General Chemistry I Review Questions
Course Introduction
General Chemistry I introduces the foundational principles and concepts of chemistry, providing students with a comprehensive understanding of the structure of matter, atomic theory, chemical bonding, stoichiometry, states of matter, thermochemistry, and solutions. The course emphasizes the development of problem-solving skills and the application of theoretical knowledge to laboratory experiments. Students will explore the fundamental laws of chemical reactions, the behavior of gases, and the periodic properties of elements, preparing them for more advanced study in the chemical sciences and related fields.
Recommended Textbook Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder
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Page 2
Chapter 1: Basic Concepts of Chemistry
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Sample Questions
Q1) ________ energy is the energy associated with the separation of two electrical charges.
Answer: Electrostatic
Q2) Which one of the following statements is not a comparison of physical properties?
A) Potassium reacts with water more quickly than calcium reacts with water.
B) The electrical conductivity of aluminum is greater than copper.
C) The density of copper is less than the density of lead.
D) The solubility of NaCl in hot water is greater than the solubility in cold water.
E) The boiling point of water is greater than the boiling point of ethanol.
Answer: A
Q3) A mass of 10 g of table salt dissolves in water to form a(n)________ mixture (i.e.,a mixture that is uniform throughout).
Answer: homogeneous
Q4) Properties,such as color and density,which can be observed or measured without changing the composition of a substance are called ________ properties.
Answer: physical
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Page 3
Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry
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Sample Questions
Q1) Convert 0.440 ng to milligrams and express the answer in scientific notation using the correct number of significant figures.
A) 4.40 \(\times\) 10<sup>-5</sup> mg
B) 4.40 \(\times\) 10<sup>-7</sup> mg
C) 4.4 \(\times\) 10<sup>-7</sup> mg
D) 0.440 \(\times\) 10<sup>-8</sup> mg
E) 0.440 \(\times\) 10<sup>-7</sup> mg
Answer: B
Q2) What is the difference between the accuracy of measurements and the precision of measurements?
Answer: Accuracy is an indicator of how close a measurement,or the average of a set of measurements,is to the correct value.Precision is an indicator of how close two measurements are to each other,or how much numerical spread is present in a set of measurements.
Q3) Assuming the density of water is 1.00 g/cm<sup>3</sup>,the mass of 1.0 cubic meter (m<sup>3</sup>) of water is ________ grams.
Answer: 1.0 \(\times\) 10<sup>6</sup>
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Page 4
Chapter 3: Atoms, molecules, and Ions
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Sample Questions
Q1) If 1.00 g of an unknown molecular compound contains 8.35 \(\times\) 10<sup>21</sup> molecules,what is its molar mass?
A) 44.0 g/mol
B) 66.4 g/mol
C) 72.1 g/mol
D) 98.1 g/mol
E) 132 g/mol
Answer: C
Q2) What is the correct formula for calcium nitrate?
A) CaN
B) Ca<sub>3</sub>N<sub>2</sub>
C) CaNO<sub>2</sub>
D) Ca<sub>3</sub>(NO<sub>3</sub>)<sub>2</sub>
E) Ca(NO<sub>3</sub>)<sub>2</sub>
Answer: E
Q3) Millikan's oil drop experiment determined the charge of the ________.
Answer: electron
Q4) In reactions,metals generally lose electrons to become ________,and nonmetals gain electrons to become anions.
Answer: cations
Page 5
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Chapter 4: Chemical Reactions
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Q1) Nitric acid is the product of the reaction of ____ and H<sub>2</sub>O.
A) SO<sub>3</sub>
B) NO<sub>2</sub>
C) N<sub>2</sub>
D) NH<sub>3</sub>
E) N<sub>3</sub><sup>-</sup>
Q2) Which one of the following compounds is a nonelectrolyte when dissolved in water?
A) HCl
B) CaCl<sub>2</sub>
C) CCl<sub>4</sub>
D) Cu(NO<sub>3</sub>)<sub>2</sub>
E) NaCH<sub>3</sub>CO<sub>2</sub>
Q3) Metal oxides react with water to produce ____.
A) bases
B) hydrogen gas
C) oxygen gas
D) acids
E) hydronium ions
Q4) A(n)________ agent gains electrons in an oxidation-reduction reaction.
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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions
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Q1) What volume of 0.464 M Na<sub>2</sub>CO<sub>3</sub> solution contains 74.7 g of Na<sub>2</sub>CO<sub>3</sub>?
A) 0.327 L
B) 1.71 \(\times\) 10<sup>4</sup> L
C) 1.52 L
D) 3.67 \(\times\) 10<sup>3</sup> L
E) 0.658 L
Q2) Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows:
Cu<sub>2</sub>S(s)+ O<sub>2</sub>(g)\(\to\) 2Cu(s)+ SO<sub>2</sub>(g)
If the reaction of 0.630 kg of copper(I)sulfide with excess oxygen produces 0.190 kg of copper metal,what is the percent yield?
A) 75.5 %
B) 39.9 %
C) 30.2 %
D) 151 %
E) 37.8 %
Q3) The reaction of 5.07 g N<sub>2</sub> with 0.722 g H<sub>2</sub> produces 1.27 g NH<sub>3</sub>.The percent yield of this reaction is ________.
Page 7
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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions
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Sample Questions
Q1) Calculate \(\Delta\)U of a gas for a process in which the gas absorbs 19 J of heat and does 49 J of work by expanding.
A) 30 J
B) 68 J
C) -68 J
D) 0,because \(\Delta\)U is a state function
E) -30 J
Q2) Which of the following statements is/are CORRECT?
1)A system is defined as an object or collection of objects being studied.
2)Surroundings are defined as the entire universe,including the system.
3)In an endothermic reaction,heat is transferred from the system to the surroundings.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3
Q3) Why are you at greater risk from being burned by steam at 100 S1U1P1\(\circ\)S1S1P0C than from liquid water at the same temperature?
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Chapter 7: The Structure of Atoms
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Q1) Which type of experiment demonstrates that an electron has the properties of a wave?
A) nuclear fission
B) electron diffraction
C) light emission from atomic gases
D) mass spectroscopy
E) photoelectric effect
Q2) What is the binding energy of an electron in a photosensitive metal (in kJ/mol)if the longest wavelength of light that can eject electrons from the metal is 205 nm?
A) 279 kJ/mol
B) 584 kJ/mol
C) 792 kJ/mol
D) 1.71 \(\times\) 10<sup>19</sup> kJ/mol
E) 5.84 \(\times\) 10<sup>-20</sup> kJ/mol
Q3) The difference in energy between adjacent energy levels in an atom _____ as n increases.
Q4) What evidence does the photoelectric effect provide that photons are not only waves?
Q5) A point in a standing wave that has zero amplitude is called a(n)________.
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Chapter 8: The Structure of Atoms and Periodic Trends
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Q1) If the ground state electron configuration of an element is [Ar]3d<sup>10</sup>4s<sup>2</sup>4p<sup>5</sup>,what is the typical charge on the monatomic anion of the element?
A) 4+
B) 2+
C) 1-
D) 2-
E) 3-
Q2) An atom of which of the following elements has the smallest ionization energy?
A) Cl
B) P
C) Si
D) Na
E) S
Q3) An atom of which of the following elements has the largest atomic radius?
A) Se
B) Te
C) S
D) Po
E) O
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Chapter 9: Bonding and Molecular Structure
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Q1) When both of the electrons in a molecular bond originate from the same atom,the bond is called a(n)
A) sigma bond.
B) coordinate covalent bond.
C) pi bond.
D) metallic bond.
E) ionic bond.
Q2) Which of the following bonds would be the most polar?
A) N-N
B) N-P
C) N-C
D) N-As
E) N-Ge
Q3) What is the formal charge on carbon in CH<sub>2</sub>Cl<sub>2</sub>?
A) +2
B) +1
C) 0
D) -1
E) -2
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Page 11
Chapter 10: Bonding and Molecular Structure: Orbital
Hybridization and Molecular Orbitals
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Q1) Which diatomic molecule or ion has valence electron molecular orbital configuration provided below?
[core electrons](\(\sigma\)<sub>2s</sub>)<sup>2</sup>(\(\sigma\)*<sub>2s</sub>)<sup> 2</sup>(\(\sigma\)<sub>2p</sub>)<sup>2</sup>(\(\pi\)<sub>2p</sub>)<sup>4</sup >(\(\pi\)*<sub>2p</sub>)<sup>1</sup>
A) C<sub>2</sub>
B) O<sub>2</sub><sup>+</sup>
C) O<sub>2</sub><sup>+</sup>.
D) Ne<sub>2</sub>
E) H<sub>2</sub>
Q2) To form a molecule with a linear electron pair geometry,what set of pure atomic orbitals must be mixed?
A) one s and one p
B) one s and two p
C) one s and three p
D) two s and one p
E) zero s and three p
Q3) Which theory,valence bond or molecule orbital,correctly predicts the existence of paramagnetic molecules?
Page 12
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Chapter 11: Gases and Their Properties
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Sample Questions
Q1) A sample of helium gas occupies 14.7 L at 23°C and 0.956 atm.What volume will it occupy at 40°C and 1.20 atm?
A) 19.5 L
B) 20.4 L
C) 11.1 L
D) 12.4 L
E) 14.9 L
Q2) Gaseous chlorine is held in two separate containers at identical temperature and pressure.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.33 L.How many moles of the gas are in container 2?
A) 12.0 mol
B) 20.3 mol
C) 0.452 mol
D) 3.74 mol
E) none of these
Q3) The gas constant,R,expressed in SI units has a value of 8.314.The units of the constant are ________.
Q4) Robert Boyle observed that the volume of a fixed amount of gas is inversely proportional to its ________.
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Chapter 12: Intermolecular Forces and Liquids
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Q1) Which of the following has the \(\underline{\text{ greatest }}\)boiling point?
A) Ne
B) N<sub>2</sub>
C) Cl<sub>2</sub>
D) I<sub>2</sub>
E) F<sub>2</sub>
Q2) When a water molecule forms a hydrogen bond with another water molecule,which atoms are involved in the interaction?
A) a hydrogen from one molecule and a hydrogen from the other molecule
B) a hydrogen from one molecule and an oxygen from the other molecule
C) an oxygen from one molecule and an oxygen from the other molecule
D) an oxygen and a hydrogen from the same molecule
E) two hydrogens from one molecule and one hydrogen from the other molecule
Q3) What is the \(\underline{\text{ strongest }}\) intermolecular force present in solid NH<sub>3</sub>?
A) London dispersion
B) hydrogen-bonding
C) dipole-dipole
D) ion-dipole
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Page 14
Chapter 13: The Chemistry of Solids
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Sample Questions
Q1) Gold crystallizes in a face-centered cubic lattice with an edge length of 407.8 pm.What is the density of gold?
A) 1.21 g/cm<sup>3</sup>
B) 4.82 g/cm<sup>3</sup>
C) 2.41 g/cm<sup>3</sup>
D) 9.65 g/cm<sup>3</sup>
E) 19.3 g/cm<sup>3</sup>
Q2) Which of the following might be used as a dopant in a silicon host to create a p-type semiconductor?
A) Al
B) P
C) As
D) S
E) Ge
Q3) A salt with a 1:1 ratio of anions to cations may pack in a face-centered cubic unit cell with the anions at the lattice points and the cations occupying one-half of the ________ holes.Zinc sulfide is an example of this structure.
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Chapter 14: Solutions and Their Behavior
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Q1) What is the mole fraction of urea,CH<sub>4</sub>N<sub>2</sub>O,in an aqueous solution that is 54% urea by mass?
A) 0.26
B) 0.74
C) 0.54
D) 0.37
E) 0.80
Q2) What mass of Zn(NO<sub>3</sub>)<sub>2</sub> must be diluted to a mass of 1.00 kg with H<sub>2</sub>O to prepare 97 ppm Zn<sup>2+</sup>(aq)?
A) 7.8 \(\times\) 10<sup>-6</sup> g
B) 7.8 \(\times\) 10<sup>-3</sup> g
C) 3.3 \(\times\) 10<sup>-2</sup> g
D) 1.3 \(\times\) 10<sup>-1</sup> g
E) 2.8 \(\times\) 10<sup>-1</sup> g
Q3) Henry's law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid.This law holds correct for gases such as nitrogen and oxygen.However,Henry's law does not hold correct for hydrogen chloride gas.Why?
Q4) ________ are colloidal dispersions of one liquid in another liquid.
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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions
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Q1) Molecules must overcome a barrier called the activation energy if they are to react.The highest energy point reached during the progress of a reaction is called the
A) rate determining step
B) transition state
C) half-life
D) elementary step
E) intermediate state
Q2) Calculate the activation energy,E<sub>a</sub>,for N<sub>2</sub>O<sub>5</sub>(g)\(\to\) 2 NO<sub>2</sub>(g)+ 1/2 O<sub>2</sub>(g)
Given k (at 45.0 S1U1P1\(\circ\)S1S1P0C)= 5.79 \(\times\) 10<sup>-4</sup> s<sup>-1</sup> and k (at 60.0 S1U1P1\(\circ\)S1S1P0C)= 3.83 \(\times\) 10<sup>-3</sup> s<sup>-1</sup>.(R = 8.314 J/K.mol)
A) 0.256 kJ/mol
B) 2.83 kJ/mol
C) 31.1 kJ/mol
D) 111 kJ/mol
E) 389 kJ/mol
Q3) Termolecular elementary steps are rare.Why?
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Q4) The pre-exponential,A,in the Arrhenius equation is called the ________ factor.
Chapter 16: Principles of Reactivity: Chemical Equilibria
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Q1) In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.
Q2) If the reaction quotient,Q,is equal to K in a gas phase reaction,then
A) the chemical system has reached equilibrium.
B) the temperature must be increased for the reaction to proceed in the forward direction.
C) the reaction will proceed in the forward direction until equilibrium is established. D) the reaction will proceed in the backward direction until equilibrium is established. E) the reaction will proceed in the direction that increases the number of gas phase particles.
Q3) If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.
Q4) The symbol Q is called the ________.
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Chapter 17: The Chemistry of Acids and Bases
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Q1) What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq)and 50.0 mL of 0.30 M NaOH(aq)at 25 S1U1P1\(\circ\)S1S1P0C? (K<sub>a</sub> of HF = 7.2 \(\times\) 10<sup>-4</sup>)
A) 1.98
B) 5.84
C) 8.16
D) 10.85
E) 12.02
Q2) What is the pOH of 0.067 M HI(aq)at 25 S1U1P1\(\circ\)S1S1P0C? (K<sub>w</sub> = 1.01 \(\times\) 10<sup>-14</sup>)?
A) 2.70
B) 12.83
C) 11.30
D) 15.17
E) 1.17
Q3) Which is the stronger Brønsted-Lowry acid,Fe(H<sub>2</sub>O)<sub>6</sub><sup>2+</sup> or Fe(H<sub>2</sub>O)<sub>6</sub><sup>3+</sup>? Explain.
Q4) When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.
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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria
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Q1) What is the solution pH when 0.10 mol of H<sup>+</sup> is added to a 2.0-liter buffered solution created from 0.45 M NH<sub>3</sub> (K<sub>b</sub> = 1.8 \(\times\) 10<sup>-5</sup>)and 0.26 M NH<sub>4</sub>F.
A) 8.07
B) 4.63
C) 9.37
D) 10.34
E) 4.85
Q2) A 25.00-mL sample of propionic acid,HC<sub>3</sub>H<sub>5</sub>O<sub>2</sub>,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?
A) 0.295 M
B) 0.125 M
C) 0.082 M
D) 0.143 M
E) 0.250 M
Q3) If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.
Page 20
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Chapter 19: Entropy and Free Energy
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Q1) Which of the following changes lead to a \(\underline{\text{ decrease }}\) in entropy?
A) the sublimation (vaporization)of dry ice (solid carbon dioxide)
B) sugar dissolving in coffee
C) evaporation of water from a lake
D) diffusion of perfume throughout a room
E) halving the volume of a gas
Q2) If a chemical reaction is exothermic,but not spontaneous,which of the following must be true?
A) (\(\Delta\)<sub>r</sub>G) > 0,\(\Delta\)<sub>r</sub>S > 0 and \(\Delta\)<sub>r</sub>H > 0
B) (\(\Delta\)<sub>r</sub>G) < 0,\(\Delta\)<sub>r</sub>S > 0 and \(\Delta\)<sub>r</sub>H > 0
C) (\(\Delta\)<sub>r</sub>G) > 0,\(\Delta\)<sub>r</sub>S < 0 and \(\Delta\)<sub>r</sub>H > 0
D) (\(\Delta\)<sub>r</sub>G) < 0,\(\Delta\)<sub>r</sub>S < 0 and \(\Delta\)<sub>r</sub>H < 0
E) (\(\Delta\)<sub>r</sub>G) > 0,\(\Delta\)<sub>r</sub>S < 0 and \(\Delta\)<sub>r</sub>H < 0
Q3) At what temperature (in kelvin units)is the entropy of a pure crystal 0.0 J/K.
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Chapter 20: Principles of Reactivity: Electron Transfer Reactions
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Q1) What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> for 160 min using a constant current of 15.0 A? Assume 100% current efficiency.(F = 96485 C/mol)
A) 0.431 g
B) 25.9 g
C) 232.8 g
D) 0.187 g
E) 38.8 g
Q2) Which of the following statements concerning a voltaic cell is/are correct?
1)Reduction occurs at the cathode.
2)A spontaneous reaction generates an electric current in a voltaic cell.
3)Without a salt bridge charge buildup will cause the cell reaction to stop.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
Q3) If electric current is passed through a solution of molten KBr,the product at the cathode is ________.
Page 22
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Chapter 21: Environmental Chemistry Earths
Environment,energy,and Sustainability
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Q1) Most hydrogen gas is produced industrially by
A) electrolysis.
B) solar energy.
C) steam reforming.
D) bacteria.
E) fuel cells.
Q2) Which of the following is not a greenhouse gas?
A) CO<sub>2</sub>
B) CH<sub>4</sub>
C) H<sub>2</sub>O
D) N<sub>2</sub>O
E) N<sub>2</sub>
Q3) Which of the following is not responsible for the formation and/or release of methane into the atmosphere?
A) aerobic bacteria
B) cows
C) landfills
D) mining
E) termites
Q4) Explain why the melting of Arctic sea ice will not raise the sea level.
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Chapter 22: The Chemistry of the Main Group Elements
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Q1) Oxides of the alkaline earth family form ____ upon reaction with water.
A) basic solutions
B) acidic solutions
C) alkaline earth hydrides
D) oxygen gas
E) hydrogen gas
Q2) Aluminum is resistant to corrosion because
A) the surface of aluminum is coated with unreactive AlN.
B) the surface of aluminum is coated with unreactive Al<sub>2</sub>O<sub>3</sub>.
C) aluminum is a noble metal.
D) aluminum has the greatest density of all naturally occurring metals.
E) aluminum has a large positive standard reduction potential.
Q3) Which one of the following elements would react with chlorine most rapidly?
A) Li
B) Na
C) K
D) Rb
E) Cs
Q4) Give two examples of the allotropes of elemental oxygen.
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Chapter 23: The Chemistry of the Transition Elements
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Q1) Which of the following salts would \(\underline{\text{ not }}\) be expected to have unpaired d-electrons?
A) NiCl<sub>2</sub>
B) CoCl<sub>2</sub>
C) MnCl<sub>2</sub>
D) TiCl<sub>3</sub>
E) ScCl<sub>3</sub>
Q2) As bound ligands,which of the following causes the largest splitting of d-orbitals?
A) phen
B) H<sub>2</sub>O
C) I<sup>-</sup>
D) CN<sup>-</sup>
E) C<sub>2</sub>O<sub>4</sub><sup>2-</sup>
Q3) One method of recovering metals from their ores involves aqueous solutions; a second method involves heat.The method involving heat is called ________.
Q4) The complex ion [NiCl<sub>4</sub>]<sup>2-</sup> is paramagnetic,but the complex ion [Ni(NH<sub>3</sub>)<sub>4</sub>]<sup>2+</sup> is diamagnetic.Why do the magnetic properties of these two nickel complexes differ?
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Chapter 24: Carbon: Not Just Another Element
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Q1) Name the following:
CH<sub>3</sub>-(CH<sub>2</sub>)<sub>5 </sub>-CH<sub>3</sub>
A) heptane
B) pentane
C) butane
D) octane
E) hexane
Q2) Formulas for derivatives of hydrocarbons may be written as R-X,where R is a hydrocarbon lacking a hydrogen atom and X is a functional group.Which of the following formulas represents a primary amine?
A) RNH<sub>2</sub>
B) RCONH<sub>2</sub>
C) R<sub>2</sub>NH
D) RCO<sub>2</sub>R'
E) R<sub>3</sub>N
Q3) Molecules with nonsuperimposable mirror images are termed chiral.Pairs of nonsuperimposable,mirror image molecules are called ________.
Q4) Cis-1,2-dichloroethylene and trans-1,2-dichloroethylene are examples of ________ isomers.
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Chapter 25: Biochemistry
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54 Verified Questions
54 Flashcards
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Sample Questions
Q1) Which of the following is not a polysaccharide?
A) glycogen
B) lactose
C) cellulose
D) amylose starch
E) amylopectin starch
Q2) Which of the following statements concerning enzyme chemistry is/are correct?
1)Enzymes are biological catalysts.
2)A reaction occurs when substrate binds the enzyme active site.
3)Enzymes catalyze multiple types of reactions.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
Q3) The amide linkages in a protein and also called ___ bonds.
Q4) A compound which contains both a positive and negative charge is called a ____.
Q5) The process by which a double stranded of DNA is copied is called ___.In the process,a ___ strand of DNA is produced from each single strand of the original double-stranded DNA.
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Chapter 26: Nuclear Chemistry
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Sample Questions
Q1) One means of enriching the percentage of uranium-235 for use as nuclear fuel is
A) liquid distillation
B) gaseous centrifugation
C) mass spectroscopy
D) gamma ray bombardment
E) ion chromatography
Q2) Explain the treatment named boron neutron capture therapy (BNCT).
Q3) What role do the cadmium control rods play in a fission reactor?
A) The rods control the rate of fission by absorbing neutrons.
B) The cadmium combines with spent uranium fuel to produce a non-radioactive product.
C) The rods focus the neutrons toward the center of the reactor.
D) The cadmium acts as a catalyst,enabling fission to occur at lower temperatures.
E) The rods move forward and backward,driving the pistons that turn the turbines.
Q4) A unit used to quantify biological damage is called the ________ or rem.
Q5) All isotopes of atomic number greater than ________ are unstable and radioactive.
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