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Study Guide: Formulas
oxide |
O, 2- |
sulfide |
S, 2- |
sulfate |
SO4, 2- |
sulfite |
SO3, 2- |
carbonate |
CO3, 2- |
phosphate |
PO4, 3- |
fluoride |
F, 1- |
chloride |
Cl, 1- |
bromide |
Br, 1- |
iodide |
I, 1- |
hydroxide |
OH, 1- |
acetate |
CH3COO, 1- (C2H3O2) |
nitrate |
NO3, 1- |
magnesium |
Mg, 2+ |
calcium |
Ca, 2+ |
zinc |
Zn, 2+ |
copper (I) |
Cu, 1+ |
copper (II) |
CU, 2+ |
iron (II) |
Fe, 2+ |
iron (III) |
Fe, 3+ |
aluminum |
Al, 3+ |
lithium |
Li, 1+ |
sodium |
Na, 1+ |
potassium |
K, 1+ |
ammonium |
NH4, 1+ |
silver |
Ag, 1+ |
mole |
6.022x10^23 |
deg F to deg C |
(F-32)/1.8 |
deg C to deg F |
(1.8 X C) + 32 |
deg C to K |
C + 273 |
K to deg C |
K - 273 |
mega |
M, 10^6 |
kilo |
k, 10^3 |
deci |
d, 10^-1 |
centi |
c, 10^-2 |
milli |
m, 10^-3 |
micro |
u, 10^-6 |
nano |
n, 10^-9 |
pico |
p, 10^-12 |
1 liter |
1000 mL |
1 cubic centimeter |
1 mL |
water |
H20 |
hydrogen peroxide |
H2O2 |
hydrogen chloride |
HCl (called hydrochloric acid if dissolved in water) |
sulfuric acid - strong acid |
H2SO4 |
nitric acid - strong acid |
HNO3 |
acetic acid - weak acid |
CH3COOH |
ammonia |
NH3 |
sulfur dioxide |
SO2 |
sulfur trioxide |
SO3 |
carbon monoxide |
CO |
carbon dioxide |
CO2 |
methane |
CH4 |
ethane |
C2H6 |
propane |
C3H8 |
butane |
C4H10 |
benzene |
C6H6 |
methanol |
CH3OH |
ethanol |
CH3CH2OH |
acetone |
CH3COCH3 |
diethyl either |
CH3CH2OCH2CH3 |
Hund's Rule |
electrons occupy orbitals of a given subshell singly before pairing begins |
Pauli Exclusion |
no two electrons in an atom may have the same set of four quantum numbers |
JJ Thompson |
discoverer of electrons; modified cathode ray tube experiments |
Eugene Goldstein |
discoverer of protons; canal rays |
Robert Millikan |
oil drop experiment determined charge and mass of electron because he realized that charges were multiples of a single value |
Group IA |
alkali metals |
Group IIA |
alkali earth metals |
Group VIIA |
halogens (means "salt formers") |
Group VIIIA |
noble gases |
Strong Acids |
"hydrochloric acid HCl
hyrdrobromic acid HBr
hydroiodic acid HI
nitric acid HNO3
sulfuric acid H2SO4
chloric acid HClO3
perchloric acid HClO4" |
Weak Acids |
"hydrofluoric acid HF
acetic acid CH3COOH
hydrocyanic acid HCN
nitrous acid HNO2
carbonic acid H2CO3
sulfurous acid H2SO3
phosphoric acid H3PO4
oxalic acid (COOH)2" |
Strong Bases (common) |
"lithium hydroxide LiOH
sodium hydroxide NaOH
potassium hydroxide KOH
rubidium hydroxide RbOH
cesium hydroxide CsOH
calcium hydroxide CA(OH)2
strontium hydroxide Sr(OH)2
barium hydroxide Ba(OH)2
notice they are all hydroxides of group IA and IIA metals!" |
Solubility Guidelines |
"1) common inorganic acids are water soluble
2) low-molecular weight organic acids are water soluble
3) common compounds of group IA metal ions and the ammonium ion are water soluble
4) common nitrates, acetates, chlorates, perchlorates are water soluble
5) common chlorides are water soluble EXCEPT AgCl, Hg2Cl, PbCl2
6) common bromides and iodides behave like the chlorides
7) commn fluorides are water soluble EXCEPT MgF2, CaF2, SrF2, BaF2, PbF2
8) Common sulfates are water soluble EXCEPT PbSO4, BaSO4, HgSO4; MODERATELY SOLUBLE are CaSO4, SrSO4, Ag2SO4
9) common metal hydroxides are water insoluble EXCEPT
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
10) common carbonates, phosphates, arsenates are water insoluble EXCEPT group IA metals and NH4+ and MODERATELY SOLUBLE MgCO3
11) common sulfides are water insoluble EXCEPT IA metals and NH4+ plus IIA metals" |
Soluble ionic salts |
... |