SCH4U

SCH4U

Organic Chemistry
1. Types of Solvents
  1. Esters
    1. An organic compound where the hydrogen in the compound's carboxyl group is replaced with a hydrocarbon group.
  2. Carboxylic Acids
    1. Hydrocarbons that contain a carboxyl group
  3. Ethers
    1. Hydroxyl groups that are bound to a saturated cabon
  4. Alcohols
  5. Amides
    1. Cabonyl group bonded to a nitrogen atom
  6. Alkanes/Alkenes/Alkynes
    1. Hydrocarbons that contain single/double/triple bonds
2. Physical Properties
  1. Intermolecular Forces
    1. London Forces
      1. Weak forces that create temporary dipoles
    2. Dipole Dipole
      1. Attraction between the negative end of a polar molecule and the positive end of another
    3. Hydrogen Bonding
      1. Weak attractive force between a proton and an electronegative adjacent atom
    4. Polar
      1. Non Uniform postive and negative charged ends
    5. Non Polar
      1. Symetrical
  2. Boiling Point
    1. The point at which a liquid turns to a gas
  3. Melting Point
    1. The point at which a solid turns into a liquid
3. Reactions
  1. Oxidation
    1. A process by which a carbon atom gains bonds to more electronegative elements.
  2. Addition
    1. Two smaller molecules are combined by means of addition.
  3. Condensation
    1. A reaction in which molecules are added to the main molecule, resulting in a new molecule and water.
  4. Substitution
    1. A chemical reaction during which one functional group in a chemical compound is replaced by another functional group.
  5. Dehydration
4. Bonds
5. Structural Isomers
  1. Chemical formulas that can be drawn in a variety of structures
6. Fundamental Groups
  1. Structural units that are defined by specific bonding arrangements between specific atoms.
7. Nomenclature
8. Polymers
  1. Addition Polymers
  2. Condensation Polymers
Electrochemistry
1. Lewis Structures
  1. Central Atoms
    1. The atom that the structure is based around
  2. Electrons
    1. A particle with a negative charge in an atom
  3. Electronegativity
  4. Formal Charge
    1. Charge assigned to an atom, based on electronegativity
  5. Octet Rule
    1. All main-group atoms should have 8 electrons in their valance shell
  6. Bonds
2. Galvanic Cells
  1. Reactions
  2. Solutions
  3. Voltage
  4. Electron Potential
    1. The measure of the potential difference between two half cells in an electrochemical cell
  5. Half Reactions
  6. Salt Bridges
    1. A tube containing an electrolyte, providing electrical contact between two solutions
  7. Spontaneous Reactions
    1. Reactions that occur without any outside forces
3. Electrolytic Cells
  1. Electrical Currents
  2. Non-Spontaneous Reactions
4. Redox
  1. Half Reactions
    1. Shows either reduction OR oxidation, but not both.
  2. Balancing
    1. Acidic
      1. Add H2O and H+ to Balance
    2. Basic
      1. Add OH to both sides to balance
  3. Oxidation
    1. Anode
    2. Loss of Electrons
    3. Strongest Oxidation Agent
      1. A substance that has the ability to oxidize other substances
  4. Reduction
    1. Gain of Electrons
    2. Cathode
    3. Strongest Reduction Agent
      1. A substance that has the ability to reduce other substances
  5. Electrochemical Reactions
    1. Spontaneous Reactions
      1. Galvanic Cells
        Derives electrical energy from spontaneous redox reactions within the cell
      2. Batteries
    2. Non-Spontaneous Reactions
      1. Electrolytic Cells
        A cell that needs an electrical current for a reaction to occur
5. Oxidation Numbers
  1. Represents the number of electrons lost or gained by an atom
Structures and Properties
1. Solids
  1. Ionic
    1. Ion (Cation + Anion)
    2. Ionic Bonds
      1. Bonds formed from atoms of opposite charges
    3. Ionic Bonds Break to Melt
    4. Less Strong
  2. Molecular
    1. Molecules
    2. Intermolecular Forces
    3. Least Strong
  3. Covalent Networks
    1. Atoms
    2. Covalent Bonds
      1. Pi
        Two loves overlap with two lobes of another atom
      2. Sigma
        Head-on overlapping between atomic orbitals.
    3. Lots of Energy Needed to Break Bonds
    4. Very Hard
  4. Metallic
    1. Metallic Bonds
      1. No Direction
    2. Not Super Strong
2. Atomic Properties
  1. Electron Configuration
    1. "Bus Seat" Principle
      1. Orbitals of the same energy are each filled with one electron before filling any with a second.
    2. Orbitals
      1. Patterns of electron density that may be formed in an atom or molecule by one or more electrons
  2. Attraction/Repel
    1. Ferra/Para/Dia
      1. Magnetism
        Based on the number of electrons in the valence layer
    2. Ending Levels
      1. S Orbitals
      2. P Orbitals
      3. D Orbitals
      4. F Orbitals
  3. Valence Bond Theory
    1. Sigma and Pi Bonds
    2. Electron Density
      1. Atom
      2. Lone Pair
3. Lewis Structures
  1. Hybridization
    1. AXE
    2. Orbital Geometry
      1. Molecular Geometry
        Intermolecular Forces
    3. Mixing atomic orbitals into new hybrid orbitals
Rates and Energy
1. Rate Laws
  1. Equation that links the reaction rate with the concentrations or pressures of the reactants and constant parameters.
2. Hess' Law
  1. Hess's law states that the change of enthalpy in a chemical reaction is independent of the pathway between the initial and final states.
3. Le Chatliers Principle
  1. A principle stating that if a constraint is applied to a system in equilibrium, the equilibrium will shift so as to tend to counteract the effect of the constraint.
4. Enthalpies
  1. Heat Content of a System
  2. Endothermic
    1. Absorption of heat in a chemical process
  3. Exothermic
    1. Release of heat in a chemical process
  4. Entahlipies of Formation
    1. Change in enthalpy when one mole of a substance in the standard state is formed from its pure elements under the same conditions
5. pH
  1. Measure of the concentration of H30 or H+ in a substance
6. pOH
  1. Measure of the concentration of OH- in a substance
7. Acids and Bases
8. Titration
  1. Process to find an unknown concentration of a substance from another solution of known concentration
9. Bond Energy
  1. Measure of bond strength in a chemical bond
10. Reaction Mechanisms
  1. The step by step sequence of elementary reactions by which overall chemical change occurs.
11. Dissolving Process
  1. Process by which these original states become solutes
12. Thermochemistry
  1. The branch of chemistry concerned with the quantities of heat evolved or absorbed during chemical reactions.
Equilibrium
1. Ksp
2. Equlibrium Constants
3. ICE Tavles
4. Bronsteds Lowry Acids and Bases
  1. Acid
  2. Base
5. Titration Curves
6. Auto Ioniation of water
7. Indicators
8. Reversible Reactions
9. Dynamic Equilibrium

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	Created by BRANDON INGRAM almost 7 years ago