Course Introduction
General Chemistry I Solved Exam Questions
General Chemistry I introduces fundamental concepts in chemistry with an emphasis on the structure and properties of matter, atomic theory, periodic trends, chemical bonding, stoichiometry, and chemical reactions. The course covers the foundational principles that explain how and why chemical reactions occur, the quantitative relationships in chemical processes, and the basic behavior of gases, liquids, and solids. Laboratory work is often integrated to develop practical skills and reinforce theoretical concepts through hands-on experimentation, preparing students for more advanced studies in chemistry and related fields.
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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50 Verified Questions
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Sample Questions
Q1) Which one of these elements is a transition element?
A)Sr
B)Pb
C)As
D)Fe
E)H
Answer: D
Q2) The alkali metal elements are found in _______ of the periodic table.
A)Group 1A
B)Group 2A
C)Group 3A
D)Period 7
E)Period 1
Answer: A
Q3) C(graphite) and C(diamond) are examples of:
A)isotopes of carbon.
B)allotropes of carbon.
C)the law of definite proportions.
D)different carbon ions.
Answer: B
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Chapter 2: Electrons and the Periodic Table
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107 Verified Questions
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Sample Questions
Q1) Which of these species make an isoelectronic pair: Cl<sup> </sup>, O<sup>2 </sup>, F, Ca<sup>2+</sup>, Fe<sup>3</sup><sup>+</sup>?
A)Ca<sup>2+</sup> and Fe<sup>3+</sup>
B)O<sup>2 </sup> and F
C)F and Cl<sup> </sup>
D)Cl<sup> </sup> and Ca<sup>2+</sup>
E)None of the above species are part of an isoelectronic series.
Answer: D
Q2) How many dots does the Lewis dot symbol for magnesium have around it?
A)1
B)2
C)0
D)3
E)7
Answer: B
Q3) Each shell (principal energy level) of quantum number n contains n subshells.
A)True
B)False
Answer: True
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Page 4
Chapter 3: Compounds and Chemical Bonds
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Sample Questions
Q1) Which of these compounds is most likely to be covalent?
A)Rb<sub>2</sub>S
B)SrCl<sub>2</sub>
C)CS<sub>2</sub>
D)CaO
E)MgI<sub>2</sub>
Answer: C
Q2) Which one of the following formulas of ionic compounds is the least likely to be correct?
A)NH<sub>4</sub>Cl
B)Ba(OH)<sub>2</sub>
C)Na<sub>2</sub>SO<sub>4</sub>
D)Ca<sub>2</sub>NO<sub>3</sub>
E)Cu(CN)<sub>2</sub>
Answer: D
Q3) The rusting of a piece of iron under environmental conditions is a physical change.
A)True
B)False
Answer: False
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Page 5
Chapter 4: How Chemists Use Numbers
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Sample Questions
Q1) The density of mercury, the only metal to exist as a liquid at room temperature, is 13.6 g/cm<sup>3</sup>.What is that density in pounds per cubic inch? (1 in = 2.54 cm; 1 lb = 454 g)
A)849 lb/in<sup>3</sup>
B)491 lb/in<sup>3</sup>
C)376 lb/in<sup>3</sup>
D)0.491 lb/in<sup>3</sup>
E)1.83 × 10<sup> </sup><sup>3</sup> lb/in<sup>3</sup>
Q2) Select the smallest unit.
A)mm
B) m
C)nm
D)km
E)dm
Q3) The number 1.050 × 10<sup>9</sup> has how many significant figures?
E)13
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Chapter 5: The Mole and Chemical Formulas
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Sample Questions
Q1) What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?
A)4.0 × 10<sup>2</sup> g
B)25.0 g
C)17.0 g
D)4.00 × 10<sup> </sup><sup>2</sup> g
E)2.50 × 10<sup> </sup><sup>3</sup> g
Q2) What is the mass of 0.0250 mol of P<sub>2</sub>O<sub>5</sub>?
A)35.5 g
B)5676 g
C)0.0250 g
D)1.51 × 10<sup>22</sup> g
E)3.55 g
Q3) What is the mass, in grams, of one arsenic atom? (N<sub>A</sub> = 6.022 × 10<sup>23</sup> mol<sup> </sup><sup>1</sup>)
A)5.48× 10<sup> </sup><sup>23</sup> g
B)33.0 g
C)74.9 g
D)1.24 × 10<sup> </sup><sup>22</sup> g
E)8.04 × 10<sup>21</sup> g
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Page 7
Chapter 6: Molecular Shape
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Sample Questions
Q1) Place the following in order of increasing electronegativity. Cs O S
A)O < S < Cs
B)S < O < Cs
C)Cs < S < O
D)Cs < O < S
E)O < Cs < S
Q2) What does the abbreviation VSEPR stand for?
A)Very Specific Electron and Proton Repair
B)Variable Selective of Electron and Protons
C)Valence Shell for Every Proton
D)Very Selective Electron Pair theory
E)Valence-Shell Electron-Pair Repulsion
Q3) Which one of the following pure substance has both dispersion forces and dipole-dipole forces?
A)HCl
B)BCl<sub>3</sub>
C)Br<sub>2</sub>
D)H<sub>2</sub>
E)CO<sub>2</sub>
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Chapter 7: Solids, Liquids, and Phase Changes
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Sample Questions
Q1) What is the process in which molecules undergo a phase change from the liquid phase to the gas phase?
A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation
Q2) Which of the substances would form an ionic solid?
A)NCl<sub>3</sub>
B)NH<sub>4</sub>Cl
C)Ag
D)He
E)OF<sub>2</sub>
Q3) Which state of matter is described as taking on the shape and volume of its container?
A)solid
B)liquid
C)gas
D)solution
E)mixture
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Chapter 8: Gases
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Sample Questions
Q1) What is the volume occupied by 35.2 g of methane gas (CH<sub>4</sub>) at 25°C and 1.0 atm? (R = 0.08206 L atm/K mol)
A)0.0186 L
B)4.5 L
C)11.2 L
D)49.2 L
E)53.7 L
Q2) What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?
A)163 K
B)294 K
C)3.09 K
D)217 K
E)475 K
Q3) Which of the following is/are characteristic(s) of gases?
A)High compressibility
B)Relatively large distances between molecules
C)Formation of homogeneous mixtures regardless of the nature of gases
D)Choice 1 and 2 only
E)Choice 1, 2, and 3
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Chapter 9: Physical Properties of Solutions
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Sample Questions
Q1) What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H<sub>3</sub>PO<sub>4</sub>?
A)0.20 L
B)0.57 L
C)1.8 L
D)3.6 L
E)5.1 L
Q2) Determine the molarity of a solution made by dissolving 11.7 g of NaNO<sub>3</sub> in water where the final volume of the solution is 250.0 mL.
A)0.138 M
B)0.551 M
C)0.0468 M
D)0.0311 M
E)0.214 M
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11
Chapter 10: Chemical Reactions and Chemical Equations
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Sample Questions
Q1) Balance the following equation: Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + SiO<sub>2</sub>(s) + C(s) CaSiO<sub>3</sub>(s) + CO(g) + P<sub>4</sub>(s)
A)Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + 3SiO<sub>2</sub>(s) + 8C(s)
3CaSiO<sub>3</sub>(s) + 8CO(g) + P<sub>4</sub>(s)
B)Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + 3SiO<sub>2</sub>(s) + 14C(s)
3CaSiO<sub>3</sub>(s) + 14CO(g) + P<sub>4</sub>(s)
C)Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + 3SiO<sub>2</sub>(s) + 8C(s)
3CaSiO<sub>3</sub>(s) + 8CO(g) + 2P<sub>4</sub>(s)
D)2Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + 6SiO<sub>2</sub>(s) + 10C(s)
6CaSiO<sub>3</sub>(s) + 10CO(g) + P<sub>4</sub>(s)
E)2Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s) + 6SiO<sub>2</sub>(s) + 10C(s)
6CaSiO<sub>3</sub>(s) + 10CO(g) + 4P<sub>4</sub>(s)
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Chapter 11: Using Balanced Chemical Equations
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Sample Questions
Q1) What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO<sub>2</sub> in excess HCl(aq)? MnO<sub>2</sub>(s) + 4HCl(aq) MnCl<sub>2</sub>(aq) + 2H<sub>2</sub>O(l) + Cl<sub>2</sub>(g) (R = 0.08206 L atm/K mol)
A)5.36 × 10<sup> 3</sup> L
B)0.138 L
C)0.282 L
D)3.09 L
E)3.55 L
Q2) What volume of 0.200 M H<sub>2</sub>SO<sub>4</sub> solution is required to react exactly with 50.0 mL of 0.100 M KOH? H<sub>2</sub>SO<sub>4</sub>(aq) + 2KOH(aq) 2H<sub>2</sub>O(l) + K<sub>2</sub>SO<sub>4</sub>(aq)
A)62.5 mL
B)12.5 mL
C)50.0 mL
D)25.0 mL
E)75.0 mL
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Page 13
Chapter 12: Acids and Bases
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Sample Questions
Q1) What is the pOH of a 0.025 M HI solution?
A)0.025
B)0.94
C)1.60
D)12.40
E)10.31
Q2) The substance NH<sub>3</sub> is considered to be
A)a weak acid.
B)a weak base.
C)a strong acid.
D)a strong base.
E)neither acidic nor basic.
Q3) What is the conjugate acid of the acetate ion?
A)CH<sub>3</sub>O<sup>2 </sup>
B)COOH
C)HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub>
D)H<sub>2</sub>O
E)CH<sub>4</sub>
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14
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) During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?
A)Elementary process
B)Reversible reaction
C)Rate law
D)Rate constant
E)Equilibrium
Q3) At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.
A)True
B)False
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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 CH<sub>3</sub> CH=CH<sub>2</sub>?
A)CH<sub>3</sub>Cl + CH<sub>2</sub>=CH<sub>2</sub>
B)CH<sub>3</sub> CHCl=CH<sub>2</sub>
C)CH<sub>3</sub> CHCl-CH<sub>3</sub>
D)CH<sub>3</sub> CH<sub>2</sub> CH<sub>2</sub>Cl
E)None of these choices is correct.
Q2) Which class or family of compounds contains both the carbonyl group and the amine group?
A)Alcohols
B)Esters
C)Amide
D)Carbohydrates
E)Ketones
Q3) Organic chemistry is defined as the study of compounds containing which element?
A)Carbon
B)Silicon
C)Hydrogen
D)Sodium
E)Carbon and hydrogen
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Chapter 15: Biochemistry
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Sample Questions
Q1) Which of the following describes a steroid?
A)A group of molecules that have a special grouping of 5- and 6-member rings in common.
B)A relatively small, water-soluble molecule that contains either a ketone or an aldehyde functional group.
C)A large biological polymer composed of amino acids.
D)And ester of phosphoric acid where one or more of the ionizable hydrogen atoms has been replaced by an R group.
E)A group of molecules that make up a lipid bilayer.
Q2) An amino acid is a compound that contains at least
A)one amino group and one amide group.
B)two amino groups and one carboxylic acid group.
C)one hydroxyl group and one methyl group.
D)one carboxylic acid group and one amino group.
E)one methyl group and one amide group.
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) Which of the following is used to image the brain?
A)(<sup>18</sup>O)
B)(<sup>131</sup>I)
C)(<sup>123</sup>I)
D)(<sup>24</sup>Na)
E)(<sup>99</sup>Tc)
Q2) What is the nuclear process called where small nuclei are combined into larger ones?
A)Photonuclear reactions
B)Nuclear fission
C)Thermal conductivity
D)Nuclear combination
E)Nuclear fusion
Q3) Which of the following is used to test the activity of the thyroid?
A)(<sup>18</sup>O)
B)(<sup>131</sup>I)
C)(<sup>123</sup>I)
D)(<sup>24</sup>Na)
E)(<sup>99</sup>Tc)
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18
Chapter 17: Electrochemistry
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Sample Questions
Q1) Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of A)Pb.
B)Ag.
C)Sn.
D)Mg.
E)Cu.
Q2) Consider the following balanced redox reaction. Mn<sup>2</sup><sup>+</sup>(aq) + S<sub>2</sub>O8<sup>2 </sup>(aq) + 2H<sub>2</sub>O(l) MnO<sub>2</sub>(s) + 4H<sup>+</sup>(aq) + 2SO<sub>4</sub><sup>2 </sup>(aq) Which of the following statements is ?
A)Mn<sup>2</sup><sup>+</sup>(aq) is the oxidizing agent and is reduced.
B)Mn<sup>2</sup><sup>+</sup>(aq) is the oxidizing agent and is oxidized.
C)Mn<sup>2</sup><sup>+</sup>(aq) is the reducing agent and is oxidized.
D)Mn<sup>2</sup><sup>+</sup>(aq) is the reducing agent and is reduced.
E)Manganese does not change its oxidation number in this reaction.
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Page 19