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Study Guide for Exam, Philosophy of Science - Introduction to Chemistry | CHEM 110, Exams of Chemistry

Material Type: Exam; Professor: Leland; Class: INTRODUCTION TO CHEMISTRY; Subject: CHEMISTRY; University: Black Hawk College; Term: Unknown 1989;

Typology: Exams

Pre 2010

Uploaded on 08/19/2009

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Outline โ€“ Chemistry 110
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; Problem solving
a. Measurement โ€“ accuracy, precision; Metric and SI Units
i. Significant figures โ€“ method of indicating precision
ii. Unit conversions โ€“ English/Metric, prefixes; Applications โ€“ density, dosages
b. Density โ€“ mass per unit of volume
i. Density and specific gravity - floating and sinking
ii. Density calculations โ€“ problem solving
3) Classification of matter
a. Classification of matter โ€“ gas, liquid, solid
b. Classification of matter โ€“ pure and mixture
c. Classification of matter โ€“ element and compound
4) Physical changes โ€“ Phase changes; Heat flow
a. Six types of phase change
i. Melting/Freezing
ii. Evaporation/Condensation
iii. Sublimation/Deposition
b. Mass and Energy Conservation โ€“ mass-energy conservation
i. Heat flow โ€“ Exothermic, Endothermic
ii. FACT โ€“ Heat does not rise; hot air rises
c. Energy and Temperature โ€“ types of energy; energy and temperature units
d. Specific Heat Capacity โ€“ energy per gram per degree; Calorimetry
i. Specific heat calculations โ€“ problem solving
5) Chemical changes โ€“ Conservation of mass and energy; Heat flow
a. Chemical equations โ€“ notation
b. Heat flow โ€“ Exothermic, Endothermic
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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; Problem solving a. Measurement โ€“ accuracy, precision; Metric and SI Units i. Significant figures โ€“ method of indicating precision ii. Unit conversions โ€“ English/Metric, prefixes; Applications โ€“ density, dosages b. Density โ€“ mass per unit of volume i. Density and specific gravity - floating and sinking ii. Density calculations โ€“ problem solving
  3. Classification of matter a. Classification of matter โ€“ gas, liquid, solid b. Classification of matter โ€“ pure and mixture c. Classification of matter โ€“ element and compound
  4. Physical changes โ€“ Phase changes; Heat flow a. Six types of phase change i. Melting/Freezing ii. Evaporation/Condensation iii. Sublimation/Deposition b. Mass and Energy Conservation โ€“ mass-energy conservation i. Heat flow โ€“ Exothermic, Endothermic ii. FACT โ€“ Heat does not rise; hot air rises c. Energy and Temperature โ€“ types of energy; energy and temperature units d. Specific Heat Capacity โ€“ energy per gram per degree; Calorimetry i. Specific heat calculations โ€“ problem solving
  5. Chemical changes โ€“ Conservation of mass and energy; Heat flow a. Chemical equations โ€“ notation b. Heat flow โ€“ Exothermic, Endothermic

First midterm exam (FRI 31 OCT) โ€“ Covers topics 1- Read Chapter 1 entire chapter Read Chapter 2 entire chapter ๏‚ท Exercises 2. 5-9, 14 ๏‚ท Problems 2. 29-32, 41-50, 53, 67-69, 85, 93-97, 105, 111, 115 ๏‚ท Lab manual Exponential Notation and Significant Figures โ€“ Sets 1, 2 Read Chapter 3 entire chapter ๏‚ท Exercises 3. 4-8, 13-18, 20- ๏‚ท Problems 3. 29-31, 35-37, 41-45, 59-61, 71-73, 97, 99, 113 ๏‚ท Lab manual Dimensional Analysis โ€“ Set 1

Second midterm exam (FRI 14 NOV) โ€“ Covers topics 6- Read Chapter 4 entire chapter ๏‚ท Exercises 4. 7, 10, 15-19, 21- ๏‚ท Problems 4. 33, 35, 37, 43-49, 53-57, 67, 69, 73, 77-85, 97-93, 109 Read Chapter 17 Sections 17.1 โ€“ 17. ๏‚ท Exercises 17. x ๏‚ท Problems 17. x Read Chapter 5 entire chapter ๏‚ท Exercises 5. 3, 5-8, 10-14, 17- ๏‚ท Problems 5. 23, 29-33, 39, 41, 45, 55-61, 65, 67-71, 73, 77-79, 81, ๏‚ท Lab manual Naming Inorganic Compounds โ€“ Sets 2- Read Chapter 6 entire chapter ๏‚ท Exercises 6. x ๏‚ท Problems 6. x ๏‚ท Lab manual Dimensional Analysis โ€“ Sets 2-

  1. Stoichiometry โ€“ titration calculations; Limiting reagent determination a. Balancing chemical equations โ€“ mass conservation b. General methods c. Yield of reactions โ€“ problem solving d. Limiting reagent determination โ€“ problem solving e. Percent yield
  2. Single replacement reactions โ€“ oxidation/reduction a. Characteristic reactions b. Reduction of metal ores
  3. Double replacement reactions โ€“ precipitation; neutralization; effervescence a. Characteristic reactions b. Precipitation โ€“ solid formation c. Neutralization โ€“ acid plus base produces salt plus water d. Effervescence โ€“ evolution of CO 2 and H 2
  4. Solutions a. Solubility of Salts โ€“ precipitation reactions; Melting point โ€“ lattice energy i. Solubility โ€“ ionic compounds b. Precipitation reactions โ€“ net ionic equations c. Solution concentration โ€“ percent volume, molarity; Dilution calculations i. Percent concentration - %w/v and %v/v ii. Molar concentration โ€“ moles of solute per liter of solution d. Dilution calculations โ€“ problem solving e. Solution stoichiometry 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
  1. Covalent compounds 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 ii. Polarity โ€“ bond polarity and molecular symmetry b. Non-polar compounds โ€“ hydrocarbons 17)Gases โ€“ gas stoichiometry; Gas Laws โ€“ ideal gases; Non-ideality a. Gas Laws โ€“ simple gas laws, ideal gas law b. 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) d. Melting and boiling points โ€“ heat of fusion, heat of vaporization e. Vapor pressure โ€“ liquids, solids; Boiling point and vapor pressure f. 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 c. Changing conditions โ€“ concentration, temperature, pressure d. 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
  5. 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

Read Chapter 10 entire chapter

  • Third midterm exam (FRI 28 NOV) โ€“ Covers topics 11-
  • Read Chapter 7 Sections 7.3 โ€“ 7. - 8. 3-5, 8-11, ๏‚ท Exercises 7. 6, 51-54 (optional 37,39)
    • ๏‚ท Problems 8. 17-21, 25, 31, 33, 37, 43, 45-49, 53, 57-59, 65, 69, 71, 75,
      • Solving Stoichiometric Problems โ€“ Sets 1- ๏‚ท Lab manual Writing and Balancing Chemical Equations โ€“ Sets 1,7(1)
    • ๏‚ท Exercises 7. 3, 5, 9-13, 15- Read Chapter 7 entire chapter (7.5 โ€“ 7.10)
    • ๏‚ท Problems 7. 29-31, 65, 67, 73, 75, 83, 85, 87,
    • ๏‚ท Lab manual Writing and Balancing Chemical Equations โ€“ Sets 2-
  • Read Chapter 13 Sections 13.1 โ€“ 13.
    • ๏‚ท Exercises 13. 3-5, 7, 13, 19, 23-
    • ๏‚ท Problems 13. 31, 33, 43-45, 51, 61-63, 79-81, 83-
  • Read Chapter 14 Sections 14.1 โ€“ 14.5, 14.8 โ€“ 14.
    • ๏‚ท Exercises 14. 3-7, 9-10, 17, 19, 21, 26-27,
    • ๏‚ท Problems 14. 35, 45, 53, 61, 67, 73, 75,
  • No midterm exam for topics 16-
    • ๏‚ท Exercises 10. 5, 8, 11, 15, 23-
    • ๏‚ท Problems 10. 27, 29, 33, 47-49, 63-67, 87,
    • ๏‚ท Exercises 11. 1, 7, 11, 19, 23, Read Chapter 11 entire chapter
    • ๏‚ท Problems 11. 33, 37, 43, 57, 63, 71, 77, 79,
    • ๏‚ท Exercises 12. 5, 11-15, 17, 19, 21, 23, 25, 27, Read Chapter 12 entire chapter
    • ๏‚ท Problems 12. 37-41, 47-49, 51-
  • Read Chapter 15 Sections 15.1 โ€“ 15.4, 15.7 โ€“ 15.
    • ๏‚ท Exercises 15. 9,
    • ๏‚ท Problems 15. 39, 65-97,
  • Read Chapter 13 Sections 13.9 โ€“ 13.
    • ๏‚ท Exercises 13. 5-9, 12-15, 21-
    • ๏‚ท Problems 13. 35-38, 47,
  • Read Chapter 9 Sections 9.1 โ€“ 9.
    • ๏‚ท Exercises 9. 5-7, 13, 19, 21, 23, 25,
    • ๏‚ท Problems 9. 31-37, 41, 45, 49-51, 61, 69, 75-83,