Cheatography
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Acids and Bases, Polyatomic Ions, Formulas, and constants
This is a draft cheat sheet. It is a work in progress and is not finished yet.
Polyatomic Ions
Ion |
Name |
Charge |
NH4 |
Ammonium |
1+ |
Hg2 |
Mercury(1) |
2+ |
NO3 |
Nitrate |
1- |
NO2 |
Nitrite |
1- |
HSO4 |
Bisulfate |
1- |
OH |
Hydroxide |
1- |
CN |
Cyanide |
1- |
H2PO4 |
Dihydrogen Phosphate |
1- |
NCS |
Thiocyanate |
1- |
HCO3 |
Bicarbonate |
1- |
ClO |
Hypochlorite |
1- |
ClO2 |
Chlorite |
1- |
ClO3 |
Chlorate |
1- |
ClO4 |
Perchlorate |
1- |
C2H3O2 |
Acetate |
1- |
MnO4 |
Permanganate |
1- |
SO3 |
Sulfite |
2- |
SO4 |
Sulfate |
2- |
HPO4 |
Hydrogen Phosphate |
2- |
CO3 |
Carbonate |
2- |
Cr2O7 |
Dichromate |
2- |
CrO4 |
Chromate |
2- |
O2 |
Peroxide |
2- |
C2O4 |
Oxalate |
2- |
TeO2 |
Hypotellurite |
2- |
TeO3 |
Tellurite |
2- |
TeO4 |
Tellurate |
2- |
TeO5 |
Pertellurate |
2- |
PO4 |
Phosphate |
3- |
PO3 |
Phosphite |
3- |
|
|
Strong Acids
Name |
Formula |
Hydrochloric Acid |
HCl |
Hydrobromic Acid |
HBr |
Hydroiodic Acid |
HI |
Chloric Acid |
HClO3 |
Perchloric Acid |
HClO4 |
Nitric Acid |
HNO3 |
Sulfuric Acid |
H2SO4 |
Strong Bases
Name |
Formula |
Lithium Hydroxide |
LiOH |
Sodium Hydroxide |
NaOH |
Potassium Hydroxide |
KOH |
Rubidium Hydroxide |
RbOH |
Calcium Hydroxides |
Ca(OH)2 |
Strontium Hydroxide |
Sr(OH)2 |
Other Acids
Name |
Formula |
Acetic Acid |
CH3COOH |
|
|
Water Energies
Delta H Sublimation |
46.6 kJ/mol |
Delta H Fusion |
6.02 kJ/mol |
Delta H Vaporization |
40.6 kJ/mol |
Intermolecular Forces
Dipole - Dipole Forces |
Neutral Polar molecules attract each other when the positive end of one molecule it near the negative end of another. Smaller molecules have a higher dipole-dipole attractive forces. |
London Dispersion Forces |
Neutral non-polar molecules due to the instantaneous distribution of electrons. Temporary dipole on one atom induces a similar dipole on adjacent atom causing the atoms to be attracted to each other. |
Hydrogen Bonds |
An attraction between the hydrogen atom in a polar bond that is bonded to an electronegative atom and the lone pairs of electrons on another atom. Stronger than dipole-dipole or London Dispersion forces. |
Molarity
Molarity (M) = (moles of solute)/(Liters of Solution) |
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