Chemistry for Environmental Science Mock Exam - 3323 Verified Questions

Chemistry for Environmental Science

Mock Exam

Course Introduction

Chemistry for Environmental Science provides an introduction to the fundamental principles of chemistry with a focus on their application to environmental issues. The course covers topics such as atomic structure, chemical bonding, reactions, and the properties of matter, emphasizing how these concepts relate to environmental processes. Students will explore the chemical basis of pollution, the behavior of contaminants in air, water, and soil, and the role of chemistry in analyzing and solving environmental problems. Laboratory and case study components offer practical experience in monitoring environmental parameters and understanding chemical cycles in nature, preparing students to assess and address ecological challenges using chemical knowledge.

Recommended Textbook

General Chemistry Principles and Modern Applications 11th Edition by Ralph

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28 Chapters

3323 Verified Questions

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Page 2

Chapter 1: Matter: Its Properties and Measurement

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Sample Questions

Q1) Which of the following is the lowest temperature?

A)42 °C

B)57 °F

C)318 K

D)All of these temperatures are equal.

Answer: B

Q2) From ammonia gas,one can obtain two different gases,each of which is a pure substance.Using only this information,it can be said with certainty that:

A)one of the products is an element

B)neither of the products can be an element

C)ammonia cannot be an element

D)both products are elements

E)gases do not produce solids

Answer: C

Q3) Which of the following is the smallest volume?

A)11 cm³

B)0.25 dL

C)1.4 × 10³ mL

D)2.5 × 10⁷ nL

Answer: A

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Chapter 2: Atoms and the Atomic Theory

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Sample Questions

Q1) What is the mass of a sample containing 1.2 moles of Ni?

A)49 g

B)59 g

C)34 g

D)61 g

E)70 g

Answer: E

Q2) 24.9 g of Mn is equivalent to how many moles of Mn?

A)2.21 moles

B)0.453 moles

C)0.461 moles

D)0.996 moles

E)1.00 mole

Answer: B

Q3) Isotopes have different atomic number (Z)but the same mass number (A).

A)True

B)False

Answer: False

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Chapter 3: Chemical Compounds

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Sample Questions

Q1) Fumaric acid,C₄H₄O₄,can be extracted from plants and can be used as a substitute for citrus acid in fruit drinks.The percent composition by mass of fumaric acid is ________.

A)C 33.33% H 33.33% O 33.33%

B)C 39.80% H 6.68% O 53.52%

C)C 40.00% H 6.67% O 53.33%

D)C 41.39% H 3.47% O 55.14%

E)C 0.25% H 0.25% O 0.50%

Answer: D

Q2) How many hydrogen atoms are there in 12.4 g of Al₂(HPO₄)₃?

A)6.55 × 10^{22 H atoms}

B)1.09 × 10^{22 H atoms}

C)6.07 × 10^{22 H atoms}

D)1.32 × 10^{23 H atoms}

E)4.39 × 10^{22 H atoms}

Answer: A

Q3) Determine the mass percent (to the hundredths place)of H in sodium bicarbonate (NaHCO₃).

Answer: 1.20

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) When 11.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction.

Ca(s)+ 2 H₂O(l) Ca(OH)₂(aq)+ H₂(g)

A)12.3%

B)24.6%

C)45.5%

D)84.0%

Q2) (aq)indicates that the compound is dissolved in alcohol.

A)True

B)False

Q3) How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?

CaCl₂(aq)+ K₂CO₃(aq) 2 KCl(aq)+ CaCO₃(aq)

A)0.896 g

B)1.12 g

C)2.23 g

D)4.47 g

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Page 6

Chapter 5: Introduction to Reactions in Aqueous Solutions

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Sample Questions

Q1) What volume of 0.38 M hydrochloric acid is required for complete neutralization of 15 mL of 0.19 M calcium hydroxide?

A)38 mL

B)30 mL

C)19 mL

D)15 mL

E)7.5 mL

Q2) In an acid-base neutralization reaction,38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

A)0.194 mol L^-1

B)0.387 mol L^-1

C)0.775 mol L^-1

D)1.29 mol L^-1

Q3) When dissolved in water,KOH behaves as:

A)an acid that forms K⁺ and OH^- ions

B)an acid that forms KO^- and H⁺ ions

C)a base that forms K⁺ and OH^- ions

D)a base that forms KO^- and H⁺ ions

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Page 7

Chapter 6: Gases

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Sample Questions

Q1) If 0.50 mole H₂(g)and 1.0 mole He(g)are compared at standard temperature and pressure,the two gases will:

A)have equal effusion rates

B)have equal average molecular velocities

C)have equal average molecular kinetic energies

D)occupy equal volumes

E)have equal weights

Q2) If 250.L of nitrogen reacts with 582 L of hydrogen by the reaction: N₂(g)+ 3 H₂(g) 2 NH₃(g),

How much nitrogen is unreacted? All gases are at the same temperature and pressure.

A)1.9 × 10² L

B)3.3 × 10²L

C)56 L

D)3.0 × 10²L

E)41 L

Q3) Liquid mercury freezes at a temperature of -39 °C.The freezing point of mercury on the Kelvin scale is 234 K.

A)True

B)False

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Page 8

Chapter 7: Thermochemistry

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Sample Questions

Q1) H₂S(g)+ 3/2 O₂(g) H₂O (l)+ SO₂(g) _rH° = -562.3 kJ/mol

1/8 S₈(s)+ O₂(g) SO₂(g) _rH° = -297.0 kJ/mol

H₂(g)+ 1/2O₂ H₂O (l) _rH° = -266.9 kJ/mol

Compute _rH° for H₂(g)+ 1/8 S₈ (s) H₂S(g)in kJ/mol.

A)562.3 kJ/mol

B)276.6 kJ/mol

C)265.3 kJ/mol

D)20.5 kJ/mol

E)-1.6 kJ/mol

Q2) A system absorbs 623 J of heat while doing 457 J of work.What is the value of U?

A)+1080 J

B)-166 J

C)+166 J

D)-1080 J

E)+623 J

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Chapter 8: Electrons in Atoms

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Sample Questions

Q1) What is the wavelength,in nm,of light with an energy content of 550 kJ/mol?

A)0.218 nm

B)0.419 nm

C)157 nm

D)218 nm

E)6579 nm

Q2) The relationship between the frequency of light and the energy of the light was postulated by:

A)Max Planck

B)Johann Balmer

C)Johannes Rydberg

D)Albert Einstein

E)Robert Bunsen

Q3) For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

A)656.3 nm

B)486.2 nm

C)364.6 nm

D)2.057 × 10^-3 nm

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Chapter 9: The Periodic Table and Some Atomic Properties

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Sample Questions

Q1) Which of the following has the largest number of unpaired electrons: S,CrS1U1P12+ S1S1P0,N,K,Ne?

A)S

B)CrS1U1P12+ S1S1P0

C)N

D)K

E)Ne

Q2) The first ionization potential for S is lower than the first ionization potential for P because:

A)Hund's rule is violated

B)P has a p³ configuration

C)ionization potentials decrease across a representative period

D)P is to the right of S on the periodic table

E)P is below S on the periodic table

Q3) Which of the following species will have the highest ionization energy?

A)K⁺

B)Ar

C)Cl^-

D)S^2-

Q4) Which 1+ ion is isoelectronic with S^2-?

Page 11

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Chapter 10: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which of the following molecules contains polar bonds but has a zero dipole moment?

A)N₂

B)NH₃

C)CO₂

D)CH₃Cl

E)BrCl

Q2) Of the following elements,which has the highest electronegativity?

A)S

B)Cl

C)Ti

D)Se

Q3) What is the correct molecular geometry for SeBr₃⁺?

A)trigonal pyramidal

B)tetrahedral

C)trigonal planar

D)bent

E)T-shaped

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Chapter 11: Chemical Bonding Ii: Valence Bond and

Molecular Orbital Theories

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Sample Questions

Q1) Using the VSEPR model,the molecular geometry of the central atom in NCl₃ is:

A)linear

B)trigonal planar

C)tetrahedral

D)bent

E)trigonal pyramidal

Q2) Three of the molecular shapes which a sp³^d hybridized molecule can have are:

A)triangular,trigonal bipyramid,linear

B)linear,square planar,T-shaped

C)irregular tetrahedron,T-shaped,bent

D)T-shaped,linear,trigonal bipyramid

E)linear,tetragonal pyramid,octahedral

Q3) A double bond is two sigma bonds.

A)True

B)False

Q4) Unhybridized p orbitals must be present for electron delocalization to occur.

A)True

B)False

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Chapter 12: Intermolecular Forces: Liquids and Solids

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Sample Questions

Q1) Gold crystallizes in a face-centred cubic structure.What is the edge length of the unit cell if the atomic radius of gold is 144 pm?

A)204 pm

B)288 pm

C)333 pm

D)407 pm

Q2) Which of the following compounds exhibits hydrogen bonding?

A)CH₃Cl

B)HI

C)CH₃OC H₃

D)NH₃  

Q3) Arrange the following compounds in order of increasing boiling point: HCl,HBr,HI.

A)HCl,HBr,HI

B)HBr,HI,HCl

C)HI,HBr,HCl

D)HCl,HI,HBr

E)HI,HCl,HBr

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Chapter 13: Spontaneous Change: Entropy and Gibbs Energy

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Sample Questions

Q1) For the reaction N₂O₃(g) NO(g)+ NO₂(g) _rG° = -4.78 kJ/mol.Calculate K_eq at 25 °C.

A)1.023

B)1.002

C)1.005

D)0.9484

E)0.9981

Q2) If G < 0 for a reaction,then the reaction is said to be:

A)endothermic

B)reversible

C)spontaneous

D)exothermic

E)fast

Q3) An increase in entropy is observed when a liquid forms from a gas.

A)True

B)False

Q4) An increase or a decrease in the number of microstates parallels an increase or decrease in the number of microscopic particles and the space available to them.

A)True

B)False

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Chapter 14: Solutions and Their Physical Properties

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Sample Questions

Q1) A saline solution begins to freeze at -1.13 °C.Express the concentration of NaCl in this solution in mass %.K_f for water is 1.86 °C m^-1.

A)3.48%

B)1.74%

C)0.870%

D)17.8%

E)8.90%

Q2) An unsaturated solution will have some undissolved solid in the bottom of the container.

A)True

B)False

Q3) Which of the following is an example of a colloid?

A)sucrose in water

B)whipped cream

C)steel

D)salt in water

Q4) Gas solubility always increases with temperature.

A)True

B)False

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Chapter 15: Principles of Chemical Equilibrium

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Sample Questions

Q1) In the reaction:

2 N₂O(g)+ N₂H₄(g) 3 N₂(g)+ 2 H₂O(g),

One starts with 0.10 mol N₂O and 0.25 mol N₂H₄ in a 10.0 L container.If there are 0.06 mol N₂O at equilibrium,how many moles of N₂ are present?

A)0.02

B)0.04

C)0.06

D)0.09

E)0.07

Q2) Equilibrium reactions are noted by a single straight arrow for a yield sign.

A)True

B)False

Q3) Changes in temperature cause change in the equilibrium position.

A)True

B)False

Q4) One method to aid in working out equilibrium problems is the ICE table.

A)True

B)False

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Chapter 16: Acids and Bases

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Sample Questions

Q1) What is the pH of a 0.120 M aqueous solution of the sodium salt of acetylsalicylic acid (aspirin)?

K_a (aspirin)= 3.3 × 10^-4

A)7.0

B)11.8

C)2.2

D)5.7

E)8.3

Q2) CO₂ acts as an acid in the reaction CaO(s)+ CO₂ CaCO₃(s)because it ________.

A)turns blue litmus red

B)reacts with a metal

C)is a proton donor

D)is an electron-pair acceptor

E)is a gas containing a non-metal

Q3) The first ionization step is approximately 100% for H₂SO₃.

A)True

B)False

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Chapter 17: Additional Aspects of Acidbase Equilibria

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Sample Questions

Q1) What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl(aq)requires 28.30 mL of 0.50 mol L^-1 HCl(aq)for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

A)0.30

B)3.18

C)3.76

D)4.03

Q2) What is the pH of a solution prepared by mixing equal volumes of 0.10 M aqueous hydrochloric and 0.1 M aqueous hydrofluoric acid? (K_a for HF is 6.6 × 10^-4)

A)1.0

B)1.3

C)1.6

D)2.2 E)5.0

Q3) The common ion in an aqueous solution of a weak acid and a strong acid is the hydronium ion.

A)True

B)False

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Page 19

Chapter 18: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) A swimming pool was sufficiently alkaline so that the carbon dioxide absorbed from the air produced a solution in the pool that was 2 × 10^-4 M in carbonate ion.If the pool originally contained 4 × 10^-3 M Mg²⁺,6 × 10^-4 M Ca²⁺,and 8 × 10^-7 M Fe²⁺,then the precipitate that was formed consisted of ________. (K_sp values are: CaCO₃,4.7 × 10^-9;MgCO₃,4.0 × 10^-5;FeCO₃,2.0 × 10^-11)

A)only MgCO₃

B)only CaCO₃

C)only FeCO₃

D)only CaCO₃ and FeCO₃

E)MgCO₃,CaCO₃,and FeCO₃

Q2) The solubility of a salt MX₂ with a molar mass of 114 g/mol is 3.42 g/L.Calculate K_sp.

A)2.70 × 10^-5

B)1.08 × 10^-4

C)9.00 × 10^-4

D)2.25 × 10^-4

E)6.75 × 10^-8

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Chapter 19: Electrochemistry

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Sample Questions

Q1) Determine E°_cell for the reaction: 2 Ag⁺(aq)+ Mg(s) 2 Ag(s)+ Mg²⁺(aq).The half reactions are: Mg²⁺(aq)+ 2 e^- Mg(s)E° = -2.356 V Ag⁺(aq)+ e^- Ag(s)E° = 0.800 V

A)0.756 V

B)-0.756 V

C)3.156 V

D)-1.556 V

E)1.556 V

Q2) What is E_cell at 25 °C of the spontaneous cell made from Ag⁺(aq)/Ag(s)(0.80 V)and Cl₂(g)/Cl^-(aq)(1.36 V)half cells if [Ag⁺] = 1 × 10^-2 M and [Cl^-] = 1 × 10^-4 M with _P(Cl₂)= 1.1 atm?

A)0.65 V

B)0.38 V

C)0.74 V

D)0.92 V

E)0.20 V

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Chapter 20: Chemical Kinetics

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Sample Questions

Q1) If increasing the concentration of A in a chemical reaction 2 A B + C causes no increase in the rate of the reaction,then we may say:

A)A is a catalyst

B)the reaction rate is zero order in A

C)the reaction rate is zero order in [A]

D)the reaction rate is first order in [A]

E)A is not involved in the reaction

Q2) The reaction A + B C + D is second order in A and zero order in B.The value of k is 0.012 M^-1 min^-1.What is the rate of this reaction when [A] = 0.125

M and [B] = 0.435 M?

A)5 × 10^-4 M min^-1

B)3.4 × 10^-3 M min^-1

C)1.3 M min^-1

D)1.9 × 10^-4 M min^-1

E)1.5 × 10^-3 M min^-1

Q3) Adding a catalyst lowers the activation energy of a reaction.

A)True

B)False

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Chapter 21: Chemistry of the Main-Group Elements I:

Groups 1,2,13,and 14

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Sample Questions

Q1) The molecular geometry for CO₂ is ________.

A)trigonal planar

B)trigonal bipyramid

C)bent

D)linear

E)trigonal pyramidal

Q2) Which of the following statements about the use of sodium is FALSE?

A)Sodium vapor lamps are used outdoors.

B)Sodium is used in reactors because it has a low melting point.

C)Sodium is used in reactors because it has a high boiling point.

D)Sodium is used in reactors because it has a high thermal conductivity.

E)A typical sodium vapor lamp uses several grams of sodium.

Q3) Choose the INCORRECT statement.

A)The diagonal relationship is the similarity of properties of the top element of one group to the second element of the next group.

B)Li - Mg is a diagonal relationship.

C)C - P is a diagonal relationship.

D)Be - Al is a diagonal relationship.

E)B - Si is a diagonal relationship.

Page 23

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Chapter 22: Chemistry of the Main-Group Elements Ii:

Groups 18,17,16,15,and Hydrogen

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Sample Questions

Q1) Write a balanced half equation for the following couple: ClO₂^-(aq)| Cl^-(aq)(basic)

A)ClO₂^-(aq)+ 2 H₂O(l)+ 4 e^- Cl^-(aq)+ 4 OH^-(aq)

B)ClO₂^-(aq)+ 4 H⁺(aq)+ 4 e^- Cl^-(aq)+ 2 H₂O(l)

C)ClO₂^-(aq)+ H₂O(l)+ e^- Cl^-(aq)+ OH^-(aq)

D)ClO₂^-(aq)+ H⁺(aq)+ e^- Cl^-(aq)+ H₂O(l)

E)ClO₂^-(aq)+ 4 H₂O(l)+ 8 e^- Cl^-(aq)+ 4 OH^-(aq)

Q2) Choose the INCORRECT statement.

A)Hydrazine is N₂H₂.

B)Hydroxylamine is NH₂OH.

C)Hydrazine and its derivatives are used as rocket fuels.

D)HN₃ is hydrazoic acid.

E)Nitrogen is a key element in organic and biochemical molecules.

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Chapter 23: The Transition Elements

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Q1) List the following in order of increasing atomic radius: Ti,Cr,V,Ca.

A)V < Ti < Ca < Cr

B)Ca < V < Cr < Ti

C)Ca < Ti < Cr < V

D)Cr < V < Ti < Ca

E)Cr < V < Ca < Ti

Q2) Choose the INCORRECT statement about the most common oxidation state of transition elements.

A)For Ti,it is +4.

B)For Sc,it is +2.

C)For V,it is +5.

D)For Cr,it is +6.

E)For Mn,it is +7.

Q3) Choose the INCORRECT statement about transition elements.

A)Ferromagnetism occurs only in elements with paired electrons.

B)Ferromagnetism is unique to Fe,Co and Ni.

C)Ferromagnetism occurs due to atoms combining in the solid state in domains.

D)Paramagnetism is due to unpaired electrons.

E)Ferromagnetism requires that interatomic distances be of the right magnitude to generate domains.

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Chapter 24: Complex Ions and Coordination Compounds

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Q1) In the cation [CoCl₂(en)₂]⁺,the oxidation state of cobalt and its coordination number,respectively,are ________.

A)-3 and two

B)+2 and six

C)+4 and four

D)+3 and six

E)-4 and six

Q2) High spin refers to the maximum number of ligands attached to the metal ion.

A)True

B)False

Q3) Which of the following complexes has no geometric isomers?

A)[Pt(NH₃)₄F₂]

B)[Pt(NH₃)F₅]^-3

C)[Co(NH₃)₄F₂]⁺

D)[Co(NH₃)₃F₃]

E)[Co(NH₃)₂F₄]^-

Q4) Unpaired electrons cause a complex ion to be diamagnetic.

A)True

B)False

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Chapter 25: Nuclear Chemistry

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Q1) An employee at a chemical laboratory studying radioisotopes would wear a badge to keep a check on the amount of radiation to which he is exposed.This radiation dosage would be measured in the unit:

A)curie

B)rad

C)rem

D)joules

E)joules per kilogram

Q2) Which of the following statements concerning alpha decay is INCORRECT?

A)It involves nuclides with atomic number larger than 83 and mass number larger than 200.

B)It has great penetrating power,but little ionizing power.

C)It often leaves the nucleus in an excited state.

D)The atomic number decreases by two.

E)The alpha particle is made up of two protons and two neutrons.

Q3) The nuclear binding energy for cobalt-59 is the energy released when:

A)27 protons and 32 neutrons form cobalt-59

B)iron-56 and 2 protons form cobalt-59

C)27 protons and 27 neutrons form cobalt-59

D)cobalt-58 and 1 neutron form cobalt -59

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Chapter 26: Structures of Organic Compounds

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Sample Questions

Q1) Give the condensed structural formula for 3-bromopentane.

A)CH₃CH₂CHBrCH₂CH₂CH₃

B)CH₃CHBrCH₂CH₂CH₃

C)(CH₃)₃CHBrCH₂CH₃

D)CH₃CH₂CHBrCH₂CH₃

E)CH₃CH₂CBr₃CH₂CH₃

Q2) An alcohol of formula C₃H₈O in which there are only three different kinds of hydrogens is:

A)2-propanol

B)1-propanol

C)cyclopropanol

D)ethanol

E)None of the above

Q3) Constitutional isomers have different bond connectivities,and as a consequence they have different skeletal structures.

A)True

B)False

Q4) Cis-trans isomerism is a type of isomerism generally known as stereoisomerism.

A)True

B)False

Page 28

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Chapter 27: Reactions of Organic Compounds

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Sample Questions

Q1) Which of the following groups would be ortho,para directors in electrophilic aromatic substitution?

I.-CN

II.-SO₃H

III.-NH₂

IV.-OH

V.-Br

A)III ,IV ,and V

B)II ,III ,and V

C)I ,III ,and IV

D)I ,II and IV

E)II ,IV and V

Q2) Give the product(s)of the reaction (in H₂SO₄):

CH₂=CHCH₃ + H₂O product(s)

A)CH₂OHCH(OH)CH₃

B)CH₂OHCH₂CH₃

C)CH₂OHCHOHCH₃ + H₂

D)CH₃CH₂CH₃ + H₂O₂

E)CH₃CH(OH)CH₃

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Chapter 28: Chemistry of the Living State

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Sample Questions

Q1) What is the direction of migration of the amino acid phenylalanine in a gel that is 0.25 M in NaH₂PO₄ and 0.50 M in Na₂HPO₄? For phenylalanine,pI = 5.74.

Q2) All amino acids always contain one chemical element which is absent in the structures of carbohydrates.This element is ________.

A)carbon

B)nitrogen

C)phosphorus

D)sulfur

E)oxygen

Q3) Salt linkages:

A)occur between acidic and basic R groups

B)join two halves of cysteine

C)occur between purine and pyrimidine bases

D)occur in sugars

E)connect the cell with the environment

Q4) In DNA,guanine always pairs with cytosine.

A)True

B)False

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