General Chemistry I Review Questions - 2610 Verified Questions

General Chemistry I Review Questions

Course Introduction

General Chemistry I is an introductory course that explores the fundamental principles of chemistry, including atomic structure, periodic properties, chemical bonding, stoichiometry, chemical reactions, and the properties of gases, liquids, and solids. The course emphasizes the development of problem-solving skills and the application of chemical concepts to real-world situations. Students will engage with laboratory experiments to reinforce theoretical knowledge and gain hands-on experience with basic chemical techniques, data analysis, and safety protocols. This foundational course prepares students for more advanced studies in chemistry and related scientific disciplines.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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24 Chapters

2610 Verified Questions

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Page 2

Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) What length of a cylindrical piece of tungsten wire having a radius of 2.11 mm has a mass of 66.6 g? The density of tungsten is 19.25 g/cm³.

A)2.47× 10^-3 m

B)1.79 × 10² m

C)2.47 × 10^-1 m

D)4.04 × 10^-2 m

E)4.04 × 10^-4 m

Answer: C

Q2) A sample that cannot be separated into two or more substances by physical means is

A)a heterogeneous mixture.

B)a compound.

C)either a compound or an element.

D)an element.

E)a homogeneous mixture.

Answer: C

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) What is the subscript of potassium in the formula for potassium carbonate? A)2 B)5 C)3

D)4

E)1

Answer: A

Q2) The correct name for FeO is

A)iron(I)oxide.

B)iron oxide.

C)iron monoxide.

D)iron(II)oxide.

E)iron(III)oxide.

Answer: D

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Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) An organic compound that has the empirical formula CHO has a molecular mass of 174 amu.Its molecular formula is

A)C₇H₇O₇.

B)C₄H₄O₄.

C)C₂H₂O₂.

D)C₆H₆O₆.

E)C₁₀H₁₀O₁₀.

Answer: D

Q2) What is the mass in grams of one propene,C₃H₆,molecule?

A)6.99× 10^-23 g

B)2.53 × 10²⁵ g

C)44.0 g

D)42.0 g

E)1.99 × 10^-23 g

Answer: A

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) What is the reduction half-reaction for the reaction between iron(II)sulfate and potassium permanganate in a sulfuric acid solution?

5Fe²⁺(aq)+ MnO₄^-(aq)+ 8H⁺(aq) 5Fe³⁺(aq)+ Mn²⁺(aq)+ 4H₂O(l)

A)MnO₄^-(aq)+ 3e^- Mn²⁺(aq)+ 4H₂O(l)

B)MnO₄^-(aq)+ 8H⁺(aq)+ 5e^- Mn²⁺(aq)+ 4H₂O(l)

C)5Fe²⁺(aq) 5Fe³⁺(aq)+ 5e^- D)Fe²⁺(aq)+ 2e^- Fe(s)

E)MnO₄^-(aq)+ 5e^- Mn²⁺(aq)+ SO₄^2-(aq)

Q2) To dilute 1.00 L of a 0.600 M to 0.100 M,the final volume must be A)60 L.

B)0.7 L.

C)1/6 the original volume.

D)More information is needed to answer this question.

E)6 times the original volume.

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Chapter 5: The Gaseous State

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Sample Questions

Q1) 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.

Q2) A flexible vessel contains 43 L of gas where the pressure is 1.3 atm.What will the volume be when the pressure is 0.61 atm,the temperature remaining constant?

A)0.011 L

B)20 L

C)43 L

D)0.044 L

E)92 L

Q3) At STP,as the molar mass of the molecules that make up a pure gas increases,the

A)root mean square speed of the molecules increases.

B)root mean square speed of the molecules decreases.

C)root mean square speed of the molecules remains constant.

D)root mean square speed increases to a maximum,then decreases.

E)none of the above.

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Page 7

Chapter 6: Thermochemistry

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Sample Questions

Q1) Which of the following processes will result in the lowest final temperature of the metal-water mixture at equilibrium?

A)the addition of 100 g of silver (s = 0.237 J/(g °C))at 95°C to 100 mL of water at 25°C in an insulated container

B)the addition of 100 g of cobalt (s = 0.418 J/(g °C))at 95°C to 100 mL of water at 25°C in an insulated container

C)the addition of 100 g of chromium (s = 0.447 J/(g °C))at 95°C to 100 mL of water at 25°C in an insulated container

D)the addition of 100 g of copper (s = 0.385 J/(g °C))at 95°C to 100 mL of water at 25°C in an insulated container

E)the addition of 100 g of gold (s = 0.129 J/(g °C))at 95°C to 100 mL of water at 25°C in an insulated container

Q2) Which of the following is not a fuel-oxidizer mixture used in rockets?

A)kerosene-oxygen

B)hydrogen-oxygen

C)octane-oxygen

D)aluminum-ammonium perchlorate

E)hydrazine-dinitrogen tetroxide

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Page 8

Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) What is the wavelength of an electron traveling at of 3.74% the speed of light? (m_e=9.109×10^-31 kg,c=3.00×10⁸ m/s,h=6.63×10^-34 J·s)

A)1.54×10¹⁰ m

B)2.43×10^-12 m

C)6.49×10^-11 m

D)1.54×10¹² m

E)6.49×10^-13 m

Q2) What is the wavelength of photons that have molar energy of 515 kJ/mol? (c = 3.00 × 10⁸ m/s,h = 6.63 × 10^-34 J · s,N_A = 6.02 × 10²³ mol^-1)

A)1.29 × 10⁶nm

B)8.55 × 10^-10nm

C)233 nm

D)3.86 × 10^-22nm

E)2.33 × 10⁵nm

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9

Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) The change in energy for which of the following processes corresponds to the electron affinity of bromine?

A)Br₂(g) 2Br(g)

B)Br(g)+ e^- Br^-(g)

C)Br⁺(g)+ Br^-(g) Br₂(l)

D)Br(g) Br⁺(g)+ e^-

E)Br^-(g) Br(g)+ e^-

Q2) In which of the series of elements listed below would the elements have most nearly the same atomic radius?

A)Na,K,Rb,Cs

B)F,Cl,Br,I

C)Na,Mg,Al,Si

D)Sc,Ti,V,Cr

E)B,Si,As,Te

Q3) The elements that are filling the 5f subshell are called

A)alkali metals.

B)transition elements.

C)lanthanides.

D)actinides.

E)main-group elements.

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Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) During the formation of a chemical bond between two hydrogen atoms,which of the following statements is always true?

A)Energy is released during the formation of the bond.

B)A polar covalent bond is formed.

C)Electrons always are between the nuclei of the atoms.

D)One of the hydrogen atoms is ionized.

E)Resonance stabilizes the bond.

Q2) Which of the following species represents an exception to the octet rule?

A)SiO₂

B)HBr

C)SF₄

D)PCl₃

E)CO₂

Q3) What is the total number of valence electrons in the monohydrogen phosphate ion,HPO₄^2-?

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Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) Which molecule or ion does not have a tetrahedral molecular geometry?

A)BF₄^-

B)NF₄⁺

C)GeF₄

D)XeF₄

E)BeF₄^2-

Q2) Which of the following characteristics does not apply to PF₃?

A)has three bonds

B)contains polar bonds

C)polar molecule

D)one lone pair of electrons on phosphorus

E)trigonal planar

Q3) Which molecule or ion is nonlinear?

A)CO₂

B)NF₂^-

C)OCN^-

D)NO₂⁺

E)HCCH

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) Which of the following is a molecular solid?

A)carborundum,SiC

B)quartz

C)glass

D)hydrogen chloride

E)potassium

Q2) Which of the following involves a change in temperature during the phase transition?

A)condensation of water

B)liquifaction of ammonia

C)fusion of ethanol

D)all of the above

E)none of the above

Q3) Which of the following pure substances has the highest normal melting point?

A)NO₂

B)SiO₂

C)CO₂

D)P₄O₁₀

E)N₂O₅

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Page 13

Chapter 12: Solutions

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Sample Questions

Q1) The fact that the boiling point of a pure solvent is lower than the boiling point of a solution of the same solvent is a direct consequence of the A)freezing-point depression of the solution.

B)vapor pressure of the solution being higher than the vapor pressure of the pure solvent.

C)osmotic pressure of the solvent being lower than the osmotic pressure of the solution. D)vapor pressure of the solution being lower than the vapor pressure of the pure solvent. E)osmotic pressure of the solvent being higher than the osmotic pressure of the solution.

Q2) What is the molality of a solution that contains 9.16 g of glucose,C₆H₁₂O₆,in 228.5 g of water?

A)0.223 m

B)0.0509 m

C)0.00399 m

D)0.0116 m

E)0.0401 m

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Chapter 13: Rates of Reaction

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Sample Questions

Q1) One mechanism for the depletion of ozone in the stratosphere is proposed as follows:

Cl + O₃ ClO + O₂

ClO + O Cl + O₂<sub>

</sub>Identify any catalysts and intermediates in the reaction.

A)Cl is a catalyst,there are no intermediates

B)O is an intermediate,ClO is a catalyst

C)O₂ is a catalyst,O is an intermediate

D)ClO is a catalyst,there are no intermediates

E)Cl is a catalyst,ClO is an intermediate

Q2) Which of the following statements is always true?

A)Exothermic reactions have lower activation energies than endothermic reactions.

B)The rate of a catalyzed reaction is independent of the concentration of the catalyst.

C)The rate for a reaction depends on the concentrations of all the reactants.

D)The rate constant is independent of the concentrations of the reacting species.

E)The rate law can be determined from the stoichiometric equation.

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) For which of the following values of the equilibrium constant does the reaction mixture contain mostly products?

A)10⁰

B)10¹

C)10⁹

D)10^-1

E)10^-9

Q2) For a specific reaction,which of the following statements can be made about the equilibrium constant?

A)It can be changed by the addition of a catalyst.

B)It increases when the concentration of one of the products is increased.

C)It increases when the concentration of one of the reactants is increased.

D)It always remains the same.

E)It changes with changes in the temperature.

Q3) Which of the following represents a dynamic equilibrium?

A)a stoppered flask half full of water

B)a coin spinning in mid-air

C)two people of equal mass balanced on the ends of a seesaw

D)an open pan of boiling water

E)an object traveling at a constant speed

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Chapter 15: Acids and Bases

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Sample Questions

Q1) What is the hydronium-ion concentration in a solution formed by combining 450 mL of 0.10 M NaOH with 150 mL of 0.30 M HCl?

NaOH(aq)+ HCl(aq) NaCl(aq)+ H₂O(l)

A)0.045 M

B)1.7 × 10^-13 M

C)1.0 × 10^-7 M

D)0.30 M

E)0.10 M

Q2) The acid strength decreases in the series HBr > HSO₄^- >

CH₃COOH > HCN > HCO₃^-.Which of the following is the strongest base?

A)SO₄^2-

B)CO₃^2-

C)CH₃COO^-

D)Br^-

E)CN^-

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Which of the following solutions will not yield an effective NaH₂PO₄/Na₂HPO₄ buffer?

A)2.0 M NaH₂PO₄ + 1.0 M NaOH

B)1.0 M NaH₂PO₄ + 1.0 M Na₂HPO₄

C)1.0 M H₃PO₄ + 1.0 M Na₃PO₄

D)2.0 M Na₂HPO₄ + 1.0 M HCl

E)1.0 M H₃PO₄ + 1.0 M NaH₂PO₄

Q2) Which of the following would be the best mole ratio of conjugate acid to conjugate base for a large buffer capacity?

A)100:1

B)1:1

C)1:100

D)1:10

E)10:1

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18

Chapter 17: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) Which of the following solutions should be added to a solution containing both copper(II)ions and silver(I)ions in order to precipitate only one of the ions?

A)HCl(aq)

B)H₂S(aq)

C)HNO₃(aq)

D)H₂S(aq)+ HCl(aq)

E)H₂S(aq)+ HNO₃(aq)

Q2) What is the molar solubility of lead(II)sulfate at 25°C? The solubility product constant for lead(II)sulfate is 1.7 × 10^-8 at 25°C.

A)1.7 × 10^-8 M

B)5.7 × 10^-3 M

C)8.5 × 10^-9 M

D)1.6 × 10^-3 M

E)1.3 × 10^-4 M

Q3) What is the solubility product expression for Pb(IO₃)₄?

A)K_sp = [Pb⁴⁺][4IO₃^-]⁴

B)K_sp = [Pb⁴⁺][IO₃^-]

C)K_sp = [Pb][IO₃]⁴

D)K_sp = [Pb⁴⁺][IO₃^-]⁴

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Page 19

Chapter 18: Thermodynamics and Equilibrium

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Sample Questions

Q1) The enthalpy of vaporization ( H°_vap)of benzene is 30.7 kJ/mol at its normal boiling point of 353.3 K.What is S°_vap at this temperature?

A)86.9 J/(mol·K)

B)0.087 J/(mol·K)

C)11.5 J/(mol·K)

D)0.0115 J/(mol·K)

E)383 J/(mol·K)

Q2) From these two reactions at 298 K, V₂O₃(s)+ 3CO(g) 2V(s)+ 3CO₂(g); H° = 369.8 kJ; S° = 8.3 J/K

V₂O₅(s)+ 2CO(g) V₂O₃(s)+ 2CO₂(g); H° = -234.2 kJ; S° = 0.2 J/K

Calculate G° for the following at 298 K: 2V(s)+ 5CO₂(g) V₂O₅(s)+ 5CO(g)

A)+133.1 kJ

B)+601.6 kJ

C)-601.6 kJ

D)-133.1 kJ

E)+1.6 kJ

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Page 20

Chapter 19: Electrochemistry

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Sample Questions

Q1) What is the equilibrium constant (K)at 25°C for the following cell reaction?

Sn(s)+ Pb²⁺(aq) Sn²⁺ (aq)+ Pb(s); E°_cell = 0.014 V

A)0.014

Q2) When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for Rb⁺(aq)?

Rb(s)+ Sr²⁺(aq) Rb⁺(aq)+ Sr(s)

A)5

B)4

C)1 D)3 E)2

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21

Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) Relative to the sum of the masses of its constituent nucleons (neutrons + protons),the mass of a nucleus is

A)always greater.

B)sometimes the same and sometimes smaller.

C)always smaller.

D)always the same.

E)sometimes greater and sometimes smaller.

Q2) Consider a certain type of nucleus that has a rate constant of 2.43 × 10^-2 min^-1.Calculate the time required for the sample to decay to one-fourth of its initial value.

A)28.5 min

B)35.6 min

C)0.0486 min

D)57.0 min

E)2.43 min

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22

Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) What is the principal source of commercial helium?

A)Certain natural gas wells.

B)Fractional distillation of air.

C)It is a byproduct of commercial fusion research.

D)It is a byproduct of commercial fission reactors.

E)The mineral cleveite,a uranium ore.

Q2) Which of the following compounds is not an allotrope of carbon?

A)diamond

B)All are allotropes of carbon.

C)methane

D)graphite

E)buckminsterfullerene

Q3) Which of the following is not a normal characteristic of a metal?

A)ability to form cations

B)low ionization energy

C)conductor of electricity

D)high electron affinity

E)malleability

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23

Chapter 22: The Transition Elements and Coordination Compounds

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Sample Questions

Q1) In which of these pairs of elements can both elements normally exhibit multiple oxidation states?

A)K and O

B)Cs and Cl

C)Mg and Se

D)Co and Cu

E)Sc and Al

Q2) The oxidation number of which of the following elements is often +2 but can be as great as +7?

A)manganese

B)cobalt

C)aluminum

D)bismuth

E)chromium

Q3) Fe has __________ that is(are)unpaired in its d orbitals.

A)3 electrons

B)4 electrons

C)1 electron

D)2 electrons

E)5 electrons

Page 24

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Chapter 23: Organic Chemistry

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Sample Questions

Q1) Which functional group does not contain an oxygen atom?

A)aldehyde

B)alkyne

C)alcohol

D)ester

E)ketone

Q2) What is the molecular geometry around each carbon atom in a saturated hydrocarbon?

A)tetrahedral

B)trigonal planar

C)trigonal bipyramidal

D)linear

E)bent

Q3) Which of the following reactions is a substitution reaction?

A)C₆H₆ + F₂ C₆H₅F + HF

B)CH₂=CH₂ + F₂

CH₂FCH₂F

C)CH₂=CH₂ + HF CH₃CH₂F

D)CH₂=CH₂ + H₂

CH₃CH₃

E)HC CH + 2F₂ CHF₂CHF₂

Page 25

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Chapter 24: Polymer Materials: Synthetic and Biological

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Sample Questions

Q1) Where in the cell does protein synthesis cell take place?

A)ribosome

B)nucleus

C)gene

D)chromosome

E)codon

Q2) Which of the following is the zwitterionic form of glycine (R = H)?

A)(^-NHCH₂CO₂H)

B)NH₂CHCO₂H⁺

C)(⁺NH₂CH₂CO₂^-)

D)(⁺NH₃CH₂CO₂^-)

E)(NH₂CH₂CO₂^-)

Q3) Which of the following is(are)not necessary for protein synthesis at the time and place where synthesis occurs?

A)ribosomes

B)DNA

C)mRNA

D)amino acids

E)tRNA

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Page 26