Chemistry for Allied Health Test Preparation
Course Introduction
Chemistry for Allied Health introduces students to the fundamental principles of chemistry as they relate to the health sciences. The course covers core topics including atomic structure, chemical bonding, acids and bases, solutions, and the properties of gases, with a focus on their practical applications in human biology and medicine. Emphasis is placed on understanding biochemical processes, drug interactions, nutrition, and diagnostic techniques, enabling students pursuing allied health professions to apply chemical concepts to real-world healthcare scenarios and better interpret scientific information relevant to patient care.
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) Which statement about the scientific method is TRUE?
A)The scientific method emphasizes reason as the way to understand the world.
B)The scientific method emphasizes observation and reason as the way to understand the world.
C)The scientific method emphasizes observation and experimentation as the way to understand the world.
D)The scientific method emphasizes scientific laws as the way to understand the world.
E)All of the above statements are false.
Answer: C
Q2) What term best describes a brief statement that summarizes many past observations and predicts new ones?
A)experiment
B)hypothesis
C)scientific law
D)theory
E)none of the above
Answer: C
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Page 3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) In multiplication or division calculations,the answer will have the same number of decimal places as the number carrying the most decimal places.
A)True
B)False
Answer: False
Q2) Which of the following statements is NOT part of the rules for determining significant figures?
A)Non-zero digits at the end of a number are not significant.
B)Zeroes between two numbers are significant.
C)Zeroes to the left of the first non-zero number are not significant.
D)Zeroes at the end of a number,but before a decimal are ambiguous.
E)All of the above statements are part of the rules.
Answer: A
Q3) Suppose a perfectly symmetric metal rod of the element lead has a density of 11.4 g/cm<sup>3</sup>.If this rod is cut in half,the density of each piece is now 5.7 g/cm<sup>3</sup>.
A)True
B)False
Answer: False
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Page 4
Chapter 3: Matter and Energy
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Sample Questions
Q1) An energy diagram that shows the reactants having greater energy than the products illustrates an
A)endothermic reaction.
B)exothermic reaction.
C)isothermic reaction.
D)impossible reaction.
E)none of the above
Answer: B
Q2) An amorphous solid has long range,repeating order.
A)True
B)False
Answer: False
Q3) Like mass,energy can neither be created nor destroyed.
A)True
B)False
Answer: True
Q4) Temperature is simply a measure of the motion of atoms and molecules.
A)True
B)False
Answer: True
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) Which of the following is NOT a correct name,symbol combination?
A)calcium,Ca
B)gold,Au
C)manganese,Mn
D)chromium,Cr
E)potassium,P
Q2) John Dalton was the first person recorded as thinking that matter was ultimately composed of atoms.
A)True
B)False
Q3) Which of the following is NOT a correct name,symbol combination?
A)beryllium,Be
B)phosphorus,P
C)iron,Fe
D)manganese,Mg
E)silicon,Si
Q4) Main-group elements tend to form ions that have the same number of total electrons as the nearest halogen.
A)True
B)False
Page 6
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) Type II metal cations are usually found in the section of the periodic table known as the transition metals.
A)True
B)False
Q2) SO<sub>2</sub> is an ionic compound.
A)True
B)False
Q3) 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
Q4) What is the formula mass of sulfurous acid?
A)82.08 amu
B)98.08 amu
C)83.09 amu
D)66.08 amu
E)none of the above
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Chapter 6: Chemical Composition
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Sample Questions
Q1) Which of the following statements about empirical formulas is incorrect?
A)An empirical formula represents a molecule.
B)An empirical formula gives the smallest whole number ratio of each type of atom in a molecule.
C)An empirical formula must be multiplied by an integer to obtain the molecular formula.
D)The molecular formula can be the same as the empirical formula in some situations.
E)All statements are correct.
Q2) The mole has a value of 6.023 × 10<sup>22</sup>.
A)True
B)False
Q3) What would the empirical formula be for the molecular compound
C<sub>6</sub>H<sub>9</sub>O<sub>4</sub>?
A)C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>
B)CH<sub>3</sub>O<sub>2</sub>
C)C<sub>3</sub>H<sub>6</sub>O<sub>2</sub>
D)C<sub>3</sub>H<sub>9</sub>O<sub>4</sub>
E)none of the above
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) What is the net ionic equation for the reaction of hydrochloric acid with potassium hydroxide?
A)H<sup>+</sup> + Cl<sup>-</sup> + K<sup>+</sup> + OH<sup>-</sup> H<sub>2</sub>O + K<sup>+</sup> + Cl<sup>-</sup>
B)HCl + KOH H<sub>2</sub>O + KCl
C)H<sup>+</sup> + OH<sup>-</sup> H<sub>2</sub>O D)2H<sup>+</sup> +2Cl<sup>-</sup> + K<sup>2</sup><sup>+</sup> + 2OH<sup>-</sup> H<sub>2</sub>O + K<sup>2</sup><sup>+</sup> +2 Cl<sup>-</sup>
E)none of the above
Q2) What type of reaction is the generic equation A + B \(\to\) AB?
A)synthesis/combination
B)decomposition
C)single displacement
D)double-displacement
E)none of the above
Q3) A net ionic equation shows all ionic species that are present in solution.
A)True
B)False
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9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Which ingredient is the limiting reactant if you have 6 cups of flour,9 eggs and 2 tbs of oil?
Given: 2 cups flour + 3 eggs + 1 tbs oil 4 waffles
A)flour
B)eggs
C)oil
D)waffles
E)not enough information
Q2) How many grams of NO<sub>2</sub> are theoretically produced if we start with 1.20 moles of S and 9.90 moles of HNO<sub>3</sub>?
Reaction: S<sub> </sub>+ 6HNO<sub>3 </sub> H<sub>2</sub>SO<sub>4</sub> + 6NO<sub>2</sub> + 2H<sub>2</sub>O
A)7.20
B)331
C)455
D)786
E)not enough information
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) Which subshell letter corresponds to a 4-leaf clover orbital pattern?
A)s
B)p
C)d
D)f
E)not enough information
Q2) Which of the statements about light is FALSE?
A)Light travels through space at a speed of 3.00 × 10<sup>8</sup> m/s.
B)Light travels much faster than sound.
C)A packet of light energy is called a photon.
D)A characteristic feature of light that determines its color is its wavelength.
E)All of the above statements are true.
Q3) Which of the following elements has the electron configuration of 3s<sup>2</sup>3p<sup>4</sup> in its outermost shell?
A)Al
B)Si
C)S
D)Cl
E)none of the above
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Page 11
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 potassium in KCl is: K<sup>+</sup>.
A)True
B)False
Q3) Lewis theory predicts that the formula for a compound between barium and sulfur is:
A)BaS
B)Ba<sub>2</sub>S
C)BaS<sub>2</sub>
D)BaS<sub>3</sub>
E)none of the above
Q4) The VSEPR theory predicts that the H-C-H angle in CH<sub>4</sub> measures 120°.
A)True
B)False
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Chapter 11: Gases
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Sample Questions
Q1) What happens to the volume of a gas when you double the number of moles of gas while keeping the temperature and pressure constant?
A)The volume is halved.
B)The volume doubles.
C)The volume decreases,but more information is needed.
D)The volume increases,but more information is needed.
E)none of the above
Q2) For all gas law calculations,the temperature must be in kelvins.
A)True
B)False
Q3) What is the third most abundant component of dry air?
A)carbon dioxide
B)oxygen
C)nitrogen
D)argon
E)smog
Q4) Gases fill the entire volume of their container.
A)True
B)False
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) You can increase the vapor pressure of a liquid by:
A)increasing temperature.
B)increasing the viscosity.
C)establishing dynamic equilibrium.
D)using a nonvolatile compound.
E)all of the above
Q2) Which state of matter has a high density and a definite volume?
A)solids
B)liquids
C)gases
D)both solids and liquids
E)none of the above
Q3) Intermolecular forces determine if a substance is a solid,liquid or gas at room temperature.
A)True
B)False
Q4) Atoms in a solid are always arranged in a well-ordered pattern.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) An osmosis cell is constructed of a "U" shaped tube with a semipermeable membrane separating the two arms of the tube.Suppose a concentrated solution is placed in the left arm of the U-tube,and a dilute concentration of the same substance is poured into the other arm to the same height.After a period of time has elapsed,you would expect to find that
A)the level of liquid in the left arm is now higher.
B)the level of the liquid in the right arm is now higher.
C)the levels in both arms stay at the same height.
D)no molecules of any type cross the membrane.
E)none of the above
Q2) How many grams of barium sulfate are produced if 25.34 mL of 0.113 M BaCl<sub>2</sub> completely react given the reaction: BaCl<sub>2</sub> (aq)+ Na<sub>2</sub>SO<sub>4</sub>(aq) BaSO<sub>4</sub> (s)+ 2NaCl (aq)
A)5.90
B)26.3
C)1039
D)0.668
E)none of the above
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Page 15
Chapter 14: Acids and Bases
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Sample Questions
Q1) Bases have a bitter taste.
A)True
B)False
Q2) In the following reaction: HCO<sub>3</sub><sup>-</sup><sup> </sup>(aq)+ H<sub>2</sub>O (aq) H<sub>2</sub>CO<sub>3</sub><sup> </sup>(aq)+ OH<sup>-</sup><sup> </sup>(aq)
A)HCO<sub>3</sub><sup>-</sup><sup> </sup>is an acid and H<sub>2</sub>CO<sub>3 </sub>is its conjugate base.
B)H<sub>2</sub>O is an acid and OH<sup>-</sup> is its conjugate base.
C)HCO<sub>3</sub><sup>-</sup><sup> </sup>is an acid and OH<sup>-</sup> is its conjugate base.
D)H<sub>2</sub>O is an acid and H<sub>2</sub>CO<sub>3</sub> is its conjugate base.
E)H<sub>2</sub>O is an acid and HCO<sub>3</sub><sup>-</sup> is its conjugate base.
Q3) A strong acid is one that is very concentrated.
A)True
B)False
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) For the reaction Ag<sub>2</sub>S(s) 2 Ag<sup>+</sup> (aq)+ S<sup>2-</sup> (aq),K<sub>eq</sub> = 2.4 × 10<sup>-4</sup>,and the equilibrium concentration of sulfide ion is [S<sup>2-</sup>] = 0.0023 M..What is [Ag<sup>+</sup>] at equilibrium?
A)0.052 M
B)0.32 M
C)0.015 M
D)0.10 M
E)none of the above
Q2) What happens to the equilibrium constant when a catalyst is added to the reaction mixture?
A)increases
B)decreases
C)does not change
D)varies
E)none of the above
Q3) A reversible reaction is one that can be stopped and then restarted as needed. A)True
B)False
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17
Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) The half-reaction 2 Br <sup>1</sup><sup>-</sup> Br<sub>2</sub> + 2 e<sup>-</sup> is balanced with respect to mass but it is not balanced with respect to charge.
A)True
B)False
Q2) What is the oxidation state of the underlined element in the reaction: NaHCO<sub>3</sub> + HCl \(\to\) NaCl + CO<sub>2</sub> + H<sub>2</sub>O
A)0
B)+1
C)-1
D)+2
E)-2
Q3) Identify the substance being oxidized in the following reaction: CH<sub>4</sub> + 2O<sub>2</sub> \(\to\) CO<sub>2</sub> + 2H<sub>2</sub>O.
A)CH<sub>4</sub>
B)O<sub>2</sub>
C)CO<sub>2</sub>
D)H<sub>2</sub>O
E)none of the above
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Page 18
Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Nuclear fusion:
A)requires intense temperatures that make it impossible to harness as an energy source with our current technology.
B)is the basis of the hydrogen bomb.
C)can be done but requires the detonation of a traditional fission bomb.
D)is a possible energy source of the future.
E)all of the above
Q2) 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
Q3) Madam Curie discovered two new elements.
A)True
B)False
Q4) C-14 dating has been verified using old iron ore samples of known age.
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) Which of the following statements is FALSE about polymers?
A)Several monomer units link together without eliminating any atom or group to form addition polymers.
B)During condensation polymerization an atom or group is eliminated.
C)Copolymers contain more than one kind of polymer.
D)Nylon 6,6 and polyurethane are examples of copolymers.
E)none of the above.
Q2) The reaction CH<sub>2</sub>=CH<sub>2</sub> + H<sub>2</sub> CH<sub>3</sub>CH<sub>3</sub> would best be described as: A)substitution.
B)combustion.
C)addition.
D)hydrogenation.
E)none of the above
Q3) A compound named "propanal" would be classified as an A)alcohol. B)amine. C)aldehyde. D)ether.
E)none of the above
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Chapter 19: Biochemistry
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Sample Questions
Q1) The portion of the cell that contains the genetic information is called:
A)cytoplasm.
B)membrane.
C)nucleus.
D)mitochondria.
E)none of the above
Q2) Glucose is an example of a monosaccharide.
A)True
B)False
Q3) All of the following are usable forms of carbohydrates by humans EXCEPT: A)glucose.
B)sucrose.
C)cellulose.
D)glycogen.
E)both C and D
Q4) Quaternary protein structure is simply the sequence of amino acids in that protein's chain.
A)True
B)False
Q5) Summarize the main features of the four categories of protein structure.
Page 21
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