Basic Chemistry Test Questions
Course Introduction
Basic Chemistry introduces students to the fundamental concepts and principles of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and the periodic table. Emphasis is placed on understanding the properties and behaviors of elements and compounds, chemical reactions, and the relevance of chemistry to everyday life. Through theoretical lessons and practical laboratory experience, students develop foundational skills in observation, analysis, and scientific reasoning, preparing them for further study in scientific disciplines.
Recommended Textbook
Introductory Chemistry 4th Edition by Steve Russo
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1785 Verified Questions
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Chapter 1: What Is Chemistry
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Sample Questions
Q1) Which of the following represents a physical change only?
A)barbecuing a steak
B)adding electricity to water to produce hydrogen and oxygen gas
C)chopping a piece of wood
D)burning a propane camping stove
Answer: C
Q2) What chemical symbol has been given to the element sodium?
A)S
B)K
C)Na
D)Sr
Answer: C
Q3) Which of the following is not a chemical property of carbon dioxide?
A)It is a critical component in photosynthesis.
B)It is used in fire extinguishers because it does not support combustion.
C)It is used to pump up bicycle tires.
D)It is soluble in blood.
Answer: C
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Chapter 2: The Numerical Side of Chemistry
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Sample Questions
Q1) C is the derived SI unit that measures coulombs (electrical charge).
A)True
B)False
Answer: True
Q2) Which of the following correctly expresses (in normal decimal notation)the number 1.06 × 10<sup>-</sup><sup>4</sup>?
A)10,600
B)106
C)0.0106
D)0.000106
Answer: D
Q3) The number 0.0040600 has ________ trailing zeros.
A)0
B)1
C)2
D)6 Answer: C
Q4) Convert 302 cubic inches to liters (1 inch = 2.54 centimeters).
Answer: 4.95 L
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Chapter 3: The Evolution of Atomic Theory
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Sample Questions
Q1) Sulfur belongs to the chalcogen family.
A)True
B)False
Answer: True
Q2) Which of the following terms applies to the horizontal rows found on a periodic table?
A)Arrangement
B)Group
C)Period
D)Isotope
Answer: C
Q3) How is the term "atomic number" defined for a given atom or isotope?
A)as the mass of one mole of that element or isotope
B)as the sum of the protons, neutrons, and electrons it contains
C)as the sum of the protons and neutrons its nucleus contains
D)as the number of protons its nucleus contains
Answer: D
Q4) uranium-235
Answer: atomic number 92, mass number 235, symbol U
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Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) The total number of electrons that can be accommodated in 3d is ________.
A)5
B)2
C)6
D)10
Q2) Which feature of Bohr's atomic model is no longer accepted as true by today's scientists?
A)that most of an atom's mass is located within the nucleus
B)that electrons have only certain, allowed energy values
C)that electrons orbit the nucleus in circular paths
D)that each principal quantum level can hold a maximum of 2n<sup>2</sup> electrons
Q3) Which of the following elements is the largest size halogen?
A)He
B)Br
C)F
D)Kr
Q4) The atom size decreases as one proceeds from left to right across a period.
A)True
B)False
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Chapter 5: Chemical Bonding and Nomenclature
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Sample Questions
Q1) A single bond is always represented by two electrons.
A)True
B)False
Q2) The ferrous ion is also referred to as iron (III).
A)True
B)False
Q3) The number of valence electrons in the carbonate anion is ________.
A)20
B)22
C)24
D)26
Q4) The expected formula between magnesium and sulfur is ________.
A)MgS
B)MgS<sub>2</sub>
C)Mg<sub>2</sub>S
D)Mg<sub>2</sub>S<sub>3</sub>
Q5) How many valence electrons are required when constructing a complete Lewis dot structure of the compound CF<sub>2</sub>C1<sub>2</sub>?
Q6) H<sub>2</sub>Se
Q7) BF<sub>3</sub>
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) Which of the following is tetrahedral?
A)sulfur trioxide
B)sulfur dioxide
C)sulfur dichloride
D)ammonium ion
Q2) NO<sub>3</sub><sup>-</sup>
Q3) What is the steric number of the central atom in carbon disulfide?
A)1
B)2
C)3
D)4
Q4) Which of the following will be the least soluble in water?
A)CH<sub>3</sub>OH
B)CH<sub>4</sub>
C)NH<sub>3</sub>
D)CH<sub>3</sub>CH<sub>2</sub>OH
Q5) CHC1<sub>3</sub>
Q6) The ball-and-stick model emphasizes the bonding pattern.
A)True
B)False
8
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) Which of the following will have the highest boiling point?
A)HI
B)HBr
C)HCl
D)HF
Q2) Quartz and diamond are non-molecular covalent substances.
A)True
B)False
Q3) Which of the following sublimes?
A)sugar
B)iron
C)mothballs
D)margarine
Q4) Vancomycin is the first line of defense against bacteria.
A)True
B)False
Q5) iodine, I<sub>2</sub>
Q6) ethanol, C<sub>2</sub>H<sub>6</sub>O, m.p.: -117 °C
Q7) silicon carbide, SiC, m.p.: 2700 °C
Q8) glucose, C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) After balancing the equation Fe<sub>2</sub>O<sub>3</sub> + Al Al<sub>2</sub>O<sub>3</sub> + Fe the correct coefficients are respectively ________.
A)1: 2: 1: 2
B)2: 3: 2: 3
C)1: 2: 2: 1
D)2: 3: 3: 4
Q2) Which hydroxide is water insoluble?
A)sodium hydroxide
B)barium hydroxide
C)aluminum hydroxide
D)calcium hydroxide
Q3) It takes ________ moles of potassium hydroxide to neutralize ________ moles of sulfuric acid.
A)1; 1
B)1; 2
C)2; 1
D)3; 1
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Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) The balanced equation involves the corresponding coefficients ________.
A)2: 2: 3
B)1: 2: 3
C)2: 1: 3
D)3: 3: 2
Q2) One mole of oxygen gas has fewer atoms than one mole of ozone gas.
A)True
B)False
Q3) The theoretical number of carbon dioxide moles produced from 6 moles NaHCO<sub>3</sub> is ________.
A)1
B)3
C)6
D)12
Q4) What is the mass in grams of 1.000 mole of P<sub>2</sub>O<sub>5</sub>?
A)239.03 g
B)61.96 g
C)141.96 g
D)46.98 g
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) The charge of chlorine in the perchlorate ion is ________.
A)+8
B)+7
C)-1
D)+6
Q2) In a chemical bond, which atom gets to own the shared electrons?
A)the larger element
B)the smaller element
C)the more electronegative element
D)the most electropositive element
Q3) Electricity is the flow of electrons.
A)True
B)False
Q4) The oxidation state of oxygen gas is ________.
A)-4
B)+2
C)-2
D)0
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) How many moles of gas are found in a container that occupies a volume of 5.50 L with a pressure of 0.335 atm at 25 °C?
A)0.0753
B)0.898
C)13.3
D)1.11
Q2) A gas sample occupies a volume of 8 L at 20 °C. The temperature at which the gas would double its volume is ________.
A)40 °C
B)10 °C
C)273 K
D)586 K
Q3) The lowest temperature that can theoretically be achieved is -273.16 °C
A)True
B)False
Q4) 947 mbar is equal to 0.933 atm (given 1 atm= 1.015 bar).
A)True
B)False
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Chapter 12: Solutions
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Sample Questions
Q1) In a dilute saline solution the solute is in the form of ________.
A)Na<sup>+</sup> and Cl<sup>-</sup>
B)NaCl (s)
C)NaCl ()
D)both A and B
Q2) Which of the following solutions are possible?
A)Both the solvent and solute are liquids.
B)Both the solvent and solute are solids.
C)The solvent is a liquid and the solute is a gas.
D)All of them are possible.
Q3) A 2.154 g sample of an unknown non-electrolyte is dissolved in 50 g of water (K<sub>f</sub> 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) Use the general rule "like dissolves like" to briefly explain why vegetable oil (nonpolar)will not dissolve in water (polar).
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Chapter 13: When Reactants Turn Into Products
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Sample Questions
Q1) A catalyst can be recovered at the end of the reaction.
A)True
B)False
Q2) When the products are higher in energy than the reactants, the reaction is endothermic.
A)True
B)False
Q3) Which of the following statements is false?
A)The rate determining step is always the slowest step in a multistep mechanism.
B)The rate constant always changes with a variation in temperature.
C)The energy of activation controls the speed of reaction.
D)The rate of a reaction is independent of the concentration of reactants.
Q4) 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.
Q5) A high energy of activation leads to more products favored in the reaction.
A)True
B)False
Page 15
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.
A)True
B)False
Q2) Consider the reaction: A + 3B 2C. Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________.
A)[A] < [B]
B)[A] > [B]
C)[A] = [B]
D)One cannot say unless the equilibrium constant value is known.
Q3) Refer to the equilibrium shown above. Adding excess oxygen will ________.
A)shift the reaction to the right
B)shift the reaction to the left
C)have no effect
D)cannot be determined, since the temperature is not known
Q4) H<sub>2</sub> (g)+ F<sub>2</sub> (g) 2HF (g)
Q5) HCl (g)+ H<sub>2</sub>O (l) H<sub>3</sub>O<sup>+</sup> (aq)+ Cl<sup>-</sup> (aq)
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Chapter 15: Electrolytes, Acids, and Bases
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Sample Questions
Q1) Which of the following is the weakest base?
A)ammonia, K<sub>b</sub> = 1.7 × 10<sup>-</sup><sup>5</sup>
B)aniline, K<sub>b</sub> = 4.2 × 10<sup>-</sup><sup>10</sup>
C)trimethylamine, K<sub>b</sub> = 7.4 × 10<sup>-</sup><sup>5</sup>
D)methylamine, K<sub>b</sub> = 4.4 × 10<sup>-</sup><sup>4</sup>
Q2) The acid in the forward reaction HCO<sub>3</sub><sup>-</sup> + H<sub>2</sub>O
H<sub>2</sub>CO<sub>3</sub> + OH<sup>-</sup> is ________.
A)HCO<sub>3</sub><sup>-</sup>
B)H<sub>2</sub>O
C)H<sub>2</sub>CO<sub>3</sub>
D)OH<sup>-</sup>
Q3) Which substance is the most acidic?
A)coffee
B)milk
C)oven cleaner
D)baking soda
Q4) Aqueous salt solution is a strong electrolyte.
A)True
B)False
Q5) What were the defining characteristics of bases as known to the alchemists?
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) <sup>An electron is a nucleon.</sup>
A)True
B)False
Q2) The daughter isotope of <sup>196</sup>Po when it undergoes alpha-emission is <sup>200</sup>Pb.
A)True
B)False
Q3) Which of the following does not carry neutrons?
A)(<sup>1</sup>n)
B)alpha rays
C)(<sup>1</sup>H)
D)deuterium
Q4) What is the mass defect of the lithium-9 isotope in g/mol? Lithium-9 has an atomic mass of 9.0273 g/mol.
Q5) An alpha particle is neutral.
A)True
B)False
Q6) <sup>146</sup>Sm ______ + <sup>142</sup>Nd
Q7) <sup>238</sup>U + ______ <sup>239</sup>Np + <sub>-</sub><sub>1</sub>e
Q8) <sup>16</sup>O + <sup>4</sup>He ______
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Chapter 17: The Chemistry of Carbon
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Sample Questions
Q1) Convert the hydrocarbon formula C<sub>3</sub>H<sub>6</sub> to a line drawing representation of this same formula.
Q2) Octane has a lower boiling point than decane.
A)True
B)False
Q3) Which of the following unbranched/acyclic hydrocarbons is saturated?
A)C<sub>6</sub>H<sub>14</sub>
B)C<sub>10</sub>H<sub>20</sub>
C)C<sub>12</sub>H<sub>22</sub>
D)C<sub>5</sub>H<sub>10</sub>
Q4) Which of the following unbranched/acyclic hydrocarbons may have a triple bond?
A)C<sub>6</sub>H<sub>1</sub><sub>4</sub>
B)C<sub>10</sub>H<sub>20</sub>
C)C<sub>12</sub>H<sub>22</sub>
D)C<sub>5</sub>H<sub>10</sub>
Q5) CH<sub>3</sub>NH<sub>2</sub> is a primary amine.
A)True
B)False
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) Nylon contains only one type of monomer.
A)True
B)False
Q2) According to the text, the number of amino acids that a human body cannot synthesize is ________.
A)5
B)10
C)15
D)20
Q3) Teflon's monomer is ________.
A)tetrafluoroethane
B)tetrafluoroethene
C)tetrafluorooctane
D)tetrafluorobenzene
Q4) Which of the following does not appear in a DNA strand?
A)deoxyribose sugar
B)phosphate
C)amino acids
D)amine base
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