Fundamentals of Chemistry Review Questions
Course Introduction
Fundamentals of Chemistry introduces students to the basic principles and concepts essential to understanding chemical phenomena. Topics include atomic and molecular structure, periodic properties of elements, chemical bonding, stoichiometry, states of matter, chemical reactions, thermochemistry, and basic concepts of acids, bases, and solutions. Emphasis is placed on developing scientific reasoning and problem-solving skills through theoretical concepts and practical laboratory techniques, providing a strong foundation for further study in chemistry and related sciences.
Recommended Textbook
Introductory Chemistry 5th Edition by Nivaldo J. Tro
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19 Chapters
2146 Verified Questions
2146 Flashcards
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Page 2
Chapter 1: The Chemical World
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59 Verified Questions
59 Flashcards
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Sample Questions
Q1) The properties of water do not depend on how the atoms are bonded together in the molecule.
A)True
B)False
Answer: False
Q2) Who discovered the law of conservation of mass?
A)John Dalton
B)Antoine Lavoisier
C)Nivaldo Tro
D)John Dalton and Antoine Lavoisier
E)none of the above
Answer: B
Q3) What are the important characteristics of the scientific method?
Answer: The important characteristics of the scientific method include the observation of phenomena,the formulation of a hypothesis to explain the observed phenomena,the testing of the hypothesis by experiment,and the formulation of laws and theories.
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Page 3
Chapter 2: Measurement and Problem Solving
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131 Verified Questions
131 Flashcards
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Sample Questions
Q1) The correct prefix for the multiplier 0.000001 is:
A)mega.
B)milli.
C)micro.
D)nano.
E)none of the above
Answer: C
Q2) There are 1000 kilometers in one meter.
A)True
B)False
Answer: False
Q3) Suppose a symmetrical metal rod of the element lead has a density of 11.4 g/cm<sup>3</sup>.If this rod is cut in half,the density of each piece is now 5.7 g/cm<sup>3</sup>.
A)True
B)False
Answer: False
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Page 4
Chapter 3: Matter and Energy
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Sample Questions
Q1) In calculating the relationship between the amount of heat added to a substance and the corresponding temperature change,the specific heat capacity is usually represented by which symbol?
A)C
B)q
C) T
D)m
E)K
Answer: A
Q2) Which of the following is NOT true?
A)The degree "symbol" is not used with the Kelvin scale.
B)A kelvin degree is the same size as a Celsius degree.
C)The Kelvin temperature scale avoids use of negative numbers.
D)Water boils at the same temperature value on both the Kelvin and Celsius scales.
E)none of the above
Answer: D
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Chapter 4: Atoms and Elements
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Sample Questions
Q1) What is the charge on a calcium atom that contains 18 e-?
A)1+
B)20+
C)2+
D)2-
E)none of the above
Q2) An atom of a carbon-14 isotope would contain:
A)6 protons,8 neutrons,and 6 electrons.
B)8 protons,6 neutrons,and 8 electrons.
C)6 protons,8 neutrons,and 8 electrons.
D)14 protons,6 neutrons,and 6 electrons.
E)20 protons,6 neutrons,and 20 electrons.
Q3) A fictional element has two isotopes and an atomic mass of 87.08 amu.If the first isotope is 86 amu and the second isotope has a mass of 90 amu.Which isotope has the greatest natural abundance?
A)86 amu
B)90 amu
C)There are equal amounts.
D)Not enough information provided.
E)none of the above
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) The phosphorous-to-hydrogen mass ratio is 10.2 for a compound.This ratio could correspond to the compound: A)PH.
B)PH<sub>2.</sub>
C)PH<sub>3.</sub>
D)PH<sub>6.</sub>
E)none of the above
Q2) Which formula shows the proper use of parentheses?
A)Ca(F)<sub>2</sub>
B)Ca(SO<sub>4</sub>)
C)(NH<sub>4</sub>)<sub>3</sub>(PO<sub>4</sub>)
D)Ca(NO<sub>3</sub>)<sub>2</sub>
E)none of the above
Q3) How many total atoms are in the formula Al<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub>?
A)8
B)9
C)12
D)14
E)none of the above
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Chapter 6: Chemical Composition
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Sample Questions
Q1) One mole of argon has more atoms in it than one mole of neon.
A)True
B)False
Q2) Which of the following contains 9.02 × 10<sup>23 </sup>atoms?
A)4.00 g H<sub>2</sub>
B)9.00 g H<sub>2</sub>O
C)28.0 g N<sub>2</sub>
D)32.0 g O<sub>2</sub>
E)none of the above
Q3) An estrogen compound with the empirical formula
C<sub>12</sub>H<sub>17</sub>O<sub>2</sub> has a molecular mass of 386.6 g/mol.What is the value of n necessary to find the molecular formula?
A)0.2
B)1
C)2
D)20
E)none of the above
Q4) Water is 11.2% hydrogen by mass.
A)True
B)False
Page 8
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) Which of the following compounds is SOLUBLE?
A)copper carbonate
B)calcium carbonate
C)potassium carbonate
D)strontium carbonate
E)none of the above
Q2) The following equation IS balanced: CH<sub>4</sub> + 2O<sub>2</sub>
CO<sub>2</sub> + H<sub>2</sub>O
A)True
B)False
Q3) What is the net ionic equation for the reaction of hydrochloric acid with potassium hydroxide?
A)H<sup>+</sup> + Cl<sup>-</sup> + K<sup>+</sup> + OH<sup>-</sup>
H<sub>2</sub>O + K<sup>+</sup> + Cl<sup>-</sup>
B)HCl + KOH H<sub>2</sub>O + KCl
C)H<sup>+</sup> + OH<sup>-</sup> H<sub>2</sub>O
D)2H<sup>+</sup> +2Cl<sup>-</sup> + K<sup>2+</sup> + 2OH<sup>-</sup>
H<sub>2</sub>O + K<sup>2+</sup> +2 Cl<sup>-</sup>
E)none of the above
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Page 9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Stoichiometry is a chemist's version of following a recipe.
A)True
B)False
Q2) How many grams of NO<sub>2</sub> are theoretically produced if we start with 1.20 moles of S and 9.90 moles of HNO<sub>3</sub>?
Reaction: S<sub> </sub>+ 6HNO<sub>3 </sub> H<sub>2</sub>SO<sub>4</sub> + 6NO<sub>2</sub> + 2H<sub>2</sub>O
A)7.20
B)331
C)455
D)786
E)not enough information
Q3) The limiting reactant is not necessarily the reactant with the least mass.
A)True
B)False
Q4) The limiting reactant determines what the actual yield is.
A)True
B)False
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) The elements will lose or gain electrons as needed to have an electron configuration that matches a noble gas.
A)True
B)False
Q2) Which form of electromagnetic radiation has the longest wavelength?
A)Radio Waves
B)Microwaves
C)X-rays
D)Gamma Rays
E)Infrared Radiation
Q3) The orbital diagram for fluorine shows 1 unpaired electron in a p orbital.
A)True
B)False
Q4) Which one of the following types of electromagnetic radiation has a higher energy per photon than visible radiation?
A)microwave
B)ultraviolet
C)radio
D)infrared
E)none of the above
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) The Lewis model predicts that the formula for a compound between barium and sulfur is:
A)BaS
B)Ba<sub>2</sub>S
C)BaS<sub>2</sub>
D)BaS<sub>3</sub>
E)none of the above
Q2) It is important to identify lone pairs around a central atom because they do not repel other electron groups.
A)True
B)False
Q3) What is the angle between electron groups in the linear electron geometry?
A)90°
B)109.5°
C)120°
D)180°
E)not enough information
Q4) The sulfate ion contains 28 valence electrons.
A)True
B)False
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Chapter 11: Gases
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Sample Questions
Q1) A "shielding gas" mixture of argon and carbon dioxide is sometimes used in welding to improve the strength of the weld.If a gas cylinder of this two-part mixture was at 4.0 atm pressure and this mixture was 90.% argon,what would be the pressure due to the carbon dioxide gas component?
A)3.6 atm
B)0.40 atm
C)10.atm
D)4.0 atm
E)none of the above
Q2) What is the final volume (L)of a 10.0 L system that has the pressure quartered?
A)0.250
B)17.1
C)2.50
D)40.0
E)none of the above
Q3) As we climb a mountain to a higher altitude,we experience a pressure decrease.
A)True
B)False
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13
Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Which statement about boiling point is FALSE?
A)The boiling point is higher for compounds with strong intermolecular forces.
B)The boiling point is higher for compounds with a high viscosity.
C)The boiling point of a compound is an absolute constant.
D)The boiling point of a compound is higher for nonvolatile compounds.
E)All of the above statements are true.
Q2) Which substance below is an ionic solid?
A)Cu (s)
B)H<sub>2</sub>O (s)
C)MgO (s)
D)C<sub>6</sub>H<sub>12</sub>O<sub>6 </sub>(s)
E)none of the above
Q3) Ice is an example of a molecular solid.
A)True
B)False
Q4) Ice can float in a glass of liquid water because the solid form of water is more dense than the liquid form.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) In order for a solute to dissolve in solution:
A)the solute-solvent forces must be greater than the solute-solute forces.
B)the solute-solute forces must be greater than the solute-solvent forces.
C)the solute-solvent forces must equal the solute-solute forces.
D)the polarity of the solute and solvent must be opposite.
E)none of the above
Q2) Air is an example of a gaseous solution.
A)True
B)False
Q3) The tragedy at Lake Nyos in Cameroon,West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.
A)True
B)False
Q4) A stock solution is a more concentrated form than what is typically used in a lab.It often requires further dilution.
A)True
B)False
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15
Chapter 14: Acids and Bases
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Sample Questions
Q1) A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?
A)H<sub>2</sub>S
B)H<sub>2</sub>SO<sub>4</sub>
C)HCl
D)Na<sub>2</sub>SO<sub>4</sub>
E)none of the above
Q2) A buffer solution is all of the following EXCEPT:
A)a solution that resists a change in pH when a base is added.
B)a solution that resists a change in pH when an acid is added.
C)a solution that contains both a weak acid and its conjugate base.
D)a solution that regulates pH because it is such a strong acid or base.
E)All of the above are true.
Q3) The sour taste of bases warns humans against eating poisonous alkaloids found in some plants.
A)True
B)False
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Page 16
Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Adding heat to an endothermic reaction causes the reaction to shift to the right.
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) Placing a [ ] around the formula of a chemical means that we are referring to the molar concentration of that chemical.
A)True
B)False
Q4) Le Chatelier's principle states that when a chemical system at equilibrium is disturbed,the system shifts in a direction that minimizes the disturbance.
A)True
B)False
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Distinguish between a galvanic (voltaic)cell and an electrolytic cell.
Q2) Alkaline batteries are used in automobiles.
A)True
B)False
Q3) What must be done to the following half-reactions before they can be added together?
Mn (s) Mn <sup>2+</sup>(aq)+ 2e<sup>-</sup>
Fe <sup>3+</sup> (aq)+ 3 e<sup>-</sup> Fe (s)
A)Double the Mn half-reaction.
B)Double the Mn half-reaction and triple the Fe half-reaction.
C)Triple the Mn half-reaction and double the Fe half-reaction.
D)Add H<sup>+</sup> ions to the left-side of the Mn reaction.
E)none of the above
Q4) The oxidizing agent typically:
A)loses electrons.
B)gains oxygen.
C)is the reactant that is reduced.
D)is oxidized.
E)none of the above
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Nuclear fusion:
A)is the formation of heavier elements from lighter ones.
B)releases a larger amount of heat than nuclear fission.
C)is the energy source of the sun and stars.
D)produces non-radioactive elements.
E)all of the above
Q2) A positron particle comes from the decay of a proton into a neutron and a positron.
A)True
B)False
Q3) One method of nuclear medicine uses radioactive isotopes to scan specific regions of the body.
A)True
B)False
Q4) Briefly distinguish between nuclear fission and nuclear fusion.
Q5) Carbon-14 dating is based on the fact that C-14 is continuously being made in the upper atmosphere.
A)True
B)False
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) The generic condensed structural formula for carboxylic acids is RCOOH.
A)True
B)False
Q2) Which of the following compounds is an alkene?
A)C<sub>2</sub>H<sub>6</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>4</sub>H<sub>6</sub>
D)C<sub>5</sub>H<sub>12</sub>
E)none of the above
Q3) Based on the molecular formulas shown below,which compound shown below could be classified as a cyclical alkane?
A)C<sub>4</sub>H<sub>10</sub>
B)C<sub>3</sub>H<sub>8</sub>
C)C<sub>5</sub>H<sub>12</sub>
D)C<sub>12</sub>H<sub>24</sub>
E)C<sub>9</sub>H<sub>20</sub>
Q4) Hydrocarbons contain carbon,hydrogen and oxygen.
A)True
B)False
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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) In the formation of a secondary protein structure,the primary protein structure is destroyed.
A)True
B)False
Q3) Carbohydrates provide short term energy storage in cells.
A)True
B)False
Q4) Which of the following is an unsaturated fatty acid?
A)oleic acid
B)palmitic acid
C)myristic acid
D)butyric acid
E)All of the above are saturated fatty acids.
Q5) Summarize the main features of the four categories of protein structure.
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