Chemistry for Engineers
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Course Introduction
Chemistry for Engineers is a foundational course designed to introduce engineering students to core chemical principles and their practical applications in engineering contexts. The course covers topics such as atomic and molecular structure, chemical bonding, stoichiometry, thermodynamics, kinetics, equilibrium, and material properties. Emphasis is placed on the relevance of chemistry to various engineering disciplines, including the understanding of material behavior, chemical processes in industrial operations, and environmental considerations. Through lectures, laboratory experiments, and problem-solving sessions, students gain critical insights into how chemical concepts underpin engineering solutions and innovations.
Recommended Textbook
Introductory Chemistry An Atoms First Approach 1st Edition by Julia Burdge
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Chapter 1: Atoms and Elements
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Sample Questions
Q1) In the periodic table, atoms are arranged in order of
A)increasing atomic mass.
B)increasing atomic number.
C)physical properties.
D)periodicity.
E)chemical reactivities.
Answer: B
Q2) Give the number of protons (p), electrons (e), and neutrons (n) in one atom of chlorine-37.
A)37 p, 37 e, 17 n
B)17 p, 17 e, 37 n
C)17 p, 17 e, 20 n
D)37 p, 17 e, 20 n
E)17 p, 37 e, 17 n
Answer: C
Q3) When applying the scientific method, it is important to avoid any form of hypothesis.
A)True
B)False
Answer: False
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Page 3
Chapter 2: Electrons and the Periodic Table
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Sample Questions
Q1) Which one of these ions is not isoelectronic with Kr?
A)As<sup>3+</sup>
B)Se<sup>2 </sup>
C)Rb<sup>+</sup>
D)Sr<sup>2+</sup>
E)Br<sup> </sup>
Answer: A
Q2) What is the emission of light at only specific wavelengths?
A)Emission spectra
B)Hydrogen spectrum
C)Wave spectra
D)Limited spectra
E)Line spectra
Answer: E
Q3) Determine which sublevel designation is legitimate.
A)1f
B)2d
C)3c
D)4s
Answer: D
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Chapter 3: Compounds and Chemical Bonds
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Sample Questions
Q1) Which of these compounds is most likely to be ionic?
A)NCl<sub>3</sub>
B)BaCl<sub>2</sub>
C)CO
D)SO<sub>2</sub>
E)SF<sub>4</sub>
Answer: B
Q2) Determine the formula of the compound formed from K<sup>+</sup> and O<sup>2 </sup>.
A)K<sub>3</sub>O<sub>2</sub>
B)K<sub>2</sub>O
C)K<sub>2</sub>O<sub>3</sub>
D)KO<sub>2</sub>
Answer: B
Q3) The rusting of a piece of iron under environmental conditions is a physical change.
A)True
B)False
Answer: False
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5
Chapter 4: How Chemists Use Numbers
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Sample Questions
Q1) Zero kelvin 0 K < 0°F < 0°C
A)True
B)False
Q2) The mass of a sample is 550 milligrams.Which of the following expresses that mass in kilograms?
A)5.5 × 10<sup>8</sup> kg
B)5.5 × 10<sup>5</sup> kg
C)5.5 × 10<sup> </sup><sup>4</sup> kg
D)5.5 × 10<sup> </sup><sup>6</sup> kg
E)5.5 × 10<sup> </sup><sup>1</sup> kg
Q3) Convert 8.513 × 10<sup>5</sup> mg/kL into units of ng/L.
A)8.513 × 10<sup>11</sup> ng/L
B)8.513 × 10<sup>8</sup> ng/L
C)8.513 × 10<sup>2</sup> ng/L
D)8.513 × 10<sup>14</sup> ng/L
E)8.513 × 10<sup> </sup><sup>10</sup> ng/L
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Chapter 5: The Mole and Chemical Formulas
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Sample Questions
Q1) Calculate the mass of 3.00 moles of CF<sub>2</sub>Cl<sub>2</sub>.
A)3.00 g
B)174 g
C)363 g
D)1.81 × 10<sup>24</sup> g
E)40.3
Q2) Which of the following substances contains the greatest mass of carbon?
A)100 g CH<sub>4</sub>
B)100 g C<sub>2</sub>H<sub>4</sub>
C)100 g CCl<sub>4</sub>
D)100 g CH<sub>2</sub>Cl<sub>2</sub>
E)100 g CO<sub>2</sub>
Q3) How many nitrate ions are in 24.4 grams of Ca(NO<sub>3</sub>)<sub>2</sub>?
A)1.79 × 10<sup>23</sup> nitrate ions
B)0.149 nitrate ions
C)1.47 × 10<sup>25</sup> nitrate ions
D)8.95 × 10<sup>22</sup> nitrate ions
E)0.297 nitrate ions
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Chapter 6: Molecular Shape
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Sample Questions
Q1) Which is the most reasonable prediction for the H-C-H bond angle in CH<sub>4</sub>?
A)90°
B)109.5°
C)120°
D)107°
E)105°
Q2) Which of the following pure substances has the strongest dispersion forces?
A)C<sub>4</sub>H<sub>10</sub>
B)C<sub>5</sub>H<sub>12</sub>
C)C<sub>6</sub>H<sub>14</sub>
D)C<sub>7</sub>H<sub>16</sub>
E)C<sub>8</sub>H<sub>18</sub>
Q3) Place the following in order of decreasing electronegativity. Mg Cl F
A)Mg > Cl > F
B)F > Cl > Mg
C)Cl > F > Mg
D)Cl > Mg > F
E)F > Mg > Cl
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Page 8
Chapter 7: Solids, Liquids, and Phase Changes
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Sample Questions
Q1) What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?
A)Surface tension
B)Adhesion
C)Polarity
D)Viscosity
E)Cohesion
Q2) What is the process in which molecules undergo a phase change from the gas phase to the liquid phase?
A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation
Q3) Which of the following terms refers to the resistance of a liquid to flow?
A)Surface tension
B)Capillary action
C)Viscosity
D)Adhesion
E)Cohesion
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Chapter 8: Gases
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Sample Questions
Q1) Determine the mole fraction of CO in a gas mixture composed of 782.4 grams of CO<sub>2</sub> and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.
A)0.11
B)0.89
Q2) A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L.What will the gas pressure be if the volume is increased to 321 L at 125°C?
A)212 torr
B)289 torr
C)356 torr
D)441 torr
E)359 torr
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10
Chapter 9: Physical Properties of Solutions
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Sample Questions
Q1) Which of these compounds is a nonelectrolyte?
A)NaOH
B)HNO<sub>3</sub>
C)C<sub>2</sub>H<sub>6</sub>O (ethanol)
D)KF
E)CH<sub>3</sub>COOH (acetic acid)
Q2) Which is defined as the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature?
A)precipitation
B)combustion
C)solubility
D)super saturation
E)dilution
Q3) Which process defines how an ionic compounds break apart into its constituent ions upon dissolution?
A)electrolysis
B)dissociation
C)division
D)ionization
E)decomposition
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Chapter 10: Chemical Reactions and Chemical Equations
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Sample Questions
Q1) If aqueous solutions of KMnO<sub>4</sub>, FeSO<sub>4</sub> and H<sub>2</sub>SO<sub>4,</sub> are mixed, which ions are spectator ions? 2KMnO<sub>4</sub>(aq) + 10FeSO<sub>4</sub>(aq) + 8H<sub>2</sub>SO<sub>4</sub>(aq) K<sub>2</sub>SO<sub>4</sub>(aq) + 2MnSO<sub>4</sub>(aq) + 5Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>(aq) + 8H<sub>2</sub>O(l)
A)only K<sup>+</sup><sup> </sup>
B)only SO<sub>4</sub><sup>2 </sup>
C)only K<sup>+</sup><sup> </sup>and SO<sub>4</sub><sup>2 </sup>
D)only K<sup>+</sup>, SO<sub>4</sub><sup>2 </sup><sub>,</sub> and Fe<sup>2+</sup>
E)only K<sup>+</sup>, SO<sub>4</sub><sup>2 </sup>, Fe<sup>2+</sup>, and Mn<sup>2+</sup>
Q2) Which salt is formed in the neutralization reaction of hydrochloric acid with calcium hydroxide?
A)CaO
B)CaCl
C)CaH<sub>2</sub>
D)CaCl<sub>2</sub>
E)NaCl
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Chapter 11: Using Balanced Chemical Equations
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Sample Questions
Q1) What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V<sub>2</sub>O<sub>5</sub> with 4.0 moles of calcium based on the following chemical equation? V<sub>2</sub>O<sub>5</sub>(s) + 5Ca(l) 2V(l) + 5CaO(s)
A)1.0 mol
B)1.6 mol
C)2.0 mol
D)0.80 mol
E)3.2 mol
Q2) Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.
A)Chlorine is the limiting reactant; 1.14 g of potassium remain.
B)Potassium is the limiting reactant; 2.00 g of chlorine remain.
C)Potassium is the limiting reactant; 2.47 g of chlorine remain.
D)Chlorine is the limiting reactant; 3.07 g of potassium remain.
E)Potassium is the limiting reactant; 4.50 g of chlorine remain.
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Chapter 12: Acids and Bases
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Sample Questions
Q1) What is the name given to a substance that can act as a Brønsted acid or as a Brønsted base according to what it is reacting with?
A)hydrophilic
B)hydrophobic
C)amphoteric
D)isoprotic
E)isoelectronic
Q2) Which solution is the most acidic?
A)pH = 1.00
B)pH = 10.00
C)pH = 5.00
D)pH = 3.00
E)pH = 4.00
Q3) What is the H<sup>+</sup> ion concentration in a 2.1 × 10<sup> 4</sup> M
Ca(OH)<sub>2</sub> solution?
A)7.3 × 10<sup> 4</sup> M
B)4.2 × 10<sup> 4</sup> M
C)2.1 × 10<sup> 4</sup> M
D)2.4 × 10<sup> 11</sup> M
E)4.8 × 10<sup> 11</sup> M
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Chapter 13: Equilibrium
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Sample Questions
Q1) When a reaction system reaches equilibrium, the forward and reverse reactions stop.
A)True
B)False
Q2) What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?
A)Reversibility expression
B)Reaction expression
C)Equilibrium expression
D)Product quotient
E)Mass action
Q3) At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.
A)True
B)False
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Chapter 14: Organic Chemistry
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Sample Questions
Q1) Which type of organic compound does not contain a carbonyl group?
A)Ethers
B)Carboxylic acids
C)Ketones
D)Aldehydes
E)Esters
Q2) Which one of these compounds will result from the addition of HCl to CH<sub>3</sub> CH=CH<sub>2</sub>?
A)CH<sub>3</sub>Cl + CH<sub>2</sub>=CH<sub>2</sub>
B)CH<sub>3</sub> CHCl=CH<sub>2</sub>
C)CH<sub>3</sub> CHCl-CH<sub>3</sub>
D)CH<sub>3</sub> CH<sub>2</sub> CH<sub>2</sub>Cl
E)None of these choices is correct.
Q3) What label is given to an alkyl group?
A)Alk
B)A
C)K
D)R
E)AG
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Page 16
Chapter 15: Biochemistry
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Sample Questions
Q1) The breaking apart of a dissacharide into its monosaccharide components involves the addition of a water molecule and is called _______.
A)condensation
B)peptide linkage
C)secondary structure
D)hydrolysis
E)transport
Q2) Which of the following is not a carbohydrate?
A)C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>
B)C<sub>5</sub>H<sub>10</sub>O<sub>5</sub>
C)C<sub>10</sub>H<sub>18</sub>O<sub>9</sub>
D)C<sub>6</sub>H<sub>14</sub>O<sub>6</sub>
E)C<sub>12</sub>H<sub>22</sub>O<sub>11</sub>
Q3) Which of the following refers to a primary structure?
A)The shape the protein chain adopts as the result of hydrogen bonding.
B)The sequence of amino acids that make up a protein chain.
C)The folding of a protein into a characteristic shape.
D)The shape formed by two or more folded protein chains coming together.
E)None of the above.
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Page 17
Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) What is the nuclear process called in which a heavy nuclear of mass number greater than 200 divides to form smaller nuclei of intermediate mass and one or more neutron(s)?
A)Photonuclear reactions
B)Nuclear fission
C)Thermal conductivity
D)Nuclear combination
E)Nuclear fusion
Q2) Beta particles are identical to A)protons.
B)helium atoms.
C)hydrogen atoms.
D)helium nuclei.
E)electrons.
Q3) Which of the following is used to test the activity of the thyroid?
A)(<sup>18</sup>O)
B)(<sup>131</sup>I)
C)(<sup>123</sup>I)
D)(<sup>24</sup>Na)
E)(<sup>99</sup>Tc)
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Chapter 17: Electrochemistry
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Sample Questions
Q1) Consider the reaction CuO(s) + H<sub>2</sub>(g) Cu(s) + H<sub>2</sub>O(l)
In this reaction, which substances are the oxidizing agent and reducing agent, respectively?
A)CuO and H<sub>2</sub>
B)H<sub>2</sub> and CuO
C)CuO and Cu
D)H<sub>2</sub>O and H<sub>2</sub>
E)Cu and H<sub>2</sub>O
Q2) Complete and balance the following redox equation.Now sum the coefficients of all species in the balanced equation.(Remember to add the coefficients that are equal to one, and to add the coefficients of any species added to the equation.) The sum of the smallest whole number coefficients is Bi(OH)<sub>3</sub> + SnO<sub>2</sub><sup>2 </sup> Bi + SnO<sub>3</sub><sup>2 </sup> (basic solution)
A)32
B)25
C)16
D)13
E)4
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