Chemistry for Allied Health Practice Questions
Course Introduction
Chemistry for Allied Health provides a foundational understanding of the key chemical principles relevant to careers in healthcare and related fields. The course covers topics such as atomic and molecular structure, chemical bonding, solutions, acids and bases, and basic organic and biochemistry concepts. Emphasis is placed on the application of chemical knowledge to physiological processes, pharmacology, and laboratory techniques commonly used in medical environments. Through lectures, discussions, and laboratory work, students learn to apply chemical reasoning to real-world health scenarios, preparing them for further study and professional roles in nursing, allied health, or medical technology.
Recommended Textbook
Foundations of College Chemistry 13th Edition by Morris Hein
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Chapter 1: An Introduction to Chemistry
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Sample Questions
Q1) Chemistry is the science that deals with the composition of substances and thetransformations they undergo.
A)True
B)False
Answer: True
Q2) In which phase do the particles possess the greatest amount of kinetic energy?
A)solid
B)liquid
C)gas
D)crystal
Answer: C
Q3) The statement,"An apple a day keeps the doctor away",is best described as a(n)
A)observation
B)law
C)theory
D)hypothesis
Answer: D
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Page 3
Chapter 2: Standards for Measurement
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Sample Questions
Q1) A piece of metal has a mass of 86.24g and a volume of 13.4mL.What is its density?
A)0.155g/mL
B)6.44g/mL
C)72.8g/mL
D)99.6g/mL
Answer: B
Q2) When expressed in proper scientific notation the number 4289 is
A)4.289 X 10<sup>-4</sup>
B)4.289 X 10<sup>-3</sup>
C)4.289 X 10<sup>3</sup>
D)4.289 X10<sup>4</sup>
Answer: C
Q3) Convert 76.9 L to cm<sup>3</sup>.
A)76900 cm<sup>3</sup>
B)7690 cm<sup>3</sup>
C)76900000 cm<sup>3</sup>
D)769000 cm<sup>3</sup>
Answer: A
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4
Chapter 3: Elements and Compounds
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Sample Questions
Q1) Which is best classified as a semiconductor?
A)Diamond
B)Silicon
C)Lead
D)Sodium chloride
Answer: B
Q2) What is the symbol of the element that is classified as a metalloid and is in Group IVA and period 3?
A)C
B)Ge
C)Ti
D)Si
Answer: D
Q3) How many atoms of calcium are indicated in the formula Ca(NO<sub>3</sub>)<sub>2</sub>?
A)1
B)2
C)3
D)9
Answer: A
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Chapter 4: Properties of Matter
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Sample Questions
Q1) When water boils it is converted into hydrogen and oxygen.
A)True
B)False
Q2) How many kilojoules of energy are absorbed when 800.0g of water is heated from 20.0<sup>º</sup> C to 50.0<sup>º</sup> C?
A)39.0 kJ
B)163 kJ
C)100.kJ
D)62.8 kJ
Q3) When 9.44g of calcium is heated in air,13.22g of calcium oxide is formed.What is the percent by mass of oxygen in this compound?
A)28.6%
B)40.0%
C)71.4%
D)13.2%
Q4) Melting and boiling are examples of physical changes.
A)True
B)False
Q5) Explain what happens at the molecular level when water freezes.
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Chapter 5: Early Atomic Theory and Structure
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Sample Questions
Q1) In 1911 Ernest Rutherford performed an experiment known as the "Gold Foil Experiment."
He fired a stream of positively charged alpha particles at a sheet of gold foil which was approximately 1000 atoms thick.Alpha particles have a mass of 4 amu and a charge of +2.
Almost all of the alpha particles passed straight through 1000 atoms of gold.A few particleswere deflected or even bounced back from the foil.Alpha particles are more than 7000 times more massive than electrons.What can you conclude regarding the structure of the atom from these observations?
Q2) What is the relative mass of an electron?
A)1/1837 amu
B)½ amu
C)1 amu
D)2 amu
Q3) Which contains the fewest neutrons?
A)H-2
B)H-3
C)He-4
D)He-5
Q4) Explain why the atomic masses of elements are not whole numbers.
Page 7
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Chapter 6: Nomenclature of Inorganic Compounds
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Sample Questions
Q1) What is the correct name for the Fe<sup> +3</sup> ion?
A)Iron (III)
B)Fluorine (III)
C)Phosphorous (III)
D)Iodine (III)
Q2) Which is an anion?
A)A strontium ion
B)A manganese (II)ion
C)A sulfide ion
D)A zinc ion
Q3) Which is sodium chlorite?
A)NaClO<sub> </sub>
B)NaClO<sub>2</sub>
C)NaClO<sub>3</sub>
D)NaClO<sub>4</sub>
Q4) Which is sodium oxalate?
A)NaO
B)NaCO<sub> </sub><sub> </sub>
C)NaC<sub>2</sub>O<sub>4</sub>
D)Na<sub>2</sub>C<sub>2</sub>O<sub>4</sub>
Page 8
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Chapter 7: Quantitative Composition of Compounds
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Sample Questions
Q1) A mole contains Avogadro's number of particles.
A)True
B)False
Q2) One mole of oxygen has a mass of 8.00g.
A)True
B)False
Q3) Which of the following contains the greatest number of atoms?
A)1.0g of lithium
B)1.0g of sodium
C)1.0g of aluminum
D)1.0g of silver
Q4) What is the molecular formula of a compound with the empirical formula
CH<sub>2</sub>O and molar mass of 60.06g? <sub> </sub>
A)CH<sub>2</sub>O
B)C<sub>2</sub>H<sub>4</sub>O<sub>2</sub>
C)C<sub>3</sub>H<sub>6</sub>O<sub>3</sub>
D)C<sub>4</sub>H<sub>8</sub>O<sub>4</sub>
Q5) C<sub>12</sub>H<sub>22</sub>O<sub>11</sub> is an empirical formula.
A)True
B)False
Page 9
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Chapter 8: Chemical Equations
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Sample Questions
Q1) Given the unbalanced equation: H<sub>2</sub>O \(\rarr\)H<sub>2</sub> + O<sub>2</sub>. When properly balanced,the sum of the balancing coefficients is A)4
B)5
C)6
D)7
Q2) The quantity of heat produced by a reaction is known as heat of reaction.
A)True
B)False
Q3) A neutralization reaction is a double-displacement reaction. A)True
B)False
Q4) Which of the following combinations will not form a precipitate?
A)Pb(NO<sub>3</sub>)<sub>2</sub> + NaCl
B)SnCl<sub>2</sub> + KOH
C)FeCl<sub>2</sub> + (NH<sub>4</sub>)<sub>2</sub>S D)NH<sub>4</sub>Br + K<sub>2</sub>SO<sub>4</sub>
Q5) When acids and bases react they always produce a new acid and a new base. A)True
B)False
Page 10
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Chapter 9: Calculations From Chemical Equations
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Sample Questions
Q1) How many moles of Cl<sub>2</sub> are consumed when 0.500 moles of AlCl<sub>3</sub> are produced in the following equation? 2Al + 3Cl<sub>2</sub> \(\rarr\) 2AlCl<sub>3</sub>
A)0.333
B)0.500
C)0.750
D)1.00
Q2) What mass of H<sub>2</sub>O is produced when 12.0g of HCl react completely in the following equation?
6HCl + Fe<sub>2</sub>O<sub>3</sub> \(\rarr\)2FeCl<sub>3</sub> + 3H<sub>2</sub>O
A)2.97g
B)39.4g
C)27.4g
D)110.g
Q3) What mass of sodium hydroxide will neutralize completely 3.612 moles of HCl?
A)3.612 grams
B)144.5 grams
C)11.07 grams
D)0.09030 grams
Q4) Nitrogen gas to water
11
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Chapter 10: Modern Atomic Theory and the Periodic Table
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Sample Questions
Q1) The element with an abbreviated electron configuration [Kr]5s<sup>2</sup>4d<sup>6</sup> is:
A) ruthenium
B) manganese
C) bromine
D) iron
Q2) The ground state electron configuration for an atom of sodium is A)1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>1</sup>
B)1s<sup>2</sup> 2s<sup>2</sup>
C)1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup>
D)1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>4</sup>
Q3) The "alkali" metals are in group
A)1A
B)2A
C)7A
D)8A
Q4) The 4s energy sublevel fills before the 3d energy sublevel.
A)True
B)False
Q5) In the designation 4p<sup>3</sup>;what is the significance of 4,p,and 3?
Page 12
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Chapter 11: Chemical Bonds: the Formation of Compounds
From Atoms
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Sample Questions
Q1) Covalent bonds will most likely form between A)two atoms with a high ionization energy.
B)two atoms with a low ionization energy.
C)an atom with a high ionization energy and an atom with a low ionization energy.
D)no correct answer is given.
Q2) Which compound has double covalent bonds within its molecular structure?
A)NaCl
B)CO<sub>2</sub>
C)CH<sub>4</sub>
D)H<sub>2</sub>O
Q3) The shape of a carbon dioxide molecule is A)bent.
B)linear.
C)trigonal planar.
D)tetrahedral.
Q4) Which type of chemical bond involves the unequal sharing of electrons?
A)Ionic
B)Polar covalent
C)Nonpolar covalent
13
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Chapter 12: The Gaseous State of Matter
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Sample Questions
Q1) Under which set of conditions will a real gas be least likely to act as an ideal gas?
A)High temperature and high pressure
B)High temperature and low pressure
C)Low temperature and high pressure
D)Low temperature and low pressure
Q2) A sample of a gas is held at constant temperature.If the number of moles of gas in the sample is doubled while the pressure is halved,what will happen to the volume of the gas sample?
A)It will increase.
B)It will decrease.
C)It will not change.
Q3) As the temperature of a sample of gas is increased at constant pressure,its volume will
A)increase.
B)decrease.
C)remain the same.
Q4) The volume of one mole of any gas at STP is 22.4 L.
A)True
B)False
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Chapter 13: Liquids
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Sample Questions
Q1) The amount of energy required to change one gram of a liquid,at its boiling point,to a gas is called its heat of A)fusion.
B)freezing.
C)vaporization. D)sublimation.
Q2) What quantity of heat must be removed from 20.0 g of liquid water at 0<sup> </sup><sup>°</sup>C to completely freeze the water? The heat of fusion of ice is 335 J/g.
A)315 J
B)16.8 J
C)6700 J
D)0.0597 J
Q3) Which has the lowest vapor pressure?
A)25 mL of water at 283 K
B)10 mL of water at 298 K
C)50 mL of water at 293 K
D)5 mL of water at 323 K
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Chapter 14: Solutions
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Sample Questions
Q1) What mass of water must be added to 30.5 g of KNO<sub>3</sub> to prepare a 45.0% by mass solution?
A)13.7 g
B)44.2 g
C)37.3 g
D)67.8 g
Q2) What is the molality of a solution in which 0.3 moles of solute is dissolved in 1500.g of solvent?
A)0.0002 m
B)0.002 m
C)0.02 m
D)0.2 m
Q3) Which salt is most soluble in water?
A)Chromium(III)nitrate
B)Calcium carbonate
C)Silver iodide
D)Barium phosphate
Q4) Salt water has a higher freezing point than pure water.
A)True
B)False
Page 16
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Chapter 15: Acids, Bases, and Salts
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Sample Questions
Q1) Boron trifluoride is a Lewis acid.
A)True
B)False
Q2) What mass of ethanol,C<sub>2</sub>H<sub>5</sub>OH,should be added to 200.0 g of water in order to increase its boiling point to 102.5°C? The K<sub>b</sub> for water is 0.512°C/m.Consider if the solute is an electrolyte or a nonelectrolyte.
A)4.9 g
B)0.98 g
C)45 g
D)90.g
Q3) How many times more concentrated is the hydrogen ion concentration in a solution with a pH of 3 than that with a pH of 5?
A)2 times
B)10 times
C)100 times
D)1000 times
Q4) A base solution contains 0.400 moles of OH<sup> -1</sup>.The base solution is neutralized by 43.4 mL of sulfuric acid.What is the molarity of the sulfuric acid solution?
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Page 17
Chapter 16: Chemical Equilibrium
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Sample Questions
Q1) A solution in which equilibrium is reached between dissolved and undissolved solute is
A)saturated.
B)unsaturated.
C)supersaturated.
Q2) The addition of a catalyst to a chemical reaction would change the A)heat of reaction.
B)enthalpy of the reactants.
C)enthalpy of the products.
D)activation energy.
Q3) Calculate the percent ionization of a 0.200 M aqueous solution of HNO<sub>2</sub> having a pH of 2.80.
A)7.1%
B)1.4%
C)2.0%
D)0.79%
Q4) A solution of NaNO<sub>3</sub> would be A)acidic.
B)basic. C)neutral.
Page 18
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Chapter 17: Oxidationreduction
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Sample Questions
Q1) In the following reaction,the chlorine atoms 2 Na + Cl<sub>2</sub> \(\rarr\)2 NaCl
A)gain electrons.
B)lose electrons.
C)gain protons.
D)lose protons.
Q2) All the following are true for a galvanic cell except
A)Oxidation occurs at the cathode
B)A spontaneous reaction takes place in the cell
C)Cations are attracted to the cathode
D)The salt bridge allows the migration of ions
Q3) What is the oxidation number of hydrogen in H<sub>2</sub>O<sub>2</sub>?
A)-2
B)-1
C)+1
D)+2
Q4) The algebraic sum of the oxidation numbers of the elements in a polyatomic ion is zero.
A)True
B)False
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Chapter 18: Nuclear Chemistry
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Sample Questions
Q1) The half-life of Sn-110 is 4 hours.If you have 20.g of this isotope,how much would remain 8 hours later?
A)40.g
B)5.0 g
C)10.g
D)80.g
Q2) If Rn-222 loses an alpha particle the resulting isotope is
A)Pb-218
B)At-222
C)Fr-222
D)Po-218
Q3) If it takes 25 years for a radioactive element to decay to 25% of its initial mass,then its half-life is 12.5 years.
A)True
B)False
Q4) How many protons are in the nucleus of radon-222?
A)222
B)86
C)136
D)88
Page 20
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Chapter 19: Introduction to Organic Chemistry Online Only
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Sample Questions
Q1) Which is toluene?
A)C<sub>6</sub>H<sub>6</sub>
B)C<sub>7</sub>H<sub>8</sub>
C)C<sub>6</sub>H<sub>8</sub>
D)C<sub>8</sub>H<sub>7</sub>
Q2) The number of possible isomers of C<sub>6</sub>H<sub>14</sub> is
A)3
B)5
C)6
D)8
Q3) C<sub>2</sub>H<sub>6</sub> is A)propane. B)ethane. C)butane. D)methane.
Q4) What is the total number of carbon atoms in a molecule of toluene?
A)1
B)6
C)7
D)12
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Chapter 20: Introduction to Biochemistry Online Only
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Sample Questions
Q1) A monosaccharide containing four carbon atoms is called a pentose.
A)True
B)False
Q2) In RNA,thymine is replaced by A)cytosine.
B)adenine.
C)guanine.
D)uracil.
Q3) Fats and oils are prepared from one molecule of glycerine and A)one molecule of fatty acid.
B)two molecules of fatty acid.
C)three molecules of fatty acid.
D)four molecules of fatty acid.
Q4) Which is a component of DNA?
A)Deoxyribose
B)Dextrose
C)Dodecane
D)Doryl
Q5) Explain the structure of RNA.
Q6) Explain how RNA and DNA are different.
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