1. Intermolecular Forces
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding

2. Occurs between noble gases or nonpolar molecules (H2, N2, etc.)
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding
London Dispersion
Occurs between noble gases or nonpolar molecules (H2, N2, etc.)
For an instant, the electrons are not evenly distributed around the atom/molecule

3. Neighboring molecules can be affected and an induced dipole can occur
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding
London Dispersion
Because of the uneven distribution, temporary, instantaneous dipole is created
Neighboring molecules can be affected and an induced dipole can occur

4. These forces are very weak and short-lived
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding
London Dispersion
These forces are very weak and short-lived
As the size of an atom/molecule increases, the LDF also increases
In order for a substance that has LDF to freeze, the molecules must be moving extremely slow so freezing points are low

5. Force of attraction between two polar molecules
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding
Dipole-Dipole
Force of attraction between two polar molecules
The dipole in each molecule is not temporary/instantaneous
These are about 1/100 of the strength of covalent bonds

6. This is a form of dipole-dipole interaction
London Dispersion
Dipole-dipole
Hydrogen Bonding
Covalent Bonding
Ionic Bonding
Hydrogen Bonding
This is a form of dipole-dipole interaction
Occurs when a hydrogen atom (small) is bonded to N, O, or F (highly electronegative)
Electronegativity can affect strength (O>N)
About 4x stronger than dipole-dipole

7. Ionic, Molecular, Atomic Solids
Ionic (NaCl)
between ions
repeating pattern, packed together
High melting point
Molecular (Ice)
Fundamental particle is molecule, but has many of these molecules
Low melting point
Atomic (Diamond)
Covalent bonds between the same atom over and over
One huge molecule, NOT a collection of many small ones

8. Metallic Bonds

9. Aluminum-13 _
Now only 10 e- _ _ + _
13 p+ _ + _ _ _ _ _ _ _ _
Cation!

10. _ _ _ + + + + _ _
Conductors! _ + + + + _ _ _ + + _ _ + + _ + _ _ _

11. + + + + + + + + + + + + + + + + + + + + Malleable! Ductile! _ _ _ _ _

12. Ionic Compounds are not malleable/ductile…+ _ + + _ + _ + _ + _ + _ + + _ _ _ _ + _ + _ + + + _ + _ _ _ +

13. Molarity Moles per liter Must convert grams to moles; mL to L
Has to do with solubility
How much of a solute (solid) is dissolved in a solvent (liquid)
“like dissolves like” –polarities
Terminology: saturated, unsaturated, supersaturated, dilute, concentrated

14. Dilutions Only water is added to a stock solution to dilute something
The amount of SOLUTE before the dilution is the same as the amount of solute after the dilution
Will stay the same
Will increase

15. Dilutions M1 x V1 = M2 x V2 M1 x V1 = moles of solute = M2 x V2
Or you can just use
M1 x V1 = M2 x V2