Review Sheet 1St Semester Honors Chemistry
REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY
UNIT 1 INTRODUCTORY
- An example of a chemical change is
(A)freezing of water.
(B)burning a match.
(C)boiling carbon tetrachloride.
(D)dissolving alcohol in water.
(E)stretching a rubber band.
- Which involves a chemical change?
(A)powdering sugar
(B)condensing steam
(C)magnetizing an iron bar
(D)separating cream from milk
(E)exposing photographic film to light
- Which process is a chemical change?
(A)the melting of ice
(B)the burning of a candle
(C)the magnetizing of steel
(D)the liquefaction of oxygen
- The graph was obtained by plotting the volume of a material vs. the mass of that same material.
What is the density of the material?
(A)1.5 g·cm
(B)2.0 g·cm
(C)0.67 g·cm
(D)0.50 g·cm
- Which is a unit for expressing volume?
(A)mm
(B)g
(C)cm3
(D)g·cm
- The number 149,000,000 is usually written in scientific notation as
(A)0.149 109
(B)149 x 106
(C)1.49 x 108
(D)1490 x 105
- Which measurement is the most uncertain?
(A)1.00 ± 0.01 cm
(B)2.00 ± 0.05 L
(C)10 ± 1 g
(D)200 ± 1 mL
- Which unit represents l 10–3 mol?
(A)decimole
(B)kilomole
(C)millimole
(D)micromole
- The volume of one milliliter most nearly equals
(A)454 g
(B)1000 L
(C)1 mg
(D)1 in3
(E)1 cm3
- 10.0 mL of a pure liquid substance has a mass of 25.0 g. What is the mass of 3.00 L of the substance?
(A)83 g
(B)120 g
(C)1,200 g
(D)7,500 g
(E)25,000 g
- The metric prefix for 10–6 is
(A)mega–
(B)kilo–
(C)micro–
(D)milli–
UNIT 2 MOLES
- Which expression represents the number of atoms in 1.0 10–3 g of lead?
(A)
(B)
(C)
(D)
(E)
- How many atoms are in one mole of hydrogen sulfide, H2S?
(A)34 6.02 1023
(B)3 6.02 1023
(C)3
(D)34
- A substance whose density is 4.00 g·cm–3 occupies a volume of 12.0 cm3. What is its mass?
(A)0.333 g
(B)8.00 g
(C)48.0 g
(D)4.00 g
- How many moles of oxygen atoms are present in one mole of beryllium sulfate tetrahydrate, BeSO4·4H2O?
(A)eight
(B)five
(C)four
(D)two
- Which statement best accounts for the fact that gases can be greatly compressed?
(B)The collisions of molecules are elastic.
(C)Molecules of gases are in constant motion.
(D)The molecules of a given gas are identical.
(E)Molecules of gases are relatively far from each other.
- Gases may be most easily liquefied by
(A)raising the temperature and lowering the pressure.
(B)raising the pressure and lowering the temperature.
(C)lowering both the temperature and pressure.
(D)raising both the temperature and pressure.
(E)lowering the temperature and keeping the presure unchanged.
- If the temperature and pressure are the same, one gram of hydrogen has about the same number of atoms as
Atomic Molar Masses
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)1 g of oxygen. .
(B)2 g of oxygen. .
(C)8 g of oxygen.
(D)16 g of oxygen
(E)32 g of oxygen
- One liter of oxygen at STP contains approximately the same number of molecules as
(A)2 L of He at STP.
(B)1/3 L of O3 at STP.
(C)l L of CO2 at STP
(D)1/5 L of CH4 at STP.
(E)(D) (E)250 mL of NH3 at STP.
- According to the Avogadro Principle, one liter of gaseous hydrogen and one liter of gaseous ammonia contain the same number of
(A) atoms at standard conditions.
(B) molecules at all conditions.
(C) molecules only at standard conditions.
(D) atoms if conditions in both containers are the
same.
(E) molecules if conditions in both containers are the
same.
- Which is STP?
(A)0 °C and 76 mmHg
(B)0 K and 76 mmHg
(C)0 K and 760 mmHg
(D)100 °C and 76 cmHg
(E)273 K and 760 mmHg
- A student collects one liter samples of O2, CO2, and CH4 at laboratory conditions. What quantity is the same for all three samples?
(A)number of atoms divided by the number of molecules in each sample
(B)number of molecules in each sample
(C)number of atoms in each sample
(D)mass of each sample
- Each of three identical containers holds a mole of gas, all at the same temperature.
Which gas exerts the greatest pressure? Assume ideal behavior.
(A)CH4
(B)O2
(C)SO2
(D)They all exert the the same pressure.
- A weather balloon contains 12 L of hydrogen at 740 mmHg pressure. At what pressure in mmHg will the volume become 20 L (temperature constant)?
(A)370
(B)444
(C)760
(D)1230
(E)1480
- A gas occupies a volume of 2.0 cubic feet at 13 atm. How many cubic feet does this gas occupy at 1.0 atm, temperature constant?
(A)6.5
(B)13
(C)15
(D)26
- A sample of gas at 1.00 atm of pressure occupies a volume of 500 L. If the volume is decreased to 125 L and the temperature is held constant, what is the new pressure in atmospheres?
(A)0.250
(B)2.00
(C)1.25
(D)4.00
- For a given amount of dry gas at constant temperature, when the pressure is doubled the volume is
(A)halved.
(B)unchanged.
(C)doubled.
(D)increased, but not doubled.
- Approximately how many molecules are in 11 g of carbon dioxide, CO2, gas?
Atomic Molar Masses
C 12.0 g·mol–1
O 16.0 g·mol–1
(A)1.5 1023
(B)3.0 1023
(C)6.0 1023
(D)2.4 1023
- What is the mass of one mole of calcium nitrate, Ca(NO3)2?
Atomic Molar Masses
Ca 40. g·mol–1
N 14. g·mol–1
O 16. g·mol–1
(A)82 g
(B)102 g
(C)164 g
(D)204 g
- The number of moles of water in 1,000 g of water is
Atomic Molar Masses
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)18.0
(B)55.5
(C)180.0
(D)1000.0
(E)18,000.0
- The molar mass of magnesium acetate, Mg(C2H3O2)2, in g·mol–1 is
Atomic Molar Masses
C 12. g·mol–1
H 1. g·mol–1
Mg 24. g·mol–1
O 16. g·mol–1
(A)15
(B)16
(C)83
(D)142
(E)166
- How many mole(s) of calcium carbonate, CaCO3, is represented by 50 g of the compound?
Atomic Molar Masses
Ca 40.1 g·mol–1
C 12.0 g·mol–1
O 16.0 g·mol–1
(A)1.0
(B)2.0
(C)0.20
(D)4.0
(E)0.50
- The molar mass of aluminum sulfate, Al2(SO4)3, is
Atomic Molar Masses
Al 27 g·mol–1
O 16 g·mol–1
S 32 g·mol–1
(A)150 g·mol–1
(B)170 g·mol–1
(C)278 g·mol–1
(D)342 g·mol–1
(E)450 g·mol–1
- The mass of one mole of ammonium carbonate, (NH4)2CO3, is approximately
Atomic Molar Masses
C 12.0 g·mol–1
H 1.0 g·mol–1
N 14.0 g·mol–1
O 16.0 g·mol–1
(A)43.0 g
(B)72.0 g
(C)78.0 g
(D)96.0 g
- The number of molecules present in 22.0 g of carbon dioxide at STP is
Atomic Molar Masses
C 12.0 g·mol–1
O 16.0 g·mol–1
(A)2.01 1012
(B)6.03 1012
(C)2.06 1022
(D)3.01 1023
(E)6.02 1023
- What mass of nitrogen dioxide, NO2, has the same number of molecules as 18.0 g of water, H2O?
Atomic Molar Masses
H 1.0 g·mol–1
N 14.0 g·mol–1
O 16.0 g·mol–1
(A)6.02 g
(B)18.0 g
(C)23.0 g
(D)46.0 g
- Calculate the mass of 12.0 1023 molecules of chlorine gas, Cl2.
Atomic Molar Mass
Cl 35.5 g·mol–1
(A)35.5 g
(B)71.0 g
(C)142 g
(D)284 g
UNIT 3 NOMENCLATURE
- The correct formula for iron(III) sulfate is
(A)FeSO4(D)Fe2(SO4)3
(B)Fe(SO4)2 (E)Fe3(SO4)2
(C)Fe2SO4
- The one correct formula among these is
(A)Na2OH(D)Zn(NO3)3
(B)Cu(SO4)2 (E) BaNO3
(C)ZnCl2
- Which formula is incorrect?
(A)BaHCO3(B)Ca(OH)2(C)Al2O3(D)K2SO4
(E)ZnCO3
- Which formula is incorrect?
(A)Al2(SO4)3(D)NH4HSO4
(B)BaHCO3(E)LiH
(C)Ca(OH)2
- What is the formula for aluminum sulfate?
(A)AlSO4
(B)Al2SO4
(C)Al3SO4
(D)Al3(SO4)2
(E)Al2(SO4)3
- What is the formula for chromium(III) oxide?
(A)CrO(B)Cr2O(C)Cr3O(D)Cr2O3
- What is the formula for strontium sulfide?
(A)SrS(B)Sr2S(C)SrS2(D)SrS3
- What is the formula for copper(II) hydroxide?
(A)CuOH(B)Cu(OH)2(C)Cu2OH(D)CuOH2
- Which is the formula for ammonium nitrate?
(A)NH3N(B)NH4N(C)NH4NO2
(D)NH4NO3
- What is the formula for sodium carbonate?
(A)NaHCO3 (C)So2CO3
(B)NaCO3(D)Na2CO3
- What is the formula for chromium(III) sulfate?
(A)Cr2(SO4)3(C)Cr2(SO3)3
(B)Cr3(SO4)2(D)Cr3SO4
- Which formula is followed by its correct name?
(A)FeCl3, iron(III) chloride
(B)FeS, iron(II) sulfite
(C)Mg3N2, magnesium nitrite
(D)KNO2, potassium nitrate
(E)HClO, hydrochloric oxide
- The compound not properly named is
(A)Fe2O3, iron(III) oxide.
(B)Pb3O4, lead(III) tetraoxide.
(C)CuCl2, copper(II) chloride.
(D)Pb3(PO4)2, lead(III) phosphate.
(E)P2S5, diphosphorus pentasulfide.
- What is the name of the compound having the formula CaH2?
(A)calcium amide(C)calcium hydrate
(B)calcium hydride(D)calcium hydroxide
- What is the name of the compound Fe2(SO4)3?
(A)iron(II) sulfate (C)iron(II) trisulfate
(B)iron(III) sulfate(D)iron(II) sulfate(III)
- What is the correct name for Fe(NO3)2?
(A)iron(II) nitrate (C)iron(III) nitrate
(B)iron(II) nitrite (D)iron(III) nitrite
- The formula for hydrogen bromate is HBrO3, and the formula for dysprosium oxide is Dy2O3. What is the formula for dysprosium bromate?
(A)Dy2BrO3 (C)Dy(BrO3)3
(B)Dy3BrO3 (D)Dy2(BrO3)3
- The formula for ytterbium sulfate is Yb2(SO4)3. What is the formula for ytterbium chloride?
(A)YbCl2(B)Yb2Cl3(C)Yb2Cl2(D)YbCl3
- In which pair of anions do both names end in ‘–ate’?
(A)Cl–, ClO3–(C)NO2–, NO3–
(B)ClO3–, NO3–(D)HS–, HSO4–
- Barium perrhenate has this formula: Ba(ReO4)2. The perrhenate ion is
(A)ReO4–(B)ReO42–(C)ReO43–(D)ReO44–
- What is the total number of oxygen atoms represented by the formula KAl(SO4)2·12H2O?
(A)9
(B)16
(C)20
(D)48
(E)96
- Which is the number of atoms of hydrogen in one molecule of glycerine, C3H5(OH)3?
(A)14(B)8(C)6(D)5
- The total number of atoms represented by the formula K3Fe(CN)6 is
(A)4
(B)10
(C)11
(D)16
(E)36
- The total number of atoms represented by 5Al(C2H3O2)3 is
(A)22
(B)60
(C)71
(D)84
(E)110
- The number of atoms of oxygen indicated by the formula Ca3(PO4)2 is
(A)12
(B)8
(C)7
(D)4
(E)3
- How many atoms are in one molecule of acetone, CH3COCH3 ?
(A)1(B)6(C)3(D)10
- Using only these formulas,
XY2X2ZQZ
what formula would you expect for a compound of elements Q and Y?
(A)QY(B)QY2(C)Q2Y(D)QY4
- Which set consists only of compounds?
(A)Na, Ca, He(C)NaCl, CH4, Br2
(B)H3O+, Cl–, I3–(D)H2S, CuCl2, KI
- Which substance contains only one kind of atom?
(A)water(C)aluminum
(B)ethanol(D)carbon dioxide
UNIT4 BALANCE EQUATIONS (REG, IONIC, NET-IONIC STOICHIOMETRY AND LIMITNG REACTANTS
- Which property is always conserved during a chemical reaction?
(A)mass(B)volume(C)pressure(D)solubility
- The equation
Cu + 4HNO3 Cu(NO3)2 + 2H2O + ?
would be completed and balanced by using
(A)NO2(B)2NO2(C)3NO2(D)4NO2
(E)2NO
- When the equation
? Sb + ? Cl2? SbCl3
is correctly balanced, the sum of the coefficients is
(A)2(B)3(C)6(D)7
(E)9
- Which expression is correctly balanced?
(A)Na2O2 + 2H2O 2NaOH + O2
(B)2Na2O2 + 2H2O 4NaOH + 2O2
(C)4Na2O2 + 3H2O 4NaOH + 2O2
(D)2Na2O2 + 2H2O 4NaOH + O2
(E)3Na2O2 + 2H2O 6NaOH + O2
- Which set of coefficients balances this equation?
? CH4(g)? C3H8(g) + ? H2(g)
(A)3, 1, 1(B)3, 2, 1(C)3, 1, 2(D)6, 2, 2
(E)6, 2, 6
- Consider the unbalanced expression:
? CH3CH2CHO(l) + ? O2(g) ? CO2(g) + ? H2O(g)
Which set of coefficients balances the equation?
(A)2, 8, 3, 6 (D)1, 8, 3, 3
(B)3, 8, 6, 6 (E)1, 4, 3, 3
(C)1, 4, 3, 2
- Consider the unbalanced expression:
? Cu(s) + ? NO3–(aq) + ? H+(aq)
? Cu2+(aq) + ? NO(g) + ? H2O(l)
Which set of coefficients correctly balances the equation?
(A)4, 5, 3, 8, 2, 3 (D)3, l, 8, 7, 4, 2
(B)2, 4, 3, 8, 3, 3 (E)3, 2, 8, 3, 2, 4
(C)3, 2, 8, 7, 2, 4
- The expression for pentane, C5H12, burning in oxygen is
? C5H12(g) + ? O2(g) ? CO2(g) + ? H2O(g)
What set of coefficients balances the equation?
(A)1, 8, 5, 6 (C)1, 8, 5, 12
(B)2, 8, 10, 6(D)1, 11, 5, 12
- Which set of coefficients correctly balances the equation?
? Al(s) + ? H+(aq) ? Al3+(aq) + ? H2(g)
(A)1, 2, 1, 2 (C)3, 2, 3, 2
(B)2, 6, 2, 3 (D)2, 3, 2, 3
- Which equation represents the complete combustion of acetylene in an excess of air?
(A)C2H2 + 2O2 2CO2 + H2
(B)C2H2 + O2 2CO + H2
(C)C2H2 + O 2C + H2O
(D)C2H2 + O2 2C + H2O2
(E)2C2H2 + 5O2 4CO2 + 2H2O
- Dysprosium oxide, Dy2O3, reacts with hydrochloric acid to produce only water and a salt. The salt is
(A)Dy2Cl3(B)DyCl2(C)DyCl3(D)DyCl6
- Which equation represents the dissolving of sodium sulfate, Na2SO4, in water?
(A)Na2SO4(s) Na2+(aq) + SO42–(aq)
(B)Na2SO4(s) 2Na+(aq) + SO42–(aq)
(C)Na2SO4(s) Na22+(aq) + S2–(aq) + 4O2–(aq)
(D)Na2SO4(s) 2Na2+(aq) + S2–(aq) + O2–(aq)
- What is the net ionic equation for the reaction between solutions of sodium chloride, NaCl, and silver nitrate, AgNO3?
(A)Na+(aq) + NO3–(aq) Na(s) + 1/2N2(g) + 3/2O2(g)
(B)Ag+(aq) + Cl–(aq) Ag(s) + 1/2Cl2(g)
(C)Ag+(aq) + Cl–(aq) Ag+(aq) + Cl–(aq)
(D)Ag+(aq) + Cl–(aq) AgCl(s)
- Which equation represents the dissolving (dissociation) of aluminum sulfate, Al2(SO4)3, in water?
(A)Al2(SO4)3(s) 2Al3+(aq) + 3S6+(aq) + 4O2–(aq)
(B)Al2(SO4)3(s) 2Al3+(aq) + 3SO42–(aq)
(C)Al2(SO4)3(s) 2Al2+(aq) + 3SO43–(aq)
(D)Al2(SO4)3(s) Al3+(aq) + SO43–(aq)
- The overall equation for the reaction between KCl and AgNO3 is
K+(aq) + Cl–(aq) + Ag+(aq) + NO3–(aq)
K+(aq) + NO3–(aq) + AgCl(s)
What is the net ionic equation?
(A)Ag+(aq) + Cl–(aq) AgCl(s)
(B)K+(aq) + Cl–(aq) KCl(s)
(C)K+(aq) + NO3–(aq) KNO3(s)
(D)K+(aq) + Cl–(aq) + Ag+(aq) + NO3–(aq)
Ag+(aq) + K+(aq) + Cl–(aq) + NO3–(aq)
- Complete the equation for the reaction between solutions of lead nitrate, Pb(NO3)2, and ammonium sulfide, (NH4)2S.
Pb2+(aq) + 2NO3–(aq) + 2NH4+(aq) + S2–(aq)
(A)2NH4NO3(s) + Pb2+(aq) + S2–(aq)
(B) Pb(NO3)2(s) + 2 NH4+(aq) + S2–(aq)
(C)(NH4)2S(s) + Pb2+(aq) + 2NO3–(aq)
(D)PbS(s) + 2NH4+(aq) + 2NO3–(aq)
- Which is the balanced net ionic equation for the formation of the precipitate silver chromate, Ag2CrO4?
(A)2Ag+(aq) + CrO42–(aq) Ag2CrO4(s)
(B)Ag+(aq) + CrO42–(aq) Ag2CrO4(s)
(C)Ag0(aq) + CrO42–(aq) Ag2CrO4(s)
(D)Ag2CrO4(s) 2Ag+(aq) + CrO42–(aq)
- Which two ions do not participate in the reaction between solutions of silver nitrate, AgNO3, and potassium chloride, KCl?
(A)K+ and Ag+(C)K+ and Cl–
(B)K+ and NO3–(D)Ag+ and Cl–
- In the equation:
BaCl2(aq) + Na2SO4(aq) BaSO4(s) +2NaCl (aq)
What is the net ionic equation for this reaction?
(A) Cl–(aq) + Na+(aq) NaCl (aq)
(B)Cl22–(aq) + Na22+(aq) 2NaCl (aq)
(C)Ba2+(aq) + SO42–(aq) BaSO4(s)
(D)BaCl2(s) + Na2SO4(s)
Ba2+(aq) + 2Cl–(aq) + 2Na+(aq) + SO42–(aq)
- Which is the net ionic equation for the reaction of
lead(II) nitrate and sodium chromate?
(A)Pb2+(aq) + CrO42–(aq) PbCrO4(s)
(B)Pb(NO3)2(aq) + Na2CrO4(aq)
PbCrO4(s) + 2NaNO3(aq)
(C)2Na+(aq) + CrO42–(aq) Na2CrO4(aq)
(D)Pb2+(aq) + NO3–(aq) + Na+(aq) + CrO42–(aq)PbCrO4(s) + Na+(aq) + NO3–(aq)
- What is the net ionic equation for the reaction between lead(II) nitrate and potassium sulfide?
(A)Pb2+(aq) + S2–(aq) PbS(s)
(B)K+(aq) + NO3–(aq) KNO3(aq)
(C)Pb(NO3)2(aq) + K2S(aq) PbS(s) + 2KNO3(aq)
(D)Pb2+(aq) + 2NO3–(aq) + 2K+(aq) + S2–(aq)
PbS(s) + 2K+(aq) + 2NO3–(aq)
STOICHIOMETRY W/LIMITING REACTANTS
- 50.0 g of water is heated from 22.0 °C to 36.0 °C. How much heat is absorbed?
Specific Heat Capacity for Water
4.18 J·°C–1·g–1
(A)1510 J(B)2930 J(C)4520 J(D)4600 J
(E)7520 J
- How much heat is required to raise the temperature of 25.0 g of iron from 10.0 °C to 40.0 °C?
Specific Heat Capacity of Iron
0.444 J·g–1·°C–1
(A)750 J(B)444 J(C)333 J(D)313 J
- What volume is occupied by 2.00 g of a substance having a density of 5.00 g·cm–3?
(A)0.400 cm3(C)7.00 cm3
(B)2.50 cm3 (D)10.0 cm3
- If 50 mL of a 200 mL sample of 0.10 M sodium chloride solution is spilled, what is the concentration of the remaining solution?
(A)0.20 M(B)0.10 M(C)0.075 M(D)0.025 M
- In the reaction
4Al + 3O2 2Al2O3
how many moles of aluminum oxide, Al2O3, are produced from one mole of aluminum, Al?
(A)0.5(B)2(C)3(D)4
- Given the equation
N2 + 3H2 2NH3
Theoretically, the number of moles of ammonia produced from 2 mol of nitrogen is
(A)1(B)2(C)3(D)4
(E)5
- In an experiment, 0.0041 mol of maleic acid, C4H4O4, reacted with 0.0082 mol of sodium hydroxide, NaOH. Which equation describes the reaction?
(A)C4H4O4 + NaOH NaC4'H3O4 + H2O
(B)C4H4O4 + 2NaOH Na2C4H2O4 + 2H2O
(C)C4H4O4 + 3NaOH Na3C4HO4 + 3H2O
(D)C4H4O4 + 4NaOH Na4C4O4 + 4H2O
- In neutralizing 0.015 mol of H3PO3, 0.030 mol of NaOH was consumed. Which equation describes this reaction?
(A)H3PO3 + NaOH NaPO3 + H2O
(B)H3PO3 + NaOH NaH2PO3 + H2O
(C)H3PO3 + 3NaOH NaPO3 + 3H2O
(D)H3PO3 + 2NaOH Na2HPO3 + 2H2O
- Silica, SiO2, reacts with hydrofluoric acid, HF, according to this equation
SiO2 + 4HF 2H2O + SiF4
Which reagent is completely consumed when 2 mol of SiO2 is added to 6 mol of HF?
(A)SiF4(B)H2O(C)HF(D)SiO2
- How many grams of calcium carbonate, CaCO3, would be needed to produce 44.8 L of carbon dioxide gas, CO2, measured at STP?
Atomic Molar Masses
Ca 40.1 g·mol–1
C 12.0 g·mol–1
O 16.0 g·mol–1
CaCO3 + 2HCl CaCl2 + H2O + CO2
(A)50.0(B)100(C)111(D)200
- What volume of oxygen, O2, at STP can be prepared by the complete decomposition of 0.100 mol of potassium chlorate, KClO3?
2KClO3 2KCl + 3O2
(A)1.49 L(B)3.36 L(C)4.80 L(D)6.72 L
- The equilibrium equation for the Haber process at 500 °C is
N2 + 3H2 2NH3 + heat
When one liter of nitrogen combines with three liters of hydrogen the maximum volume of ammonia produced is
(A)1 L(B)2 L(C)3 L(D)4 L
(E)6 L
- The volume of pure oxygen needed to burn completely 800 mL of acetylene (C2H2) gas is
(A)800 mL(D)10000 mL
(B)1600 mL (E)20000 mL
(C)2000 mL
- A mixture of 2.0 g of hydrogen and 32 g of oxygen is exploded and produces water. What mass of gas remains uncombined?
Atomic Molar Masses
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)1.0 g of hydrogen(D)16 g of oxygen
(B)1.0 g of oxygen(E)24 g of oxygen
(C)8.0 g of oxygen
- The equation for the complete combustion of butane gas, C4H10, is
2C4H10 + 13O2 8CO2 + 10H2O
How many liters of carbon dioxide is produced when a mixture of 1.00 L of butane gas and 13.0 L of oxygen is burned? (measured under the same conditions)
(A)1.00 L(B)l. 63 L(C)8.00 L(D)4.00 L
(E)13.0 L
- The mass of potassium chloride formed by the complete decomposition of 490 g of potassium chlorate is
Atomic Molar Masses
Cl 35.5 g·mol–1
K 39.1 g·mol–1
O 16.0 g·mol–1
(A)96 g(B)122.5 g(C)149 g(D)298 g
(E)490 g
- In the reaction
2Al + 3H2SO4 3H2 + Al2(SO4)3
the mass of aluminum that reacts with 1 mol of hydrogen ions is approximately
(A)3.0 g(B)9.0 g(C)13.5 g(D)27.0 g
(E)81.0 g
- What is the maximum mass of tungsten (W) obtained from the use of 18 g of hydrogen according to the equation
WO3 + 3H2 W + 3H2O
Atomic Molar Masses
H 1. g·mol–1
W 184. g·mol–1
(A)1 184 g (D)18 184 g
(B)3 184 g (E)184 g + 3 16 g
(C)9 184 g
- In the reaction represented by the equation
COCl2 + 2NaI 2NaCl + CO + I2
what is the maximum mass of iodine that can be liberated from 60.0 g of sodium iodide?
Molar Masses
NaI 150. g·mol–1
I2 254. g·mol–1
(A)5.00 g(B)25.4 g(C)50.8 g(D)127 g
(E)254 g
- What mass of iron oxide, Fe3O4, is produced from 2.00 mol of iron, Fe?
3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g)
Molar Mass
Fe3O4 231. g·mol–1
(A)154 g(B)231 g(C)462 g(D)693 g
- What mass of calcium hydroxide, Ca(OH)2, is obtained from 18.7 g of calcium oxide, CaO?
Atomic Molar Masses
Ca 40.1 g·mol–1
H 1.0 g·mol–1
O 16.0 g·mol–1
CaO + H2O Ca(OH)2
(A)18.7 g(B)24.7 g(C)56.1 g(D)74.1 g
- Consider the equation:
2Al(OH)3 Al2O3 + 3H2O
When 15.0 g of aluminum hydroxide, Al(OH)3 is decomposed, how many grams of water will be formed?
Atomic Molar Masses
Al 27.0 g·mol–1
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)3.86 g(B)5.19 g(C)4.20 g(D)22.5 g
- What mass of water is produced by complete combustion of 126 g of propene, C3H6?
2C3H6 + 9O2 6H2O + 6CO2
Atomic Molar Masses
C 12.0 g·mol–1
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)18.0 g(B)54.0 g(C)126 g(D)162 g
- If 10.0 g of iron, Fe, and 10.0 g of sulfur, S, are heated together, how many grams of iron(II) sulfide, FeS, could be formed?
Atomic Molar Masses
Fe 55.8 g·mol–1
S 32.1 g·mol–1
Fe + S FeS
(A)10.0(B)15.7(C)27.6(D)88.0
- The equation for the complete combustion of propane, C3H8, is
C3H8(g) + 5O2(g) 3CO2(g) + 4H2(g)
What is the maximum mass of carbon dioxide produced when a mixture of 0.500 mol of propane and 3.00 mol of oxygen is ignited?
Atomic Molar Masses
C 12.0 g·mol–1
O 16.0 g·mol–1
(A)22.0 g(B)29.3 g(C)44.0 g(D)66.0 g
(E)132. g
- Consider the equation:
CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
How many moles of reactant are in excess when 2.0 mol of CH4(g) are ignited in 2.0 mol of O2(g)?
(A)l.0 mol CH4(C)0.5 mol CH4
(B)2.0 mol O2(D)no excess of either reactant
- How many grams of water, H2O, can be prepared when 2.00 mol of hydrogen, H2, and 2.00 mol of oxygen, O2, are mixed and reacted in this process?
2H2 + O2 2H2O
Atomic Molar Masses
H 1.0 g·mol–1
O 16.0 g·mol–1
(A)18.0 g(B)36.0 g(C)68.0 g(D)72.0 g
EMPIRICAL FORMULAS
- Upon analysis a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. Its simplest formula is
Atomic Molar Masses
B 11 g·mol–1
Na 23 g·mol–1
O 16 g·mol–1
(A)Na2B4O7 (D)Na3B4O
(B)NaBO(E)Na3BO4
(C)NaB2O5
- A compound contains 85.71% carbon and 14.29% hydrogen by mass. Its simplest formula is
Atomic Molar Masses
C 12 g·mol–1
H 1 g·mol–1
(A)CH2(B)CH(C)C2H(D)C2H2
(E)C2H4
- Decomposition of 12 g of a compound containing only carbon and hydrogen yields 9 g of carbon and 3 g of hydrogen. What is the simplest formula of the compound?
Atomic Molar Masses
C 12.0 g·mol–1
H 1.0 g·mol–1
(A)CH2(B)CH4(C)C2H5(D)C3H7
(E)C3H9
- A sample of a compound contains 3.21 g of sulfur, S, and 11.4 g of fluorine, F. Find the empirical formula of the compound.
Atomic Molar Masses
F 19.0 g·mol–1
S 32.0 g·mol–1
(A)SF(B)SF2(C)SF3(D)SF6
- A compound has the empirical formula CH2O and the molecular mass 180 g·mol–1. What is its molecular formula?
(A)CH8O10(C)C12H4O2
(B)C6H12O6 (D)C12H24O12
- A substance has an empirical (simplest) formula of CH3 and a molar mass of 30 g·mol–1. The molecular (true) formula is
Atomic Molar Masses
C 12.0 g·mol–1
H 1.0 g·mol–1
(A)(CH3)1(B)(CH3)2(C)(CH3)3(D)(CH3)4
- A compound whose empirical formula is CH2 has a molar mass of 28 g·mol–1. What is the molecular formula?
Atomic Molar Masses
C 12.0 g·mol–1
H 1.0 g·mol–1
(A)CH2(B)C2H4(C)C2H2(D)CH4
- A gaseous compound contains a ratio of one atom of sulfur to one atom of fluorine. A mole of this gas has a mass of approximately 102 g. What is the molecular formula?
Atomic Molar Masses
F 19. g·mol–1
S 32. g·mol–1
(A)SF(B)S2F2(C)S3F3(D)SF4
UNIT 7 atomic theory9-10 PERIOD TABLE/TRENDS
- A calcium ion is a calcium atom that has
(A)lost one electron.(D)lost two electrons.
(B)gained one electron.(E)gained two electrons.
(C)gained one ion.
- An atom that loses or gains an electron becomes
(A)an ion.(D)a molecule.
(B)a radical.(E)an electrolyte.
(C)an isotope.
- Metallic atoms become ions by
(A)losing protons.(C)gaining protons.
(B)losing electrons.(D)gaining electrons.
- How many electrons are in a chromium(III) ion, Cr3+?
(A)52(B)27(C)24(D)21
- The number of neutrons in the nucleus of an atom of Be is
(A)36(B)13(C)9(D)5
(E)4
- Which symbol represents an atom that contains the largest number of neutrons?
(A)U (B)U(C)Np(D)Pu
(E)Pa
- An ion has 13 electrons, 12 protons, and 14 neutrons. What is the mass of the ion?
(A)14 u(B)25 u(C)26 u(D)27 u
(E)39 u
- The symbol that represents 11 protons, 12 neutrons, and 10 electrons would be:
(A)Na+(B)Na(C)Mg2+(D)Mg
- The atomic number of an element is determined by the number of
(A)protons in each of its atoms.
(B)neutrons in each of its atoms.
(C)particles in each of its atoms.
(D)protons plus neutrons in each of its atoms.
(E)protons plus electrons in each of its atoms.
- All positive ions differ from their corresponding atoms by having
(A)larger diameters.
(B)fewer electrons.
(C)a charge of +1.
(D)greater atomic masses.
(E)stronger metallic properties
- Which group represents particles that contain the same number of electrons?
(A)F, Ne, Na (D) O2–, S2–, Se2–
(B)Mg, Al, Si(E)Ca2+, Fe2+, Zn2+
(C)Cl–, Ar, K+
- Note the chart of interactions of equal volumes of various 0.100 M aqueous solutions. (Symbols of elements or ions have been replaced by capital letters, and soluble products are indicated by “S”) What is the formula of the precipitate?
(A)DY(B)BY(C)AX(D)CX
- An odorless, colorless, tasteless gas is suspected to be oxygen. Which result would support this hypothesis?
(A)The gas would extinguish a flame.
(B)The gas would turn limewater milky.
(C)The gas would burn in air producing only water.
(D)A glowing splint would burst into flame in the gas.
- The chemical properties of atoms depend principally upon
(A)their atomic masses.
(B)the masses of the nuclei involved.
(C)the number of neutrons in their nuclei.
(D)the ratio in which the atoms combine with other atoms.
(E)the number of electrons in their outermost shells.
- The similar chemical behavior of the elements in a given family in the periodic table is best accounted for by the fact that atoms of these elements have
(A)the same number of electrons in the outermost shell.
(B)the same number of electrons.
(C)the same number of protons.
(D)similar nuclear structures.
(E)a common origin
- The best explanation of the extreme activity of fluorine as compared to other halogens is that the fluorine atom
(A)has the smallest atomic radius.
(B)has the smallest nuclear charge.
(C)has seven valence electrons.
(D)is the strongest reducing agent.
(E)needs one electron to complete its outermost shell.
- In the modern periodic table the elements are arranged in the order of increasing
(A)atomic masses.(C)atomic numbers.
(B)atomic radii.(D)atomic volumes.
140. In which set are the three elements in the same family?
(A)B, C, N(C)Hg, Ga, Sr
(B)N, O, F(D)Zn, Cd, Hg
- Which scientist is given credit for developing the periodic table?
(A)Rutherford(C)Dalton
(B)Mendeleev(D)Planck
- lf XO2 is the correct formula for an oxide, the formula for the chloride of X is
(A)XCl2(B)XCl4(C)XCl(D)X2Cl3
(E)XCl3
- M represents a metallic element, the oxide of which has the formula M2O. The formula of the chloride of M is
(A)MCl(B)MCl2(C)MCl3(D)MCl4
(E)M2Cl
- What is the most probable formula for a compound of silicon, Si, and hydrogen, H?
(A)SiH(B)SiH2(C)SiH6(D)SiH4
- A hypothetical element, Z, forms a chloride with the formula ZCl5. What is the most probable formula for its oxide?
(A)ZO2(B)ZO5(C)Z2O5(D)Z5O2
- Based on the position of the elements in the periodic chart, the most likely formula for strontium nitride is
(A)Sr2N5(B)Sr5N2(C)Sr2N3(D)Sr3N2
- Which family of elements always forms ions with an oxidation number of +2 in compounds?
(A)halogens(C)transition metals
(B)alkali metals(D)alkaline–earth metals
- Which element is the most electronegative?
(A)Be(B)Mg(C)Ca(D)Sr
(E)Ba
- Since sodium and potassium are both members of Group 1A in the periodic table, a sodium and a potassium atom have the same
(A)atomic mass.