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

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

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

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

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

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

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

Metallic Bonds

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

_ _ _ + + + + _ _ Conductors! _ + + + + _ _ _ + + _ _ + + _ + _ _ _

+ + + + + + + + + + + + + + + + + + + + Malleable! Ductile! _ _ _ _ _

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

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

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

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