Chemistry for Health Sciences
Exam Questions
Course Introduction
Chemistry for Health Sciences provides an essential foundation in the principles of general, organic, and biological chemistry, tailored specifically for students pursuing careers in health-related fields. The course emphasizes the chemical structures and reactions most relevant to biological systems and human health, including the chemistry of biomolecules, acids and bases, solutions, and metabolic pathways. Through lectures, laboratory exercises, and real-world applications, students gain a thorough understanding of how chemical processes impact physiology, disease, diagnostics, and therapies, equipping them with the scientific literacy necessary for advanced studies and professional practice in healthcare and biomedical sciences.
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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Sample Questions
Q1) 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
Q2) Which of the following statements about soda pop is FALSE?
A)Soda pop is a chemical mixture of mostly sugar,water and carbon dioxide.
B)The molecules important to fizzing are carbon dioxide and water.
C)The carbon dioxide is forced to mix with the water by the presence of sugars.
D)When a can is opened,the pressure release allows carbon dioxide to form bubbles.
E)All of the above statements are true.
Answer: C
Q3) John Dalton proposed the atomic theory.
A)True
B)False
Answer: True
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Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) A lead ball has a mass of 55.0 grams and a density of 11.4 g/cm<sup>3</sup>.What is the volume of the ball?
A)0.207 mL
B)0.207 L
C)4.82 mL
D)4.82 L
E)none of the above
Answer: C
Q2) There are exactly 2.54 centimeters in 1 inch.When using this conversion factor,how many significant figures are you limited to?
A)1
B)3
C)ambiguous
D)depends on if you are using it in multiplication/division or addition/subtraction E)infinite number of significant figures
Answer: E
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Chapter 3: Matter and Energy
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Sample Questions
Q1) Temperature is simply a measure of the motion of atoms and molecules.
A)True
B)False
Answer: True
Q2) The melting of ice is a physical change.
A)True
B)False
Answer: True
Q3) A solid form of matter in which there is long range repeating order is called
A)amorphous
B)rigid
C)crystalline
D)fixed
E)none of the above
Answer: C
Q4) The energy of position is called kinetic energy.
A)True
B)False
Answer: False
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) You can continually divide matter into smaller and smaller pieces without ever coming to an end.
A)True
B)False
Q2) The relative amount of each different isotope in a naturally occurring sample of an element is always the same.
A)True
B)False
Q3) Metals are located on the left side of the periodic table.
A)True
B)False
Q4) How many neutrons are found in Ne-21?
A)11
B)21
C)10
D)0
E)none of the above
Q5) A cation forms when an atom gains an electron.
A)True
B)False
Page 6
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) What is the oxygen-to-hydrogen mass ratio for H<sub>2</sub>O<sub>2</sub>?
A)0.125
B)4
C)8
D)16
E)none of the above
Q2) What is the name of the ionic compound made of beryllium and chlorine?
A)beryllium(II)chloride
B)beryllium dichloride
C)beryllium chloride
D)monoberyllium dichloride
E)none of the above
Q3) Life could not exist with just 91 elements if they did not combine to form compounds. A)True
B)False
Q4) The formula of a compound comprised of two nitrogen atoms and one oxygen atom should be written properly as ON<sub>2</sub>.
A)True
B)False
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Chapter 6: Chemical Composition
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Sample Questions
Q1) How many atoms are in 15.6 grams of silicon?
A)2.64 × 10<sup>26</sup>
B)3.34 × 10<sup>23</sup>
C)0.555
D)438
E)none of the above
Q2) Mass is used as a method of counting atoms.
A)True
B)False
Q3) How many moles of fluorine are in 3.2 moles of xenon hexafluoride?
A)22.4
B)12.8
C)19.2
D)16
E)none of the above
Q4) One mole of chlorine gas has a mass of 35.45 grams.
A)True
B)False
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) What type of reaction is the generic equation AB \(\to\) A + B?
A)synthesis/combination
B)decomposition
C)single displacement
D)double-displacement
E)none of the above
Q2) Decomposition reactions usually require energy to initiate the reaction.
A)True
B)False
Q3) A reaction which forms a gaseous product is an example of a(n)________.
A)oxidation-reduction reaction
B)combustion reaction
C)precipitation reaction
D)gas evolution reaction
E)none of the above
Q4) A net ionic equation shows all ionic species that are present in solution.
A)True
B)False
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) What is the excess reactant for the following reaction given we have 2.6 moles of HCl and 1.4 moles of Ca(OH)<sub>2</sub>?
Reaction: 2HCl + Ca(OH)<sub>2 </sub> 2H<sub>2</sub>O<sub> </sub>+ CaCl<sub>2</sub>
A)Ca(OH)<sub>2</sub> B)HCl
C)H<sub>2</sub>O
D)CaCl<sub>2</sub>
E)not enough information
Q2) What is the limiting reactant for the reaction below given that you start with 10.0 grams of Al and 19.0 grams of O<sub>2</sub>?
Reaction: 4Al + 3O<sub>2</sub> 2Al<sub>2</sub>O<sub>3</sub>
A)Al
B)O<sub>2</sub>
C)Al<sub>2</sub>O<sub>3</sub>
D)both Al and O<sub>2</sub>
E)not enough information
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) What happens to an atom when it absorbs energy?
A)The atom stores the energy for later use.
B)The extra energy increases the speed of the electrons in their orbitals.
C)The atom re-emits the energy as heat.
D)The atom re-emits the energy as light.
E)none of the above
Q2) How many electrons are unpaired in the orbitals of carbon?
A)12
B)6
C)4
D)2
E)none of the above
Q3) A principal shell with a value of n=3 would contain s,p,d,and f orbitals.
A)True
B)False
Q4) The ground state is when an electron in an atom is excited into the lowest possible vacant orbital.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) What is the angle between electron groups in the trigonal planar electron geometry?
A)90°
B)109.5°
C)120°
D)180°
E)not enough information
Q2) Which of the following statements is TRUE for the covalent molecule HCl?
A)Chlorine is more electronegative and the shared electron pair is likely to be found on the hydrogen atom.
B)Chlorine is more electronegative and the shared electron pair is likely to be found on the chlorine atom.
C)Hydrogen is more electronegative and the shared electron pair is likely to be found on the hydrogen atom.
D)Hydrogen is more electronegative and the shared electron pair is likely to be found on the chlorine atom.
E)none of the above
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12
Chapter 11: Gases
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Sample Questions
Q1) What is the temperature (°C)of 2.48 moles of gas stored in a 30.0 L container at 1559 mm Hg?
(R= 0.0821 L atm/ mol K)
A)302
B)189
C)29
D)-84
E)none of the above
Q2) A gas cylinder contains only the gases radon,nitrogen,and helium.The radon has a pressure of 222 torr while the nitrogen has a pressure of 446 torr.If the total pressure inside the cylinder is 771 torr,what is the pressure that is due to the helium?
A)771 torr
B)668 torr
C)549 torr
D)103 torr
E)none of the above
Q3) The expected order of density for matter is gases < liquids < solids.
A)True
B)False
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Page 13
Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Heat is released when a liquid freezes into a solid.
A)True
B)False
Q2) Substance A is a molecular compound that dissolves in gasoline but not in water.The molecules of A are very likely:
A)metallic.
B)nonmetallic.
C)polar.
D)nonpolar.
E)none of the above
Q3) Which intermolecular force is common to all polar molecules but NOT nonpolar molecules?
A)dispersion forces
B)dipole-dipole forces
C)hydrogen bonding
D)X-forces
E)none of the above
Q4) Hydrogen bonding occurs whenever hydrogen is present.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) How many grams of LiF would be present in 575 mL of 0.750 M LiF solution?
A)11.2
B)0.0338
C)1.12 × 10<sup>4</sup>
D)19.9
E)33.8
Q2) Steel is an example of a solid solution.
A)True
B)False
Q3) A supersaturated solution is unstable and crystallization usually occurs.
A)True
B)False
Q4) The oxygen in the air we breath is classified as:
A)the solute in a homogeneous gas mixture.
B)the solvent in a homogeneous gas mixture.
C)the solute in a heterogeneous gas-liquid mixture.
D)the solvent in a simple mixture.
E)none of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) What is the concentration of the hydroxide ions in an acidic solution?
A)0.0 M
B)1.0× 10<sup>-7</sup> M
C)1.0 × 10<sup>-</sup><sup>14</sup> M
D)> 1.0× 10<sup>-7</sup> M
E)< 1.0× 10<sup>-7</sup> M
Q2) An Arrhenius base is a proton acceptor.
A)True
B)False
Q3) Pure water cannot conduct electricity so why do we have to be careful with electrical appliances near water?
A)OSHA regulations
B)Water can be broken down by electricity.
C)Water always has some ions dissolved in it.
D)Water dissociates fully into its ions.
E)none of the above
Q4) A pH of 7 is equivalent to a pOH of 7.
A)True
B)False
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Which of the following changes will increase reaction rate?
1.An increase in the concentration of reactants
2.An increase in temperature
3.Higher-energy collisions between reacting molecules
A)1 and 2 only
B)1 and 3 only
C)2 and 3 only
D)All of 1,2,and 3
E)Neither 1,2,or 3
Q2) Iron(II)carbonate (K<sub>sp</sub> = 3.07 ×10<sup>-</sup><sup>11</sup>)is more soluble than calcium fluoride (K<sub>sp</sub> = 1.46 ×10<sup>-</sup><sup>10</sup>).
A)True
B)False
Q3) Le Chatelier's principle states that when a chemical system at equilibrium is disturbed,the system shifts in a direction that minimizes the disturbance.
A)True
B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Reduction is the gain of electrons.
A)True
B)False
Q2) Balance the redox reaction: Br<sup>-</sup>(aq)+ Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup>(aq) \(\to\) Cr<sup>3+</sup> + Br<sub>2</sub> (l)
A)4 Br<sup>-</sup> + Cr<sub>2</sub>O<sub>7</sub><sup>2</sup><sup>-</sup><sup> </sup>+ 7 H<sup>+</sup> 2 Cr<sup>3+</sup> + 2 Br<sub>2</sub> + 7 H<sub>2</sub>O
B)6 Br<sup>-</sup> + Cr<sub>2</sub>O<sub>7</sub><sup>2</sup><sup>-</sup><sup> </sup>+ 147 H<sup>+</sup> 2 Cr<sup>3+</sup> + 3 Br<sub>2</sub> + 7 H<sub>2</sub>O
C)2 Br<sup>-</sup>+ Cr<sub>2</sub>O<sub>7</sub><sup>2</sup><sup>-</sup><sup> </sup>+ 147 H<sup>+</sup> 2 Cr<sup>3+</sup> + Br<sub>2</sub> + 7 H<sub>2</sub>O
D)2 Br<sup>-</sup> + 2 Cr<sub>2</sub>O<sub>7</sub><sup>2</sup><sup>-</sup><sup> </sup>+ 147 H<sup>+</sup> 4 Cr<sup>3+</sup>+ Br<sub>2</sub> + 14 H<sub>2</sub>O E)none of the above
Q3) 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) Nuclear power plants produce energy by fission reactions.
A)True
B)False
Q2) In a Geiger-Muller counter,radioactive particles pass through NaI which emits UV-Vis light.
A)True
B)False
Q3) Iodine-131 has a half-life of 8 days.How much of a 1000 milligram sample of iodine-131 would be left after 32 days?
A)500 milligram
B)250 milligram
C)125 milligram
D)62.5 milligram
E)31.25 milligram
Q4) One method of nuclear medicine uses radioactive isotopes to scan specific regions of the body.
A)True
B)False
Q5) Briefly distinguish between nuclear fission and nuclear fusion.
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) All organic molecules contain carbon but not all carbon compounds are organic compounds.
A)True
B)False
Q2) Hydrocarbons contain carbon,hydrogen and oxygen.
A)True
B)False
Q3) The prefix "but-" means that the base chain contains how many carbon atoms?
A)2
B)4
C)6
D)8
E)all of the above
Q4) Which is the name of C<sub>6</sub>H<sub>14</sub>?
A)n-butane
B)n-hexane
C)n-heptane
D)n-pentane
E)all of the above
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Chapter 19: Biochemistry
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Sample Questions
Q1) What is the difference between saturated and unsaturated fatty acids?
Q2) The complementary strand of DNA to the pattern GAATC is TCCGA.
A)True
B)False
Q3) Protein structures are expressed in terms of amino acid sequence,the short-term repeating pattern,the long-term bend and folds and finally how proteins structures interact with themselves.
A)True
B)False
Q4) An alpha helix is an example of which type of structure?
A)Primary Structure
B)Secondary Structure
C)Tertiary Structure
D)Quaternary Structure
E)Pental Structure
Q5) A pentose sugar contains more carbon atoms than does a hexose sugar.
A)True
B)False
Q6) Summarize the main features of the four categories of protein structure.
Page 21
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