General Chemistry I Practice Questions
Course Introduction
General Chemistry I provides a comprehensive introduction to the fundamental principles of chemistry. Students explore atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, periodic trends, and basic chemical reactions. Through lectures, laboratory experiments, and problem-solving exercises, the course emphasizes the development of analytical thinking and foundational laboratory skills essential for further study in the sciences.
Recommended Textbook
Introductory Chemistry 5th Edition by Nivaldo J. Tro
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19 Chapters
2146 Verified Questions
2146 Flashcards
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Chapter 1: The Chemical World
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Sample Questions
Q1) If a hypothesis is falsifiable,it means that the hypothesis was once considered true but is now considered false.
A)True
B)False
Answer: False
Q2) Observations from experiments are used to test theories.
A)True
B)False
Answer: True
Q3) What is chemistry?
Answer: Chemistry is branch of science that explains the properties and behavior of different forms of matter,in the broadest sense,by helping us understand the atoms and molecules that compose them.
Q4) John Dalton proposed the atomic theory.
A)True
B)False
Answer: True
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3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) The base unit of length in the SI system is the cm.
A)True
B)False
Answer: False
Q2) Given that 1 inch equals 2.54 centimeters,then 1 cubic inch equals 16.387 cubic centimeters.
A)True
B)False
Answer: True
Q3) Determine the answer to the following equation with correct number of significant figures:
106 ÷ 9.02 × 1.9 = ________
A)22.32816
B)22.328
C)22.3
D)22
E)none of the above
Answer: D
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4
Chapter 3: Matter and Energy
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Sample Questions
Q1) When methane is burned with oxygen,the products are carbon dioxide and water.If you produce 9 grams of water and 11 grams of carbon dioxide from 16 grams of oxygen,how many grams of methane were needed for the reaction?
A)4
B)20
C)31
D)40
E)none of the above
Answer: A
Q2) Which among the following statements is false?
A)A solid has a definite shape and a definite volume.
B)A liquid has a definite volume;but it has no definite shape.
C)A gas has neither definite volume nor definite shape.
D)Both solids and liquids are incompressible while gases are compressible.
E)none of the above
Answer: E
Q3) Matter is defined as anything that is visible to the human eye.
A)True
B)False
Answer: False
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) An element is discovered that is a solid,has one valence electron,and readily forms a 1+ ion.This element would be correctly classified as a nonmetal.
A)True
B)False
Q2) What is the charge on an ion that has an atomic number of 24 and contains 22e-?
A)2+
B)2-
C)1+
D)1-
E)none of the above
Q3) The atomic mass of individual atoms of an element may vary.
A)True
B)False
Q4) What is the atomic symbol for silver?
A)S
B)Ag
C)Au
D)Si
E)none of the above
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) What is the proper name for HBr (aq)?
A)hydrobromous acid
B)hydrousbromic acid
C)hydrobromic acid
D)bromous acid
E)none of the above
Q2) How many of each type of atom are there in the formula Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>?
A)Ca = 3,P = 1,O = 4
B)Ca = 3,P = 2,O = 4
C)Ca = 3,P = 2,O = 8
D)Ca = 3,P = 1,O = 8
E)none of the above
Q3) What is the name of Ca(NO<sub>3</sub>)<sub>2</sub>?
A)calcium dinitrite
B)calcium nitrate
C)calcium nitride
D)calcium nitrite
E)none of the above
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Page 7
Chapter 6: Chemical Composition
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Sample Questions
Q1) How many moles of iron are contained in 1.75 kg of iron?
A)3.13 × 10<sup>-2</sup>
B)3.13 × 10<sup>-4</sup>
C)31.3
D)3.13 × 10<sup>4</sup>
E)none of the above
Q2) C<sub>2</sub>H<sub>3</sub>O<sub>2</sub> could be an empirical formula.
A)True
B)False
Q3) How many moles of Pb are in 4.71 × 10<sup>21</sup> Pb atoms?<sup> </sup>
A)0.00782
B)2.84 × 10<sup>45</sup>
C)207.2
D)6.022 × 10<sup>23</sup>
E)none of the above
Q4) The lighter the atom,the less mass in one mole of that atom.
A)True
B)False
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) Which of the following statements about writing molecular,complete and net ionic equations is FALSE?
A)A molecular equation is a chemical equation showing the complete,neutral formulas for every compound in a reaction.
B)A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution.
C)A net ionic equation is an equation showing only the species that actually participate in the reaction.
D)A spectator ion remains unchanged in the reaction and appears on both sides of the equation.
E)All of the statements are true.
Q2) The following equation IS balanced: 2 C<sub>4</sub>H<sub>10</sub>O + 13 O<sub>2</sub> 8 CO2 + 10 H<sub>2</sub>O A)True B)False
Q3) A net ionic equation shows all ionic species that are present in solution. A)True B)False
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) When viewing a chemical equation,the limiting reactant can never be a chemical on the product side of the equation.
A)True
B)False
Q2) Given the recipe: 2 cups flour + 1 egg + 3 oz blueberries 4 muffins. You can make 1 dozen muffins from 3 eggs.
A)True
B)False
Q3) Given the chemical equation: 2 Ca + O<sub>2</sub> 2 CaO, if 2 moles of CaO are formed in this reaction,then 2 moles of O<sub>2</sub> must have reacted.
A)True
B)False
Q4) One of the advantages of burning fossil fuels is that it produces O<sub>2</sub> for humans to breathe.
A)True
B)False
Q5) An exothermic reaction has a negative enthalpy of reaction.
A)True
B)False
10
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) 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
Q2) What is the electron configuration for Ga?
A)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>3d<su p>10</sup>4s<sup>2</sup>4p<sup>6</sup>
B)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<su p>2</sup>3d<sup>10</sup>4p<sup>1</sup>
C)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>5</sup>3d<s up>10</sup>4s<sup>2</sup>4p<sup>1</sup>
D)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<su p>2</sup>4d<sup>10</sup>4p<sup>1</sup>
E)none of the above
Q3) A particle of light is called a packet.
A)True
B)False
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Page 11
Chapter 10: Chemical Bonding
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Sample Questions
Q1) Drugs to fight HIV have been developed using bonding theory models.
A)True
B)False
Q2) When you have 4 electron groups,the electron geometry is tetrahedral.
A)True
B)False
Q3) When calculating the number of electrons for the Lewis structure of a polyatomic ion,you must add one electron for each negative charge and subtract one electron for each positive charge.
A)True
B)False
Q4) The VSEPR theory predicts that the H-C-H angle in CH<sub>4</sub> measures 120°. A)True
B)False
Q5) The elements with the highest electronegativity values tend to be found in the:
A)upper right-side of the periodic table.
B)lower right-side of the periodic table.
C)upper left-side of the periodic table.
D)lower left-side of the periodic table.
E)center of the periodic table.
Page 12
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Chapter 11: Gases
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Sample Questions
Q1) What is the major component of the air we breathe?
A)nitrogen
B)oxygen
C)argon
D)carbon dioxide
E)smog
Q2) If the kelvin temperature of a gas is doubled,the volume is doubled provided that the pressure and the number of particles remains constant.
A)True
B)False
Q3) At STP,12.69 g of a noble gas occupies 14.09 L.What is the identity of the noble gas?
(R= 0.0821 L atm/ mol K)
A)He
B)Ne
C)Ar
D)Kr
E)not enough information
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Which sequence correctly shows the increasing density of the three phases of water?
A)solid < liquid < gas
B)gas < liquid < solid
C)gas < solid < liquid
D)liquid < gas < solid
E)none of the above
Q2) Rank the compounds NH<sub>3</sub>,CH<sub>4</sub>,and PH<sub>3</sub> in order of increasing boiling point.
A)NH<sub>3</sub> < CH<sub>4</sub>< PH<sub>3</sub>
B)CH<sub>4</sub>< NH<sub>3</sub> < PH<sub>3</sub>
C)NH<sub>3</sub> < PH<sub>3</sub>< CH<sub>4</sub>
D)CH<sub>4 </sub>< PH<sub>3 </sub>< NH<sub>3</sub>
E)PH<sub>3</sub>< NH<sub>3</sub> < CH<sub>4</sub>
Q3) Which intermolecular force is the strongest?
A)dispersion force
B)dipole-dipole force
C)hydrogen bonding
D)ion-dipole force
E)none of the above
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Page 14
Chapter 13: Solutions
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Sample Questions
Q1) We dissolve 2.45 g of sugar in 200.0 g water.What is the mass percent of sugar in the solution?
A)1.21%
B)1.23%
C)2.42%
D)123%
E)none of the above
Q2) Which of the following aqueous solutions has the highest molar concentration of Na<sup>+</sup> (aq)?
(Assume each compound is fully dissolved in water. )
A)3.0M NaCl (sodium chloride)
B)3.0M NaC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> (sodium acetate)
C)1.5M Na<sub>2</sub>SO<sub>4</sub> (sodium sulfate)
D)1.0M Na<sub>3</sub>PO<sub>4</sub> (sodium phosphate)
E)All of these solutions have the same concentration of Na<sup>+</sup> (aq).
Q3) The solubility of gases in water decreases with increasing temperature.
A)True
B)False
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15
Chapter 14: Acids and Bases
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Sample Questions
Q1) Substances that can act both as an acid and as a base are called:
A)neutral.
B)buffers.
C)indicators.
D)amphoteric.
E)none of these
Q2) Which of the following common bases is commonly used for manufacturing fertilizer?
A)NH<sub>3</sub>
B)NaHCO<sub>3</sub>
C)KOH
D)NaOH
E)all of the above
Q3) Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water?
A)OSHA regulations
B)Water can be broken down by electricity.
C)Water always has some ions dissolved in it.
D)Water dissociates fully into its ions.
E)none of the above
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Which statement about activation energy is FALSE?
A)Activation energy is an energy hump that normally exists between reactants and products.
B)The higher the activation energy,the slower the reaction rate.
C)The lower the activation energy,the faster the reaction rate.
D)Increasing the temperature lowers the activation energy.
E)All of the above are true.
Q2) The effect of a catalyst is to:
A)increase the number of collisions between reactants.
B)increase the temperature of the reactants whereby more products are formed.
C)change the position of the equilibrium.
D)change the stoichiometry of the reaction.
E)lower the activation energy of a reaction whereby making it easier for the reactants to get over the energy hump.
Q3) A catalyst speeds up a chemical reaction as it is being consumed.
A)True
B)False
Q4) Equilibrium involves the ideas of sameness and constancy.
A)True
B)False
Page 17
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Electrical current can be used to drive a nonspontaneous redox reaction.
A)True
B)False
Q2) Reduction typically involves:
A)the loss of electrons.
B)the gain of oxygen.
C)the gain of electrons.
D)the gain of water.
E)none of the above
Q3) Rusting of iron requires the presence of both oxygen and water.
A)True
B)False
Q4) The oxidation number of Cr in Cr<sub>2</sub>O<sub>7</sub> <sup>2- </sup>is: A)+2.
B)-2.
C)+7.
D)+6.
E)none of the above
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) Antoine-Henri Becquerel discovered X-rays.
A)True
B)False
Q2) A 1.2 kg sample of Th-228 has a half-life of 1.9 years.How many grams of Th is left after 5.7 years?
A)150
B)75
C)300
D)0
E)none of the above
Q3) Which of the following is NOT a type of radioactive emission?
A)alpha rays
B)beta rays
C)gamma rays
D)positrons
E)All of the above are types of radioactive emissions.
Q4) A nuclear reaction typically changes the identity of the element involved.
A)True
B)False
Q5) Briefly distinguish between nuclear fission and nuclear fusion.
Page 19
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) The reaction CH<sub>3</sub>CH<sub>3</sub> + Br<sub>2</sub> CH<sub>3</sub>CH<sub>2</sub>Br + HBr would best be described as:
A)substitution.
B)combustion.
C)addition.
D)hydrogenation.
E)none of the above
Q2) Organic compounds have to come from living things.
A)True
B)False
Q3) A compound named "propanal" would be classified as an: A)alcohol.
B)amine. C)aldehyde.
D)ether.
E)none of the above
Q4) Esters are best known for their awful odors such as that associated with the smell of rotten fish.
A)True
B)False
Page 20
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Chapter 19: Biochemistry
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Sample Questions
Q1) A seven-carbon sugar is known as:
A)tetrose.
B)sevose.
C)hexose.
D)heptose.
E)none of the above
Q2) Which of the following is a complex carbohydrate?
A)monosaccharide
B)disaccharide
C)polysaccharide
D)all of these
E)none of these
Q3) Which of the statements regarding phospholipids is FALSE?
A)A phospholipid has nearly the same structure as a triglyceride.
B)Unlike triglycerides,phospholipids have a polar region.
C)Phospholipids are common in the cell membrane.
D)A cell membrane is a bilayer of phospholipids and glycolipids.
E)All of the above statements are true.
Q4) What is the difference between saturated and unsaturated fatty acids?
Q5) Summarize the main features of the four categories of protein structure.
Page 21
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