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Electrons, Bonds, and molecular properties - Coggle Diagram

- - - - e are attracted to higher electronegativity atoms.
      - The greater the difference in electronegativity, the more polar the bond.
  - - - Explain the wave motion in mathematics (a function of location)
      - Solve the wave equations and get the wavefunctions
      - The squared value is the probability of finding the electron
    - - The type of the orbitals
    - - The Alfbau Principle
        
        The lowest energy orbital is filled first.
      - The Pauli Exclusion Principle
        
        Each orbital can accommodate a maximum of 2 e spinning oppositely.
      - Hund's Rule
        
        Before e are paired up,
        one e is placed in each orbital first.
  - - - Valence Bond Theory
        
        Constructive
        
        High amplitude
        Sharing of e density between 2 atoms
        
        Desrtuctive
        
        Node
      - MO Theory
        
        Bonding
        
        Low energy, constructive
        
        Anti-bonding
        
        High energy, destructive, node
        
        Energy
        
        HOMO
        
        Highest occupied molecular orbitals
        
        LUMO
        
        Lowest unoccupied molecular orbitals
        
        LUMO > HOMO
        
        Explore the overlap of atomic orbitals with mathematics.
        
        Mathematically combine atomic orbitals to molecular orbitals,
        
        Bond Order
        
        ("bonding" - "anti-bonding")/2
        No bond when BO = 0
      - Hybridized Atomic Orbitals
        
        Atoms undergo hybridization to form equal atomic orbitals.
        
        Equal in energy
        
        The shape and the energy of the hybridized atoms depends on the ratio of s and p orbitals.
      - Sigma and Pi Bonds
        
        Sigma
        
        Head-on overlap
        
        Pi
        
        Side-by-side overlap
        
        Both constructive and destructive interference
- - - - 4
        
        sp3 (Tetrahedral)
        
        Tetrahedral
        
        Trigonal pyramidal
      - 3
        
        sp2 (Trigonal Planar)
        
        Bent
        
        Trigonal Planar
      - 2
        
        sp (Linear)
        
        Linear
  - - - Induction
        
        Dipole Moment (Vector)
        = "Partial Charge" × "The Distance" (debye/D)
  - - - Hydrogen Bonding
        
        especially strong type of d-d attraction
        
        When a H shares e with a highly electronegativity atom (O, N, F)
        
        20 times weaker that covalent bonds
        
        Protic
        
        The strong the H-bond, the high the m.p.
        
        m.p.
      - Dispersion/London/Fleeting dipole-dipole Forces
        
        Random motion of the e
        
        Temporary dipole causes induction.
        
        weak
        
        The greater the surface area,
        the more possible the temporary dipole, the higher the b.p.
        
        b.p.
      - Dipole-dipole Interactions
        
        Polar molecules