Basic Chemistry Test Bank

Course Introduction

Basic Chemistry introduces students to the foundational principles of chemistry and how they apply to everyday life. The course covers essential topics such as atomic structure, the periodic table, chemical bonding, chemical reactions, stoichiometry, states of matter, and the properties of acids and bases. Emphasis is placed on developing problem-solving skills and understanding fundamental concepts through practical examples and laboratory exercises. By the end of the course, students should be able to explain chemical phenomena, perform basic calculations relevant to chemical processes, and safely handle common laboratory materials.

Recommended Textbook

Foundations of College Chemistry 13th Edition by Morris Hein

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20 Chapters

2040 Verified Questions

2040 Flashcards

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Page 2

Chapter 1: An Introduction to Chemistry

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56 Verified Questions

56 Flashcards

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Sample Questions

Q1) "When Jill opened the bottle containing a clear liquid,the whole room smelled likeroses." Based on this statement we can infer that:

A)The liquid is a homogeneous mixture.

B)The liquid is a compound.

C)Inside the bottle there were a liquid and a gas.

D)Opening the bottle caused the liquid to evaporate.

Answer: C

Q2) Which has both a definite shape and a definite volume?

A)solid

B)vapor

C)gas

D)liquid

Answer: A

Q3) Which has neither a definite shape nor a definite volume?

A)crystal

B)solid

C)gas

D)liquid

Answer: C

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Page 3

Chapter 2: Standards for Measurement

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106 Verified Questions

106 Flashcards

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Sample Questions

Q1) Subtract 14.3 from 130.670.The difference expressed to the correct number of significant figures is

A)116

B)116.3

C)116.4

D)116.37

Answer: C

Q2) The number,14.74999,when rounded to three digits is

A)15.0

B)14.8

C)14.7

D)10.0

Answer: C

Q3) How many significant figures are in the number 14.04?

A)1

B)2 C)3

D)4

Answer: D

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Page 4

Chapter 3: Elements and Compounds

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108 Flashcards

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Sample Questions

Q1) Which element is not reactive?

A)Hydrogen

B)Oxygen

C)Iron

D)Helium

Answer: D

Q2) The ultimate particle of water is a(n) A)atom.

B)molecule.

C)anion.

D)cation.

Answer: B

Q3) The symbol for one crystalline form of sulfur is S8.This symbol indicates A)one molecule composed of eight atoms.

B)eight molecules.

C)one atom composed of eight molecules.

D)one ion containing eight electrical charges.

Answer: A

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Chapter 4: Properties of Matter

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Sample Questions

Q1) The specific heat of aluminum is 0.900 J/gºC.A 300.0g sample of aluminum at 300.0ºC is dropped into 200.0g of water at 20.0ºC.Assume no heat is lost to the environment.

A.What will be the final temperature of the water?

B.What will be the final temperature of the aluminum?

Q2) The correct SI unit for energy is the joule.

A)True

B)False

Q3) According to the Law of Conservation of Mass,matter can be A)created.

B)destroyed.

C)created and destroyed.

D)converted from one form to another.

Q4) 8.50g of potassium combines with 7.71g of chlorine to form potassium chloride.What is the percent by mass of potassium in potassium chloride?

A)52.4%

B)64.8%

C)47.6%

D)60.7%

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Chapter 5: Early Atomic Theory and Structure

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Sample Questions

Q1) Naturally occurring neon exists as three isotopes.90.51% is Ne-20 with a mass of 19.99 amu,0.27% is Ne-21 with a mass of 20.99 amu,and 9.22% is Ne-22 with a mass of 21.99 amu.What is the atomic mass of neon?

A)10.00 amu

B)20.18 amu

C)20.99 amu

D)62.97 amu

Q2) What is the atomic number of magnesium?

A)12

B)24

C)25

D)55

Q3) One isotope of oxygen has the atomic number 8 and the mass number 18.An atom of this isotope contains

A)8 neutrons

B)10 electrons

C)8 protons

D)18 electrons

Q4) How are the different isotopes of an element alike;how are they different?

Q5) Explain why the atomic masses of elements are not whole numbers.

Page 7

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Chapter 6: Nomenclature of Inorganic Compounds

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Sample Questions

Q1) An oxide ion forms when an oxygen atom

A)gains one electron.

B)gains two electrons.

C)goses one electron.

D)goses two electrons.

Q2) The formula of an ionic compound is XY.Which pair of atoms is most likely to be X and Y?

A)Na and K

B)Li and S

C)K and N

D)Ca and O

Q3) HNO2 is

A)nitric acid.

B)nitrous acid.

C)hydronitric acid.

D)hydronitrous acid.

Q4) The formula of copper (II)sulfate is Cu2S.

A)True

B)False

Q5) Identify four elements that can form more than one cation.

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Chapter 7: Quantitative Composition of Compounds

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Sample Questions

Q1) What is the molecular formula of a compound with the empirical formula

CHO2 and molar mass of 90.04g?

A)CHO2

B)C2H2O4

C)C3H3O6

D)C4H4O8

Q2) How many moles are present in 0.140g of HCl?

A)0.140 moles

B)0.00384 moles

C)1.40 moles

D)5.01 moles

Q3) In which pair would both compounds have the same empirical formula?

A)C2H4 and C3H6

B)K2CrO4 and K2Cr2O7

C)NaHCO3 and Na2CO3

D)FeCl3 and FeCl2

Q4) A sample of magnesium with a mass of 7.76g is combined with 15.00g of sulfur to produce magnesium sulfide.What mass of sulfur does not react?

Q5) How many carbon atoms have about the same mass as one mole of titanium atoms?

Page 9

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Chapter 8: Chemical Equations

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Sample Questions

Q1) Sulfuric acid is prepared commercially by the following series of reactions:

A.Sulfur is burned in oxygen to produce sulfur dioxide.

B.Sulfur dioxide is further reacted with oxygen to form sulfur trioxide.

C.Sulfur trioxide is reacted with sulfuric acid to produce pyrosulfuric acid,H2S2O7.

D.Pyrosulfuric acid is reacted with water to produce sulfuric acid. Write a balanced chemical equation for each step in the commercial production of sulfuric acid.

Q2) When the equation Cr2S3 + HCl \(\rarr\) CrCl3 + H2S is balanced,a term in the balanced equation is A)3HCl

B)CrCl3

C)3H2S

D)2Cr2S3

Q3) The Greenhouse Effect is causing global warming.

A)True

B)False

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Page 10

Chapter 9: Calculations From Chemical Equations

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101 Flashcards

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Sample Questions

Q1) Which is the limiting reactant when 3.00 moles of MnO2 are reacted with 10.0 moles of HClin the following equation? MnO2 + 4HCl \(\rarr\)MnCl2 + 2H2O + Cl2

A)MnO2

B)HCl

C)MnCl2

D)H2O

Q2) How many moles of Cl2 are consumed when 0.500 moles of AlCl3 are produced in the following equation? 2Al + 3Cl2 \(\rarr\) 2AlCl3

A)0.333

B)0.500

C)0.750

D)1.00

Q3) In all chemical reactions,the reactants are always completely consumed.

A)True

B)False

Q4) The limiting reactant in a chemical reaction is the substance in excess.

A)True

B)False

Page 11

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Chapter 10: Modern Atomic Theory and the Periodic Table

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Sample Questions

Q1) Atoms of which element have the following electron configuration? 1s2 2s2 2p6 3s1

A)Sulfur

B)Strontium

C)Sodium

D)Nitrogen

Q2) On the periodic table,the "transition elements" fill their last electrons in the _____ sublevel.

A)s

B)p

C)d

D)f

Q3) Each horizontal row on the periodic table is called a A)period

B)family

C)group

D)cohort

Q4) In the ground state,electrons tend to occupy orbitals of the lowest energy. A)True

B)False

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Chapter 11: Chemical Bonds: the Formation of Compounds

From Atoms

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102 Verified Questions

102 Flashcards

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Sample Questions

Q1) Which of the following characterizes covalent bonding?

A)The formation of ions

B)The type of bond normally found between metals and nonmetals

C)The loss of electrons

D)The formation of true,discrete molecules

Q2) Which type of chemical bond involves the transfer of electrons?

A)Ionic

B)Polar covalent

C)Nonpolar covalent

Q3) What is the empirical formula of lithium nitride?

A)LiN

B)Li3N

C)LiN3

D)Li2N

Q4) The shape of a carbon dioxide molecule is A)bent.

B)linear.

C)trigonal planar.

D)tetrahedral.

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Chapter 12: The Gaseous State of Matter

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Sample Questions

Q1) What volume of sulfur dioxide gas will be consumed when 12.0 L of oxygen is consumed in the following equation? 2 SO2(g)+ O2(g)\(\rarr\) 2 SO3(g)

A)6.00 L

B)12.0 L

C)24.0 L

D)60.0 L

Q2) The volume of a gas,at constant temperature,is inversely proportional to its pressure. A)True

B)False

Q3) A 3.00 L sample of a gas at a pressure of 4.00 atm is compressed to 2.00 L at a constant temperature.What is the pressure of the gas?

A)2.00 atm

B)6.00 atm

C)12.0 atm

D)24.0 atm

Q4) What is the molar mass of a gas if 36.4 g of the gas occupies 100.0 L at 32.0 ° C and 0.800 atm?

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Page 14

Chapter 13: Liquids

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Sample Questions

Q1) How many moles of water will be produced when 15.0 g of calcium chloride dihydrate are heated?

A)0.134 moles

B)0.0510 moles

C)0.204 moles

D)0.102 moles

Q2) Which of the following properties of water is not affected by hydrogen bonding?

A)Boiling point

B)Freezing point

C)Vapor pressure

D)Molar mass

Q3) A hydrogen bond is

A)a covalent bond between water molecules

B)a dipole-dipole attraction between molecules that contain H bonded to F,O,or N.

C)an ionic bond between water molecules.

D)a covalent bond between molecules that contain H bonded to F,O,or N.

Q4) Water purification often involves screening,flocculation and sedimentation,sand filtration,aeration,and disinfection.Explain what is meant by each of these terms.

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Page 15

Chapter 14: Solutions

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100 Flashcards

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Sample Questions

Q1) A sulfuric acid solution that is 34.0 % by mass has a density of 1.25 g/mL. What is the molarity of the solution?

Q2) What is the molarity of the resulting solution when 20.0 mL of a 2.00 M aqueous solution is diluted by the addition of 30.0 mL of water?

A)5.00 M

B)3.00 M

C)1.33 M

D)0.800 M

Q3) What mass of ethanol,C2H5OH,is required to decrease the freezing point of 2.000 L of water to -10.00° C? (The freezing point depression constant for water is 1.86° C/m)

Q4) The freezing point of pure water is 273 K.As a solute dissolves in water,the freezing point of the solution will A)increase.

B)decrease.

C)remain the same.

Q5) Salt water has a higher freezing point than pure water.

A)True

B)False

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Chapter 15: Acids, Bases, and Salts

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Sample Questions

Q1) In a basic solution the

A)concentration of hydronium ion is greater than that of hydroxide ion

B)concentration of hydroxide ion is greater than that of hydronium ion

C)concentration of hydronium ion and hydroxide ion are equal

Q2) Arrhenius defined an acid as a substance whose aqueous solution contains an excess of

A)sodium ion.

B)hydroxide ion.

C)chloride ion.

D)hydrogen ion.

Q3) According to the Lewis acid definition,an acid is a substance that is able to accept a pair of electrons.

A)True

B)False

Q4) A solution of a strong acid has a pH of 3.The concentration of hydronium ions in this solution is

A)0.001 M

B)3 M

C)0.3 M.

D)0.003 M

Page 17

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Chapter 16: Chemical Equilibrium

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Sample Questions

Q1) The main reason for the increase in the rate of reaction as temperature increases is A)molecules can be closer together to react.

B)the number or frequency of collisions between molecules increases.

C)molecules have less energy to move away from each other.

D)more energy is available to overcome the activation energy.

Q2) Which solution has the highest pH?

A)0.1 M HNO2

B)0.1 M HCl

C)0.1 M KOH

D)0.1 M NH4Cl

Q3) The addition of a catalyst will change the value of Keq in an equilibrium system.

A)True

B)False

Q4) Equilibrium is reached in a chemical reaction when

A)the reactants are completely consumed.

B)the concentrations of all reactants and products become equal.

C)the rates of the opposing reactions become equal.

D)the forward and reverse reactions stop.

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Chapter 17: Oxidationreduction

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Sample Questions

Q1) What is the oxidation number of chromium in Cr2O7-2?

A)+12

B)0

C)+6 D)-4

Q2) In the electrolysis of fused (molten)calcium chloride,the product at the anode is

A)Cl-1

B)Cl2

C)Ca+2

D)Ca

Q3) Which species is oxidized in the following equation? 2 H2O \(\rarr\) 2

H2 + O2

A)H2

B)O2

C)H+1

D)O-2

Q4) Explain why in a voltaic cell the anode is negative and the cathode is positive.

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Page 19

Chapter 18: Nuclear Chemistry

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Sample Questions

Q1) When Kr-85 emits gamma radiation,the remaining nucleus is

A)Rb-85

B)Se-81

C)Kr-85

D)Rb-84

Q2) The nucleus of Fe-56 has a mass of 55.9207 amu.

The mass of a proton is 1.0073 amu.

The mass of a neutron is 1.0087 amu.

A mass defect of 1.0000 g indicates a binding energy of 9.0 X 1013 joules.

A.Calculate the mass defect of Fe-56 in g/mole.

B.Calculate the nuclear binding energy of Fe-56 in J/mole.

Q3) Bismuth-214 can be formed by either alpha or beta decay.The two isotopes that can do this are

A)Po-214 and At-218

B)Pb-214 and Tl-210

C)Po-218 and Bi-210

D)Pb-214 and At-218

Q4) Define the term "half-life".Why are half-lives important when using radioactive tracers for medical purposes?

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Chapter 19: Introduction to Organic Chemistry Online Only

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Sample Questions

Q1) What is the total number of carbon atoms in a molecule of 2-methyl-4-ethyloctane?

A)8

B)11

C)14

D)17

Q2) Two or more different compounds with the same molecular formula are

A)Isomers

B)Isotopes

C)Hypermeres

D)Hypertopes

Q3) Both C2H4 and C4H8 belong to the alkyne series.

A)True

B)False

Q4) All the isomers of C3H8O have the same properties.

A)True

B)False

Q5) Name and write the formulas for the three structural isomers of pentane.

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Chapter 20: Introduction to Biochemistry Online Only

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Sample Questions

Q1) Carbohydrates supply about 17 kJ of energy per gram.What mass of glucose would yieldapproximately 340 kJ of energy?

A)5800 g

B)0.050 g

C)20.g

D)357 g

Q2) A complex carbohydrate is a A)protein.

B)polypeptide.

C)lipid.

D)polysaccharide.

Q3) Which is a monosaccharide?

A)Sucrose

B)Fructose

C)Lactose

D)Maltose

Q4) Fats are digested in the stomach and converted to glucose.

A)True

B)False

Q5) Explain the structure of DNA.

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