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Module 2 Chapter 5 (5.3 Covalent Bonding (Average bond enthalpy…

- - - - S
        
        1 orbital
        
        2 electrons
      - P
        
        3 orbitals
        
        6 electrons
      - D
        
        5 orbitals
        
        10 electrons
      - F
        
        7 orbitals
        
        14 electrons
      - Orbital
        
        Volume of space that can hold a maximum of two electron providing the have opposite spins
      - 4s fills before 3d as it has less energy
      - Electrons in boxes
      - Only pair up when they have to otherwise they fill singularly
      - Electron configuration Nitrogen= 1s2 2s2 2p3
  - - - S-orbitals= spherical
      - P-orbitals= dumb bell and arranged at right angles to each other
- - - - High m and b points
      - Lots of energy needed to overcome strong electrostatic bonds= high temps needed to provide energy
      - Depends on ionic charges and size of ions
      - Higher charger= stronger bond
      - Smaller ions- stronger bond
    - - Many ionic compounds dissolve in polar solvents
      - e.g. H2O
        
        Polar H2O molecules break down the lattice and surround each ion in solution
        
        Polar H2O molecules are attracted to oppositely charged ions
        
        Water molecules bond to the ions weakening ionic bonding
        
        Ionic bonds are broken
        
        Ions surrounded by polar water molecules and are free to move
    - - Solid
        
        Ions in fixed positions
        
        No mobile charge carriers
        
        No electrical conductivity
      - Liquid or aqueous
        
        Ions free to move
        
        Ions= mobile charge carriers
        
        Electricity is conducted
- - - - Dot and cross= Shared pair of electrons
      - Two dots= lone pair of electrons
  - - - Electrostatic attraction is between 3 shared pairs of electrons the the nuclei of the bonding atoms
      - e.g. N2
        
        1 triple bond- very strong so N2 not reactive, 1 lone pair of electrons per atom
    - - Electrostatic attraction between two shared pairs of electrons and the nuclei
      - e.g.O2
        
        1 double bond, two lone pairs of electrons per atom
        
        O=O
    - - Shared pair of electrons where the bonded pair has been provided by one of the bonded atoms only
      - Shown as an arrow- arrow points away from atom contributing
      - e.g. Carbon monoxide
        
        - 2 shared pairs of electrons and one dative bond
        
        C≡O Arrow from O to C as O provides 2 extra electrons