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Molecular behavior (Theories and representations of molecular behavior…

- - - - Weakly attracted to magnetic poles
  - - - Linear (2 groups) (180 degrees)
      - Trigonal planar (3 groups) (120 degrees)
      - Tetrahedral (4 groups) (109.5 degrees)
      - Trigonal bipyramidal (5 groups) (120 and 90 degrees)
      - Octahedral (6 groups) (90 degrees)
- - - - Results from the balance of the nuclei attracting the electron and both nuclei repelling each other
        
        The bonding pair is a pair of electrons shared covalently between two nonmetal atoms
        
        A lone pair is a pair of electrons not involved in bonding
    - - Bond order
        
        The number of electron pairs being shared between two atoms
        
        Single, double, and triple bonds
      - Bond energy
        
        The energy required to overcome the attraction between nuclei and shared electrons and break the bond (like lattice energy)
        
        Endothermic process
        
        Stronger bonds have a larger bond energy
      - Bond length
        
        The distance between the nuclei of two bonded atoms
        
        Just an estimated (like bond energy)
        
        A double bonded atom's nuclei are drawn closer together (shorter bond length) and are harder to seperate
    - - Like covalent bonds, except with a bit of ionic grab
    - - Equal distribution of electrons in a covalent bond
  - - - This accounts for metal's conductivity, malleability, ductility, and low volatility
    - - Brass, bronze, and stainless steel are examples
  - - - Energy is absorbed during electron transfer
        
        Exothermic reactions occur during the attraction of the resulting ions
        
        Lattice energy is the amount of energy that it takes to seperate a mole of solid ionic compound into gaseous ions
        
        Lattice energy is calculated with the Born-Haber cycle (a series of steps from elements to ionic solids)
        
        Smaller ions attract more strongly than larger ones
        
        As ionic charge increases, so does lattice energy
        
        Gaseous ionic molecules are called ion pairs
  - - - Fluorine is the highest, at 4.0
    - - This is directly related to polarity
        
        Diatomic elements are 0.0
        
        The largest EN difference is 3.3 (fluorine with cesium)
- - - - Dumbbell (infinity/8) shape
      - There are three p orbitals (px, py, and px)
      - P orbitals have positive and negative portions, and nodes
        
        There is no chance of finding an electron in the node (that's where the nucleus is
    - - 4-leaf clover shape
    - - Sphere shape
  - - - "The azimuthal qunatum number"
      - Represents angular momentum
      - Describes the shape of the orbital
        
        L=0 is s (one per energy level), L=1 is p (three per energy level), L=2 is d (five per energy level), L=3 is f (seven per energy level)
      - Any value from 0 to n-1
        
        If n=3, then L can be 0, 1, or 2
    - - "The magnetic quantum number"
      - Ranges from -L to L
      - Accounts for limitations in shapes in energy shell
    - - Any positive number
      - The energy level of the electron (energy shell)
      - "The principal quantum number"
    - - "The electron spin quantum number
      - Always either 1/2 or -1/2