Chemistry for Health Sciences Pre-Test Questions - 4358 Verified Questions

Chemistry for Health Sciences

Pre-Test Questions

Course Introduction

This course introduces fundamental concepts in chemistry with a focus on their applications in the health sciences. Topics include atomic and molecular structure, chemical bonding, states of matter, solutions, acids and bases, and the principles of chemical reactions. Emphasis is placed on the relevance of chemistry to biological systems, pharmaceuticals, and clinical practice. Through lectures, laboratory experiments, and problem-solving exercises, students will develop an understanding of how chemical principles underpin processes in the human body and the safe use of chemicals in health professions.

Recommended Textbook Chemistry 7th Edition by John E. McMurry

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Page 2

Chapter 1: Chemical Tools: Experimentation and Measurement

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Sample Questions

Q1) The factor 0.01 corresponds to which prefix?

A)deka

B)deci

C)centi

D)milli

Answer: C

Q2) The fundamental SI unit of mass is the ________.

Answer: kilogram

Q3) Round off 477,503 to four significant figures.

A)4775

B)4776

C)4.775 × 10⁵

D)4.776 × 10⁵

Answer: C

Q4) The factor 10^-2 corresponds to which prefix?

A)deka

B)deci

C)centi

D)milli

Answer: C

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which of the following is a part of Dalton's atomic theory?

A)Atoms are rearranged but not changed during a chemical reaction.

B)Atoms break down during radioactive decay.

C)Atoms contain protons,neutrons,and electrons.

D)Isotopes of the same element have different masses.

Answer: A

Q2) How many electrons are in the ion,P^3-?

A)12

B)18

C)28

D)34

Answer: B

Q3) Na₂S is named

A)sodium disulfide.

B)sodium sulfide.

C)sodium(II)sulfide.

D)sodium sulfur.

Answer: B

Q4) The number of neutrons in a neutral atom of uranium-238 is ________.

Answer: 146

4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) The balanced equation for the decomposition of water is shown below.

2 H₂O 2 H₂ + O₂

If 0.72 g of water react completely in this reaction,what is the theoretical yield of H₂?

Answer: 0.080 g

Q2) How many moles of O₂ react with 3.600 mol of Cu₂O in the following reaction? 2 Cu₂O(s)+ O₂(g) 4 CuO(s)

A)7.200 mol

B)3.600 mol

C)1.800 mol

D)5.400 mol

Answer: C

Q3) What is the molar mass of aspartic acid,C₄O₄H₇N?

A)43 g/mol

B)70 g/mol

C)133 g/mol

D)197 g/mol

Answer: C

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Page 5

Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) Which outcome corresponds to the reaction: H₃AsO₄ + 3 OH^- 3 H₂O + AsO₄^3-?

A)box (a)

B)box (b)

C)box (c)

D)None of these

Q2) The reaction Cu(s)+ 2 HCl(aq) CuCl₂(aq)+ H₂(g)is predicted not to occur because Cu is ________ than H⁺ in the activity series.

Q3) Using the following portion of the activity series for oxidation half reactions Li(s) Li⁺(aq)+ e^-

Al(s) Al³⁺(aq)+ 3e^-

Fe(s) Fe²⁺(aq)+ 2e^-

Pt(s) Pt²⁺(aq)+ 2e^-

Determine which pairs of reactions will occur.

A)Al(s)with Fe²⁺(aq)and Pt(s)with Li⁺(aq)

B)Fe(s)with Al(s)and Al³⁺(aq)with Pt²⁺(aq)

C)Fe(s)with Pt²⁺(aq)and Al(s)with Pt²⁺(aq)

D)Li(s)with Al³⁺(aq)and Fe(s)with Al³⁺(aq)

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Page 6

Chapter 5: Periodicity and the Electronic Structure of Atoms

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Sample Questions

Q1) Which one of these spheres represents an atom of As?

A)sphere (a)

B)sphere (b)

C)sphere (c)

D)sphere (d)

Q2) Which of the following is not a valid set of quantum numbers?

A)n = 2,l = 1,m_l = 0,and m_s = +1/2

B)n = 2,l = 1,m_l = -1,and m_s = +1/2

C)n = 3,l = 0,m_l = 0,and m_s = +1/2

D)n = 3,l = 2,m_l = 3,and m_s = +1/2

Q3) Which of the following is not quantized?

A)the charge on a monatomic ion

B)the distance between two objects

C)the population of the United States

D)the static charge on a balloon rubbed with wool

Q4) Of the following,which atom has the smallest atomic radius?

A)K

B)As

C)Rb

D)Sb

Page 7

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Chapter 6: Ionic Compounds: Periodic Trends and Bonding

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Sample Questions

Q1) The group 4A element that always obeys the octet rule in its stable compounds is

Q2) Which of the following represents the change in electronic configuration that is associated with the first ionization energy of barium?

A)[Xe]6s¹6p¹ [Xe]6s¹ + e^-

B)[Xe]6s² [Xe]6s¹6p¹

C)[Xe]6s² [Xe]6s¹ + e^-

D)[Xe]6s² + e^- [Xe]6s²6p¹

Q3) How many electrons are in the outermost shell of the Al³⁺ ion in its ground state?

A)2

B)3

C)6

D)8

Q4) Which of the above pictures are more likely to represent ionic compounds?

A)pictures (a)and (b)

B)pictures (a)and (d)

C)pictures (b)and (c)

D)pictures (b)and (d)

Q5) The number of electrons in the ion K⁺ is ________.

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Chapter 7: Covalent Bonding and Electron-Dot Structures

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Sample Questions

Q1) Which of the following contains an atom that does not obey the octet rule?

A)LiBr

B)CO₂

C)PCl₃

D)CCl₄

Q2) A::A represents A)a double bond.

B)a quadruple bond.

C)one lone pair of electrons.

D)two lone pairs of electrons.

Q3) How many lone pairs are on the Br atom in BrI₂^-?

A)0

B)1

C)2

D)3

Q4) How many lone pairs of electrons are on the P atom in PF₃?

A)0

B)1

C)2

D)3

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Chapter 8: Covalent Compounds: Bonding Theories and

Molecular Structure

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Sample Questions

Q1) Based on molecular orbital theory,in order to weaken the N-N bond in N₂,electrons should be A)added.

B)removed.

C)either added or removed.

D)neither added nor removed.

Q2) What is the hybridization of the oxygen atom labeled O₁?

A)sp

B)sp²

C)sp³

D)sp⁴

Q3) In the drawing of acetic acid,CH₃CO₂H,a partial positive charge ( +)occurs on A)only atom (a).

B)only atom (b).

C)atoms (a)and (c).

D)atoms (b)and (d).

Q4) Are the -bonds in CH₃CO₂^- delocalized or localized?

Q5) The molecular geometry of OCCl₂ is ________.

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Chapter 9: Thermochemistry: Chemical Energy

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Sample Questions

Q1) The energy of motion is

A)electrical energy.

B)dam energy.

C)reserve energy.

D)kinetic energy.

Q2) When 8.00 g of Ba(s)is added to 100.00 g of water in a container open to the atmosphere,the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 77.62°C.If the specific heat of the solution is 4.18 J/(g °C),calculate H for the reaction,as written. Ba(s)+ 2 H₂O(l)

Ba(OH)₂(aq)+ H₂(g) H = ?

A)-431 kJ

B)-3.14 kJ

C)3.14 kJ

D)431 kJ

Q3) For the reaction: A + 2 B 3 C, H° = -203 kJ.For the reaction 12 C 4 A + 8 B, H° = ________ kJ.

Q4) The sign of S° for reaction below is expected to be ________. 2 H₂(g)+ O₂(g) 2 H₂O(g)

Q5) ________ energy is the kinetic energy of molecular motion.

Q6) Is a hydroelectric dam a form of kinetic or potential molecular energy?

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Chapter 10: Gases: Their Properties and Behavior

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Sample Questions

Q1) A 0.529-g sample of gas occupies 125 mL at 60.cm of Hg and 25°C.What is the molar mass of the gas?

A)11 g/mol

B)81 g/mol

C)110 g/mol

D)130 g/mol

Q2) What is the pressure (in mm Hg)of the gas inside the above apparatus if the outside pressure,P_atm,is 750 mm Hg and the difference in mercury levels, h,is 50 mm Hg?

A)50 mm Hg

B)700 mm Hg

C)750 mm Hg

D)800 mm Hg

Q3) Gases do not behave ideally under conditions of ________ pressure and ________ temperature.

Q4) At an atmospheric pressure of 745 mm Hg,what is the pressure of He gas inside a cylinder that is attached to an open-end manometer in which the level of mercury in the open side of the manometer is 25 mm Hg higher than the side that is attached to the gas cylinder?

Q5) At 298 K which is larger rate of effusion or rate of diffusion?

Page 12

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Chapter 11: Liquids, solids, and Phase Changes

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Sample Questions

Q1) How many Br^- ions are around each Na⁺ ion in NaBr,which has a cubic unit cell with Br^- ions on each corner and each face?

A)1

B)4

C)6

D)8

Q2) Which transition could occur if a solid is heated at a pressure below the triple point pressure?

A)condensation

B)deposition

C)melting

D)sublimation

Q3) Which of the following forms a molecular solid?

A)CaCl₂ 

B)C₉H₈O₄

C)C,graphite

D)palladium

Q4) The phase change H₂(g) H₂(s)is called ________,and the enthalpy change, H,for this phase change has a ________ sign.

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Chapter 12: Solutions and Their Properties

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Sample Questions

Q1) To make a 3.00 m solution,one could take 3.00 moles of solute and add

A)1.00 L of solvent.

B)1.00 kg of solvent.

C)enough solvent to make 1.00 L of solution.

D)enough solvent to make 1.00 kg of solution.

Q2) Which of the following is not an application of colligative properties?

A)adding silver to mercury to lower the vapor pressure of mercury

B)desalinating sea water by reverse osmosis

C)melting snow by application of salt

D)reduced boiling points of pure liquids at increased altitudes

Q3) When a particular solid begins to dissolve in water,the temperature rises dramatically.For the dissolving of this solid in pure water

A) H_soln is always negative and S_soln may be negative or positive.

B) H_soln is always negative and S_soln is always positive.

C) H_soln is always positive and S_soln may be negative or positive.

D) H_soln is always positive and S_soln is always positive.

Q4) Molarity is defined as ________,whereas molality is defined as ________.

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) For the hypothetical second order reaction: A products,the general rate law is: rate = k[A]².How long is the third half-life of the reaction if [A]₀ is 0.080 M and the first half-life is 22 minutes?

A)0.57 min

B)1.7 min

C)7.3 min

D)88 min

Q2) A reaction has a rate constant,k = 1.2 × 10^-12 s^-1 at 273 K and k = 5.1 × 10^-7 s^-1 at 373 K has an activation energy,E_a = ________ kJ/mol.

Q3) A mechanism for a naturally occurring reaction that destroys ozone is: Step 1: O₃(g)+ HO(g) HO₂(g)+ O₂(g)

Step 2: HO₂(g)+ O(g) HO(g)+ O₂(g)

Which species is a catalyst and what type of catalysis is occurring?

A)HO,homogeneous

B)HO,heterogeneous

C)O₃,homogeneous

D)O,heterogeneous

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) At a certain temperature,hydrogen and iodine react to form hydrogen iodide: H₂(g)+ I₂(g) 2 HI(g).

When initial amounts of H₂,I₂,and HI are mixed,the concentration of HI increases.Which statement below is true?

A)K_c < Q

B)K_c > Q

C)K_c = Q

D)More information is needed to make a statement about K_c.

Q2) If the volume of the equilibrium mixture is decreased,what will happen to the number of AB molecules and the number of B atoms?

A)The number of AB molecules and the number of B atoms will both decrease.

B)The number of AB molecules will increase;the number of B atoms will decrease.

C)The number of AB molecules will decrease;the number of B atoms will increase.

D)The number of AB molecules and the number of B atoms will both increase.

Q3) A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

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Page 16

Chapter 15: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.050 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

A)1.5 × 10^-4 M

B)4.3 × 10^-7 M

C)2.2 × 10^-8 M

D)5.6 × 10^-11 M

Q2) Of the elements indicated on the periodic table shown above,which forms the weakest oxoacid acid with the formula H₂XO₃ or HXO₃,where X = A,B,C,or D?

A)A

B)B

C)C

D)D

Q3) A 0.50 M KNO₂ solution will have a pH ________ seven.

Q4) Erythromycin is a basic antimicrobial with pK_b = 5.2.A 1.0 × 10^-3 M solution of erythromycin has a pH of ________ and a ________ percent ionization.

Q5) The pH of a 0.055 M KOH solution is ________.

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Chapter 16: Applications of Aqueous Equilibria

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Sample Questions

Q1) Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?

A)HF(aq)+ LiOH(aq) H₂O(l)+ LiF(aq)

B)H₃O⁺(aq)+ OH^-(aq) 2 H₂O(l)

C)HI(aq)+ NH₃(aq) NH₄I(aq)

D)H₃O⁺(aq)+

NH₄⁺(aq)+ H₂O(l)

NH₃(aq)

Q2) Which pair of ions can be separated by the addition of chloride ion?

A)Ag⁺ and Zn²⁺

B)Ni²⁺ and Bi³⁺

C)Pb²⁺ and Hg₂²⁺

D)Ca⁺ and Li⁺

Q3) If solution (1)is a saturated solution of CaCO₃,which of solutions (1)-(4)represents the solution after a small amount of Ca(NO₃)₂ is added and equilibrium is restored?

A)(1)

B)(2)

C)(3)

D)(4)

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Page 18

Chapter 17: Thermodynamics: Entropy, free Energy, and Equilibrium

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Sample Questions

Q1) The Boltzmann formula is S = k ln W.A perfect crystal has a molar entropy of 0 at absolute zero because

A)W = 0.

B)W = 1.

C)W = N_A.

D)k = 1.

Q2) For the reaction N₂(g)+2 O₂(g) 2 NO₂(g), H° = 66.4 kJ/mol and S° = -121.5 J/K. S_total for this reaction is ________ J/K,and the reaction is ________ (spontaneous,nonspontaneous)at 25°C.

Q3) Which of the following processes is non-spontaneous at standard temperature and pressure?

A)Iron metal,oxygen,and water form rust (Fe₂O₃).

B)Melting of solid ice to ice water.

C)Diffusion of perfume molecules across a room.

D)A reaction at equilibrium moves to non-equilibrium.

Q4) A reaction for which H° = + 98.8 kJ and S° = + 141.5 J/K is ________ (spontaneous or nonspontaneous)at low temperatures and ________ (spontaneous or nonspontaneous)at high temperatures.

Q5) What is the entropy of 50 molecules in a system of 1000 boxes?

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Chapter 18: Electrochemistry

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Sample Questions

Q1) What are the coefficients in front of NO₃^-(aq)and Cu(s)when the following redox equation is balanced in an acidic solution: ________ NO₃^-(aq)+ ________ Cu(s) ________ NO(g)+ ________ Cu²⁺(aq)?

A)2,3

B)2,6

C)3,4

D)3,6

Q2) A cell based on the reaction below has a standard potential of +0.42 V at 25°C.If all of the species are at standard conditions except [H⁺],at what pH will the cell have a potential of zero? H₂O₂(aq)+ 2 H⁺(aq)+ 2 Cl^-(aq) Cl₂(aq)+ 2 H₂O(l)

A)3.55

B)7.09

C)10.6

D)14.2

Q3) If a constant current of 1.50 × 10⁸ A is passed through a molten mixture of aluminum oxide and cryolite for 4.00 hour ________ kg of aluminum can be produced.

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Page 20

Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) If the age of the Earth is 4.5 billion years and the half-life of ⁴⁰K is 1.26 billion years,what percent of the Earth's original amount of ⁴⁰K remains today?

A)4.2%

B)8.4%

C)12%

D)16%

Q2) When a substance decays by alpha radiation,the mass number of the nucleus ________ and the atomic number ________.

A)increases by 4,increases by 2

B)reduces by 4,reduces by 2

C)increases by 1,increases by 4

D)reduces by 3,reduces by 1

Q3) Relative to the amount of energy released in a typical chemical reaction,the amount of energy released in a typical fission reaction is about

A)the same.

B)1/2 times greater.

C)10⁸ times greater

D)10⁷times greater

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Page 21

Chapter 20: Transition Elements and Coordination Chemistry

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Sample Questions

Q1) Which exist as enantiomers?

A)All exist as enantiomers.

B)isomers (1)and (3)

C)isomers (2)and (4) D)None exist as enantiomers.

Q2) The coordination number of cobalt in [Co(NH₃)₄Cl₂]F is ________.

Q3) Which first row transition element has the highest melting point?

A)Sc

B)V

C)Fe

D)Zn

Q4) How many d electrons are there on the Fe metal atom in Li₃[Fe(OH)₆]?

A)1

B)3

C)5

D)6

Page 22

Q5) The element that forms a 2+ ion with the electron configuration [Xe] 4f¹⁴ 5d⁸ is ________.

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Chapter 21: Metals and Solid-State Materials

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Q1) Below the superconducting transition temperature T_c,superconductors

A)become perfect conductors.

B)become perfect magnets.

C)become perfect resistors.

D)fail to work.

Q2) Which picture corresponds to Mo?

A)picture (1)

B)picture (2)

C)picture (3)

D)picture (4)

Q3) The superconductor Tl₂Ba₂Ca₂Cu₃O₁₀ has a critical temperature T_c = 125 K.In order for each of the atoms to have a whole-number oxidation number,the oxidation numbers of Tl,Ba,Ca,Cu,and O must be ________,________,________,________,and ________,respectively.

Q4) Which picture corresponds to Zn?

A)picture (1)

B)picture (2)

C)picture (3)

D)picture (4)

Page 23

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Chapter 22: The Main-Group Elements

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Q1) What is the geometric structure of BF₃ and the hybridization of the B atom?

A)trigonal planar and sp² hybridization

B)trigonal planar and sp³ hybridization

C)pyramidal and sp hybridization

D)tetrahedral and sp² hybridization

Q2) Which one of the following is a pseudohalide?

A)CO₃^2-

B)OH^-

C)CN^-

D)SO₄^2-

Q3) What is the likely formula for the binary compound formed from the elements represented by letters B and D on the periodic table above?

A)BD

B)B₃D

C)BD₃

D)B₂D₃

Q4) The number of metallic elements in period 3 of the periodic table is ________.

Q5) Elements in group 3A of the periodic table have the valence electron configuration

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Chapter 23: Connections to Organic and Biological Chemistry

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Sample Questions

Q1) Which of the following is not a geometric (cis-trans)isomer?

A)1,1-dichloro-1-pentene

B)1,2-dichloro-1-hexene

C)2-hexene

D)2-chloro-2-heptene

Q2) How many geometrical and structural isomers are there of butene?

A)3

B)4

C)5

D)6

Q3) In leu-ala-arg-val-tyr-his-pro-gln,the amino acid with the N-terminal is A)gln.

B)val.

C)leu.

D)tyr.

Q4) What hybrid orbitals are used by carbon to form covalent bonds with hydrogen?

A)sp

B)sp²

C)sp³

D)sp³^d

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