Principles of Chemistry
Final Exam
Course Introduction
Principles of Chemistry provides a foundational understanding of chemical concepts, theories, and laboratory techniques essential for the study of the physical sciences. This course covers topics such as atomic structure, periodic properties, chemical bonding, stoichiometry, states of matter, solutions, chemical reactions, thermochemistry, and the basics of equilibrium and kinetics. Emphasis is placed on problem-solving and the application of chemical principles to everyday life and to further study in science and engineering disciplines.
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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Chapter 1: The Chemical World
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Sample Questions
Q1) If experimental results contradict a hypothesis,the hypothesis must be either revised or discarded.
A)True
B)False
Answer: True
Q2) Quantification is an important tool in understanding chemistry.
A)True
B)False
Answer: True
Q3) When a sealed can of soda pop is opened,the carbon dioxide gas fizzes out because the pressure is released.
A)True
B)False
Answer: True
Q4) Both carbon dioxide molecules and water molecules consist of three atoms bonded together in a straight line.
A)True
B)False
Answer: False
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Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) The correct prefix for the multiplier 0.1 is:
A)tera.
B)deci.
C)femto.
D)pico.
E)none of the above
Answer: B
Q2) One mile measures 5,280 feet long,so one square mile is equivalent to 5,280 square feet.
A)True
B)False Answer: False
Q3) You do not need to write units in calculations as long as you can remember them.
A)True
B)False Answer: False
Q4) The prefix nano represents the multiplier 0.000000001.
A)True
B)False Answer: True
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Chapter 3: Matter and Energy
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Sample Questions
Q1) An energy diagram that shows the products having higher energy than the reactants illustrates an endothermic reaction.
A)True
B)False
Answer: True
Q2) Chemical properties of a substance are those that can be observed without changing the composition of a substance.
A)True
B)False
Answer: False
Q3) Temperature is simply a measure of the motion of atoms and molecules. A)True
B)False
Answer: True
Q4) Skim milk is a heterogeneous mixture.
A)True
B)False
Answer: False
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Page 5
Chapter 4: Atoms and Elements
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Sample Questions
Q1) The elements within a group on the periodic table tend to have similar properties.
A)True
B)False
Q2) When an atom gains an electron,the resulting particle is called:
A)a proton.
B)an anion.
C)a cation.
D)an isotope.
E)none of the above
Q3) What is the atomic symbol for silver?
A)S
B)Ag
C)Au
D)Si
E)none of the above
Q4) If two atoms each contain different numbers of protons,the atoms must be from different elements.
A)True
B)False
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Chapter 5: Molecules and Compounds
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Sample Questions
Q1) Which formula shown is incorrect for the name given?
A)magnesium nitrite: Mg(NO<sub>2</sub>)<sub>3</sub>
B)calcium carbonate: CaCO<sub>3</sub>
C)aluminum sulfate: Al<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>
D)sodium hydrogen carbonate: NaHCO<sub>3</sub>
E)potassium hydroxide: KOH
Q2) What is the formula for an ionic compound made of magnesium and sulfur?
A)MgS
B)MgS<sub>2</sub>
C)Mg<sub>2</sub>S
D)Mg<sub>2</sub>S<sub>3</sub>
E)none of the above
Q3) What is the proper name for HBr (aq)?
A)hydrobromous acid
B)hydrousbromic acid
C)hydrobromic acid
D)bromous acid
E)none of the above
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Chapter 6: Chemical Composition
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Sample Questions
Q1) 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
Q2) One mole of CO<sub>2</sub> gas contains 1 mole of carbon atoms and 2 moles of oxygen atoms.
A)True
B)False
Q3) The simplest formula for hydrogen peroxide is HO.To determine its molecular formula,it is necessary to know:
A)the properties of hydrogen peroxide.
B)the density of hydrogen peroxide.
C)the molar mass of hydrogen peroxide.
D)the number of moles of hydrogen peroxide in 1.00 g of the substance.
E)none of the above
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8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) In an oxidation-reduction reaction,if one substance loses electrons,then another substance must gain electrons.
A)True
B)False
Q2) When solid NaCl is stirred into water,which of the following is NOT true?
A)Individual sodium and chloride ions are present.
B)The solution will conduct electricity.
C)The solution will taste salty.
D)The NaCl will fail to dissociate.
E)none of the above
Q3) Considering the following precipitation reaction:
Pb(NO<sub>3</sub>)<sub>2</sub>(aq)+ 2KI(aq)
2KNO<sub>3</sub>(aq)
Which ion would NOT be present in the complete ionic equation?
A)Pb<sup>2+</sup>
B)K<sup>+</sup>
C)NO<sub>3</sub><sup>-</sup>
D)I<sup>-</sup>
E)All the above ions are in the complete ionic equation.
PbI<sub>2</sub>(s)+
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Page 9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Given the reaction: 2 Na(s)+ Cl<sub>2</sub>(g) 2 NaCl(s) The conversion factor for chlorine gas to sodium chloride is: 1 mol Cl<sub>2 </sub> 2 mol NaCl
A)True
B)False
Q2) The primary source for the rising carbon dioxide levels is respiration of the Earth's growing population.
A)True
B)False
Q3) Given the chemical equation: 2 Ca + O<sub>2</sub> 2 CaO, if 2 moles of CaO are formed in this reaction,then 2 moles of O<sub>2</sub> must have reacted.
A)True
B)False
Q4) 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
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) Bromine has 28 core electrons.
A)True
B)False
Q2) Which of the atoms represented below is the largest in size?
A)N
B)As
C)Sb
D)Bi
E)P
Q3) An accepted abbreviation format is to write an electron configuration that includes a noble gas symbol in brackets.If you were writing an electron configuration for a bromine atom,which elemental symbol would you place in the bracket?
A)He
B)Ne
C)Ar
D)Kr
E)Xe
Q4) Blue light travels at a faster speed than red light.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) The triple bond present in diatomic nitrogen,N<sub>2</sub>,is what makes this molecule so reactive.
A)True
B)False
Q2) The VSEPR theory predicts that the angle between the central carbon atom and the two oxygen atoms in CO<sub>2</sub> measures 180°.
A)True
B)False
Q3) The Lewis structure of water has two sets of lone pair electrons.
A)True
B)False
Q4) Boron forms compounds that violate the octet rule.
A)True B)False
Q5) Li : is the proper Lewis structure (dot structure)for lithium. A)True
B)False
Q6) Carbon monoxide contains resonance Lewis structures. A)True B)False
Page 12
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Chapter 11: Gases
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Sample Questions
Q1) Which conditions can cause nonideal gas behavior by 1)decreasing the space between gas particles or 2)by slowing gas particles so that interactions are significant?
A)1)high pressure;2)high temperature
B)1)high pressure;2)low temperature
C)1)low pressure;2)high temperature
D)1)low pressure;2)low temperature
E)none of the above
Q2) If the kelvin temperature of a gas is doubled,the volume is doubled provided that the pressure and the number of particles remains constant.
A)True
B)False
Q3) There is a large distance between gas particles as compared to their relative size. A)True B)False
Q4) Gases and liquids are compressible,but solids are not.
A)True
B)False
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13
Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Dispersion forces result from the temporary distortion of the electron cloud in an atom or molecule which increases in magnitude with increasing size.
A)True
B)False
Q2) Which substance below has dipole-dipole forces?
A)CH<sub>4</sub>
B)CO<sub>2</sub>
C)F<sub>2</sub>
D)H<sub>2</sub>S
E)none of the above
Q3) The shapes of protein molecules are determined by intermolecular forces.
A)True
B)False
Q4) Dipole-dipole forces are weaker than dispersion forces.
A)True
B)False
Q5) The rate of evaporation will increase if you pour a liquid out onto a large surface.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) Vitamin C is a water-soluble vitamin,so it is likely that this vitamin is polar.
A)True
B)False
Q2) 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
Q3) Which of the following substances is NOT a solution?
A)air
B)brass
C)vodka
D)copper
E)All of the above are solutions.
Q4) A 0.10 molality solution of the sugar glucose (molecular weight = 180.10 g/mol)and a 0.10 molality solution of sucrose (molecular weight = 342.34 g/mol)would both boil at the same temperature.
A)True
B)False
Page 15
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Chapter 14: Acids and Bases
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Sample Questions
Q1) A strong acid is one that is very concentrated.
A)True
B)False
Q2) The pH of a 0.0001 M NaOH solution is 4.
A)True
B)False
Q3) Which solution below is considered to have basic character?
A)pOH = 7
B)pH = 2
C)pOH = 4
D)pOH = 13
E)none of the above
Q4) The products of a neutralization reaction are carbon dioxide and water.
A)True
B)False
Q5) In a titration,the indicator is used to signal when the endpoint has been reached.
A)True
B)False
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) For a given chemical equation,the coefficients for each substance become the exponents for each substance in the written equilibrium expression.
A)True
B)False
Q2) What happens to the equilibrium constant when a catalyst is added to the reaction mixture?
A)increases
B)decreases
C)does not change
D)varies
E)none of the above
Q3) Which of the following changes will increase the reaction rate?
A)an increase in the concentration of the products
B)a decrease of the reaction temperature
C)allowing more time for the reaction
D)an increase in the concentration of reactants
E)all of the above
Q4) The rate of a chemical reaction is inversely proportional to the temperature.
A)True
B)False
Page 17
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) Balance the following half reaction in base solution: H<sub>2</sub>0 (l) H<sub>2</sub> (g)
A)2H<sub>2</sub>O (l)+ 2 e<sup>-</sup> H<sub>2</sub> (g)+ 2 OH<sup>-</sup> (aq)
B)2H<sub>2</sub>O (l) 2H<sub>2</sub> (g)+ 2 e<sup>-</sup> + O<sub>2</sub>
C)2H<sub>2</sub>O (l) H<sub>2</sub> (g)+ 2 H<sup>+</sup> + 2e<sup>-</sup>
D)H<sub>2</sub>O (l) 2H<sup>+</sup> + 2OH<sup>-</sup>
E)2H<sub>2</sub>O (l) H<sub>2</sub> (g)+ 2OH<sup>-</sup> (aq)+ 5 e<sup>-</sup>
Q2) Alkaline batteries are used in automobiles.
A)True
B)False
Q3) An electrolytic cell is a spontaneous redox reaction.
A)True
B)False
Q4) Reduction typically involves:
A)the loss of electrons.
B)the gain of oxygen.
C)the gain of electrons.
D)the gain of water.
E)none of the above
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Nuclear power plants produce energy by fission reactions.
A)True
B)False
Q2) The effort to build an atomic bomb during WWII was prompted by a fear that Germany was already working on nuclear weapons.
A)True
B)False
Q3) The radioactive gas radon:
A)is a product of the radioactive decay series of uranium.
B)is the single greatest source of human radiation exposure.
C)is more hazardous for smokers than nonsmokers.
D)all of the above
E)none of the above
Q4) Madam Curie discovered two new elements.
A)True
B)False
Q5) A nuclide with a shorter half-life would be considered more active than a nuclide with a longer half-life.
A)True
B)False
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Even though the aromatic ring of the compound benzene can be drawn with alternating single and double bonds,all the carbon to carbon bonds are the same.
A)True
B)False
Q2) 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
Q3) What is the formula for propyne?
A)C<sub>3</sub>H<sub>8</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>3</sub>H<sub>4</sub>
D)C<sub>3</sub>H<sub>3</sub> E)none of the above
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Chapter 19: Biochemistry
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Sample Questions
Q1) What is the difference between saturated and unsaturated fatty acids?
Q2) Humans must synthesize some of the proteins they need because they cannot obtain them from the foods they eat.
A)True
B)False
Q3) How many total number of DNA bases are needed to code for the amino acids in a protein containing 27 amino acids?
A)9
B)27
C)81
D)4
E)none of the above
Q4) The most common repeating pattern that is found along the secondary structure of a protein chain is:
A) -helix.
B) -pleated sheet.
C) -turn.
D)random coil.
E)none of the above
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