Basic Chemistry Chapter Exam Questions - 929 Verified Questions

Basic Chemistry

Chapter Exam Questions

Course Introduction

Basic Chemistry provides an introduction to the fundamental concepts and principles of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, chemical reactions, and the properties of gases, liquids, and solids. The course emphasizes the development of problem-solving skills and the application of chemical principles to real-world situations. Students will also gain hands-on experience with laboratory experiments to reinforce theoretical concepts and develop practical scientific skills necessary for further study in the sciences.

Recommended Textbook

Introductory Chemistry An Atoms First Approach 1st Edition by Julia Burdge

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17 Chapters

929 Verified Questions

929 Flashcards

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Page 2

Chapter 1: Atoms and Elements

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Sample Questions

Q1) 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

Q2) Which element would be expected to have properties similar to calcium?

A)Ba

B)K

C)Sc

D)Na

E)Rb

Answer: A

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) What is the correct electron configuration for a germanium (Ge) atom?

A)1s²2s²2p⁶3s²3p⁶4s<su p>2</sup>4p²

B)1s²2s²2p⁶3s²3p⁶4s<su p>2</sup>3d¹⁰4p²

C)1s²2s²2p⁶3s²3p²

D)1s²2s²3s²3p⁵

E)None of the answers is correct.

Answer: B

Q2) How many dots does the Lewis dot symbol for sodium have around it?

A)1

B)2

C)0

D)3

E)7

Answer: A

Q3) Each shell (principal energy level) of quantum number n contains n subshells.

A)True

B)False

Answer: True

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Chapter 3: Compounds and Chemical Bonds

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Sample Questions

Q1) The juice from an orange is a mixture.

A)True

B)False

Answer: True

Q2) The chemical formula for iron(II) nitrate is

A)Fe₂(NO₃)₃

B)Ir(NO₂)₂

C)Fe₂N₃

D)Fe(NO₃)₂

E)Fe(NO₂)₂

Answer: D

Q3) Which of the following is the oxoanion of bromine called the bromate ion?

A)BrO₃

B)BrO₃²

C)BrO₄²

D)BrO₂

E)BrO

Answer: A

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Page 5

Chapter 4: How Chemists Use Numbers

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Sample Questions

Q1) The speed needed to escape the pull of Earth's gravity is 11.3 km/s.What is this speed in mi/h? (1 mile = 1609 m)

A)65,500 mi/h

B)25,300 mi/h

C)18,200 mi/h

D)1,090 mi/h

E)5.2 × 10³ mi/h

Q2) How many significant figures are in 0.006570?

A)3

B)4

C)5

D)6

E)7

Q3) How many milliliters is 0.0055 L?

A)0.55 mL

B)5.5 mL

C)0.5 mL

D)0.0000055 mL

E)182 mL

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Page 6

Chapter 5: The Mole and Chemical Formulas

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Sample Questions

Q1) What is the molar mass of nicotine, C₁₀H₁₄N₂?

A)134 g/mol

B)148 g/mol

C)158 g/mol

D)210 g/mol

E)162 g/mol

Q2) Determine the mass of hydrogen (in grams) that contains 5.08 × 10¹⁵ hydrogen atoms.

A)5.12 × 10¹⁵ g

B)3.06 × 10³⁹ g

C)3.06 × 10⁹ g

D)8.50 × 10⁹ g

E)8.5 × 10¹⁵ g

Q3) What is the percent sulfur in iron(III) sulfate?

A)28%

B)32%

C)24%

D)48%

E)42%

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Page 7

Chapter 6: Molecular Shape

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Sample Questions

Q1) The number of resonance structures for the nitrate ion that satisfy the octet rule is A)1.

B)2.

C)3.

D)4.

E)none of these

Q2) Which one of the following molecules is polar?

A)CH₄

B)CHBr₃

C)F₂

D)CBr₄

E)CO₂

Q3) The Lewis structure for a chlorate ion, ClO₃^-, should show ____ single bond(s), ____ double bond(s), and ____ lone pair(s).

A)2, 1, 10

B)3, 0, 9

C)2, 1, 8

D)3, 0, 10

E)2, 1, 9

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Chapter 7: Solids, Liquids, and Phase Changes

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Sample Questions

Q1) What amount of energy (heat) is required to warm a 65.0-g sample of liquid water from 25.0ºC to 96.5ºC? The specific heat capacity of water is 4.184 J/gºC.

A)4.60 J

B)1.11 × 10³ J

C)2.62 × 10⁴ J

D)1.94 ×10⁴ J

E)1.61 J

Q2) If liquid bromine is cooled to form a solid, which type of solid does it form?

A)atomic

B)metallic

C)molecular

D)ionic

E)covalent

Q3) Ethanol (C₂H₅-OH) will have a greater viscosity than ethylene glycol (HO-CH₂CH₂-OH) at the same temperature.

A)True

B)False

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Page 9

Chapter 8: Gases

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Sample Questions

Q1) A sample of an ideal gas has its volume doubled while its temperature remains constant.If the original pressure was 100 torr, what is the new pressure?

A)10 torr

B)50 torr

C)100 torr

D)200 torr

E)1000 torr

Q2) If 2.38 mol of a gas has a volume of 120.0 mL, what is the volume of 1.97 mol of the gas at the same temperature and pressure?

A)25.6 mL

B)99.3 mL

C)119 mL

D)145 mL

E)563 mL

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Chapter 9: Physical Properties of Solutions

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Sample Questions

Q1) 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

Q2) Which substance is present in the smallest proportion in a solution?

A)liquid

B)gas

C)solvent

D)solid

E)solute

Q3) What is defined as the difference between the freezing point of a pure solvent and the freezing point of the solution?

A)Freezing point

B)freezing-point elevation

C)freezing-point depression

D)Subzero freezing

E)Supercooling

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Chapter 10: Chemical Reactions and Chemical Equations

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Sample Questions

Q1) Based on the solubility rules, which of these processes will occur if solutions of CuSO₄(aq) and BaCl₂(aq) are mixed?

A)CuCl₂ will precipitate; Ba²⁺ and SO₄² are spectator ions.

B)CuSO₄ will precipitate; Ba²⁺ and Cl are spectator ions.

C)BaSO₄ will precipitate; Cu²⁺ and Cl are spectator ions.

D)BaCl₂ will precipitate; Cu²⁺ and SO₄² are spectator ions.

E)No precipitate will form.

Q2) If aqueous solutions of ammonium sulfide and copper(II) nitrate are mixed, which insoluble precipitate is formed?

A)CuS

B)Cu₂S

C)NH₄NO₃

D)NH₄(NO₃)₂

E)CuSO₄

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Page 12

Chapter 11: Using Balanced Chemical Equations

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Sample Questions

Q1) What is the maximum number of grams of ammonia, NH₃, which can be obtained from the reaction of 10.0 g of H₂ and 80.0 g of N₂?

N₂ + 3H₂ 2NH₃

A)34.1 g

B)48.6 g

C)56.3 g

D)90.0 g

E)97.3 g

Q2) What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole of V₂O₅ with 6.0 mole of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) 2V(l) + 5CaO(s)

A)1.0 mol

B)1.6 mol

C)2.0 mol

D)2.4 mol

E)4.0 mol

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Page 13

Chapter 12: Acids and Bases

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Sample Questions

Q1) Which is a weak base?

A)NH₃

B)Ca(OH)₂

C)Ba(OH)₂

D)NaOH

E)CH₃COOH

Q2) Which of the following is a weak acid?

A)H₂SO₄

B)HNO₃

C)HF

D)HBr

E)HCl

Q3) What is the concentration of OH in a 0.083 M NaOH solution?

A)0.083 M

B)1.21 × 10¹³ M

C)8.30 × 10¹⁶ M

D)7 M

E)8.30 × 10¹² M

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Chapter 13: Equilibrium

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Sample Questions

Q1) If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as

A)a reversible process.

B)an elementary process.

C)at equilibrium.

D)forbidden.

E)a forward process.

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

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Chapter 14: Organic Chemistry

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Sample Questions

Q1) Which one of these compounds will result from the addition of HCl to CH₃ CH=CH₂?

A)CH₃Cl + CH₂=CH₂

B)CH₃ CHCl=CH₂

C)CH₃ CHCl-CH₃

D)CH₃ CH₂ CH₂Cl

E)None of these choices is correct.

Q2) What name is given to a compound containing a -COOR group?

A)Aldehyde

B)Ketone

C)Alcohol

D)Carboxylic acid

E)Ester

Q3) How many structural isomers are there of C₄H₁₀?

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Page 16

Chapter 15: Biochemistry

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Sample Questions

Q1) Which of the following is not a protein?

A)hormones, such as oxytocin

B)structural substances, such as keratin

C)antibodies, such as immunoglobulin

D)transport facilitators, such as hemoglobin

E)saturated triglycerides, such as triolein

Q2) Which of the following refers to a secondary 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.

Q3) A peptide bond (also called an amide bond) joins two amino acids together.What atoms are linked by this bond?

A)C - O

B)C - H

C)C - N

D)N - S

E)S - C

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Page 17

Chapter 16: Nuclear Chemistry

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Sample Questions

Q1) In the equation below, what particle or type of radiation needs to be included to balance the equation? ²⁰⁸Pb ? + ²⁰⁴Hg

A)Gamma particle

B)Alpha particle

C)Proton

D)Beta particle

E)Positron

Q2) What fraction of radioactive atoms remains in a sample after six half-lives?

A)zero

B)1/6

C)1/16

D)1/32

E)1/64

Q3) Charcoal found under a stone at Stonehenge, England, has a carbon-14 activity that is 0.60 that of new wood.How old is the charcoal? (The half-life of carbon-14 is 5730 years.)

A)Less than 5730 yr

B)Between 5730 and 11,460 yr

C)Between 11,460 and 17,190 yr

D)More than 17,190 yr

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Chapter 17: Electrochemistry

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Sample Questions

Q1) 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)₃ + SnO₂² Bi + SnO₃² (basic solution)

A)32

B)25

C)16

D)13

E)4

Q2) What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H⁺(aq) + NO₃(aq) NO(g) + H₂O(l) + Cu²⁺(aq)

A)Cu

B)H⁺

C)NO₃

D)NO

E)Cu²⁺

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Page 19