General Chemistry I Final Exam Questions
Course Introduction
General Chemistry I provides a comprehensive introduction to the fundamental principles of chemistry, including atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, and basic chemical reactions. The course emphasizes quantitative problem-solving and the application of conceptual understanding to real-world phenomena. Laboratory sessions reinforce theoretical concepts through hands-on experiments, focusing on precise measurement, observation, and data analysis. This course lays the foundation for advanced studies in chemistry and related scientific disciplines.
Recommended Textbook
Chemistry 6th Edition by John E. McMurry
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Page 2
Chapter 1: Chemistry: Matter and Measurement
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Sample Questions
Q1) The quantity 1.0567 qt rounded to two significant figures is ________ qt.
Answer: 1.1
Q2) What symbol is used to represent the factor 10<sup>-9</sup>?
A)M
B)m
C)
D)n
Answer: D
Q3) What is the chemical symbol for platinum?
A)P
B)Pa
C)Pt
D)Pu
Answer: C
Q4) Which of the following volumes is equal to 40 mL?
A)40 cm<sup>3</sup>
B)40 dm<sup>3</sup>
C)0)40 L
D)0)000 40 kL
Answer: A
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) The number of moles of Li in 34.7 g Li is ________.
Answer: 5.00 mol
Q2) The symbol of the isotope having Z = 88 and A = 226 is ________.
Answer: 11ea7a38_c8cd_82a1_aa4c_f511e3c2a7ee_TB4939_11
Q3) What is the chemical formula for strontium hydride?
A)SrH<sub>2</sub>
B)SrOH
C)SrOH<sub>2</sub>
D)Sr(OH)<sub>2</sub>
Answer: A
Q4) Which are isotopes? An atom that has an atomic number of 34 and a mass number of 76 is an isotope of an atom that has
A)an atomic number of 32 and a mass number of 76.
B)an atomic number of 34 and a mass number of 80.
C)42 neutrons and 34 protons.
D)42 protons and 34 neutrons.
Answer: B
Q5) Atoms of the same element always have the same number of ________ in their nuclei.
Answer: protons
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Chapter 3: Formulas, equations, and Moles
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Sample Questions
Q1) What is the concentration of NO<sub>3</sub><sup>-</sup> ions in a solution prepared by dissolving 15.0 g of Ca(NO<sub>3</sub>)<sub>2</sub> in enough water to produce 300.mL of solution?
A)0)152 M
B)0)305 M
C)0)403 M
D)0)609 M
Answer: D
Q2) Oxygen can be produced from the catalytic decomposition of KClO<sub>3</sub> as shown in the balanced equation below. 2 KClO<sub>3</sub> 2 KCl + 3 O<sub>2</sub>
What is the percent yield if 3.20 grams of oxygen are formed from the reaction of 12.3 grams of KClO<sub>3</sub>?
Answer: 66.4%
Q3) The empirical formula of a compound that contains 82.66% carbon and 17.34% hydrogen is ________.
Answer: C<sub>2</sub>H<sub>5</sub>
Q4) How many moles are in 7.8 g of acetamide,CH<sub>3</sub>CONH<sub>2</sub>?
Answer: 0.13
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Chapter 4: Reactions in Aqueous Solutions
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Sample Questions
Q1) Determine the number of water molecules necessary to balance the reduction half reaction of ____ ClO<sub>3</sub><sup>-</sup>(aq) ____ Cl<sup>-</sup> (aq)that occurs in an acidic solution.
A)1
B)3
C)5
D)7
Q2) Which species functions as the reducing agent in the following reduction-oxidation reaction?
2 P(s)+ 3 Br<sub>2</sub>(l) 2 PBr<sub>3</sub>(l)
A)Br<sup>-</sup>(aq)
B)Br<sub>2</sub>(l)
C)P(s)
D)P<sup>3+</sup>(aq)
Q3) Which of the following compounds is not an Arrhenius acid?
A)CH<sub>3</sub>CO<sub>2</sub>H
B)CH<sub>3</sub>NH<sub>2</sub>
C)HNO<sub>3</sub>
D)H<sub>2</sub>SO<sub>4</sub>
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Chapter 5: Periodicity and the Atomic Structure of Atoms
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Sample Questions
Q1) Which atom in each group (I and II)has the smallest atomic radius?
(I)Ba,Hf,At (II)As,Sb,Bi
A)Ba;As
B)Ba;Bi
C)At;As
D)At;Bi
Q2) The property of a wave that is associated with brightness or intensity is ________.
Q3) For an orbital,a node is
A)the midpoint of the orbital.
B)a surface inside which there is a 90% chance of finding the electron.
C)a surface where there is a maximum probability of finding the electron.
D)a surface where there is no chance of finding the electron.
Q4) According to the Balmer-Rydberg equation,electromagnetic radiation with the shortest wavelength will be emitted when an electron undergoes which of the following transitions?
A)m = 1 n = 2
B)m = 2 n = 3
C)n = 2 m = 1
D)n = 3 m = 2
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Chapter 6: Ionic Bonds and Some Main-Group Chemistry
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Sample Questions
Q1) Which sphere represents the monatomic cation?
A)A
B)B
C)C
D)D
Q2) Which element,indicated by letter on the periodic table above,has a 3+ ion with the electron configuration 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup>?
A)A
B)B
C)C
D)D
Q3) Which picture corresponds to fluorine?
A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)
Q4) The oxidation number of the oxygen atoms in SrO<sub>2</sub> is ________.
Q5) Using shorthand notation,the ground-state electron configuration of the platinum ion in Cs<sub>2</sub>Pt is ________.
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Chapter 7: Covalent Bonds and Molecular Structure
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Sample Questions
Q1) A molecular compound that obeys the octet rule in which all atoms have a zero formal charge is
A)BaCl<sub>2</sub>
B)BrF<sub>3</sub>
C)NCl<sub>3</sub>
D)XeF<sub>4</sub>
Q2) Which molecular orbitals for homonuclear diatomic molecules are degenerate?
A) molecular orbitals
B) molecular orbitals
C) molecular orbitals and molecular orbitals
D)neither molecular orbitals nor molecular orbitals
Q3) Using only the elements Ba,Cl,and P,give the formula of a compound having largely ionic bonds.
Q4) Which element can accommodate more than eight electrons in its valence shell?
Q5) Based on formal charges,the best Lewis electron-dot structure of BF<sub>3</sub> has a B-F bond order equal to ________.
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Chapter 8: Thermochemistry: Chemical Energy
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Sample Questions
Q1) It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C.What is the specific heat of benzene?
A)1)14 J/(g °C)
B)1)72 J/(g °C)
C)3)48 J/(g °C)
D)5)25 J/(g °C)
Q2) The sum of the potential and kinetic energies for every molecule or ion in a system is the ________ energy of the system and is given the symbol ________.
Q3) For the reaction: A + 2 B 3 C, H° = -203 kJ.For the reaction 6 C 2 A + 4 B, H° = ________ kJ.
Q4) For the reaction,C<sub> </sub>H<sub>4</sub>(g) C(g)+ 4 H(g),one would expect
A) H° to be negative and S° to be negative.
B) H° to be negative and S° to be positive.
C) H° to be positive and S° to be negative.
D) H° to be positive and S° to be positive.
Q5) Heat transferred in a chemical reaction or physical change is expressed as E when the heat is transferred under constant ________ and is expressed as H when heat is transferred under constant ________ conditions.
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Chapter 9: Gases: Their Properties and Behavior
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Sample Questions
Q1) In the laboratory,hydrogen gas is usually made by the following reaction: Zn(s)+ 2 HCl(aq) H<sub>2</sub>(g)+ ZnCl<sub>2</sub>(aq)
How many liters of H<sub>2</sub> gas,collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C,can be made from 3.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C.
A)0)0975 L
B)1)30 L
C)1)33 L
D)1)36 L
Q2) What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?
A)-23°C
B)228°C
C)250°C
D)500°C
Q3) According to Graham's law,the rate of effusion of a gas is inversely proportional to the ________.
Q4) The burning of sulfur-containing coal can lead to acid rain due to the formation of ________ acid.
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Chapter 10: Liquids,solids,and Phase Changes
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Sample Questions
Q1) Which of the following molecules does not have a dipole moment?
A)CH<sub>2</sub>=CH<sub>2</sub>
B)NH<sub>3</sub>
C)CH<sub>3</sub>NH<sub>2</sub>
D)HCl
Q2) Which covalent bond is the most polar?
A)N-F
B)C-F
C)Cl-F
D)F-F
Q3) Solids having no ordered long-range structure are classified as
A)amorphous
B)crystalline
C)metallic
D)molecular
Q4) Pt(NH<sub>3</sub>)<sub>2</sub>Cl<sub>2</sub> is square planar.The isomer of Pt(NH<sub>3</sub>)<sub>2</sub>Cl<sub>2</sub> that has a non-zero dipole moment has a Cl-Pt-Cl bond angle of ________ degrees.
Q5) The property of a liquid that is a measure of the liquid's resistance to increase its surface area is ________.
Page 12
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Chapter 11: Solutions and Their Properties
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Sample Questions
Q1) What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>,in 125.9 g of water?
A)7)94 × 10<sup>- 4</sup> m
B)0)143 m
C)0)695 m
D)0)794 m
Q2) A solution of LiCl in water has X<sub>LiCl</sub> = 0.0 900.What is the molality?
A)4)46 m LiCl
B)5)00 m LiCl
C)5)49 m LiCl
D)9)89 m LiCl
Q3) What is the weight percent of a caffeine solution made by dissolving 4.35 g of caffeine,C<sub>8</sub>H<sub>10</sub>N<sub>4</sub>O<sub>2</sub>,in 75 g of benzene,C<sub>6</sub>H<sub>6</sub>?
A)0)055%
B)0)058%
C)5)5%
D)5)8%
Q4) Molarity is defined as ________,whereas molality is defined as ________.
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Chapter 12: Chemical Kinetics
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Sample Questions
Q1) The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N<sub>2</sub>O<sub>5</sub>(g) 4 NO<sub>2</sub>(g)+ O<sub>2</sub>(g)
If the rate of disappearance of N<sub>2</sub>O<sub>5</sub> is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO<sub>2</sub> at that moment?
A)0)700 mol/min
B)1)40 mol/min
C)2)80 mol/min
D)5)60 mol/min
Q2) Intermediates occur at which reaction stages?
A)reaction stages 1 and 5
B)reaction stages 2,3,and 4
C)reaction stages 2 and 4
D)reaction stage 3
Q3) For the zeroth-order reaction: A products,what will happen to the rate of reaction if the concentration of A is doubled?
A)The rate will be halved.
B)The rate will be doubled.
C)The rate will be quadrupled.
D)The rate will remain the same.
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Chapter 13: Chemical Equilibrium
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Sample Questions
Q1) If K<sub>c</sub> equals 0.11 at 25°C for the reaction: N<sub>2</sub>O<sub>4</sub>(g) 2 NO<sub>2</sub>(g),what is K<sub>c</sub> for the reaction: NO<sub>2</sub>(g) 1/2 N<sub>2</sub>O<sub>4</sub>(g)?
A)0)33
B)3)0
C)4)5
D)9)1
Q2) Which of the following statements about a catalyst is true?
A)A catalyst changes the position of the equilibrium in a reaction.
B)A catalyst increases the temperature of a reaction.
C)A catalyst is consumed in a chemical reaction.
D)A catalyst provides a lower energy pathway for a reaction.
Q3) The decomposition of ammonia is: 2 NH<sub>3</sub>(g)= N<sub>2</sub>(g)+ 3 H<sub>2</sub>(g).If K<sub>p</sub> is 1.5 × 10<sup>3</sup> at 400°C,what is the partial pressure of ammonia at equilibrium when N<sub>2</sub> is 0.10 atm and H<sub>2</sub> is 0.15 atm?
A)2)2 × 10<sup>-7</sup> atm
B)4)7 × 10<sup>-4</sup> atm
C)2)1 × 10<sup>3</sup> atm
D)4)4 × 10<sup>6</sup> atm
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Chapter 14: Aqueous Equilibria: Acids and Bases
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Sample Questions
Q1) Which one of the following is not considered to be a Lewis base?
A)H<sub>2</sub>O
B)NH<sub>3</sub>
C)NH<sub>4</sub><sup>+</sup>
D)Cl<sup>-</sup>
Q2) A Br nsted-Lowry acid is best defined as a substance that can
A)accept a hydroxide ion.
B)donate a hydroxide ion.
C)accept a proton.
D)donate a proton.
Q3) Which one of the following salts,when dissolved in water,produces the solution with the highest pH?
A)KH CO<sub>3</sub>
B)CsClO<sub>4</sub>
C)RaO
D)CH<sub>3</sub>CH<sub>3</sub>NH<sub>3</sub>Cl
Q4) Phenobarbital has a pK<sub>a</sub> = 7.4.Compared to a 1.0 × 10<sup>-3</sup> M solution,1.0 × 10<sup>-4</sup> M phenobarbital will have a ________ (higher,lower)pH and a ________ (higher,lower)percent ionization.
Q5) A proton hydrated by four water molecules has the formula ________.
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Chapter 15: Applications of Aqueous Equilibria
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Sample Questions
Q1) State whether the solubility of Cu(OH)<sub>2</sub> will increase or decrease upon the addition of aqueous solutions of a)HCl,b)NaOH,c)NH<sub>3</sub>.
Q2) What is the equation relating the equilibrium constant K<sub>n</sub> for the neutralization of a weak acid with a weak base to the K<sub>a</sub> of the acid,the K<sub>b</sub> of the base and K<sub>w</sub>?
Q3) What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.K<sub>a</sub> =1.8 × 10<sup>-5</sup> for CH<sub>3</sub>CO<sub>2</sub>H.
A)5)28
B)7)00
C)8)72
D)10.02
Q4) What is the characteristic pH-titration curve for the titration of a weak acid by a strong base?
A)A
B)B
C)C
D)D
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Chapter 16: Thermodynamics: Entropy, free Energy, and Equilibrium
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Sample Questions
Q1) Which of the following is true?
A)As a reaction at constant temperature and pressure goes to equilibrium,| G| decreases.
B)The larger G°,the faster the reaction.
C)The standard state for solutes is the pure solute at 1 atm.
D)When a reaction reaches equilibrium, G° = 0.
Q2) What is the entropy change associated with the expansion of one mole of an ideal gas from an initial volume of V to a final volume of V of 2.50V at constant temperature?
A) S = 2.50 R ln (V<sub>f</sub>/V<sub>i</sub>)
B) S = -2.50 R ln (V<sub>f</sub>/V<sub>i</sub>)
C) S = R ln 2.50
D) S = -R ln 2.50
Q3) How will the spontaneity of this reaction vary with temperature? This reaction is
A)nonspontaneous at all temperatures.
B)nonspontaneous at high temperatures and spontaneous at low temperatures.
C)spontaneous at high temperatures and nonspontaneous at low temperatures.
D)spontaneous at all temperatures.
Q4) What is the entropy of 10 molecules in a system of 1000 boxes?
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Chapter 17: Electrochemistry
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Sample Questions
Q1) Consider the following standard reduction potentials, Al<sup>3+</sup>(aq)+ 3 e<sup>-</sup> Al(s)E° = -1.66 V I<sub>2</sub>(s)+ 2 e<sup>-</sup> 2 I<sup>-</sup>(aq)E° = +0.54 V
Under standard conditions,
A)Al<sup>3+</sup>(aq)is a stronger oxidizing agent than I<sub>2</sub>(s),and I<sup>-</sup>(aq)is a stronger reducing agent than Al(s).
B)I<sub>2</sub>(s)is a stronger oxidizing agent than Al<sup>3+</sup>(aq),and Al(s)is a stronger reducing agent than I<sup>-</sup>(aq).
C)Al(s)is a stronger oxidizing agent than I<sup>-</sup>(aq),and Al<sup>3+</sup>(aq)is a stronger reducing agent than I<sub>2</sub>(s).
D)I<sup>-</sup>(aq)is a stronger oxidizing agent than Al(s),and I<sub>2</sub>(s)is a stronger reducing agent than Al<sup>3+</sup>(aq).
Q2) For the hypothetical reaction 3 A + 2 B<sup>x</sup> 3 A<sup>y</sup> + 2 B,E° = 0.85 V and G° = -495 kJ.For this reaction the values of x and y are ________ and ________.
Q3) In the shorthand notation for a galvanic cell,a single vertical line (|)represents a ________,and a double vertical line (||)represents a ________.
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Chapter 18: Hydrogen, oxygen, and Water
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Sample Questions
Q1) Which hydride has the lowest melting point?
A)hydride (1)
B)hydride (2)
C)hydride (3)
D)hydride (4)
Q2) Which one of the following binary oxides is the most acidic?
A)P<sub>2</sub>O<sub>5</sub>
B)As<sub>2</sub>O<sub>5</sub>
C)Bi<sub>2</sub>O<sub>5</sub>
D)Cl<sub>2</sub>O<sub>7</sub>
Q3) How many liters of hydrogen gas are needed to produce 90.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?
2 H<sub>2</sub>(g)+ O<sub>2</sub>(g) 2 H<sub>2</sub>O(l)
A)61.1 L
B)122 L
C)183 L
D)366 L
Q4) At 25°C the dissociation constant K<sub>w</sub> for T<sub>2</sub>O is 0.06 × 10<sup>-14</sup>.What is the molar concentration of OT<sup>-</sup> in 0.025 M TCl?
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Chapter 19: The Main-Group Elements
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Q1) Disproportionation is a reaction in which a reactant is both oxidized and reduced in the same reaction.In the disproportionation reaction below,the oxidation number of chlorine in Cl<sub>2</sub>,ClO<sup>-</sup>,and Cl<sup>-</sup> is ________,________,and ________,respectively.
Cl<sub>2</sub>(g)+ 2 OH<sup>-</sup>(aq) ClO<sup>-</sup>(aq)+ Cl<sup>-</sup>(aq)+ H<sub>2</sub>O(l)
Q2) The percentage of carbon in the endohedral fullerene complexes KrC<sub>60</sub> and XeC<sub>60</sub> is ________%C and ________%C,respectively.
Q3) Which element indicated on the above periodic table forms a binary hydride with molecular structure (2)shown above?
A)element A
B)element B
C)element C
D)element D
Q4) What is a convenient synthetic method for the preparation of SO<sub>2</sub>?
A)2 SO<sub>3</sub>(g)+ heat 2 SO<sub>2</sub>(g)+ O<sub>2</sub>(g)
B)S<sub>8</sub>(s)+ 8 O<sub>2</sub>(g)+ heat 8 SO<sub>2</sub>(g)
C)H<sub>2</sub>SO<sub>3</sub>(aq) H<sub>2</sub>O(l)+ SO<sub>2</sub>(aq)
D)FeSO<sub>3</sub>(s)+ heat FeO(s)+ SO<sub>2</sub>(g)
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Chapter 20: Transition Elements and Coordination Chemistry
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Q1) What is the coordination number of the Fe atom in K<sub>3</sub>[Fe(C<sub>2</sub>O<sub>4</sub>)<sub>3</sub>]?
A)2
B)3
C)4
D)6
Q2) The short hand electron configuration of iron in [FeF<sub>6</sub>]<sup>3-</sup> is
Q3) Identify the classification of isomers illustrated by [Co(NO<sub>2</sub>)(NH<sub>3</sub>)<sub>5</sub>]<sup>2+</sup> and [Co(ONO)(NH<sub>3</sub>)<sub>5</sub>]<sup>2+</sup>.
A)linkage isomers
B)ionization isomers
C)geometric isomers
D)optical isomers
Q4) The number of unpaired electrons in Co(NH<sub>3</sub>)<sub>6</sub><sup>3+</sup> is ________.
Q5) [Co(NH<sub>3</sub>)<sub>5</sub>NCS]<sup>2+</sup> and [Co(NH<sub>3</sub>)<sub>5</sub>SCN]<sup>2+</sup> are examples of ________ isomers.
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Chapter 21: Metals and Solid-State Materials
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Sample Questions
Q1) Which picture corresponds to V?
A)picture (1)
B)picture (2)
C)picture (3)
D)picture (4)
Q2) What is not a major component of slag?
A)CaSiO<sub>3</sub>
B)Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>
C)Fe<sub>2</sub>O<sub>3</sub>
D)MnSiO<sub>3</sub>
Q3) Because nanoparticles have a larger percentage of atoms on the surface of the nanoparticle than on the surface of bulk material,nanoparticles have ________ melting points and ________ chemical reactivity than the bulk material.
Q4) Which of these elements is likely to be found in nature as a carbonate?
A)element A
B)element B
C)element C
D)element D
Q5) Nonoxide ceramics include silicon nitride,the formula of which is ________.
Page 23
Q6) The number of electrons that half fill a composite s-d band is ________.
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Chapter 22: Nuclear Chemistry
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Q1) A binding energy curve is a plot of binding energy per nucleon versus atomic number.In what region of the binding energy curve are the most stable elements found?
A)in the lower left region (low atomic mass)
B)in the central top region (moderate atomic mass)
C)in the lower right region (heavy atomic mass)
D)binding energy is not dependent on atomic mass
Q2) An average person receives 40 mrem of radiation from medical procedures annually.If a dose as low as 25 rem can lead to a decrease in white blood cell count,what is the maximum number of medical procedures that involve radiation allowable before white blood cell count decrease occurs?
Q3) The masses of <sup>4</sup>He,<sup>6</sup>Li,and <sup>10</sup>B are 4.0015,6.0135,and 10.0102 amu respectively.The fission of a boron-10 nucleus into He-4 and Li-6 would
A)absorb energy.
B)evolve energy.
C)result in no energy change.
D)Need more information
Q4) The mass defect for the chemical reaction shown below is ________ g. 2 F F<sub>2</sub> E = -159 kJ/mol
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Chapter 23: Organic and Biological Chemistry
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Sample Questions
Q1) What is the product when pure water and ethene are mixed?
A)an alcohol
B)a carboxylic acid
C)an ether
D)no reaction occurs
Q2) What is the H-C-C bond angle?
A)90°
B)109.5°
C)120°
D)180°
Q3) Which one of the following compounds is an alcohol?
A)CH<sub>3</sub>OCH<sub>3</sub>
B)CH<sub>3</sub>COCH<sub>3</sub>
C)(CH<sub>3</sub>)<sub>2</sub>CHOH
D)CH<sub>3</sub>CO<sub>2</sub>H
Q4) The number of different monochloro substitution products (C<sub>5</sub>H<sub>11</sub>Cl)that can form from the reaction of 2-methylbutane with Cl<sub>2</sub> is ________.
Q5) The molecule H<sub>2</sub>NCH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>OH contains an ________ functional group and an ________ functional group.
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