Chemistry for Health Sciences
Midterm Exam
Course Introduction
Chemistry for Health Sciences is an introductory course designed to provide students with a fundamental understanding of chemical principles and their applications in the health sciences. The course covers the basics of general, organic, and biological chemistry, emphasizing topics relevant to human health, such as the structure and function of biomolecules, metabolic pathways, chemical reactions in the body, and the role of chemistry in pharmaceuticals and medical diagnostics. Students will develop problem-solving skills and learn how chemical concepts underpin physiological processes and influence evidence-based healthcare practices. This foundational knowledge prepares students for advanced studies in health-related fields and supports their success in clinical and laboratory environments.
Recommended Textbook
Introductory Chemistry 4th Edition by Steve Russo
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Chapter 1: What Is Chemistry
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Q1) Which of the following is a pure substance?
A)blood
B)block of aluminum
C)air
D)orange juice
Answer: B
Q2) What is another name for a homogeneous mixture?
A)pure substance
B)compound
C)solution
D)element
Answer: C
Q3) Evaporated ethanol can be isolated by cooling, without changing its disinfectant properties.
A)True
B)False
Answer: True
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Chapter 2: The Numerical Side of Chemistry
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Sample Questions
Q1) Which of the following correctly expresses (in normal decimal notation)the number 1.06 × 10<sup>-</sup><sup>4</sup>?
A)10,600
B)106
C)0.0106
D)0.000106
Answer: D
Q2) The United States has the unit of currency dollars (unit symbol: $). Which of the following is a proper expression of the value seventy seven hundred dollars +/- 1 dollar?
A)$ 7.7 × 10<sup>-4</sup>
B)$ 7.7 × 10<sup>-3</sup>
C)$ 7700
D)$ 7.700 × 10<sup>-3</sup>
Answer: D
Q3) There are 4 pints in a gallon.
A)True
B)False
Answer: False
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Chapter 3: The Evolution of Atomic Theory
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Sample Questions
Q1) Earth's gravitational force is incapable of keeping the atmospheric helium from escaping into space.
A)True
B)False
Answer: True
Q2) 24.3 g of magnesium yield 40.3 g MgO upon combustion with oxygen. How much magnesium needs to be burned to yield 12.1 g MgO?
A)4.3 g
B)6.1 g
C)7.3 g
D)8.4 g
Answer: C
Q3) The amu for an atom is the weighted average of all the naturally occurring isotopes.
A)True
B)False
Answer: True
Q4) strontium-90
Answer: atomic number 38, mass number 90, symbol Sr
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Page 5
Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) Microwave is radiation of a lower energy than that of visible light.
A)True
B)False
Q2) The relative ratio of atoms in the binary compound Al<sub>x</sub>O<sub>y</sub> is
A)x=2, y=3
B)x=3, y=2
C)x=5, y=2
D)x=2, y=5
Q3) Atoms in which of the following groups will likely lose three electrons?
A)IIIA
B)VA
C)IIA
D)IVA
Q4) How many electrons can be "stored" in a completely filled 4f sublevel?
A)14
B)10
C)7
D)28
Q5) Which element is the more reactive, sodium (Na)or potassium (K)?
Page 6
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Chapter 5: Chemical Bonding and Nomenclature
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Sample Questions
Q1) A single, neutral chlorine atom has seven valence electrons.
A)True
B)False
Q2) What is the chemical name of the compound whose formula is K<sub>2</sub>O?
A)dipotassium oxygen
B)potassium oxide
C)potasside oxygen
D)potassium oxygen
Q3) In the set H, S, Cl, Na, sodium is the least electronegative.
A)True
B)False
Q4) Hydrogen may have a +1 or -1 charge.
A)True
B)False
Q5) The number of valence electrons in aluminum is ________.
A)2
B)3
C)5
D)7
Q6) O<sub>3</sub> (ozone)
Page 7
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) Sulfur dioxide is linear.
A)True
B)False
Q2) When drawing the three-dimensional structure diagram of a molecule the bold line
A)projects out from the page
B)goes back behind the page
C)the bond is in the plane of the page
D)One cannot say unless the formula of the molecule is known.
Q3) CS<sub>2</sub>
Q4) SO<sub>2</sub>
Q5) Which of the following is tetrahedral?
A)sulfur trioxide
B)sulfur dioxide
C)sulfur dichloride
D)ammonium ion
Q6) In the VSEPR model the multiple bond is treated as a single electron group, just the way a single bond is treated.
A)True
B)False
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) Between individual molecules of NO<sub>2</sub> in the solid state, which of the following types of intermolecular forces would you expect to be dominant?
A)hydrogen bonding
B)London forces
C)van der Waals forces
D)dipole forces
Q2) To form hydrogen bonds, molecules must contain ________.
A)an N-H bond
B)an O-H bond
C)an H-F bond
D)at least one of the above mentioned bonds
Q3) Nonpolar molecules may exhibit ________.
A)London forces
B)hydrogen bonding
C)dipolar forces
D)all of the above
Q4) The terms "dispersion forces" and "London forces" are interchangeable.
A)True
B)False
Q5) magnesium chloride, MgC1<sub>2</sub>, m.p.: 714 °C
Page 9
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) Which of the following equations has 1:2:1:1 as the relative ratio of coefficients when balanced?
A)H<sub>2</sub>SO<sub>4</sub> + KOH K<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O
B)Zn + HCl H<sub>2</sub> + ZnCl<sub>2</sub>
C)CH<sub>4</sub> + O<sub>2</sub> CO<sub>2</sub> + H<sub>2</sub>O
D)NaOH + HCl NaCl + H<sub>2</sub>O
Q2) When aqueous solutions of sodium nitrate and potassium chloride are mixed, the spectator ions are ________.
A)potassium and nitrate
B)sodium and chloride
C)both A and B
D)no spectator ions are present
Q3) The equation Zn + CuCl<sub>2</sub> Cu + ZnCl<sub>2</sub> is an example of a ________ reaction.
A)combination
B)single replacement
C)double replacement
D)decomposition
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Page 10
Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) Which of the following has its empirical formula different than its molecular formula?
A)CH<sub>2</sub>S
B)C<sub>2</sub>H<sub>7</sub>N<sub>3</sub>
C)C<sub>3</sub>H<sub>6</sub>N<sub>3</sub>
D)C<sub>5</sub>H<sub>7</sub>O<sub>3</sub>
Q2) The % yield of an experiment in which 1 mole NaHCO<sub>3</sub> was used and 22 g carbon dioxide was isolated is ________.
A)100%
B)50%
C)37.5%
D)25%
Q3) How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine?
A)1.5
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) In a chemical bond the less electronegative element gets complete ownership of both the shared electrons.
A)True
B)False
Q2) The cathode is the electrode where oxidation occurs.
A)True
B)False
Q3) The lowest oxidation state sulfur can have is in the sulfite form.
A)True
B)False
Q4) The only element that is more electronegative than oxygen is ________.
A)chlorine
B)fluorine
C)nitrogen
D)sulfur
Q5) Assign the oxidation state of:
a)barium, in BaCl<sub>2</sub>
b)sodium, in Na<sub>2</sub>O
c)selenium, in H<sub>2</sub>SeO<sub>3</sub>
d)aluminum, in Al<sub>2</sub>O<sub>3</sub>
Page 12
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Chapter 11: What If There Were No Intermolecular Forces
the Ideal Gas
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Sample Questions
Q1) The density of sulfur vapor at 1273 K and 740 torr is 0.5977 g/L. Its molar mass is
A)32
B)64
C)96
D)128
Q2) As the temperature of a gas increases, its pressure increases as long as the volume is kept constant.
A)True
B)False
Q3) If the pressure of a given gas sample doubles, what happens to the volume of gas?
(Assuming that the amount of gas and the temperature of the gas stay the same).
A)increase by a factor of 2
B)decrease by a factor of 2
C)stay exactly the same
Q4) Ideal gas molecules undergo non-elastic collisions.
A)True
B)False
Page 13
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Chapter 12: Solutions
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Sample Questions
Q1) Vinegar is a liquid solution where acetic acid serves as the solvent.
A)True
B)False
Q2) The solvent in a saline solution is water.
A)True
B)False
Q3) 25 mL of 0.2 M NaOH will neutralize 10 mL 0.5 M HCl solution.
A)True
B)False
Q4) How are solubility and temperature generally related in a system consisting of a solid solute and a liquid solvent?
A)Solubility generally increases with increasing temperature.
B)Solubility generally increases with decreasing temperature.
C)Changing the temperature has no effect on solubility.
D)Solubility generally decreases with increasing temperature.
Q5) Henry's law gives the relationship between ________.
A)colligative properties and the freezing point
B)solubility of a gas and concentration
C)solubility of a gas and pressure
D)hydrophobic and hydrophilic solutions
Page 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 = 50 kJ/mole; Energy of reaction = -30 kJ/mole; Energy of transition state = 90 kJ/mole.
The energy of products for the reaction is ________ kJ/mole.
A)-30
B)20
C)30
D)80
Q2) When the products are higher in energy than the reactants, the reaction is endothermic.
A)True
B)False
Q3) The slow step in the multistep mechanism of a reaction ________.
A)controls the rate at which the products are formed
B)is the only step that involves the breaking of bonds
C)is equally significant in measuring the rate
D)is insignificant in the formation of products
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Predict the shift in the direction of the reaction for the following chemical reaction:
CH<sub>4</sub> + O<sub>2</sub> CO<sub>2</sub> + H<sub>2</sub>O
a)if methane (CH<sub>4</sub>)is added.
b)if carbon dioxide (CO<sub>2</sub>)is added.
c)if water (H<sub>2</sub>O)is removed.
Q2) SO<sub>2</sub> (g)+ NO<sub>2</sub> (g) SO<sub>3</sub> (g)+ NO (g)
Q3) Refer to the equilibrium shown above. Adding a couple of drops of an aqueous KCl solution will ________.
A)turn the solution red.
B)turn the solution less red.
C)turn the solution clear.
D)have no effect on the color.
Q4) 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)
Q5) 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) Which of the following is a weak electrolyte when dissolved in distilled water?
A)phosphoric acid
B)nitric acid
C)potassium chloride
D)glucose
Q2) The conjugate base of H<sub>2</sub>PO<sub>4</sub><sup>-</sup> is ________.
A)H<sub>3</sub>PO<sub>4</sub>
B)HPO<sub>4</sub><sup>-</sup><sup>2</sup>
C)PO<sub>4</sub><sup>-</sup><sup>3</sup>
D)H<sub>4</sub>PO<sub>4</sub><sup>+</sup>
Q3) Which of the following produces more than one H<sub>3</sub>O<sup>+</sup> ion per molecule of acid when dissolved in water?
A)hydrobromic
B)carbonic
C)hypochlorous
D)acetic
Q4) Sucrose (table sugar)is a strong electrolyte.
A)True
B)False
Q5) What is the OH<sup>-</sup> concentration of a solution of pH 8.36?
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) The main problem nuclear reactors have when uranium-235 serves as the fuel is
A)the production of more neutrons that the reaction consumes
B)the production of gamma rays
C)the consumption of more alpha particles than the available alpha particles
D)the immense amount of energy produced
Q2) How long will it take for a 5.0 g tritium sample to decay down to 0.313 g? The half-life of tritium is 12 years.
A)12 yrs
B)24 yrs
C)48 yrs
D)96 yrs
Q3) <sup>238</sup>U + ______ <sup>239</sup>Np + <sub>-</sub><sub>1</sub>e
Q4) What is the missing particle in the reaction below? <sup>1</sup>p + <sup>0</sup>e ?
A)(<sup>2</sup>p)
B)(<sup>1</sup>H)
C)(<sup>1</sup>n)
D)(<sup>4</sup>He)
Q5) <sup>22</sup>Na ______ + <sub>+</sub><sub>1</sub>e
Page 18
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Chapter 17: The Chemistry of Carbon
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Q1) The H-C-H angle in alkanes is about 109°.
A)True
B)False
Q2) Which of the following is a hydrocarbon?
A)C<sub>4</sub>H<sub>8</sub>O
B)C<sub>4</sub>H<sub>10</sub>O
C)C<sub>4</sub>H<sub>8</sub>O<sub>2</sub>
D)C<sub>4</sub>H<sub>6</sub>
Q3) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,4,4-trimethyl-2-pentene.
Q4) Construct a line drawing for the hydrocarbon whose IUPAC name is 2-methyl-2-butene.
Q5) The general formula for an ether is R-O-R.
A)True
B)False
Q6) Ethers were once (in times long past)extensively used as ________.
A)antibiotics (germ-killers)
B)paint thinners
C)fuel for automobiles
D)anesthetics
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Chapter 18: Synthetic and Biological Polymers
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Q1) The number of amino acids that define the difference in shape between a normal hemoglobin molecule and that of a sickle-cell anemia patient is ________.
A)1
B)5
C)10
D)all
Q2) 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
Q3) The number of amino acids that are used to build all proteins is ________.
A)4
B)10
C)20
D)30
Q4) Teflon is synthesized with a monomer containing carbons and chlorines.
A)True
B)False
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