Chemistry for Life Sciences Test Preparation - 986 Verified Questions

Chemistry for Life Sciences

Test Preparation

Course Introduction

Chemistry for Life Sciences introduces students to the fundamental principles of chemistry with a focus on their applications in biological systems. The course covers atomic structure, chemical bonding, thermodynamics, acids and bases, and chemical reactions, emphasizing concepts essential for understanding molecular interactions in living organisms. Students will explore topics such as biomolecules, metabolism, and the chemical basis of physiological processes, equipping them with the chemical literacy necessary for advanced studies in biological and health sciences. Laboratory sessions reinforce theoretical knowledge through hands-on experiments designed to develop practical skills and an appreciation of the role of chemistry in life sciences.

Recommended Textbook

Introductory Chemistry An Active Learning Approach 6th Edition by Mark S. Cracolice

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21 Chapters

986 Verified Questions

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Chapter 2: Matter and Energy

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Sample Questions

Q1) What type of pure substance can be decomposed chemically into other pure substances?

A)A compound

B)An element

C)A mixture

D)A solution

E)Heterogeneous matter

Answer: A

Q2) Which of the following correctly describes a homogeneous sample?

A)Uniform appearance and composition throughout

B)Visibly different parts or phases

C)A mixture of diamond and graphite, which are both forms of carbon

D)Reacts with all elements

E)Reacts with all natural elements

Answer: A

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Chapter 3: Measurement and Chemical Calculations

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Sample Questions

Q1) Convert 3.77 × 10⁸ pL to mL,daL,and dL.1 pL = 10^-12 L,1 dL = 10^-1 L,1 daL = 10¹ L

A)3.77 × 10²³ mL, 3.77 × 10¹⁹ daL, 3.77 × 10²¹ dL

B)3.77 × 10¹⁷ mL, 3.77 × 10²¹ daL, 3.77 × 10¹⁹ dL

C)3.77 × 10^-1 mL, 3.77 × 10^-5 daL, 3.77 × 10^-3 dL

D)3.77 × 10^-4 mL, 3.77 × 10^-5 daL, 3.77 × 10^-3 dL

E)3.77 × 10^-7 mL, 3.77 × 10^-3 daL, 3.77 × 10^-5 dL

Answer: C

Q2) Convert 1.57 g to kg,cg,and mg.

A)1570 kg, 0.0157 cg, 0.00157 mg

B)0.00157 kg, 0.0157 cg, 1570 mg

C)0.00157 kg, 157 cg, 1570 mg

D)157 kg, 1570 cg, 0.00157 mg

E)1570 kg, 0.00157 cg, 157 mg

Answer: C

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4

Chapter 4: Introduction to Gases

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Sample Questions

Q1) 4.27 L of a gas are collected at 53 °C and 527 torr.What would this volume be if adjusted to STP?

A)0 L

B)7.35 L

C)5.16 L

D)3.54 L

E)2.48 L

Q2) A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m³ at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m³?

A)0.00145 torr

B)0.00127 torr

C)781 torr

D)563 torr

E)688 torr

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Chapter 5: Atomic Theory: The Nuclear Model of the Atom

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Sample Questions

Q1) Which of the following statements is false?

A)Atoms of the same element that have different masses are called isotopes

B)The masses of isotopes vary because they have different numbers of electrons

C)The mass number of an isotope is the total number of protons and neutrons in the nucleus

D)You can find the mass number of an atom given the number of protons and neutrons, but without being given the number of electrons

E)Every atom of a particular element has the same number of protons

Q2) Which of the following is not a description of atoms according to Dalton's atomic theory?

A)Atoms cannot be destroyed or created

B)Atoms of different elements may combine in the ratio of small, whole numbers to form compounds

C)Atoms of the same element that have different masses are called isotopes

D)All atoms of one element have the same mass

E)Atoms of two different elements have different masses

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Chapter 6: Chemical Nomenclature

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Sample Questions

Q1) What is the name of Fe(NO₃)₃ 9 H₂O?

A)Iron(III) nitrate ninhydrate

B)Iron(III) nitrate nonahydrate

C)Iron(III) nitrate heptahydrate

D)Iron(III) nitrite nonahydrate

E)Iron(III) nitrite heptahydrate

Q2) Which of the following formula-name pairs is/are correct?

i.GaCl₂,gallium chloride (gallium,Z = 31)

ii.HS,hydrosulfuric acid

iii.Pb(NO₂)₂,lead(II)nitrate

iv.NaClO₂,sodium chlorate

v.K₃PO₄,potassium phosphate

A)all are correct

B)i, iii, and v

C)v only

D)i, ii, iii, and iv

E)none is correct

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Page 7

Chapter 7: Chemical Formula Relationships

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Sample Questions

Q1) What is the empirical formula of a compound that contains 80.0% carbon and 20.0% hydrogen by mass?

A)CH₃

B)CH₂

C)CH

D)C₃H

E)C₂H₃

Q2) Which of the following statements is/are incorrect?

A)One mole is that amount of any substance that contains the same number of units as the number of atoms in exactly 12 grams of carbon-12

B)To three significant figures, there are 6.02 × 10²³ units per mole

C)The number of particles in a mole is called Avogadro's number

D)The mass of 1/12 mole of carbon-12 is 1 gram

E)The mole is a fundamental constant derived from the laws of nature

Q3) Calculate the number of atoms in 0.377 grams of Ar.

A)1.57 × 10^-26

B)2.50 × 10^-23

C)5.67 × 10²¹

D)9.08 × 10²⁴

E)9.42 × 10^-3

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Chapter 8: Chemical Reactions

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Sample Questions

Q1) Bromine is added to a solution of sodium iodide.Write the balanced chemical equation for this reaction.What is the sum of the coefficients?

A)4 or less

B)5

C)6

D)7

E)8 or more

Q2) Calcium combines with bromine to make calcium bromide.Write the balanced chemical equation for this reaction.What is the coefficient for bromine?

A)1

B)2

C)3

D)4

E)5

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Chapter 9: Chemical Change

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Sample Questions

Q1) Write the net ionic equation for the reaction that occurs,if any,when solutions of silver chlorate and sodium sulfide are combined.What are the reactants (with appropriate coefficients)?

A)Na⁺(aq) + Cl^-(aq)

B)Na⁺(aq) + ClO₃^-(aq)

C)Ag²⁺(aq) + S^2-(aq)

D)2 Ag⁺(aq) + SO₄^2-(aq)

E)2 Ag⁺(aq) + S^2-(aq)

Q2) What are the formulas of the major species present in a mixture of HNO₃ and HF in water?

A)HNO₃(aq) + HF(aq)

B)HNO₃(aq) + H⁺(aq) + F^-(aq)

C)H⁺(aq) + NO₃(aq) + F^-(aq)

D)H⁺(aq) + NO₃^-(aq) + HF(aq)

E)H₂(g) + NO₃^-(aq) + F⁺(aq)

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Chapter 10: Quantity Relationships in Chemical Reactions

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Sample Questions

Q1) A chemist combines hydrochloric acid with a sodium hydroxide solution,transferring 5.75 kJ of heat.Express this in calories.

A)2.41 × 10^-2 cal

B)2.41 × 10¹ cal

C)2.41 × 10⁴ cal

D)1.37 × 10^-3 cal

E)1.37 × 10³ cal

Q2) The decomposition of potassium chlorate is written as shown below.What energy change occurs when 12.3 g of KClO₃ decompose?

2 KClO₃(s)+ 89.6 kJ 2 KCl(s)+ 3 O₂(g)

A)Release of 8.99 kJ

B)Absorption of 8.99 kJ

C)Release of 4.49 kJ

D)Absorption of 4.49 kJ

E)Release of 0.00112 kJ

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11

Chapter 11: Atomic Theory: The Quantum Model of the Atom

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Sample Questions

Q1) Which of the following statements is/are incorrect?

i.The Bohr model successfully predicts energies in the ultraviolet portion of the hydrogen spectrum

ii.The Bohr model successfully predicts energies in the infrared portions of the sodium spectrum

iii.The Bohr model associates electron energy with the radius at which an electron orbits the nucleus

iv.The Bohr model does not explain the failure of an electron to lose energy as it travels a circular path around a nucleus

A)i only

B)ii only

C)iii only

D)iv only

E)iii and iv

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12

Chapter 12: Chemical Bonding

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Sample Questions

Q1) In a covalent bond,the valence electrons from atoms are:

A)shared

B)transferred to the less metallic element

C)transferred to the more metallic element

D)gained by the anion

E)gained by the cation

Q2) In deciding whether a bond is polar or nonpolar,what has to be considered?

A)The electromagnetic field surrounding the molecule

B)Whether a magnet will attract the bonded atoms

C)The electronegativity difference between the atoms

D)The number of lone pairs

E)The number of bonds between the two atoms

Q3) Which of the following is the best classification for a bond in which bonding electrons are shared unequally?

A)Nonpolar covalent

B)Polar covalent

C)Electronegative

D)Multiple

E)Completely ionic

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Page 13

Chapter 13: Structure and Shape

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Sample Questions

Q1) Which of the following molecules is/are nonpolar?

i.NH₃

ii.H₂O

iii.HCl

iv.CH₄

v.CH₂Cl₂

A)i only

B)iv only

C)iv and v

D)i, ii, and iii

E)i, ii, iii, iv, and v

Q2) What is the electron pair geometry surrounding the boron atom in BH₃?

A)Trigonal planar

B)Linear

C)Angular (Bent)

D)Trigonal pyramid

E)Tetrahedral

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Chapter 14: The Ideal Gas Law and Its Applications

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Sample Questions

Q1) What is the molar volume of CO₂ at 39°C and 652 torr?

A)0.0335 L/mol

B)0.0393 L/mol

C)3.73 L/mol

D)29.9 L/mol

E)1.32 × 10³ L/mol

Q2) If 26.0 liters of methane,CH₄,measured at 1.09 atm and 23.0? 0°C,are converted to acetylene,C₂H₂,what volume of acetylene,measured at 0.941 atm and 185?

0°C,will result?

2 CH₄ C₂H₂ + 3 H₂

A)9.73 L

B)17.4 L

C)23.3 L

D)93.2 L

E)0.0429 L

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Chapter 15: Gases, Liquids, and Solids

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Sample Questions

Q1) Acetone,a highly volatile liquid,is placed in a closed container.The amount of liquid decreases,but eventually becomes stable.The volume of the closed space above the liquid is increased.The amount of liquid then...

A)May or may not change, but no prediction can be made without additional information about temperature

B)May or may not change, but no prediction can be made without additional information about the magnitude of the volume increase

C)Remains the same

D)Increases

E)Decreases

Q2) The specific heat of solid gold is 0.13 J/g °C.How much heat is needed to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C?

A)3.5 kJ

B)3.4 kJ

C)0.14 kJ

D)2.0 × 10³ kJ

E)3.3 kJ

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Chapter 16: Solutions

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Sample Questions

Q1) Potassium hydrogen phthalate is used as a primary standard in finding the concentration of a solution of sodium hydroxide by the reaction KHC₈H₄O₄ + NaOH NaKC₈H₄O₄ + H₂O.What is the molarity of the base if 32.75 mL is required to titrate 1.732 g of the primary standard?

A)0.5189 M

B)0.2590 M

C)1.732 M

D)3.861 M

E)3.275 M

Q2) An unknown substance is known to be a nonelectrolyte,and it dissolves in water.Determine the approximate molar mass of the substance if 37.7 g of the substance dissolved in 1.00 × 10² mL of water has a boiling temperature of 102.73°C.K_b for water is 0.52°C/m.

A)5.3 g/mol

B)1.4 g/mol

C)2.0 × 10² g/mol

D)3.8 × 10² g/mol

E)72 g/mol

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Chapter 17: Acidbase Proton Transferreactions

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Sample Questions

Q1) In Brønsted-Lowry acid-base reactions,which of the following species are favored at equilibrium?

A)The weaker acid and the weaker base

B)The weaker acid and the stronger base

C)The stronger acid and the weaker base

D)The stronger acid and the stronger base

E)At equilibrium, neither side is favored

Q2) A solution has a hydroxide ion concentration of 1 × 10^-11 M.What is the pH of the solution,and is it acidic or basic?

A)pH = 11, basic

B)pH = 3, basic

C)pH = 3, acidic

D)pH = -11 acidic

E)pH = -11, basic

Q3) The pH of a solution is 5.330.Find [OH^-].

A)[OH^-] = 2.14 × 10^-9 molar

B)[OH^-] = 4.70 × 10^-11 molar

C)[OH^-] = 5.33 × 10^-7 molar

D)[OH^-] = 4.70 × 10^-6 molar

E)[OH^-] = 5.33 molar

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Chapter 18: Chemical Equilibrium

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Sample Questions

Q1) Which of the following statements are incorrect?

i.When opposing reversible reactions occur at different rates,the faster reaction gradually becomes slower.ii.Equilibrium is established when forward and reverse reaction rates become equal

iii.In the development of a chemical equilibrium,the reverse reaction rate decreases over time until equilibrium is established

A)iii only

B)i and ii

C)i and iii

D)ii and iii

E)i, ii, and iii

Q2) What kind of molecular collisions will not lead to the formation of product in a reaction?

A)Only those without sufficient kinetic energy

B)Only those with the wrong orientation, regardless of the kinetic energy

C)Collisions between molecules that have more energy than the minimum required

D)Those without sufficient kinetic energy and with the wrong orientation

E)Those with effective collisions

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Chapter 19: Oxidationreduction Electron Transferreactions

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Sample Questions

Q1) Which of the following substances is most likely to be a reducing agent?

A)NH₄⁺

B)S^2-

C)Mg²⁺

D)KMnO₄

E)Cl₂

Q2) Silver metal will not react with hydrochloric acid.What does this suggest about silver and hydrochloric acid?

A)HCl is a weak acid

B)HCl is a strong acid

C)Ag is a weaker reducing agent than H⁺ in HCl(aq)

D)Ag is a stronger oxidizing agent than HCl

E)No conclusion can be made based on this information

Q3) Which of the following processes is a reduction reaction?

A)2 Br^- becoming Br₂

B)Ni²⁺ becoming Ni³⁺

C)Hg₂²⁺ becoming 2 Hg

D)Tin(II) becoming tin(IV)

E)Iron(II) becoming iron(III)

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Page 20

Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) Consider the following description of an instrument used to detect radioactivity: A tube contains argon at low pressure.A high electrical potential is established between a positively charged wire in the center and the negatively charged case.Radiation enters the window and ionizes the argon.The ions move toward the electrodes,producing a measurable electrical pulse and an audible "click." What is the name of this instrument?

A)Gamma camera and scanner

B)Scintillation counter

C)Geiger counter

D)Cloud chamber

E)Spectrophotometer

Q2) Which of the following correctly matches the three principal forms of radioactive emission with their respective electrical charges?

A) has no charge, is -, is +

B) is -, has no charge, is +

C) is -, is +, has no charge

D) is +, has no charge, is -

E) is +, is -, has no charge

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Chapter 21: Organic Chemistry

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Sample Questions

Q1) Which of the following compounds is/are (a)ketone(s)?

i.CH₃-OH

ii.CH₃-CO-CH₃

iii.CH₃-O-CH₃

iv.CH₃-CHO

v.CH₃-COO-CH₃

A)ii only

B)ii, iii, and v

C)ii, iii, iv, and v

D)i, ii, iii, and iv

E)All are ketones

Q2) What is the product of the hydrogenation of trans-2-pentene?

A)isopentane

B)neopentane

C)cis-2-pentane

D)trans-2-pentane

E)n-pentane

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Chapter 22: Biochemistry

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Sample Questions

Q1) Which of the following is the best definition of the term lipid?

A)A molecule made of two or more simpler sugar molecules

B)A substance that is found in living organisms and is insoluble in water but soluble in nonpolar solvents

C)A nucleic acid monomer

D)A small molecule characterized by a carboxyl group at one end of the carbon chain and an amine group on the carbon next to the carboxyl group

E)A catalyst that controls chemical reactions in a living system

Q2) Which of the following are the two types of nucleic acids in all living systems?

i.Deoxyribonucleic acid

ii.Gluconucleic acid

iii.Ribonucleic acid

iv.Fructonucleic acid

A)i and ii

B)i and iii

C)i and iv

D)ii and iii

E)ii and iv

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