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O.Chem CH 1
| Formal charge | VE- (bonds+ lone electrons) |
| Types of molecular geometry and their bond angles | - linear = 180 - Bent = 105 - tetrahedral = 109.5 -trigonal planar =120 - trigonal pyramidal <109.5 |
| Steric # | the # of lone e- pairs + # of atoms around the central atom |
| For H, B, O, S, C, N, P how many bonds and LP do they need for a FC of 0 | H- 1 bond B - 3 bonds, 0 LP O - 2 bonds, 2 lP S - 2 bonds, 2 LP C - 4 bonds, 0 LP N, P - 3 bonds w 1 LP |
| Electronegativity | how strong an atom attracts shared E-. Increases from left to right on the periodic table, and from top to bottom. F has the highest EN. if EN difference >0.5 then bond is polar. |
| Types of intermolecular forces | - London dispersion C-H - Dipole-dipole - Hydrogen bonds: O-H, N-H, H-F |
| London dispersion bonds | formed by two non-polar bonds. The higher the molecular mass the higher the london dispersion. If MM is the same, the more linear has more LDF b/c it has more contact surface. CH (hydrocarbon bonds are always non-polar. Only dissolve in non-polar solvent |
| Dipole-Dipole bonds | Formed by two non-polar bonds |
| Hydrogen bonds | Have the highest intermolecular force, formed with H. Highest polarity and highest boiling points. |
| Dipole moment | When 2 vectors of the same magnittude ar4e going the opposite direction then the some of the dipole force is 0 and it is nonpolar |
| Polar molecules vs non-polar | Polar compounds have central atoms that have either lone pairs or multiple types of atoms. Nonpolar compounds do not have lone pairs on the central atom or different atoms.VB |
| VBT | Valence bond theory: covalent bonds formed when two atomsw of hybrid orbitals interact with each other. create SP, SP2, and SP3 orbitals |
| Hydrid orbitals | Combination formed by combining atom orbitals. # of hybrid orbitals formed = # of atomic orbitals combined. |
| Types of orbitals | 1 type of S orbital, 3 types of P orbitals. (XYZ) and then followed by d and F |
| The central atoms uses what vs the terminal atom? | central atom use the hybrid atom, while the terminal atom uses the atomic orbital. |
| Sigma VS Pi bonds | Sigma bonds are single bonds while pi bonds are more than 1 and are formed from unhybridized P orbital. |
| What is needed for a high boiling/melting point? | A strong intermolecular force, because more energy is needed to separate them. |
| Long non-polar chains do what to polar atoms. | polar atoms with long nonpolar chains have reduced solubility, |
| Molecular orbital theory | MOT, electrons have a wave like function, |
| constructive interference | 2 + waves reinforce each other to create one constructive wave. They are more stable and bc of their lower energy. Only constructive interference result in a bond |
| Destructive wave | 1+ and 1- waves interact and cancel to create a destructive wave. does not result in a bond |
| Bonding molecular | lower energy and is more stable |
| antibonding | higher energy and more reactive. |
| HOMO | Highest occupied molecular orbital |
| LUMO | Lowest unoccupied molecular orbital |
| Induction | Shifting of the e- within an orbital and result in dipole moment, which is the amount of partial charge x distance the partial charge is separated. |
| Dipole moment | the amount of partial charge x distance the partial charge is separated. are reported in units of debye (p) which is equal to 10 +8 electrostatic unit x cm. |
| % ionic character | = the observed dipole moment/units of dipole moment x 100% |
Created by:
Acrob89
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