Fundamentals of Chemistry Study Guide Questions
Course Introduction
Fundamentals of Chemistry introduces students to the essential principles and concepts of chemistry, including atomic and molecular structure, chemical bonding, stoichiometry, states of matter, and thermochemistry. The course emphasizes the development of problem-solving skills, laboratory techniques, and an understanding of the role of chemistry in everyday life and broader scientific contexts. Through theoretical lessons and hands-on experiments, students gain a solid foundation necessary for advanced studies in chemistry and other related scientific fields.
Recommended Textbook
General Chemistry 11th Edition by Darrell D. Ebbing
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2610 Flashcards
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Chapter 1: Chemistry and Measurement
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Sample Questions
Q1) Express the volume 657.8 cm<sup>3</sup> in liters.
A)6.578 L
B)0.06578 L
C)0.6578 L
D)65.78 L
E)657.8 L
Answer: C
Q2) The boiling of water is a
A)physical change because the water merely disappears.
B)chemical change because heat is needed for the process to occur.
C)physical change because the gaseous water is chemically the same as the liquid.
D)chemical and physical change.
E)chemical change because a gas (steam)is given off.
Answer: C
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) Which of the following atomic symbols represents an isotope of <sup>94</sup>Mo?
A)(<sup>93</sup>Nb)
B)(<sup>95</sup>Tc)
C)(<sup>94</sup>Tc)
D)(<sup>95</sup>Mo)
E)(<sup>94</sup>Nb)
Answer: D
Q2) How many neutrons are there in the cobalt-59 nuclide?
A)27
B)2
C)86
D)59
E)32
Answer: E
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Chapter 3: Calculations With Chemical Formulas and Equations
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Sample Questions
Q1) One step in the isolation of pure rhodium metal (Rh)is the precipitation of rhodium(III)hydroxide from a solution containing rhodium(III)sulfate according to the following balanced chemical equation: Rh<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>(aq)+ 6NaOH(aq) 2Rh(OH)<sub>3</sub>(s)+ 3Na<sub>2</sub>SO<sub>4</sub>(aq)
If the reaction of 0.500 g of rhodium(III)sulfate with excess sodium hydroxide produces 0.330 g of rhodium(III)hydroxide,what is the percent yield?
A)423 %
B)211 %
C)52.9 %
D)66 %
E)105 %
Answer: E
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Chapter 4: Chemical Reactions
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Sample Questions
Q1) Which of the following reactions involves neither oxidation nor reduction?
A)N<sub>2</sub>(g)+ 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g)
B)NH<sub>4</sub>NO<sub>2</sub>(s) N<sub>2</sub>(g)+ 2H<sub>2</sub>O(l)
C)Cu(s)+ 2Ag<sup>+</sup>(aq) Cu<sup>2+</sup>(aq)+ 2Ag(s)
D)2CrO<sub>4</sub><sup>2-</sup>(aq)+
2H<sup>+</sup>(aq)
Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup>(aq)+ H<sub>2</sub>O(l)
E)C<sub>2</sub>H<sub>4</sub>(g)+
C<sub>2</sub>H<sub>6</sub>(g)
H<sub>2</sub>(g)
Q2) All of the following reactions can be described as displacement reactions except
A)Zn(s)+ FeCl<sub>2</sub>(aq) ZnCl<sub>2</sub>(aq)+ Fe(s).
B)C<sub>6</sub>H<sub>6</sub>(l)+
Cl<sub>2</sub>(g) C<sub>6</sub>H<sub>5</sub>Cl(l)+ HCl(g).
C)2Na(s)+ 2H<sub>2</sub>O(l) 2NaOH(aq)+ H<sub>2</sub>(g).
D)Cu(s)+ 2AgNO<sub>3</sub>(aq) Cu(NO<sub>3</sub>)<sub>2</sub>(aq)+ 2Ag(s). E)CuSO<sub>4</sub>(aq)+ Fe(s) Cu(s)+ FeSO<sub>4</sub>(aq).
Q3) Which of the following compounds is soluble in water?
A)Sc<sub>2</sub>O<sub>3</sub>
B)Li<sub>3</sub>P
C)CuS
D)Hg<sub>2</sub>I<sub>2</sub> E)NiS
Page 6
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Chapter 5: The Gaseous State
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Sample Questions
Q1) A sample of hydrogen was collected by water displacement at 23.0°C and an atmospheric pressure of 735 mmHg.Its volume is 568 mL.After water vapor is removed,what volume would the hydrogen occupy at the same conditions of pressure and temperature? (The vapor pressure of water at 23.0°C is 21 mmHg.)
A)509 mL
B)539 mL
C)552 mL
D)568 mL
E)585 mL
Q2) For an ideal gas,which of the following statements is true?
A)P is inversely proportional to n at constant V and T.
B)V is inversely proportional to T at constant n and P.
C)V is inversely proportional to n at constant P and T.
D)n is inversely proportional to T at constant P and V.
E)P is inversely proportional to T at constant n and V.
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Chapter 6: Thermochemistry
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Sample Questions
Q1) The quantity of heat required to raise the temperature of a sample of a substance by 1°C is the sample's
A)work.
B)calorimetry.
C)heat capacity.
D)specific heat.
E)enthalpy.
Q2) Under conditions of constant pressure,for which of the following reactions is the magnitude of pressure-volume work going to be smallest?
A)BaO(s)+ SO<sub>3</sub>(g) BaSO<sub>4</sub>(s)
B)2NO(g)+ O<sub>2</sub>(g) 2NO<sub>2</sub>(g)
C)2H<sub>2</sub>O<sub>2</sub>(l) 2H<sub>2</sub>O(l)+ O<sub>2</sub>(g)
D)2KClO<sub>3</sub>(s) 2KCl(s)+ 3O<sub>2</sub>(g)
E)H<sub>2</sub>(g)+ Cl<sub>2</sub>(g) 2HCl(g)
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Chapter 7: Quantum Theory of the Atom
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Sample Questions
Q1) When an electron in an atom makes a transition from n = 4 to n = 5,which of the following statements is/are correct?
I.Energy is emitted.
II.Energy is absorbed.
III.The electron loses energy.
IV.The electron gains energy.
V.The electron cannot make this transition.
A)II and IV
B)II and III
C)I and IV
D)I and III
E)V
Q2) An orbital with the quantum numbers n = 5,l = 2,m<sub>l</sub> = -1 may be found in which subshell?
A)5f
B)5d
C)5p
D)5g
E)5s
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Chapter 8: Electron Configurations and Periodicity
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Sample Questions
Q1) The statement that "the lowest-energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as
A)the aufbau principle.
B)Hund's rule.
C)the Pauli exclusion principle.
D)Heisenberg uncertainty principle.
E)the quantum model.
Q2) Two elements that have the same ground-state valence shell configuration of ns<sup>2</sup>np<sup>2</sup> are
A)K and Mg.
B)O and Se.
C)Al and Ga.
D)Ge and Pb.
E)Mg and Ca.
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Chapter 9: Ionic and Covalent Bonding
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Sample Questions
Q1) In which of the following molecules is the octet rule violated?
A)PF<sub>5</sub>
B)OF<sub>2</sub>
C)ClF
D)PF<sub>3</sub>
E)SiF<sub>4</sub>
Q2) In the Lewis formula for phosphine,PH<sub>3</sub>,the number of lone pairs of electrons around the phosphorus atom is A)1.
B)2.
C)0.
D)3.
E)4.
Q3) How many valence electrons are present in the Lewis formula for the chlorate ion,C1O<sub>3</sub><sup>-</sup>?
A)32
B)24
C)30
D)26
E)28
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Chapter 10: Molecular Geometry and Chemical Bonding Theory
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Sample Questions
Q1) Which molecule does not have a planar molecular geometry?
A)SO<sub>3</sub>
B)HCCH
C)N<sub>2</sub>H<sub>4</sub>
D)HNNH
E)C<sub>2</sub>F<sub>4</sub>
Q2) What is the molecular geometry around an atom in a molecule or ion which is surrounded by five single bonds and no lone pairs of electrons.
A)trigonal bipyramidal
B)octahedral
C)linear
D)trigonal planar
E)tetrahedral
Q3) Which of the following characteristics does not apply to PF<sub>3</sub>?
A)has three bonds
B)contains polar bonds
C)polar molecule
D)one lone pair of electrons on phosphorus
E)trigonal planar
12
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Chapter 11: States of Matter; Liquids and Solids
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Sample Questions
Q1) Which of the following compounds has the highest normal boiling point?
A)CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>CH<sub>3</sub>
B)CH<sub>3</sub>Cl
C)CH<sub>3</sub>CH<sub>2</sub>OH
D)CH<sub>3</sub>OCH<sub>3</sub>
E)CH<sub>3</sub>CH<sub>2</sub>CH<sub>3</sub>
Q2) Which of the following pure substances has the lowest melting point?
A)LiBr
B)RbBr
C)CsBr
D)KBr
E)NaBr
Q3) The triple point of iodine is at 90 torr and 115°C.This means that liquid I<sub>2</sub>
A)cannot have a vapor pressure less than 90 torr.
B)is more dense than I<sub>2</sub>(s).
C)cannot exist at 1 atmosphere pressure.
D)cannot exist above 115°C.
E)can exist at pressure of 10 torr.
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Chapter 12: Solutions
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Sample Questions
Q1) What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.1010? The density of the solution is 1.2219 g/mL.
A)20.0%
B)12.0%
C)68.9%
D)12.3%
E)3.3%
Q2) A concentrated acetic acid solution has a density of 1.05 g/mL at 25°C and is 17.4
M.What is the percent by mass of CH<sub>3</sub>COOH in the solution?
A)99.5% CH<sub>3</sub>COOH by mass
B)1.7% CH<sub>3</sub>COOH by mass
C)0.6% CH<sub>3</sub>COOH by mass
D)2.8% CH<sub>3</sub>COOH by mass
E)57.1% CH<sub>3</sub>COOH by mass
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Chapter 13: Rates of Reaction
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Sample Questions
Q1) Which of the following experimental methods cannot be used to measure the rate of a reaction?
A)measurement of the absorbance of a colored reactant with time
B)measurement of the change in the partial pressure of a gas-phase product over time
C)measurement of the equilibrium concentration of an acidic product via titration with a strong base
D)measurement of the absorbance of a colored product with time
E)measurement of the change in the partial pressure of a gas-phase reactant over time
Q2) For which of the following hypothetical rate laws would the units of the rate constant have the general form M<sup>-3</sup>·time 1?
A)rate = k[A]<sup>4</sup>
B)rate = k
C)rate = k[A]
D)rate = k[A]<sup>2</sup>
E)rate = k[A]<sup>3</sup>
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Which of the following statements is true in a reaction system at equilibrium?
A)The equilibrium constant is zero.
B)The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products.
C)Reactants are reacting to form products at the same rate as products are reacting to form reactants.
D)Reactants and products are present in equimolar amounts.
E)The product of the concentrations of the products divided by the product of the concentrations of the reactants is always a constant.
Q2) The _____ is an economical process for making nitric acid in which nitric oxide is prepared by the oxidation of ammonia.
A)Hall-Héroult process
B)Ostwald process
C)Frasch process
D)Bessemer process
E)Castner process
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Chapter 15: Acids and Bases
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Sample Questions
Q1) Which of the following solutions has the highest hydroxide-ion concentration?
A)0.1 M HCl
B)a solution with pH = 5
C)0.1 M H<sub>2</sub>SO<sub>4</sub>
D)pure water
E)a solution with pOH = 12
Q2) A solution has a pH of 10.20 at 25°C.What is the hydroxide-ion concentration at 25°C?
A)3.8 M
B)2.2 × 10<sup>-2</sup> M
C)1.6 × 10<sup>-4</sup> M
D)6.3 × 10<sup>-11</sup> M
E)1.0 × 10<sup>-7</sup> M
Q3) At 25°C,what is the pH of a 10.0 M HNO<sub>3</sub> solution?
A)1.000
B)0.000
C)10.000
D)-1.000
E)14.000
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Chapter 16: Acid-Base Equilibria
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Sample Questions
Q1) What is the pH of a solution that is formed at 25°C by combining 400 mL of 0.030 M NaOH with 400 mL of 0.030 M HCl?
A)2.0
B)3.0
C)5.0
D)7.0
E)1.0
Q2) What is the pH at the equivalence point of the titration of a strong acid with a strong base?
A)3.9
B)4.5
C)8.2
D)7.0
E)none of these
Q3) Which of the following solutions has the highest hydroxide-ion concentration?
A)0.10 M NH<sub>4</sub>ClO<sub>4</sub>
B)0.10 M NaI
C)0.10 M NaNO<sub>3</sub>
D)0.10 M NH<sub>4</sub>Cl
E)0.10 M NaCN
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Chapter 17: Solubility and Complex-Ion Equilibria
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Q1) In which of the following solutions would CaC<sub>2</sub>O<sub>4</sub> have the highest molar solubility?
A)0.01 M Na<sub>2</sub>C<sub>2</sub>O<sub>4</sub>
B)0.01 M NaCl
C)0.01 M HCl
D)0.01 M Ca(NO<sub>3</sub>)<sub>2</sub>
E)0.01 M NaHC<sub>2</sub>O<sub>4</sub>
Q2) Which of the following salts has the lowest molar solubility?
A)SrCO<sub>3</sub> (K<sub>sp</sub> = 9.3 × 10<sup>-10</sup>)
B)MnS (K<sub>sp</sub> = 2.5 × 10<sup>-10</sup>)
C)BaF<sub>2</sub> (K<sub>sp</sub> = 1 × 10<sup>-6</sup>)
D)BaSO<sub>4</sub> (K<sub>sp</sub> = 1.1 × 10<sup>-10</sup>)
E)AgCl (K<sub>sp</sub> = 1.8 × 10<sup>-10</sup>)
Q3) What is the solubility product expression for Al(OH)<sub>3</sub>?
A)K<sub>sp</sub> = [Al<sup>3+</sup>][3OH<sup>-</sup>]
B)K<sub>sp</sub> = 3[Al<sup>3+</sup>][OH<sup>-</sup>]<sup>3</sup>
C)K<sub>sp</sub> = [Al<sup>3+</sup>][OH<sup>-</sup>]<sup>3</sup>
D)K<sub>sp</sub> = [Al<sup>3+</sup>][3OH<sup>-</sup>]<sup>3</sup>
E)K<sub>sp</sub> = [Al<sup>3+</sup>][OH<sup>-</sup>]
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Chapter 18: Thermodynamics and Equilibrium
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Sample Questions
Q1) For which of the following reactions is S° > 0 at 25°C?
A)2H<sub>2</sub>(g)+ O<sub>2</sub>(g) 2H<sub>2</sub>O(g)
B)2ClBr(g) Cl<sub>2</sub>(g)+ Br<sub>2</sub>(g)
C)I<sub>2</sub>(g) I<sub>2</sub>(s)
D)2NO(g)+ O<sub>2</sub>(g) 2NO<sub>2</sub>(g)
E)NH<sub>4</sub>HS(s) NH<sub>3</sub>(g)+ H<sub>2</sub>S(g)
Q2) For a reaction that has an equilibrium constant of 6 × 10<sup>9</sup>,which of the following statements must be true?
A) S° is positive.
B) G° is negative.
C) G° is positive.
D) H° is negative.
E) H° is positive.
Q3) The third law of thermodynamics states that
A)the entropy of the universe is increasing.
B)the entropy of the universe is constant.
C)the entropy of the universe equals the sum of the entropy of system and that of the surroundings.
D)the absolute entropy of a substance decreases with increasing temperature.
E)the entropy is zero at 0 K for a perfect crystal.
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Chapter 19: Electrochemistry
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Q1) A piece of iron half-immersed in a sodium chloride solution will corrode more rapidly than a piece of iron half-immersed in pure water,because
A)the ions,which are not present in pure water,balance the accumulation of charge in each of the half-cells.
B)the chloride ions increase the pH of the solution.
C)the sodium ions oxidize the iron atoms.
D)the chloride ions form a precipitate with iron.
E)the chloride ions oxidize the iron atoms.
Q2) What is the SI unit of potential difference?
A)coulomb
B)farad
C)volt
D)joule
E)ampere
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Chapter 20: Nuclear Chemistry
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Sample Questions
Q1) One of the first nuclear bombs based on the fission of U-235 had a maximum yield of 7.5 x10<sup>13</sup> J.If the fission of U-235 releases 1.8 × 10<sup>13</sup> J/mol,approximately what mass of U-235 was used in this bomb? (U-235 has a molar mass of 235.04 g/mol)
A)9.8 × 10<sup>2</sup> g U-235
B)56 g U-235
C)0.018 g U-235
D)0.0010 g U-235
E)2.3 × 10<sup>2</sup> g U-236
Q2) Which of the following nuclides will produce <sup>192</sup>Pt upon undergoing beta decay?
A)(<sup>192</sup>Ir)
B)(<sup>193</sup>Pt)
C)(<sup>192</sup>Au)
D)(<sup>196</sup>Hg)
E)(<sup>188</sup>Os)
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Chapter 21: Chemistry of the Main-Group Metals
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Sample Questions
Q1) Which of the following metals is expected to have the fastest reaction with water?
A)Li
B)K
C)Cs
D)Na
E)Rb
Q2) Which of the following reactions describes the formation of an ionic hydride?
A)2H<sub>2</sub>(g)+ O<sub>2</sub>(g) 2H<sub>2</sub>O(l)
B)H<sub>2</sub>(g)+ Cl<sub>2</sub>(g) 2HCl(g)
C)2K(s)+ H<sub>2</sub>(g) 2KH(s)
D)H<sub>2</sub>(g)+
C<sub>2</sub>H<sub>6</sub>(g)
C<sub>2</sub>H<sub>4</sub>(g)
E)N<sub>2</sub>(g)+ 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g)
Q3) The Group 8A elements in the periodic table are called _____.
A)noble gases
B)metalloids
C)lanthanides
D)alkali metals
E)ideal gases
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Chapter 22: The Transition Elements and Coordination Compounds
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Q1) Which of the following species is least likely to function as a ligand in a transition-metal coordination compound?
A)NH<sub>3</sub>
B)CO<sub>3</sub><sup>2-</sup>
C)H<sub>2</sub>O
D)BF<sub>3</sub>
E)Cl<sup>-</sup>
Q2) How many unpaired electrons are there in an octahedral cobalt(III)complex with weak-bonding ligands?
A)1
B)2
C)4
D)3
E)0
Q3) What is the maximum oxidation state for rhenium,Re?
A)6
B)3
C)2
D)7
E)4
24
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Chapter 23: Organic Chemistry
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Sample Questions
Q1) What is the IUPAC name for the substance having the following condensed structural formula?
(CH<sub>3</sub>)<sub>3</sub>CCH<sub>2</sub>COOH
A)3,3-dimethyl-1-butanone
B)3,3-dimethylbutanoic acid
C)4,4-dimethylpentanal
D)3,3-dimethylpropanoic acid
E)hexanoic acid
Q2) What is the major product upon addition of HCl to propene?
A)CH<sub>3</sub>CHClCH<sub>2</sub>Cl
B)CH<sub>3</sub>CH<sub>2</sub>CH<sub>3</sub>
C)CH<sub>3</sub>CHClCH<sub>3</sub>
D)CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>Cl
E)CH<sub>3</sub>CHCl=CH<sub>2</sub>
Q3) Which of the following alcohols is a tertiary alcohol?
A)HOCH<sub>2</sub>CH(OH)CH<sub>2</sub>OH
B)CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>OH
C)HOCH<sub>2</sub>CH<sub>2</sub>OH
D)(CH<sub>3</sub>)<sub>3</sub>COH
E)CH<sub>3</sub>CH<sub>2</sub>CH(OH)CH<sub>3</sub>
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Chapter 24: Polymer Materials: Synthetic and Biological
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Sample Questions
Q1) In an electrically conducting polymer,what is a "hole"?
A)It is a region of negative charge.
B)It is a delocalized electron.
C)It is an antibonding molecular orbital.
D)It is a molecular orbital from which a electron has been abstracted.
E)It is an ion,such as I<sub>3</sub><sup>-</sup>,added to increase the conductivity of the polymer.
Q2) Where in the cell does protein synthesis cell take place?
A)ribosome
B)nucleus
C)gene
D)chromosome
E)codon
Q3) The nucleic acid sequence that is complementary to the DNA sequence GAC TAC GTT AGC is
A)CTG ATG CAA TCG.
B)GAC TAC GTT AGC.
C)CGA TTG CAT CAG.
D)TCA GCA TGG CTA.
E)none of these
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