) Rb2CO3 e) Ba3(PO4)2

155. Which of the following reactions is a decomposition reaction?a) 2 H2(g) + O2(g) 2 H2O(l) b) Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)c) 2 KClO3(s) 2 KCl(s) + 3 O2(g) d) 2 AgNO3(aq) + Zn(s) 2 Ag(s) + Zn(NO3)2(aq)

156. Which of the following is an oxidation-reduction (redox) reaction?a) FeCl2(aq) + 2 AgNO3(aq) 2 AgCl(aq) + Fe(NO3)2(aq)b) AgNO3(aq) + NaBr(aq) AgBr(s) + NaNO3(aq)

c) Zn(s) + 2 AgNO3(aq) 2 Ag(s) + Zn(NO3)2(aq)d) 3HCl(aq) + Cr(OH)3(s) CrCl3(aq) + 3H2O(l)


18/69

157. What is the reducing agent in the following reaction?Cu(s) + 4 H+(aq) + SO4

2(aq) Cu2+(aq) + 2 H2O(l) + SO2(g)a) Cu b) H+ c) SO4

2 d) Cu2+ e) SO2

158. In the following reaction CO is ____________. Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)a) the oxidizing agent and is oxidized. b) the oxidizing agent and is reduced.

c) the reducing agent and is oxidized. d) the reducing agent and is reduced.e) neither an oxidizing agent nor a reducing agent.

159. What is the net ionic equation for the following formula unit equation?Cu(NO3)2(aq) + H2S(aq) CuS(s) + 2 HNO3(aq)

a) Cu2+(aq) + H2S(aq) CuS(s) + 2 H+(aq)b) Cu2+(aq) + S2(aq) CuS(s)c) Cu2+(aq) + 2 H+(aq) + S2(aq) CuS(s) + 2 H+(aq)d) [Cu2+(aq) + 2 NO3

(aq)] + H2S(aq) CuS(s) + 2 [H+(aq) + 2 NO3(aq)]e) Cu2+(aq) + 2 NO3

(aq) + 2 H+(aq) + S2(aq) CuS(s) + 2 H+(aq) + 2 NO3(aq)

160. Will a precipitate form when 0.1 M aqueous solutions of CrCl3 and (NH4)2S are mixed? If it doesform, identify the precipitate and give the net ionic equation for the reaction.a) No precipitate formsb) NH4Cl precipitates: NH4+(aq) + Cl(aq) NH4Cl (s)c) Cr2S3 precipitates: 2 Cr

3+(aq) + 3 S2(aq) Cr2S3(s)d) Cr3S2 precipitates: 3 Cr

3+(aq) + 2 S2(aq) Cr3S2(s)e) Cr2S3 precipitates: 2 CrCl3(aq) + 3(NH4)2S(aq) Cr2S3(s) + 6 NH4Cl(aq)

161. The equation, 2 H+(aq) + CO32(aq) H2O(l) + CO2(g), is the net ionic equation for the reaction

of an aqueous mixture of:

a) CaCO3 and HCl. b) Na2CO3 and HCl. c) H2CO3 and NaOHd) BaCO3 and H2SO4. e) (COOH)2 and KOH.

162. Which one of the following salts is insoluble in water?a) Li3PO4 b) Na2SO4 c) (NH4)3AsO4 d) BaSO4 e) K2CO3

163. Which one of the following salts is insoluble in water?a) KHCO3 b) Mg3(PO4)2 c) AgNO3 d) CrCl3 e) (NH4)2S

164. Which one of the following is a strong acid?a) H2SO3 b) CH3COOH c) HF d) H2CO3 e) HNO3


a) Cu2+(aq) + H2S(aq) CuS(s) + 2 H+(aq)b) [Cu2+(aq)+2 NO3

(aq)] + H2S(aq) CuS(s) + 2[H+(aq)+2 NO3(aq)]c) Cu2+(aq) + S2-(aq) CuS(s)d) Cu2+(aq) + 2 H+(aq) + S2(aq) CuS(s) + 2 H+(aq)e) Cu2+(aq) + 2 NO3

(aq) + 2 H+(aq) + S2(aq) CuS(s) + 2 H+(aq) + 2 NO3(aq)


19/69

166. Which of the following statements about strong soluble bases isFALSE?a) They are composed of either alkali metals or some of the more reactive alkaline earth metals.b) They are all metal hydroxides.c) Their solutions conduct electricity.d) They are classified as weak electrolytes.e) They produce OH in aqueous solution.

167. Which one of the following salts is insoluble in water?a) FeCl2 b) PbS c) KCH3COO d) NH4Cl e) Pb(NO3)2

168. Which statement regarding nitric acid is FALSE?a) It is soluble in water. b) It only slightly ionizes in aqueous solution.c) Its solutions conduct electricity. d) It is a strong electrolyte.e) It produces H+ and NO3

- in aqueous solution.

169. Will a precipitate form when 0.1 M aqueous solutions of Ba(NO3)2 and H2CO3 are mixed? If aprecipitate does form, identify the precipitate and give the net ionic equation for the reaction.

a) No precipitate forms.b) BaCO3 precipitates. Ba2+(aq) + H2CO3(aq) BaCO3(s) + 2 H+(aq)

c) BaCO3 precipitates. Ba2+(aq) + H2CO3(aq) BaCO3(s) + H2(g)

d) H2(NO3)2 precipitates. 2 H+(aq) + 2 NO3

(aq) H2(NO3)2(s)e) BaCO3 precipitates. Ba

2+(aq) + CO32(aq) BaCO3(s)

170. Which one of the following represents the net ionic equation for the reaction of nitric acid withaluminum hydroxide?a) 3 NO3

(aq) + Al3+(aq) Al(NO3)3(aq)b) H+(aq) + OH(aq) H2O(l)c) 3 H+(aq) + Al(OH)3(s) Al3+(aq) + 3H2O(l)d) 3 HNO3(aq) + Al(OH)3(s) 3 Al(NO3)3(aq) + 3 H2O(l)e) 2 H+(aq) + Al(OH)2(s) Al2+(aq) + 2 H2O(l)

171. Which of the following equations is the net ionic equation for the reaction of iron(II) sulfide andhydrochloric acid?a) Fe2S3(s) + 6 H

+(aq) 3 H2S(g) + 2 Fe3+(aq) b) Fe2S(s) + 2 H+(aq) Fe22+ + H2S(g)c) Fe2+(aq) + 2 Cl FeCl2(s) d) FeS(s) + 2 H+(aq) Fe2+(aq) + H2S(g)e) S2(aq) + 2 H+(aq) 2 H2S(g)

172. Which response contains all of the following that are oxidation-reduction reactions and no

others?I. PCl3(l) + 3 H2O(l) 3 HCl(aq) + H 3PO3(aq)II. Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)III. CaCO3(s) + 2 HClO3(aq) Ca(ClO3)2(aq) + CO2(g) + H2O(l)

a) I and II b) III c) II and III d) I e) II

173. What is (are) the spectator (unreactive) ion(s) in the following reaction?2 HClO3(aq) + Sr(OH)2(aq) Sr(ClO3)2(aq) + 2 H2O(l)

a) H+ b) Sr2+, ClO3 c) OH d) Sr2+, OH e) H+, OH


20/69

174. Which of the following responses contains all the TRUE statements and no others?I. The elements at the far right of the periodic table, except the noble gases, have the greatest

tendency to form anions.II. The elements with the least tendency to form ions are those at the far left of the periodic

table.III. Bonds in compounds consisting of two adjacent elements in the periodic table are likely to

be covalent.IV. The elements at the far left of the periodic table possess poor electrical conductivity.

a) IV b) I, II, and III c) I and III d) II and IV e) I, II, and IV

175. Which one of the following is a strong acid?a) HNO2 b) H2SO3 c) HF d) HClO3 e) HClO


a) Cu2+(aq) + S2(aq) CuS(s)b) Cu2+(aq) + H2S(aq) CuS(s) + 2 H+(aq)

c) Cu2+

(aq) + 2 H+

(aq) + S2

(aq) CuS(s) + 2 H+

(aq)d) Cu2+(aq) + 2 NO3(aq) + 2 H+(aq) + S2(aq) CuS(s) + 2 H+(aq) + 2 NO3(aq)

e) [Cu2+(aq)+2 NO3(aq)] + H2S(aq) CuS(s) + 2[H+(aq) + 2 NO3(aq)]

177. Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope.a) 38 p, 38 n, 38 e b) 38 p, 90 n, 38 e c) 52 p, 38 n, 52 ed) 38 p, 52 n, 38 e e) 90 p, 38 n, 90 e

178. Which one of the following substances is insoluble in water?a) BaCO3 b) RbOH c) Na3PO4 d) KSCN e) LiBr

179. What is the reducing agent in the following reaction?Cu(s) + 4 H+(aq) + SO4

2(aq) Cu2+(aq) + 2 H2O(l) + SO2(g)a) SO4

2 b) Cu c) H+ d) Cu2+ e) SO2

180. Isotopes are atoms of the same element that:a) have different numbers of protons. b) have different numbers of neutrons.c) have different nuclear charges. d) have different atomic numbers.e) have different numbers of electrons.

181. Which response includes all of the following substances that are strong electrolytes, and no

others?I. K2CO3 II. HNO3 III. H2SO3 IV. CuCO3a) II, III, and IV b) I and IV c) I, II, and III d) III and IV e) I and II

182. Identify the INCORRECT statement below:a) The difference between the mass number of an atom and the atomic number is always equal to thenumber of protons.b) The mass number of an atom is the number of neutrons in the atom.c) The number of electrons in a neutral atom of an element is always equal to the atomic number of theelement.d) Atomic number is the number of protons in the nucleus of an atom.


21/69

183. Consider the following three statements:I. The mass of a proton and a neutron are virtually identical.II. The charge of an electron and a proton are equal but opposite.III. The mass of the electrons is a small fraction of the total mass of any atom.

a) All are correct. b) I and II are correct but III is false.c) II and III are correct but I is false. d) I and III are correct but II is false.

184. The neutral 31P isotope has how many protons, neutrons, and electrons?a) 15 p, 15 n, 15 e b) 31 p, 31 n, 31 e c) 15 p, 16 n, 15 e d) 16 p, 15 n, 15 e

185. The characteristic wavelength of a 1 kilogram object moving at 1 meter/second will be:a) about the size of the object itself.b) about the same as the that of the electron in an atom.c) large compared to the atomic scale.d) immeasurably small compared to any dimensions we care about.

186. Which is the following is an INCORRECT electron configuration?

a) Fe = [Ar]3d

6

4s

2

b) H = 1s

1

c) Se = [Ar]3d

10

4s

2

4p

4

d) O = [Ne]2s

2

2p

4

187. Identify the INCORRECT statement below:a) The total number of electrons that can have n=3 in a many-electron atom is 1.b) The total number of electrons that can fit in the 4f sublevel is 14.c) The total number of electrons that can fit in the 2px atomic orbital is 2.d) The total number of electrons required to fill the n=2 level is 8.

188. Identify the INCORRECT statement below:a) The mass number of an atom is the number of neutrons plus protons in the atom.b) The neutron has nearly the same mass as the proton but zero charge.

c) Two elements differ from one another by having a differing mass number.d) Atomic number is the number of protons in the nucleus of an atom.e) The mass of the electrons is a small fraction of the total mass of any atom.

189. The element Fluorine has only one really stable isotope. What is the composition of its nucleus?a) 19 protons b) 9 protons and 19 neutronsc) 9 protons and 10 neutrons d) 10 protons and 9 neutrons

190. A neutral atom of the 235U isotope has how many protons, neutrons, and electrons?a) 92 p, 143 n, 92 e b) 235 p, 235 n, 235 ec) 92 p, 92 n, 92 e d) 92 p, 235 n, 92 e

191. Rank the following types of radiation from highest energy to lowest:ultraviolet / visible / xray / microwave / infrared

a) xray, ultraviolet, microwave, infrared, visibleb) ultraviolet, xray, visible, infrared, microwavec) infrared, microwave, ultraviolet, visible, xrayd) xray, ultraviolet, infrared, visible, microwavee) xray, ultraviolet, visible, infrared, microwave


22/69

192. According to the de Broglie equation, the characteristic wavelength of an electron moving aroundan atomic nucleus will be:a) about the size of the nucleus.b) about the same size as the atom.c) large compared to the atomic scale.d) immeasurably small compared to any dimensions we care about.

193. Which of the following is an INCORRECT electron configuration?a) Ti = [Ar]4s24p2 b) S = [Ne]2s22p4 c) Li = 1s22s1 d) C = [He]2s22p2

194. Identify the INCORRECTstatement below:a) The total number of electrons required to fill the n=1 level is 2.b) The total number of electrons that can have n=2 in a many-electron atom is 8.c) The total number of electrons that can occupy an atomic orbital is 2.d) The total number of electrons that can "fit" in the 3d sublevel is 5.

195. The statement that no two electrons can have the same set of four quantum numbers in any atom

is a consequence of:a) The Aufbau Principle. b) The Heisenberg Uncertainty Principle.c) The Pauli Exclusion Principle. d) Hund's Rule.

196. Which of the following full notations for the electron state is consistent with the last electronadded in forming the electron configuration of Scandium (Sc)?a) (3, 2, 1, +1/2) b) (4, 0, 0, +1/2) c) (4, 2, 0, +1/2) d) (4, 2, 1, +1/2)

197. Fill in the blank: The l quantum number tells which sublevel the electron is in and most directlyspecifies the _______ of the atomic orbital.a) orientation b) size c) energy d) shape

198. The number of electrons present in p orbitals in the outermost electron shell of the Group VIIAelements is:a) two b) three c) one d) four e) five

199. Which one of the following ground state electron configurations isINCORRECT?a) 54Xe [Kr]4d

105s25p6 b) 50Sn [Kr]4d105s25p2 c) 29Cu [Ar]3d

104s1d) 25Mn [Ar]4s

24d5 e) 20Ca 1s22s22p63s23p6 4s2

200. Which of the responses contains all the true statements and no others regarding electromagneticradiation (light)?

I. As wavelength increases frequency decreases.II. As energy increases frequency decreases.III. As wavelength increases energy decreases.IV. The product of wavelength and frequency is constant.

a) I, III, and IV b) III and IV c) I, II, and IV d) II III, and IV e) I and II

201. The amount of energy absorbed in the process in which an electron is added to a neutral gaseousatom is defined as __________.a) electron affinity b) shielding effect c) electronegativityd) standard reduction potential e) first ionization energy

202. Arrange the following elements in order ofINCREASING atomic radii. K, Na, Mg, Cs, Cla) Cl / Mg / Na / Cs / K b) Na / Mg / Cl / K / Cs c) Cl / Mg / Na / K / Csd) Cl / Mg / Cs / K / Na e) Cs / K / Cl / Mg / Na


23/69

203. The orientation in space of an orbital is designated by which quantum number?a) n b) s c) ml d) e) l

204. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is astatement of _________.a) Planck's Theory b) Hund's Rule c) the Aufbau Principled) the Heisenberg Uncertainty Principle e) the Bohr Theory

205. Which comparison of electronegativities is NOT correct?a) O is greater than S b) N is greater than Be c) Br is greater than Sed) K is greater than Mg e) I is greater than Ba

206. The minimum energy required to remove the most loosely held electron is:a) electron affinity b) electronegativity c) potential energyd) first ionization energy e) kinetic energy

207. Which of the following statements is FALSE?

a) The third energy level has 5 d orbitals.b) A set of p orbitals in a given energy level are equal in energy.c) An f set of orbitals is filled with 10 electrons.d) The 5d and 4f orbitals are very close in energy.e) The 4s orbitals are lower in energy the 3d orbitals.

208. Which one of the following pairs contains isoelectronic species?a) F2, Cl2 b) Na, Na

+ c) S2, Se2 d) Na+, O2 e) S, Se

209. The total number of electrons that can be accommodated in the n=4 level is _________.a) 18 b) 50 c) 8 d) 2 e) 32

210. Which response includes all the following statements that are true, and no others?I. An s orbital can accommodate a maximum of two electrons.II. A set of d orbitals can accommodate a maximum of ten electrons.III. Each d orbital within a set consists of two lobes, 180 apart.IV. There are nine f orbitals in a set of f orbitals.

a) II and IV b) II, III, and IV c) I and IV d) I and II e) I, III, and IV

211. Which of the following atoms has the greatest number of unpaired electrons in its ground state?a) S b) N c) Ti d) Cu e) Cl

212. Which of the following has a negative charge?a) electron b) nucleus c) neutron d) alpha particle e) proton

213. Which two subatomic particles have approximately the same mass?a) electrons and nuclei b) neutrons and electrons c) protons and alpha particlesd) protons and electrons e) protons and neutrons

214. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is astatement of ______________.a) the Bohr Theory b) the Heisenberg Uncertainty Principle c) Planck's Theoryd) the Aufbau Principle e) Hund's Rule


24/69

215. What is the electron configuration of silicon, Si?a) 1s22s22p63s23p2 b) 1s22s22p63s23p4 c) 1s21p62s22p4 d) 1s21p62s22p2 e)1s22s22p62d4

216. The total number of electrons in p orbitals in a palladium atom (atomic number = 46) in itsground state is ____________.a) 12 b) 24 c) 18 d) 30 e) 6

217. What would be the outer electron configuration of group VIA (O, S, Se, . . .)?a) ns0np6 b) ns2np6 c) ns2np2 d) ns2np4 e) np6

218. Which element has the largest atomic radius?a) Sn b) Cl c) Se d) Kr e) F

219. Which element has the highest electronegativity in this list?a) At b) O c) Ge d) B e) Ca

220. Arrange the following elements in order ofincreasing electronegativities: At, Bi, Cl, F, Ia) F / Cl / Bi / I / At b) Bi / At / I / Cl / F c) At / Bi / I / Cl / Fd) At / Bi / Cl / F / I e) F / Cl / I / At / Bi

221. The atomic number of an element gives the number of _____________ and _____________ inthe atom while the mass number gives the total number of _____________ and _____________.a) neutrons, electrons; protons, electrons b) protons, electrons; neutrons, electronsc) neutrons, electrons; neutrons, protons d) protons, electrons; neutrons, protonse) neutrons, protons; neutrons, electrons

222. An element has the following outer electron configuration in its ground state, where n represents

the highest occupied energy level: (n - 1)d10

ns2

np4

. Which of the elements listed below could it be?a) Si b) Se c) S d) Ge e) none of these

223. Which of the following has a negative charge?a) nucleus b) neutron c) proton d) electron e) alphaparticle

224. Which two subatomic particles have approximately the same mass?a) protons and neutrons b) protons and electrons c) electrons and nucleid) neutrons and electrons e) protons and alpha particles

225. The number of electrons in a neutral atom of an element is always equal to the _______ of theelement.a) mass number b) atomic number c) atomic mass unitd) isotope number e) Avogadro's number

226. Which statement about electromagnetic radiation isFALSE?a) As frequency increases, wavelength decreases. b) As wavelength increases, energy increases.c) As wavelength increases, frequency decreases. d) Wavelength and energy are inverselyproportional.e)Wavelength and frequency are inversely proportional.


25/69

227. The difference between the mass number of an atom and the atomic number of the atom is alwaysequal to ....a) 6.02 x 1023. b) the number of protons in the nucleus. c) the atomic massunit.d) the atomic number of the element. e) the number of neutrons in the nucleus.

228. Isotopes are atoms of the same element that:a) have different numbers of electrons. b) have different numbers of protons.c) have different atomic numbers. d) have different numbers of neutrons.e) have different nuclear charges.

229. The atomic number of a certain element is 19, and its atomic weight is 39. An atom of theelement contains _____ protons, _____ neutrons, and the chemical symbol for the element is _____.a) 19, 19, F b) 19, 20, F c) 19, 20, K d) 20, 19, K e) none ofthese

230. Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope.

a) 38 p, 38 n, 38 e b) 38 p, 90 n, 38 e c) 52 p, 38 n, 52 ed) 38 p, 52 n, 38 e e) 90 p, 38 n, 90 e

231. Give the number of protons, neutrons, and electrons in the 2141Sc3+ ion.

a) 21 p, 20 n, 21 e b) 21 p, 20 n, 18 e c) 21 p, 20 n, 24 ed) 20 p, 21 n, 17 e e) 21 p, 41 n, 18 e

232. The Heisenberg Uncertainty Principle states that ________.a) no two electrons in the same atom can have the same set of four quantum numbers.b) two atoms of the same element must have the same number of protons.c) it is impossible to determine accurately both the position and momentum of an electron

simultaneously.d) electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly beforethey pair up in any orbital of the set.e) charged atoms (ions) must generate a magnetic field when they are in motion.

233. A(An) ______ is a region of space in which there is a high probability of finding an electron in anatom.a) shell b) atomic orbital c) core d) major energy level e) nucleus

234. Which quantum number is often designated by the letters s, p, d and f?a) n b) l c) ml d) ms e)

235. What is the total number of orbitals in the fourth energy level (n = 4.)a) 4 b) 24 c) 16 d) 9 e) 18

236. The maximum number of electrons that can occupy an energy level or shell (n = principlequantum number) is _____.a) n b) 2n c) n + 1 d) n 1 e) 2n2

237. Which of the following is not a valid magnetic quantum number for the 3d set of orbitals?a) 1 b) 2 c) 0 d) -2 e) -3


26/69

238. No two electrons in the same atom can have the same set of four quantum numbers is a statementof _____.a) the Aufbau Principle b) the Pauli Exclusion Principle c) Dalton's Theoryd) Hund's Rule e) the Heisenberg Uncertainty Principle

239. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is astatement of _____.a) the Heisenberg Uncertainty Principle b) the Bohr Theory c) the AufbauPrincipled) Planck's Theory e) Hund's Rule

240. The electron configuration 1s22s22p63s23p6 4s23d6 represents the element _____.a) Mn b) Se c) Fe d) Co e) Kr

241. Which of the following is the electron configuration of O2-?a) 1s22s22p6 b) 1s22s22p4 c) 1s22s22p33s23p6 d) 1s22s22p1 e)1s22s22p43s23p4

242. What is the electron configuration of tin, Sn?a) [Kr]5s23d103f145p4 b) [Kr]5s23d104d145p4 c) [Kr]5s23d104f145p2d) [Kr]5s24d105p2 e) [Xe]5s24d105p2

243. Which one of the following electron configurations is INCORRECT?a) Cl-; 1s22s22p63s23p6 b) Ge; [Ar]3d104s23p3 c) Sc; [Ar]3d14s2d) O; [He]2s22p4 e) N3-; 1s22s22p6

244. Which element has the following electron configuration?

a) Na b) Mg c) Cl d) Br e) P

245. What is the electron configuration of the iron(III) ion?a) [Ar]4s23d3 b) [Ar]3d5 c) [Ar]4s23d3 d) [Ar]3d5 e) [Kr]3d5

246. Which of the following sets of quantum numbers COULD represent the "last" electron added tocomplete the electron configuration for a ground state atom of Br according to the Aufbau Principle. n;l; ml; msa) 4; 0; 0; -1/2 b) 4; 1; 1; -1/2 c) 3; 1; 1; -1/2 d) 4; 1; 2; +1/2 e) 4; 2; 1; -1/2

247. Which statement is FALSE?a) If an electron has quantum number n = 3, the electron could be in a d sublevel.b) If an electron has quantum number l = 2, the only possible values of ml are 0 and 1.c) If an electron has ml = 1, it might be in a p, d, or f sublevel but not in an s sublevel.d) An electron that has n = 3 cannot be in an f sublevel.e) An electron that has n = 5 could be in an s, p, d, or f sublevel.


27/69

248. The TOTAL number of electrons in p orbitals in a palladium atom (atomic number = 46) in itsground state is _____.a) 6 b) 12 c) 18 d) 24 e) 30

249. An element that has four electrons in its outer shell in its ground state is _____.a) Nb b) Cr c) Sn d) Ti e) O

250. The number of electrons present in the p orbitals in the outermost electron shell (major energylevel, n) of the halogen atoms is _______.a) one b) two c) six d) seven e) five

251. In predicting the electron configuration of the elements by the Aufbau Principle, to whichsublevel is one adding electrons in traversing from element 39, Y, to element 48, Cd?a) 4f b) 5p c) 4d d) 5d

252. The number of valence electrons in the Group including nitrogen, phosphorus, and arsenic is:a) 5 b) 4 c) 3 d) 7 e) 6

253. Of the 3 elements fluorine, bromine, and calcium, which has the highest and which the lowestionization energy?a) Bromine has the highest and calcium has the lowest.b) Calcium has the highest and fluorine has the lowest.c) Fluorine has the highest and bromine has the lowest.d) Fluorine has the highest and calcium has the lowest.

254. Rank the following five atomic species in order of increasing atomic radius (smallest to largest):Si, Na, K, F, Oa) K, Na, Si, O, F b) F, O, Si, Na, K c) O, F, Si, Na, K d) O, F, Na, Si, K

255. The hydride ion has ____ electrons.a) 2 b) 1 c) 0 d) 3 e)

256. Which ionic species would you predict to be the largest? Na+, Mg2+, N3-, O2-a) Mg2+ b) O2 c) Na+ d) N3

257. The Mg2+ ion is isoelectronic with which neutral atom?a) Si b) Na c) Ne d) Ar e) He

258. Between which two species out of the following three elements is there the largest

electronegativity difference? O, Se, Mga) Between Mg and Se, with Se being the highest EN.b) Between O and Se, with O being the highest EN.c) Between Mg and O, with Mg being the highest EN.d) Between O and Mg, with O being the highest EN.

259. Identify the INCORRECT statement below:a) Nonmetals generally have the higher electronegativities and tend to attract electrons to themselvesin a chemical bond.b) Elements with high ionization energies tend to have large atomic radii.c) Elements with high electronegativities generally have large negative electron affinities.d) The second ionization energy is always larger than the first ionization energy.


28/69

260. Which of the following processes is responsible for the yellowish-brown gas commonly found inthe air over large metropolitan areas?a) The electric spark in electric motors. b) The combustion of coal with high sulfurcontent.c) The combustion of materials containing nitrogen. d) The combustion of natural gas.

261. What is the total number of available valence electrons in the Lewis dot structure of theammonium ion, NH4+?a) 8 b) 9 c) 10 d) 7

262. The Lewis dot formula for Br2 shows:a) a single ionic bond b) a double covalent bondc) a triple covalent bond d) a single covalent bond

263. Which is the correct Lewis dot structure of magnesium chloride?

264. Based on the Lewis electron dot structure of the diatomic molecule O2, what kind of bond existsbetween the oxygen atoms?a) a triple covalent bond b) a double covalent bondc) a single covalent bond d) a single ionic bond

265. Which is the correct Lewis structure of the SO32- ion?

a) b) c) d) e)

266. In which species is there a violation of the octet rule?a) N2 b) SF6 c) O2 d) CCl4

267. Which of the following statements about chemical periodicity isINCORRECT?a) The chemical properties of elements are periodic functions of their atomic number.b) Electronegativity decreases as you go from left to right across a period.c) Atomic radii decrease as you go across a period.d) Electron affinity becomes more negative as you go up a family or group of elements.

268. Which of the following elements has an ns2np2 outer level electron configuration?a) Ne b) N c) O d) Cl e) C

269. Which outer shell electron configuration is typical of an alkaline earth metal?a) ns1 b) ns2np4 c) ns2 d) ns2np6 e) ns2np5

270. Which sublevel is being filled in proceeding from element Y to element Cd?a) 4d b) 3d c) 5d d) 4f e) 5s

271. Which species is INCORRECTLY matched with the electron configuration?

a) Na+

= 1s2

2s2

2p6

b) S2-

= 1s2

2s2

2p6

3s2

3p2

c) Ca2+ = 1s22s22p63s23p6 d) Sc3+ = 1s22s22p63s23p6

272. Which of the following species is NOT isoelectronic with the others?


29/69

a) N3 b) O2 c) F d) K+ e) Al3+

273. Which atom below is the largest?a) S b) Ca c) Al d) K e) F

274. Which atom below has the largest first ionization energy?a) N b) O c) S d) Li e) Cs

275. Which elements below has the largest electronegativity?a) Li b) S c) O d) Na e) Cs

276. Which element pair will form the most ionic bond?a) C, H b) C, O c) Li, H d) Na, Cl

277. Which statement is INCORRECT?a) Electron affinity is the amount of energy needed to attach an electron to a gaseous element.b) Once an electron has been removed from a neutral atom, the second electron is usually easier to

remove.c) First ionization is the minimum amount of energy required to remove the most loosely held electronfrom a gaseous atom.d) Metals have lower ionization energies than nonmetals.e) Elements with low ionization energies typically form ionic compounds with nonmetals by losingelectrons.

278. How many valence electrons does carbon have?a) 3 b) 6 c) 1 d) 4 e) 2

279. In which of the following species would one expect to find RESONANCE?

I. CO2 II. HNO2 III. SO2 IV. CO32-

a) All of them b) II, III and IV c) III and IV d) I only

280. In which of the following species would one expect to find the presence of double bonds?I. CH3F II. CO2 III. CS2

a) All of them b) II only c) I only d) II and III

281. Which of the following species contain at least one POLAR covalent bond?I. HBr II. CO III. CCl4 IV. Cl2

a) All of them b) I, II and III c) I and II d) I, II and IV e) IV only

282. Which response below lists the elements in order of decreasing atomic radius?a) Cl > F > Pb > Si > P b) Pb > Si > P > F > Cl c) Pb > Si > P > Cl > Fd) Pb > Cl > P > Si > F e) Pb > Cl > Si > P > F

283. Which element below has the highest first ionization energy?a) O b) N c) Be d) C e) B

284. Which of the following elements has the most negative electron affinity?a) S b) Se c) Si d) Te e) P

285. Which element below has the highest electronegativity?a) Li b) N c) K d) As e) Ba

286. Which pair of elements would be least likely to combine to form an ionic compound?


30/69

a) Cs, O b) Mg, Br c) Al, F d) C, N e) Na, S

287. The two acids that are major contributors to "acid rain" are:a) H2CO3 and HNO3 b) H2SO4 and H3PO4 c) H2CO3 and H2SO4d) H2SO4 and HNO3 e) H3PO4 and HNO3

288. Which is the following is an INCORRECT electron configuration for the ground state of thesespecies?a) Sc = [Ar]4s23d1 b) Se = [Ar]4s24p4 c) Li = 1s22s1 d) N = [He]2s22p3

289. Identify the INCORRECT statement below:a) The total number of electrons required to fill the n=2 level is 8.b) The total number of electrons that can have n=3 in a many-electron atom is 18.c) The total number of electrons that can occupy an atomic orbital is 1.d) The total number of electrons that can "fit" in the 4f sublevel is 14.

290. The observation that electrons "prefer" going into separate atomic orbitals in a sublevel having

more than one orbital is a consequence of:a) The Aufbau Principle. b) The Heisenberg Uncertainty Principle.c) Hund's Rule. d) The Pauli Exclusion Principle.

291. Which of the following full notations for the electron state is consistent with thelast electronadded in forming the electron configuration of Gallium (Ga)?a) (3, 2, 1, +1/2) b) (4, 0, 0, +1/2) c) (4, 2, 0, +1/2)d) (4, 2, 1, +1/2) e) (4, 1, 0, +1/2)

292. Fill in the blank: The n quantum number tells which level the electron is in and most directlyspecifies the _______ of the atomic orbital.

a) orientation b) angular momentum c) energy d) shape e) mass

293. Which of the following species does NOT have an ns2np6 outer level electron configuration?a) F b) N3 c) O2 d) Cl e) Ne

294. Which outer shell electron configuration is typical of a neutral halogen element?a) ns1 b) ns2np4 c) ns2 d) ns2np5 e) ns2np7

295. Which subshell is being filled in proceeding from element Sc to element Zn?a) 4d b) 3d c) 5d d) 4f e) 5s

296. Which species is INCORRECTLY matched with the electron configuration for the ground stateof these species?a) K+ = [Ar] b) Na+ = 1s22s22p6 c) H- = 1s2 d) O2- = [He]2s22p2

297. Which of the following species is NOT isoelectronic with the others?a) N3- b) O2- c) Mg d) Na+ e) Al3+

298. Which atom below is the largest?a) O b) K c) Al d) Mg e) F

299. Which atom below has the largest first ionization energy?a) N b) F c) Mg d) Li e) Na

300. Which elements below has the lowest electronegativity?


31/69

a) Li b) S c) O d) Na e) Cs

301. Which statement is INCORRECT?a) Elements with low ionization energies typically form ionic compounds with nonmetals by gainingelectrons.b) Electron affinity is the amount of energy needed to attach an electron to a gaseous element.c) Once an electron has been removed from a neutral atom, the second electron is harder to remove.d) First ionization is the minimum amount of energy required to remove the most loosely held electronfrom a gaseous neutral atom.e) Metals have lower ionization energies than nonmetals.

302. In constructing the Lewis electron dot formula of H2O, the oxygen atom becomes isoelectronicwith:a) H b) He c) Ne d) F e) N

303. The number of valence electrons in the group including carbon and silicon is:a) 5 b) 4 c) 3 d) 7

304. The hydrogen ion has ____ electrons.a) 2 b) 1 c) 0 d) 3

305. The Mg2+ ion is isoelectronic with which neutral atom?a) Ne b) Na c) Si d) Ar

306. What is the total number of available valence electrons in the Lewis dot structure of the CO32-

ion?a) 24 b) 22 c) 20 d) 2 e) 26

307. The Lewis dot formula for N2 shows:a) a single ionic bond b) a double covalent bondc) a triple covalent bond d) a single covalent bond

308. Which of the following atoms has the largest radius?a) Cs b) Rb c) K d) Na

309. Which of the following atoms has the smallest radius?a) Br b) As c) Ca d) K

310. Which of the following atoms has the largest radius?

a) Rb b) Si c) S d) O

311. Which of the following atoms has the smallest radius?a) Na b) Al c) N d) F

312. Which atom has the lowest first ionization energy?a) Na b) Ba c) Ca d) Cs

313. Which atom has the highest first ionization energy?a) Cs b) Ca c) Al d) O

314. Which atom has the highest electron affinity?a) Rb b) Mg c) Ga d) F


32/69

315. Which atom has the lowest electron affinity?a) Be b) Sr c) Ca d) Mg

316. Which element has below the highest electronegativity?a) Ge b) O c) B d) Ca e) H

317. Which atom has the greatest attraction for electrons in a covalent bond?a) Ge b) Se c) As d) Br e) Kr

318. Which of the following ions would least likely form?a) Cu+2 b) Ca+2 c) Ti+2 d) K+2

319. The relationship known as Charles Law is valid:a) at constant temperature and amount of gas. b) at constant pressure and amount of gas.c) at constant volume and amount of gas. d) at constant temperature and volume.

320. A sample of a gas having a volume of 1 L at 25C and 1 atm pressure is subjected to an increase

in pressure and a decrease in temperature. The volume of the gas:a) decreases b) increases c) remains the samed) either increases or decreases, depending on the sizes of the pressure and temperature changes

321. A sample of a gas having a volume of 1 L at 25C and 1 atm pressure is subjected to an increasein pressure and an increase in temperature. The volume of the gas:a) decreases b) increases c) remains the samed) either increases or decreases, depending on the sizes of the pressure and temperature changes

322. Consider the following statements concerning ideal gases:I. Boyle's Law establishes the inverse proportionality between volume and pressure of a fixed

amount of ideal gas at fixed temperature.II. Charles' Law establishes the direct proportionality between temperature and pressure of afixed amount of ideal gas at fixed volume.

III. Dalton's Law establishes the additivity of partial pressures of a mixture of ideal gases.IV. Avogadro's hypothesis establishes the direct proportionality between volume and moles of

ideal gas present, holding pressure and temperature fixed.a) all are true except I b) all are true except IIc) all are true except III d) all are true statements

323. A sample of a gas having a volume of 1 L at 25C and 1 atm pressure is subjected to a decreasein volume and an increase in temperature. The pressure of the gas:

a) remains the same b) decreases c) increasesd) either increases or decreases, depending on the sizes of the pressure and temperature changes

324. Which gas has the highest density if all are in the same state?a) N2 b) O2 c) Ar d) He e) all have the same density

325. Which of the following gases is not in the top three most abundant substances by mass in dry air?a) Ar b) He c) O2 d) N2


33/69

326. Consider the following statements concerning ideal gases:I. Charles' Law establishes that if you double the Celsius temperature of a gas you double its

volume, assuming amount of gas and pressure are fixed.II. Boyle's Law establishes that if you compress a gas to half its volume, you double its

pressure, assuming amount of gas and temperature are fixed.III. Dalton's Law was used in the calculations of the moles of oxygen in the collection flask in

lab.IV. Avogadro's hypothesis predicts that in standard state a one gram sample of helium and a

one gram sample of nitrogen gas will occupy the same volume.a) I and III are true, the others false b) II and IV are true, the others falsec) only II is true d) II and III are true, the others falsee) all are true statements

327. A fixed quantity of a gas is subjected to a decrease in pressure and a increase in temperature. Thevolume of the gas:a) remains the same b) decreases c) increasesd) either increases or decreases, depending on the sizes of the pressure and temperature changes

328. Which gas has the highest mass density, given all are in the same state?a) N2 b) O2 c) CO2 d) air e) all have the same density

329. The number of regions of high electron density on the central atom in O3, according to VSEPRtheory is:a) two b) three c) four d) five

330. The electronic geometry of SF4 is:a) tetrahedral b) see-saw c) octahedral d) trigonal bipyramidal

331. The molecular geometry of SbCl5 is:a) square planar b) tetrahedral c) trigonal bipyramidal d) octahedral

332. The number of unshared regions of high electron density on the central atom in the H2O moleculeis:a) zero b) one c) two d) three e) four

333. Consider the following statements below concerning a given sample of ideal gas at STP:I. The average speed of the molecules is directly proportional to the square root of the

temperature of the sample and independent of their mass.II. Molecules are in constant chaotic motion moving in straight lines between collisions.

III. The physical dimensions of the molecules occupy a very small fraction of the total systemvolume.

IV. All molecules are traveling at the same speed.a) all are true b) only I and III are true c) only II and III are trued) only I, II, and III are true e) none are true

334. Which of the following gases will have the fastest effusion rate?a) CH4 b) CO2 c) N2 d) O2 e) Ar

335. In the separation of gaseous helium from hydrogen (H2) by an effusion process, the hydrogen willeffuse from the container at about ______ the rate of helium effusion.a) same rate b) twice c) half d) 7/10ths e) 1.4 times


34/69

336. Identify the INCORRECT statement concerning the kinetic theory of gases:a) Gases consist of particles in continuous random straight-line motion with fixed velocities.b) Collisions between gas molecules and the walls are elastic.c) Between collisions molecules exert no attractive or repulsive forces on one another.d) Gases consist of particles which are very far apart compared to their own sizes.e) The pressure exerted by the gas is due to molecules striking the container walls.

337. Identify the INCORRECT statement below:a) The average kinetic energy of gas molecules is directly proportional to the temperature of thesample.b) The average kinetic energy of molecules of different gases are equal at a given temperature.c) The average speed of gas molecules is directly proportional to the square root of the temperature.d) The average speed of molecules of different gases are equal at a given temperature.

338. At STP which of the following gases would have the lowest average molecular speed?a) NH3 b) CO2 c) Ar d) H2

339. The intermolecular forces that are most significant in accounting for the high boiling point ofliquid water relative to other substances of similar molecular weight are the:a) ion-ion attractions b) London dispersion forcesc) hydrogen bonding forces d) dipole-dipole attractions

340. Identify the INCORRECT statement below:a) When the vapor pressure of a liquid equals the surrounding pressure, the liquid boils.b) The boiling point is the temperature at which the vapor pressure of the liquid equals the surroundingpressure.c) The normal boiling point is the temperature at which the vapor pressure of the liquid equals 1 atm.d) The vapor pressure of a liquid increases as the temperature of the liquid increases.

e) Easily vaporized liquids are called volatile liquids, having low vapor pressures.

341. Identify the INCORRECT statement below concerning a given sample of pure argon gas at STP:a) Molecules are in constant chaotic motion moving in straight lines between collisions.b) The physical dimensions of the molecules occupy a very small fraction of the total system volumeavailable.c) All molecules are traveling at the same speed.d) The average kinetic energy of the molecules is directly proportional to the temperature of thesample and independent of their mass.

342. In the separation of gaseous argon from neon by an effusion process, the neon will effuse from

the container at about _____ times the rate of argon effusion.a) 1 b) 2 c) 0.5 d) 0.7 e) 1.4

343. Which of the following gases will have the slowest effusion rate?a) CH4 b) CO2 c) N2 d) O2 e) Ar

344. The interaction responsible for the cohesive intermolecular forces of liquid nitrogen is:a) hydrogen bonding b) the London dispersion forcec) dipole-dipole interaction d) covalent bonding


35/69

345. Identify the INCORRECT statement below:a) The vapor pressure of liquid water at 100C is 760 Torr (1 atm).b) The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquidequals 1 atm.c) The boiling point of a liquid increases as the surrounding pressure decreases.d) Vapor pressure of a liquid increases as the temperature increases.e) A liquid boils when its vapor pressure equals the surrounding pressure.

346. The smallest repeat unit of a crystalline solid is called:a) a point group b) a lattice point c) a unit cell d) a crystalline element

347. The type of solid which is characterized as positive ions embedded in a sea of delocalizedelectrons is called:a) a metallic solid b) a ionic solid c) a molecular solid d) a covalent (network)solid

348. Diamond (pure carbon) would be classified as which type of solid:

a) a metallic solid b) a ionic solid c) a molecular solid d) a covalent (network)solid

349. Which of the following is NOT true?a) Temperature is an example of an intensive property.b) The mass percentage of calcium in calcium phosphate is an extensive property.c) Separations of a solid from a liquid by filtration is an example of a physical process.d) Density is an intensive property.

350. Which of the following is NOT paired with the proper classification?a) iron/element b) chromium (III) oxide/compound

c) pizza/heterogeneous mixture d) a solution of aqueous sulfuric acid/heterogeneous mixture

351. The atomic mass unit (amu) is defined as:a) the mass of a proton. b) 1/16 the mass of the most common atom of oxygen

test questions 2009

Documents