Basic Chemistry
Final Exam
Course Introduction
Basic Chemistry introduces students to the fundamental concepts and principles of chemistry, including atomic structure, chemical bonding, the periodic table, chemical reactions, stoichiometry, states of matter, and the properties of acids, bases, and solutions. This course aims to build a strong foundation in chemical concepts and problem-solving skills, preparing students for more advanced studies in chemistry and related scientific fields. Through lectures, laboratory experiments, and practical exercises, students gain a deeper understanding of the role chemistry plays in everyday life and natural phenomena.
Recommended Textbook
Introductory Chemistry 4th Edition by Steve Russo
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18 Chapters
1785 Verified Questions
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Page 2
Chapter 1: What Is Chemistry
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Sample Questions
Q1) The "disappearance" of mothballs is an example of ________.
A)melting
B)evaporation
C)condensation
D)sublimation
Answer: D
Q2) The only way one can change an element to another is via ________.
A)a chemical reaction
B)a physical reaction
C)a nuclear reaction
D)applying heat
Answer: C
Q3) Which of the following represents a chemical change?
A)sugar dissolving into hot coffee
B)ice melting to form liquid water
C)water boiling to form steam
D)steel turning to rust in salt air
Answer: D
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Chapter 2: The Numerical Side of Chemistry
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Sample Questions
Q1) 40 °C is equivalent to 40 °F.
A)True
B)False
Answer: False
Q2) An 80.0 g sample of metal A displaces 20.0 mL of water, while a 56.0 g sample of metal B displaces 14.0 mL of water. The conclusion one may draw from this information is that ________.
A)A and B are the same metal
B)A and B are not the same metal
C)A and B may be the same metal, but more studies are needed to decide if they are the same
D)The above results tell us nothing about the nature of A and B.
Answer: C
Q3) Which of the following correctly converts 0.000001546 mi in scientific notation?
A)1.546 × 10<sup>6</sup> mi
B)1.546 × 10<sup>5</sup> mi
C)1.546 × 10<sup>-</sup><sup>5</sup> mi
D)1.546 × 10<sup>-</sup><sup>6</sup> mi
Answer: D
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Page 4
Chapter 3: The Evolution of Atomic Theory
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Sample Questions
Q1) An atomic mass unit, also known as amu, is equal to ________ the mass of a <sup>12</sup>C atom.
A)1/2
B)1/12
C)1/6
D)1/1840
Answer: B
Q2) The conservation of mass law states that matter can neither be created nor destroyed during a chemical reaction.
A)True
B)False
Answer: True
Q3) An alpha particle consists of two protons and two neutrons.
A)True
B)False
Answer: True
Q4) The oxygen-17 isotope has more protons than neutrons in its nucleus.
A)True
B)False
Answer: False
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Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) A non-metal is an element that tends to gain valence electrons in chemical reactions becoming a cation in the process.
A)True
B)False
Q2) Which of the following does not have the neon electron configuration?
A)S<sup>4+</sup>
B)Mg<sup>2+</sup>
C)O<sup>2-</sup>
D)Al<sup>3</sup><sup>+</sup>
Q3) The scientist credited with developing the current mathematical model of the atom is ________.
A)Bohr
B)Schrodinger
C)Planck
D)Rutherford
Q4) Which of the following elements is the largest size halogen?
A)He
B)Br
C)F
D)Kr
Page 6
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Chapter 5: Chemical Bonding and Nomenclature
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Sample Questions
Q1) Which of the following anions does not have its number of oxygen atoms equal to 2 and a net charge of -1?
A)sulfite
B)nitrite
C)chlorite
D)peroxide
Q2) When electrons in a bond are shared unequally the bond is ________.
A)ionic
B)non-polar covalent
C)hydrogen bonding
D)polar covalent
Q3) Silicon dioxide is the expected formula of the compound that forms between silicon and oxygen.
A)True
B)False
Q4) The number of valence electrons in the carbonate anion is ________.
A)20
B)22
C)24
D)26
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) Which of the following will be affected by the presence of an electric field?
A)H<sub>2</sub>
B)O<sub>2</sub>
C)HCl
D)N<sub>2</sub>
Q2) In a molecule having three pairs of electrons around a central atom and a planar triangle shape, how many lone pairs of electrons does the central atom have?
A)1
B)0
C)2
D)3
Q3) What is the molecular shape of NO<sub>2</sub><sup>-</sup>
A)tetrahedral
B)pyramidal
C)linear
D)bent
Q4) When naming the shape of a molecule count the lone pairs.
A)True
B)False
Q5) CHC1<sub>3</sub>
8
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) How does vancomycin function to kill bacteria?
A)destroys the bacterial DNA
B)interferes with cell wall construction
C)inhibits protein synthesis
D)prevents bacteria metabolism
Q2) Which of these has the highest melting point?
A)diamond
B)iron
C)sodium
D)bromine
Q3) Which of the following chemical substances would you expect to have the highest melting point?
A)water, H<sub>2</sub>O
B)methyl alcohol, CH<sub>3</sub>OH
C)nitrogen dioxide, NO<sub>2</sub>
D)hydrogen sulfide, H<sub>2</sub>S
Q4) sodium fluoride, NaF, m.p.: 993 °C
Q5) copper (II)carbonate, CuCO<sub>3</sub> (or cupric carbonate
Q6) iodine, I<sub>2</sub>
Q7) magnesium chloride, MgC1<sub>2</sub>, m.p.: 714 °C
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) What is the sum of all coefficients after the following equation is balanced C<sub>8</sub>H<sub>18</sub> + O<sub>2</sub> CO<sub>2</sub> + H<sub>2</sub>O?
A)4
B)18
C)32
D)61
Q2) In a decomposition reaction one compound breaks down into two or more simpler compounds or elements.
A)True
B)False
Q3) Which sulfate is water insoluble?
A)ammonium sulfate
B)strontium sulfate
C)sodium sulfate
D)potassium sulfate
Q4) All hydroxides are water insoluble
A)True
B)False
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Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) Determine the molecular formula for a compound that has a molar mass of 157.01 g/mol and is
45.9% C, 50.9% Br, and 3.21% H by mass.
Q2) What is the theoretical mass of carbon dioxide produced from one mole of C<sub>6</sub>H<sub>14</sub>?
A)6 g
B)44 g
C)132 g
D)264 g
Q3) For the process 2H<sub>2</sub> + O<sub>2</sub> 2H<sub>2</sub>O, which reactant is the limiting reagent if 6 mol of H<sub>2</sub> and 4 mol of O<sub>2</sub> are used?
A)O<sub>2</sub>
B)H<sub>2</sub>
C)neither H<sub>2</sub> nor O<sub>2</sub>
D)both H<sub>2</sub> and O<sub>2</sub>
Q4) The % composition of carbon is equal to the % composition of oxygen in carbon monoxide, CO.
A)True
B)False
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) Identify the reducing agent in the following chemical process (a lead storage battery): Pb + PbO<sub>2</sub> + 2H<sup>+</sup> + 2HSO<sub>4</sub><sup>-</sup>
2PbSO<sub>4</sub> + 2H<sub>2</sub>O .
A)PbO<sub>2</sub>
B)Pb
C)H<sup>+</sup>
D)2HSO<sub>4</sub><sup>-</sup>
Q2) The oxidation state of non-metals is almost always a negative number.
A)True
B)False
Q3) Which of the following elements may have a +3 charge when it becomes an ion?
A)magnesium
B)aluminum
C)carbon
D)chlorine
Q4) Which of the following is the most easily reduced?
A)(K<sup>+</sup>)
B)(Na<sup>+</sup>)
C)(Au<sup>+</sup>)
D)(<sup>Hg2+</sup>)
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Chapter 11: What If There Were No Intermolecular Forces
the Ideal Gas
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Sample Questions
Q1) The molar volume of any gas is equal to 22.4 L at any temperature.
A)True
B)False
Q2) The density of hydrogen gas at STP is ________ the density of oxygen under identical conditions.
A)four times larger than B)eight times larger than C)sixteen times smaller than D)equal to, since both densities are taken under the same conditions
Q3) Which statement is true for an ideal gas?
A)The pressure of a gas increases when its volume decreases.
B)The pressure of a gas increases when its temperature increases.
C)The pressure of a gas increases when the number of gas moles increases.
D)All of the above statements are correct.
Q4) The molar volume of any gas whether diatomic or monoatomic is 22.4 L at STP.
A)True B)False
Q5) 1 torr is equal to 1 cm Hg.
A)True B)False
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Chapter 12: Solutions
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Sample Questions
Q1) What are two physical properties of water that make it an especially useful and common solvent?
Q2) How many grams of water are in 100 g of a 30 mass % sugar solution?
A)30
B)60
C)70
D)100
Q3) An impurity ________ the boiling point of a compound.
A)decreases
B)increases
C)has no effect on
D)One cannot say unless the physical properties of the compound are known.
Q4) Which of the following has the highest hydration energy?
A)sodium chloride
B)magnesium chloride
C)aluminum chloride
D)silicon tetrachloride
Q5) C<sub>8</sub>H<sub>18</sub><sub> </sub>will dissolve in CCl<sub>4</sub>.
A)True
B)False
14
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Chapter 13: When Reactants Turn Into Products
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Sample Questions
Q1) Consider the reaction X Y with the following data: Energy of reactants = 25 kJ/mole; Energy of products = 75 kJ/mole;
Energy of transition state = 100 kJ/mole.
The energy of activation for the reverse reaction is ________ kJ/mole.
A)25
B)50.
C)75
D)100
Q2) Consider the reaction A + B C. Doubling the concentration of A leads to doubling the rate, while doubling the concentration of B quadruples the rate. The rate equation is, therefore, ________.
A)Rate = -k[A][B]<sup>2</sup>
B)Rate = -k[A]
C)Rate = - k[A]<sup>2</sup>
D)Rate = -k[A]<sup>2</sup>[B]
Q3) The reaction energy profile can tell if a reaction is exothermic or endothermic.
A)True
B)False
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15
Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) If the value of the equilibrium constant for the reverse reaction is 2.5 × 10<sup>-</sup><sup>6</sup>, the value of the equilibrium constant for the forward reaction is ________.
A)-2.5 × 10<sup>-</sup><sup>6</sup>
B)4.0 × 10<sup>5</sup>
C)2.5 × 10<sup>6</sup>
D)4.0 × 10<sup>7</sup>
Q2) Predict the direction in which the reaction will shift for the following reactions if the temperature is decreased (heat is removed):
a)SO<sub>3</sub> + NO SO<sub>2</sub> + NO<sub>2</sub> (endothermic)
b)CH<sub>4</sub> + H<sub>2</sub>O CO + H<sub>2</sub> (endothermic)
c)N<sub>2</sub> + 3H<sub>2</sub> 2NH<sub>3</sub> (exothermic)
Q3) Consider the equation N<sub>2</sub> (g)+ 3H<sub>2</sub> (g) 2NH<sub>3</sub> (g). Removing ammonia as soon as it is formed will ________.
A)shift the reaction to the right
B)shift the reaction to the left
C)have no effect
D)cannot be determined, since the temperature is unknown
Q4) H<sub>2</sub> (g)+ F<sub>2</sub> (g) 2HF (g)
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Chapter 15: Electrolytes, Acids, and Bases
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Sample Questions
Q1) Water can serve both as a Bronsted-Lowry acid and Bronsted-Lowry base.
A)True
B)False
Q2) Which of the following does not qualify as a Bronsted-Lowry base?
A)CH<sub>4</sub>
B)NH<sub>3</sub>
C)PH<sub>3</sub>
D)H<sub>2</sub>O
Q3) Which of the following is a strong electrolyte when dissolved in distilled water?
A)sodium chloride
B)sucrose
C)acetone (nail polish remover)
D)ethyl alcohol
Q4) The pH of natural rainwater is close to ________.
Q5) What were the defining characteristics of bases as known to the alchemists?
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) The half-life of chlorine-34 is 1.52 seconds. How much time will pass before a given sample of chlorine-34 decays by 60%?
Q2) Which is the lightest among the following particles?
A)proton
B)neutron
C)alpha particle
D)beta particle
Q3) Nuclear radiation can cause biological damage by the weakening or breaking of bonds.
A)True
B)False
Q4) <sup>3</sup>H + <sup>2</sup>H ______ + <sup>1</sup>n
Q5) Uranium-238 can capture a neutron inside a nuclear reactor (a so-called breeder reactor), producing an isotope of plutonium and two beta particles. The plutonium can then itself be used as a nuclear fuel. Write a balanced equation for the breeder reactor's production of plutonium (include isotope number)from uranium-238.
Q6) The half life of <sup>14</sup>C is close to 6,000 years.
A)True
B)False
Page 18
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Chapter 17: The Chemistry of Carbon
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Sample Questions
Q1) Unlike carbon, nitrogen has the potential of bonding to other atoms of itself, but cannot form long chains.
A)True
B)False
Q2) Ethers were once (in times long past)extensively used as ________.
A)antibiotics (germ-killers)
B)paint thinners
C)fuel for automobiles
D)anesthetics
Q3) The formula C<sub>2</sub>H<sub>6</sub>O may be attributed to an alcohol or an ether.
A)True
B)False
Q4) Organic amines are acidic.
A)True
B)False
Q5) The formula C<sub>5</sub>H<sub>10</sub>O may be applicable to an aldehyde or a ketone.
A)True
B)False
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Chapter 18: Synthetic and Biological Polymers
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Sample Questions
Q1) Think for a moment about the terms "polymer" and "polysaccharide". Is it right to refer to polysaccharides as "nature's polymers"? Why or why not?
Q2) Nylon contains only one type of monomer.
A)True
B)False
Q3) Which of the following is not an amino acid?
A)threonine
B)tyrosine
C)thymine
D)lysine
Q4) What two functional groups are found at the ends of any protein structure?
A)alcohol and amine
B)amine and carboxlyic acid
C)alcohol and carboxlyic acid
D)amine and aldehyde
Q5) Which of the following is made out of PVC?
A)tiles
B)raincoats
C)plumbing pipes that carry sewage
D)all of the above
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