Introductory Chemistry Exam Preparation Guide
Course Introduction
Introductory Chemistry provides a foundational exploration of the principles and concepts essential to understanding the nature and behavior of matter. This course covers key topics such as atomic structure, chemical bonding, stoichiometry, states of matter, chemical reactions, and the periodic table. Emphasis is placed on developing problem-solving skills, conducting basic laboratory experiments, and applying chemical principles to everyday life scenarios. Designed for students with limited background in chemistry, the course prepares learners for advanced studies by fostering scientific reasoning and analytical thinking.
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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Sample Questions
Q1) What is chemistry?
Answer: Chemistry is branch of science that explains the properties and behavior of different forms of matter,in the broadest sense,by helping us understand the atoms and molecules that compose them.
Q2) 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.
Q3) A hypothesis can never be proven as wrong.
A)True
B)False
Answer: False
Q4) The first step in acquiring scientific knowledge is often the observation or measurement of some aspect of nature.
A)True
B)False
Answer: True
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3
Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) The base unit of length in the SI system is the cm.
A)True
B)False Answer: False
Q2) You do not need to write units in calculations as long as you can remember them.
A)True
B)False Answer: False
Q3) How many significant figures are in the number 2903?
A)2
B)5
C)4
D)3
E)none of the above Answer: C
Q4) When the number 2.35 is rounded to contain 2 significant figures it becomes 2.4.
A)True
B)False Answer: True
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Chapter 3: Matter and Energy
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Sample Questions
Q1) All of the following can be considered physical properties EXCEPT:
A)taste.
B)color.
C)flammability.
D)density.
E)boiling point.
Answer: C
Q2) Which of the following statements about energy is FALSE?
A)An object possessing energy can do work on another object.
B)Energy can neither be created nor destroyed.
C)Energy is the single main component of the universe.
D)Energy is the capacity to do work.
E)All of the above statements are true.
Answer: C
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) The smell of the ocean is caused by atoms.
A)True
B)False
Q2) An element is discovered that is a solid,has one valence electron,and readily forms a 1+ ion.This element would be correctly classified as a nonmetal.
A)True
B)False
Q3) There is very little of the element astatine (symbol = At)on earth.If astatine formed an ion,it would most likely have the charge of:
A)1+
B)1-
C)2+
D)2-
E)none of the above
Q4) The nucleus of an atom is a very small,dense region that contains over 99.9% of the atomic mass.
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 name of the molecular compound SF<sub>5</sub>?
A)sulfur hexafluoride
B)sulfur heptafluoride
C)monosulfur tetrafluoride
D)sulfur pentafluoride
E)none of the above
Q3) Suppose that in an ionic compound,"M" represents a metal that could form more than one type of ion.In the formula MP ,the charge of the M ion would be:
A)+1
B)-1
C)+2
D)-3
E)+3
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Page 7
Chapter 6: Chemical Composition
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Sample Questions
Q1) The mole has a value of 6.023 × 10<sup>22</sup>.
A)True
B)False
Q2) A 7.96 gram sample of silver reacts with oxygen to form 8.55 gram of the metal oxide.What is the formula of the oxide?
A)AgO
B)AgO<sub>2</sub>
C)Ag<sub>2</sub>O
D)Ag<sub>3</sub>O
E)none of the above
Q3) How many moles of Pb are in 4.71 × 10<sup>21</sup> Pb atoms?<sup> </sup>
A)0.00782
B)2.84 × 10<sup>45</sup>
C)207.2
D)6.022 × 10<sup>23</sup>
E)none of the above
Q4) One mole of water contains 16 grams of oxygen atoms.
A)True
B)False
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Chapter 7: Chemical Reactions
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Sample Questions
Q1) Which of the following types of compounds will NOT undergo a gas evolution reaction when acid is added?
A)sulfides
B)carbonates
C)hydroxides
D)bisulfites
E)none of the above
Q2) When balancing a chemical equation you may alter the coefficients but not the subscripts in the equation.
A)True
B)False
Q3) What type of a reaction occurs when a hydrochloric acid solution is mixed with a sodium bicarbonate solution?
A)precipitation
B)acid-base neutralization
C)oxidation-reduction
D)gas evolution
E)no reaction
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Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) How many moles of chlorine gas are needed to make 0.6 moles of sodium chloride?
Given the reaction: 2Na + Cl<sub>2</sub> 2NaCl
A)0.6
B)0.3
C)1.2
D)3.6
E)not enough information
Q2) How many grams of water are made from the reaction of 4.0 grams of hydrogen gas?
Given the reaction: 2H<sub>2</sub> + O<sub>2</sub> 2H<sub>2</sub>O
A)18
B)72
C)36
D)4.5
E)not enough information
Q3) Global warming is due to the greenhouse gases preventing heat from Earth escaping into space.
A)True
B)False
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Page 10
Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) A principal shell with a value of n=3 would contain s,p,d,and f orbitals.
A)True
B)False
Q2) What happens to an atom when it absorbs energy?
A)The atom stores the energy for later use.
B)The extra energy increases the speed of the electrons in their orbitals.
C)The atom re-emits the energy as heat.
D)The atom re-emits the energy as light.
E)none of the above
Q3) Which form of electromagnetic radiation has the shortest wavelength?
A)Radio Waves
B)Microwaves
C)X-rays
D)Gamma Rays
E)Infrared Radiation
Q4) The great success of the Bohr model of the atom is that it predicted the emission spectrum lines of multi-electronic elements like helium.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) Which term matches the definition: The ability of an element to attract electrons within a covalent bond?
A)coulombic attraction
B)dipole moment
C)polar covalent
D)nonpolar covalent
E)electronegativity
Q2) What is the molecular geometry if you have 4 single bonds around the central atom?
A)bent
B)linear
C)tetrahedral
D)trigonal pyramidal
E)not enough information
Q3) Which compound below is a polar molecule AND has a linear molecular geometry?
A)CO
B)CO<sub>2</sub>
C)CH<sub>4</sub>
D)H<sub>2</sub>O
E)none of the above
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Chapter 11: Gases
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Sample Questions
Q1) What is the equivalent pressure of 968 mm Hg in units of atm?
A)1.27 atm
B)0.785 atm
C)968 atm
D)1.30 atm
E)none of the above
Q2) If each of the following gas samples have the same temperature and pressure,which sample has the greatest volume?
A)1 gram of O<sub>2</sub>
B)1 gram of Ar
C)1 gram of H<sub>2</sub>
D)all have the same volume
E)not enough information
Q3) Which set of conditions reflect STP?
A)298 K,1 atm
B)25°C,14.7 psi
C)373 K,760 torr
D)273 K,1 Pa
E)273 K,760 mm Hg
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Page 13
Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Which intermolecular force is the strongest?
A)dispersion force
B)dipole-dipole force
C)hydrogen bonding
D)ion-dipole force
E)none of the above
Q2) Gases typically have high densities in comparison to solids.
A)True
B)False
Q3) Which statement about surface tension is FALSE?
A)Liquids tend to minimize their surface area.
B)Molecules on the surface of the liquid have fewer molecules to interact with.
C)Increased intermolecular forces increase surface tension.
D)Items with densities lower than water will sink due to surface tension.
E)All of the above statements are true.
Q4) Intermolecular forces hold atoms and molecules in place in a solid.
A)True
B)False
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14
Chapter 13: Solutions
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Sample Questions
Q1) Why is it NOT a good idea to drink seawater when people are lost at sea?
A)The high concentration of salt forces water out of the cells lining your stomach and intestine.
B)The osmotic pressure builds up in the cells of your intestine until they potentially rupture.
C)The semipermeable membrane protecting your stomach is ruptured during osmosis.
D)The seawater has fish urine in it and who wants to drink that?
E)none of the above
Q2) When a chunk of gold is melted and poured into the shape of an ingot,an aqueous solution of gold has been created.
A)True
B)False
Q3) How many moles of NaF are in 34.2 grams of a 45.5% by mass NaF solution?
A)0.814
B)75.2
C)15.6
D)0.371
E)none of the above
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15
Chapter 14: Acids and Bases
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Sample Questions
Q1) A solution of pH 2 contains ten times more H<sub>3</sub>O<sup>+ </sup>than a solution of pH 3.
A)True
B)False
Q2) Which of the following acids is a monoprotic,strong acid?
A)sulfuric acid
B)phosphoric acid
C)hydrobromic acid
D)carbonic acid
E)none of the above
Q3) Which solution below has the highest concentration of hydroxide ions?
A)pH = 3.21
B)pH = 12.49
C)pH = 7.00
D)pH = 10.12
E)pH = 7.93
Q4) Bases have a bitter taste.
A)True
B)False
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Which of the following is TRUE for a system that is in dynamic equilibrium?
A)The forward reaction goes to 100% completion.
B)The reaction rate of the forward reaction approaches zero.
C)The concentration of products is equal to the concentration of the reactants.
D)Both the forward and reverse reactions come to a halt.
E)none of the above
Q2) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
A)True
B)False
Q3) It is not necessary to have a balanced equation before writing an equilibrium constant expression.
A)True
B)False
Q4) Which of the following is FALSE about enzymes?
A)They act as biological catalysts.
B)They lower the activation energy of biological reactions.
C)They increase the temperature of biological reactions to speed them up.
D)They are highly specific in their catalytic activity.
E)none of the above
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Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) The oxidizing agent is the substance being reduced.
A)True
B)False
Q2) Which battery system is based on half reactions involving zinc metal and manganese dioxide?
A)alkaline batteries
B)fuel cells
C)lead-acid storage batteries
D)dry-cell batteries
E)none of the above
Q3) Which fact about fuel cells is FALSE?
A)Fuel cell automobiles are powered by water and the only emission is hydrogen.
B)Fuel cells are based on the tendency of some elements to gain electrons from other elements.
C)Fuel cell automobiles are whisper quiet.
D)Fuel cell automobiles are environmentally friendly.
E)all of the above
Q4) The oxidation number of a chlorine atom is -1.
A)True
B)False
Page 18
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) What happens to the mass number of a nucleus that emits a positron?
A)It remains the same.
B)It increases by one.
C)It decreases by one.
D)It increases by two.
E)It decreases by two.
Q2) Which fact about carbon-14 dating is FALSE?
A)C-14 is formed by neutron bombardment of nitrogen in the upper atmosphere.
B)C-14 dating can only work on items that come from a living source.
C)C-14 dating only works as far back as 50,000 years.
D)C-14 accuracy is verified by dating antique items of a known age.
E)All of the above statements are true.
Q3) The self-amplifying reaction in which neutrons produced by the fission of one nucleus would induce fission in other nuclei is called:
A)critical mass.
B)chain reaction.
C)nuclear fusion.
D)positron emission.
E)none of the above
Q4) Briefly distinguish between nuclear fission and nuclear fusion.
Page 19
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Hydrocarbon combustion reactions are highly endothermic - they absorb large amounts of heat.
A)True
B)False
Q2) Compare a six-carbon open-chain (noncyclic)hydrocarbon alkane,alkene,and alkyne.Which of these compounds would have the fewest number of hydrogen atoms?
A)the alkane
B)the alkyne
C)the alkene
D)all of these have the same number of hydrogen atoms
E)none of these contain hydrogen atoms
Q3) Which of the following statements is FALSE about polymers?
A)Several monomer units link together without eliminating any atom or group to form addition polymers.
B)During condensation polymerization an atom or group is eliminated.
C)Copolymers contain more than one kind of monomer.
D)Nylon 6,6 and polyurethane are examples of copolymers.
E)none of the above.
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Page 20
Chapter 19: Biochemistry
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Sample Questions
Q1) Protein synthesis occurs at the ribosome.
A)True
B)False
Q2) Monosaccharides typically rearrange in aqueous solution to form double helix structures.
A)True
B)False
Q3) Which base is found in RNA but NOT in DNA?
A)uracil
B)thymine
C)guanine
D)cytosine
E)adenine
Q4) Saturated fats tend to be solid at room temperature.
A)True
B)False
Q5) Fatty acids differ only in their "R" group.
A)True
B)False
Q6) Summarize the main features of the four categories of protein structure.
Page 21
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