Do Now Turn in labs from last week if you did not do so

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Presentation transcript:

Do Now Turn in labs from last week if you did not do so Plan for today: go over Lewis Structures, hybridization Unit 10 Quest WED 12/16 SOL: TUES 1/5

Hybridization Hybridization: combining/mixing of electron orbitals when atoms bond. The hybridization is determined by the # things around the central atom The shape is determined by the lone pairs on the central atom

Common Hybridizations # Sets Orbital Hybridization 2 sp 3 sp2 4 sp3 Note: “sets” refer to bonded atoms as well as lone pairs on the central atom

VSEPR Theory Valence Shell Electron Pair Repulsion A=Central Atom X=Bonded Atoms E=electron pairs (non-bonding) on the central atom

These are REFERENCES…not all the possible hybridizations!

sp linear Tetra-hedral sp3 sp2 sp3 sp3 bent AX2 AX4 Trigonal planar AX3E pyramidal sp3 AX2E2 bent

sp3 AXE3 linear All diatomic molecules are linear in shape

Polarity of Molecules (Compound) Comparing electronegativity difference between 2 atoms in a bond, for all bonds in the compound If there is an electronegativity difference between bonded atoms, and the molecule is asymmetrical, then the compound is polar

Polarity of Molecules If there is an electronegativity difference between bonded atoms, and the molecule is completely symmetrical then the compound is nonpolar

Polarity of Molecules If there is no electronegativity difference between bonded atoms, and the molecule is completely symmetrical then the compound is nonpolar

linear no polar yes nonpolar yes nonpolar no polar no polar yes nonpolar

Intermolecular Forces (sometimes referred to as “Van der Waals forces”) Attractive forces between molecules are NOT BONDS, which is an attraction between 2 atoms Lots of H2O molecules

Types of IMFs: London Dispersion Forces The weakest intermolecular force Is the main attractive force between nonpolar molecules

Types of IMFs Dipole-Dipole Forces Stronger than dispersion forces The main attractive force between polar molecules

Types of IMFs Hydrogen Bonding: is an intermolecular force; it is NOT actually a bond! The strongest intermolecular force Only occur in molecules containing Hydrogen AND one of the following: Nitrogen, Oxygen, or Fluorine (NOF)

Practice polar yes Hydrogen bonding London dispersion nonpolar no no Dipole-dipole polar yes Hydrogen bonding nonpolar no London dispersion