Lewis Structure

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IB Chemistry SL 1 IB Chemistry SL I (Atomic Structure/Bonding) Mind Map on Lewis Structure, created by hollandblumer6 on 18/11/2014.
hollandblumer6
Mind Map by hollandblumer6, updated more than 1 year ago
hollandblumer6
Created by hollandblumer6 over 9 years ago
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Resource summary

Lewis Structure
  1. A 2-dimensional model
    1. Straight Lines=covalent bonds
      1. unbonded valence electrons=dots
      2. Bonding Pairs=bonds are formed by pairs of valence electrons in a space between two atoms
        1. Lone Pairs: Pairs of electrons that are attracted to only on atom
          1. Atoms are most stable when their outer most electron shells are filled.
            1. Exceptions: Hydrogen can only hold two electrons. Elements in the third row of the periodic table and below often have more than eight valence electrons
            2. Sidenotes
              1. Model: anything that represents something else physical or conceptual
                1. The only thing connecting two atoms together in a chemical bond is a bunch of electrons-> they are in constant motion
                  1. 1916 Gilbert Newton Lewis Described covalent bonds as 2 atoms sharing electrons
                  2. Process
                    1. 1. Figure out how many valence electrons are in each atom. Hydrogen has 1 valence electron. Oxygen has 6 valence electrons.
                      1. 2. Multiply the number of valence electrons by the number of atoms. H=1 valence electron per atom x 2 atoms = 2 electrons. O= 6 valence electrons x 1 atom = 6 electrons
                        1. 3. Layout the molecules and create the bond
                          1. Types of Bonds
                            1. Double Bond: Bond in which two pairs of electrons are shared by a pair of atoms (=)
                              1. Triple Bond: bond in which three pairs of electrons are shared by a pair of atoms
                        2. H20
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