Preparatory Chemistry Practice
Questions
Course Introduction
Preparatory Chemistry is designed to equip students with foundational knowledge and essential skills needed for success in college-level chemistry courses. The course covers fundamental concepts such as atomic structure, chemical bonding, stoichiometry, states of matter, and basic chemical reactions. Emphasis is placed on problem-solving, laboratory techniques, and safe handling of chemicals. Through lectures, demonstrations, and hands-on experiments, students will develop a strong understanding of chemical principles and gain confidence in their ability to perform laboratory procedures, interpret data, and apply critical thinking to chemical problems. This course is ideal for students who need to strengthen their background in chemistry before advancing to more complex topics.
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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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) What is the definition of a scientific theory?
A)a brief statement that summarizes past observations and predicts future ones
B)a model that explains the underlying reasons for observations and laws
C)the equivalent of a scientific opinion which others may disagree with
D)a method of learning that emphasizes reason as the way to understand the world
E)none of the above
Answer: B
Q3) Which statement about a hypothesis is TRUE?
A)It is a tentative interpretation or explanation.
B)It has the potential to be proven wrong.
C)It can be tested by experiments.
D)It is part of the scientific method.
E)All of the above statements are true.
Answer: E
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3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) There are exactly 2.54 centimeters in 1 inch.When using this conversion factor,how many significant figures are you limited to?
A)1
B)3
C)ambiguous
D)depends on if you are using it in multiplication/division or addition/subtraction
E)infinite number of significant figures
Answer: E
Q2) The number 7.20 × 10<sup>3</sup> contains three significant figures.
A)True
B)False
Answer: True
Q3) The prefix nano represents the multiplier 0.000000001.
A)True
B)False
Answer: True
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Chapter 3: Matter and Energy
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Sample Questions
Q1) In physical changes,the atoms or molecules that compose the matter do not change their identity,even though the matter may change its appearance.
A)True
B)False
Answer: True
Q2) Even with the most recent advances in microscopy,it is impossible to image an atom.
A)True
B)False
Answer: False
Q3) If a pure material decomposes when heated into simpler substances,this proves that the material was a compound.
A)True
B)False
Answer: True
Q4) An example of a chemical change is burning a wood log to give a pile of ashes.
A)True
B)False
Answer: True
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) How many neutrons are found in Ne-21?
A)11
B)21
C)10
D)0
E)none of the above
Q2) 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
Q3) The only known atom that does not contain a neutron is one of the isotopes of hydrogen.The mass number,symbolized as "A" in the text,of this hydrogen isotope must be:
A)1.01
B)0
C)1
D)2
E)none of the above
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6
Chapter 5: Molecules and Compounds
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Sample Questions
Q1) Which of the following species is a molecular element?
A)neon
B)sodium
C)chlorine
D)carbon dioxide
E)none of the above
Q2) The charge of a vanadium ion in the compound V<sub>2</sub>O<sub>5</sub> is:
A)5+
B)2+
C)10+
D)10-
E)none of the above
Q3) Chemical formulas normally list the most metallic elements first.
A)True
B)False
Q4) If a chemical reaction produces the molecular element oxygen,the formula of oxygen should be written as O<sub>2</sub> .
A)True
B)False
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Chapter 6: Chemical Composition
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Sample Questions
Q1) Calculate the molar mass of calcium nitrate.
A)136.03 g/mol
B)102.09 g/mol
C)132.10 g/mol
D)164.10 g/mol
E)none of the above
Q2) What is the mass percent of Na in sodium chloride?
A)58.4
B)60.7
C)39.3
D)47.5
E)none of the above
Q3) What is the mass percent of carbon in oxalic acid,H<sub>2</sub>C<sub>2</sub>O<sub>4</sub>?
A)2.24
B)13.3
C)26.7
D)34.5
E)none of the above
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) What type of a reaction occurs when a potassium nitrate solution is mixed with a barium acetate solution?
A)precipitation
B)acid-base neutralization
C)oxidation-reduction
D)gas evolution
E)no reaction
Q2) The formation of a new solid or gas is evidence of a chemical reaction.
A)True
B)False
Q3) Considering the following precipitation reaction:
Pb(NO<sub>3</sub>)<sub>2</sub>(aq)+ 2KI(aq)
2KNO<sub>3</sub>(aq)
Which ion(s)would NOT be spectator ions?
A)Pb<sup>2+</sup>,NO<sub>3</sub><sup>-</sup>
B)K<sup>+</sup>,I<sup>-</sup>
C)NO<sub>3</sub><sup>-</sup>,Pb<sup>2+</sup>
D)Pb<sup>2+</sup>,I <sup>-</sup>
E)All the above ions are in the net ionic equation.
PbI<sub>2</sub>(s)+
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Page 9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Consider a reaction of chemicals depicted as A + B C + D.Suppose reaction of 17.8 grams of A with 29.5 grams of B gave 24.7 grams of C.However,the theoretical yield of C for this reaction was 33.3 grams.What was the percent yield of chemical C?
A)74.2
B)47.3
C)11.7
D)135
E)none of the above
Q2) For the following reaction you have 8 grams of hydrogen and 2 grams of oxygen. 2H<sub>2</sub> + O<sub>2</sub> 2H<sub>2</sub>O The limiting reagent is the oxygen.
A)True
B)False
Q3) 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
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) A particle of light is called a packet.
A)True
B)False
Q2) Which of the atoms represented below is the largest in size?
A)N
B)As
C)Sb
D)Bi
E)P
Q3) A red shirt appears red to our eyes because the shirt absorbs the red wavelengths of visible light.
A)True
B)False
Q4) The principal quantum number (n):
A)specifies the 3-D shape of the orbital.
B)specifies the subshell of the orbital.
C)specifies the maximum number of electrons.
D)specifies the principal shell of the orbital.
E)none of the above
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) What is the molecular geometry of SiH<sub>4</sub>?
A)bent
B)linear
C)tetrahedral
D)trigonal pyramidal
E)not enough information
Q2) Which substance listed below is a polar molecule?
A)NH<sub>4</sub><sup>+</sup>
B)Cl<sub>2</sub>O
C)SiCl<sub>4</sub>
D)all of the compounds
E)none of the compounds
Q3) The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:
A)AlBr
B)Al<sub>2</sub>Br
C)AlBr<sub>3</sub>
D)AlBr<sub>2</sub>
E)none of the above
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Page 12
Chapter 11: Gases
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Sample Questions
Q1) Ammonia gas decomposes according to the equation: 2NH<sub>3</sub>(g) N<sub>2</sub>(g)+ 3H<sub>2</sub>(g)
If 15.0 L of nitrogen is formed at STP,how many liters of hydrogen will be produced (also measured at STP)?
A)15.0 L
B)30.0 L
C)45.0 L
D)90.0 L
E)not enough information
Q2) If the volume of a gas container at 32.0°C changes from 1.55 L to 755 mL,what will the final temperature be?
A)149°C
B)353°C
C)273°C
D)-124°C
E)none of the above
Q3) The molar volume of any gas at conditions of standard temperature and pressure is 22.4 liters.
A)True
B)False
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Oil would be considered a nonvolatile liquid while gasoline would be considered volatile.
A)True
B)False
Q2) Viscosity increases with increased intermolecular force because the molecules attract each other strongly which hinders the flow.
A)True
B)False
Q3) Assuming that the molecules carbon monoxide (CO)and nitrogen (N<sub>2</sub>)have similar electron clouds,which statement below is TRUE?
A)CO has the higher boiling point because it experiences dipole-dipole forces.
B)N<sub>2</sub> has the higher boiling point because it experiences dipole-dipole forces.
C)The N<sub>2</sub> has the higher boiling point because it has greater dispersion forces.
D)Both CO and N<sub>2</sub> must have the same boiling point. E)none of the above
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Chapter 13: Solutions
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Sample Questions
Q1) Which of the following substances is NOT a solution?
A)humid air
B)beer
C)oxygen
D)steel
E)All of the above are solutions.
Q2) If the solubility of sodium chloride is 36 grams per 100 grams of water,which of the following solutions would be considered unsaturated?
A)5.8 moles of NaCl dissolved in 1 L of water
B)3.25 moles of NaCL dissolved in 500 ml of water
C)1.85 moles of NaCl dissolved in 300 ml of water
D)none of the above
Q3) The oxygen in the air we breath is classified as:
A)the solute in a homogeneous gas mixture.
B)the solvent in a homogeneous gas mixture.
C)the solute in a heterogeneous gas-liquid mixture.
D)the solvent in a simple mixture.
E)none of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) In general,the stronger the acid,the weaker is its conjugate base.
A)True
B)False
Q2) Aluminum is one of the few metals that dissolves in a strong base.
A)True
B)False
Q3) A Bronsted-Lowry acid is a proton donor.
A)True
B)False
Q4) The burning of fossil fuels produces nitrogen oxides and sulfur oxides which can react to form acid rain (nitric and sulfuric acids).
A)True
B)False
Q5) The sour taste of bases warns humans against eating poisonous alkaloids found in some plants.
A)True
B)False
Q6) The pH of 0.001 M HCl is 3.0.
A)True
B)False
Page 16
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Equilibrium involves the ideas of sameness and constancy.
A)True
B)False
Q2) When writing the expression for an equilibrium constant,which type of substance IS included?
A)solids
B)pure liquids
C)gases
D)all of the above
E)none of these
Q3) A catalyst speeds up a chemical reaction as it is being consumed.
A)True
B)False
Q4) Living things are in equilibrium with their surroundings.
A)True
B)False
Q5) If an equilibrium reaction shifts to the right when the system is cooled,this indicates that the reaction is endothermic.
A)True
B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Assign the oxidation state of each atom in sodium sulfate,Na<sub>2</sub>SO<sub>4</sub>.
A)Na = +1,S = +4,O = -2
B)Na = +1,S = -2,O = +4
C)Na = +2,S = +6,O = -2
D)Na = +1,S = +6,O = -2
E)Na = +2,S = -2,O = 0
Q2) Which battery system is based on half reactions involving zinc metal and manganese dioxide?
A)alkaline batteries
B)fuel cells
C)lead-acid storage batteries
D)dry-cell batteries
E)none of the above
Q3) In an electrochemical cell,which of the following statements is FALSE?
A)The anode is the electrode where oxidation occurs.
B)A salt bridge provides electrical contact between the half-cells.
C)The cathode is the electrode where reduction occurs.
D)A spontaneous electrochemical cell is called a galvanic cell.
E)All of the above are true.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) The combination of two light nuclei to form a heavier one is known as nuclear fission.
A)True
B)False
Q2) In a Geiger-Muller counter,radioactive particles pass through NaI which emits UV-Vis light.
A)True
B)False
Q3) Radioactive particles can pass through matter.
A)True
B)False
Q4) One danger of a nuclear power plant is that a chain reaction could produce a bomb.
A)True
B)False
Q5) Briefly describe the main features of the three types of radiation: alpha,beta,and gamma.Also explain what happens to the nucleus of an atom when it is exposed to each of these.
Q6) Briefly distinguish between nuclear fission and nuclear fusion.
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Alkanes cannot undergo addition reactions because they do not have a multiple bond.
A)True
B)False
Q2) 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
Q3) Aldehydes and ketones both contain a carbonyl group.
A)True
B)False
Q4) Alkynes are compounds with at least one triple bond.
A)True
B)False
Q5) It was originally thought that organic compounds had to come from living things.
A)True
B)False
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Chapter 19: Biochemistry
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Sample Questions
Q1) The complementary base sequence to GTAGCT is:
A)CATCGA.
B)ACGATC.
C)GCAGTA.
D)AGTCGA.
E)none of the above
Q2) The two strands that form the double helix of DNA are held to each other by:
A)peptide bonds.
B)covalent bonds.
C)hydrogen bonds.
D)ester linkages.
E)none of the above
Q3) The human genome project is expected to:
A)help identify people who are susceptible to certain diseases.
B)produce important drugs in the lab by using the blueprint our body provides.
C)help develop new drugs to fight genetic diseases.
D)help understand the genetic basis for intelligence.
E)all of the above
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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