Introductory Chemistry Final Exam Questions - 1785 Verified Questions

Introductory Chemistry

Final Exam Questions

Course Introduction

Introductory Chemistry provides a foundational understanding of the principles and concepts in chemistry. The course covers atomic and molecular structure, chemical bonding, chemical reactions, stoichiometry, states of matter, solutions, and basic thermochemistry. Designed for students with little or no prior background in chemistry, it emphasizes the development of problem-solving skills, laboratory techniques, and scientific reasoning, preparing students for further studies in chemistry and related disciplines.

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Introductory Chemistry 4th Edition by Steve Russo

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18 Chapters

1785 Verified Questions

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Chapter 1: What Is Chemistry

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Sample Questions

Q1) What is the name given to the element with the symbol "K"?

A)Kallium

B)Potassium

C)Phosphorus

D)Krypton Answer: B

Q2) Iced tea, with sugar completely dissolved in it, is an example of homogeneous matter.

A)True

B)False Answer: True

Q3) What is the name given to the element with the symbol "P"?

A)Polonium

B)Protactinium

C)Phosphorus

D)Palladium Answer: C

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Page 3

Chapter 2: The Numerical Side of Chemistry

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Sample Questions

Q1) Which of the following is the hottest temperature?

A)90 °C

B)104 °F

C)353 K

D)All of the above are the same.

Answer: A

Q2) The Kelvin temperature is not always higher than the equivalent Celsius temperature.

A)True

B)False

Answer: False

Q3) Which of the following is the shortest?

A)18 inches

B)0.58 m

C)580 mm

D)1.9 ft

Answer: A

Q4) It is 1148 miles from Grand Rapids, Michigan, to Starkville, Mississippi. What is the same distance in kilometers (1 mile = 1.61 kilometers)?

Answer: 1848 kilometers (although it seems much longer by car)

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Chapter 3: The Evolution of Atomic Theory

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Sample Questions

Q1) The structure of individual atoms can roughly be described as ________.

A)positively charged center and mostly empty space

B)an even mixture of mass and charge scattered throughout a spherical shape

C)positively charged, low-mass pieces in orbit around a massive, negatively charged center

D)positively charged pieces in orbit around a low-mass, negatively charged center

Answer: A

Q2) The oxygen-17 (-2)isotopic anion contains more electrons than either protons or neutrons.

A)True

B)False

Answer: True

Q3) A neutral atom's atomic number is equal to ________.

A)the number of nucleons

B)the sum of protons and neutrons

C)the number of electrons

D)the number of neutrons

Answer: C

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Chapter 4: The Modern Model of the Atom

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Sample Questions

Q1) A metal is an element that tends to ________ valence electrons in chemical reactions, becoming a(n)________ in the process.

A)lose; cation

B)gain; anion

C)lose; anion D)gain; cation

Q2) Write the complete electronic ground state configuration of the Se^2- ion. Which other element (if any)shares this electronic configuration?

Q3) Which of the following anions will have the electronic configuration

1s²2s²2p⁶3s²3p^{6 ?}

A)K^1-

B)Cl¹^-

C)S²^-

D)Br¹^-

Q4) The speed of light is about 186,000 miles per minute.

A)True

B)False

Q5) Which element is the more reactive, sodium (Na)or potassium (K)?

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Chapter 5: Chemical Bonding and Nomenclature

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Sample Questions

Q1) The chlorate , bisulfate and chromate anions are also called oxyanions.

A)True

B)False

Q2) Carbon tetrafluoride has ________ total valence electrons.

A)24

B)28

C)32

D)36

Q3) There are twice as many hydrogen as oxygen atoms in the acetate anion.

A)True

B)False

Q4) The compound H₂SO₃ is called ________.

A)sulfurous acid

B)sulfuric acid

C)hydrogen sulfide

D)sulfite acid

Q5) Metals are always going to be the more electropositive elements in a bond as long as they are attached to a non-metal.

A)True

B)False

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Chapter 6: The Shape of Molecules

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Sample Questions

Q1) CS₂

Q2) When drawing the three-dimensional structure diagram of a molecule the solid (not bold or dotted)line ________.

A)projects out from the page B)goes back behind the page C)the bond is in the plane of the page D)One cannot say unless the formula of the molecule is known.

Q3) The angle around carbon in hydrogen cyanide is ________.

A)105°

B)109°

C)120°

D)180°

Q4) What is the steric number of the central atom in boron trichloride?

A)1

B)2

C)3

D)4

Q5) The bond angle in carbon tetrachloride is 109°.

A)True

B)False

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Chapter 7: Intermolecular Forces and the Phases of Matter

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Sample Questions

Q1) silicon carbide, SiC, m.p.: 2700 °C

Q2) Which of the following will have the highest boiling point?

A)HI

B)HBr

C)HCl

D)HF

Q3) Which of the three phases of matter (solid, liquid, or gas)features particles in a fixed, rigid arrangement?

A)solid

B)liquid

C)gas

D)All three phases of matter have rigid arrangements of particles.

Q4) Which intermolecular force is important for the function of the antibiotic vancomycin?

A)London forces

B)van der Waals forces

C)hydrogen bonding

D)dipole forces

Q5) ethanol, C₂H₆O, m.p.: -117 °C

Q6) glucose, C₆H₁₂O₆

Page 9

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Chapter 8: Chemical Reactions

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Sample Questions

Q1) When aqueous solutions of sodium phosphate and calcium nitrite are mixed, the spectator ions are ________.

A)calcium and nitrite

B)sodium and phosphate

C)calcium and phosphate

D)sodium and nitrite

Q2) The equation Zn + CuCl₂ Cu + ZnCl₂ is an example of a ________ reaction.

A)combination

B)single replacement

C)double replacement

D)decomposition

Q3) Which of the following equations is not a single replacement reaction?

A)H₂SO₄ + Mg(OH)₂ H₂O + MgSO₄

B)Zn + HCl H₂ + ZnCl₂

C)Al + Fe₂O₃ Al₂O₃ + Fe

D)Na + H₂O NaOH + H₂

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Page 10

Chapter 9: Stoichiometry and the Mole

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Sample Questions

Q1) The number of phosphorus atoms in one molecule of H₃PO₄ is ________.

A)1

B)8

C)6.02 × 10²³

D)4.8 × 10²³

Q2) What is the % yield if 52 g ammonia produce 45 g NO?

A)100%

B)50%

C)25%

D)18%

Q3) A sample of methane gas that contains Avogadro's number of atoms has a mass of ________.

A)3.2 g

B)6.4 g

C)16.0 g

D)80.0 g

Q4) The % composition of chlorine in C₆H₈NCl is 23.4%.

A)True

B)False

11

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Chapter 10: Electron Transfer in Chemical Reactions

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Sample Questions

Q1) Which of the following reactions is an oxidation-reduction reaction?

A)NaOH + HCl NaCl + H₂O

B)AgNO₃ + NaCl AgCl + NaNO₃

C)CH₄ + 2 O₂ CO₂ + 2 H₂O

D)CaO + CO₂ CaCO₃

Q2) Which of the following is most easily oxidized?

A)Ni

B)Pb

C)Li

D)Cr

Q3) The cathode is the electrode where oxidation occurs.

A)True

B)False

Q4) Which of the following is the most easily reduced?

A)(K⁺)

B)(Na⁺)

C)(Au⁺)

D)(^Hg2+)

Q5) For each reaction above that can be classified as an electron transfer reaction, state which element(s)gain, and which element(s)lose, electrons.

Page 12

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Chapter 11: What If There Were No Intermolecular Forces

the Ideal Gas

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Sample Questions

Q1) 855 torr is equal to ________ cm Hg.

A)1.13

B)85.5

C)855

D)8550

Q2) Which gas has a density equal to 1.43 g/L at STP?

A)nitrogen

B)oxygen

C)helium

D)carbon monoxide

Q3) As the temperature of a gas increases, its pressure increases as long as the volume is kept constant.

A)True

B)False

Q4) The molar volume of any gas whether diatomic or monoatomic is 22.4 L at STP.

A)True

B)False

Q5) The boiling point of water is 373 K.

A)True

B)False

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Chapter 12: Solutions

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Sample Questions

Q1) C₈H₁₈will dissolve in CCl₄.

A)True

B)False

Q2) A saline solution will boil at 100 °C.

A)True

B)False

Q3) A 2.154 g sample of an unknown non-electrolyte is dissolved in 50 g of water (K_f of water = 1.86 °C). If the solution freezes at -1.23 °C, the molecular mass of the non-electrolyte is ________.

A)33

B)65

C)130

D)260

Q4) An impurity ________ the melting point of a compound. A)decreases

B)increases

C)has no effect on D)One cannot say unless the physical properties of the compound are known.

Q5) What are the three ways a given solution's "percent composition" can be described?

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Chapter 13: When Reactants Turn Into Products

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Sample Questions

Q1) Which of the following is an exothermic reaction?

A)burning propane gas in a barbecue

B)burning gasoline when driving a car

C)creating an explosion by detonating nitroglycerine

D)All of the above are exothermic reactions.

Q2) For an endothermic reaction, the value for E_rxn is a negative number.

A)True

B)False

Q3) A catalyst need not be present in large quantities.

A)True

B)False

Q4) The rate of a reaction is proportional to ________.

A)the total number of collisions that occur per unit time

B)the fraction of collisions with energy larger than the energy of activation

C)the fraction of collisions with the proper orientation

D)All of the above are correct.

Q5) A high energy of activation leads to more products favored in the reaction.

A)True

B)False

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) In an endothermic reaction, adding heat will ________.

A)increase the amount of products

B)decrease the amount of reactants

C)decrease the amount of products

D)both A and B

Q2) For which of the following values of an equilibrium constant (K_e_q)would you expect the equilibrium to lie farthest to the left (reactants most highly favored)?

A)0.491, at 20 °C

B)1.04, at 20 °C

C)10.6, at 20 °C

D)1.46 × 10^-4, at 20 °C

Q3) If the solubility of copper(II)sulfate is 4.9 × 10^-³ M, the solubility product is ________.

A)2.4 × 10^-⁵

B)9.6 × 10^-⁵

C)1.2 × 10^-²

D)8.7 × 10^-⁸

Q4) H₂ (g)+ F₂ (g) 2HF (g)

Q5) 3O₂ (g) 2O₃ (g)

Page 16

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Chapter 15: Electrolytes, Acids, and Bases

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Sample Questions

Q1) Which of the following does not produce more than one H₃O⁺ ion per molecule of acid when dissolved in water?

A)carbonic

B)sulfurous

C)phosphoric

D)acetic

Q2) Sodium hydroxide is a non-electrolyte.

A)True

B)False

Q3) The conjugate base of H₂PO₄^- is ________.

A)H₃PO₄

B)HPO₄^-²

C)PO₄^-³

D)H₄PO₄⁺

Q4) An aqueous solution of HCl is called hydrochloric acid.

A)True

B)False

Q5) CH₃CO₂H has four acidic hydrogens.

A)True

B)False

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Chapter 16: Nuclear Chemistry

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Sample Questions

Q1) The daughter isotope of ¹⁹⁶Po when it undergoes alpha-emission is ²⁰⁰Pb.

A)True

B)False

Q2) When an unstable nucleus expels a positron ________.

A)its mass number is decreased by four units

B)its atomic number is decreased by one unit

C)its atomic number is increased by one unit

D)its mass number is decreased by one unit

Q3) ^{An electron is a nucleon.}

A)True

B)False

Q4) Which of the following transformations is not an alpha emission?

A)(¹⁴C ¹⁴N)

B)(²²⁵Ac ²²¹Fr)

C)(²⁴¹Am ²³⁷Np)

D)(²¹⁸Po ²¹⁴Pb)

Q5) What is the mass defect of the carbon-14 isotope (in g/mol)? Carbon-14 has an atomic mass of 14.0032 g/mol.

Page 18

Q6) ³⁷Ar + _-₁e ______

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Chapter 17: The Chemistry of Carbon

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Sample Questions

Q1) Which of the following formulas may be attributed to a ketone?

A)C₄H₈O

B)C₄H₁₀O

C)C₄H₈O₂

D)C₄H₆

Q2) The ability of carbon to connect and link together is called ________.

A)isomerism

B)allotropism

C)catenation

D)ring formation

Q3) Ethanol may be obtained via the fermentation of grains.

A)True

B)False

Q4) CH₃Br is an alkyl halide.

A)True

B)False

Q5) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,2,4-trimethylpentane.

Q6) Draw the structure of butanal.

Page 19

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Chapter 18: Synthetic and Biological Polymers

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Sample Questions

Q1) Cellulose and starch are both polysaccharides of glucose. Explain why humans can consume and digest starch but not cellulose.

Q2) The name of the bond that combines two amino acids together is called

A)peptide

B)glycoside

C)acetal

D)ketal

Q3) The number of amino acids that define the difference in shape between a normal hemoglobin molecule and that of a sickle-cell anemia patient is ________.

A)1

B)5

C)10

D)all

Q4) Which of the following statements about a DNA molecule is incorrect?

A)All DNA molecules are made from a repeating unit consisting of a phosphate group, a sugar group, and an amine base.

B)Complementary base pairs in DNA molecules are held together by hydrogen bonds.

C)Normal DNA is double-stranded and helical in shape.

D)Complementary bases in DNA molecules are held together by covalent bonds.

Page 20

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