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FINAL EXAM (CH3: Molecules, Compounds, and Chemical Equations (Writing…
FINAL EXAM
CH3: Molecules, Compounds, and Chemical Equations
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Classifying Substances as Atomic Elements,
Molecular Elements, Molecular Compounds,
or Ionic Compounds (3.4)
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CH12: Solutions
-Be able to determine solubility of solute in a given solution (12.2) If there are C-OH or C-N or C-F then it will likely be polar making it water soluble but if the dipoles cancel out or molecular is made of mainly C-C then it will be fat soluble or non-polar
-Using Henry’s Law to Predict the Solubility of Gases with
Increasing Pressure (12.4) Sgas = kH x (Pgas) (Henry’s law)
-Calculating Concentrations of Solutions (12.5) Percent by Mass will convert grams into grams of total solution
- Converting between Concentration Units (12.5) Molarity , Molality, Percent by Mass, Mole Fraction, Mole Percent
-Determining the Vapor Pressure of a Solution Containing a
Nonelectrolyte and Nonvolatile Solute (12.6)
Psolution = Xsolvent x Vapor Pressure
Solvent
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- Calculating Freezing Point Depression (12.6) Change in Freezing Point Temp = molality x Freezing Point Elevation
-Calculating Boiling Point Elevation (12.6) Change in Boiling Point Temp = molality x Boiling Point Elevation
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- Determining and Using the van’t Hoff Factor (12.7)
- Determining the Vapor Pressure of a Solution
Containing an Ionic Solute (12.7)
CH5: Gases
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Determining P , V , n , or T
using the Ideal Gas Law (5.4)
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Calculating the Molar Mass of a Gas with the Ideal Gas Law (5.5) 
Calculating Total Pressure, Partial
Pressures, and Mole Fractions
of Gases in a Mixture (5.6)Link Title
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Calculating the Root Mean Square
Velocity of a Gas (5.8)
Calculating the Effusion Rate or the Ratio of Effusion Rates of two Gases (5.9)
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CH11: Liquids, Solids, Intermolecular Forces
Determining Whether a Molecule Has
Dipole–Dipole Forces (11.3) A molecule has dipole–dipole forces if it is polar. To determine if a molecule is polar,
(1) determine if the molecule contains polar bonds and (2) determine if the polar
bonds add together to form a net dipole moment
Determining Whether a Molecule Displays
Hydrogen Bonding (11.3) H-N , H-O, H-F
Direct Hydrogen Bonds = Higher Boiling Point
Using the Heat of Vaporization in Calculations (11.5) Use Heat of Vaporization Relationship (kJ/mol) & Molar Mass to find how many grams of compounds can be vaporized with a GIVEN Energy
Using the Clausius–Clapeyron Equation (11.5)
Using Bragg’s Law in X-Ray
Diffraction Calculations (11.10)
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Summarizing Intermolecular Forces: 1. Dispersion forces are present in all molecules and atoms and
increase with increasing molar mass. These forces are always
weak in small molecules but can be significant in molecules
with high molar masses. 2. Dipole–dipole forces are present in polar molecules. 3. Hydrogen bonds, the strongest of the intermolecular forces
that can occur in pure substances (second only to ion–dipole
forces in general), are present in molecules containing hydrogen bonded directly to
fluorine, oxygen, or nitrogen. 4. Ion–dipole forces are present in mixtures of ionic compounds and polar compounds.
These forces are very strong and are especially important in aqueous solutions of
ionic compounds.
Summarizing Process of Vaporization: ▶ The rate of vaporization increases with increasing temperature.
▶ The rate of vaporization increases with increasing surface area.
▶ The rate of vaporization increases with decreasing strength of intermolecular forces.
Be able to Identify Phase Diagram
(Normal Boiling Points/ Melting Points which are 1atm)
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CH2: Atoms and Elements
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Working with Atomic Numbers, Mass Numbers, and Isotope
Symbols (2.6)
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CH1: Matter, Measurement, and Problem Solving
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Converting between the Temperature Scales: Fahrenheit,
Celsius, and Kelvin (1.6)
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CH10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory
Using VSEPR Theory to Predict the
Basic Shapes of Molecules (10.2)
Predicting Molecular Geometries Using VSEPR Theory and
the Effects of Lone Pairs (10.4)
Predicting the Shapes of Larger Molecules (10.4)
Select Individual Atom and determine it's molecular/geometry shape
Using Molecular Shape to Determine
Polarity of a Molecule (10.5)
Symmetrical = Non-Polar
Asymmetrical = Polar
Writing Hybridization and Bonding Schemes Using
Valence Bond Theory (10.7)
See Worksheet given in class
Drawing Molecular Orbital Diagrams
to Predict Bond Order and
Magnetism of a Diatomic
Molecule (10.8)
Bond Order =
((# of e- in bonding MO) - (# of e- in antibonding MO)) / 2
Diamagnetic: Each e- has a pair
Paramagnetic: e- are missing their pair this causes magnetic properties