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chem 1 - Coggle Diagram

- - - - difference between molecular formula & empirical formula
        molecular formula > types and number of atom ic a molecule
        empirical formula > the simplest form
        it is used to indicate the mole ratio of all elements present in the compound
        eg. glucose: MF -C6H12O6
        EF - CH2O
  - - - laws of conservation of mass
        1.cannot be created or destroyed
        2.numbers of moles must be the same for both reactant and product
        
        redox reaction must have the same charges on both reactants and product
    - - precent yield% = actual yield / theoretical yield X 100%
        * percent yield % < 100
        percent purity% = mass of pure substance / mass of impure X 100%
    - - types of solutions
- - - - group 1A > alkali metals
        group 2A > alkaline earth metal
        group 7A > halogen
        group 8A > noble gases
    - - how to describe an atomic orbital
        
        each shells have subshells / sublevels (l)
        f > d > p > s ( energy level of subshell )
        
        magnetic quantum number (ml)
        the orientation/ direction of the orbital momentum
        
        energy level are arrange depending of the principal quantum number (n)
        
        'n' is the distance of valence electron to the nucleus
        
        the larger 'n' is, the larger the average distance between the valence electron and the nucleus
        
        number of shells increase = energy level increase
        max number electron of shells = 2n^2
    - - aufbau principal
        electrons fill subshell orbitals with lower energy level before fill subshell orbitals with higher energy level
        exceptions :
        
        chromium (Cr)
        reason > only 4s orbital and 3d orbital have similar energy level. electron occupy the 3d orbital to ease the electron-electron repulsion.
        
        copper (Cu)
        reason > to increase stability
        
        ** electrons in group 6 and group 11 have similar deviation
      - pauli exclusion principal
        hold up to max 2 electron
        electrons must be opposite turns when paired
      - hund's rule
        electrons will occupy all orbitals with same energy level before pairing