Survey of Chemistry
Midterm Exam
Course Introduction
Survey of Chemistry provides an overview of fundamental chemical concepts and principles for students from various academic backgrounds. The course covers topics such as atomic structure, chemical bonding, stoichiometry, states of matter, solutions, chemical reactions, and introductory organic and biochemistry. Emphasis is placed on understanding the relevance of chemistry in everyday life, developing problem-solving skills, and exploring the impact of chemical processes on society and the environment. This course is designed to offer a broad foundation for students who may not pursue further studies in chemistry but require a general understanding of its applications.
Recommended Textbook
Conceptual Chemistry 5th Edition by John A. Suchocki
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Chapter 1: About Science
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Sample Questions
Q1) Which of the following would be considered applied research?
A)determining the lightest and strongest metal to be used for an airplane wing
B)testing the strength of a piece of metal
C)determining the melting temperature of a metal
D)examining how susceptible a metal is to bending
E)determining how readily a metal corrodes in a wet environment
Answer: A
Q2) Which statement is false?
A)We have the technology to solve world hunger.
B)We have the technology to solve the world's energy needs.
C)We have the technology to develop global communication.
D)We lack the technology to solve most of the Earth's environmental problems.
Answer: D
Q3) Scientific research usually leads to ________.
A)expected results
B)the discovery of new questions
C)social well-being
D)inconclusive results
Answer: B
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Page 3
Chapter 2: Particles of Matter
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Sample Questions
Q1) Which temperature is the hottest?
A)100°C
B)100 K
C)100°F
D)They are all equal.
E)none of the above
Answer: A
Q2) Why is it not possible for the scanning probe microscope (SPM)to make images of the inside of an atom?
A)The most representative "image" of the inside of the atom would be a picture of empty space.
B)The SPM works by passing a current across a tiny gap between the tip of an ultrathin needle and the surface being studied. No gap, no image.
C)The SPM ultrathin needle itself is made of atoms and so is not tiny enough to pierce through an atom much like a sewing needle can pierce into a Ping-Pong ball.
D)All of the above are reasonable answers.
Answer: D
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4
Chapter 3: Elements of Chemistry
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Sample Questions
Q1) Germanium, Ge (number 32), computer chips operate faster than silicon, Si (number 14), computer chips. So how might a gallium, Ga (number 31), chip compare with a germanium chip?
A)A gallium chip would be even faster because the gallium is more metallic.
B)A gallium chip would be slower because its electrons are more loosely held.
C)Gallium is located just below aluminum, which is widely known to be an electrical insulator.
D)Gallium is more nonmetallic and so it does not conduct electrons very well.
Answer: A
Q2) Someone argues that he or she doesn't drink tap water because it contains thousands of molecules of some impurity in each glass. How would you respond in defense of the water's purity, if it indeed does contain thousands of molecules of some impurity per glass?
A)Impurities aren't necessarily bad, in fact, they may be good for you.
B)The water contains water molecules and each water molecule is pure.
C)There's no defense. If the water contains impurities it should not be drunk.
D)Compared to the billions and billions of water molecules, a thousand molecules of something else is practically nothing.
Answer: D
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Chapter 4: Subatomic Particles
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Sample Questions
Q1) The ________ represents the complete range of frequencies of light energy from radio waves to gamma rays.
A)electromagnetic spectrum
B)electron configuration
C)probability cloud
D)frequency dependence
E)spectroscopic model
Q2) If you remove two protons and two electrons from a sulfur atom (S), what new element is formed?
A)Si
B)Si<sup>+2</sup>
C)Al<sup>+2</sup>
D)Al
E)Ar<sup>-</sup><sup>2</sup>
Q3) Which of the following statements describes an isotope?
A)element with the same number of protons but a different number of neutrons
B)element with the same number of protons but a different number of electrons
C)element with the same number of neutrons but a different number of electrons
D)element with the same number of neutrons but a different number of protons
E)none of the above
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Chapter 5: The Atomic Nucleus
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Sample Questions
Q1) Is the mass of an atomic nucleus greater or less than the sum of the masses of the nucleons composing it? Why don't the nucleon masses add up to the total nuclear mass?
A)Greater. We need to add the masses of the surrounding electrons to the masses of the nucleons.
B)Neither. The mass of the atomic nucleus is exactly the sum of the masses of the nucleons.
C)Less. The individual nucleons have greater mass when separated from the nucleus. This additional mass is a result of the energy of separation.
D)Greater. The mass of the atomic nucleus also has mass of the "atomic glue" that holds the nucleons together in the nucleus.
Q2) If three samples have the half-lives listed below, which is the most radioactive?
A)a sample with a half-life of 20 minutes
B)a sample with a half-life of 20 hours
C)a sample with a half-life of 20 years
D)a sample with a half-life of 20 million years
E)none of the above
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Chapter 6: How Atoms Bond
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Sample Questions
Q1) Which of the following describes the reason for the following application of metals? designer jewelry
A)do not conduct heat well
B)conduct electricity
C)are shiny
D)are strong but can be bent
E)c and d
Q2) Which molecule is most polar?
A)S=C=S
B)O=C=O
C)O=C=S
D)These all have the same polarity.
Q3) Which of the following molecules would contain a dipole?
A)H-F
B)Cl-Cl
C)H-H
D)F-F
E)all of the above
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8
Chapter 7: How Molecules Mix
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Sample Questions
Q1) Which of the following material phases cannot form a solution?
A)solids
B)liquids
C)gases
D)All of the above can form solutions.
E)None of the above can form solutions.
Q2) Many solvents expand to occupy greater volumes with increasing temperature. What happens to the concentration of a solution made with such a solvent as its temperature is increased?
A)Since concentration depends on how much mass is dissolved in a given volume, as the volume increases, the concentration decreases.
B)The concentration of a solution increases as the solute fits into the new spaces between the molecules.
C)Since it has a greater ability to dissolve more solute at a higher temperature, its concentration has decreased.
D)Since it has a greater ability to dissolve more solute at a higher temperature, its concentration has increased.
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Chapter 8: How Water Behaves
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Sample Questions
Q1) From the diagram above describing the phase of xenon relative to temperature and pressure which is more dense: liquid xenon or solid xenon?
A)solid
B)liquid
C)The density of xenon is the same in both the solid and liquid phase.
D)Density information can not be determined from the diagram.
Q2) If the heat of melting of a sample is 135 J/g, what would the heat of freezing for the sample be?
A)-135 J/g
B)135 J/g
C)The heat depends on the mass.
D)The heat depends on the temperature.
E)The heat of freezing is unrelated to the heat of melting.
Q3) An adhesive force is best described as ________.
A)attraction between two liquid molecules
B)attraction between a liquid molecule and a solute
C)the force that allows for molecular adhesion
D)the force that holds together the nucleus
E)attraction between two different molecules
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Page 10
Chapter 9: How Chemicals React
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Sample Questions
Q1) Which of the following has the greatest mass?
A)1 mole of Pb
B)1 mole of H<sub>2</sub>
C)1 mole of Be
D)1 mole of Na
E)All have the same mass.
Q2) In a chemical reaction, the bonds being formed are ________.
A)the same as the ones broken
B)different from the ones broken
C)more energetic than the ones broken
D)less energetic than the ones broken
Q3) For the following balanced equation, which has the highest coefficient? 4
H<sub>2</sub> + 2 C 2 CH<sub>4</sub>
A)H<sub>2</sub>
B)C
C)CH<sub>4</sub>
D)H<sub>4</sub>
E)none of the above
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Chapter 10: Acids and Bases in Our Environment
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Sample Questions
Q1) What would the concentration of OH<sup>-</sup> be if the concentration of H<sub>3</sub>O<sup>+</sup> was 1 × 10<sup>-5</sup>M? [H<sub>3</sub>O<sup>+</sup>] × [OH<sup>-</sup>] = K<sub>w </sub>= 1 × 10<sup>-14</sup>
A)1 × 10<sup>-14</sup>
B)1 × 10<sup>-5</sup>
C)1 × 10<sup>9</sup>
D)1 × 10<sup>5</sup>
E)1 × 10<sup>-9</sup>
Q2) As the pH increases, the hydroxide ion concentration ________.
A)goes down
B)gets larger
C)starts to affect the H<sup>+</sup> concentration
D)starts to decrease because it is reacting with the excess hydronium ions
E)stays constant
Q3) Which of the following solutions is the most acidic?
A)a solution with a pH = 14
B)a solution with a pH = 10
C)a solution with a pH = 7
D)a solution with a pH = 4
E)All of the solutions are basic.
Page 12
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Chapter 11: Oxidations and Reductions Charge the World
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Sample Questions
Q1) What is oxidation?
A)the loss of electrons
B)the reaction with oxygen
C)the reduction of oxygen
D)the gaining of electrons
E)the addition of an electron to the valence shell
Q2) The following set of redox reactions takes place between iron dipped in a solution of copper ions. Fe Fe<sup>2+</sup> + 2e-
Cu<sup>2+</sup> + 2e- Cu
Which of the following describes what is happening on the surface of the iron?
A)The copper starts to plate out on iron.
B)The iron rusts in the water.
C)The iron starts to plate out on the copper.
D)The iron corrodes the copper.
E)none of the above
Q3) The elements that make the best reducing agents are the ________.
A)group 18 noble gases
B)group 17 halogens
C)transition metals
D)group 1 alkali metals
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Chapter 12: Organic Compounds
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Sample Questions
Q1) Why is a phenol more acidic than a regular alcohol?
A)Phenols have the ability to spread out the negative charge that forms.
B)Phenols have the ability to readily accept the positive charge of the proton.
C)The negative charge is very concentrated on the oxygen ring of the phenol.
D)The phenol has more negative charge and therefore is more stable.
E)Phenols are not more acidic than a regular alcohol.
Q2) What is a functional group?
A)a set of atoms bonded together that give molecules containing them similar properties
B)a group that adds function
C)a group of hydrocarbons that can be used to make new materials
D)a set of molecules that are grouped together to form a functional material
E)none of the above
Q3) Which of the above molecules would you use to make an amide?
A)a
B)b
C)c
D)d
E)a or d
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Page 14
Chapter 13: Nutrients of Life
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Sample Questions
Q1) Two proteins joining together to form a larger protein complex describes a
A)primary structure
B)secondary structure
C)tertiary structure
D)quaternary structure
Q2) The following statement describes what level of structure in a protein? Several separate proteins link together to form an active enzyme.
A)primary structure
B)secondary structure
C)tertiary structure
D)quaternary structure
E)none of the above
Q3) What is the purpose of the plasma membrane?
A)It acts as a boundary, but also lets molecules in and out.
B)It acts as a cell wall to give the cell structure and support.
C)It keeps water in the cell to keep it from dehydrating.
D)It stores the genetic material of the cell.
E)none of the above
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Chapter 14: Medicinal Chemistry
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Sample Questions
Q1) How is a set of neurons different from a wire conductor?
A)Neurons do not need to physically touch to conduct.
B)Wires are made of metal.
C)One conducts electricity; the others do not.
D)The wire can carry more information.
E)all of the above
Q2) Where are antibiotics obtained?
A)molds
B)fungi
C)bacteria
D)all of the above
E)only A and B
Q3) Ethyl alcohol is ________.
A)a stimulant
B)a depressant
C)an opioid
D)all of the above
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Chapter 15: Optimizing Food Production
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Sample Questions
Q1) What is a similarity between pesticides and medical drugs?
A)They need to selectively target the invader but not harm the host.
B)They have to have a minimum amount of side effects.
C)They should be readily decomposed into non-harmful byproducts.
D)all of the above
E)only A and B
Q2) What feature, besides their ability to kill insects, makes chlorinated hydrocarbons like DDT attractive as an insecticide?
A)They are not water soluble.
B)They do not degrade rapidly.
C)They accumulate in fat.
D)all of the above
E)only A and B
Q3) Plants need nitrogen primarily so that they can build ________.
A)carbohydrates
B)lipids
C)amino acids
D)vitamins
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Chapter 16: Protection Water and Air Resources
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Sample Questions
Q1) How is global temperature estimated from ice samples?
A)by looking at the types of gases dissolved in the ice
B)by measuring the density of the ice
C)by measuring the depth of the ice
D)by looking at the pollen trapped in the air pockets in the ice
E)none of the above
Q2) Would you expect a can of warm soda or other carbonated beverage to foam more or less while flying on a airplane?
A)The amount of foam would decrease.
B)The amount of foam would increase.
C)The amount of foam would be the same.
D)Airplanes are pressurized so there is no change in pressure.
E)none of the above
Q3) Which of the following statements about natural waters is untrue?
A)The microorganisms in fresh water are harmful.
B)Microorganisms help replenish the nutrients in the water.
C)Aerobic bacteria only decompose organic matter in the presence of oxygen.
D)all of the above
E)only a and b
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Page 18
Chapter 17: Capturing Energy
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Sample Questions
Q1) What are some disadvantages of producing ethanol by fermenting food biomass?
A)It is a waste of good food.
B)It could destabilize the world oil market.
C)It is a rather costly process.
D)all of the above
Q2) Which of the following has a typical peak power output of about 1,500 megawatts?
A)a coal-fired power plant
B)a hydroelectric dam
C)a nuclear reactor
D)a fusion reactor
E)All of the above have the same capacity.
Q3) Where does the chemical energy in fossil fuels ultimately come from?
A)solar radiation
B)the soil
C)wind energy
D)nuclear fission
E)none of the above
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