Basic Chemistry Final Exam - 2556 Verified Questions

Basic Chemistry

Final Exam

Course Introduction

Basic Chemistry provides an introduction to the fundamental concepts of chemistry, covering topics such as atomic structure, chemical bonding, stoichiometry, states of matter, the periodic table, chemical reactions, and basic laboratory techniques. Emphasis is placed on developing an understanding of matter and its interactions, the principles governing chemical changes, and quantitative problem-solving methods essential for further studies in the sciences. This course equips students with the foundational knowledge needed to appreciate the chemical processes that underpin everyday life and scientific phenomena.

Recommended Textbook

General Chemistry The Essential Concepts 7th Edition by Raymond Chang

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Page 2

Chapter 1: Introduction

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Sample Questions

Q1) A US barrel is 4.21 cubic feet. Express this volume in liters.

A)3.99 * 10^-5 L

B)1.99 * 10^-2 L

C)19.9 L

D)105 L

E)119 L

Answer: E

Q2) Dry ice (carbon dioxide)changes from a solid to a gas at -78.5^\(\circ\)C. What is this temperature in ^\(\circ\)F?

A)-173^\(\circ\)F

B)-12.6^\(\circ\)F

C)-109^\(\circ\)F

D)-75.6^\(\circ\)F

E)none of them are within 2^\(\circ\)F of the right answer Answer: C

Q3) The volume of a sphere is given by V = (4/3)\(\pi\)r³ where r is the radius. What is the mass of a magnesium sphere with a radius of 0.80 cm? (The density of magnesium is 1.74 g/cm³.)

Answer: 3.7 g

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Page 3

Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) When J. J. Thomson discovered the electron, what physical property of the electron did he measure?

A)its charge, e

B)its charge-to-mass ratio, e/m

C)its temperature, T

D)its mass, m

E)its atomic number, Z

Answer: B

Q2) Write the formula for the acid formed from the nitrite anion, and then name the acid.

Answer: HNO₂, nitrous acid

Q3) Which of the following is the formula for hydrobromic acid?

A)KBr

B)HBr

C)HBrO

D)HBrO₂

E)HBrO₃

Answer: B

Q4) How many electrons, protons, and neutrons does an iron-55 atom have?

Answer: 26 electrons, 26 protons, and 29 neutrons

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Chapter 3: Stoichiometry

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Sample Questions

Q1) Balance the following chemical equation: C₄H₁₀ + O₂ \(\rarr\) CO₂ + H₂O

Answer: 2C₄H₁₀ + 13 O₂ \(\rarr\) 8CO₂ + 10H₂O

Q2) How many ICl₃ molecules are present in 1.75 kg of ICl₃?

Answer: 4.52 * 10²⁴

Q3) Calculate the number of moles of xenon in 12.0 g of xenon.

A)1.00 mol

B)0.0457 mol

C)0.183 mol

D)7.62 * 10^-3 mol

E)0.0914 mol

Answer: E

Q4) When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced. What is the empirical formula of the compound?

Answer: C₂H₆O

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5

Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) The oxidation number of S in K₂SO₄ is A)+6.

B)+4.

C)+2.

D)-1.

E)None of the above.

Q2) Calcium sulfate dihydrate (commonly known as gypsum)dissolves in cold water to the extent of 0.241 g per 100. cm³. What is the concentration of calcium ions in this solution?

A)1.77 * 10^-2 M

B)2.80 * 10^-2 M

C)1.77 * 10^-3 M

D)3.54 * 10^-2 M

E)1.40 * 10^-2 M

Q3) The distinguishing characteristic of all electrolyte solutions is that they

A)contain molecules.

B)conduct electricity.

C)react with other solutions.

D)always contain acids.

E)conduct heat.

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Chapter 5: Gases

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Sample Questions

Q1) Calculate the density, in g/L, of SF₆ gas at 27°C and 0.500 atm pressure.

A)3.38 * 10^-3 g/L

B)2.96 g/L

C)22.4 g/L

D)32.9 g/L

E)3.38 kg/L

Q2) What volume of oxygen gas at 320 K and 680 torr will react completely with 2.50 L of NO gas at the same temperature and pressure? 2NO(g)+ O₂(g) \(\rarr\)2NO₂(g)

A)1.25 L

B)2.50 L

C)3.00 L

D)1.00 L

E)5.00 L

Q3) Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water. What volume of carbon dioxide at STP is generated as a result of the combustion of 1.0 gal of gasoline?

(The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)

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Page 7

Chapter 6: Energy Relationships in Chemical Reactions

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Sample Questions

Q1) Methanol (CH₃OH)burns according to the equation 2CH₃OH(l)+ 3O₂(g)\(\rarr\) 2CO₂(g)+ 4H₂O(l), \(\Delta\)H°_rxn = -1454 kJ/mol.

How much heat, in kilojoules, is given off when 75.0 g of methanol is burned?

A)727 kJ

B)3.22 * 10³ kJ

C)1.45 * 10³ kJ

D)1.70 * 10^-3 kJ

E)3.41 * 10³ kJ

Q2) A feverish student weighing 75 kilograms was immersed in 400. kg of water at 4.0°C to try to reduce the fever. The student's body temperature dropped from 40.0°C to 37.0°C. Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

Q3) An endothermic reaction causes the surroundings to A)warm up.

B)become acidic.

C)condense.

D)decrease in temperature.

E)release CO₂ .

Q4) Define specific heat.

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Chapter 7: The Electronic Structure of Atoms

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Sample Questions

Q1) Which of the following ground-state atoms is diamagnetic?

A)Ca

B)As

C)Cu

D)Fe

E)none of these

Q2) What is the wavelength of radiation that has a frequency of 5.39 * 10¹⁴ s^-1? (c = 2.9979 * 10⁸ m/s)

A)1.80 * 10^-3 nm

B)556 nm

C)618 nm

D)6180 nm

E)1.61 * 10²³ nm

Q3) What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm?

A)6.46 * 10^-16 J

B)6.46 * 10^-25 J

C)2.46 * 10^-4 J

D)12.4 kJ

E)246 kJ

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Chapter 8: The Periodic Table

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Sample Questions

Q1) Which of the elements listed below has the greatest atomic radius?

A)B

B)Al

C)S

D)P

E)Si

Q2) Which one of the following elements is a transition element?

A)Sr

B)Pb

C)As

D)Fe

E)H

Q3) Write the ground-state electron configuration for Ca²⁺.

Q4) Which of the following elements behaves chemically similarly to oxygen?

A)magnesium

B)sodium

C)sulfur

D)chlorine

E)iron

F)beryllium

Page 10

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Chapter 9: Chemical Bonding I: the Covalent Bond

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Sample Questions

Q1) Which one of these polar covalent bonds would have the greatest percent ionic character?

A)H - Br

B)H - Cl

C)H - F

D)H - I

Q2) Write the Lewis structure of ammonia (nitrogen trihydride).

Q3) How many covalent bonds will be drawn to phosphorous in PO₄^3- for the dot structure that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s)?

A)4

B)5

C)6

D)7

E)8

Q4) Write a Lewis structure for the phosphate ion, PO₄^3-, that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for PO₄^3- that obey the octet rule.

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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization

of Atomic

Orbitals

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Sample Questions

Q1) How does the geometrical structure of PF₅ differ from that of IF₅?

Q2) What is the hybridization of the iodine atom in the IF₅ molecule?

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q3) What is the hybridization of the As atom in the AsF₅ molecule?

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q4) A bonding molecular orbital is of lower energy (more stable)than the atomic orbitals from which it was formed.

A)True

B)False

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Q5) According to the VSEPR theory, will the molecule PF₅ be polar or nonpolar?

Chapter 11: Introduction to Organic Chemistry

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Sample Questions

Q1) The alkane with six carbon atoms is called A)butane.

B)hexane.

C)heptane.

D)butene.

E)none of these.

Q2) The formula CH₃CH₂CH₂CH=CH₂ represents

A)an alkane.

B)a cycloalkane.

C)an alkene.

D)an alkyne.

E)an aromatic compound.

Q3) The reaction of an alcohol and a carboxylic acid yields A)a hydrocarbon.

B)an ester.

C)an ether.

D)an aldehyde.

E)a ketone.

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Page 13

Chapter 12: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) Copper crystallizes in a face-centered cubic unit cell. The density of copper is 8.94 g/cm³. Calculate the length of the edge of the unit cell in pm.

Q2) Which of the following characteristics indicates the presence of weak intermolecular forces in a liquid?

A)a low heat of vaporization

B)a high critical temperature

C)a low vapor pressure

D)a high boiling point

E)None of the above.

Q3) Which of the following substances would have the highest critical temperature?

A)CH₃Cl

B)C₂H₆

C)F₂

D)H₂

E)CO₂

Q4) Sodium iodide, NaI, melts at 651°C. In its liquid state NaI conducts electricity. What kind of crystal is this?

Q5) Of the given pair of compounds, which would have the higher boiling point? NH₃ or CH₄

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Chapter 13: Physical Properties of Solutions

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Sample Questions

Q1) Which of the following aqueous solutions has the lowest freezing point?

A)0.18 m KCl

B)0.15 m Na₂SO₄

C)0.12 m Ca(NO₃)₂

D)pure water

E)0.20 m C₂H₆O₂ (ethylene glycol)

Q2) The vapor pressure of water at 20°C is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 2.00 * 10² g of sucrose (C₁₂H₂₂O₁₁)and 3.50 * 10² g water?

A)0.51 mmHg

B)16.0 mmHg

C)17.0 mmHg

D)18.0 mmHg

E)19.4 mmHg

Q3) For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

A)True

B)False

Q4) Define solvation.

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) The rate law for the reaction H₂O₂ + 2H⁺ + 2I^-\(\rarr\) I₂ + 2H₂O is rate = k[H₂O₂][I^-]. The following mechanism has been suggested. H₂O₂ + I^-\(\rarr\) HOI + OH slow

OH^- + H⁺ \(\rarr\) H₂O fast HOI + H⁺ + I^-\(\rarr\) I₂ + H₂O fast

Identify all intermediates included in this mechanism.

A)H⁺ and I^-

B)H⁺ and HOI

C)HOI and OH^-

D)H⁺ only

E)H₂O and OH^-

Q2) A reaction mechanism usually is

A)the same as the balanced chemical equation.

B)restricted to only one possible explanation.

C)obvious if the reaction order is known.

D)difficult, if not impossible, to prove.

E)obvious if the activation energy is known.

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Page 16

Chapter 15: Chemical Equilibrium

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Q1) Equilibrium is established for the reaction 2X(s)+ Y(g)\(\rarr\)2Z(g)at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

A)3.2 M

B)3.5 M

C)4.5 M

D)7.1 M

E)None of these.

Q2) For the common allotropes of carbon (graphite and diamond), C(gr)\(\rarr\)C(dia)with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm³/mol and 3.42 cm³/mol; \(\Delta\)H_f of diamond is 1.90 kJ/mol. This data suggests that the formation of diamond is favored at

A)low temperatures and low pressures.

B)high temperatures and low pressures.

C)low temperatures and high pressures.

D)high temperatures and high pressures.

Q3) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

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Page 17

Chapter 16: Acids and Bases

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Q1) When 2.0 * 10^-2 mole of nicotinic acid (a monoprotic acid)is dissolved in 350. mL of water, the pH is 3.05. What is the K_a of nicotinic acid?

Q2) Identify the conjugate acid of SO₄^2- in the reaction CO₃^2- + HSO₄^- \(\rarr\) HCO₃^- + SO₄^2-

A)CO₃^2-

B)HSO₄^-

C)OH^-

D)H₃O⁺

E)SO₄^2-

Q3) A 8.0 M solution of formic acid (HCOOH)is 0.47% ionized. What is the K_a of formic acid?

Q4) Hard water deposits (calcium carbonate)have built up around your bathroom sink. Which one of these substances would be most effective in dissolving the deposits?

A)ammonia

B)bleach (sodium hypochlorite)

C)lye (sodium hydroxide)

D)vinegar (acetic acid)

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Page 18

Chapter 17: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10^-3

M MgCl₂ are added to 500. mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

A)Yes, Q > K_sp

B)No, Q < K_sp

C)No, Q = K_sp

D)Yes, Q < K_sp

Q2) Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8?

A)CH₃COO₂Na / CH₃COOH (K_a = 1.8 * 10^-5)

B)NH₃ / NH₄Cl (K_a = 5.6 * 10^-10)

C)NaOCl / HOCl (K_a = 3.2 * 10^-8)

D)NaNO₂ / HNO₂ (K_a = 4.5 * 10^-4)

E)NaCl / HCl

Q3) Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer.

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19

Chapter 18: Thermodynamics

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Sample Questions

Q1) Arrange these compounds in order of increasing standard molar entropy at 25°C: C₃H₈(g), C₂H₄(g), ZnS(s), and H₂O(l).

A)ZnS(s)< H₂O(l)< C₃H₈(g)< C₂H₄(g)

B)C₂H₄(g)< H₂O(l)< C₃H₈(g)< NaCl(s)

C)ZnS(s)< C₃H₈(g)< C₂H₄(g)< H₂O(l)

D)C₃H₈(g)<

C₂H₄(g)< H₂O(l)< ZnS(s)

E)ZnS(s)< H₂O(l)<

C₂H₄(g)< C₃H₈(g)

Q2) For a certain reaction, \(\Delta\)G° = 87 kJ/mol, \(\Delta\)H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that \(\Delta\)S° and \(\Delta\)H° are temperature-independent?

Q3) How does the entropy change when a molecular solid is dissolved in water?

Q4) Choose the substance with the higher entropy per mole at a given temperature: CO₂(g)or CO₂(aq).

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Chapter 19: Redox Reactions and Electrochemistry

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Q1) The measured voltage of a cell in which the following reaction occurs is 0.96 V: H₂(g, 1.0 atm)+ 2Ag⁺(aq, 1.0 M)\(\rarr\)2H⁺(aq, pH = ?)+ 2Ag(s)

Calculate the pH of the H⁺(aq)solution.

A)1.4

B)2.7

C)5.4

D)7.1

E)14.9

Q2) Complete and balance the following redox equation. What is the coefficient of H₂S when the equation is balanced using the set of smallest whole-number coefficients? H₂S + MnO₄^- \(\rarr\) Mn²⁺ + SO₄^2- (acidic solution)

A)1

B)2

C)4

D)5

E)None of these.

Q3) Complete and balance the following redox reaction under acidic conditions: ClO₂^-(aq)\(\rarr\) ClO₂(g)+ Cl^-(aq)

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Chapter 20: The Chemistry of Coordination Compounds

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Q1) Two well-known complex ions containing Ni are [Ni(H₂O)₆]²⁺, which is green, and [Ni(en)₃]²⁺, which is purple. Which one of these statements is true?

A)The crystal field splitting energy (\(\Delta\))is greater for [Ni(en)₃]²⁺ than for [Ni(H₂O)₆]²⁺.

B)[Ni(en)₃]²⁺ absorbs energy in the red region of the spectrum.

C)Both complex ions are diamagnetic.

D)[Ni(H₂O)₆]²⁺ transmits light with wavelengths of approximately 650-700 nm.

E)The green complex absorbs green light.

Q2) Which of these complex ions would absorb light with the longest wavelength?

A)[Co(H₂O)₆]²⁺

B)[Co(NH₃)₆]²⁺

C)[CoF₆]^4-

D)[Co(CN)₆]^4-

E)[Co(en)₆]²⁺

Q3) What is the coordination number of silver in [Ag(NH₃)₂]Cl?

Q4) Write the chemical formula of diamminedichloroplatinum(II).

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Chapter 21: Nuclear Chemistry

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Q1) If 12% of a certain radioisotope decays in 5.2 years, what is the half-life of this isotope?

A)0.59 yr

B)1.7 yr

C)22 yr

D)28 yr

E)32 yr

Q2) What would the atom ratio of ²⁰⁶Pb to ²³⁸U be in a uranium mineral from a rock that is 1.0 * 10⁹ years old? t_1/2(²³⁸U)= 4.5 * 10⁹ yr.

A)0.14

B)0.16

C)0.22

D)0.86

E)1.16

Q3) Tritium is a radioisotope of hydrogen having a half-life of 12.3 years. If you initially had 1.0 * 10^-7 mole of tritium, how many moles of tritium would be left after 78 years?

Q4) Thorium-225 undergoes alpha decay. Write a balanced equation for this reaction.

Q5) Lead-209 undergoes beta decay. Write a balanced equation for this reaction.

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Chapter 22: Organic Polymerssynthetic and Natural

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Q1) A polymer made in a polymerization reaction that also produces small molecules (such as water)is classified as

A)an addition polymer.

B)a natural polymer.

C)a condensation polymer.

D)an elimination polymer.

E)a copolymer.

Q2) Which one of these molecules is part of the make-up of both DNA and RNA?

A)deoxyribose

B)ribose

C)phosphate

D)thymine

E)uracil

Q3) A peptide bond (also called an amide bond)joins two amino acids together. What atoms are linked by this bond?

A)C - O

B)C - H

C)C - N

D)N - S

E)S - C

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