Course Introduction
Introduction to Chemistry Exam
Questions
Introduction to Chemistry provides students with a foundational understanding of the principles and concepts underlying the science of matter. Topics covered include atomic structure, periodic trends, chemical bonding, stoichiometry, states of matter, chemical reactions, and the basics of thermochemistry and equilibrium. Through lectures, laboratory experiments, and problem-solving exercises, students develop critical thinking and scientific skills essential for further study in chemistry and related disciplines. This course is designed for those new to chemistry, preparing them for more advanced coursework in the physical sciences and allied health fields.
Recommended Textbook
Conceptual Chemistry 5th Edition by John A. Suchocki
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2174 Verified Questions
2174 Flashcards
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Page 2
Chapter 1: About Science
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Sample Questions
Q1) Which of the following would not be considered matter?
A) light
B) trees
C) air
D) clouds
E) rain
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) The American Chemistry Council is ________.
A) a society of chemistry educators
B) a special interest group
C) an organization of environmental lawyers
D) an advisory panel to the U.S. Congress
Answer: B
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Page 3
Chapter 2: Particles of Matter
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Sample Questions
Q1) 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
Q2) Which of the following is an example of something with potential energy?
A) a boulder at the top of a cliff
B) an arrow poised in a stretched bow
C) chemical bonds
D) gasoline in the gas tank of your car
E) all of the above
Answer: E
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Chapter 3: Elements of Chemistry
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Sample Questions
Q1) The probe tip of a scanning probe microscope ________.
A) floats above the atoms of a sample
B) etches into the atoms of a sample
C) chemically changes the atoms of a sample
D) injects a magnetic field into the atoms of a sample
Answer: A
Q2) Which chemical family is composed almost entirely of synthetic elements?
A) the actinides
B) the lanthanides
C) the halogens
D) all of the above
E) none of the above
Answer: A
Q3) Which of the following is a mixture?
A) air
B) gold
C) salt
D) iron
E) helium
Answer: A
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Chapter 4: Subatomic Particles
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Sample Questions
Q1) In Rutherford's gold foil experiment, alpha particles ________.
A) passed through the atomic nucleus
B) touched the atomic nucleus
C) were deflected by the atomic nucleus
D) were invisible to the atomic nucleus
Q2) Which of the following could best be represented by a physical model?
A) a cell
B) an atom
C) rationality
D) ecosystem
E) both A and B
Q3) Which experiences a greater effective nuclear charge, an electron in the outer shell of neon (atomic number 10) or an electron in the outer shell of sodium (atomic number 11)?
A) sodium because it contains more protons
B) neon because of less inner shell shielding
C) sodium because it contains a greater number of shells
D) neon because it is a smaller atom
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6
Chapter 5: The Atomic Nucleus
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Sample Questions
Q1) Why wouldn't you use carbon-14 dating on a piece of shell that was estimated to be 1 million years old?
A) Sea shells do not have radioisotopes.
B) Carbon dating is only useful on plants.
C) Uranium dating is better for items older than 1/2 million years.
D) Carbon dating can only be used on items that were once alive.
E) The amount of radioactive carbon in the sample would probably too small to measure.
Q2) A shorter half-life means that a radioactive substance is relatively ________.
A) stable
B) unstable
C) difficult to detect
D) common
Q3) Which of the following statements about radiation is true?
A) Your body contains a number of radioactive isotopes.
B) One rem is enough to kill approximately 50 percent of the average population.
C) Radiation damages cells beyond repair.
D) Radiation can make you glow in the dark.
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Chapter 6: How Atoms Bond
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Sample Questions
Q1) Three kids sitting equally apart around a table are sharing jelly beans. One of the kids named Billy, however, tends only to take jelly beans and only rarely gives one away. If each jelly bean represents an electron, who ends up being slightly negative? Who ends up being slightly positive?
A) Billy ends up being slightly negative, while the two other kids are both slightly positive.
B) Billy ends up being slightly positive, while the two other kids are both slightly negative.
C) One of the two kids other than Billy ends up slightly negative, but Billy and the third kid will both end up slightly positive.
D) One of the two kids other than Billy ends up slightly positive, but Billy and the third kid will both end up slightly negative.
Q2) What does the line in the following example actually represent? H-H
A) a shared pair of electrons
B) a covalent bond
C) an ionic bond
D) a pair of nonbonding electrons
E) A and B
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Chapter 7: How Molecules Mix
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Sample Questions
Q1) How many moles of sugar, C<sub>12</sub>H<sub>22</sub>O<sub>11</sub>, are there in 200. grams?
A) 0.585 moles
B) 68,400 moles
C) 1.71 moles
D) 0.684 moles
Q2) What is the molarity of 0.50 liters of a solution with five moles of sucrose in it?
A) 10. molar
B) 0.5 molar
C) 5 molar
D) 2.5 molar
E) 1 molar
Q3) Why is a large quantity of water used in industrial processes in the U.S. purified by desalinization?
A) The sources are brackish or metal ion rich.
B) The sources are ocean water.
C) There is not enough fresh water.
D) It is less expensive than using fresh water.
E) none of the above
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Page 9
Chapter 8: How Water Behaves
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Sample Questions
Q1) Given the following specific heats and that each sample had the same mass, which would require the greatest amount of heat energy to increase its temperature 50°C?
A) ammonia, 4.70 J/(g°C)
B) water, 4.184 J/(g°C)
C) aluminum, 0.90 J/(g°C)
D) silver, 0.24 J/(g°C)
E) All of the above require the same amount of heat energy.
Q2) Which of the following contains the most heat energy?
A) 1 gram of steam at 100°C
B) 1 gram of water at 100°C
C) 1 gram of water at 50°C
D) 1 gram of water at 0°C
E) 1 gram of ice at 0°C
Q3) What happens when pressure is applied to ice crystals?
A) The regular arrangement of the ice is disrupted and the ice melts.
B) The temperature rises and the ice melts.
C) The regular arrangement of ice causes it to harden.
D) The freezing temperature of the molecules decreases.
E) The volume occupied by the material increases.
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Page 10
Chapter 9: How Chemicals React
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Sample Questions
Q1) Is it possible to have a macroscopic sample of oxygen that has a mass of 14 atomic mass units?
A) Yes, but it would need to be made of oxygen atoms that each had less than the normal number of neutrons.
B) No, this is less than than the mass of a single oxygen atom.
C) Yes, but it would have the same density as nitrogen.
D) No, because oxygen is a gas at room temperature.
Q2) What is the mass of an oxygen atom, O, in atomic mass units?
A) 12 amu
B) 16 amu
C) 18 amu
D) 32 amu
Q3) What is a chemical equation?
A) It is a shorthand notation for illustrating a chemical reaction.
B) It is the sum of the masses of the products and reactants.
C) It is the chemical combination of equal numbers of reactants and products.
D) It is a picture of the atoms undergoing a chemical equalization.
E) It is any type of reaction that takes place at the equator.
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Chapter 10: Acids and Bases in Our Environment
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Sample Questions
Q1) Which of the above illustrations shows a neutral aqueous solution?
A) A
B) B
C) C
D) All of the above are neutral solutions.
E) none of the above
Q2) If you had a 1 M solution of a strong base what would be its pH?
A) 1
B) 6
C) 7
D) 8
E) 13
Q3) For the following reaction, identify whether the compound in bold is behaving as an acid or a base. H<sub>3</sub>PO<sub>4</sub> + H<sub>2</sub>O H<sub>2</sub>PO<sub>4</sub><sup>-</sup> + H<sub>3</sub>O<sup>+</sup>
A) acid
B) base
C) neither
D) both
E) none of the above
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Chapter 11: Oxidations and Reductions Charge the World
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Sample Questions
Q1) In an operating photovoltaic cell, electrons move through the external circuit to the negatively charged p-type silicon wafer. How can the electrons move to the negatively charged silicon when they themselves are negatively charged? Don't like signs repel each other?
A) This is a technological hurdle that has greatly inhibited the advancement of photovoltaic technology.
B) An electric current is possible because the energy from the sun momentarily reverses the charge of the electrons, which are then called positrons (p-type).
C) The p-type silicon wafer is actually positively charged.
D) The energy of the sunlight knocks the electrons into a direction that they would otherwise not go.
Q2) How does a blast furnace work?
A) A reductant is added that reacts with oxygen atoms at high temperature.
B) The high temperature reduces the metal.
C) The high temperature oxidizes the metal
D) An oxidant is added that reacts with iron atoms at high temperature.
E) none of the above
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Chapter 12: Organic Compounds
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Sample Questions
Q1) Which of the above molecules would you use to make an amide?
A) a
B) b
C) c
D) d
E) a or d
Q2) If an alcoholic beverage is 20 percent alcohol by volume, what is its proof?
A) 40 proof
B) 20 proof
C) 10 proof
D) Proof is a measure of flammability.
E) Proof is a measure of the age of a fermented beverage.
Q3) Which of the above molecules is an alcohol?
A) a
B) b
C) c
D) d
E) a and d
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Chapter 13: Nutrients of Life
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Sample Questions
Q1) Cold cereal is often fortified with all sorts of vitamins and minerals but is deficient in the amino acid lysine. How might this deficiency be compensated for?
A) eat a peanut butter sandwich at lunch
B) have beans with your dinner
C) pour milk on your cereal
D) all of the above
Q2) The cells of your body are about as small as ________.
A) the head of an ant
B) the point of a sewing needle
C) a water molecule
D) the nucleus of an atom
Q3) Which of the following plays the most active role in protein manufacture?
A) DNA
B) RNA
C) genes
D) nucleotides
E) none of the above
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Chapter 14: Medicinal Chemistry
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Sample Questions
Q1) Why is methadone not very useful in the treatment of cocaine addiction?
A) Methadone is a stimulant, which is the opposite of what is needed for the treatment of cocaine addiction.
B) Methadone is not readily available "on the streets" and so the cocaine user might have a hard time finding any.
C) Methadone blocks the action of cocaine, which means the user's withdrawal symptoms would be too dramatic.
D) Methadone provides only a depression of nerve signals, which is opposite of what the cocaine addict is seeking.
Q2) What is an advantage of synaptic clefts between neurons rather than direct connections?
A) It allows the body to regulate the passage of nerve impulses.
B) It allows for nerve signals to travel faster from one neuron to the next.
C) It makes it so that the neurons need not be extremely long.
D) It allows neurons to change their connections to other neurons.
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Chapter 15: Optimizing Food Production
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Sample Questions
Q1) Why do slowly degraded molecules like DDT have a tendency to accumulate in creatures higher in the food chain?
A) Since it takes more energy to feed a large animal, they take in more of the toxin.
B) Since things higher on the food chain are large they have more fat, which means they can store more of the toxin.
C) Larger animals do not excrete toxins as efficiently as smaller animals.
D) Carnivores do not have the needed enzyme to biodegrade the toxin that herbivores have.
E) none of the above
Q2) Which of the following soil horizons is the deepest?
A) substratum
B) subsoil
C) topsoil
D) bottom soil
E) humus
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17
Chapter 16: Protection Water and Air Resources
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Sample Questions
Q1) 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
Q2) Water consumption from all aquifers, on average, is less than the amount of water returned to the aquifer by natural processes. Why should we worry about water use?
A) The average amount does not reflect that drier areas have a harder time refilling the aquifers.
B) Because the water returned is contaminated.
C) The average amount does not take into account the water consumed during photosynthesis to make carbohydrates.
D) Water is nothing to worry about.
E) none of the above
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18
Chapter 17: Capturing Energy
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Sample Questions
Q1) How is it that here on the Earth we can derive energy from the Moon, which is 400 thousand kilometers away?
A) We can gather radiation from the Moon.
B) We can take advantage of the tidal forces between the Earth and the Moon.
C) We can utilize the interaction between the Earth and the Moon's magnetic fields.
D) We can collect moon rocks high in plutonium.
Q2) Which of the following methods can produce a net output of fusion energy?
A) using a fission reaction to generate the heat needed to start a fusion reaction
B) using lasers to crush and fuse fuel pellets
C) using very strong magnetic fields to contain star-hot atoms
D) using electromagnetic compression waves to detonate fuel pellets
E) none of the above
Q3) In 2010, the world's leading producer of ethanol was ________.
A) Brazil
B) the Pacific Ocean
C) the United States
D) China
E) Nigeria
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19