Pre-Medical Chemistry Solved Exam Questions - 4358 Verified Questions

Course Introduction

Pre-Medical Chemistry Solved

Exam Questions

Pre-Medical Chemistry is designed to provide students with a foundational understanding of the principles and concepts central to general and organic chemistry, with a focus on their applications in medicine and the health sciences. The course covers topics such as atomic structure, chemical bonding, stoichiometry, chemical reactions, thermodynamics, acids and bases, organic functional groups, and the properties of biomolecules. Emphasis is placed on developing problem-solving skills, laboratory techniques, and conceptual knowledge essential for success in advanced science coursework and future medical studies. This course serves as a critical stepping stone for students planning to enter medical, dental, or other health professional programs.

Recommended Textbook

Chemistry 7th Edition by John E. McMurry

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Chapter 1: Chemical Tools: Experimentation and Measurement

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Sample Questions

Q1) Convert 98.6 cm³ to m³.

A)98.6 × 10^-4 m³

B)98.6 × 10¹ m³

C)98.6 × 10⁶ m³

D)98.6 × 10⁸ m³

Answer: A

Q2) A sailor circumnavigated the earth and covered 4,264,000 meters.Express this number in standard scientific notation.

A)4.264 × 10^-7 m

B)4.264 × 10^-6 m

C)4.264 × 10⁶ m

D)4.264 × 10⁷ m

Answer: C

Q3) The diameter of an atom is approximately 1 × 10^-10 m.What is the diameter in millimeters?

A)1 × 10^-16 mm

B)1 × 10^-13 mm

C)1 × 10^-7 mm

D)1 × 10^-4 mm

Answer: C

Page 3

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Most elements in the periodic table are A)metals.

B)non-metals.

C)noble gases.

D)semi-metals.

Answer: A

Q2) Which of the following statements concerning ionic compounds is true?

A)Essentially all ionic compounds are solids at room temperature and pressure.

B)Ionic compounds do not contain any covalent bonds.

C)Ionic compounds contain the same number of positive ions as negative ions.

D)The chemical formula for an ionic compound must show a nonzero net charge.

Answer: A

Q3) Which is most likely to form a binary oxide with the formula MO₃ (where M = element A,B,C,or D)?

A)element A

B)element B

C)element C

D)element D

Answer: D

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) Which of the following has the greatest mass?

A)6.0 × 10²³ atoms of O

B)3.0 × 10²³ molecules of O₂

C)2.0 × 10²³ molecules of O₃

D)All have the same mass.

Answer: D

Q2) In the combustion analysis of an unknown compound containing only carbon,hydrogen,and oxygen,the grams of oxygen are found from the grams of A)CO₂ only.

B)H₂O only.

C)CO₂and H₂O only.

D)CO_2,H₂O and unknown compound.

Answer: D

Q3) The number of grams in 0.250mol of urea, (NH₂)₂CO,is

Answer: 15.0 g

Q4) The fundamental SI unit for measuring matter is the ________.

Answer: mole

Q5) What is the empirical formula of benzene,C₆H₆?

Answer: CH

Page 5

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) Which outcome corresponds to the mixing of sodium and sulfate ions shown in the following equation? 2 Na⁺(aq)+ SO₄^2-(aq) ?

A)box (a)

B)box (b)

C)box (c)

D)None of these

Q2) When NaOH(aq)is mixed with CuSO₄(aq)a precipitate forms.Based on solubility guidelines the formula of the precipitate is ________.

Q3) If 200.mL of 0.100 M Na₂SO₄ is added to 200.mL of 0.150 M NaCl,what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

A)0.05 M

B)0.175 M

C)0.125 M

D)0.250 M

Q4) The balanced net ionic equation for the reaction Li₂SO₄(aq)+ Ca(NO₃)₂(aq) CaSO₄(s)+ 2 LiNO₃(aq)is ________.

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Chapter 5: Periodicity and the Electronic Structure of Atoms

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Sample Questions

Q1) What is the frequency of a helium-neon laser light with a wavelength of 632.8 nm?

The speed of light is 3.00 × 10⁸ m/s.

A)4.74 × 10¹⁴ s^-1

B)4.74 × 10⁵ s^-1

C)2.11 × 10^-15 s^-1

D)1.58 × 10^-15 s^-1

Q2) A radio station that broadcasts at 99.1 MHz is broadcasting at a frequency of ________ s^-1.

Q3) Wave (b)has the

A)higher frequency and higher energy than wave (a).

B)higher frequency and lower energy than wave (a).

C)lower frequency and higher energy than wave (a).

D)lower frequency and lower energy than wave (a).

Q4) What is the energy of a wavelength of light of 550 nm?

A)1.09 × 10^-31J

B)3.61 × 10^-37J

C)3.61 × 10^-19J

D)1.09 × 10^-22J

Q5) An orbital with n = 5 and l = 2 is a ________ orbital.

Q6) Using shorthand notation,the electron configuration of Ni is ________.

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Chapter 6: Ionic Compounds: Periodic Trends and Bonding

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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 lowest first ionization energy,E_i1?

A)A

B)B

C)C

D)D

Q2) Which of the following atoms with the specified electronic configurations would have the lowest first ionization energy?

A)[He]2s²2p³

B)[Ne]3s²3p⁴

C)[Xe]6s¹

D)[Xe]6s²4f¹⁴5d¹⁰6p¹

Q3) The element in period 4 with the smallest first ionization energy is ________.

Q4) Which element,indicated by letter on the periodic table above,has a 3+ ion with the electron configuration [Kr]4d⁵?

A)A

B)B

C)C

D)D

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Chapter 7: Covalent Bonding and Electron-Dot Structures

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Sample Questions

Q1) What bond distance is expected to be longest?

A)A carbon-carbon bond with a bond order of 0

B)A carbon-carbon bond with a bond order of 1

C)A carbon-carbon bond with a bond order of 2

D)A carbon-carbon bond with a bond order of 3

Q2) A reactive element with a relatively high electronegativity would be expected to have a relatively

A)small negative electron affinity and a relatively low ionization energy.

B)small negative electron affinity and a relatively high ionization energy.

C)large negative electron affinity and a relatively low ionization energy.

D)large negative electron affinity and a relatively high ionization energy.

Q3) How many carbon-carbon bonds are present in C₃H₈?

Q4) The number of Lewis electron dot resonance structures required to describe NO₂^- is ________.

Q5) Based on formal charges,the P-O bond order in POCl₃ is expected to be ________.

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Chapter 8: Covalent Compounds: Bonding Theories and Molecular

Structure

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Sample Questions

Q1) In order to complete an electron-dot structure of alanine,the nitrogen atom needs

A)1 additional bond and 1 nonbonded pair of electrons.

B)1 additional bond and 2 nonbonded pairs of electrons.

C)1 nonbonded pair of electrons.

D)2 nonbonded pairs of electrons.

Q2) A triple bond is generally composed of A)three bonds.

B)two bonds and one bond.

C)one bond and two bonds.

D)three bonds.

Q3) In C₃H₇NHC₃H₇,which intermolecular forces are present?

A)Dispersion,hydrogen bonding and dipole-dipole forces are present.

B)Only dipole-dipole and ion-dipole forces are present.

C)Only dispersion and dipole-dipole forces are present.

D)Only hydrogen bonding forces are present.

Q4) Of NH₄⁺and NH₄^-the one with the smaller bond angles is

Q5) The polarity of CCl₄ is ________.

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Chapter 9: Thermochemistry: Chemical Energy

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Q1) At constant pressure,the combustion of 25.0 g of C₂H₆(g)releases 1300 kJ of heat.What is H for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g) 4 CO₂(g)+ 6 H₂O(l)

A)-215 kJ

B)-390 kJ

C)-1560 kJ

D)-3120 kJ

Q2) Find H° for the reaction C₃H₈(g)+ 5 O₂(g) 3 CO₂(g)+ 4 H₂O(l). H° = -2046 kJ for the reaction: C₃H₈(g)+ 5 O₂(g) 3 CO₂(g)+ 4 H₂O(g)

The heat of vaporization of water is 44.0 kJ/mol.Note that H₂O is a liquid in the first reaction and a gas in the second.

A)-2222 kJ

B)-2090 kJ

C)-2002 kJ

D)-1870 kJ

Q3) The SI unit for energy is the ________.

Q4) Is thermal energy 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) If the total pressure in the container is 900 mm Hg,what is the partial pressure of neon?

A)90 mm Hg

B)180 mm Hg

C)270 mm Hg

D)450 mm Hg

Q2) What is the volume of 10.0 g of oxygen gas at 157°C and 2.50 kPa pressure?

A)51.5 L

B)163 L

C)1.61 L

D)447 L

Q3) According to Graham's law,the rate of effusion of a gas is inversely proportional to the ________.

Q4) Which of the following would have a density of 3.04 g/L at 7.0°C and 0.987 atm?

A)Ar

B)Cl₂

C)He

D)N₂

Q5) The region of the atmosphere that is closest to the earth's surface is the ________.

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Chapter 11: Liquids, solids, and Phase Changes

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Sample Questions

Q1) What is the physical phase of the substance at T = 100 K and P = 0.1 atm?

A)gas

B)liquid

C)solid

D)supercritical fluid

Q2) 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

Q3) What is the empirical formula of the mineral?

A)MM'A

B)MM'A₃

C)M₂M'A₃

D)M₈M'A₆

Q4) The cubic closest-packed arrangement of atoms is the same as which cubic unit cell?

Q5) Ni has a face-centered unit cell.The number of Ni atoms in the unit cell is ________.

Page 13

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Chapter 12: Solutions and Their Properties

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Sample Questions

Q1) To make a 0.125 M solution,one could take 0.125 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) Calculate the freezing point of a solution of 30.0 g methyl salicylate,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆.K_f for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

A)-1.56°C

B)1.56°C

C)3.93°C

D)7.06°C

Q3) Although there are exceptions,which is most likely to be true for the dissolving of a solid in a liquid?

A) H_soln is positive.

B) H_soln is negative.

C) S_soln is positive.

D) S_soln is negative.

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) Hydrochloric acid in the hydrolysis of an ester to form an alcohol and a carboxylic acid is an example of a ________ (heterogeneous,homogeneous)catalyst.

Q2) What is the order of reaction with respect to A?

A)0

B)1/2

C)1

D)2

Q3) What is the rate law for the elementary reaction shown below? 2 HI H₂ + I₂

A)Rate = k[HI]

B)Rate = k[HI]²

C)Rate = k[H₂][I₂]

D)Rate = k[H₂][I₂]/[HI]²

Q4) The elementary reaction: 2 HF H₂ + F₂,is an example of a ________ reaction.

A)unimolecular

B)bimolecular

C)termolecular

D)tetramolecular

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) Which statement is true for a reaction with K_c equal to 8.90 × 10^-12?

A)Increasing the temperature will not change the value of K_c.

B)There are appreciable concentrations of both reactants and products.

C)The reaction proceeds hardly at all towards completion.

D)The reaction proceeds nearly all the way to completion.

Q2) Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: M_aX_b(s) a M^b+(aq)+ b X^a-(aq).Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

A)AgCl,K_c = 1.8 × 10^-10

B)Ag₂SO₄,K_c = 1.2 × 10^-5

C)CaCO₃,K_c = 2.6 × 10^-9

D)CaF₂,K_c = 1.5 × 10^-10

Q3) The reaction CaCO₃(s) CaO(s)+ O₂(g)is endothermic 298

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

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Chapter 15: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Which acid has the smallest value of K_a?

A)HX

B)HY

C)HZ

D)All have the same K_a value.

Q2) If the ionization constant of water,K_w,at 40°C is 2.92 × 10^-14,then what is the hydronium ion concentration for a neutral solution?

A)[H₃O⁺] < 1.00 × 10^-7 M

B)[H₃O⁺] > 1.71 × 10^-7 M

C)[H₃O⁺] = 1.71 × 10^-7 M

D)[H₃O⁺] < 1.71 × 10^-7 M

Q3) At 25°C,the pH of a vinegar solution is 2.60.What are the values of [H₃O⁺] and [OH^-] in the solution?

A)3.99 × 10^-12 M,2.51 × 10^-3 M

B)2.51 × 10^-3 M,3.98 × 10^-12 M

C)2.51 × 10^-3 M,11.40 M

D)2.60 M,11.40 M

Q4) A 0.50 M KNO₂ solution will have a pH ________ seven.

Q5) A proton hydrated by ten water molecules has the formula ________.

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Chapter 16: Applications of Aqueous Equilibria

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Q1) What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1.8 × 10^-5. HNO₂(aq)+ NH₃(aq) NH₄NO₂(aq)

A)8.1 × 10⁵

B)1.8 × 10⁹

C)4.5 × 10¹⁰

D)8.1 × 10¹⁹

Q2) The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

A)2.34

B)4.85

C)5.59

D)6.72

Q3) What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

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

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Q1) 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

Q2) For the evaporation of water during perspiration on a hot,dry day,

A) H is positive and T S = H.

B) H is positive and T S > H.

C) H is positive and T S < H.

D) H is negative and T S is positive.

Q3) The reaction 2 H₂(g)+ O₂(g) 2 H₂O(g)is spontaneous at 25°C.The addition of a catalyst will ________ (decrease,increase,not change)the rate of reaction and ________ (decrease,increase,not change)the spontaneity of the reaction.

Q4) A 1.8 mole sample of gas at STP has a ________ entropy than 1.8 mole of gas at 273 K and 835 mm Hg.

Q5) What is the entropy of 12 molecules in a system of 100 boxes?

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Chapter 18: Electrochemistry

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Q1) Based on the following information, F₂(g)+ 2 e^- 2

F^-(aq)E° = +2.87 V

Mg²⁺(aq)+ 2 e^- 2 Mg(s)E° = -2.37 V

Which of the following chemical species is the strongest reducing agent?

A)F₂(g)

B)Mg²⁺(aq)

C)F^-(aq)

D)Mg(s)

Q2) How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 3.50 moles of copper metal?

A)0.267 hours

B)0.533 hours

C)1.88 hours

D)3.75 hours

Q3) A salt bridge is used to

A)provide reactants in a fuel cell.

B)determine the direction of the cell reaction.

C)control whether the cell is electrolytic.

D)allow the ion flow necessary for cell neutrality.

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Chapter 19: Nuclear Chemistry

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Q1) If a sample of ²³³Pa takes 62.7 days to decrease to 20.0% of its original mass,what is its half-life?

A)0.0370 days

B)27.0 days

C)157 days

D)195 days

Q2) A becquerel is

A)the amount of sample that undergoes 1 disintegration per second.

B)the amount of sample that undergoes 3.7 × 10¹⁰ disintegrations per second.

C)the amount of tissue damage done by radiation.

D)equal to 0.01 J of energy absorbed per kilogram of tissue.

Q3) Radium occurs only in uranium ores,typically with an observed Ra/U ratio of 1mg/3kg.Uranium ores normally contain only about 200 ppm of U.How many kilograms of uranium ore must be processed to obtain 1 mg of radium?

A)1700 kg ore

B)15,000 kg ore

C)6.0 × 10⁸ kg ore

D)None of these

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Chapter 20: Transition Elements and Coordination Chemistry

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Q1) Based on the variation in Z_eff,which M²⁺ ion should be the strongest reducing agent?

A)Ti

B)Cr

C)Fe

D)Zn

Q2) Which has the lowest density?

A)Y

B)Mo

C)Rh

D)Cd

Q3) The formula for tetraamminediiodochromium(III)bromide is ________.

Q4) Which one of the following objects is chiral?

A)a bottle

B)a chair

C)a blank paper

D)a shoe

Q5) Inner transition elements are found in the ________-block of the periodic table.

Q6) Transition elements are located in the ________-block of the periodic table.

Q7) The coordination number of chromium in [Cr(EDTA)]^- is ________. Page 22

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Chapter 21: Metals and Solid-State Materials

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Q1) Alumina-titanium is a composite material used in hip replacements.Composite materials can be classified as ceramic-ceramic,ceramic-metal,or ceramic-polymer.Alumina-titanium is classified as ________.

Q2) Which of these elements is likely to be found in nature as a sulfide?

A)element A

B)element B

C)element C

D)element D

Q3) What metal is isolated from the ore rutile and what is the chemical formula of rutile?

A)aluminum,Al₂O₃ xH₂O

B)cassiterite,SnO₂

C)cinnabar,HgS

D)titanium,TiO₂

Q4) The number of electrons that half fill a composite s-d band is ________.

Q5) Because nanoparticles have a larger percentage of atoms on the surface of the nanoparticle than on the surface of bulk material,nanoparticles have ________ melting points and ________ chemical reactivity than the bulk material.

Q6) The principal source of chromium is chromite.What is the formula of chromite?

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Chapter 22: The Main-Group Elements

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Q1) Using principles discussed in chapters 15 and 19,determine which of the following is the strongest acid.

A)HClO₂

B)HClO₃

C)HBrO₃

D)HIO₃

Q2) What is the range of oxidation states that are exhibited by P?

A)from -3 to 0

B)from -2 to +2

C)from -3 to +5

D)from -1 to +5

Q3) Which element indicated on the above periodic table forms a binary hydride with molecular structure (4)shown above?

A)element A

B)element B

C)element C

D)element D

Q4) If niobium loses all of its valence electrons when it reacts with fluorine,what is the formula of the neutral binary compound that results?

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Chapter 23: Connections to Organic and Biological Chemistry

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Q1) In the figure above,which are branched hydrocarbons?

A)All are branched hydrocarbons.

B)None are branched hydrocarbons.

C)only (1)and (4)

D)only (1), (2),and (4)

Q2) Which one of the following contains a polar carbonyl group,C=O?

A)a carboxylic acid

B)an alkyne

C)an amine

D)an alkane

Q3) The condensed formula of the smallest molecule that contains the ether functional group is ________.

Q4) None of the listed compounds contains a ring.Which could have one carbon-carbon triple bond?

A)C₃H₈

B)C₂H₂

C)C₁₀H₂₀

D)All of these

Q5) Does tyrosine contain an aromatic ring?

Page 26

Q6) Linoleic acid,a fatty acid,contains ________ carbons and ________ double bonds.

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