Introductory Chemistry Question Bank
Course Introduction
Introductory Chemistry provides students with a foundational understanding of key chemical principles and concepts. Topics covered include the structure of atoms and molecules, the periodic table, chemical bonding, stoichiometry, basic thermodynamics, and chemical reactions. The course emphasizes practical problem-solving skills, laboratory techniques, and real-world applications of chemistry in everyday life and various scientific fields. It serves as a stepping stone for further studies in chemistry and related disciplines, making it suitable for students with little or no prior experience in the subject.
Recommended Textbook
Chemistry The Central Science 14th Edition by Theodore E. Brown
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24 Chapters
3674 Verified Questions
3674 Flashcards
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Page 2
Chapter 1: Introduction: Matter, energy, and Measurement
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163 Verified Questions
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Sample Questions
Q1) One edge of a cube is measured and found to be 13 cm.The volume of the cube in m<sup>3</sup> is ________.
A)2.2 × 10<sup>-3</sup>
B)2.2 × 10<sup>-6</sup>
C)2.2
D)2.2 × 10<sup>3</sup>
E)2.2 × 10<sup>6</sup>
Answer: A
Q2) How many significant figures should be retained in the result of the following calculation?
12.00000 × 0.9893 + 13.00335 × 0.0107
A)2
B)3
C)4
D)5
E)6
Answer: C
Q3) Gases do not have a fixed ________ as they are able to be ________.
Answer: volume,compressed
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3
Chapter 2: Atoms, molecules, and Ions
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249 Flashcards
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Sample Questions
Q1) The correct name for HIO<sub>2 </sub>is ________.
A)hypoiodic acid
B)hydriodic acid
C)periodous acid
D)iodous acid
E)periodic acid
Answer: D
Q2) The correct name for Na<sub>2</sub>O<sub>2</sub> is ________.
A)sodium oxide
B)sodium dioxide
C)disodium dioxide
D)sodium peroxide
E)disodium oxide
Answer: D
Q3) H<sub>2</sub>SeO<sub>4</sub> is called selenic acid.
A)True
B)False
Answer: True
Q4) The formula for potassium sulfide is ________.
Answer: K<sub>2</sub>S
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Chapter 3: Chemical Reactions and Reaction Stoichiometry
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Sample Questions
Q1) Gaseous neon has a density of 0.900 g/L at standard conditions.How many neon atoms are in 1.00 L of neon gas at standard conditions?
A)5.42 × 10<sup>23</sup>
B)1.35 × 10<sup>25</sup>
C)7.41 × 10<sup>-26</sup>
D)2.69 × 10<sup>22</sup>
E)6.02 × 10<sup>23</sup>
Answer: D
Q2) The formula weight of silver chromate (Ag<sub>2</sub>CrO<sub>4</sub>)is ________ amu.
A)159.87
B)223.87
C)331.73
D)339.86
E)175.87
Answer: C
Q3) A compound was found to contain 90.6% lead (Pb)and 9.4% oxygen.The empirical formula for this compound is ________.
Answer: Pb<sub>3</sub>O<sub>4</sub>
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Page 5
Chapter 4: Reactions in Aqueous Solution
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Sample Questions
Q1) Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.
A)0.175
B)4.37
C)0.525
D)0.350
E)0.874
Q2) ________ is an oxidation reaction.
A)Ice melting in a soft drink
B)Table salt dissolving in water for cooking vegetables
C)Rusting of iron
D)The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate
E)Neutralization of HCl by NaOH
Q3) If it took 49.33 mL of 0.2454 M KOH solution to neutralize 35.0 mL of arsenic acid (H<sub>3</sub>AsO<sub>4</sub>),what is the concentration (M)of the arsenic acid solution?
Q4) 325 mL of a 5.50 M phosphoric acid solution was prepared for laboratory.How many grams of phosphoric acid was in this solution.
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Chapter 5: Thermochemistry
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Sample Questions
Q1) Given the following reactions N<sub>2</sub> (g)+ O<sub>2</sub> (g) 2NO (g) H = +180.7 kJ
2NO( g)+ O<sub>2</sub> (g) 2NO<sub>2</sub> (g) H = -113.1 kJ
The enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen
2NO<sub>2</sub> (g) N<sub>2</sub> (g)+ 2O<sub>2</sub> (g) Is ________ kJ.
A)67.6
B)-67.6
C)293.8
D)-293.8
E)45.5
Q2) Renewable energy sources are essentially exhaustible.
A)True
B)False
Q3) Petroleum is a liquid that can be refined to produce fuels such as gasoline,diesel oil,and kerosene.
A)True
B)False
Q4) ________ is defined as the energy used to move an object against a force.
Page 7
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Chapter 6: Electronic Structure of Atoms
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Sample Questions
Q1) A mole of yellow photons of wavelength 527 nm has ________ kJ of energy.
A)165
B)227
C)4.56 × 10<sup>-46</sup>
D)6.05 × 10<sup>-3</sup>
E)2.74 × 10<sup>-19</sup>
Q2) The valence shell of the element X contains 2 electrons in a 5s subshell.Below that shell,element X has a partially filled 4d subshell.What type of element is X?
A)main group element
B)chalcogen
C)halogen
D)transition metal
E)alkali metal
Q3) The condensed electron configuration of argon,element 18,is ________.
A)[Ne]3s<sup>4</sup>
B)[Ar]3s<sup>2</sup>3p<sup>2</sup>
C)[Ne]3s<sup>2</sup>3p<sup>6</sup>
D)[He]2s<sup>4</sup>2p<sup>10</sup>
E)[He]3s<sup>4</sup>
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Page 8
Chapter 7: Periodic Properties of the Elements
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Sample Questions
Q1) Elements in the modern version of the periodic table are arranged in order of increasing ________.
A)oxidation number
B)atomic mass
C)average atomic mass
D)atomic number
E)number of isotopes
Q2) The element in the periodic table that looks like a metal,is a poor thermal conductor,and acts as an electrical semiconductor is ________.
A)Sn
B)B
C)As
D)Si
E)Ge
Q3) ________ is a unique element and does not truly belong to any family.
A)Nitrogen
B)Radium
C)Hydrogen
D)Uranium
E)Helium
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Chapter 8: Basic Concepts of Chemical Bonding
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Sample Questions
Q1) To convert from one resonance structure to another,________.
A)only atoms can be moved
B)electrons and atoms can both be moved
C)only electrons can be moved
D)neither electrons nor atoms can be moved
E)electrons must be added
Q2) In the Lewis structure of HCO<sub>3</sub><sup>-</sup>,the formal charge on H is ________,and the formal charge on C is ________.
A)-1, -1
B)0, 0
C)0, -1
D)+1, -1
E)-1, +1
Q3) The greater the lattice energy,the greater the charges on the participatory ions and the smaller their radii.
A)True
B)False
Q4) Polyatomic ions with an even number of electrons will follow the ________ rule.
Q5) Draw the Lewis structure of ICl<sub>2</sub><sup>+</sup>.
Q6) Which halogen,bromine or iodine,will form the more polar bond with phosphorus?
Page 10
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Chapter 9: Molecular Geometry and Bonding Theories
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Sample Questions
Q1) Electrons in ________ bonds remain localized between two atoms.Electrons in ________ bonds can become delocalized between more than two atoms.
A)pi, sigma
B)sigma, pi
C)pi, pi
D)sigma, sigma
E)ionic, sigma
Q2) A triatomic molecule cannot be linear if the hybridization of the central atoms is
A)sp
B)sp<sup>2</sup>
C)sp<sup>3</sup>
D)sp<sup>2</sup> or sp<sup>3</sup>
E)sp<sup>2</sup>d or sp<sup>3</sup>d<sup>2</sup>
Q3) Mixing one s atomic orbital and one p atomic orbital gives rise to ________.
A)three sp<sup>2</sup> hybrid orbitals
B)two sp<sup>2</sup> hybrid orbitals
C)two sp<sup>3</sup> hybrid orbitals
D)three sp hybrid orbitals
E)two sp hybrid orbitals
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Chapter 10: Gases
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Sample Questions
Q1) What is the density of nitrogen dioxide gas (g/L)contained in a 4.77 L pressure tank at 738.4 mm Hg and 45.0 °C?
A)1.71
B)1300
C)12.1
D)0.0169
E)8.17
Q2) Arrange the following gases in order of increasing average molecular speed at 25 °C. He,O<sub>2</sub>,CO<sub>2</sub>,N<sub>2</sub>
A)He < N<sub>2</sub> < O<sub>2</sub> < CO<sub>2</sub>
B)He < O<sub>2</sub> < N<sub>2</sub> < CO<sub>2</sub>
C)CO<sub>2</sub> < O<sub>2</sub> < N<sub>2</sub> < He
D)CO<sub>2</sub> < N<sub>2</sub> < O<sub>2</sub> < He
E)CO<sub>2</sub> < He < N<sub>2</sub> < O<sub>2</sub>
Q3) How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?
Q4) What volume (L)of HCl gas is required to react with an excess of sodium to generate 19.5 L of hydrogen gas at 1.31 atm and 51.0 °C?
Q5) What is the rms speed (m/s)of oxygen molecules at 36.0 °C?
Q6) Calculate the density of hydrogen gas (in g/L)at 43.0 °C and 700.0 torr.
Page 12
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Chapter 11: Liquids and Intermolecular Forces
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Sample Questions
Q1) What is the predominant intermolecular force in CH<sub>4</sub>?
A)London-dispersion forces
B)ion-dipole attraction
C)ionic bonding
D)dipole-dipole attraction
E)hydrogen bonding
Q2) The phase diagram of a substance is given above.The region that corresponds to the solid phase is ________.
A)w
B)x
C)y
D)z
E)x and y
Q3) Which one of the following exhibits dipole-dipole attraction between molecules?
A)NH<sub>3</sub>
B)CF<sub>4</sub>
C)C<sub>10</sub>H<sub>22</sub>
D)O<sub>2</sub>
E)SF<sub>6</sub>
Q4) The conversion of a solid to a liquid is called ________.
Page 13
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Chapter 12: Solids and Modern Materials
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Sample Questions
Q1) Molecular solids consist of atoms or molecules held together by ________.
A)dipole-dipole forces only
B)Metallic bonds only
C)London dispersion forces and hydrogen bonds only
D)hydrogen bonds only
E)dipole-dipole forces, London dispersion forces, and/or hydrogen bonds
Q2) An unknown metal crystallizes in a body-centered cubic unit cell.There are ________ atoms of the unknown metal per unit cell.
Q3) Define a body-centered cubic lattice.
Q4) An unknown metal crystallizes in a body-centered cubic structure with a unit cell edge length of 4.35 Å.The radius of the unknown atom is ________ Å.
A)1.88
B)3.77
C)2.18
D)8.70
E)4.35
Q5) An insulator does not conduct electricity.
A)True
B)False
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Chapter 13: Properties of Solutions
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160 Flashcards
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Sample Questions
Q1) Of the following,a 0.1 M aqueous solution of ________ will have the lowest freezing point.
A)NaCl
B)Al(NO<sub>3</sub>)<sub>3</sub>
C)K<sub>2</sub>CrO<sub>4</sub>
D)Na<sub>2</sub>SO<sub>4</sub>
E)sucrose
Q2) Pressure has an appreciable effect on the solubility of ________ in liquids.
A)gases
B)solids
C)liquids
D)salts
E)solids and liquids
Q3) A solution contains 11% by mass of sodium chloride.This means that ________.
A)there are 11 g of sodium chloride in in 1.0 mL of this solution
B)100 g of the solution contains 11 g of sodium chloride
C)100 mL of the solution contains 11 g of sodium chloride
D)the density of the solution is 11 g/mL
E)the molality of the solution is 11
Q4) What is the formula weight of iron(III)chloride hexahydrate?
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Chapter 14: Chemical Kinetics
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Sample Questions
Q1) Heterogeneous catalysts have different phases from reactants.
A)True
B)False
Q2) The rate of a second order reaction can depend on the concentrations of more than one reactant.
A)True
B)False
Q3) Which of the following is correct regarding the overall order of the reaction?
A)the overall order is found by subtracting the individual orders for ClO<sub>2</sub> and OH<sup>-</sup>, so it is 1 for this reaction
B)the overall order for this reaction is based on the individual order for OH<sup>-</sup>, so it is 1
C)the overall order is found by adding the individual orders for ClO<sub>2</sub> and OH<sup>-</sup>, so it is 3 for this reaction
D)the overall order for this reaction is based on the individual order for ClO<sub>2</sub>, so it is 2
E)the overall order cannot be determined
Q4) A unimolecular elementary reaction involves ________ reactant molecule(s).
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Page 16
Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of energy.
A)True
B)False
Q2) Which one of the following will change the value of an equilibrium constant?
A)changing temperature
B)adding other substances that do not react with any of the species involved in the equilibrium
C)varying the initial concentrations of reactants
D)varying the initial concentrations of products
E)changing the volume of the reaction vessel
Q3) If a reaction is endothermic,________ the reaction temperature results in an decrease in K.
Q4) Le Châtelier's principle states that if a system at equilibrium is disturbed,then more products are produced.
A)True
B)False
Q5) If a reaction is exothermic,________ the reaction temperature results in an increase in K.
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Chapter 16: Acid-Base Equilibria
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Sample Questions
Q1) A substance that is capable of acting as both an acid and as a base is ________. A)autosomal B)conjugated C)amphiprotic D)saturated E)miscible
Q2) An aqueous basic solution has a concentration of 0.050 M and K<sub>b</sub> is 4.4 × 10<sup>-4</sup>.What is the concentration of hydronium ion in this solution (M)?
A)2.2 × 10<sup>-13</sup>
B)2.2 × 10<sup>-12</sup>
C)2.9 × 10<sup>-13</sup>
D)0.050
E)4.5 × 10<sup>-13</sup>
Q3) What is the conjugate acid of OH<sup>-</sup>?
A)O<sub>2</sub>
B)H<sub>2</sub>O
C)O<sup>-</sup>
D)O<sup>2-</sup>
E)H<sub>3</sub>O<sup>+</sup>
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Page 18
Chapter 17: Additional Aspects of Aqueous Equilibria
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Sample Questions
Q1) The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)<sub>2</sub> and 150.0 mL of 0.125 M HCl is ________.
A)6.29
B)4.11
C)1.14
Q2) A 50.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.The concentration of the monoprotic acid is about ________ mol/L.
A)0.120
B)25.0
C)0.240
D)0.0600
E)0.100
Q3) CaCO<sub>3</sub> is very soluble in the presence of ________.
Q4) A complex ion is when a metal ion binds to a ________.
Q5) In general,the solubility of a slightly soluble salt is decreased by the presence of a second solute that furnishes a ________.
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Chapter 18: Chemistry of the Environment
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Sample Questions
Q1) The greenhouse effect of a methane molecule far exceeds the effect of a carbon dioxide molecule.
A)True
B)False
Q2) Which one of the following substances found in the atmosphere will absorb radiation in the infrared portion of the spectrum?
A)N<sub>2</sub>
B)O<sub>2</sub>
C)Kr
D)H<sub>2</sub>O
E)He
Q3) The three most concentrated ions in seawater are ________.
Q4) Sulfur released into the troposphere arises from both natural and human activity.What is the ratio of human to natural sources of sulfur compounds?
A)3:1
B)2:1
C)1:1
D)1:2
E)1:3
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Chapter 19: Chemical Thermodynamics
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Sample Questions
Q1) The value of H° for the decomposition of gaseous sulfur trioxide to its component elements, 2SO<sub>3</sub> (g) 2S (s,rhombic)+ 3O<sub>2</sub> (g) Is ________ kJ/mol.
A)+790.4
B)-790.4
C)+395.2
D)-395.2
E)+105.1
Q2) The value of S° for the decomposition of phosphorous trichloride into its constituent elements, 2PCl<sub>3 </sub>(g) P<sub>2 </sub>(g)+ 3Cl<sub>2</sub>( g) Is ________ J/K mol.
A)-311.7
B)+311.7
C)+263.6
D)+129.4
E)-129.4
Q3) What is the G° (kJ/mol)for the formation of silver chloride at 25 °C? K<sub>sp</sub> = 1.8 × 10<sup>-10</sup>
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Page 21
Chapter 20: Electrochemistry
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Sample Questions
Q1) What is the oxidation number of oxygen in H<sub>2</sub>O<sub>2</sub>? A)0 B)+1
Q2) Which element is oxidized in the following reaction? Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup> + 6S<sub>2</sub>O<sub>3</sub><sup>2-</sup> + 14H<sup>+</sup> 2Cr<sup>3+</sup> +
3S<sub>4</sub>O<sub>6</sub><sup>2-</sup> + 7H<sub>2</sub>O A)S<sub>4</sub>O<sub>6</sub><sup>2-</sup>
B)Cr
C)H D)O
E)S
Q3) Define a coulomb.
Q4) The potential (E)to move K<sup>+</sup> from the extracellular fluid to the intracellular fluid necessitates work.The sign for this potential is ________.
Q5) The major product of a ________ fuel cell is water.
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Chapter 21: Nuclear Chemistry
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Sample Questions
Q1) What happens to the mass number and the atomic number of an element when it undergoes alpha decay?
A)The mass number decreases by 4 and the atomic number decreases by 2.
B)The mass number does not change and the atomic number increases by 1.
C)The mass number increases by 4 and the atomic number does not change.
D)The mass number increases by 2 and the atomic number decreases by 1.
E)The mass number does not change and the atomic number increases by 2.
Q2) Radioactive decay is a first order kinetic process.
A)True
B)False
Q3) What is the atomic number of a neutron?
A)3
B)1
C)2
D)0
E)4
Q4) What happens in the nucleus of an atom that undergoes positron emission?
Q5) The conversion of matter to energy and mass loss occurs in ________ reactions?
Q6) The amount of fissionable material necessary to maintain a chain reactions is called the ________.
Page 23
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Chapter 22: Chemistry of the Nonmetals
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Sample Questions
Q1) A borane is a ________.
A)compound containing only boron and oxygen
B)compound containing only boron and aluminum
C)compound containing only boron and hydrogen
D)compound containing only boron and carbon
E)three-dimensional covalent network of boron atoms
Q2) The oxidation number of N in NO<sub>2</sub><sup>- </sup>is ________.
A)+1
B)+2
C)+3
D)+4
E)+5
Q3) Of Li,K,P and Ne which is the most electronegative?
Q4) B<sub>2</sub>O<sub>3</sub> is the anhydride of ________.
A)borous acid
B)diborane
C)tetraboric acid
D)boric acid
E)borax
Q5) The acid and salts of which halogen-oxyanion are the most stable?
Page 24
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Chapter 23: Transition Metals and Coordination Chemistry
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Sample Questions
Q1) The porphyrin compound that contains Mg (II)is called ________.
Q2) Which element has the largest bonding atomic radius?
A)scandium
B)titanium
C)vanadium
D)chromium
E)manganese
Q3) In humans,what percent of absorbed iron is found in blood?
A)15
B)25
C)40
D)60
E)75
Q4) A racemic mixture is ________.
A)an equal mixture of both enantiomers of an optically active species
B)a mixture of an optically active species with an optically inactive species
C)an equal mixture of cis- and trans-isomers
D)a mixture of metal ions and ligands in equilibrium
E)a mixture of structural isomers
Q5) Name the compound,Ca[AlH<sub>4</sub>]<sub>2</sub>.
Page 25
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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry
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Sample Questions
Q1) Racemic mixtures of enantiomers do not rotate the plane of polarized light.
A)True
B)False
Q2) The doubly ionized form of an amino acid is called a(n)________.
Q3) Primary alcohols can be oxidized to produce ________.
A)amides
B)esters
C)aldehydes
D)secondary alcohols
E)amines
Q4) Which one of the following is a monosaccharide?
A)fructose
B)lactose
C)sucrose
D)maltose
E)none of the above
Q5) Write the formula for 2-methyl-4-propylnonane.
Q7) Hydrogenation of what alkyne produces propane? Page 26
Q6) The aromas of different fruit are due to the chemical compounds known as
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