Chemistry Exam Review Sheet
The midterm exam includes Chapters 1-9 and Chapter 21 in the Holt Modern Chemistry Book. Any additional topics that
were covered in class through notes, labs, sample problems, worksheets, and etc. are also fair game for the test. The
Chapter Highlights at the end of each chapter and Chapter Reviews are a great place review. Good Luck!!!
Unit 1 – Safety, Measurement, and Classification of Matter (Chapters 1 & 2)
• Safety
o See Safety Contract and Safety Lab
o Intro pages xviii – xxi
• Measurement with metric system and SI base units (pp 33 – 42)
o Practice p. 40 and p. 42
o Section Review p. 42
o Chapter review p. 59 # 5 – 10
• Density w/ graphical analysis (mass vs. volume) (pp. 38 – 40)
o Practice p. 40
o Chapter Review p. 59 # 16 -19
• Significant Figures (p 46 – 50)
o Sample Problem D p. 47
o Practice 1 & 2 p. 48
o Sample Problem E p. 49
o Practice 1 – 4 p. 50
o Chap. Review p. 60 # 29, 30, 40, 41
• Scientific Notation (50 – 54)
o Sample Problem F p. 54
o Practice p. 54 1 – 4
o Chapter Review p. 60 # 31, 43, 44
• Unit Conversions w/ Dimensional Analysis (pp. 40 – 42)
o Be able to perform conversions between metric prefixes
• Theory vs. Law (pp. 29 – 32)
o Section Review p. 31 # 1 – 5
o Chapter Review p. 59 # 1 – 3
• Accuracy vs. Precision (pp. 44 – 45)
o Practice p. 45 # 1 – 2
• Quantitative vs. Qualitative Data (p. 29)
o Define and distinguish between the two, also, be able to provide examples
• What is Chemistry? What is a chemical? (pp. 3 – 4)
o Section Review p. 5 # 1 – 4
o Chapter Review p. 22 # 1 & 3
• Extensive and Intensive Properties of Matter (p. 7)
o Chapter Review p. 22 # 9
• Chemical and Physical Properties and Changes (p. 7 – 10)
o Section Review # 1 – 4
o Chapter Review p. 22 # 10 – 13
• Differentiate between Atoms, Elements, Compounds, and Mixtures
• Classification of Matter Flowchart
o Look at your notes
• Homogenous vs. Homogenous Mixtures (p. 12)
o Define and distinguish between the two, also, be able to provide examples
• Characteristics of States of Matter and State Changes
Unit 2 History of the Atom, Atomic Structure w/Isotopes, Electron Configuration, Nuclear Decay, and Energy
(Chapter 3 – Chapter 5 and Chapter 21)
• History of the Atom (Democritus p. 67, Lavosier p. 303, Mendeleev p. 133-134)
• Rutherford’s Gold Foil Experiment (p. 74)
• Dalton’s Atomic Theory (5 parts, some that are not correct) (p. 68)
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Law of Conservation of Mass
o Section Review p. 71 #3
Composition of an Atom (protons, neutrons, electrons) (p. 75)
Nuclear Notation ( ZA X ) and Isotopes (pp. 77 – 80)
o Practice # 1 - 3
Determination of Protons, Neutrons, and Electrons from Periodic Table or Nuclear Notation
Periodic Table Development (Hint: Nuts and Bolts Lab)
Periodic Table Organization (Groups, Periods, Atomic #) (p. 135)
Periodic Trends (Atomic Radius, Electronegativity, Ionization Energy) (p. 151, 161 – 162)
o Section Review p.166 #5-7, 16 b, 22-23, 27-32
Isotopes w/ weighted average atomic mass (pg. 82)
Bohr Atomic Model (2, 8, 8, 18 …)
Modern Atomic Model w/ Electron Orbitals (s, p, d, f) (p. 107-110)
Electron Configuration (Longhand and Noble Gas Configuration) (p. 111-122)
o Chapter Review p. 125 #32-33e, 34-41
Electron Orbitals (shapes, # electrons in each, periodic table location) (p. 108, 111-122)
o Chapter Review p.125 #22-24
Electron Orbital Diagram Rules (Aufbau, Hund’s, Pauli Exclusion) (p.111-112)
o Chapter Review p. 125 #26-28a
Orbital Diagrams
o Chapter Review p. 125 # 31
Families of Elements (ex. Noble Gases) and Periodic Table Location (p. 142-148)
Properties of & Periodic Table Location of Metals, Nonmetals, and Metalloids
o Look at the periodic table you colored
Properties of Elements in Groups (Alkali Metals, Noble Gases)
o Chapter Review p. 125-126 #30, 31, 43e, 48
o p. 166 #8-16a, 17-21
o p. 129 #7-9, 11
Balancing Nuclear Equations and Types of Nuclear Decay (pgs. 681 – 687)
o Practice and Section Review pg. 684
Radioactive Decay and Half-life Calculations (pgs. 688-689)
o Practice pg. 689
Nuclear Fission and Fusion (pgs. 697-699)
Emission Spectra and Energy Calculations (pg. 97 – 103)
o Refer to notes for sample calculations and wave properties
o Flame Test
Unit 3 Chemical Formulas, Chemical Bonding, and Chemical Equations (Chapters 6 – 8)
• What is a Chemical Bond? Why do most atoms bond? (p. 175 intro)
o Section Review p. 177 #1
• Properties of Ionic and Covalent Bonds (p.175-177, 190-194)
o Section Review p. 194 #4
• Types of Elements that form Ionic and Covalent Bonds
o Section Review p. 177 #2-4, Section Review p. 194 #1
• Molecule vs. Compound (p. 179)
• Periodic Trend for Valence Electrons
• Octet and Duet Rule with Exceptions (p.182-183)
o Section Review p. 189 # 2
• Lewis Dot Structures and Resonance Structures (p.184-187)
o Section Review p.189 #3-4
o Practice p.188 #1-2, p.186 #1-4
• Polarity and Electronegativity (p.176, 204-205)
o Chapter Review p. 209 #6, 38-39, 46
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VSEPR Theory and Molecular Shape (p. 197-200)
o Chapter Review p.210 #33a, p. 212 #60
Hybridization of Atomic Orbitals (pg. 201 – 203)
Intermolecular Forces (pg. 203 – 207)
Naming Covalent Compounds (hint: know the prefixes!!) (p.227-229)
o Practice p. 229 #1-2
o Section Review p. 231 #2-4
o Chapter Review p. 251 #2-11, 16-18, p.253 #44, p.254 #48
Ions and Ionic Charges (Common Ion Sheet) (p. 219-221)
Writing Ionic Formulas (p. 222-226)
o Practice p.223 #1-2
Naming Ionic Compounds (p. 222-226)
o Practice p. 225 #1-2, p.227 #1-2
Formula Mass/Molar Mass (pgs. 237-242)
o Practice pg. 239
o Practice pg. 242
Percentage Composition (pgs. 242-244)
o Practice and Section Review pg. 244
Calculation of Empirical and Molecular Formula (245 – 249)
o Practice pg. 247
o Practice and Section Review pg. 249
Chemical Equations (reactants, products) (p.262-267)
o Section Review p. 274 #1
Chemical Reactions and Evidence (p. 261-262)
o Think about Copper Recycle Lab
Counting Atoms in a Compound (see balancing worksheets)
o Chapter Review p. 290 # 10
Coefficients and Subscripts in Chemical Formulas and Equations(p. 263)
Balancing Chemical Equations (p. 270-272)
o Practice p. 268 # 1-3, p. 272 # 1-2, p. 274 # 1
o Section Review p. 274 # 2-5
Diatomic Elements: GEN U INE / Magic 7 Elements / HON Halo / BrINClHOF
Types of Chemical Reactions (p. 276-284)
o Section Review p. 284 #1-5
o CHAPTER REVIEW p. 290-291 #1-6, 8, 11-15, 17-18, 22-23, 24-30, 38, 41, 43-44, 47
Predicting Products of Chemical Reactions
Activity Series of Metals with Single Replacement Reactions (pg. 285 – 287)
o Practice and Section Review pg. 287
Solubility Rules and Precipitate Formation with Double Replacement Reactions
o Solubility Rules handout
Unit 4 Stoichiometry (Chapter 3, pgs. 82 – 87 and Chapter 9)
• Basic Mole Conversions (molg, gmol, molmolecule, moleculemol, moleculeg, and gmolecule)
o Both Practice pg. 85
o Practice pg. 86
o Practice and Section Review pg. 87
• Stoichiometric Calculations (molAmolB, gAmolB, molAgB, gAgB)
o Section Review pg. 301
o Practice pg. 306
o Practice pg. 308
o Practice pg. 309
o Practice and Section Review pg. 311