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Chem 109 Final
Term | Definition |
---|---|
JJ Thompson | Cathode Ray Tube; Discovered and identified the mass to charge to ratio for electrons |
Robert Millikan | Oil Drop Experiment; Discovered the charge of the electron |
Ernest Rutherford | Characterized beta and alpha particles ; discovered the proton w/a mass spectrometer; discovered the nucleus w/the gold foil experiment; proposed the nuclear theory |
Dalton's Atomic Theory 1 | Matter consists of tiny particles called atoms. |
Dalton's Atomic Theory 2 | In a sample of a pure element, all atoms are identical & have the same properties. |
Dalton's Atomic Theory 3 | Atoms of different elements differ in mass & other properties. |
Dalton's Atomic Theory 4 | Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms |
Dalton's Atomic Theory 5 | Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions. |
Charge of Beta Particle | -1 |
Charge of Alpha Particle | +2 |
Law | describe and predict |
Theory | encompasses a number of laws; explains laws |
Tera Sign | T |
Tera Exponent | 10^12 |
Giga Sign | G |
Giga Exponent | 10^9 |
Mega Sign | M |
Mega Exponent | 10^6 |
Kilo Sign | k |
Kilo Exponent | 10^3 |
Deci Sign | d |
Deci Exponent | 10^-1 |
Centi Sign | c |
Centi Exponent | 10^-2 |
Milli Sign | m |
Milli Exponent | 10^-3 |
Micro Sign | u |
Micro Exponent | 10^-6 |
Nano Sign | n |
Nano Exponent | 10^-9 |
Pico Sign | p |
Pico Exponent | 10^-12 |
Law of Conservation of Mass | In a chemical reaction, mass isn't gained or lost |
Law of Definite Proportions | In a chemical compound, elements are combined in the same proportions by mass. |
Accuracy | How close the measured value is to the actual value |
Precision | How close a series of measurements are to one another (how reproducible) |
Temp in F= | (9/5 * temp in C) +32F |
Diatomic Molecules | H2, N2, O2, F2, Cl2, Br2, I2 |
Acetate Formula | CH3COO |
Acetate Charge | - |
Carbonate Formula | CO3 |
Carbonate Charge | 2- |
Chlorate Formula | ClO3 |
Chlorate Charge | - |
Hydroxide Formula | OH |
Hydroxide Charge | - |
Nitrate Formula | NO3 |
Nitrate Charge | - |
Permanganate Formula | MnO4 |
Permanganate Charge | - |
Phosphate Formula | PO4 |
Phosphate Charge | 3- |
Sulfate Formula | SO4 |
Sulfate Charge | 2- |
Thiocyanate Formula | SCN |
Thiocyanate Charge | - |
Ammonium Formula | NH4 |
Ammonium Charge | + |
HCl | Strong Acid (Hydrochloric Acid) |
HBr | Strong Acid (Hydrobromic Acid) |
HI | Strong Acid (Hydroiodic Acid) |
HNO3 | Strong Acid (Nitric Acid) |
HClO3 | Strong Acid (Chloric Acid) |
HClO4 | Strong Acid (Perchloric Acid) |
H2SO4 | Strong Acid (Sulfuric Acid) |
LiOH | Strong Base (Lithium Hydroxide) |
NaOH | Strong Base (Sodium Hydroxide) |
KOH | Strong Base (Potassium Hydroxide) |
RbOH | Strong Base (Rubidium Hydroxide) |
CsOH | Strong Base (Cesium Hydroxide) |
Ca(OH)2 | Strong Base (Calcium Hydroxide) |
Sr(OH)2 | Strong Base (Strontium Hydroxide) |
Ba(OH)2 | Strong Base (Barium Hydroxide) |
HF | Weak Acid (Hydroflouric Acid) |
HC2H3O2 | Weak Acid (Acetic Acid / Vinegar) |
NH3 | Weak Base (Ammonia) |
KE= (Unit 2) | 1/2 *mv^2 |
w= (Unit 2) | -PdV |
dE= (Unit 2) | q+w |
1 atm = ___Pa | 101325 |
c= | wavelength * frequency |
E= (Unit 3) | hv OR hc/v |
hv= (Unit 3) | BE+KE |
E= (Unit 3 Energy Levels) | -2.18E-18J (1/n^2f - 1/n^2i) |
1/wavelength= (Unit 3 Energy Levels) | 109,678 cm^-1 (1/n^2(1) - 1/n^2(2)) |
wavelength= (DeBroglie's) | h/ (mass *velocity) |
Coffee Cup Calorimeter Equation | -msdT |
Bomb Calorimeter Equation | -CdT |
Expansion | - |
Contraction | + |