Survey of Chemistry Test Bank - 4331 Verified Questions

Survey of Chemistry Test Bank

Course Introduction

Survey of Chemistry is an introductory course designed to provide students with a broad overview of fundamental chemical concepts and their real-world applications. The course covers essential topics such as atomic structure, chemical bonding, states of matter, chemical reactions, stoichiometry, solutions, acids and bases, and basic organic and biochemistry principles. Emphasis is placed on developing problem-solving skills, understanding scientific reasoning, and appreciating the role of chemistry in everyday life, health, and the environment. This course is suitable for non-science majors and those seeking a foundational understanding of chemistry.

Recommended Textbook Chemistry 6th Edition by John E. McMurry

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23 Chapters

4331 Verified Questions

4331 Flashcards

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Chapter 1: Chemistry: Matter and Measurement

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219 Verified Questions

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Sample Questions

Q1) The fundamental SI unit of mass is the A)centigram.

B)gram. C)kilogram.

D)milligram.

Answer: C

Q2) The symbol for mercury is ________. Answer: Hg

Q3) The density of aluminum is 2.702 g/cm³.What is the final liquid level of water if 1.130 ounces of aluminum is dropped into a graduated cylinder containing 15.90 mL of water?

A)17.08 mL

B)21.66 mL

C)27.76 mL

D)47.95 mL

Answer: C

Q4) Pb is the symbol for the element ________. Answer: lead

Q5) In a periodic table rows are called ________ and columns are called ________.

Answer: periods,groups

3

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) What is the chemical formula for magnesium hydride?

A)MgH₂

B)MgOH

C)MgOH₂

D)Mg(OH)₂

Answer: A

Q2) What is the chemical formula for iron(II)phosphate?

A)Fe₂P

B)Fe₂PO₄

C)Fe₃P₂

D)Fe₃(PO₄)₂

Answer: D

Q3) Beta decay of ²⁴Na produces a beta particle and

A)(²⁰F.)

B)(²³Na.)

C)(²⁴Ne.)

D)(²⁴Mg.)

Answer: D

Q4) The symbol of the isotope having Z = 88 and A = 226 is ________.

Answer: 11ea7a38_c8cd_82a1_aa4c_f511e3c2a7ee_TB4939_11

Page 4

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Chapter 3: Formulas, equations, and Moles

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Sample Questions

Q1) How many chloride ions are in 1.50 mol of aluminum chloride?

A)3)00 chloride ions

B)4)50 chloride ions

C)9)03 × 10²³ chloride ions

D)2)71 × 10²⁴ chloride ions

Answer: D

Q2) What is the molar mass of hydrogen gas?

A)1)00 g/mol

B)2)00 g/mol

C)6)02 × 10²³ g/mol

D)1)20 × 10²³ g/mol

Answer: B

Q3) When iron(III)oxide reacts with hydrochloric acid,iron(III)chloride and water are formed.How many grams of iron(III)chloride are formed from 10.0 g of iron(III)oxide and 10.0 g of hydrochloric acid?

A)11.1 g

B)14.8 g

C)20.3 g

D)35.1 g

Answer: B

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent?

C₂O₄2- (aq)+ MnO₄^-(aq) CO₂(aq)+ Mn²⁺(aq)

A)1

B)2

C)5

D)10

Q2) When Na₂CrO₄(aq)and AgNO₃(aq)are mixed,a red colored precipitate forms which is A)Ag.

B)Ag₂CrO₄.

C)AgNO₂.

D)NaNO₃.

Q3) Which of the following compounds is an Arrhenius base in water?

A)C₆H₁₂O₆

B)HOClO₂

C)H₂SO₄

D)NH₃

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Chapter 5: Periodicity and the Atomic Structure of Atoms

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Sample Questions

Q1) Middle C on a piano has a frequency of 262 Hz.In a vacuum 262 Hz has a corresponding wavelength of ________ m.

Q2) Of the following,which atom has the smallest atomic radius?

A)Mg

B)S

C)Sr

D)Te

Q3) The amount of data that can be stored in an optical disc storage medium is related to the wavelength of the laser employed.Blu-Ray discs that are read by a laser having a wavelength of 405 nm have a much greater storage capacity than a DVD that is read by a 650 nm laser.The color of the 405 nm laser beam is ________,whereas the color of the 650 nm laser is ________.

Q4) According to the Balmer-Rydberg equation,electromagnetic radiation with wavelength = 486.1 nm will be absorbed when an electron undergoes which of the following transitions?

A)m = 2 n = 3

B)m = 2 n = 4

C)n = 3 m = 2

D)n = 4 m = 2

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Chapter 6: Ionic Bonds and Some Main-Group Chemistry

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Sample Questions

Q1) The element in period 3 with the smallest seventh ionization energy is ________.

Q2) Most of the compounds of the 2+ ions of the first row of the transition metals from Mn to Zn are colored due to absorption of visible light promoting an electron from one 3d orbital to another.Which of these ions should tend to form colorless compounds?

A)Mn²⁺

B)Co²⁺

C)Cu²⁺

D)Zn²⁺

Q3) Of the following,which element has the highest first ionization energy?

A)Al

B)Cl

C)Na

D)P

Q4) Predict the product(s)when the reactants Be(s)+ Br₂(l)are mixed.

A)BeBr(s)

B)BeBr₂(s)

C)Be₂Br(s)

D)BeBr₃(s)

Q5) Potassium reacts with oxygen to form a superoxide with the formula ________.

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Chapter 7: Covalent Bonds and Molecular Structure

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Sample Questions

Q1) According to molecular orbital theory,is the highest energy orbital that contains an electron antibonding or bonding in O₂^2-?

Q2) How many lone pairs of electrons are on the P atom in PF₃?

A)0

B)1

C)2

D)3

Q3) Element A has an electronegativity of 0.8 and element B has an electronegativity of 3.0.Which statement best describes the bonding in A₃B?

A)The AB bond is largely covalent with a - on A.

B)The AB bond is largely covalent with a + on A.

C)The compound is largely ionic with A as the cation.

D)The compound is largely ionic with A as the anion.

Q4) Using only the elements Ba,F,and P,give the formula of a compound having largely polar covalent bonds.

Q5) When an electron is added to the lowest unoccupied molecular orbital of N₂,the electron is added to a(n)________ (antibonding,bonding)molecular orbital and the N-N bond order will ________ (decrease,increase).

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Chapter 8: Thermochemistry: Chemical Energy

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Sample Questions

Q1) Which of the following is not a type of energy or energy transfer?

A)chemical energy

B)heat

C)temperature

D)work

Q2) When 50.0 mL of 0.400 M Ca(NO₃)₂ is added to 50.0 mL of 0.800 M NaF,CaF₂ precipitates,as shown in the net ionic equation below.The initial temperature of both solutions is 25.00°C.Assuming that the reaction goes to completion,and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g °C),calculate the final temperature of the solution. Ca²⁺(aq)+ 2 F^-(aq) CaF₂(s) H° = -11.5 kJ

A)24.45°C

B)25.55°C

C)26.10°C

D)26.65°C

Q3) Kinetic energy increases with increasing ________ and increasing ________.

Q4) Is thermal energy a form of kinetic or potential molecular energy?

Q5) The SI unit for energy is the ________.

Q6) ________ energy is the kinetic energy of molecular motion.

Page 10

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Chapter 9: Gases: Their Properties and Behavior

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Sample Questions

Q1) If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg,the level of mercury in the tube will

A)be 118 mm higher in the arm open to the atmosphere.

B)be 118 mm higher in the arm connected to the gas cylinder.

C)be 870 mm higher in the arm open to the atmosphere.

D)be 870 mm higher in the arm connected to the gas cylinder.

Q2) Which one of the following gases will have the highest rate of effusion?

A)NO₂

B)N₂O

C)N₂O₄

D)NO₃

Q3) If the total pressure in the container is 900 mm Hg,what is the partial pressure of chlorine?

A)90 mm Hg

B)180 mm Hg

C)270 mm Hg

D)450 mm Hg

Q4) The molecule believed to be most responsible for global warming is ________.

Q5) When using the ideal gas law the temperature must be expressed in ________.

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Chapter 10: Liquids,solids,and Phase Changes

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Sample Questions

Q1) How many cations M are in the unit cell?

A)1

B)2

C)4

D)8

Q2) Melting occurs along the A)AC line.

B)CB line.

C)CD line.

D)All of these

Q3) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

A)N₂

B)HBr

C)CO₂

D)H₂O

Q4) Helium can be liquefied when He atoms are attracted to one another by intermolecular ________ forces.

Q5) In the molecule BF₃ there is a + charge on the ________ atom and acharge on the ________ atom.

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Chapter 11: Solutions and Their Properties

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Sample Questions

Q1) A solution is prepared by dissolving 17.75 g sulfuric acid,H₂SO₄,in enough water to make 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the mole fraction H₂SO₄ in the solution?

A)0)0181

B)0)0338

C)0)0350

D)19.0

Q2) Assume that the vapor at point c is condensed and reboiled.What is the vapor composition during reboiling?

A)100% decane

B)composition at point b

C)composition at point c

D)composition at point e

Q3) When two similar liquids mix to form a solution,the entropy of solution ( S_soln)is expected to be

A)negative.

B)zero.

C)positive.

D)negative at low temperatures but positive at high temperatures.

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Chapter 12: 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) What is the order of reaction with respect to A₂?

A)0

B)1

C)2

D)3

Q3) The reaction below is first order in H₂ and second order in NO.What is the rate law for this reaction?

2 H₂(g)+ 2 NO(g) N₂(g)+ 2 H₂O(g)

A)Rate = 2k[H₂][NO]

B)Rate = k[H₂][NO]²

C)Rate = k[H₂]²[NO]²

D)Rate = 2k[H₂]²[NO]²

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Page 14

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) For the reaction shown below the value of K_p is ________ than the value of K_c,because n = ________.

N₂O₄(g) 2 NO₂(g)

Q3) Which of the following changes in reaction conditions will alter the composition of an equilibrium mixture of gases for a reaction having unequal moles of gaseous products and gaseous reactants?

A)addition of reactants or products

B)decreasing the pressure or volume

C)increasing the temperature

D)All of these will alter the equilibrium concentrations.

Q4) Which equilibrium below is homogeneous?

A)BaSO₄(s) Ba²⁺(aq)+ SO₄^2-(aq)

B)2 H₂O₂(l) 2 H₂O(l)+ O₂(g)

C)NH₄NO₃(s) N₂O(g)+ 2 H₂O(g)

D)2 CO(g)+ O₂(g) 2 CO₂(g)

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Chapter 14: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Which one of the following salts,when dissolved in water,produces the solution with a pH closest to 7.00?

A)NH₄Cl

B)BaO

C)NaHSO₄

D)RbI

Q2) Using the conjugate acid-base pairs listed below,complete the following equation with the pair that gives an equilibrium constant K_c > 1.

_____ + HSO₃^- _____ + H₂SO₃

A)CH₃CO₂H/ CH₃CO₂^-

B)HCO₂H/ HCO₂^-

C)HNO₂/NO₂^-

D)HNO₃/NO₃^-

Q3) If an equal number of moles of the weak acid HCN and the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

A)acidic

B)basic

C)neutral

D)There is insufficient information provided to answer this question.

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Chapter 15: Applications of Aqueous Equilibria

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Sample Questions

Q1) Which solution has the lowest pH?

A)(1)

B)(2)

C)(3)

D)(4)

Q2) A solution may contain the following ions

Ag⁺,Cu²⁺,Mn²⁺,Ca²⁺,and Na⁺.No precipitate formed when 0.10 M NaCl was added but a dark colored precipitate formed when H₂S was added to an acidic portion of the solution.After the removal of the solid the solution was made basic and more H₂S was added and a dark precipitate again formed.Treatment of the filtrate with (NH₄)₂CO₃ resulted in a white precipitate.If no further tests were made then what conclusions can you draw?

A)possible ions present Cu²⁺,Mn²⁺,Na⁺ B)possible ions present Cu²⁺,Mn²⁺,Ca²⁺

C)possible ions present Cu²⁺,Mn²⁺,Ca²⁺,Na⁺ D)possible ions present Ag⁺,Cu²⁺,Mn²⁺,Ca²⁺,Na<sup>+</sup >

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

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Sample Questions

Q1) The most common white pigment until the 1880s was lead white,sometimes called basic lead carbonate: (PbCO₃)₂Pb(OH)₂.Paintings containing lead white turned black in the presence of moist H₂S from natural sources and polluted air due to the formation of PbS.The PbCO₃ portion of this reaction is shown below. PbCO₃(s)+

H₂S(aq)

PbS(s)+ H₂CO₃(aq)

If H° = -60.9 kJ/mol and S° = 26.6 J/K,what are S_surr and S_total for this reaction at 25°C??

Q2) At constant pressure and temperature,which statement is true?

A)All reactions for which H < 0 are spontaneous.

B)All reactions for which S < 0 are spontaneous.

C)All reactions for which G < 0 are spontaneous.

D)All reactions for which K < 1 are spontaneous.

Q3) If G is small and positive,

A)the forward reaction is spontaneous and the system is far from equilibrium.

B)the forward reaction is spontaneous and the system is near equilibrium.

C)the reverse reaction is spontaneous and the system is far from equilibrium.

D)the reverse reaction is spontaneous and the system is near equilibrium.

Page 18

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

Q5) What is the entropy of 10 molecules in a system of 100 boxes?

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Page 19

Chapter 17: Electrochemistry

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Sample Questions

Q1) The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is

2 NiO(OH)(s)+ Cd(s)+ 2 H₂O(l) 2 Ni(OH)₂(s)+ Cd(OH)₂(s).

What is the standard free energy change for this reaction?

A)-38.7 kJ

B)-116 kJ

C)-232 kJ

D)-463 kJ

Q2) For a galvanic cell,the cathode has a ________ sign and is the site of ________.

A)negative,oxidation

B)negative,reduction

C)positive,oxidation

D)positive,reduction

Q3) Using Table 17.1,find E° for 2 H₂O(l) 2 H₂(g)+ O₂(g).

A)-2.06 V

B)-1.23 V

C)-0.80 V

D)-0.40 V

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Chapter 18: Hydrogen, oxygen, and Water

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Sample Questions

Q1) Which is an ionic binary hydride?

A)HCl

B)KH

C)both HCl and KH

D)neither HCl nor KH

Q2) What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.340 grams of H₂O₂ at 700°C and 755 mm Hg according to the chemical equation shown below? H₂O₂(l) H₂(g)+ O₂(g)

A)402 mL

B)804 mL

C)1210 mL

D)1610 mL

Q3) The direct methanol fuel cell (DMFC),a galvanic cell proposed for use in consumer products,employs the overall reaction shown below.How many liters of oxygen at 25°C and 1.00 atm are required to completely react with 0.641 g of CH₃OH? 2 CH₃OH(aq)+ 3 O₂(g) 2 CO₂(g)+ 4 H₂O(l)

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21

Chapter 19: The Main-Group Elements

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Sample Questions

Q1) Which of these molecules is most likely to contain good overlap of p orbitals,as shown in figure (a),rather than poor overlap of p orbitals,as shown in figure (b)?

A)Cl₂

B)N₂

C)P₄

D)S₈

Q2) What statement about nitric acid is not true?

A)It is a strong oxidizing agent.

B)It is one of the more common strong acids and is essentially 100% dissociated in water.

C)It often has a yellow color due to the formation of NO₂.

D)Its anhydride is N₂O₃.

Q3) In which compound is phosphorus in its lowest oxidation state?

A)P₄O₆

B)PCl₃

C)PH₃

D)PCl₅

Q4) The charge,n,on the cyclic anion Si₆O₁₈ⁿ that is found in the mineral beryl is ________.

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Page 22

Chapter 20: Transition Elements and Coordination Chemistry

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Sample Questions

Q1) What is the coordination number of the Au atom in K [Au(CN)₂(SCN)₂]?

A)2

B)3

C)4

D)6

Q2) Based on the variation in Z_eff,which oxoanion should be the weakest oxidizing agent?

A)VO₄^3-

B)CrO₄^2-

C)MnO₄^2-

D)FeO₄^2-

Q3) Fe³⁺ has ________ valence electrons.

Q4) What is the characteristic outer electron configuration for transition elements?

A)(n - 1)d^10-x^ns²

B)(n)d^10-x^ns²

C)(n + 1)d^10-x^ns¹

D)(n - 1)d^10-x(n + 1)s²

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Q5) The number of unpaired electrons in tetrahedral NiBr₄^2- is

Chapter 21: Metals and Solid-State Materials

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Q1) Tin exists in two forms: gray tin and white tin.The electrical conductivity of gray tin increases with an increase in temperature,whereas the electrical conductivity of white tin decreases with an increase in temperature.The form of tin that is a semiconductor is ________ tin.

Q2) Relative to a bulk sample of gold,nanoparticles of gold have

A)greater reactivity and higher melting point.

B)greater reactivity and lower melting point.

C)lower reactivity and higher melting point.

D)lower reactivity and lower melting point.

Q3) Which of these materials has the highest electrical conductivity?

A)material (1)

B)material (2)

C)material (3)

D)material (4)

Q4) In this picture the valence band is given by letter(s)

A)a)

B)b)

C)c)

D)a and b.

Q5) The number of electrons that half fill a composite s-d band is ________.

Page 24

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Chapter 22: Nuclear Chemistry

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Sample Questions

Q1) A binding energy curve is a plot of binding energy per nucleon versus atomic number.In what region of the binding energy curve are the most stable elements found?

A)in the lower left region (low atomic mass)

B)in the central top region (moderate atomic mass)

C)in the lower right region (heavy atomic mass)

D)binding energy is not dependent on atomic mass

Q2) Which one of the following is most penetrating?

A)alpha particles

B)beta particles

C)gamma rays

D)positrons

Q3) Elements with ________ atomic mass are best possible candidates for a fission reaction.

A)very low

B)moderate

C)moderate to heavy

D)very heavy

Q4) 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) The base sequences in mRNA that code for particular amino acids are Trp: UGG,Phe: UUU,and Glu: GAA.What is the peptide that is produced from the DNA sequence: CTTACCAAA?

A)Glu-Phe-Trp

B)Glu-Trp-Phe

C)Phe-Trp-Glu

D)Trp-Glu-Phe

Q2) What type of compound is formed when a carboxylic acid reacts with an alcohol?

A)an aldehyde

B)an amide

C)an aromatic

D)an ester

Q3) Which one of the following molecules can rotate freely around its carbon-carbon bond?

A)acetylene

B)cyclopropane

C)ethane

D)ethylene

Q4) Individual amino acids that make up a protein are called ________.

Q5) Monosaccharides are classified as either ________ or ________.

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