Chemistry for Non-Majors Practice Exam
Course Introduction
This course presents the fundamental concepts of chemistry in a manner tailored for students whose major field of study is not chemistry. Topics include the basic principles of atomic and molecular structure, chemical reactions, states of matter, energy changes, and the role of chemistry in everyday life. Through lectures, demonstrations, and laboratory experiments, students will gain an appreciation of the significance of chemistry in health, industry, the environment, and society, developing scientific literacy and critical thinking skills for informed decision-making.
Recommended Textbook
Introductory Chemistry 4th Edition by Nivaldo J. Tro
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19 Chapters
1962 Verified Questions
1962 Flashcards
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Page 2
Chapter 1: The Chemical World
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54 Verified Questions
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Sample Questions
Q1) If experimental results contradict a hypothesis,the hypothesis must be either revised or discarded.
A)True
B)False
Answer: True
Q2) The scientific method emphasizes reason as the way to understand the world.
A)True
B)False
Answer: False
Q3) The definition of a scientific law is:
A)the same as a hypothesis.
B)a way of learning that emphasizes observation and experimentation.
C)the underlying reason for a scientific theory.
D)a number of similar observations generalized into a brief statement summarizing past observations and predicting new ones.
E)none of the above
Answer: D
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Page 3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) What is the standard SI unit for length?
A)mile
B)centimeter
C)foot
D)meter
E)none of the above
Answer: D
Q2) Determine the answer for the equation below with correct number of significant figures:
3.215 × 13.2 ÷ 0.218 = ________
A)194.669
B)195
C)194.7
D)194.67
E)none of the above
Answer: B
Q3) All solids have the same density.
A)True
B)False
Answer: False
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Chapter 3: Matter and Energy
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Sample Questions
Q1) If a solid piece of shiny sodium metal is exposed to chlorine gas,a large amount of heat is released and the white solid sodium chloride (table salt)forms.Based on this information,which of the following statements is TRUE?
A)This process represents a physical change.
B)Mass is lost during this process.
C)Sodium chloride is an element.
D)This process was exothermic.
E)none of the above
Answer: D
Q2) An energy diagram that shows the reactants having greater energy than the products illustrates an
A)endothermic reaction.
B)exothermic reaction.
C)isothermic reaction.
D)impossible reaction.
E)none of the above
Answer: B
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) Metalloids are located where on the periodic table?
A)left side
B)right side
C)middle
D)zig-zag diagonal line
E)none of the above
Q2) If two atoms each contain different numbers of protons,the atoms must be from different elements.
A)True
B)False
Q3) How many electrons would be in a -2 charged anion of sulfur?
A)2
B)16
C)18
D)36
E)none of the above
Q4) J.J.Thomson discovered the existence of protons.
A)True
B)False
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) What is the formula for an ionic compound made of carbon and oxygen?
A)CO<sub>2</sub>
B)C<sub>2</sub>O
C)CO
D)CO<sub>3</sub>
E)Carbon and oxygen do not form an ionic compound.
Q2) The charge of a vanadium ion in the compound V<sub>2</sub>O<sub>5</sub> is:
A)5+
B)2+
C)10+
D)10-
E)none of the above
Q3) The ionic compound that forms between aluminum and oxygen is AlO.
A)True
B)False
Q4) Ionic compounds have a net charge of zero.
A)True
B)False
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Chapter 6: Chemical Composition
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Sample Questions
Q1) The chemical formula clearly indicates the relationship between the mass of each element in the formula.
A)True
B)False
Q2) The number 6.022 × 10<sup>23</sup> is six times larger than the number 6.022 × 10<sup>22</sup>.
A)True
B)False
Q3) A 15.5 gram sample of diphosphorous pentoxide contains how many grams of phosphorous?
A)3.38
B)1.69
C)6.76
D)13.5
E)none of the above
Q4) The lighter the atom,the less mass in one mole of that atom.
A)True
B)False
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) Mixing HNO<sub>3</sub> (aq)and NaHCO<sub>3</sub> (aq)will produce carbon dioxide gas as a product.
A)True
B)False
Q2) All of the following compounds are soluble in water EXCEPT A)NaCl.
B)CaCl<sub>2.</sub>
C)FeCl<sub>3.</sub>
D)NH<sub>4</sub>Cl.
E)PbCl<sub>2.</sub>
Q3) Considering the following precipitation reaction:
Pb(NO<sub>3</sub>)<sub>2</sub>(aq)+ 2KI(aq)
2KNO<sub>3</sub>(aq)
Which ion would NOT be present in the complete ionic equation?
A)Pb<sup>2</sup><sup>+</sup>
B)K<sup>+</sup>
C)NO<sub>3</sub><sup>-</sup>
D)I<sup>-</sup>
E)All the above ions are in the complete ionic equation.
PbI<sub>2</sub>(s)+
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Page 9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Given that 4 NH<sub>3</sub> + 5 O<sub>2</sub> 4 NO + 6 H<sub>2</sub>O,when
4.50 mol of H<sub>2</sub>O are formed,the amount of NO formed is
A)1.50 mol.
B)3.00 mol.
C)4.50 mol.
D)6.75 mol.
E)none of the above
Q2) The reaction of one mole of nitrogen gas with three moles of hydrogen gas releases 92 kJ of thermal energy to the surroundings.Which of the following is TRUE?
A)This reaction is exothermic.
B)This reaction has a negative enthalpy of reaction.
C)Complete reaction of two moles of nitrogen gas would release 184 kJ of thermal Energy in this reaction.
D)All of the above are true.
E)None of the above are true.
Q3) The conversion factor for moles of carbon dioxide to mass of carbon dioxide is: 1 mole CO<sub>2</sub> 44.01 g
A)True
B)False
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Page 10
Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) The energy of each Bohr orbit increases with increasing value of "n",but levels become more closely spaced as "n" increases.
A)True
B)False
Q2) What do the alkali metals all have in common?
A)They all undergo similar reactions.
B)They all have similar physical properties.
C)They all form +1 ions.
D)They all have the same number of valence electrons.
E)all of the above
Q3) When the elements are arranged in order of increasing number of protons,certain sets of properties recur periodically.
A)True
B)False
Q4) The energy of an electron orbit is quantized.
A)True
B)False
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11
Chapter 10: Chemical Bonding
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Sample Questions
Q1) When a nonmetal bonds with a nonmetal
A)a molecular compound forms.
B)a covalent bond is involved.
C)electrons are shared.
D)all of the above are true
E)none of the above
Q2) The electron geometry of a molecule is never the same as its molecular geometry.
A)True
B)False
Q3) What is the molecular geometry of NH<sub>4</sub><sup>+</sup>?
A)bent
B)linear
C)tetrahedral
D)trigonal pyramidal
E)not enough information
Q4) The VSEPR theory predicts that the angle between the central carbon atom and the two oxygen atoms in CO<sub>2</sub> measures 180°.
A)True
B)False
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Chapter 11: Gases
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Sample Questions
Q1) What is the equivalent pressure of 760 torr in units of mm Hg?
A)760
B)1
C)14.7
D)29.92
E)none of the above
Q2) A sample of helium gas initially at 37.0°C,785 torr and 2.00 L was heated to 58.0°C while the volume expanded to 3.24 L.What is the final pressure in atm?
A)517
B)0.681
C)1.79
D)3.21
E)none of the above
Q3) What is the equivalent pressure of 0.905 atm in units of mm Hg?
A)688
B)840
C)0.905
D)13.3
E)none of the above
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Page 13
Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Which intermolecular force is due to the formation of an instantaneous dipole?
A)dispersion forces
B)dipole-dipole forces
C)hydrogen bonding
D)X-forces
E)none of the above
Q2) Intermolecular forces are the attractive forces between atoms within a compound.
A)True
B)False
Q3) Which atomic solid has the highest melting point?
A)Cu
B)Si
C)Xe
D)Fe
E)not enough information
Q4) Water has unusual physical properties which enable life to exist on earth.
A)True
B)False
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Page 14
Chapter 13: Solutions
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Sample Questions
Q1) What molarity should the stock solution be if you want to dilute 25.0 mL to 2.00 L and have the final concentration be 0.103 M?
A)0.206 M
B)8.24 M
C)4.12 M
D)0.243 M
E)none of the above
Q2) Salt water is an example of a strong electrolyte solution.
A)True
B)False
Q3) How many moles of NaF are in 34.2 grams of a 45.5% by mass NaF solution?
A)0.814
B)75.2
C)15.6
D)0.371
E)none of the above
Q4) If 50 grams of salt dissolves into 250 grams of water,the resulting solution must have a mass of 300 grams.
A)True
B)False
15
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Chapter 14: Acids and Bases
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Sample Questions
Q1) What is the concentration of H in 0.50 M hydroiodic acid?
A)0.50 M
B)1.0 M
C)<0.50 M
D)1.50 M
E)none of the above
Q2) A weak acid is a dilute acid that is not very powerful.
A)True
B)False
Q3) In a solution that has a pH = 7.0,
A)[H<sub>3</sub>O<sup>+</sup>] > [OH<sup>-</sup>]
B)[H<sub>3</sub>O<sup>+</sup>] < [OH<sup>-</sup>]
C)[H<sub>3</sub>O<sup>+</sup>] = [OH<sup>-</sup>]
D)[H<sub>3</sub>O<sup>+</sup>] + [OH<sup>-</sup>] = K<sub>w</sub>
E)none of the above
Q4) Bases feel slippery.
A)True
B)False
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Page 16
Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) For the reaction Ag<sub>2</sub>S(s) 2 Ag<sup>+</sup> (aq)+ S<sup>2-</sup> (aq),K<sub>eq</sub> = 2.4 × 10<sup>-4</sup>,and the equilibrium concentration of sulfide ion is [S<sup>2-</sup>] = 0.0023 M..What is [Ag<sup>+</sup>] at equilibrium?
A)0.052 M
B)0.32 M
C)0.015 M
D)0.10 M
E)none of the above
Q2) For the reaction 2 N<sub>2</sub>O(g) O<sub>2</sub> (g)+ 2 N<sub>2</sub> (g),what happens to the equilibrium position if the pressure decreases?
A)shifts to the left
B)shifts to the right
C)does nothing
D)doubles
E)halves
Q3) Reaction rates generally increase as a reaction proceeds.
A)True
B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Which substance below would contain a nitrogen atom with the highest oxidation number of all those shown?
A)NH<sub>4</sub> <sup>1</sup><sup>+</sup>
B)N<sub>2</sub>
C)NO<sub>2</sub>
D)NO<sub>3</sub> <sup>1</sup><sup>-</sup>
E)NH<sub>3</sub>
Q2) Reduction can be defined as the gain of oxygen atoms by another element.
A)True
B)False
Q3) In the following reaction,
Zn (s)+ CuSO<sub>4</sub> (aq) ZnSO<sub>4 </sub>(aq)+ Cu (s)
A)Zn is the reducing agent and CuSO<sub>4</sub> is the oxidizing agent.
B)CuSO<sub>4</sub> is the reducing agent and Zn is the oxidizing agent.
C)ZnSO<sub>4</sub> is the reducing agent and Cu is the oxidizing agent.
D)Cu<sup>2+</sup> is the reducing agent and Zn<sup>2</sup><sup>+</sup> is the oxidizing agent.
E)none of the above
Q4) Distinguish between a galvanic (voltaic)cell and an electrolytic cell.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) The rate of spontaneous nuclear decay:
A)can be increased by increasing the temperature.
B)can be increased by increasing the concentration of the radioactive element.
C)is independent of concentration or temperature.
D)can be increased by addition of a nuclear catalyst.
E)all of the above
Q2) Radioactive particles can pass through matter.
A)True
B)False
Q3) How was radioactivity discovered?
A)Rutherford was investigating the structure of Au atoms and discovered alpha particles.
B)Marie Curie was investigating the existence of uranic rays that occurred in some minerals.
C)Becquerel was studying X-rays and phosphorescence to see if they were related.
D)Benjamin Franklin was studying the creation of electrical current from the ionization of gases due to radioactive particles.
E)none of the above
Q4) Briefly distinguish between nuclear fission and nuclear fusion.
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) What are the products from the combustion of 2-methyl-3-ethyloctane?
A)variety of small hydrocarbons
B)carbon monoxide,carbon trioxide and water
C)carbon dioxide and water
D)carbon monoxide and water
E)none of the above
Q2) Ethyl propanoate is a(n):
A)ether.
B)carboxylic acid.
C)ester.
D)ketone.
E)none of the above
Q3) Esters are best known for their awful odors such as that associated with the smell of rotten fish.
A)True
B)False
Q4) Carbon must always form four bonds.
A)True
B)False
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Chapter 19: Biochemistry
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Sample Questions
Q1) Which type of structure is maintained by interaction between R-groups on amino acids that are separated by short distances on the same chain?
A)Primary Structure
B)Secondary Structure
C)Tertiary Structure
D)Quaternary Structure
E)Pental Structure
Q2) The portion of the cell that contains the genetic information is called:
A)cytoplasm.
B)membrane.
C)nucleus.
D)mitochondria.
E)none of the above
Q3) The polar section of a phospholipid is said to be hydrophobic.
A)True
B)False
Q4) DNA and RNA are the two types of nucleic acids.
A)True
B)False
Q5) What is the difference between saturated and unsaturated fatty acids?
Page 21
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