Chapter 6: Chemical Reactions
- Chemical changes
- Chemical reactions
- Combination
- Decomposition
- Replacement
- Double replacement
- Single replacement
- Combustion
- Reactants
- Products
- Reaction coefficients
- Balancing a Chemical Equation
- Oxidation-reduction reactions
- Oxidation - loss of electrons
- Reduction - gain of electrons
- Rate of reactions
- catalysts
- energy of activation
- Chemical equilibrium
Chapter 7: Chemical Quantities
- The mole
- Avogadro's number - 6.02 x 1023
- Molar mass
- Calculations using molar mass
- Percent composition
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Chap 7 (continued)
- Empirical formula
- Mole Relationships in Chemical Equations
- Mole-mole conversion factors
- Using mole-mole factors in calculations
- Mass calculations for reactions
- Percent yield
- Equilibrium constants
Chapter 8: Gases
- Pressure
- Atmospheric pressure
- Barometer
- 1 torr = 1 mm Hg
- 1 atm = 760 mm Hg
- Vapor pressure
- Boyle's Law (V=k/P)
- P1V1 = P2V2
- Inverse relationship
- Charles' Law (V=bT)
- V1/T1 = V2/T2 or
T1/T2=V1/V2
- Direct relationship
- Gay-Lussac's Law
- Avogadro's Law
- Combined gas law P1V1/T1=P2V2/T2
or
P1V1T2=P2V2T1
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Chap. 8 (continued)
- STP
- Ideal gas law
- PV=nRT
- Partial pressure
Compound naming review
- Valence electrons
- Electron dot structures
- Ions (Octet rule)
- Cations (+) - Na+, Al3+, Fe3+
- Anions (-) - O2-, Cl-, NO3-
- Ionic compounds
- Naming ionic compounds
- Type I (NaCl: sodium chloride)
- Type II (FeO: iron(II) oxide)
- Naming binary covalent compounds
- Type III (CO2: carbon dioxide)
- Ion names
- -ide — element as ion (S2-, O2-,
Cl-)
- -ate — anion of acid (sulfate, nitrate,
phosphate)
- -ous acid contains one less "O" than -ic acid
- -ite — anion of an -ous acid (sulfite,
nitrite, etc.)
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