Wolfe/Lentz
Unit 7 Study Guide
Terms (define):
Empirical Formula
Mole
Average Atomic Mass (amu)
Molar Mass
Mass Percent
Molecular Formula
Percent Composition
Avogadros number
Empirical Formula
Application:
How do you calculate the following?
Molar Mass
Ex: Calculate the molar mass of Sodium Nitride, Na3N
Number of Moles
Ex: What mass of cobalt contains the same number of atoms as 57.0 g of fluorine
Number of Molecules Ex:
Percent Composition
Ex: Calculate the percent by mass of each element in the following compounds
Potassium Phosphate
Sodium Sulfate
How would you determine the following:
Empirical Formula
What does it represent?
How does it differ from molecular formula?
Ex: Give the empirical formula for Sodium Peroxide, Na2O2
Ex: A compound has the following percentages by mass: barium 58.84%, sulfur 13.74%,
Oxygen 27.43%. Determine the empirical formula
Molecular Formula
What information do we need?
How does it differ from empirical formula?
Ex: A compound with the empirical formula CH4O was found in a subsequent experiment to
have a molar mass of approximately 192 grams. What is the molecular formula?
Chapter 8 Study Guide
Vocabulary
Excess reactant
Stoichiometry
Percent yield
Limiting reactant
Theoretical yield
Actual yield
Product
Reactant
Mass
Moles
Atoms
Concepts/Application
Calculating Molar Mass
Ex: Molar Mass of NaOH
Balancing Equations
Ex: NaOH + CO2-Na2CO3 +
H2O
Molar Ratio
Ex: 2Al + 6HCl 2AlCl3 + 3H2
What is the ratio of the above?
Dimensional Analysis
Ex: How many grams of Hydrogen
are released when 50.0 grams of
aluminum reacts with 49.0 grams
Hydrochloric Acid
Unit 9 Study Guide
Vocabulary
Types of Bonds
Covalent
Polar Covalent
Ionic
Single bond
Double bond
Triple Bond
Resonance
Geometric shapes
Linear
Trigonal Planar
Tetrahedral
Trigonal Pyramid
Bent (or V-shaped)
Rules
Octet Rule
Duet Rule
Electronegativity
Application
Lewis Dot Structure
How do you represent: N2, H20
How to determine number of Valence
Electrons (label each family and number of
valence electrons)
How to determine electronegativity
Study Guide
Vocabulary
Solid
Liquid
Gas
Specific Heat (Cp)
Change in Temp ( T)
Heat of fusion (Hf)
Heat vaporization (Hv)
Evaporation
Condensation
Intermolecular forces
Intramolecular forces
Dipole-dipole attraction
Hydrogen bonding
London dispersion forces
Formulas:
Q=
Cp=
T=
Q (for Hf) =
Q (for Hv) =
Application:
What are the arrangements, states, and energy required for the graph above?
Calculate the total heat energy in Joules required to raise the temperature of 36.04 g of water from
11˚C to 150˚C.
Heating and Cooling Curve for Water (label temperatures, states of matter, m.p and b.p)
Unit 11 Study Guide
Dalton’s Law
Formula:
Example Problem: What is the total pressure when 5.0 L of Hydrogen (H2) at 1.00 atm is pumped
into a 5.0 L container along with 5.0 L of Oxygen (O2) at 1.00 atm?
Avogadro’s Law
Formula:
Relationship between variables:
Example problem: If 0.412 moles of argon gas occupies a volume of 602 mL at a particular
temperature and pressure, what volume would 0.573 moles of argon occupy under the same
conditions?
Charles Law
Formula:
Relationship between variables:
Example problem: A 20 L sample of nitrogen gas is cooled from 25 deg. Celsius to a final
temperature of -100 deg. Celsius. What is the new volume of the gas?
Combined Gas Law
Formula:
Relationship between variables:
Example problem: A 250 cm3 of nitrogen gas is at 20 deg Celsius and 758 torr. What volume (in
cm3) will it occupy at -15.0 deg Celsius and 1.2 atm?
Ideal Gas Law
Formula:
Relationship between variables:
How to convert grams to moles, if needed:
Example problem: Calculate the pressure in atm of .456 mol of carbon dioxide in a 1.21 liter
container at 312K.
Boyle’s Law
Formula:
Relationship between variables:
Example problem: A submarine with a volume of 13000L has an internal pressure of 1.2 atm. If
the submarine ruptures underwater at a pressure of 250 atm and the gas is released, how large
will the bubble be?
Pressure:
Units/Conversions for Pressure
STP:
Conditions:
Unit
m.p
b.p.
Change in
Temperature
Formula
Farenheit
Celsius
Kelvin
Unit 12 Study Guide
Vocabulary
Dilute
Concentrated
Solution
Concentrated Solution
Dilute Solution
Saturated solution
Unsaturated Solution
Supersaturated Solution
Solute
Solvent
Molarity
Mass Percent
Formula for mass percent:
Application problems:
What relationship exists between solubility and temperature for most of the substances
shown?
What is the exception?
What general principle accounts for this exception?
A 135 g sample of seawater is evaporated to dryness, leaving 4.73 g of solid residue (the salts
formerly dissolved in the seawater). Calculate the mass percent of solute present in the original
seawater.
What is the concentration of 81.0 mL of a 7.0 M HCL stock solution is diluted to a new volume
of 2.00L. The concentration of this new solution is?
A 1.2 M HNO3 solution contains 3.3 moles of KNO3. How much solution is needed?
Understand how to interpret information from the following chart
Example: A saturated solution of KNO3 in 200 g of H2O at 50oC is cooled to 20oC. How
much KNO3 will precipitate out of solution?