Fundamentals of Chemistry Exam Preparation Guide - 1151 Verified Questions

Fundamentals of Chemistry Exam Preparation Guide

Course Introduction

Fundamentals of Chemistry provides an introduction to the basic principles and concepts of chemistry, serving as a foundation for further study in the field. This course covers the structure of atoms, chemical bonding, the periodic table, states of matter, chemical reactions, stoichiometry, and the properties of solutions. Emphasis is placed on developing problem-solving skills, understanding chemical equations, and exploring the practical applications of chemistry in everyday life. Students will gain hands-on experience through laboratory experiments, enhancing their comprehension of theoretical concepts and fostering analytical thinking.

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CHEM2 Chemistry in Your World 2nd Edition by Hogg

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Chapter 1: Living in a World of Chemistry

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Sample Questions

Q1) The discovery of Teflon® was A) an example of planned research.

B) accidental

C) eventually damaging to the ozone layer.

D) deemed useless by the discoverer's company.

Answer: B

Q2) A scientist is trying to make a new insecticide that will be more toxic to flies, but less toxic to humans than insecticides now available. The scientist is engaged in A) basic research.

B) applied research.

C) technology.

D) serendipity.

Answer: B

Q3) Chemistry is often defined as the study of A) matter and the changes it can undergo.

B) naturally occurring matter.

C) fundamental particles in research labs.

D) synthetically produced matter.

Answer: A

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Chapter 2: The Chemical View of Matter

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Sample Questions

Q1) How does the known number of nonmetals compare to that of metals?

A) There are fewer metals.

B) There are an equal number of each.

C) There are fewer nonmetals.

D) This cannot be predicted because not all metals and nonmetals have been discovered.

Answer: C

Q2) The most common unit of volume used in chemistry is the millimeter.

A)True

B)False

Answer: False

Q3) How many phosphorus atoms are in the formula H₃PO₄?

A) 4

B) 3

C) 7

D) 1

Answer: D

Q4) Mg is the chemical symbol for ____________________.

Answer: magnesium

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Chapter 3: Atoms and the Periodic Table

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Q1) An element with electronic structure of 2-8-3 is in which of the following groups of the periodic table?

A) 1

B) 2

C) 3

D) 4

Answer: C

Q2) Two atoms which have the same atomic number but different mass numbers are called

A) sisters.

B) neutrinos.

C) allotropes.

D) isotopes.

Answer: D

Q3) Which is the ground state of a hydrogen atom?

A) three electrons in the n = 1 level

B) one electron in the n = 2 level

C) one electron in the n = 1 level

D) one electron in the n = 1 level and one electron in the n = 2 level

Answer: C

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Chapter 4: The Air We Breathe

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Q1) The primary source of global SO₂ in the atmosphere is believed to be

A) forest fires.

B) human activity.

C) volcanoes.

D) forests.

Q2) Which substance would be present in the greatest concentration during the morning rush hour on a smoggy day in Los Angeles?

A) NO

B) O₃

C) NO₂

D) SO₃

Q3) Identify the pair that are allotropes.

A) pencil lead and a diamond

B) oxygen gas and nitrogen gas

C) gold and silver

D) mercury and bromine

Q4) The ozone layer is labeled with the number ______.

Q5) Nitrogen and oxygen are the most abundant gases in the atmosphere.

A)True

B)False

6

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Chapter 5: Chemical Bonding and States of Matter

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Q1) Which atom exists as a diatomic molecule in nature?

A) carbon

B) bromine

C) sulfur

D) phosphorous

Q2) When Na and O combine the bonding will be ionic, while when O combines with S the bonding will be covalent.

A)True

B)False

Q3) Most substances that have molecules with approximately the same weight as water molecules are gases at room temperature. Water is a liquid at room temperature because of

A) extensive hydrogen bonding between water molecules.

B) ionic bonding between hydrogen ions and oxide ions.

C) covalent bonding between hydrogen atoms and oxygen atoms.

D) the lack of motion of water molecules.

Q4) If X was the element K and Y the element O, which type of bond would form?

Q5) The total number of bonding electron pairs in hexane is____________.

Q6) The total number of single bonds in hexane is__________.

Q7) Which type of bond would be found in hydrochloric acid, HCl?

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Chapter 6: Carbon Dioxide and the Greenhouse Effect

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Sample Questions

Q1) The concentration of N₂O given in the table is equivalent to ________ppm.

Q2) Which arrow or sets of arrows do not represent only IR radiation?

A)A

B)B

C)C

D)D

Q3) The concentration of O₃ given in the table is equivalent to ________ppb.

Q4) How are carbon dioxide concentrations determined from thousands of years ago?

A) analysis of decayed plant material

B) analysis of ice samples

C) analysis of the atmosphere

D) analysis of the Earth's core

Q5) What substance naturally found in the atmosphere seems to be increasing in concentration over the years?

A) oxygen

B) nitrogen

C) carbon dioxide

D) carbon monoxide

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Chapter 7: Chlorofluorocarbons and the Ozone Layer

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Sample Questions

Q1) Which molecule is used as a replacement for CFC?

A) HFC-134a

B) HCFC-123

C) HFC-152a

D) all of the above

Q2) In the past, which of the following was not a source of atmospheric CFCs?

A) air-conditioning

B) aerosol sprays

C) refrigerants

D) blown foams

E) All of the above have been sources of atmospheric CFCs.

Q3) What does one Dobson unit (DU) equal?

A) 1 ppb of ozone

B) 1 ppm of ozone

C) 100 ppb of ozone

D) 100 ppm of ozone

Q4) In order to attain a steady state one reaction must counteract another in a cycle such as that shown. A reaction which could be used to consume ozone is reaction_______.

Q5) The reaction requiring a photon of the longest wavelength is reaction ______.

Page 9

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Chapter 8: Chemical Reactivity: Chemicals in Action

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Sample Questions

Q1) According to the first law of thermodynamics,

A) Energy is neither lost nor gained in an energy transformation.

B) Perpetual motion is possible.

C) Energy is not conserved.

D) Energy is being created as time passes.

Q2) Consider the following two statements.

"Energy can be converted from one form to another but cannot be destroyed nor created."

"The total amount of matter and energy in the universe is constant."

Both of these are included in the first law of thermodynamics.

A)True

B)False

Q3) How many moles are in 15.5 g of diphosphorous pentoxide?

A) 0.109 mol

B) 0.330 mol

C) 6.56 \(\times\) 10²³mol

D) 2.20 \(\times\) 10³mol

Q4) E_act is represented by the letter_______.

Q5) The reactants are represented by the letter _______.

Page 10

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Chapter 9: Acid-Base Reactions

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Sample Questions

Q1) What is the pH of a 0.00125 M NaOH solution?

A) 2.90

B) 11.1

C) 12.5

D) 1.25

Q2) Which one of the following is the acid in vinegar?

A) acetic acid

B) citric acid

C) muriatic acid

D) ascorbic acid

Q3) When H₂SO₃ dissolves in water, what are the solute particles in the solution?

A) H, S, O

B) H⁺, S⁺ and O^2-

C) H⁺, HSO₃^- and SO₃^2-

D) H₂²⁺ and SO₃^2-

Q4) The formula for the hydroxide ion is OH⁺.

A)True

B)False

Q5) A solution with a pH of 5.05 is ___________.

Page 11

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Chapter 10: Oxidation-Reduction Reactions

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Sample Questions

Q1) The oxidizing agent is found in compartment ______.

Q2) Free radicals are particles that

A) have an unpaired electron.

B) act as oxidizing agents.

C) grab another electron from a neighboring molecule.

D) all of the above

Q3) Which of the following equations does not fit the definition of oxidation?

A) Ag⁺ + e^- \(\to\) Ag

B) C₂H₆ \(\to\) H₂ + C₂H₄

C) C + O₂ \(\to\) CO₂

D) Na \(\to\) Na⁺ + e^-

Q4) Which of the batteries listed below is a primary battery?

A) lithium ion battery

B) alkaline battery

C) nickel-cadmium battery

D) lead acid battery

Q5) The electrons flow from electrode _____ to electrode _____.

Q6) The reducing agent in the following reaction is ___________. I₂ + Zn \(\to\) 2I^- + Zn²⁺

Page 12

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Chapter 11: Water, Water Everywhere but Not a Drop to Drink

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Sample Questions

Q1) Letter ____ shows the position of an aquifer.

Q2) The disinfectant widely used in Europe to kill harmful bacteria in water treatment plants is

A) bromine.

B) oxygen.

C) ozone.

D) sodium hypochlorite.

Q3) Biochemical oxygen demand (BOD) is

A) high for polluted water.

B) low for polluted water.

C) not affected by water pollution.

D) a measure of the amount of oxygen in the body.

Q4) Which of the following pollutants does not contribute to acid rain?

A) SO₂

B) NO₂

C) CO₂

D) O₃

Q5) Precipitation with a pH of 8.0 would classify as acid rain.

A)True

B)False

13

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Chapter 12: Energy and Hydrocarbons

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Sample Questions

Q1) The number of carbon to hydrogen single bonds that are broken is_______.

Q2) Which hydrocarbon would be isolated at the top of a fractionation column?

A) C₅H₁₂

B) C₁₀H₂₂

C) C₃H₈

D) C₁₈H₃₆

Q3) Which substance is grain alcohol?

A) methanol

B) ethanol

C) MTBE

D) benzene

Q4) Which process is used to increase the amount of the gasoline fraction in refining to match commercial demand?

A) reforming

B) oxygenating

C) cracking

D) gasification

Q5) During the combustion of one mole of ethanol, the number of O-H bonds formed is

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Chapter 13: Nuclear Changes and Nuclear Power

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Sample Questions

Q1) Cobalt-60

A) is used to treat cancerous tumors.

B) decays to both beta particles and gamma rays.

C) is a relatively stable isotope.

D) All of the above characterize cobalt-60.

Q2) Gamma radiation from cobalt-60 or cesium-137 is used in

A) agricultural research.

B) dating charcoal paintings.

C) food irradiation.

D) medical imaging.

Q3) Which of the following characterizes an alpha particle?

A) is more penetrating than a gamma ray

B) is attracted to the negitively charge plate in an electric field

C) carries a negative charge

D) is composed of electrons

E) Two of the above are corrected.

Q4) If a 500. mg sample of element X had been used, _____mg would remain after 60 hours.

Q5) The half-life of element X is _____hours.

Q6) After 20 hours, ______mg of sample X will remain.

Page 15

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Chapter 14: Organic Chemicals and Polymers

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Sample Questions

Q1) Ethylene glycol, a dialcohol, is the main ingredient in A) tobacco humectants.

B) antifreeze.

C) denaturated alcohol.

D) gasohol.

Q2) An addition polymer that finds use in fibers for rugs and fabrics is

A) polypropylene.

B) PVC.

C) nylon.

D) polyacrylonitrile.

Q3) What is the role of an organic peroxide in the polymerization of ethylene?

A) The peroxide is a copolymer.

B) The peroxide forms free radicals that initiate attack of double bonds.

C) The peroxide destroys free radicals which would stop the reaction.

D) The peroxide moderates the speed of the reaction, allowing for a more orderly process.

Q4) The type of functional group shown is this structure is called a_______________.

Q5) In the manufacture of vulcanized rubber, sulfur is used to form cross-links.

A)True

B)False

Page 16

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Chapter 15: The Chemistry of Life

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Sample Questions

Q1) Natural amino acids are L-amino acids and natural sugars are D-sugars.

A)True

B)False

Q2) The structure of a tripeptide is Ala-Ser-Aly. What are the expected elements present in the tripeptide?

A) C, H, N, O

B) C, H

C) C, H, N

D) C, H, O

Q3) The energy reservoir in animals is

A) starch.

B) dextrin.

C) glucose.

D) glycogen.

Q4) The secondary structure of proteins is

A) the amino acid sequence of amino acids in the polypeptide chain.

B) the helical structure.

C) the sheetlike structure.

D) the preferred conformation of a given protein.

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Chapter 16: Nutrition: the Basis of Healthy Living

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Sample Questions

Q1) A flavor enhancer is

A) MSG.

B) BHT.

C) an enzyme.

D) beta-carotene.

Q2) Which of the following vitamins is an antioxidant?

A) vitamin A

B) vitamin B

C) vitamin K

D) vitamin E

Q3) Which of the following foods produces more energy per gram of food?

A) sugar

B) fat

C) protein

D) starch

Q4) Which is an example of a sequestrant?

A) EDTA

B) DTT

C) vitamin C

D) MSG

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Chapter 17: Chemistry and Medicine

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Sample Questions

Q1) A new substance is synthesized in the laboratory. Among its properties is similarity to uracil. When tested in living organisms, this new substance gets involved in DNA synthesis. Which area of research would you expect this new chemical to show promise?

A) studying Reye's syndrome

B) studying how analgesics work

C) studying anticancer drugs

D) studying how antacids work

Q2) LD₅₀ refers to the dosage that is lethal to one-half of the test animal population.

A)True

B)False

Q3) In all age groups, the leading cause of death at about 26% is A) cerebrovascular diseases.

B) accidents.

C) heart disease.

D) cancer.

Q4) Analgesics include both OTC and prescription drugs.

A)True

B)False

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Chapter 18: The Chemistry of Useful Materials

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Sample Questions

Q1) Which of the following does not apply to silicates?

A) clay

B) tetrahedral units

C) contain carbon

D) SiO₂

Q2) The product of the cell reaction produced at the position indicated by the number 2 is ______________.

Q3) Over the years what element has been used as a reducing agent to reduce iron metal from its ores?

A) sulfur

B) silicon

C) sodium

D) carbon

Q4) Which metal is sufficiently concentrated in the oceans so that it is currently extracted commercially?

A) aluminum

B) copper

C) magnesium

D) iron

Q5) Selenium could be used as the dopant indicated by the letter______.

Page 20

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Chapter 19: Feeding the World

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Q1) If only very small amounts of a nutrient are required by a plant, it is referred to as a

A) primary nutrient.

B) micronutrient.

C) subnutrient.

D) secondary nutrient.

Q2) A fertilizer is labeled 6-10-12. The "12" represents the percentage of A) nitrogen.

B) potassium.

C) phosphorus.

D) oxygen.

Q3) Which soil type has the smallest soil particles?

A) silts

B) sandy soils

C) loams

D) clays

Q4) The Flavr Savr tomato is an early example of ______crop.

Q5) __________ has decreased energy costs but increased labor costs.

Q6) _____________can produce new breeds of plants ten times faster than natural breeding methods.

Page 21

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