Chemistry for Health Sciences
Final Exam
Course Introduction
Chemistry for Health Sciences is designed to provide students with a foundational understanding of chemical principles as they relate to health and biomedical fields. The course explores essential topics such as atomic structure, chemical bonding, solutions, acids and bases, and organic chemistry, with a strong emphasis on applications to human physiology, medical diagnostics, pharmaceuticals, and the biochemical processes that sustain life. Through integrated lectures and laboratory experiences, students gain practical skills in chemical analysis and problem-solving, preparing them for further study or careers in nursing, allied health, and other healthcare professions.
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) Chemistry is the science that seeks to understand what matter does by studying living organisms.
A)True
B)False
Answer: False
Q2) Molecules are responsible for scattering light which causes the colors of the sunset.
A)True
B)False
Answer: True
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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Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) You do not need to write units in calculations as long as you can remember them.
A)True
B)False
Answer: False
Q2) Scientific numbers are reported so that every digit is certain except the last,which is estimated.
A)True
B)False
Answer: True
Q3) How many cm<sup>3</sup> are there in 2.5 m<sup>3</sup>?
A)2.5 × 10<sup>6</sup>
B)2.5 × 10<sup>-</sup><sup>2</sup>
C)2.5 × 10<sup>2</sup>
D)2.5 × 10<sup>-</sup><sup>6</sup>
E)none of the above
Answer: A
Q4) The mass of an object depends on gravity.
A)True
B)False
Answer: False
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Chapter 3: Matter and Energy
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Sample Questions
Q1) How many calories are there in a 255 Calorie snack bar?
A)2.55 × 10<sup>5</sup>
B)1.07 × 10<sup>3</sup>
C)60.9
D)1 × 10<sup>3</sup>
E)none of the above
Answer: A
Q2) Chemical properties of a substance are those that can be observed without changing the composition of a substance.
A)True
B)False
Answer: False
Q3) A chemical change that will lower the potential energy of the chemical results in an endothermic reaction.
A)True
B)False
Answer: False
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Page 5
Chapter 4: Atoms and Elements
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Sample Questions
Q1) Nonmetals 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) All carbon atoms have exactly 6 protons.
A)True
B)False
Q3) Mendeleev's early periodic table predicted the existence of elements that had yet to be discovered.
A)True
B)False
Q4) The smell of the ocean is caused by atoms.
A)True
B)False
Q5) In the modern periodic table,elements are listed in order of increasing atomic number rather than increasing relative mass.
A)True
B)False
Page 6
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) The basic unit of an ionic compound is called the formula unit.
A)True
B)False
Q2) The proper name for the acid HF is hydrofluoric acid.
A)True
B)False
Q3) What is correct name of the compound whose formula is BF<sub>3</sub>?
A)boron trifluoride
B)boron fluoride
C)monoboron trifluorine
D)boron(III)fluoride
E)none of the above
Q4) What is the formula for an ionic compound made of barium and nitrogen?
A)Ba<sub>3</sub>N<sub>2</sub>
B)Ba<sub>2</sub>N<sub>3</sub>
C)BaN
D)Ba<sub>2</sub>N<sub>4</sub>
E)none of the above
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Chapter 6: Chemical Composition
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Sample Questions
Q1) What is the mass of 1.56 × 10<sup>21</sup> atoms of magnesium in grams?
A)4.72 × 10<sup>-</sup><sup>5</sup>
B)0.0630
C)0.142
D)1.07 × 10<sup>-</sup><sup>4</sup>
E)none of the above
Q2) The mole has a value of 6.023 × 10<sup>22</sup>.
A)True
B)False
Q3) A molecule that has an empirical formula of HO and a molar mass of 34.02 gram must have a molecular formula of H<sub>2</sub>O<sub>2</sub>.
A)True
B)False
Q4) C<sub>2</sub>H<sub>6</sub>O<sub>3</sub> could be an empirical formula.
A)True
B)False
Q5) The empirical formula for C<sub>6</sub>H<sub>6</sub> is C<sub>3</sub>H<sub>3</sub>.
A)True
B)False
Page 8
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) The reaction of baking soda and vinegar to produce carbon dioxide gas is an example of a precipitation reaction.
A)True
B)False
Q2) We remove the spectator ions from the complete ionic equation to form the net ionic equation.
A)True
B)False
Q3) If you had an aqueous mixture that contained Ag<sup>+</sup>,K<sup>+</sup>,and Pb<sup>+</sup><sup>2</sup> cations,how many different solids could precipitate if a chloride solution was added?
A)1
B)2
C)3
D)4
E)no solids will precipitate
Q4) An oxidation-reduction reaction must involve reaction with oxygen.
A)True B)False
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) How many moles of aluminum are needed to make 9 moles of molecular hydrogen? Given the reaction: 2 Al + 6 HCl 2 AlCl<sub>3</sub> + 3H<sub>2</sub>
A)2 moles
B)3 moles
C)4 moles
D)6 moles
E)none of the above
Q2) The conversion factor between mass and moles for a compound is the molar mass.
A)True
B)False
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
Q4) The primary cause of increasing greenhouse gases is:
A)the burning of vast amounts of rain forests.
B)the production of CO<sub>2</sub> by respiration.
C)the increased use of natural gas,petroleum and coal.
D)the release of CO<sub>2</sub> by decreasing solubility in the ocean.
E)none of the above
Page 10
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) Which of the following atoms is the smallest?
A)Li
B)Be
C)B
D)O
E)Ne
Q2) Which form of electromagnetic radiation has photons with the highest energy?
A)Radio Waves
B)Microwaves
C)X-rays
D)Gamma Rays
E)Infrared Radiation
Q3) The correct electron configuration for fluorine is: 1s<sup>2</sup>2s<sup>2</sup>2p<sup>5.</sup>
A)True
B)False
Q4) The subshells of the orbital are represented by the possible letters: s,p,d,or f.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) Which term matches the definition: A separation of charge within a bond.
A)coulombic attraction
B)dipole moment
C)polar covalent
D)nonpolar covalent
E)electronegativity
Q2) The correct Lewis structure for BF<sub>3</sub> would have exactly:
A)1 double bond.
B)2 double bonds.
C)1 triple bond.
D)no double bonds.
E)none of the above
Q3) Which of the following compounds have resonance structures?
A)CH<sub>4</sub>
B)H<sub>2</sub>O
C)NH<sub>3</sub>
D)O<sub>3</sub>
E)None of the compounds have resonance structures.
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Chapter 11: Gases
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Sample Questions
Q1) How many liters of O<sub>2</sub> (g)are needed to react completely with 56.0 L of CH<sub>4</sub> (g)at STP to produce CO<sub>2</sub> (g)and H<sub>2</sub>O (g)?
Given: CH<sub>4</sub> (g)+ 2O<sub>2</sub> (g) CO<sub>2</sub> (g)+ H<sub>2</sub>O (g)
A)28.0 L
B)56.0 L
C)84.0 L
D)112.L
E)none of the above
Q2) What is the third most abundant component of dry air?
A)carbon dioxide
B)oxygen
C)nitrogen
D)argon
E)smog
Q3) Boyle's law states that as the volume of a gas increases so does the pressure.
A)True
B)False
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Gases typically have high densities in comparison to solids.
A)True
B)False
Q2) The change of a substance from a liquid to a gaseous form is called:
A)dynamic equilibrium.
B)heat of fusion.
C)condensation.
D)vaporization.
E)volatile.
Q3) Which intermolecular force is present in all molecules and atoms?
A)dispersion forces
B)dipole-dipole forces
C)hydrogen bonding
D)X-forces
E)none of the above
Q4) Intermolecular forces determine if a substance is a solid,liquid or gas at room temperature.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) What will happen if a healthy red blood cell is placed into a container of pure water?
A)The cell will totally dissolve in the water.
B)The cell will remain unchanged.
C)The cell will become swollen.
D)The cell will shrink.
E)none of the above
Q2) What is the molarity of a solution prepared by dissolving 10.7 g NaI in 0.250 L?
A)42.8
B)0.0714
C)2.86x 10<sup>-4</sup>
D)0.286
E)none of the above
Q3) Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500.mL.
A)0.331
B)0.663
C)0.166
D)6.04
E)none of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) Which solution below is considered to have basic character?
A)pOH = 7
B)pH = 2
C)pOH = 4
D)pOH = 13
E)none of the above
Q2) 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
Q3) What is the pH of a solution that has a [H<sup>+</sup>] = 0.0045 M?
A)1.35
B)2.35
C)3.35
D)7.0045
E)none of the above
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16
Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Given N<sub>2</sub> (g)+ 3 H<sub>2</sub> (g) 2 NH<sub>3</sub> (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?
A)Place only N<sub>2</sub> into a sealed vessel.
B)Place only H<sub>2</sub> into a sealed vessel.
C)Place only NH<sub>3</sub> into a sealed vessel.
D)All of the above scenarios.
E)none of the above
Q2) Placing a [ ] around the formula of a chemical means that we are referring to the molar concentration of that chemical.
A)True
B)False
Q3) A chemical equilibrium exists when
A)reactants are completely changed to products.
B)there are equal amounts of reactants and products.
C)the rate at which reactants form products becomes zero.
D)the sum of reactant and product concentrations equals one mole.
E)the rate at which reactants form products is the same as the rate at which products form reactants.
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Page 17
Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) What is the oxidation state of sulfur in SO<sub>3</sub><sup>2</sup><sup>-</sup>?
A)0
B)-2
C)+3
D)+4
E)+6
Q2) 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
Q3) Corrosion of metals may be prevented by keeping them dry at all times.
A)True
B)False
Q4) Oxidation can be defined as the gain of oxygen atoms by another element.
A)True
B)False
Page 18
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) During the first half-life you lose half of the radioactive material,during the second half life you lose the remaining half.
A)True
B)False
Q2) When an atom emits an alpha particle,it becomes a different element.
A)True
B)False
Q3) A fusion reaction emits large amounts of energy while a fission reaction absorbs large amounts of energy.
A)True
B)False
Q4) One method of nuclear medicine uses radioactive isotopes to scan specific regions of the body.
A)True
B)False
Q5) In a Geiger-Muller counter,radioactive particles pass through NaI which emits UV-Vis light.
A)True
B)False
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Production of the synthetic polymer "polyethylene" uses an alkene as a starting monomer unit.
A)True
B)False
Q2) It was originally thought that organic compounds had to come from living things.
A)True
B)False
Q3) The compound named 2,3-dimethylpentane would have how many total number of carbons?
A)3
B)5
C)7
D)8
E)none of the above
Q4) Which of the following compounds is an alkene?
A)C<sub>2</sub>H<sub>6</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>4</sub>H<sub>6</sub>
D)C<sub>5</sub>H<sub>12</sub>
E)none of the above
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Chapter 19: Biochemistry
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Sample Questions
Q1) DNA contained within the nucleus of most cells contains a complete set of instructions to make all of the proteins in the human body.
A)True
B)False
Q2) A gene is:
A)a structure within the cell nucleus that houses DNA.
B)a portion of DNA that codes for a single protein.
C)a sequence of three nucleotides that codes for a single amino acid.
D)a portion of a protein that codes for a single amino acid.
E)none of the above
Q3) Amino acids contain a(n):
A)amine group.
B)carboxylic acid group.
C)"R" side chain.
D)all of the above
E)none of the above
Q4) DNA and RNA are the two types of nucleic acids.
A)True
B)False
Q5) Summarize the main features of the four categories of protein structure.
Page 21
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