Chemistry for Life Sciences Final Test Solutions - 4331 Verified Questions

Chemistry for Life Sciences

Final Test Solutions

Course Introduction

Chemistry for Life Sciences introduces students to fundamental chemical principles with a focus on their application in biological systems. The course covers essential topics such as atomic and molecular structure, bonding, chemical reactions, thermodynamics, acids and bases, and the structure and function of biomolecules like proteins, nucleic acids, carbohydrates, and lipids. Emphasis is placed on understanding how chemical concepts underpin processes in living organisms, providing a foundation for advanced study in biology, biochemistry, and related health sciences. Laboratory sessions reinforce theoretical knowledge through hands-on experiments relevant to life sciences.

Recommended Textbook

Chemistry 6th Edition by John E. McMurry

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23 Chapters

4331 Verified Questions

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Chapter 1: Chemistry: Matter and Measurement

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Sample Questions

Q1) The number of significant digits in 0.07090 g is ________.

Answer: four

Q2) The mass of a single copper atom is 1.055 × 10^-22 g.This is the same mass as

A)1)055 × 10^-16 mg.

B)1)055 × 10^-25 kg.

C)1)055 × 10^-28 g.

D)1)055 × 10^-31 ng.

Answer: B

Q3) Argon belongs to the ________ group of the periodic table.

A)alkali metal

B)alkaline earth

C)halogen

D)noble gas

Answer: D

Q4) Stored energy is ________ energy,and energy of motion is ________ energy.

Answer: potential,kinetic

Q5) The element that is in period 6 and group 7A has the symbol ________. Answer: At

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which of the above drawings represents a K⁺ ion?

A)drawing (a)

B)drawing (b)

C)drawing (c)

D)drawing (d)

Answer: C

Q2) What is the chemical formula for magnesium hydride?

A)MgH₂

B)MgOH

C)MgOH₂

D)Mg(OH)₂

Answer: A

Q3) In which set do all elements tend to form anions in binary ionic compounds?

A)C,S,Pb

B)K,Fe,Br

C)Li,Na,K

D)N,O,I

Answer: D

Q4) In an electron capture reaction a proton is converted into a ________.

Answer: neutron

4

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Chapter 3: Formulas, equations, and Moles

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Sample Questions

Q1) What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest whole-number coefficients? _____ C₂H₆O(l)+ _____ O₂(g) _____ CO₂(g)+ _____ H₂O(l)

A)9

B)7

C)5

D)3

Answer: D

Q2) What mass of sulfur hexafluoride,SF₆,has the same number of fluorine atoms as 25.0 g of oxygen difluoride,OF₂?

A)0)901 g

B)8)33 g

C)22.5 g

D)203 g

Answer: C

Q3) The number of grams in 0.333 mol of urea, (NH₂)₂CO,is

Answer: 20.0 g

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) According to the balanced chemical equation 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺(aq) 10 CO₂(g)+ 2 Mn²⁺(aq)+ 8 H₂O(l)

0)3500 grams of oxalic acid,H₂C₂O₄ will react with ________ mL of 0.100 M potassium permanganate,KMnO₄ solution.

A)15.5 mL

B)38.9 mL

C)77.7 mL

D)97.2 mL

Q2) Which pair of compounds is insoluble in water?

A)AgNO₃ and KNO₃

B)Na₂S and CuS

C)(NH₄)₂SO₄ and AgI

D)PbSO₄ and Pb₃(PO₄)₂

Q3) The compound K₂S is predicted to be soluble based on the solubility guideline that all ________ are soluble.

Q4) The oxidation number of hydrogen in CaH₂ is ________.

Q5) CH₃CO₂H is an example of a ________ electrolyte.

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Chapter 5: Periodicity and the Atomic Structure of Atoms

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Sample Questions

Q1) For a multielectron atom,a 3s orbital lies lower in energy than a 3p orbital because A)a 3p orbital has more nodal surfaces than a 3s orbital.

B)other electrons more effectively shield electrons in the 3s orbital from the nucleus.

C)other electrons more effectively shield electrons in the 3p orbital from the nucleus.

D)there are more p orbitals than s orbitals in a given shell.

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) The visible region of the electromagnetic radiation spectrum extends from ________ nm to ________ nm.

Q4) How many subshells are there in the shell with n = 6?

A)5

B)6

C)15

D)36

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Chapter 6: Ionic Bonds and Some Main-Group Chemistry

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Sample Questions

Q1) Atoms of which element,indicated by letter on the periodic table above,would be expected to have the highest first ionization energy,E_i1?

A)A

B)B

C)C

D)D

Q2) Which contains both covalent bonds and ionic bonds?

A)HCl

B)NaCl

C)NH₃

D)NH₄Cl

Q3) Which picture corresponds to fluorine?

A)picture (a)

B)picture (b)

C)picture (c)

D)picture (d)

Q4) The element in group 7A with the least favorable (least negative)electron affinity is

Q5) The product of the reaction of lithium with nitrogen is ________.

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Chapter 7: Covalent Bonds and Molecular Structure

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Sample Questions

Q1) What is the hybridization of the carbon atom labeled C₁?

A)sp

B)sp²

C)sp³

D)None of these

Q2) What geometric arrangement of charge clouds is expected for an atom that has five charge clouds?

A)tetrahedral

B)square planar

C)trigonal bipyramidal

D)octahedral

Q3) In the best Lewis structure for NO⁺,what is the formal charge on the N atom?

A)-1

B)0

C)+1

D)+2

Q4) Of H₂CO and CO and CO₂,the compound having the strongest C-O bond is ________.

Q5) The molecular geometry of COCl₂ is ________.

Page 9

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Chapter 8: Thermochemistry: Chemical Energy

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Sample Questions

Q1) For a process at constant pressure,49,600 calories of heat are released.This quantity of heat is equivalent to A)4)82 × 10^{- 6} J.

B)1)19 × 10⁴ J.

C)1)24 × 10⁴ J. D)2)08 × 10⁵ J.

Q2) This reaction is likely to be

A)nonspontaneous at all temperatures.

B)nonspontaneous at low temperatures and spontaneous at high temperatures. C)spontaneous at low temperatures and nonspontaneous at high temperatures. D)spontaneous at all temperatures.

Q3) When 1.0 mole of MgSO₄ is dissolved in water contained in a calorimeter,the temperature of the water and dissolved ions increases.Therefore the sign of H for this reaction is ________,heat is transferred ________ the system ________ the surroundings,and the reaction is classified as ________.

Q4) A reaction that absorbs 49.6 kJ from the surroundings in a vessel that undergoes a volume decrease of 1.25 L at a constant 4.00 atm pressure has an energy change, E = ________ kJ.

Q5) Is thermal energy a form of kinetic or potential molecular energy?

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Chapter 9: Gases: Their Properties and Behavior

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Sample Questions

Q1) A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

A)0)0680 mol

B)0)128 mol

C)0)717 mol

D)0)778 mol

Q2) Some assumptions from the kinetic molecular theory are listed below.Which one is most frequently cited to explain compressibility of a gas?

A)The average kinetic energy of gas particles is proportional to the Kelvin temperature.

B)Collisions of gas particles are elastic and total kinetic energy of the gas is constant.

C)A gas consist of tiny particles moving in random straight line motion.

D)The volume of the particles is negligible compared to the volume of the gas.

Q3) Which of the following would have a density of 1.37 g/L at 7.0°C and 0.987 atm?

A)N₂

B)O₂

C)Kr

D)Rn

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Chapter 10: Liquids,solids,and Phase Changes

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Sample Questions

Q1) The wavelength of light used to observe an object must be ________ than the object itself.

A)larger

B)smaller

C)of higher energy

D)of lower energy

Q2) The approximate normal boiling point of this substance is

A)180 K.

B)190 K.

C)300 K.

D)430 K.

Q3) The vapor pressure of liquid chloroform,CHCl₃,is 400.0 torr at 24.1°C and 100.0 torr at -6.3°C.What is H_vap of chloroform?

A)15.3 kJ/mol

B)30.1 kJ/mol

C)57.6 kJ/mol

D)86.7 kJ/mol

Q4) A certain metal can exist in two different cubic cells,body-centered cubic and face-centered cubic.Which unit cell will have the greater density?

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Chapter 11: Solutions and Their Properties

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Sample Questions

Q1) Which arrows represent H_{solute-solute} and H_{solvent-solvent}?

A)arrow (a)and arrow (b)

B)arrow (a)and arrow (c)

C)arrow (a)and arrow (d)

D)arrow (c)and arrow (d)

Q2) An aqueous solution has a normal boiling point of 102.0°C.What is the freezing point of this solution? For water K_b is 0.51°C/m and K_f = 1.86°C/m.

A)-0.55°C

B)-2.0°C

C)-3.6°C

D)-7.3°C

Q3) A solution of LiCl in water has X_LiCl = 0.0 900.What is the molality?

A)4)46 m LiCl

B)5)00 m LiCl

C)5)49 m LiCl

D)9)89 m LiCl

Q4) The volume of 0.200 M H₂SO₄ that contains 5.00 mmol of H⁺ is ________ mL.

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Chapter 12: Chemical Kinetics

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Sample Questions

Q1) The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]².The order of reaction with respect to H⁺ is ________ and the overall order is

BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq) 3 Br₂(aq)+ 3 H₂O(l)

Q2) What is the time required to achieve the molecular mixture in drawing (d)?

A)4 min

B)5 min

C)7 min

D)8 min

Q3) The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

A)H₂,homogeneous

B)N₂,homogeneous

C)NH₃,homogeneous

D)metal surface,heterogeneous

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Chapter 13: Chemical Equilibrium

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Sample Questions

Q1) The reaction CaCO₃(s) CaO(s)+ O₂(g)is endothermic 298

K.The effect of adding additional CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaCO₃ once equilibrium is reestablished.

Q2) A crude type of disappearing ink is based on the following endothermic equilibrium: [Co(H₂O)₆]Cl₂ (aq) [CoCl₂(H₂O)₄] (aq)+ 2 H₂O (l) (colorless)(blue)

If the reactant solution is used to write on a piece of paper and the paper is allowed to partially dry,what can be done to bring out the colored handwriting?

A)add water

B)decrease the volume

C)put the paper in a freezer

D)put the paper in an oven

Q3) In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

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Chapter 14: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Vinegar is a 5.0% solution by weight of acetic acid (CH₃CO₂H)in water.Given that the pH for acetic acid is 2.41,the K_a = 1.8 × 10^-5 and assuming the density of vinegar to be 1.00 g/cm³,what is the percent dissociation of acetic acid in vinegar?

A)0)47%

B)1)5%

C)4)0%

D)5)0%

Q2) Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH₃ (K_b= 1.8 × 10^-5)is

NH₃(aq)+ H₂O(l) NH₄⁺(aq)+ OH^-(aq).

A)3)0 M

B)0)056 M

C)1)8 × 10^{- 2} M

D)1)0 × 10^-3 M

Q3) The pH of a 0.025 M KOH solution is ________.

Q4) A 0.10 M KNO₂ solution will have a pH ________ seven.

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Chapter 15: Applications of Aqueous Equilibria

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Sample Questions

Q1) Which solution has the highest pH?

A)(1)

B)(2)

C)(3)

D)(4)

Q2) Which point a-d represents pK_a2?

A)point a

B)point b

C)point c

D)point d

Q3) Which picture represents the solution before the equivalence point?

A)(1)

B)(2)

C)(3)

D)(4)

Q4) What is the pH at the equivalence point of a weak acid-strong base titration?

A)pH < 7

B)pH = 7

C)pH > 7

D)pH = 14.00

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Chapter 16: Thermodynamics: Entropy, free Energy, and Equilibrium

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Sample Questions

Q1) The sign (+ or -)of H is ________ and the sign (+ or -)of S is ________ for the evaporation of water.

Q2) Solid NaHCO₃ is heated to 90°C.At equilibrium the total pressure of the gases produced is 0.545 atm.Calculate G° at 90°C for the reaction 2 NaHCO₃(s) Na₂CO₃(s)+ H₂O(g)+ CO₂(g).

A)-7.85 kJ

B)-3.67 kJ

C)+3.67 kJ

D)+7.85 kJ

Q3) An electron in an oxygen p orbital on which of the following would have the highest entropy?

A)CH₃CH₂OH

B)CH₃CH₂O^-

C)CH₃CO₂OH

D)CH₃CO₂^-

Q4) What is the entropy of 10 molecules in a system of 1000 boxes?

Q5) The entropy of water at 25° is ________ than the entropy of water at 35°C.

Q6) What is the entropy of 10 molecules in a system of 100 boxes?

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Chapter 17: Electrochemistry

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Sample Questions

Q1) Which requires the most electricity (in terms of faradays of charge transferred)per gram of useful product formed?

A)electrolysis of aqueous NaCl (chlor-alkali industry)

B)electrolysis of molten NaCl/CaCl₂ in a Downs cell

C)electrorefining copper metal

D)production of aluminum in the Hall-Heroult process

Q2) Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid,H₂CrO₄.What current is required to deposit chromium at a rate of 1.25 g/min?

A)38.1 A

B)38.7 A

C)116 A

D)232 A

Q3) Which is most often used in the laboratory to measure pH?

A)a standard hydrogen electrode

B)a glass electrode

C)a Daniell cell

D)a conductivity cell

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Chapter 18: Hydrogen, oxygen, and Water

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Sample Questions

Q1) What is not a commercial method for the preparation of hydrogen gas?

A)H₂O(g)+ CH₄(g) CO(g)+ 3 H₂(g)

B)2 H₂O(l) 2 H₂(g)+ O₂(g)

C)H₂O(g)+ C(s) CO(g)+ H₂(g)

D)4 H₂O(g)+ 3 Fe Fe₃O₄(s)+ 4 H₂(g)

Q2) What is not a characteristic of ozone,O₃?

A)It is a nonlinear triatomic system.

B)It has one single bond and one double bond.

C)It is an extremely powerful oxidizing agent.

D)It is made by passing an electrical discharge through oxygen.

Q3) What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?

2 H₂O(l) 2 H₂(g)+ O₂(g)

A)74.7 L

B)149 L

C)224 L

D)447 L

Q4) An element that forms a basic oxide tends to form a hydride that is ________ (covalent,ionic).

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Chapter 19: The Main-Group Elements

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Sample Questions

Q1) Which one of the following elements forms the most acidic binary oxide?

A)Na

B)C

C)N

D)P

Q2) The most acidic oxides of the group 5A elements are oxides of the element

Q3) Among the main-group elements the number of semimetals is ________.

A)five

B)six

C)seven

D)eight

Q4) What statement is inconsistent about carbon monoxide?

A)It is a colorless,odorless and toxic gas.

B)It is formed by burning carbon or hydrocarbon in excess oxygen.

C)One of its main industrial uses is in the synthesis of methanol,CH₃OH.

D)Toxicity of CO results from its ability to bond strongly to iron(II)atom in hemoglobin.

Q5) The fullerene C₆₀ is an ________ (allotrope,isotope,isomer)of carbon.

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Chapter 20: Transition Elements and Coordination Chemistry

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Sample Questions

Q1) Based on the variation in Z_eff,which oxoanion should be the strongest oxidizing agent?

A)VO₄^3-

B)CrO₄^2-

C)MnO₄^2-

D)FeO₄^2-

Q2) What hybridization scheme is used for Ni in the square planar complex of [Ni(CN)₄]^2-?

A)sp³

B)dsp²

C)dsp³

D)d²^sp³

Q3) Which of the following complexes has five unpaired electrons?

A)[Mn(H₂O)₆]²⁺

B)[Mn(CN)₆]^3-

C)CrCl₃(H₂O)₃

D)[Ag(NH₃)₂]⁺

Q4) The number of unpaired electrons in square planar PtCl₄^2- is ________.

Q5) The formula for tetraamminedichlorochromium(III)chloride is ________.

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Chapter

21: Metals and Solid-State Materials

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Q1) What is not part of the sol-gel process for the production of titania?

A)TiCl₄ + 4 HOCH₂CH₃ + 4 NH₃ Ti(OCH₂CH₃)₄ + 4 NH₄Cl (in benzene) B)Ti(OCH₂CH₃)₄ + 4 H₂O Ti(OH)₄ + 4 HOCH₂CH₃ C)(HO)₃-Ti-OH + HO-Ti-(OH)₃ (HO)₃-Ti-O-Ti(OH)₃ + H₂O D)4 Ti(OH)₄ + heat 2 Ti₂O₃ + 8 H₂O + O₂

Q2) What structural features appear necessary for superconductivity in the 1-2-3 YBa₂Cu₃O₇ superconductor?

A)high metallic character

B)infinite extended layers of Cu and O atoms and a fractional oxidation state for Cu C)presence of an inner transition element

D)All of these are necessary.

Q3) The balanced chemical equation for the production of silver by roasting of its sulfide is ________.

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23

Chapter 22: Nuclear Chemistry

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Q1) Which type of radiation source would pose the greatest health risk when used internally for a medical procedure?

A)an alpha emitter,t_1/2 = 6 hours

B)a beta emitter,t_1/2 = 6 hours

C)a beta emitter,t_1/2 = 15 days

D)a gamma emitter,t_1/2 = 6 hours

Q2) How much energy is released for alpha decay of ²³⁶U? The masses of ⁴He,²³²Th,and ²³⁶U are 4.002604,232.038124,and 236.045637 amu,respectively.

A)1)473 × 10⁸ kJ/mol

B)4)418 × 10⁸ kJ/mol

C)4)909 × 10⁸ kJ/mol

D)7)209 × 10⁸ kJ/mol

Q3) The mass defect for the formation of lithium-6 is 0.0343 g/mol.The binding energy for lithium-6 nuclei is ________ kJ/mol.

Q4) Among the types of radiation, , , ,and X,the one that requires the least amount of protective clothing is ________ radiation.

Q5) The mass defect for the chemical reaction shown below is ________ g.

2 F F₂ E = -159 kJ/mol

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Chapter 23: Organic and Biological Chemistry

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Sample Questions

Q1) Which compound will have the largest dipole moment?

A)cis-1,2-dichloroethylene

B)trans-1,2-dichloroethylene

C)tetrabromoethylene

D)tetrachloroethylene

Q2) Which compound is a saturated hydrocarbon?

A)benzene

B)cyclohexene

C)2-methylpentane

D)propylene

Q3) Which of the following compounds is most soluble in water?

A)decanol

B)dimethyl ether

C)ethane

D)ethanol

Q4) What is the common name for the simplest ketone,propanone?

A)acetal

B)acetone

C)carbanone

D)formalin

Page 25

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