Introductory Chemistry
Solved Exam Questions
Course Introduction
Introductory Chemistry provides a foundational understanding of the core principles and concepts of chemistry. The course covers atomic and molecular structure, the periodic table, chemical bonding, stoichiometry, states of matter, chemical reactions, and basic thermochemistry. Emphasis is placed on developing problem-solving skills and applying chemical concepts to everyday life, as well as understanding the role of chemistry in broader scientific and societal contexts. This course is designed for students with little or no previous background in chemistry and serves as a stepping stone for more advanced studies in the field.
Recommended Textbook Chemistry 6th Edition by John E.
McMurry
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23 Chapters
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Page 2
Chapter 1: Chemistry: Matter and Measurement
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Sample Questions
Q1) How many significant figures are there in the answer for the following problem?
56)4 + 0.8822 + 21 = ?
A)one
B)two
C)three
D)four
Answer: B
Q2) A piece of plastic weighing 1.157 g has a volume of 1.48 cm<sup>3</sup>.A piece of wood has the same volume but weighs 3.85 g.The density of liquid X is 0.765 g/mL and the density of liquid Z is 1.13 g/mL.The two liquids are immiscible.If the plastic and wood are added to the two liquids,what is the order of layers from top to bottom in the container?
A)liquid X,liquid Z,plastic,wood
B)liquid X,plastic,liquid Z,wood
C)plastic,wood,liquid Z,liquid X
D)wood,liquid Z,plastic,liquid X
Answer: B
Q3) Using exponential notation,there are ________ g in 1.0 kg.
Answer: 10<sup>3</sup>
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Page 3
Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) Which of the compounds
CH<sub>4</sub>,SrCl<sub>2</sub>,Cr(NO<sub>3</sub>)<sub>3</sub>,XeF<sub>2</sub> are expected to exist as molecules?
A)only CH<sub>4</sub>
B)CH<sub>4</sub> and Xe F<sub>2</sub>
C)CH<sub>4</sub>,Cr(NO<sub>3</sub>)<sub>2</sub>,and Xe F<sub>2</sub>
D)SrCl<sub>2</sub> and Cr(NO<sub>3</sub>)<sub>2</sub>
Answer: B
Q2) Atoms of the same element always have the same number of ________ in their nuclei.
Answer: protons
Q3) Li<sub>2</sub>S is named
A)lithium disulfide.
B)lithium sulfide.
C)lithium(II)sulfide.
D)lithium sulfur.
Answer: B
Q4) The number of moles of Li in 34.7 g Li is ________.
Answer: 5.00 mol
Q5) The symbol of the isotope having Z = 88 and A = 226 is ________.
Answer: 11ea7a38_c8cd_82a1_aa4c_f511e3c2a7ee_TB4939_11
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Chapter 3: Formulas, equations, and Moles
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Sample Questions
Q1) What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L?
A)2)8 × 10<sup>- 2</sup> M
B)5)2 M
C)28 M
D)5)2 × 10<sup>3</sup> M
Answer: B
Q2) What mass of dinitrogen monoxide,N<sub>2</sub>O,contains the same number of molecules as 3.00 g of trichlorofluoromethane,CCl<sub>3</sub>F?
A)0)106 g
B)0)961 g
C)1)04 g
D)9)37 g
Answer: B
Q3) A balanced equation has the same numbers and kinds of ________ on both sides of the reaction arrow.
Answer: atoms
Q4) What is the empirical formula of benzene,C<sub>6</sub>H<sub>6</sub>?
Answer: CH
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Chapter 4: Reactions in Aqueous Solutions
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Sample Questions
Q1) Which of the following is not a strong acid?
A)HF
B)HCl
C)HBr
D)HI
Q2) What are the coefficients in front of NO<sub>3</sub><sup>-</sup>(aq)and Cu(s)when the following redox equation is balanced in an acidic solution: _____ NO<sub>3</sub><sup>-</sup>(aq)+ _____ Cu(s) _____ NO(g)+ _____ Cu<sup>2+</sup>(aq)?
A)2,3
B)2,6
C)3,4
D)3,6
Q3) The mixing of which pair of reactants will result in a precipitation reaction?
A)CsI(aq)+ NaOH(aq)
B)HCl(aq)+ Ca(OH)<sub>2</sub>(aq)
C)K<sub>2</sub>SO<sub>4</sub>(aq)+ Ba(NO<sub>3</sub>)<sub>2</sub>(aq)
D)NaNO<sub>3</sub>(aq)+ NH<sub>4</sub>Cl(aq)
Q4) The reaction shown below is classified as a(n)________ reaction. AgNO<sub>3</sub>(aq)+ HCl(aq) AgCl(s)+ HNO<sub>3</sub>(aq)
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Chapter 5: Periodicity and the Atomic Structure of Atoms
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Sample Questions
Q1) An oxygen molecule has a mass of 5.3 × 10<sup>-26</sup> kg and an approximate diameter of 3.6 × 10<sup>-10</sup> m.If the molecule is moving at 400 m/s (1000 mph)with an uncertainty in velocity of 1 m/s,the uncertainty in position
A)is less than or equal to 5 × 10<sup>-26</sup> m.
B)must be equal to 5 × 10<sup>-26</sup> m.
C)must be equal to 1 × 10<sup>-9</sup> m.
D)is greater than or equal to 1 × 10<sup>-9</sup> m.
Q2) Which one of these spheres represents an atom of As?
A)sphere (a)
B)sphere (b)
C)sphere (c)
D)sphere (d)
Q3) The energy of an electron in a multielectron atom depends on the quantum numbers ________ and ________.
Q4) Which of the following is true?
A)The Bohr atom is the model currently accepted for electrons in atoms.
B)Electrons travel around the nucleus in circular orbits.
C)There is a 5% chance of finding an electron in an atom outside its orbital.
D)The square of the wave function gives the probability of finding the electron.
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Chapter 6: Ionic Bonds and Some Main-Group Chemistry
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Sample Questions
Q1) Which alkaline earth metal reacts the most vigorously with water at room temperature?
A)Be
B)Ca
C)Ba
D)Sr
Q2) Of the following,which element has the highest first ionization energy?
A)beryllium
B)boron
C)hydrogen
D)lithium
Q3) The element in group 7A with the least favorable (least negative)electron affinity is ________.
Q4) Which picture corresponds to potassium?
A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)
Q5) The oxidation number of the oxygen atoms in SrO<sub>2</sub> is ________.
Q6) The element in period 3 with the smallest seventh ionization energy is ________.
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Chapter 7: Covalent Bonds and Molecular Structure
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Sample Questions
Q1) What are the F-Po-F bond angles in PoF<sub>6</sub> ?
A)60°
B)90°
C)109.5°
D)120°
Q2) In order to complete an electron-dot structure of alanine,the nitrogen atom needs
A)1 additional bond and 1 nonbonded pair of electrons.
B)1 additional bond and 2 nonbonded pairs of electrons.
C)1 nonbonded pair of electrons.
D)2 nonbonded pairs of electrons.
Q3) Which one of the following is expected to exhibit resonance?
A)NH<sub>4</sub><sup>+</sup>
B)HCN
C)CO<sub>2</sub>
D)NO<sub>2</sub><sup>-</sup>
Q4) Of H<sub>2</sub>CO and CO and CO<sub>2</sub>,the compound having the strongest C-O bond is ________.
Q5) The carbon-carbon bond in C<sub>2</sub>H<sub>2</sub> contains ________ and ________ bonds.
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Chapter 8: Thermochemistry: Chemical Energy
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Sample Questions
Q1) The sign of G for a reaction is if the reaction is spontaneous,________ if the reaction is at equilibrium,and ________ if the reaction is nonspontaneous.
Q2) It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 25.0°C to 70.0°C.What is the specific heat of benzene?
A)1)10 J/(g °C)
B)1)72 J/(g °C)
C)3)48 J/(g °C)
D)5)41 J/(g °C)
Q3) In which case is the work done on the system always positive?
A) E > 0
B) V > 0
C) V = 0
D) V < 0
Q4) Water has an unusually high
A)electrical conductivity.
B)heat of combustion.
C)heat of formation.
D)specific heat.
Q5) Is chemical energy a form of kinetic or potential molecular energy?
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Chapter 9: Gases: Their Properties and Behavior
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Sample Questions
Q1) A 0.286-g sample of gas occupies 125 mL at 60.cm of Hg and 25°C.What is the molar mass of the gas?
A)5)9 g/mol
B)44 g/mol
C)59 g/mol
D)71 g/mol
Q2) How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP?
CH<sub>4</sub>(g)+ 2 O<sub>2</sub>(g) CO<sub>2</sub>(g)+ 2 H<sub>2</sub>O(l)
A)13.9 L
B)27.8 L
C)55.5 L
D)60.5 L
Q3) Which drawing best shows the approximate level of the mercury in the tube when the temperature of the entire apparatus is lowered from +20°C to -20°C?
A)drawing (1)
B)drawing (2)
C)drawing (3)
D)drawing (4)
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Page 11
Chapter 10: Liquids,solids,and Phase Changes
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Sample Questions
Q1) Cesium has a radius of 272 pm and crystallizes in a body-centered cubic structure.What is the edge length of the unit cell?
A)314 pm
B)385 pm
C)544 pm
D)628 pm
Q2) Arrange the following in order of increasing boiling point. CH<sub>3</sub>CH<sub>2</sub>OH CH<sub>3</sub>CH<sub>2</sub>CH<sub>3</sub> H<sub>3</sub>C-O-CH<sub>3</sub> CH<sub>3</sub>CH<sub>2</sub>NH<sub>2</sub>
I II III IV
A)IV < III < II < I
B)II < III < IV < I
C)I < IV < III < II
D)II < III < I < IV
Q3) Which of the following is most likely to have the highest viscosity at 25°C?
A)C<sub>4</sub>H<sub>10</sub>
B)HOCH<sub>2</sub>CH<sub>2</sub>OH
C)C<sub>8</sub>H<sub>18</sub>
D)C<sub>2</sub>H<sub>5</sub>NH<sub>2</sub>
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Page 12
Chapter 11: Solutions and Their Properties
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Sample Questions
Q1) Which arrow represents H<sub>solute-solvent</sub>?
A)arrow (a)
B)arrow (b)
C)arrow (c)
D)arrow (d)
Q2) A 0.51 m aqueous solution of an unknown solute has a boiling point elevation of 0.62°C.The boiling point elevation of a 0.51 m solution of a nonionizing molecular solute in water is 0.26°C.How many moles of particles are formed per mole of solute when the unknown solute is dissolved in water?
A)1)4
B)2)0
C)2)4
D)3)0
Q3) What is the expected freezing point of a 0.50 m solution of Li<sub>2</sub>SO<sub>4</sub> in water? K<sub>f</sub> for water is 1.86°C/m.
A)-0.93°C
B)-1.9°C
C)-2.8°C
D)-6.5°C
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Page 13
Chapter 12: Chemical Kinetics
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Sample Questions
Q1) The reaction below is first order in H<sub>2</sub> and second order in NO.What is the rate law for this reaction?
2 H<sub>2</sub>(g)+ 2 NO(g) N<sub>2</sub>(g)+ 2 H<sub>2</sub>O(g)
A)Rate = 2k[H<sub>2</sub>][NO]
B)Rate = k[H<sub>2</sub>][NO]<sup>2</sup>
C)Rate = k[H<sub>2</sub>]<sup>2</sup>[NO]<sup>2</sup>
D)Rate = 2k[H<sub>2</sub>]<sup>2</sup>[NO]<sup>2</sup>
Q2) For a particular first-order reaction,it takes 48 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s<sup>-1</sup>)for the reaction?
A)1)0 × 10<sup>-4</sup> s<sup>-1</sup>
B)4)8 × 10<sup>-4</sup> s<sup>-1</sup>
C)6)0 × 10<sup>-3</sup> s<sup>-1</sup>
D)2)9 × 10<sup>-2</sup> s<sup>-1</sup>
Q3) The decomposition of hydrogen peroxide occurs according to the equation 2 H<sub>2</sub>O<sub>2</sub>(aq) 2 H<sub>2</sub>O(l)+ O<sub>2</sub>(g)
A concentration-time study of this reaction produces a straight line when ln[H<sub>2</sub>O<sub>2</sub>] is plotted versus time.Therefore,this is a ________ order reaction.
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Page 14
Chapter 13: Chemical Equilibrium
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Sample Questions
Q1) At 25°C,a certain first order reaction has a rate constant equal to 1.00 × 10<sup>-3</sup> s<sup>-1</sup> and an equilibrium constant,K<sub>c</sub>,equal to 4.18.What is the rate constant for the reverse reaction?
A)2)39 × 10<sup>-4</sup> s<sup>-1</sup>
B)4)18 × 10<sup>-3</sup> s<sup>-1</sup>
C)2)39 × 10<sup>2</sup> s<sup>-1</sup>
D)4)18 × 10<sup>3</sup> s<sup>-1</sup>
Q2) The reaction CaCO<sub>3</sub>(s) CaO(s)+ O<sub>2</sub>(g)is endothermic 298 K.The effect of increasing the partial pressure of O<sub>2</sub> in the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO<sub>3</sub> once equilibrium is reestablished.
Q3) What is the best balanced chemical equation for the reaction?
A)A<sub>2</sub> + B A<sub>2</sub>B
B)A<sub>2</sub> + 2 B A<sub>2</sub>B<sub>2</sub>
C)A<sub>2</sub> + 2 B 2 AB
D)6 A<sub>2</sub> + 9 B 3 A<sub>2</sub> + 3B + 6 AB
Q4) A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.
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Page 15
Chapter 14: Aqueous Equilibria: Acids and Bases
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Sample Questions
Q1) Calculate the pH of a 0.100 M CH<sub>3</sub>NH<sub>3</sub>Cl solution.K<sub>b</sub> for methylamine,CH<sub>3</sub>NH<sub>2</sub>,is 3.7 × 10<sup>-4</sup>.
A)2)22
B)5)78
C)8)22
D)11.78
Q2) The number of waters of hydration in the hydrate proton H<sub>7</sub>O<sub>3</sub><sup>+</sup> is ________.
Q3) Benzoic acid (C<sub>6</sub>H<sub>5</sub>CO<sub>2</sub>H = HBz)solutions are sometimes used in experiments to determine the molarity of a basic solution of unknown concentration.What is the pH of a 0.100 M solution of benzoic acid if K<sub>a</sub> = 6.5 × 10<sup>-5</sup> and the equilibrium equation of interest is HBz(aq)+ H<sub>2</sub>O(l) H<sub>3</sub>O<sup>+</sup> + Bz<sup>-</sup>(aq)?
A)1)00
B)2)59
C)4)19
D)5)19
Q4) The pH of a 0.025 M KOH solution is ________.
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Chapter 15: Applications of Aqueous Equilibria
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Sample Questions
Q1) Calculate the K<sub>sp</sub> for silver sulfate if the solubility of Ag<sub>2</sub>SO<sub>4</sub> in pure water is 4.5 g/L.
A)3)0 × 10<sup>-6</sup>
B)1)2 × 10<sup>-5</sup>
C)2)1 × 10<sup>-4</sup>
D)4)2 × 10<sup>-4</sup>
Q2) What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K<sub>a</sub> = 6.76 × 10<sup>-4</sup> for HF.
A)1)74
B)5)75
C)8)25
D)12.26
Q3) 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) G = G° for a reaction
A)if Q = K.
B)if Q = 1.
C)at STP.
D)at the start of the reaction.
Q2) The sign (+ or -)of H is ________ and the sign (+ or -)of S is ________ for the evaporation of water.
Q3) Which of the following is zero at 25°C?
A) G°<sub>f</sub> for N<sub>2</sub>(g)
B) G°<sub>f</sub> for H<sub>2</sub>O (l)
C)S° for N<sub>2</sub> (g)
D)S° for H<sub>2</sub>O (l)
Q4) Which of the following gas molecules has the greatest standard molar entropy at 25°C?
A)C<sub>2</sub>H<sub>2</sub>
B)CH<sub>2</sub>CH<sub>2</sub>
C)CH<sub>3</sub>CH<sub>3</sub>
D)All have the same entropy.
Page 18
Q5) The entropy of water at 25° is ________ than the entropy of water at 35°C.
Q6) What is the entropy of 10 molecules in a system of 1000 boxes?
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Page 19
Chapter 17: Electrochemistry
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Sample Questions
Q1) The bright colors of anodized titanium are due to A)electrodeposition of organic dyes on the titanium surface. B)the formation of a titanium alloy with chromium and copper. C)iridescence involving the semitransparent outer layer of TiO<sub>2</sub>.
D)trapping of organic dye molecules in a spongy TiO<sub>2</sub> matrix.
Q2) What species is oxidized in the reaction: CuSO<sub>4</sub>(aq)+ Fe(s) FeSO<sub>4</sub>(aq)+ Cu(s)?
A)CuSO<sub>4</sub> (aq)
B)Fe (s)
C)FeSO<sub>4 </sub>(aq)
D)Cu (s)
Q3) Galvanized steel is steel coated with a layer of A)Fe<sub>2</sub>O<sub>3</sub>.
B)Mg.
C)Sn.
D)Zn.
Q4) A galvanic cell uses the reaction Mg(s)+ Pb<sup>2+</sup>(aq) Mg<sup>2+</sup>(aq)+ Pb(s). Mg(s) Mg<sup>2+</sup>(aq)+ 2 e<sup>- </sup>is the ________ half-reaction,which occurs at the ________.
Page 20
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Chapter 18: Hydrogen, oxygen, and Water
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Sample Questions
Q1) What group of elements is most likely to from ionic hydrides of the type MH<sub>2</sub>?
A)A
B)B
C)C
D)D
Q2) A 7.63-gram sample of hydrated magnesium sulfate MgSO<sub>4</sub> xH<sub>2</sub>O is heated until all of the water is driven off.If 3.72 grams of anhydrous MgSO<sub>4</sub> is obtained,how many water molecules combine with each formula unit of magnesium sulfate in the hydrate?
A)5
B)6
C)7 D)8
Q3) The strongest homonuclear single bond is
A)H-H
B)C-C
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Chapter 19: The Main-Group Elements
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Sample Questions
Q1) The strongest reducing agent in the group 3A is
A)B)
B)Al.
C)Ga.
D)Tl.
Q2) Which one of the following has a two-dimensional layer structure?
A)silica,SiO<sub>2</sub>
B)zircon,ZrSiO<sub>4</sub>
C)talc,Mg<sub>3</sub>(OH)<sub>2</sub>(Si<sub>4</sub>O<sub>10</sub>)
D)tremolite
asbestos,Ca<sub>2</sub>Mg<sub>5</sub>(Si<sub>4</sub>O<sub>11</sub>)(OH)<sub>2 </sub>
Q3) Which of the following elements forms the most ionic binary hydride?
A)K
B)Mg
C)S
D)Cl
Q4) In the reaction below,________ is the oxidizing agent and ________ is the reducing agent.
N<sub>2</sub>H<sub>4</sub>(l)+ N<sub>2</sub>O<sub>4</sub>(l) 3 N<sub>2</sub>(g)+ 4 H<sub>2</sub>O(g)
Page 22
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Chapter 20: Transition Elements and Coordination Chemistry
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Sample Questions
Q1) Which of the following complexes has five unpaired electrons?
A)[Mn(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup>
B)[Mn(CN)<sub>6</sub>]<sup>3-</sup>
C)CrCl<sub>3</sub>(H<sub>2</sub>O)<sub>3</sub>
D)[Ag(NH<sub>3</sub>)<sub>2</sub>]<sup>+</sup>
Q2) Which chromium species exists only under acidic conditions?
A)Cr(OH)<sub>2</sub>
B)Cr(OH)<sub>4</sub><sup>-</sup>
C)CrO<sub>4</sub><sup>2-</sup>
D)Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup>
Q3) Which ion would you expect to have the largest crystal field splitting ?
A)[Fe(CN)<sub>6</sub>]<sup>4-</sup>
B)[Fe(CN)<sub>6</sub>]<sup>3-</sup>
C)[Fe(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup>
D)[Fe(H<sub>2</sub>O)<sub>6</sub>]<sup>3+</sup>
Q4) [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.
Q6) Copper has the anomalous short-hand electron configuration ________. Page 23
Q5) The small sizes of third transition series atoms is referred to as the ________ contraction.
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Page 24
Chapter 21: Metals and Solid-State Materials
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Sample Questions
Q1) Which substance is a good semiconductor?
A)diamond
B)germanium
C)gold
D)phosphorus
Q2) Which of these elements is likely to be found in nature as an oxide?
A)element A
B)element B
C)element C
D)element D
Q3) How would one classify copper mixed with tin?
A)conductor
B)n-type semiconductor
C)p-type semiconductor
D)insulator
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
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Chapter 22: Nuclear Chemistry
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Sample Questions
Q1) The effects of ionizing radiation depend on
A)length of exposure to radiation.
B)location of source (internal or external).
C)type and energy of radiation.
D)All of these
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 sum of the masses of the protons and neutrons in a given nucleus minus the mass of that nucleus is always
A)negative.
B)positive.
C)temperature dependent.
D)zero.
Q4) Units used for measuring radiation include the becquerel,the curie,the gray,and the sievert,which have the abbreviations ________,________,________,and ________,respectively.
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Chapter 23: Organic and Biological Chemistry
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285 Verified Questions
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Sample Questions
Q1) Organic molecules containing only carbon and hydrogen and having only single bonds are called ________ hydrocarbons,or ________.
Q2) None of the listed compounds contains a ring.Which has at least one singly-bonded carbon atom?
A)C<sub>2</sub>H<sub>6</sub>
B)C<sub>3</sub>H<sub>4</sub>
C)C<sub>4</sub>H<sub>8</sub>
D)All of these
Q3) Name the product obtained from the addition of bromine to 3-methyl-1-butene.
A)1,1-dibromobutane
B)1,2-dibromo-3-methylbutane
C)1,2-dibromopentane
D)trans-1,2-dibromobutene
Q4) In organic molecules the molecular geometry exhibited by carbon is ________ when carbon is bonded to four atoms by four single bonds,________ when carbon is bonded to three atoms by one double bond and two single bonds,and ________ when carbon is bonded to two atoms by one triple bond and one single bond.
Q5) The amide bonds that form when two or more amino acids link together are called ________ bonds.
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