Basic Chemistry
Exam Solutions
Course Introduction
Basic Chemistry offers an introduction to the fundamental principles of chemistry, exploring the structure of matter, chemical bonding, and reactions. This course covers topics such as atomic theory, the periodic table, stoichiometry, states of matter, solutions, acids and bases, and chemical energy. Students will develop essential skills in problem-solving, laboratory techniques, and scientific reasoning, providing a strong foundation for further study in scientific disciplines and practical applications in everyday life.
Recommended Textbook
Foundations of College Chemistry 13th Edition by Morris Hein
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Chapter 1: An Introduction to Chemistry
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Sample Questions
Q1) Which has neither a definite shape nor a definite volume?
A)crystal
B)solid
C)gas
D)liquid Answer: C
Q2) A tentative explanation of certain facts that provides the basis for further experimentation is a(n)
A)observation
B)hypothesis
C)theory
D)law
Answer: B
Q3) Which is composed of particles with enough energy to completely overcome the attractive forces between them?
A)solid
B)gas
C)liquid
D)crystal Answer: B
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Chapter 2: Standards for Measurement
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Sample Questions
Q1) When expressed in proper scientific notation the number 0.000034 is
A)3.4 X 10<sup>4</sup>
B)3.4 X 10<sup>-4</sup>
C)3.4 X 10<sup>3</sup>
D)3.4 X 10<sup>-5</sup>
Answer: D
Q2) The density of copper is 8.96g/mL.The volume of 12.0g of copper is
A)0.747g
B)1.34g
C)3.04g
D)108g
Answer: B
Q3) The speed of light is 2.9987 x 10<sup>8</sup> m/s.Convert this speed to km/hr.
A)1.0795 x 10<sup>9</sup> km/hr
B)1.7992 x 10<sup>7</sup> km/hr
C)8.3297 x 10<sup>1</sup> km/hr
D)8.3297 x 10<sup>4</sup> km/hr
Answer: A
Q4) The density of ethanol is 0.7893g/mL.What is the mass of one pint of ethanol?
Answer: The mass of one pint of ethanol is 373.4g
Page 4
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Chapter 3: Elements and Compounds
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Sample Questions
Q1) Which is not a diatomic gas?
A)F<sub>2</sub>
B)N<sub>2</sub>
C)I<sub>2</sub>
D)Cl<sub>2</sub>
Answer: C
Q2) The halogens are in group
A)1A
B)2A
C)3A
D)7A
Answer: D
Q3) Which element is not reactive?
A)Hydrogen
B)Oxygen
C)Iron
D)Helium
Answer: D
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Chapter 4: Properties of Matter
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Sample Questions
Q1) The specific heat of copper is 0.386 J/g<sup>º</sup>C.A 20.0g sample of copper is heated from 25.0<sup>º</sup>C to 35.0<sup>º</sup>C.How much heat did the copper absorb?
A)837 J
B)77.2 J
C)194 J
D)270 J
Q2) If 100.0g of a fuel can raise the temperature of 8.00L of water from 22.0<sup>º</sup>C to 98.0<sup>º</sup>C,howmuch heat is given off by 1.00g of the fuel?
Q3) To heat 12.4g of water from 20.0<sup>º</sup>C to 25.0<sup>º</sup>C requires
A)1040 J
B)1300 J
C)259 J
D)1050 J
Q4) According to the Law of Conservation of Energy,energy can be A)created.
B)destroyed.
C)created and destroyed.
D)converted from one form to another.
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Chapter 5: Early Atomic Theory and Structure
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Sample Questions
Q1) The majority of the volume of an atom is empty space.
A)True
B)False
Q2) A substance has 15 protons,16 neutrons,and 15 electrons.Which isotope is it?
A)P-30
B)P-31
C)S-30
D)S-31
Q3) The concept that most of the atom's mass is concentrated in a small nucleus surrounded by electrons was the contribution of <sup> </sup>
A)Dalton
B)Thomson
C)Rutherford
D)Chadwick
Q4) The number of protons in an atom of sodium-23 is
A)11
B)12
C)16
D)23
Q5) How are the different isotopes of an element alike;how are they different?
Page 7
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Chapter 6: Nomenclature of Inorganic Compounds
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Sample Questions
Q1) NO<sub>3</sub><sup> -1</sup> is the nitrite ion.
A)True
B)False
Q2) CO is a molecular compound.
A)True
B)False
Q3) The metals in group 2A form ions with a charge of
A)+1
B)+2
C)-1
D)-2
Q4) Which compound's name ends in -ide?
A)KCl
B)KClO
C)KClO<sub>2</sub>
D)KClO<sub>3</sub>
Q5) When a chemical formula is written,the more metallic element is placed first. A)True
B)False
Q6) Identify four elements that can form more than one cation.
Page 8
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Chapter 7: Quantitative Composition of Compounds
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Sample Questions
Q1) One mole of glucose,C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>,contains 24 moles of atoms.
A)True
B)False
Q2) What is the percent by mass of hydrogen in sulfuric acid?
A)1.04%
B)2.06%
C)4.03%
D)5.93%
Q3) What is the molecular formula of a compound with the empirical formula CH and molar mass of 26.04g?
A)CH
B)C<sub>2</sub>H
C)CH<sub>2</sub>
D)C<sub>2</sub>H<sub>2</sub>
Q4) One mole of oxygen has a mass of 8.00g.
A)True
B)False
Q5) An x-gram sample of P<sub>4</sub>O<sub>6</sub> contains 455 g of phosphorus.Calculate x.
Page 9
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Chapter 8: Chemical Equations
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Sample Questions
Q1) The formula of the salt produced from the neutralization reaction between nitric acid and barium hydroxide is:
A)H<sub>2</sub>O
B)NO<sub>3</sub>OH
C)Ba(NO<sub>3</sub>)<sub>2</sub>
D)Ba(OH)<sub>2</sub>
Q2) The products of the complete combustion of the hydrocarbon methane are A)carbon monoxide and water.
B)carbon dioxide and water.
C)carbon monoxide and hydrogen.
D)carbon dioxide and hydrogen.
Q3) Complete and balance the equation for each example in which a double-displacement reaction will occur.If no reaction will occur write the words "No Reaction" on the right side of the equation
A.AlBr<sub>3</sub> + AgNO<sub>3</sub> \(\rarr\)
B.ZnBr<sub>2</sub> + Na<sub>2</sub>S \(\rarr\)
C.NH<sub>4</sub>Br + AlI<sub>3</sub> \(\rarr\)
D.K<sub>2</sub>CO<sub>3</sub> + HCl \(\rarr\)
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Chapter 9: Calculations From Chemical Equations
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Q1) How many moles of N<sub>2</sub> will be consumed when 1.60 moles of H<sub>2</sub> react completely in the following equation?<sub> </sub> N<sub>2</sub> + 3H<sub>2</sub> \(\rarr\) 2NH<sub>3</sub>
A)0.533
B)1.60
C)3.20
D)4.80
Q2) Which substance is in excess when 1.50 moles of aluminum bromide are reacted with 2.50 moles of barium hydroxide in the following equation? 2AlBr<sub>3</sub> + 3Ba(OH)<sub>2</sub> \(\rarr\) 3BaBr<sub>2</sub> + 2Al(OH)<sub>3</sub>
A)BaBr<sub>2</sub>
B)Al(OH)<sub>3</sub>
C)Ba(OH)<sub>2</sub>
D)AlBr<sub>3</sub>
Q3) In the following equation,2C + O<sub>2</sub> \(\rarr\) 2CO,the mole ratio of oxygen to carbon is 2:1.
A)True
B)False
Q4) Nitrogen gas to water
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Chapter 10: Modern Atomic Theory and the Periodic Table
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Sample Questions
Q1) How many unpaired electrons are in the ground state electron configuration of each of the following elements?
A.Boron
B.Selenium
C.Chlorine
D.Krypton
Q2) The "alkali" metals are in group
A)1A
B)2A
C)7A
D)8A
Q3) How many valence electrons are in a carbon atom in the ground state?
A)2
B)4
C)6
D)8
Q4) List the following orbitals in order of increasing energy: 4d,3p,1s,2p,4p,5s,3d,2s,6s,5p,4s,and 3s.
Q5) In the designation 4p<sup>3</sup>;what is the significance of 4,p,and 3?
Q6) Explain how a bright line spectrum is produced.
Page 12
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Chapter 11: Chemical Bonds: the Formation of Compounds
From Atoms
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Sample Questions
Q1) The series,F,Cl,P,K is arranged in order of decreasing electronegativity..
A)True
B)False
Q2) Which type of chemical bond involves the equal sharing of electrons?
A)Ionic
B)Polar covalent
C)Nonpolar covalent
Q3) Using Lewis electron dot symbols,show how potassium sulfide forms from its elements.
Q4) Which of the following statements is true for most atoms?
A)In general,as the atomic radius increases,the first ionization energy increases.
B)In general,as the atomic radius increases,the first ionization energy decreases.
C)In general,as the first ionization energy decreases,the electronegativity increases.
D)No correct answer is given.
Q5) The element with the highest electronegativity is fluorine.
A)True
B)False
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Chapter 12: The Gaseous State of Matter
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Sample Questions
Q1) A sample of gas has a volume of 850.mL at 23.0<sup> </sup><sup>°</sup><sup> </sup>C and 1.10 atm.The temperature is increased to 33.0<sup> </sup><sup>°</sup><sup> </sup>C,at what pressure will its volume be 900.mL?
A)1.20 atm
B)1.49 atm
C)1.07 atm
D)0.812 atm
Q2) A sample of gas has a volume of 400.mL at STP.What will be its volume at 20.0<sup> </sup><sup>°</sup><sup> </sup>C and700.torr?
A)466 mL
B)343 mL
C)60.1 mL
D)2660 mL
Q3) A small,0.500 mL,bubble forms at the bottom of a lake where the temperature is 2.0<sup> </sup><sup>°</sup>C and the pressure is 2.40 atm.What volume will the bubble occupy near the surface wherethe temperature is 32.0<sup> </sup><sup>°</sup><sup> </sup>C and the pressure is 1.10 atm?
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Chapter 13: Liquids
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Sample Questions
Q1) As the attractive forces between the molecules of a liquid increase,its surface tension
A)increases.
B)decreases.
C)remains the same.
Q2) The freezing point of a substance is the temperature at which its
A)solid phase is in equilibrium with its gaseous phase.
B)liquid phase is in equilibrium with its gaseous phase.
C)solid phase is in equilibrium with its liquid phase.
Q3) Which is an acidic anhydride?
A)Magnesium oxide
B)Sulfur trioxide
C)Lithium oxide
D)Sodium oxide
Q4) What quantity of heat is required to change 40.0 g of ice at melting point to liquid water? The heat of fusion of ice is 335 J/g.
A)13400 J
B)0.119 J
C)8.38 J
D)375 J
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Chapter 14: Solutions
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Sample Questions
Q1) Polar molecules tend to be soluble in water.
A)True
B)False
Q2) As pressure increases,the solubility of a gas in water
A)increases.
B)decreases.
C)remains the same.
Q3) A solution made by dissolving 20.g of NaCl in 100.0 mL of water has the same % by mass as a solution made by dissolving 10.0 g of NaCl in 50.0 mL of water.
A)True
B)False
Q4) What is the molarity of a solution in which 1.20 moles of solute is dissolved in 3.00 L of solution?
A)0.400 M
B)15.0 M
C)3.60 M
D)360.M
Q5) 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?
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Chapter 15: Acids, Bases, and Salts
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Sample Questions
Q1) An electrolyte is a substance whose aqueous solution conducts an electric current.
A)True
B)False
Q2) The pH of a solution can be calculated from the expression
A)pH = - log [OH<sup> -1</sup>]
B)pH = log [OH<sup> -1</sup>]
C)pH = - log [H<sup> +1</sup>]
D)pH = log [H<sup> +1</sup>]
Q3) What is the conjugate acid of OH<sup> -1</sup>?
A)O<sup>-2</sup>
B)H<sup> +1</sup>
C)O<sub>2</sub>H
D)HOH
Q4) A 20.0 mL sample of nitric acid is titrated to a neutral end point by the addition of 3.60 mL of a 0.80 M solution of barium hydroxide.
A.Write a balanced formula equation for this reaction.
B.What is the molarity of the nitric acid solution in this question?
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Chapter 16: Chemical Equilibrium
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Sample Questions
Q1) What is the pH of a 0.00500 M solution of barium hydroxide?
A)11.7
B)12.0
C)2.00
D)2.30
Q2) An aqueous solution containing both Na<sub>3</sub>PO<sub>4</sub> and Na<sub>2</sub>HPO<sub>4</sub> will act as a buffer.
A)True
B)False
Q3) Which solution has the lowest pH?
A)0.1 M HNO<sub>2</sub>
B)0.1 M HCl<sup> </sup> <sup> </sup>
C)0.1 M KOH
D)0.1 M NH<sub>4</sub>OH
Q4) What is the pH of a 0.10 M KOH solution?
A)1
B)7
C)13
D)14
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Chapter 17: Oxidationreduction
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Sample Questions
Q1) Which element forms ions that will migrate toward the anode in an electrolytic cell?
A)Silver
B)Chlorine
C)Copper
D)Sodium
Q2) In an electrolytic cell
A)a chemical reaction occurs spontaneously and releases energy as electricity.
B)electricity causes a chemical reaction to occur.
C)a physical change occurs spontaneously and releases energy as electricity.
D)electricity causes a physical change to occur.
Q3) In the electrolysis of fused (molten)sodium chloride,the product at the cathode is
A)Na<sup>+1</sup>
B)Na
C)Cl<sup>-1</sup>
D)Cl<sub>2</sub>
Q4) During a redox reaction,the reducing agent is oxidized.
A)True
B)False
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Chapter 18: Nuclear Chemistry
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Sample Questions
Q1) Part of a radioactive decay series begins with U-238 emitting in succession a(n)
A.Alpha particle
B.Beta particle
C.Beta particle
D.Alpha particle
E.Alpha particle
Predict the product of each successive emission.
Q2) A beta particle consists of two protons and two neutrons.
A)True
B)False
Q3) In a fusion reaction a nucleus of H-3 and a nucleus of H-1 combine to form a nucleus of
A)He-4
B)H-4
C)H-2
D)Li-4
Q4) Nuclear fusion is the process of uniting two light nuclei to form one heavier nucleus.
A)True
B)False
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Chapter 19: Introduction to Organic Chemistry Online Only
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Sample Questions
Q1) Which hydrocarbon can undergo an addition reaction?
A)CH<sub>4</sub>
B)C<sub>2</sub>H<sub>4</sub>
C)C<sub>2</sub>H<sub>6</sub>
D)C<sub>3</sub>H<sub>8</sub>
Q2) Which hydrocarbon series contains a triple covalent bond between carbon atoms?
A)Alkynes
B)Alkanes
C)Alkenes
D)Aromatics
Q3) Which pair contains two molecules from the same homologous series of hydrocarbons?
A)CH<sub>4</sub> and C<sub>2</sub>H<sub>2</sub>
B)C<sub>2</sub>H<sub>6</sub> and C<sub>5</sub>H<sub>12</sub>
C)C<sub>2</sub>H<sub>6</sub> and C<sub>3</sub>H<sub>6</sub>
D)C<sub>2</sub>H<sub>2</sub> and C<sub>2</sub>H<sub>6</sub>
Q4) Prepare a chart in which you name the four major homologous series of hydrocarbons,state the type of bonding found in each,write the general formula for each,write the molecular formula and name of the first member of each series.
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) Plants store food energy as A)glycogen.
B)glucagon.
C)starch.
D)protein.
Q2) The raw material for the repair and replacement of worn out tissue comes from A)lipids.
B)carbohydrates. C)proteins.
D)nucleic acids.
Q3) The protein portion of a conjugated enzyme is the A)apoenzyme.
B)dienzyme.
C)coenzyme.
D)sterioenzyme.
Q4) A human body contains approximately 5.80 L of blood.If the concentration of glucose in the blood is 0.00500 M,calculate the following:
A.The total mass of glucose in the blood
B.The number of molecules of glucose in the blood
Q5) Draw the structure of the dipeptide formed by serine and proline.
22
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