Lewis Structure

A 2-dimensional model
1. Straight Lines=covalent bonds
2. unbonded valence electrons=dots
Bonding Pairs=bonds are formed by pairs of valence electrons in a space between two atoms
Lone Pairs: Pairs of electrons that are attracted to only on atom
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
Sidenotes
1. Model: anything that represents something else physical or conceptual
2. The only thing connecting two atoms together in a chemical bond is a bunch of electrons-> they are in constant motion
3. 1916 Gilbert Newton Lewis Described covalent bonds as 2 atoms sharing electrons
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
        Double Bond: Bond in which two pairs of electrons are shared by a pair of atoms (=)
        Triple Bond: bond in which three pairs of electrons are shared by a pair of atoms
2. H20

Zusammenfassung der Ressource

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