Fundamentals of Chemistry Exam Practice Tests - 2610 Verified Questions

Fundamentals of Chemistry Exam Practice Tests

Course Introduction

Fundamentals of Chemistry introduces students to the basic principles and concepts of chemistry, providing a solid foundation for further study in the sciences. The course covers essential topics such as atomic structure, chemical bonding, the periodic table, stoichiometry, chemical reactions, thermochemistry, and the properties of gases, liquids, and solids. Emphasis is placed on developing problem-solving skills, understanding the scientific method, and exploring the applications of chemistry in everyday life and various scientific fields. Laboratory exercises reinforce theoretical knowledge and encourage hands-on learning of key chemical techniques and safety practices.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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24 Chapters

2610 Verified Questions

2610 Flashcards

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Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) A sample of cesium carbonate,weighing 3.80 g,requires 1.90 g of hydrogen bromide gas to completely decompose to water,cesium bromide,and carbon dioxide gas.The total mass of water and cesium bromide formed is 5.20 g and no hydrogen bromide or cesium carbonate remains.According to the law of conservation of mass,what mass of carbon dioxide must have been formed?

A)0.50 g

B)1.40 g

C)5.49 g

D)10.90 g

E)1.90 g

Answer: A

Q2) A(n)_____ is a concise statement or mathematical equation about a fundamental relationship or regularity of nature.

A)experiment

B)hypothesis

C)anomaly

D)law

E)theory

Answer: D

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3

Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) What is the ratio of oxygen atoms to hydrogen atoms in the compound

Fe₄(PO₄)₃(OH)₃ 12H₂O?

A)15:3

B)27:15

C)27:27

D)18:27

E)25:17

Answer: C

Q2) Who discovered the nucleus of an atom?

A)Thomson

B)de Broglie

C)Rutherford

D)Bohr

E)Heisenberg

Answer: C

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Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) NaHCO₃ is the active ingredient in baking soda.How many grams of oxygen are present in 0.25 g of NaHCO₃?

A)0.009 g

B)0.048 g

C)2.98 × 10³ g

D)0.016 g

E)0.14g

Answer: E

Q2) How many aluminum atoms are there in 52 g of Al₂S₃?

A)4.2 × 10²³

B)1.6 × 10²¹

C)2.1 × 10²³

D)1.1 × 10²¹

E)6.3 × 10²³

Answer: A

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) What is the final concentration of HCl in a solution prepared by addition of 922.0 mL of 4.73 M HCl to 549.0 mL of 2.03 M HCl? Assume volumes are additive.

A)3.38 M

B)0.00459 M

C)6.76 M

D)3.72 M

E)3.03 M

Q2) Identify the spectator ions in the following reaction. Ca²⁺(aq)+ 2NO₃^-(aq)+ 2Na⁺(aq)+ CO₃^2-(aq) CaCO₃(s)+ 2Na⁺(aq)+ NO₃^-(aq)

A)NO₃^- and CO₃^2-

B)Ca²⁺ and Na⁺

C)Ca²⁺ and CO₃^2-

D)Ca²⁺ and NO₃^-

E)Na⁺ and NO₃^-

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Chapter 5: The Gaseous State

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Sample Questions

Q1) Which of the following is not a postulates of the kinetic molecular theory of gases?

A)The gas molecules are in constant motion.

B)At a constant temperature,each molecule has the same kinetic energy.

C)The collisions between molecules are elastic.

D)The volumes of the molecules are negligible compared with the volume of the container.

E)The gas molecules are in rapid motion.

Q2) What is the partial pressure of carbon dioxide in a container that contains 3.63 mol of oxygen,1.49 mol of nitrogen,and 4.49 mol of carbon dioxide when the total pressure is 871 mmHg?

A)329 mmHg

B)763 mmHg

C)135 mmHg

D)406 mmHg

E)871 mmHg

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Chapter 6: Thermochemistry

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Sample Questions

Q1) What is H° for the following phase change?

NaCl(s) NaCl(l)

Substance

H°_f (kJ/mol)

NaCl(s)

-411.12

NaCl(l)

-385.92

A)797.04 kJ

B)25.20 kJ

C)-797.04 kJ

D)-25.20 kJ

E)0 kJ

Q2) Under conditions of constant pressure,for which of the following reactions is the magnitude of pressure-volume work going to be smallest?

A)BaO(s)+ SO₃(g) BaSO₄(s)

B)2NO(g)+ O₂(g) 2NO₂(g)

C)2H₂O₂(l) 2H₂O(l)+ O₂(g)

D)2KClO₃(s) 2KCl(s)+ 3O₂(g)

E)H₂(g)+ Cl₂(g) 2HCl(g)

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Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) The frequency of a radio emission is 7.22 × 10¹³/s.Determine the wavelength of the radio wave.

A)4155 nm

B)3096 nm

C)587 nm

D)828 nm

E)1256 nm

Q2) Which type of electromagnetic radiation has the lowest energy?

A)gamma rays

B)x rays

C)red light

D)blue light

E)radio waves

Q3) Which type of electromagnetic radiation has the lowest frequency?

A)microwaves

B)visible

C)ultraviolet

D)infrared

E)radio waves

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Page 9

Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) The maximum number of electrons that can be accommodated in an s subshell is A)6.

B)14.

C)10.

D)1.

E)2.

Q2) A few atoms of the new element 113 were created in 2004 by a team of Russian and American scientists.It has been given the temporary name "ununtrium" and the temporary symbol "Uut." Based on ununtrium's position on the periodic table,what type of oxide(s)should it form?

A)Ununtrium should form a basic oxide with the formula Uut₂O₃.

B)Ununtrium should form an amphoteric oxide with the formula UutO.

C)Ununtrium should form an acidic oxide with the formula Uut₂O₃.

D)Ununtrium should form two acidic oxides having the formulas Uut₂O and Uut₂O₃.

E)Ununtrium should form two basic oxides having the formulas Uut₂O and Uut₂O₃.

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Page 10

Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) What is the total number of valence electrons in N₂O?

A)16

B)17

C)34

D)11

E)22

Q2) How is a covalent bond formed?

A)By the sharing of valence protons between atoms

B)By the sharing of positrons between atoms

C)By the sharing of a pair of electrons between atoms

D)By the sharing of boson particles between atoms

E)By the sharing of a pair of neutrons between atoms

Q3) In the Lewis dot formula for the bromate ion (BrO₃^-)that minimizes formal charge,the central atom is surrounded by

A)two bonding pairs and two lone pairs of electrons.

B)four bonding pairs and one lone pair of electrons.

C)three bonding pairs and no lone pairs of electrons.

D)five bonding pairs and one lone pair of electrons.

E)three bonding pairs and one lone pair of electrons.

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Page 11

Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) Which of the following statements concerning ozone is incorrect?

A)It is generated by passing an electrical discharge through oxygen.

B)It has a partial double-bond character.

C)It is a nonpolar molecule.

D)It is an important absorber of ultraviolet radiation in the stratosphere.

E)It has a bond angle similar to that predicted for sp² hybridization.

Q2) Which of the following molecules has a dipole moment?

A)PF₅

B)FOOF

C)HCCH

D)F₂CCF₂

E)SF₆

Q3) Which of the following characteristics does not apply to PF₃?

A)has three bonds

B)contains polar bonds

C)polar molecule

D)one lone pair of electrons on phosphorus

E)trigonal planar

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) The metal lithium crystallizes in a body-centered cubic lattice.If the density of lithium is 0.535 g/cm³,what is the unit cell edge length?

A)350 pm

B)63.4 pm

C)183 pm

D)50.3 pm

E)278 pm

Q2) A low melting solid readily dissolves in water to give a nonconducting solution.The solid is most likely a

A)molecular solid.

B)ionic solid.

C)covalent network solid.

D)weak base.

E)metallic solid.

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Chapter 12: Solutions

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Sample Questions

Q1) Trimellitic acid is an organic acid that has a composition of 51.44% C,2.88% H,and 45.68% O by mass.A 6.96-g sample of trimellitic acid dissolved in 30.00 g of acetone,CH₃COCH₃,has a boiling point of 58.09°C.What is the molecular formula of trimellitic acid? (K_b for acetone is 1.71°C/m,and pure acetone has a boiling point of 56.20°C.)

A)CH₂O

B)C₉H₆O₆

C)C₃HO₂

D)C₁₈HO₁₆

E)C₆H₂O₄

Q2) If a 23.6-g sample of a nonelectrolyte is dissolved in 136.0 g of water,the resulting solution will freeze at -0.85°C.What is the molar mass of the nonelectrolyte? (K_f for water is 1.858°C/m.)

A)78 g/mol

B)0.38 g/mol

C)870 g/mol

D)270 g/mol

E)370 g/mol

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Page 14

Chapter 13: Rates of Reaction

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Sample Questions

Q1) Determine the molecularity of the following elementary reaction: O₃ O₂ + O.

A)quadmolecular

B)bimolecular

C)unimolecular

D)termolecular

E)cannot be determined

Q2) In the Arrhenius equation,the symbol A is called _____ and the symbol R is called

A)Avogadro's number,Coulomb's constant

B)Bohr's radius,gravitational constant

C)bond length,atomic mass unit

D)frequency factor,gas constant

E)bond strength,neutron mass

Q3) Which of the following statements is incorrect concerning a catalyst?

A)A catalyst decreases the activation energy of a reaction.

B)A catalyst may appear in the rate law for a reaction.

C)A catalyst alters the equilibrium distribution of reactants and products.

D)There is no net consumption of a catalyst in a reaction.

E)A catalyst provides an alternative reaction mechanism.

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) _____ states that,when a system in chemical equilibrium is disturbed by a change of temperature,pressure,or a concentration,the system shifts in equilibrium composition in a way that tends to counteract this change of variable.

A)Bernoulli's principle

B)Le Châtelier's principle

C)Fermat's principle

D)Heisenberg's uncertainty principle

E)The Pauli exclusion principle

Q2) Which of the following statements is true in a reaction system at equilibrium?

A)The equilibrium constant is zero.

B)The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products.

C)Reactants are reacting to form products at the same rate as products are reacting to form reactants.

D)Reactants and products are present in equimolar amounts.

E)The product of the concentrations of the products divided by the product of the concentrations of the reactants is always a constant.

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Chapter 15: Acids and Bases

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Sample Questions

Q1) What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.16 M HCl with 300.mL of 0.091 M NaOH at 25°C?

HCl(aq)+ NaOH(aq) NaCl(aq)+ H₂O(l)

A)1.6 × 10^-13 M

B)0.091 M

C)1.1 × 10^-12 M

D)0.055 M

E)1.0 × 10^-7 M

Q2) Which of the following species cannot act as a Lewis acid?

A)BeCl₂

B)H⁺

C)Ag⁺

D)BF₃

E)NH₄⁺

Q3) Which of the following is the strongest acid?

A)HClO₂

B)HCl

C)HClO₄

D)HClO

E)HClO₃

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) What is the equilibrium concentration of ammonium ion in a 0.33 M solution of ammonia (NH₃,K_b = 1.8 × 10^-5)at 25^oC?

A)3.0 × 10^-14 M

B)4.1 × 10^-12 M

C)2.4 × 10^-3 M

D)7.4 × 10^-3 M

E)3.3 × 10^-1 M

Q2) Which of the following would be the best mole ratio of conjugate acid to conjugate base for a large buffer capacity?

A)100:1

B)1:1

C)1:100

D)1:10

E)10:1

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18

Chapter 17: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) The insoluble salts

AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed from the metal ions A⁺,B⁺,C³⁺,D²⁺,and E³⁺ and the nonmetals V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

A)AV

B)EZ₃

C)DY₂

D)B₂W

E)C₂X₃

Q2) What is the solubility (in g/L)of calcium fluoride at 25°C? The solubility product constant for calcium fluoride is 3.4 × 10^-11 at 25°C.

A)0.00045 g/L

B)2.7 × 10^-9 g/L

C)0.015 g/L

D)1.3 × 10^-9 g/L

E)0.094 g/L

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Chapter 18: Thermodynamics and Equilibrium

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Sample Questions

Q1) Which of the following has a value of zero for the standard free energy of formation at 298 K?

A)I(l)

B)I₂(g)

C)I₂(l)

D)I₂(s)

E)I(g)

Q2) For the reaction N₂(g) 2N(g),

A) H < 0 and S < 0.

B) H > 0 and S < 0.

C) H < 0 and S > 0.

D) H = 0 and S > 0.

E) H > 0 and S > 0.

Q3) In which reaction is S° expected to be negative?

A)2C₂H₆(g)+ 7O₂(g) 4CO₂(g)+ 6H₂O(l)

B)Ga(l) Ga(s)

C)H₂O(l)+ 2SO₂(g) H₂SO₄(l)

D)CO₂(g) CO₂(s)

E)all of above

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Chapter 19: Electrochemistry

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Sample Questions

Q1) What is the cell reaction for the following electrochemical cell?

Zn | Zn²⁺(aq)|| Sc³⁺(aq)| Sc

A)3Zn(s)+ 2Sc³⁺(aq) 2Sc(s)+ 3Zn²⁺(aq)

B)2Sc(s)+ 3Zn²⁺(aq) 3Zn(s)+ 2Sc³⁺(aq)

C)Zn(s)+ Zn²⁺(aq) Sc(s)+ Sc³⁺(aq)

D)Zn(s)+ Sc³⁺(aq) Sc(s)+ Zn²⁺(aq)

E)Sc(s)+ Zn²⁺(aq) Zn(s)+ Sc³⁺(aq)

Q2) A _____ is a commercial electrochemical cell used to obtain sodium metal by the electrolysis of molten sodium chloride.

A)Downs cell

B)Bunsen cell

C)Leclanché cell

D)Daniell cell

E)Weston cell

Q3) The Faraday constant is defined as

A)The charge per mole of electrons.

B)The charge on a single electron.

C)The maximum work obtainable from an electrochemical cell.

D)The electromotive force of the cell.

E)The amount of charge moved between electrodes.

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Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) Which of the following statements is(are)true for the fission of uranium-235?

A)The electron is captured by the nucleus,which becomes unstable.

B)The nuclides produced are more stable than the uranium nuclide.

C)The nuclides produced are individually heavier than the uranium nuclide.

D)The products include neutrons.

E)Two of these statements are true.

Q2) Iodine-131,which is used to treat thyroid cancer,has a half-life of 8.04 days.How much time is required for 68% of the isotope to decay?

A)13 days

B)7 days

C)43 days

D)53 days

E)4 days

Q3) Which of the following nuclides will produce ²⁴³Am upon undergoing alpha decay?

A)(²⁴⁷Bk)

B)(²³⁹Np)

C)(²⁴³Pu)

D)(²⁴³Cm)

E)(²⁴⁴Am)

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Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) Which of the following reactions describes the formation of an ionic hydride?

A)2H₂(g)+ O₂(g) 2H₂O(l)

B)H₂(g)+ Cl₂(g) 2HCl(g)

C)2K(s)+ H₂(g) 2KH(s)

D)H₂(g)+

C₂H₆(g)

C₂H₄(g)

E)N₂(g)+ 3H₂(g) 2NH₃(g)

Q2) A superoxide ion can be distinguished from the peroxide ion and the oxide ion because

A)the superoxide ion is stable.

B)the superoxide ion is paramagnetic.

C)the superoxide ion is diamagnetic.

D)the superoxide ion is an acid.

E)the superoxide ion is a base.

Q3) Which of the following statements concerning potassium and its compounds is false?

A)Potash consists mostly of potassium carbonate.

B)Potassium is so soft that it can be cut with a butter knife.

C)Potassium reacts with oxygen to produce potassium superoxide.

D)Potassium superoxide is used in self-contained breathing apparatuses.

E)Potassium metal is prepared by electrolysis of potassium chloride.

Page 23

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Chapter 22: The Transition Elements and Coordination Compounds

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Q1) Which of the following describes a d⁶ metal-ion complex with ligands that bond strongly to the metal ion?

A)Pairing energy is less than crystal field splitting,giving a low-spin complex.

B)Pairing energy is greater than crystal field splitting,giving a low-spin complex.

C)Pairing energy is less than crystal field splitting,giving a high-spin complex.

D)A d⁶ ion has only one possible electron arrangement regardless of the ligands.

E)Pairing energy is greater than crystal field splitting,giving a high-spin complex.

Q2) The octahedral complex hexacyanoferrate(III)ion,[Fe(CN)₆]^3-,is a low-spin complex.How many unpaired electrons does the complex have?

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Chapter 23: Organic Chemistry

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Sample Questions

Q1) The functional group of an alkene consists of A)3 bonds.

B)1 bond and 1 bond.

C)2 bonds and 1 bond.

D)2 bonds.

E)2 bonds.

Q2) Equal masses of each of the following are reacted with an excess of dioxygen.Which would form the greatest amount of carbon dioxide?

A)neopentane

B)n-pentane

C)isopentane

D)Two of these would form equal amounts.

E)All of these would form equal amounts.

Q3) How many structural isomers have the molecular formula C₆H₁₄?

A)5

B)2

C)4

D)1

E)3

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Chapter 24: Polymer Materials: Synthetic and Biological

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Q1) Which of the following is(are)not necessary for protein synthesis at the time and place where synthesis occurs?

A)ribosomes

B)DNA

C)mRNA

D)amino acids

E)tRNA

Q2) A fragment of a DNA molecule has the base sequence TGAC.What is the complementary sequence?

A)GTCA

B)CAGT

C)AGTC

D)ACTG

E)TGAC

Q3) Which of the following is not an addition polymer?

A)poly(vinyl chloride)

B)polyethylene

C)polystyrene

D)polypropylene

E)polyester

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