Chemistry for Health Sciences
Exam Materials
Course Introduction
Chemistry for Health Sciences provides foundational knowledge of chemical principles with a specific focus on their application in the health and medical fields. The course covers topics such as atomic structure, chemical bonding, states of matter, solutions, acids and bases, organic and biochemistry, and the interplay of chemicals in biological systems. Emphasis is placed on understanding the chemical nature of drugs, the metabolic pathways in the human body, and laboratory techniques relevant to clinical and healthcare environments. Designed for students pursuing careers in nursing, pharmacy, allied health, or biology, this course links theoretical chemistry concepts to real-world health and physiological processes.
Recommended Textbook
Introductory Chemistry 6th Edition by Nivaldo J. Tro
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19 Chapters
2138 Verified Questions
2138 Flashcards
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Chapter 1: The Chemical World
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59 Verified Questions
59 Flashcards
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Sample Questions
Q1) Who discovered the law of conservation of mass?
A)John Dalton
B)Antoine Lavoisier
C)Nivaldo Tro
D)John Dalton and Antoine Lavoisier
E)none of the above
Answer: B
Q2) A theory is always true and can never be proven as wrong.
A)True
B)False
Answer: False
Q3) When a sealed can of soda pop is opened,the carbon dioxide gas fizzes out because the pressure is released.
A)True
B)False
Answer: True
Q4) Antoine Lavoisier proposed the atomic theory.
A)True
B)False
Answer: False
Page 3
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Chapter 2: Measurement and Problem Solving
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131 Flashcards
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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) Numbers are usually written so that the uncertainty is in the last reported digit.
A)True
B)False Answer: True
Q3) The prefix micro represents the multiplier 0.001.
A)True
B)False Answer: False
Q4) The correct prefix for the multiplier 1,000,000 is:
A)mega.
B)milli.
C)micro.
D)nano.
E)none of the above Answer: A
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Chapter 3: Matter and Energy
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Sample Questions
Q1) The temperature of 390 kelvin is warmer than which one of the following temperatures?
A)250 deg F
B)135 deg C
C)109 deg C
D)44 deg F
E)none of the above
Answer: C
Q2) How many joules are in 55.2 calories?
A)13,200
B)55,200
C)13.2
D)231
E)none of the above
Answer: D
Q3) When a chemical "cold pack" is activated,the chemical reactants absorb heat from the surroundings.
A)True
B)False
Answer: True
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) If an isotope of an element has 27 neutrons and a mass number of 52 ,how many electrons must it have?
A)25
B)27
C)52
D)79
E)none of the above
Q2) Isotopes are atoms of the same element that have a different numbers of neutrons.
A)True
B)False
Q3) John Dalton formalized an atomic theory that gained acceptance in the early 19th century.
A)True
B)False
Q4) The atomic number of nitrogen is 14.01.
A)True
B)False
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6
Chapter 5: Molecules and Compounds
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110 Flashcards
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Sample Questions
Q1) What is the correct formula for the molecular compound heptaphosphorus octafluoride?
A)P<sub>5</sub>F<sub>8</sub>
B)P<sub> 7</sub>F<sub>6</sub>
C)P<sub>6</sub>F<sub>7</sub>
D)P<sub>7</sub>F<sub>8</sub>
E)none of the above
Q2) What is the formula for an ionic compound made of magnesium and sulfur?
A)MgS
B)MgS<sub>2</sub>
C)Mg<sub>2</sub>S
D)Mg<sub>2</sub>S<sub>3</sub>
E)none of the above
Q3) Which of the following compounds have the smallest formula mass?
A)CO<sub>2</sub>
B)SO<sub>2</sub>
C)NO<sub>2</sub>
D)SiO<sub>2</sub>
E)H<sub>2</sub>O
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Page 7
Chapter 6: Chemical Composition
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118 Flashcards
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Sample Questions
Q1) The empirical formula mass is 18.0 and the molecular formula mass is 90,therefore n = 5.
A)True
B)False
Q2) The empirical formula mass must be 25.0 if the molecular formula mass is 250 and n = 5.
A)True B)False
Q3) What is the mass percent of chlorine in hydrochloric acid?
A)2.8
B)35.5
C)97.2
D)70.1
E)none of the above
Q4) The molar mass of a compound serves as a conversion factor between grams and moles.
A)True
B)False
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) What is the molecular equation for the reaction of hydrochloric acid with potassium hydroxide?
A)H<sub>2</sub>Cl + 2KOH H<sub>2</sub>O +2KCl
B)2HCl + K(OH)<sub>2</sub> 2H<sub>2</sub>O + KCl<sub>2</sub>
C)H<sup>+</sup> + OH<sup>-</sup> H<sub>2</sub>O
D)HCl + KOH H<sub>2</sub>O + KCl
E)none of the above
Q2) 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>
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.
Q3) All ionic compounds dissolve in water.
A)True
B)False
PbI<sub>2</sub>(s)+
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Page 9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) What is the excess 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
Q2) If the theoretical yield of a reaction is 42.0 grams of product and the percent yield is 75%.How many grams were actually produced?
A)5400
B)56
C)32
D)1.8
E)none of the above
Q3) The conversion factor between mass and moles for a compound is the molar mass. A)True
B)False
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) The correct electron configuration for fluorine is: 1s<sup>2</sup>2s<sup>2</sup>2p<sup>5</sup>.
A)True
B)False
Q2) Which form of electromagnetic radiation has the lowest frequency?
A)Radio Waves
B)Microwaves
C)X-rays
D)Gamma Rays
E)Infrared Radiation
Q3) The n = ________ principal shell is the lowest that may contain a d-subshell.
A)1
B)2
C)3
D)4
E)not enough information
Q4) The subshells s,p,d,and f all have the same energy as long as they are in the same principal shell.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:
A)AlBr
B)Al<sub>2</sub>Br
C)AlBr<sub>3</sub>
D)AlBr<sub>2</sub>
E)none of the above
Q2) Which of the following is considered a single electron group?
A)a lone pair of electrons
B)a single bond
C)a double bond
D)a triple bond
E)all of the above
Q3) What is the electron geometry if you have 2 electron groups around the center atom?
A)linear
B)trigonal planar
C)tetrahedral
D)trigonal bipyramidal
E)not enough information
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Chapter 11: Gases
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Sample Questions
Q1) If the number of moles of a gas initially contained in a 2.10 L vessel is doubled,what is the final volume of the gas in liters? (Assume the pressure and temperature remain constant.)
A)6.30
B)1.05
C)4.20
D)8.40
E)none of the above
Q2) A sealed bag of potato chips will expand when taken to a higher altitude.This is an example of Boyle's law.
A)True
B)False
Q3) What is the initial temperature of a gas if the volume changed from 1.00 L to 1.10 L and the final temperature was determined to be 255.0°C?
A)480°C
B)-41°C
C)232°C
D)207°C
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) When one mole of water vapor at 100°C condenses,it will release an amount of energy equivalent to its heat of vaporization (40.7 kJ).
A)True
B)False
Q2) Intermolecular forces determine if a substance is a solid,liquid or gas at room temperature.
A)True
B)False
Q3) What types of forces exist between I<sub>2</sub> molecules?
A)dispersion forces
B)dipole-dipole forces
C)hydrogen bonding
D)ion-dipole forces
E)none of the above
Q4) Intermolecular forces hold atoms and molecules in place in a solid.
A)True
B)False
Q5) Intermolecular forces are the attractive forces between atoms within a compound.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) A 0.15 M solution of BaCl<sub>2</sub> contains:
A)0.15 M Ba<sup>2+</sup> ions and 0.15 M Cl<sup>-</sup> ions.
B)0.15 M Ba<sup>2+</sup> ions and 0.30 M Cl<sup>-</sup> ions.
C)0.30 M Ba<sup>2+</sup> ions and 0.15 M Cl<sup>-</sup> ions.
D)0.30 M Ba<sup>2+</sup> ions and 0.30 M Cl<sup>-</sup> ions.
E)none of the above
Q2) A saturated solution holds the maximum amount of solute under the solution conditions.
A)True
B)False
Q3) A solution that is 13.58 percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water.
A)True
B)False
Q4) What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
A)21.9 mL
B)0.560 mL
C)257 mL
D)560.mL
E)none of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) Consider a 1.0 X 10<sup>-7</sup> M HCl solution and a 1.0 x10<sup>-7</sup> M NaOH solution.Which statement below is true?
A)The HCl solution is acidic.
B)The NaOH solution is basic.
C)Only the HCl solution is neutral.
D)Only the NaOH solution is neutral.
E)Both of these solutions are neutral.
Q2) The ion product constant for water (K<sub>w</sub>)is best stated as K<sub>w</sub> = [H<sub>2</sub>O] [H<sup>+</sup>].
A)True
B)False
Q3) What are the products of a neutralization reaction?
A)salt and carbon dioxide
B)carbon dioxide and water
C)water and salt
D)oil and water
E)none of the above
Q4) A weak acid is a dilute acid that is not very powerful.
A)True
B)False
Page 16
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) 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.
Q2) Dynamic equilibrium is established when the rate of the forward reaction goes to zero.
A)True
B)False
Q3) The effect of a catalyst is to:
A)increase the number of collisions between reactants.
B)increase the temperature of the reactants whereby more products are formed.
C)change the position of the equilibrium.
D)change the stoichiometry of the reaction.
E)lower the activation energy of a reaction whereby making it easier for the reactants to get over the energy hump.
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) What is the oxidation state of nitrogen in N<sub>2</sub>O<sub>3</sub>?
A)0
B)+1
C)+2
D)+3
E)+6
Q2) Which of the following are typically TRUE of a reducing agent?
1.It causes reduction.
2.It gains electron(s).
3.It is the oxidized substance.
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
Q3) Electrons flowing through a wire is an example of electrical current.
A)True
B)False
Q4) Suggest two methods to reduce corrosion of a metal such as iron and briefly explain how each method works.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Nuclear equations do not need to be balanced since a new element forms.
A)True
B)False
Q2) Carbon-14 dating is based on the fact that C-14 is continuously being made in the upper atmosphere.
A)True
B)False
Q3) Radioactivity is the emission of tiny,invisible radio signals by the nuclei of certain atoms.
A)True
B)False
Q4) 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
Q5) Radioactive particles can pass through matter.
A)True
B)False
Q6) Briefly distinguish between nuclear fission and nuclear fusion.
Page 19
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Which of the following terms could NOT be applied to the compound CH<sub>2</sub>=CHCH<sub>2</sub>CH<sub>2</sub>OH?
A)unsaturated
B)an alcohol
C)an alkene
D)a carboxylic acid
E)none of the above
Q2) Which of the following is an example of a polymer?
A)DNA
B)protein
C)nylon
D)plexiglass
E)all of the above
Q3) Hydrocarbon combustion reactions are highly endothermic - they absorb large amounts of heat.
A)True
B)False
Q4) R-O-R is an ether functional group.
A)True
B)False
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Chapter 19: Biochemistry
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Sample Questions
Q1) A tripeptide consists of three steroids linked together.
A)True
B)False
Q2) Protein synthesis occurs at the ribosome.
A)True
B)False
Q3) Which of the following statements is FALSE about polysaccharides?
A)They are long chain structures containing large number of repeating monosaccharide units.
B)Starch,cellulose,and glycogen are polysaccharides.
C)Table sugar is a polysaccharide.
D)They break down to produce monosaccharides during digestion.
E)none of the above
Q4) A section of DNA contains the bases ACGTC,so the correct sequence in the complementary strand is:
A)CATGA
B)UGCAG
C)TGCAG
D)GTACT
E)none of the above
Page 21
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