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Study Guide for Final Exam - General Chemistry I | Chem 105, Study notes of Chemistry

Study Guide for Final Material Type: Notes; Professor: Ritchie; Class: General Chemistry I; Subject: Chemistry & Biochemistry; University: University of Mississippi Main Campus; Term: Spring 2011;

Typology: Study notes

2010/2011

Uploaded on 05/11/2011

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Chem 105 Fall ‘09 Dr. Ritchie
A Study Guide for the CHEM 105 Final Exam
Wednesday, 5/11/11; 8:00 AM; Brevard (Old Chemistry) 134
General Tips for Finals Week:
• Get a good night's rest – try to get at least 6 hours of sleep. Being well rested will do more
for your little gray cells that continuing to cram late into the night.
• For morning tests, make sure to set your alarm clock way, way before you go to bed.
(While you are at it, go ahead and set a second alarm clock in case you sleep through
the 1st one!)
• Eat a good breakfast – breakfast is the most important meal of the day. Marathon runners
know to eat complex carbohydrates (found in cereal and bread type foods) because they
will continue to provide energy longer than the simple carbohydrates in sugary foods.
Peanut butter is a great source of protein and brain powering fatty acids. Elvis loved PB
& Ba(Na)2 sandwiches! Now really, how can you question the King?
• Don't neglect your caffeine management – if you need caffeine to function, make sure to
bring your jumbo mug of java along with you.
• DON'T PANIC – Relax, stay calm, and work the problems. Don't be afraid to ask for help if
you don't understand something during the exam. You'll do awesome!
CHEM 105 Study Hints:
• The final exam will be cumulative
• Work all the homework problems!
• Make sure you know how to do all the problems on previous midterms and quizzes
(DISCLAIMER: This list is a review for the students that covers the general topics in the book
and is not necessarily a comprehensive review of all topics to be covered on the final)
Chapter 1: Matter, Measurement and Problem Solving—Phases of Matter, SI units,
Dimensional Analysis, Significant Figures
Know: how to convert between units and apply dimensional analysis to solve problems
Chapter 2: Atoms and Elements—Atomic Theory of Matter, Atomic Weights, Molecular and
Empirical Formulas, Ionic Compounds, Naming Inorganic Compounds
Know: how to calculate atomic masses and molecular formulas, how to predict ionic charges,
and how to name inorganic compounds
Chapter 3: Molecules, Compounds, and Chemical Equations—Chemical Equations, Patterns
of Chemical Reactivity, Formula Weights, The Mole, Empirical Formulas, Limiting
Reactants, Theoretical Yields
Know: how what stoichiometry of chemical equations mean, what a combustion reaction is, how
to calculate % composition from chemical formulas, how to convert between atoms and
moles (6.022x1023 atoms/mole), determine empirical formulas from combustion analysis,
figure out limiting reactants
Chapter 4: Chemical Quantities and Aqueous Reactions—Aqueous Solutions, Solubility and
Precipitation Reactions, Acids & Bases, Redox Reactions, Concentration of Solutions
Know: Strong and Weak electrolytes, solubilities and precipitation reactions, strong and weak
acids and bases (remember the 5 strong acids), neutralization reactions, oxidation and
reduction reactions (LEO says GER), determining concentrations, and dilutions
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Chem 105 Fall ‘09 Dr. Ritchie

A Study Guide for the CHEM 105 Final Exam

Wednesday, 5/11/11; 8:00 AM; Brevard (Old Chemistry) 134 General Tips for Finals Week:

  • Get a good night's rest – try to get at least 6 hours of sleep. Being well rested will do more for your little gray cells that continuing to cram late into the night.
  • For morning tests, make sure to set your alarm clock way, way before you go to bed. (While you are at it, go ahead and set a second alarm clock in case you sleep through the 1st^ one!)
  • Eat a good breakfast – breakfast is the most important meal of the day. Marathon runners know to eat complex carbohydrates (found in cereal and bread type foods) because they will continue to provide energy longer than the simple carbohydrates in sugary foods. Peanut butter is a great source of protein and brain powering fatty acids. Elvis loved PB & Ba(Na) 2 sandwiches! Now really, how can you question the King?
  • Don't neglect your caffeine management – if you need caffeine to function, make sure to bring your jumbo mug of java along with you.
  • DON'T PANIC – Relax, stay calm, and work the problems. Don't be afraid to ask for help if you don't understand something during the exam. You'll do awesome! CHEM 105 Study Hints:
  • The final exam will be cumulative
  • Work all the homework problems!
  • Make sure you know how to do all the problems on previous midterms and quizzes (DISCLAIMER: This list is a review for the students that covers the general topics in the book and is not necessarily a comprehensive review of all topics to be covered on the final) Chapter 1: Matter, Measurement and Problem Solving —Phases of Matter, SI units, Dimensional Analysis, Significant Figures Know: how to convert between units and apply dimensional analysis to solve problems Chapter 2: Atoms and Elements —Atomic Theory of Matter, Atomic Weights, Molecular and Empirical Formulas, Ionic Compounds, Naming Inorganic Compounds Know: how to calculate atomic masses and molecular formulas, how to predict ionic charges, and how to name inorganic compounds Chapter 3: Molecules, Compounds, and Chemical Equations —Chemical Equations, Patterns of Chemical Reactivity, Formula Weights, The Mole, Empirical Formulas, Limiting Reactants, Theoretical Yields Know: how what stoichiometry of chemical equations mean, what a combustion reaction is, how to calculate % composition from chemical formulas, how to convert between atoms and moles (6.022x10^23 atoms/mole), determine empirical formulas from combustion analysis, figure out limiting reactants Chapter 4: Chemical Quantities and Aqueous Reactions —Aqueous Solutions, Solubility and Precipitation Reactions, Acids & Bases, Redox Reactions, Concentration of Solutions Know: Strong and Weak electrolytes, solubilities and precipitation reactions, strong and weak acids and bases (remember the 5 strong acids), neutralization reactions, oxidation and reduction reactions (LEO says GER), determining concentrations, and dilutions

Chem 105 Fall ‘09 Dr. Ritchie Chapter 5: Gases —Pressure, Gas Laws, Ideal Gas Equation, Volumes of Gases in chemical reactions, partial pressures, kinetic theory of gasses, effusion of gases, real gases Know: What's pressure, how to apply the gas laws, PV=nRT, density of gasses, use chemical equations to figure out volumes of gasses, determine partial pressures in gas mixtures, how the kinetic theory affects gas behavior Chapter 6: Thermochemistry —Kinetic and Potential Energy, 1st^ law of thermodynamics, enthalpies of reaction (ΔH), Calorimetry, Enthalpies of Formation(ΔH^0 f), Foods & Fuels Know: Work and Heat, Endothermic (ΔH = +) and Exothermic (ΔH = – ) reactions, heat from a reaction, Heat capacities and calorimetry, how to figure out ΔH^0 of a reaction from ΔH^0 f's, how many calories are in food Chapter 7: The Quantum Mechanical Model of the Atom —Wave nature of light, quantized energy and photons, line spectra and the Bohr atom, orbitals and quantum #s, atomic orbitals Know: Photons and quantized energy (E=hν), energy states in a hydrogen atom, draw atomic orbitals (s, p & d), quantum #s of atomic orbitals Chapter 8: Periodic Properties of the Elements —Electron configurations, Sizes of atoms, ionization energy, electron affinities, metals nonmetals and metalloids, group trends Know: how to fill in electron configurations in atoms, sizes of atoms and ions, trends in ionization energy and electron affinity, group trends on the periodic table (size, electronegativity…) Chapter 9: Chemical Bonding I: Lewis Theory —Chemical Bonds, Lewis Structures, and the Octet Rule, Ionic Bonding, Covalent Bonding, Bond Polarity and Electronegativity, Bond Enthalpies Know: how to draw Lewis structures and apply the octet rule, how electronegativity affects bond polarity and dipole moments, how to assign formal charges, how to calculate ΔH from bond enthalpies Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory —Molecular Shapes, VSEPR model, Orbital Overlap in covalent bonding, hybrid orbitals, Polar Molecules Know: how to determine molecular shapes from VSEPR, the names, shapes, and bond angles in the five basic electron domain geometries