General Chemistry I Solved Exam Questions
Course
Introduction
General Chemistry I provides an introduction to the fundamental principles of chemistry. Topics covered include atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, and the periodic table. Emphasis is placed on developing problem-solving skills and understanding how chemical principles apply to real-world phenomena. Laboratory experiments complement lecture material, offering hands-on experience with essential techniques and reinforcing core concepts. This course lays the foundation for advanced studies in chemistry and related scientific disciplines.
Recommended Textbook
Introductory Chemistry 6th Edition by Nivaldo J. Tro
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19 Chapters
2138 Verified Questions
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Page 2
Chapter 1: The Chemical World
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Sample Questions
Q1) A theory can only exist after many experiments have validated a hypothesis.
A)True
B)False
Answer: True
Q2) All things are made of atoms or molecules.
A)True
B)False
Answer: True
Q3) The first step in acquiring scientific knowledge is often the observation or measurement of some aspect of nature.
A)True
B)False
Answer: True
Q4) Antoine Lavoisier proposed the atomic theory.
A)True
B)False
Answer: False
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Page 3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) Numbers are usually written so that the uncertainty is in the last reported digit.
A)True
B)False Answer: True
Q2) The correct prefix for the multiplier 1,000 is:
A)mega.
B)milli.
C)micro.
D)nano.
E)none of the above Answer: E
Q3) How many grams are in 1.48 × 10<sup>7</sup> g?
A)1.48 × 10<sup>3</sup>
B)1.48 × 10<sup>13</sup>
C)1.48
D)14.8
E)none of the above
Answer: D
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4
Chapter 3: Matter and Energy
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Sample Questions
Q1) A chemical change occurs when matter does not change its composition.
A)True
B)False
Answer: False
Q2) Which of the following statements about physical and chemical changes is FALSE?
A)In a chemical change,matter changes its composition.
B)In a physical change,matter does not change its composition.
C)Phase changes are always physical changes.
D)Chemical reactions are chemical changes.
E)All of the above statements are true.
Answer: E
Q3) How would you classify raisin bran?
A)pure substance-compound
B)mixture-heterogeneous
C)pure substance-element
D)mixture-homogeneous
E)none of the above
Answer: B
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5
Chapter 4: Atoms and Elements
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Sample Questions
Q1) How many protons and neutrons are in Cl-37?
A)20 protons,17 neutrons
B)17 protons,37 neutrons
C)17 protons,20 neutrons
D)37 protons,17 neutrons
E)none of the above
Q2) The atomic mass unit is defined as:
A)the mass of the hydrogen atom containing only one proton.
B)the mass of electrons found in a carbon atom containing six protons and neutrons.
C)1/12 the mass of a carbon atom containing six protons and six neutrons.
D)1/14 the mass of a nitrogen atom containing 7 protons and 7 neutrons.
E)none of the above
Q3) Which of the following statements about atoms is FALSE?
A)Atoms compose all matter.
B)Atoms are responsible for the sensation of smell.
C)Atoms are the basic building block of nature.
D)An atom is the smallest identifiable unit of an element.
E)All of the above statements are true.
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6
Chapter 5: Molecules and Compounds
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Sample Questions
Q1) How many carbon atoms are in the formula
Al<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub>?
A)3
B)9
C)1
D)6
E)none of the above
Q2) What is the correct formula for potassium dichromate?
A)K(CrO<sub>4</sub>)<sub>2</sub>
B)KCr<sub>2</sub>O<sub>7</sub>
C)K<sub>2</sub>CrO<sub>4</sub>
D)K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>
E)none of the above
Q3) SO<sub>2</sub> is an ionic compound.
A)True
B)False
Q4) The proper name for SF<sub>6</sub> is sulfur tetrafluoride.
A)True
B)False
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Chapter 6: Chemical Composition
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Sample Questions
Q1) A 42.7 gram sample of potassium nitrate contains how many grams of potassium?
A)39.1
B)16.5
C)21.4
D)8.54
E)none of the above
Q2) The mass of 2.0 moles of H<sub>2</sub>O is greater than the mass of 1.0 mole of CO<sub>2</sub>.
A)True
B)False
Q3) How many hydrogen atoms are in 35.0 grams of hydrogen gas?
A)4.25 × 10<sup>25</sup>
B)2.09 × 10<sup>25</sup>
C)2.12 × 10<sup>25</sup>
D)1.05 × 10<sup>25</sup>
E)none of the above
Q4) The molecular formula is equal to the empirical formula multiplied by a whole number integer.
A)True
B)False
Page 8
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) Which of the following statements about redox reactions is FALSE?
A)Oxidation is the loss of electrons.
B)Reduction is the gain of electrons.
C)A reaction can result in either oxidation or reduction,not both.
D)A reaction involving elemental oxygen is a redox reaction.
E)All of the above statement are true.
Q2) What type of a reaction occurs when potassium metal reacts with fluorine gas?
A)precipitation
B)acid-base neutralization
C)oxidation-reduction
D)gas evolution
E)no reaction
Q3) An acid-base reaction always produces a salt plus carbon dioxide.
A)True
B)False
Q4) Evidence of a redox reaction is when a substance reacts with elemental oxygen.
A)True
B)False
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Consider the following generic chemical equation: 2A + 5B C + 3D If you react 4 units of A with 10 units of B,which statement is TRUE?
A)Substance A will be the limiting reactant.
B)Substance B will be the limiting reactant.
C)There is just enough of A and B so that everything reacts completely.
D)Substance C cannot be formed from this reaction.
E)none of the above
Q2) Which is the excess reactant in the following reaction given that you start with 15.5 g of Na<sub>2</sub>S and 12.1 g CuSO<sub>4</sub>?
Reaction: Na<sub>2</sub>S + CuSO<sub>4 </sub> Na<sub>2</sub>SO<sub>4</sub> + CuS
A)Na<sub>2</sub>S
B)CuSO<sub>4</sub>
C)Na<sub>2</sub>SO<sub>4</sub>
D)CuS
E)not enough information
Q3) The limiting reactant is not necessarily the reactant with the least mass.
A)True
B)False
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Page 10
Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) An emission spectrum results when light emitted by glowing gas is passed through a prism.
A)True
B)False
Q2) Bohr showed that the emission spectrum of hydrogen was continuous with no interruption across the entire visible wavelength range.
A)True
B)False
Q3) The higher the principal quantum number,the lower the orbital energy.
A)True
B)False
Q4) The subshell that has five orbitals and can hold up to ten electrons is the:
A)d subshell
B)f subshell
C)s subshell
D)p subshell
E)none of the above
Q5) The shorter the wavelength of light,the more energy it has.
A)True
B)False
11
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) The VSEPR theory predicts that the H-C-H angle in CH<sub>4</sub> measures 120°.
A)True
B)False
Q2) What is the molecular geometry of CCl<sub>4</sub>?
A)bent
B)linear
C)tetrahedral
D)trigonal pyramidal
E)not enough information
Q3) The Lewis model predicts that the formula for a compound between barium and sulfur is:
A)BaS
B)Ba<sub>2</sub>S
C)BaS<sub>2</sub>
D)BaS<sub>3</sub>
E)none of the above
Q4) When calculating the number of electrons for the Lewis structure of a polyatomic ion,subtract one electron for each negative charge.
A)True
B)False
Page 12
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Chapter 11: Gases
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Sample Questions
Q1) For all gas law calculations,the temperature must be in kelvins.
A)True
B)False
Q2) What problem could happen if deep sea divers used pure oxygen in their tanks?
A)hypoxia
B)oxygen toxicity
C)nitrogen narcosis
D)rapture of oxygen
E)none of the above
Q3) A sealed bag of potato chips will expand when taken to a higher altitude.This is an example of Boyle's law.
A)True
B)False
Q4) A 3.76 g sample of a noble gas is stored in a 2.00 L vessel at 874 torr and 25°C.What is the noble gas? (R= 0.0821 L atm/ mol K)
A)He
B)Ne
C)Ar
D)Kr
E)not enough information
Page 13
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Chapter 12: Liquids, solids, and Intermolecular Forces
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Sample Questions
Q1) The amount of heat required to melt one mole of a solid is called the:
A)heat of vaporization.
B)heat of fusion.
C)heating curve.
D)cooling curve.
E)none of the above
Q2) Atomic solids,such as graphite,have a weak dispersion force holding them together.
A)True
B)False
Q3) The shapes of protein molecules are determined by intermolecular forces.
A)True
B)False
Q4) Sublimation is the process of a liquid being converted directly to a gas. A)True
B)False
Q5) All intermolecular forces are broken when a liquid vaporizes into a gas.
A)True
B)False
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Page 14
Chapter 13: Solutions
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Sample Questions
Q1) How many grams of KCl are needed to make 50.0 mL of 2.45M KCl?
A)9.13
B)1.52
C)91.3
D)0.123
E)none of the above
Q2) If you put a living cell into seawater containing a higher concentration of sodium chloride,the cell loses water through osmosis.
A)True
B)False
Q3) A sugar solution is an example of a weak electrolyte solution.
A)True
B)False
Q4) Which of the following compounds is a strong electrolyte?
A) C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>
B) C<sub>7</sub>H<sub>14</sub>O<sub>5</sub>
C) C<sub>4</sub>H<sub>8</sub>O<sub>2</sub>
D) NaC<sub>2</sub>H<sub>3</sub>O<sub>2</sub>
E)all of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) What is the conjugate acid of OH ?
A) O<sup>2-</sup>
B) H<sub>2</sub>O
C)NaOH
D)OH
E)none of the above
Q2) Which of the following acids is commonly used for manufacturing fertilizer?
A)HCl
B)HNO<sub>3</sub>
C)HF
D)HBr
E)all of the above
Q3) Which of the following acids is diprotic?
A)HClO<sub>4</sub>
B)HNO<sub>3</sub>
C)HI
D) H<sub>2</sub>SO<sub>4</sub>
E)none of the above
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) The rate of a reaction increases with increasing concentrations of reactants because you have more collisions occurring in a given time period.
A)True B)False
Q2) The larger the equilibrium constant,the greater is the concentration of reactants relative to products at equilibrium.
A)True B)False
Q3) A reversible reaction is one that can be stopped and then restarted as needed. A)True B)False
Q4) Adding heat to an endothermic reaction causes the reaction to shift to the right. A)True B)False
Q5) Adding heat to an exothermic reaction will cause the reaction to remain unchanged. A)True B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) The half-reaction 2 Br <sup>1-</sup> Br<sub>2</sub> + 2 e<sup>-</sup> is balanced with respect to mass but it is not balanced with respect to charge.
A)True
B)False
Q2) An electrolytic cell is a spontaneous redox reaction.
A)True
B)False
Q3) Balance the following half reaction in base solution: H<sub>2</sub>O (l) H<sub>2</sub> (g)
A)2H<sub>2</sub>O (l)+ 2 e<sup>-</sup> H<sub>2</sub> (g)+ 2 OH<sup>-</sup> (aq)
B)2H<sub>2</sub>O (l) 2H<sub>2</sub> (g)+ 2 e<sup>-</sup> + O<sub>2</sub>
C)2H<sub>2</sub>O (l) H<sub>2</sub> (g)+ 2 H<sup>+</sup> + 2e<sup>-</sup>
D)H<sub>2</sub>O (l) 2H<sup>+</sup> + 2OH<sup>-</sup>
E)2H<sub>2</sub>O (l) H<sub>2</sub> (g)+ 2OH<sup>-</sup> (aq)+ 5 e<sup>-</sup>
Q4) A spontaneous redox reaction can be used to produce electrical current.
A)True
B)False
Q5) Distinguish between a galvanic (voltaic)cell and an electrolytic cell.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Which of the following statements about the creation of the nuclear bomb is FALSE?
A)Einstein lobbied President Roosevelt to pursue creation of the bomb.
B)American war intelligence feared the Germans were ahead of the Allies in developing nuclear weapons in WWII.
C)J.R.Oppenheimer headed the Manhattan Project.
D)The Germans were defeated by the time the bomb had been developed.
E)All of the above are true.
Q2) One danger of a nuclear power plant is that a chain reaction could produce a bomb.
A)True
B)False
Q3) Who discovered radioactivity?
A)Antoine Becquerel
B)Pierre Curie
C)Marie Curie
D)Ernest Rutherford
E)Benjamin Franklin
Q4) Briefly distinguish between nuclear fission and nuclear fusion.
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) What is the formula for propene?
A)C<sub>3</sub>H<sub>8</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>3</sub>H<sub>4</sub>
D)C<sub>3</sub>H<sub>3</sub>
E)none of the above
Q2) Which of the following statements about carbon is FALSE?
A)Carbon must always have four bonds.
B)Carbon can bond to itself.
C)Carbon can have either a tetrahedral,trigonal planar or linear geometry.
D)Carbon can form into linear,branched and cyclic compounds.
E)none of the above
Q3) An alkane would be considered a saturated compound.
A)True
B)False
Q4) Even though the aromatic ring of the compound benzene can be drawn with alternating single and double bonds,all the carbon to carbon bonds are the same.
A)True
B)False
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Chapter 19: Biochemistry
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Sample Questions
Q1) The "m" in the term mRNA represents:
A)meta.
B)mini.
C)mitosis.
D)messenger.
E)none of the above
Q2) Which protein structure provides the arrangement of polypeptides?
A)Primary Structure
B)Secondary Structure
C)Tertiary Structure
D)Quaternary Structure
E)Pental Structure
Q3) Which sequence below represents the correct base pairs that can exist in DNA?
A)A with T and C with G
B)A with C and T with G
C)A with G and C with T
D)A with U and T with G
E)none of the above
Q4) Summarize the main features of the four categories of protein structure.
Q5) What is the difference between saturated and unsaturated fatty acids?
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