Fundamentals of Chemistry Exam
Questions
Course Introduction
Fundamentals of Chemistry offers an essential introduction to the principles and practices of modern chemistry. The course covers core topics such as atomic and molecular structure, chemical bonding, stoichiometry, states of matter, solutions, thermochemistry, and basic concepts in chemical kinetics and equilibrium. Students gain hands-on experience through laboratory experiments that reinforce theoretical concepts, develop problem-solving skills, and encourage scientific inquiry. This course is designed to build a solid foundation for further studies in chemistry and related scientific fields.
Recommended Textbook
Introductory Chemistry 4th Edition by Nivaldo J. Tro
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1962 Verified Questions
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Page 2
Chapter 1: The Chemical World
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Sample Questions
Q1) Antoine Lavoisier observed that burning objects in a closed container resulted in a loss of mass.
A)True
B)False
Answer: False
Q2) Charcoal was burned in a barbecue grill.The ashes that remained weighed considerably less than the charcoal that was burned.Does this mean that the law of conservation of mass is wrong? Explain.
Answer: No.The gaseous products formed during the combustion of charcoal escaped into the air and are not accounted for.If all those products could have been collected and weighed along with the ashes,the total mass of the products would have been equal to the mass of the charcoal.
Q3) The scientific method ensures that poor theories are eliminated over time and good theories remain.
A)True
B)False
Answer: True
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Page 3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) A lead ball has a mass of 55.0 grams and a density of 11.4 g/cm<sup>3</sup>.What is the volume of the ball?
A)0.207 mL
B)0.207 L
C)4.82 mL
D)4.82 L
E)none of the above
Answer: C
Q2) The correct number of significant figures in the number 0.002320 is:
A)7
B)4
C)3
D)ambiguous
E)none of the above
Answer: B
Q3) Zeros located between two numbers are not significant.
A)True
B)False
Answer: False
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Page 4
Chapter 3: Matter and Energy
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Sample Questions
Q1) When 49.5 J of heat was transferred to 7.3 g iron at 22°C,the temperature of iron increases to 37°C.What is the specific heat of iron in J/g°C?
A)4.5
B)0.45
C)2.2
D)24
E)none of the above
Answer: B
Q2) What is the value of 27°C on the Fahrenheit scale?
A)73
B)52
C)81
D)91
Answer: A
Q3) When a chemical "cold pack" is activated,the chemical reactants absorb heat from the surroundings.
A)True
B)False
Answer: True
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Page 5
Chapter 4: Atoms and Elements
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Sample Questions
Q1) Metals are located on the left side of the periodic table.
A)True
B)False
Q2) Group 2A elements are also called:
A)noble gases.
B)halogens.
C)alkaline earth metals.
D)alkali metals.
E)none of the above
Q3) Which of the following statements about ions is INCORRECT?
A)Cations are positive ions and anions are negative ions.
B)Cations are formed when an atom loses electrons.
C)Anions are formed when an atom gains electrons.
D)Cations always have the same number of protons as electrons.
E)All statements are correct.
Q4) A cation forms when an atom gains an electron.
A)True
B)False
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) Which of the following species is a molecular element?
A)neon
B)sodium
C)chlorine
D)carbon dioxide
E)none of the above
Q2) The correct formula for calcium fluoride is CaF<sub>3</sub>.
A)True
B)False
Q3) The first chemist to formally state the law of constant composition was ________.
A)Dalton
B)Mendeleev
C)Rutherford
D)Proust
E)none of the above
Q4) Ionic compounds always contain positive and negative ions.
A)True
B)False
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Chapter 6: Chemical Composition
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Sample Questions
Q1) What is the mass in grams of 5.40 moles of lithium?
A)6.94
B)37.5
C)1.29
D)3.25 × 10<sup>24</sup>
E)none of the above
Q2) One mole of potassium sulfate contains:
A)4 moles of oxygen.
B)2 moles of sulfur.
C)1 mole of potassium.
D)3 moles of potassium.
E)none of the above
Q3) Determine the empirical formula of a compound containing 60.3% magnesium and 39.7% oxygen.
A)MgO
B)MgO<sub>2</sub>
C)Mg<sub>2</sub>O<sub>3</sub>
D)Mg<sub>2</sub>O
E)none of the above
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) A redox reaction has occurred ________.
A)when a substance reacts with elemental oxygen
B)when an alkali metal reacts with an alkaline earth metal
C)when one substance transfers protons to another
D)when one substance forms a solid
E)when all of the above occur
Q2) One of the characteristics of an acid-base reaction is that this type of reaction forms water.
A)True
B)False
Q3) An aqueous solution is:
A)any liquid with another compound dissolved in it.
B)an ionic compound with water dissolved in it.
C)water with a molecular compound dissolved in it.
D)water with another compound dissolved in it.
E)none of the above
Q4) A precipitation reaction will occur when sodium chloride is mixed with potassium nitrate.
A)True
B)False
Page 9
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) The enthalpy of reaction, H <sub>rxn</sub>,is the amount of thermal energy that flows when a reaction occurs at constant temperature.
A)True
B)False
Q2) Given the recipe: 2 cups flour + 1 egg + 3 oz blueberries 4 muffins
If you have 9 cups of flour,4 eggs and plenty of blueberries,the theoretical yield of muffins is 16.
A)True
B)False
Q3) How many moles of sodium metal are needed to make 3.6 moles of sodium chloride?
Given the reaction: 2Na + Cl<sub>2</sub> 2NaCl
A)0.9
B)7.2
C)1.8
D)3.6
E)not enough information
Q4) The percent yield can never be greater than 100%.
A)True
B)False
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) Which subshell letter corresponds to a 4-leaf clover orbital pattern?
A)s
B)p
C)d
D)f
E)not enough information
Q2) What is the electron configuration for Ga?
A)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>3d<su p>10</sup>4s<sup>2</sup>4p<sup>6</sup>
B)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<su p>2</sup>3d<sup>10</sup>4p<sup>1</sup>
C)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>5</sup>3d<s up>10</sup>4s<sup>2</sup>4p<sup>1</sup>
D)1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<su p>2</sup>4d<sup>10</sup>4p<sup>1</sup>
E)none of the above
Q3) Electrons behave like particles and we can describe their exact paths.
A)True
B)False
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Page 11
Chapter 10: Chemical Bonding
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Sample Questions
Q1) When you have 4 electron groups and 1 of them is a lone pair,the molecular geometry is bent.
A)True
B)False
Q2) Which of the following has a tetrahedral electron geometry and a trigonal pyramidal molecular geometry?
A)Br<sub>2</sub>O
B)GeH<sub>4</sub>
C)SO<sub>2</sub>
D)PF<sub>3</sub>
E)none of the above
Q3) What is the electron geometry if you have 2 electron groups around the center atom?
A)linear
B)trigonal planar
C)tetrahedral
D)trigonal bipyramidal
E)not enough information
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Chapter 11: Gases
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Sample Questions
Q1) If you had a five liter balloon of argon gas and a five liter balloon of xenon gas,and you removed 10 grams of gas from each balloon,the balloons would both shrink down to the same size.
A)True
B)False
Q2) 1 atm is equal to:
A)760 mm Hg.
B)760 torr.
C)101,325 Pa.
D)14.7 psi.
E)all of the above
Q3) What is the pressure of a 1.0 L flask containing 0.60 g of He at 25°C? (R= 0.0821 L atm/ mol K)
A)98 atm
B)3.7 atm
C)7.3 atm
D)15 atm
E)none of the above
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Oil would be considered a nonvolatile liquid while gasoline would be considered volatile.
A)True
B)False
Q2) Which intermolecular force is the strongest?
A)dispersion forces
B)dipole-dipole forces
C)hydrogen bonding
D)X-forces
E)none of the above
Q3) Which atomic solid has the highest melting point?
A)Cu
B)Si
C)Xe
D)Fe
E)not enough information
Q4) Sublimation is the process of a liquid being converted directly to a gas.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) What is the mass percent of a solution prepared by dissolving 18.9 grams of solid into 39.5 grams of water?
A)47.8%
B)58.4%
C)32.4%
D)The identity of the compound must be known.
E)none of the above
Q2) Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water.
A)27.3
B)72.3
C)47.0
D)37.6
E)none of the above
Q3) A solution is a homogeneous mixture of two or more substances.
A)True B)False
Q4) Steel is an example of a solid solution. A)True B)False
Page 15
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Chapter 14: Acids and Bases
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Sample Questions
Q1) H<sub>2</sub>SO<sub>3</sub> and H<sub>2</sub>SO<sub>4</sub> are considered an acid-base conjugate pair.
A)True
B)False
Q2) In general,the stronger the acid,the weaker is its conjugate base.
A)True
B)False
Q3) A solution that has a pH of 8.5 is considered a weak base.
A)True
B)False
Q4) Which combination below will be a buffer solution?
A)HCl and Cl
B)HNO<sub>3</sub> and NaNO<sub>3</sub>
C)HC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> and NaC<sub>2</sub>H<sub>3</sub>O<sub>2</sub>
D)NaBr and NaOH
E)All of the above are true.
Q5) Bases feel slippery.
A)True
B)False
Page 16
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) A reversible reaction is one that can be stopped and then restarted as needed.
A)True
B)False
Q2) Le Chatelier's principle states that a chemical system must have a shift in direction in order to force the system to reach equilibrium.
A)True
B)False
Q3) Given N<sub>2</sub> (g)+ 3 H<sub>2</sub> (g) 2 NH<sub>3</sub> (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?
A)Place only N<sub>2</sub> into a sealed vessel.
B)Place only H<sub>2</sub> into a sealed vessel.
C)Place only NH<sub>3</sub> into a sealed vessel.
D)All of the above scenarios.
E)none of the above
Q4) A reaction that has K<sub>eq</sub> = 2.0 × 10<sup>8</sup> will have high concentrations of products.
A)True
B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Corrosion of metals may be prevented by keeping them dry at all times.
A)True
B)False
Q2) Oxidation involves which of the following?
1.Loss of electron(s).
2.Gain of electron(s).
3.Increase in oxidation state.
A)1 only
B)2 only
C)3 only
D)1 and 3 only
E)2 and 3 only
Q3) Corrosion is the:
A)oxidation of nonmetals.
B)loss of electrons.
C)oxidation of metals.
D)formation of an insoluble hydroxide.
E)none of the above
Q4) Distinguish between a galvanic (voltaic)cell and an electrolytic cell.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) All unstable elements have the same rates of radioactive decay.
A)True
B)False
Q2) Briefly distinguish between nuclear fission and nuclear fusion.
Q3) Radiation therapy involves:
A)radioactive isotopes that are used in place of x-rays.
B)radioactive isotopes that are absorbed by specific organs.
C)destroying cancerous cells by intense radiation levels.
D)acute radiation exposure.
E)none of the above.
Q4) Which of the following types of radiation has the highest penetrating power?
A)alpha particles
B)beta particles
C)gamma rays
D)positrons
E)none of the above
Q5) Madam Curie discovered two new elements.
A)True
B)False
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) What chemical reaction was used by the German chemist Friedrich Wohler to synthesize urea for the first time?
A)evaporating urine
B)heating ammonium cyanate
C)heating ammonium cyanide
D)combining the elements carbon,hydrogen,oxygen,and nitrogen
E)none of the above
Q2) Alkanes contain double and single bonds.
A)True
B)False
Q3) Organic compounds have to come from living things.
A)True
B)False
Q4) What are the product(s)of: C<sub>2</sub>H<sub>6 </sub>+ Cl<sub>2</sub> \(\to\) ?
A)C<sub>2</sub>H<sub>6</sub>Cl<sub>2</sub>
B)C<sub>2</sub>H<sub>4</sub>Cl<sub>2</sub> + H<sub>2</sub>
C)C<sub>2</sub>H<sub>5</sub>Cl + HCl
D)all of the above
E)none of the above
Page 20
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Chapter 19: Biochemistry
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Sample Questions
Q1) An example of a polysaccharide is:
A)glucose.
B)sucrose.
C)cellulose.
D)glycogen.
E)both C and D
Q2) A seven-carbon sugar is known as A)tetrose.
B)sevose.
C)hexose.
D)heptose.
E)none of the above
Q3) A codon is:
A)a series of three bases that specifies one of the twenty amino acids.
B)a series of three phosphates that specifies one of the twenty amino acids.
C)a series of three sugars that specifies one of the twenty amino acids.
D)a series of three proteins that specify one of the twenty amino acids.
E)none of the above
Q4) What is the difference between saturated and unsaturated fatty acids?
Q5) Summarize the main features of the four categories of protein structure.
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