Basic Chemistry
Test Preparation
Course Introduction
Basic Chemistry offers an introduction to the fundamental concepts and principles of chemistry, providing a solid foundation for further study in the sciences. The course covers essential topics such as atomic structure, chemical bonding, periodic table trends, chemical reactions, stoichiometry, states of matter, and basic thermodynamics. Emphasis is placed on developing problem-solving skills, understanding chemical notation and equations, and safely conducting simple laboratory experiments. This course is designed to foster scientific literacy and critical thinking, equipping students with the knowledge and confidence to apply chemical principles to real-world situations and future coursework.
Recommended Textbook
Introductory Chemistry 6th Edition by Nivaldo J. Tro
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19 Chapters
2138 Verified Questions
2138 Flashcards
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Chapter 1: The Chemical World
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59 Verified Questions
59 Flashcards
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Sample Questions
Q1) Atoms and molecules determine how matter behaves.
A)True
B)False
Answer: True
Q2) Chemistry is the science that seeks to understand what matter does by studying living organisms.
A)True
B)False
Answer: False
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.
Q4) 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
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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) Scientific numbers are reported so that every digit is certain except the last,which is estimated.
A)True
B)False
Answer: True
Q3) How many milliliters are in 17.5 L?
A)175
B)1.75 × 10<sup>-2</sup>
C)1.75 × 10<sup>3</sup>
D)1.75 × 10<sup>4</sup>
E)none of the above
Answer: D
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Page 4
Chapter 3: Matter and Energy
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118 Verified Questions
118 Flashcards
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Sample Questions
Q1) Which of the following statements about physical and chemical changes is FALSE?
A)In a chemical change,matter changes its composition.
B)In a physical change,matter does not change its composition.
C)Phase changes are always physical changes.
D)Chemical reactions are chemical changes.
E)All of the above statements are true.
Answer: E
Q2) Which state of matter has atomic spacing that is close together and indefinite shape?
A)liquid
B)solid
C)gas
D)plasma
E)none of the above
Answer: A
Q3) Electrical energy is associated with the flow of electrical charge.
A)True
B)False
Answer: True
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Page 5
Chapter 4: Atoms and Elements
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112 Verified Questions
112 Flashcards
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Sample Questions
Q1) The names of the elements whose symbols are Si,P,Mn,and S are respectively:
A)silicon,potassium,magnesium,and sulfur.
B)silver,phosphorus,magnesium,and sulfur.
C)silicon,phosphorus,manganese,and sulfur.
D)silicon,phosphorus,magnesium,and sulfur.
E)silicon,potassium,magnesium,and sodium.
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) The atomic mass of individual atoms of an element may vary.
A)True
B)False
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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110 Flashcards
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Sample Questions
Q1) A student wrote the formula for the compound aluminum phosphate as AlPO<sub>4</sub>.What is wrong with this formula?
A)The compound is not charge-neutral.
B)Aluminum is a nonmetal so it cannot form an ionic compound.
C)The formula should be Al(PO<sub>4</sub>).
D)There cannot be three different atom types in a chemical formula.
E)Nothing is wrong with the formula.
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) What is the name of the compound whose formula is Na<sub>2</sub>O?
A)sodium monoxide
B)disodium oxide
C)disodium monoxide
D)sodium oxide
E)none of the above
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Page 7
Chapter 6: Chemical Composition
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118 Verified Questions
118 Flashcards
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Sample Questions
Q1) The empirical formula of a compound:
A)describes the mass relationships in a molecule.
B)is the same as the molecular formula.
C)indicates the structure of the molecule.
D)indicates the simplest ratio of atoms in the compound.
E)none of the above
Q2) There are 6 grams of carbon in 22 grams of carbon dioxide.
A)True
B)False
Q3) Vitamin C is known chemically by the name ascorbic acid.Determine the empirical formula of ascorbic acid if it is composed of 40.92% carbon,4.58% hydrogen,and 54.50% oxygen.
A)CHO
B)CH<sub>2</sub>O
C)C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>
D)C<sub>3</sub>H<sub>4</sub>O<sub>3</sub> E)none of the above
Q4) One hundred nickels must have the same mass as one hundred pennies. A)True B)False
Page 8
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Chapter 7: Chemical Reactions
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113 Verified Questions
113 Flashcards
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Sample Questions
Q1) The reaction 2 KClO<sub>3</sub> 2 KCl + 3 O<sub>2</sub> would be correctly classified as a decomposition reaction.
A)True
B)False
Q2) A precipitation reaction will occur when sodium chloride is mixed with potassium nitrate.
A)True
B)False
Q3) The reaction of baking soda and vinegar to produce carbon dioxide gas is an example of a precipitation reaction.
A)True
B)False
Q4) Sodium metal reacts with water to form aqueous sodium hydroxide and hydrogen gas.Which equation below best describes the balanced equation for this reaction?
A)Na + H<sub>2</sub>O NaOH (aq)+ H (g)
B)S + H<sub>2</sub>O SOH (aq)+ H (g)
C)Na + H<sub>2</sub>O NaOH (aq)+ H<sub>2</sub> (g)
D)2Na + 2H<sub>2</sub>O 2NaOH (aq)+ H<sub>2</sub> (g)
E)2Na + H<sub>2</sub>O Na<sub>2</sub>OH (aq)+ H (g)
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Chapter 8: Quantities in Chemical Reactions
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115 Verified Questions
115 Flashcards
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Sample Questions
Q1) Which is the excess reactant in the following reaction given that you start with 15.5 g of Na<sub>2</sub>S and 12.1 g CuSO<sub>4</sub>?
Reaction: Na<sub>2</sub>S + CuSO<sub>4 </sub> Na<sub>2</sub>SO<sub>4</sub> + CuS
A)Na<sub>2</sub>S
B)CuSO<sub>4</sub>
C)Na<sub>2</sub>SO<sub>4</sub>
D)CuS
E)not enough information
Q2) The limiting reactant determines what the actual yield is.
A)True
B)False
Q3) An exothermic reaction has a negative enthalpy of reaction.
A)True
B)False
Q4) If it takes 2 cups of milk and 1 cup of cocoa mix to make three servings of hot chocolate,and you only have 1 cup of each,then you cannot make any hot chocolate.
A)True
B)False
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Chapter 9: Electrons in Atoms and the Periodic Table
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111 Verified Questions
111 Flashcards
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Sample Questions
Q1) Which one of the following species has the electron configuration of 1s<sup>22s22p6</sup>?
1.Na<sup>+</sup>
2.O<sup>2-</sup>
3.F<sup>-</sup>
A)1 and 2 only
B)1 and 3 only
C)2 and 3 only
D)All of 1,2,and 3
E)Neither 1,2,or 3
Q2) When neon light is passed through a prism,what is observed?
A)continuous spectrum
B)nothing
C)bright spots or lines
D)white light
E)none of the above
Q3) Ultraviolet light produces suntans and sunburns.
A)True
B)False
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Chapter 10: Chemical Bonding
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109 Verified Questions
109 Flashcards
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Sample Questions
Q1) It is important to identify lone pairs around a central atom because they do not repel other electron groups.
A)True
B)False
Q2) What is the angle between electron groups in the tetrahedral geometry?
A)90°
B)109.5°
C)120°
D)180°
E)not enough information
Q3) The electron geometry and the molecular geometry of ammonia (NH<sub>3</sub>)are,respectively:
A)trigonal planar,bent.
B)tetrahedral,tetrahedral.
C)tetrahedral,trigonal pyramidal.
D)tetrahedral,bent.
E)none of the above
Q4) Drugs to fight HIV have been developed using bonding theory models.
A)True
B)False
Page 12
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Chapter 11: Gases
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123 Verified Questions
123 Flashcards
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Sample Questions
Q1) 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
Q2) If the number of gas particles is halved,the volume of the gas will be halved given that the temperature and pressure do not change.
A)True
B)False
Q3) Absolute zero refers to 0°C.
A)True
B)False
Q4) The expected order of density for matter is gases < liquids < solids.
A)True
B)False
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13
Chapter 12: Liquids, solids, and Intermolecular Forces
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115 Verified Questions
115 Flashcards
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Sample Questions
Q1) Consider the three compounds below,then choose the compound(s)that have hydrogen bonding.
1.H<sub>2</sub>
2.CH<sub>4</sub>
3.HF
A)Only compound 1 has hydrogen bonding.
B)Only compound 2 has hydrogen bonding.
C)Only compound 3 has hydrogen bonding.
D)All three of these compounds have hydrogen bonding.
E)None of these compounds have hydrogen bonding.
Q2) Which molecule below has hydrogen bonding?
A)CH<sub>4</sub>
B)HCl
C) H<sub>2</sub>
D) CH<sub>3</sub>CH<sub>2</sub>OH
E)all of the above
Q3) The rate of evaporation will increase if you pour a liquid out onto a large surface.
A)True
B)False
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14
Chapter 13: Solutions
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122 Verified Questions
122 Flashcards
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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) 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) How many moles of KCl are present in 95.3 mL of 2.10 M KCl?
A)0.0500
B)5.00
C)20.0
D)0.200
E)none of the above
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Chapter 14: Acids and Bases
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Sample Questions
Q1) What is the concentration of H in 0.50 M hydroiodic acid?
A)0.50 M
B)1.0 M
C)<0.50 M
D)1.50 M
E)none of the above
Q2) Which of the following statements about a base are TRUE?
1.Bases are used in the manufacturing of soap.
2.Bases have a sour taste.
3.Fertilizer manufacture and cotton processing use bases.
A)1 and 2 only
B)1 and 3 only
C)2 and 3 only
D)All of 1,2,and 3
E)Neither 1,2,or 3
Q3) A conjugate acid-base pair are two substances related to each other by the transfer of a proton.
A)True
B)False
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Page 16
Chapter 15: Chemical Equilibrium
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118 Flashcards
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Sample Questions
Q1) 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
Q2) For the reaction H<sub>2</sub> (g)+ Cl<sub>2</sub> (g) 2 HCl (g),what happens to the equilibrium position if the pressure increases?
A)shifts to the right
B)shifts to the left
C)does nothing
D)doubles
E)none of the above
Q3) 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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Page 17
Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) 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
Q2) If you properly balance the following half reaction in acid solution,how many electrons would appear on the product side of the equation? NO (g) NO<sub>3</sub><sup>1-</sup> (aq)
A)1
B)2
C)3
D)5
E)none of the above
Q3) The oxidizing agent is the substance being reduced. A)True
B)False
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) In a Geiger-Muller counter,radioactive particles pass through NaI which emits UV-Vis light.
A)True
B)False
Q2) When an atom emits an alpha particle,it becomes a different element.
A)True
B)False
Q3) A gamma ray has no charge and no mass.
A)True
B)False
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) One method of nuclear medicine uses radioactive isotopes to scan specific regions of the body.
A)True
B)False
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Chapter 18: Organic Chemistry
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108 Flashcards
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Sample Questions
Q1) Two compounds are considered as isomers if they have the:
A)same molecular formula AND different structure.
B)same molecular formula AND same structure.
C)different molecular formula AND different structure.
D)different molecular formula AND same structure.
E)same molecular formula OR same structure.
Q2) Aldehydes and ketones both contain a carbonyl group.
A)True
B)False
Q3) What are the products from the combustion of 2-methyl-3-ethyloctane?
A)variety of small hydrocarbons
B)carbon monoxide,carbon trioxide and water
C)carbon dioxide and water
D)carbon monoxide and water
E)none of the above
Q4) The formula of n-octane is:
CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>CH< sub>3</sub>
A)True
B)False
Page 20
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Chapter 19: Biochemistry
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110 Verified Questions
110 Flashcards
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Sample Questions
Q1) Which of the following is a complex carbohydrate?
A)monosaccharide
B)disaccharide
C)polysaccharide
D)all of these
E)none of these
Q2) The portion of the cell that contains the genetic information is called ________.
A)cytoplasm
B)membrane
C)nucleus
D)mitochondria
E)none of the above
Q3) Biochemistry is the study of chemical substances and processes that occur in plants,animals and microorganisms.
A)True
B)False
Q4) A gene is a portion of DNA that codes for a single protein.
A)True
B)False
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