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Outline of Chemistry 101: Topics Covered in the Course and Exam Information - Prof. Charle, Study notes of Chemistry

An outline of the topics covered in chemistry 101, including philosophy of science, physical and chemical properties, matter and energy, atomic theory and the periodic table, chemical nomenclature, stoichiometry, ionic compounds, solubility of salts, reaction thermodynamics, periodic properties and trends, light, isotopes and radioactivity, ions, solutions, acids and bases, molecular structure, gases, kinetic molecular theory, dynamic equilibrium, and colligative properties. The outline also includes information about midterm exams and the corresponding chapters and problems to be studied.

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Uploaded on 08/17/2009

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Outline โ€“ Chemistry 101
1) Philosophy of science; Chemistry as science
a) Science (L. scientia) knowledge
i) โ€œScience is the organization of thought.โ€ โ€“ Alfred North Whitehead
b) Deductive testing of falsifiable theories โ€“ Karl Popper
i) Problem of induction (reasoning from specific to general)
ii) Falsifiability versus verifiability
c) Scientific methods โ€“
i) Natural Law - summary/generalization of observations
ii) Theory - mechanistic explanation of systems
d) Objectives of Chemistry
i) Recognize patterns in the behavior of different substances.
ii) Develop a model to explain the observed patterns (quantitative if possible).
iii) Develop models that allow the prediction of the behavior of other substances.
2) Physical and chemical properties โ€“ mass, volume, density; Conservation laws
a) Measurement โ€“ accuracy, precision; Metric and SI Units
i) Unit conversions โ€“ English/Metric, prefixes; Applications โ€“ density, dosages
b) Significant figures โ€“ indicating precision
c) Density โ€“ mass per unit of volume
i) Density and specific gravity - floating and sinking
ii) Density calculations โ€“ problem solving
3) Matter and Energy โ€“ classification
a) Mass and Energy Conservation โ€“ mass-energy conservation
b) Classification of matter โ€“ pure and mixture; element and compound
c) Heat flow โ€“ Exothermic, Endothermic
i) Heat flow โ€“ heat does not rise; hot air rises
d) Physical transformations โ€“ phase changes; heat flow
i) Melting/Freezing; Evaporation/Condensation; Sublimation/Deposition
ii) Phase Diagrams โ€“ anomalous density of water; sublimation of dry ice
e) Chemical transformations โ€“ chemical reactions; heat flow
i) Chemical equations โ€“ notation
4) Atomic Theory and the Periodic Table
a) Development of modern model of atoms
i) History โ€“ Dalton, Thompson, Rutherford, Bohr
ii) Modern quantum model of atom
b) Periodic table โ€“ metals, nonmetals, semimetals (metalloids)
i) Atomic Number; Atomic Mass; Mass Number
ii) Ions; Isotopes
5) Chemical Nomenclature
a) Ionic Nomenclature โ€“ simple ions, transition metal ions, polyatomic ions, hydrated salts
b) Covalent Nomenclature โ€“ Inorganic compounds; organic compounds โ€“ simple hydrocarbons, alcohols
6) Stoichiometry โ€“ molar quantities; titration calculations; Limiting reagent determination
a) Molar mass
b) Empirical formula โ€“ by mass ratios
c) Percent mass composition โ€“ elemental analysis
d) Balancing chemical equations
e) General methods โ€“ theoretical yield, percent yield
f) Yield of reactions โ€“ problem solving
g) Titration of acids and bases โ€“ problem solving
h) Limiting reagent determination โ€“ problem solving
Version: 2008 Spring
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  1. Philosophy of science; Chemistry as science a) Science ( L. scientia ) knowledge i) โ€œScience is the organization of thought.โ€ โ€“ Alfred North Whitehead b) Deductive testing of falsifiable theories โ€“ Karl Popper i) Problem of induction (reasoning from specific to general) ii) Falsifiability versus verifiability c) Scientific methods โ€“ i) Natural Law - summary/generalization of observations ii) Theory - mechanistic explanation of systems d) Objectives of Chemistry i) Recognize patterns in the behavior of different substances. ii) Develop a model to explain the observed patterns (quantitative if possible). iii) Develop models that allow the prediction of the behavior of other substances.
  2. Physical and chemical properties โ€“ mass, volume, density; Conservation laws a) Measurement โ€“ accuracy, precision; Metric and SI Units i) Unit conversions โ€“ English/Metric, prefixes; Applications โ€“ density, dosages b) Significant figures โ€“ indicating precision c) Density โ€“ mass per unit of volume i) Density and specific gravity - floating and sinking ii) Density calculations โ€“ problem solving
  3. Matter and Energy โ€“ classification a) Mass and Energy Conservation โ€“ mass-energy conservation b) Classification of matter โ€“ pure and mixture; element and compound c) Heat flow โ€“ Exothermic, Endothermic i) Heat flow โ€“ heat does not rise; hot air rises d) Physical transformations โ€“ phase changes; heat flow i) Melting/Freezing; Evaporation/Condensation; Sublimation/Deposition ii) Phase Diagrams โ€“ anomalous density of water; sublimation of dry ice e) Chemical transformations โ€“ chemical reactions; heat flow i) Chemical equations โ€“ notation
  4. Atomic Theory and the Periodic Table a) Development of modern model of atoms i) History โ€“ Dalton, Thompson, Rutherford, Bohr ii) Modern quantum model of atom b) Periodic table โ€“ metals, nonmetals, semimetals (metalloids) i) Atomic Number; Atomic Mass; Mass Number ii) Ions; Isotopes
  5. Chemical Nomenclature a) Ionic Nomenclature โ€“ simple ions, transition metal ions, polyatomic ions, hydrated salts b) Covalent Nomenclature โ€“ Inorganic compounds; organic compounds โ€“ simple hydrocarbons, alcohols
  6. Stoichiometry โ€“ molar quantities; titration calculations; Limiting reagent determination a) Molar mass b) Empirical formula โ€“ by mass ratios c) Percent mass composition โ€“ elemental analysis d) Balancing chemical equations e) General methods โ€“ theoretical yield, percent yield f) Yield of reactions โ€“ problem solving g) Titration of acids and bases โ€“ problem solving h) Limiting reagent determination โ€“ problem solving

First midterm exam (THU 25 SEP) โ€“ Covers topics 1-

Read Chapter 1 entire chapter

๏‚ท Problems 1. 2, 8, 19, 21-23, 26, 34-36, 38-40, 44-46, 52-55, 60-63, 72, 74, 76, 83

๏‚ท Lab manual Exponential Notation and Significant Figures โ€“ Sets 1, 2

Dimensional Analysis โ€“ Set 1

Read Chapter 2 entire chapter

๏‚ท Problems 2. 3-6, 16, 20-22, 36-43, 47-49, 56, 60-63, 70-78, 84-86, 90-98, 106-110, 153

๏‚ท Lab manual Naming Inorganic Chemical Substances โ€“ #1-

Read Chapter 12 Sections 12.1 โ€“ 12.2 (optional)

๏‚ท Problems 12. 1, 4, 7, 9-11, 18

Read Chapter 3 entire chapter

๏‚ท Problems 3. 2, 8-13, 18, 27, 33-39, 44, 51-55, 63-67, 71-79, 92, 96-98, 100-102, 115

๏‚ท Lab manual Dimensional Analysis โ€“ Sets 2-

Writing and Balancing Chemical Equations โ€“ Sets 1-

Solving Stoichiometric Problems โ€“ Sets 1-

Second midterm exam (THU 23 OCT) โ€“ Covers topics 7-

Read Chapter 4 entire chapter

๏‚ท Problems 4. 9-13, 18-20, 26-27, 36-39, 82-87, 106-107, 110-

Read Chapter 6 entire chapter

๏‚ท Problems 3. 29-31, 35-37, 41, 45, 71, 73

Read Chapter 9 entire chapter

๏‚ท Problems 9. 4-13, 17, 26-28, 32, 38-40, 42, 50-53; 10.5-13, 44-47, 64-

  1. Light โ€“ EM Spectrum; Light emission โ€“ incandescent, fluorescent, LED/LASER a) Electromagnetic Spectrum โ€“ classification; applications b) Spectroscopy โ€“ UV, visible, IR c) Lighting technologies โ€“ incandescent, fluorescent, LED/LASER
  2. Isotopes and radioactivity โ€“ mass numbers and isotopic abundances a) Half-life b) Alpha/Beta/Gamma radiation โ€“ helium nucleus(positive) / electron(negative) / light(neutral) c) Fission and fusion โ€“ splitting and joining nuclei, respectively
  3. Ions โ€“ Periodic patterns and electron gain/loss a) Periodic table โ€“ Valence electrons; element groups (columns) b) Electron organization โ€“ shells, subshells, orbitals, spin c) Redox half reactions โ€“ one substance reduced or oxidized (shows number of electrons)
  4. Solutions a) Solution concentration โ€“ percent volume; molarity i) Percent concentration - %w/v and %v/v ii) Molar concentration โ€“ moles of solute per liter of solution b) Dilution calculations โ€“ problem solving
  5. Acids and Bases โ€“ neutralization reactions; pH System; Acid nomenclature a) Acid and base neutralization โ€“ baking soda and vinegar b) pH โ€“ logarithmic scale of hydrodium concentration c) Acid Nomenclature โ€“ simple inorganic acids
  6. Molecular structure โ€“ Small molecules; Molecular shape, symmetry, polarity a) Lewis Structures โ€“ valence electrons and filled electron shells i) Molecular shape โ€“ bonding and nonbonding electron pairs b) Polarity โ€“ bond polarity and molecular symmetry i) Non-polar compounds โ€“ hydrocarbons
  1. Gases โ€“ gas stoichiometry; Gas Laws โ€“ ideal gases; Non-ideality a) Gas evolution โ€“ effervescent reactions; Carbonation; Mineral testing i) Effervescent solutions ii) Carbonates โ€“ reaction with HCl b) Gas Stoichiometry c) Gas Laws โ€“ simple gas laws, ideal gas law d) Gas Law calculations โ€“ problem solving
  2. Kinetic Molecular Theory โ€“ gases; Intermolecular forces a) Assumptions for gases โ€“ limiting ideal case b) Predictions of KMT โ€“ real gases at ambient conditions c) Intermolecular forces โ€“ condensed phases (liquids and solids) i) Melting and boiling points โ€“ heat of fusion, heat of vaporization ii) Vapor pressure โ€“ liquids, solids; Boiling point and vapor pressure d) Solubility and polarity
  3. Dynamic Equilibrium โ€“ Le Chatelierโ€™s Principle a) Dynamic Equilibrium โ€“ chemical stability b) Le Chatelierโ€™s Principle โ€“ controlling chemical reactions i) Changing conditions โ€“ concentration, temperature, pressure ii) Shift in equilibrium โ€“ spontaneous processes
  4. Colligative properties โ€“ bp elevation, mp depression, osmotic pressure a) BP elevation โ€“ vapor pressure and temperature b) MP depression โ€“ crystal formation c) Osmotic pressure โ€“ mass transfer; Selective membranes

No midterm exam for topics 17-

Read Chapter 5 entire chapter

๏‚ท Problems 5. 3, 8-9, 14, 18, 22-24, 28, 40-42, 46, 50, 51-

Read Chapter 12 entire chapter

๏‚ท Problems 12. 1-6, 19-21, 25, 28, 37-40, 60-61, 67, 86-88, 113, 121

Read Chapter 13 Section 13.

๏‚ท Problems 3. 29-31, 35-37, 41, 45, 71, 73