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174 Cards in this Set
- Front
- Back
Aluminum
|
Al 3+
|
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Ammonium
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NH4+
|
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Barium
|
Ba 2+
|
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Bismuth
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Bi 3+
|
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Calcium
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Ca 2+
|
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Cesium
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Cs+
|
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Chromium(II)
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Cr 2+
|
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Chromium(III)
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Cr 3+
|
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Cobalt
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Co 2+
|
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Copper(I)
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Cu+
|
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Copper(II)
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Cu 2+
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Hydrogen
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H+
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Hydronium
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H3O+
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Iron(II)
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Fe2+
|
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Iron(III)
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Fe 3+
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Lead(II)
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Pb 2+
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Lithium
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Li+
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Magnesium
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Mg2+
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Manganese
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Mn 2+
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Mercury(I)
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Hg2 2+
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Mercury(II)
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Hg 2+
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Nickel
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Ni 2+
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Potassium
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K+
|
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Rubidium
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Rb+
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Silver
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Ag+
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Sodium
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Na+
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Strontium
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Sr 2+
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Tin(II)
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Sn 2+
|
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Tin(IV)
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Sn 4+
|
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Zinc
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Zn 2+
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Acetate
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CH3CO2 -
|
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Arsenate
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AsO4 3-
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Bromide
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Br -
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Carbonate
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CO3 2-
|
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Hydrogen carbonate
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HCO3 -
|
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Chlorate
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ClO3 -
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Chloride
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Cl-
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Chlorite
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ClO2 -
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Chromate
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CrO4 2-
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Cyanide
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CN-
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Dichromate
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Cr2O7 2-
|
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Fluoride
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F-
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Hydroxide
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OH-
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Hypochlorite
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ClO-
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Iodide
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I-
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Nitrate
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NO3 -
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Nitride
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N 3-
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Nitrite
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NO2 -
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Oxalate
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C2O4 2-
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Oxide
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O 2-
|
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Perchlorate
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ClO4 -
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Permanganate
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MnO4 -
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Peroxide
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O2 2-
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Phosphate
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PO4 3-
|
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Monohydrogen Phosphate
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HPO4 2-
|
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Dihydrogen Phosphate
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H2PO4 -
|
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Sulfate
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SO4 2-
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Hydrogen sulfate
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HSO4 -
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Sulfide
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S2 -
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Hydrogen sulfide
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HS -
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Thiocyanate
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SCN-
|
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Thiosulfate
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S2O3 2-
|
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What was the experiment in which the electron was discovered because rays were deflected towards the positive side?
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Thomson's cathode ray experiment
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What was the experiment in which electrons were shown to be very light, electrons and protons are now known to exist, and alpha, beta, and gamma particles were revealed?
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Radioactive experiment
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What was the experiment that led to atomic theory and discovered that the atom is mostly empty space?
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Rutherford's gold foil experiment
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Natural abundance of isotopes
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Sum of: (fraction of naturally occurring n * mass of n) = atomic mass of element
|
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Nomenclature for naming ionic compoinds
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Mono
Di Tri Tetra Penta Hexa Hepta Octa Nona Deca |
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Prefixes for carbon backbone nomenclature
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Meth
Eth Prop But Pent Hex Hept Oct Non Dec |
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Priorities for nomenclature (high to low)
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Carboxylic acid
Ester Amide Aldehyde Ketone Alcohol Amine Hydrocarbon |
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Hydrocarbon
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C and H only
-e |
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Amine
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N w/only carbons or NH2, NH
-amine |
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Alcohol
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-OH
-ol |
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Ketone
|
=O
-one |
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Aldehyde
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-H and =O
-al |
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Amide
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=O and N
-amide |
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Ester
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=O and O
-oate |
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Carboxylic acid
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=O and -OH
-oic acid |
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Priorities for benzenes (high to low)
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Analine
Phenol Anasole Toluene Chlorobenzene Styrene Benzoic acid Nitrobenzene |
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Analine
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NH2
|
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Phenol
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OH
|
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Anasole
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OCH3
|
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Toluene
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CH3
|
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Chlorobenzene
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Cl
|
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Styrene
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C=C
|
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Benzoic acid
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COOH
|
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Nitrobenzene
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NO2
|
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How do you name benzenes?
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1 carbon - parent
2nd carbon - ortho (o-) 3rd carbon - meta (m-) 4th carbon - para (p-) |
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How to calculate enthalpy changes from the heating or cooling curve
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sloped part: q=m(kg)*Cs*deltaT = kJ
Hvap or Hfus: #mol*Hvap or Hfus (kJ/mol) = kJ |
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Ideal gas law
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pv=nRT
|
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Substitutions possible in Ideal gas law
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n = (g/MM)
v = (g/d) |
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Energy/wavelength equality
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E (J/photon) = hV = hc/T
T = wavelength in meters V = frequency (1/sec or Hz) |
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Rydberg's equation
|
1/T = R(1/n^2 - 1/m^2)
n < m |
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Balmer/Rydberg series
|
shell 2
|
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Lyman series
|
shell 1
|
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What is vanderwaals/dispersion forces?
|
fluctuation of e- and temporary dipole (weakest!!!)
|
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What is dipole-dipole force?
|
Always present: ex O=<
partial negative charge on O, partial positive charge on C. |
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What is a hydrogen bond intermolecular force?
|
F,O,N form them with H, and they are very strong
|
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When does the behavior of a gas become non-ideal?
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Low temperatures, high pressures because these cause attractive forces
|
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What does the wave-particle duality entail?
|
Light is both waves and particles (photons)
|
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What is the photoelectric effect?
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Proves bundles of photons exist and that a certain amount of energy is required to knock out an electron; also shows that light is a particle.
|
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Does going OUT a shell take energy or release energy?
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Takes energy
|
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What is the quantum number n?
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The principle quantum number: denotes shell and distance from nucleus
|
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What is the quantum number l?
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The azimuthal quantum number: describes shape of orbital.
(0,1...(n-1)) 0 = s 1 = p 2 = d 3 = f |
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What is the quantum number ml?
|
Magnetic quantum number
-l..0..+l Describes orientation of orbital |
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What is the quantum number ms?
|
Spin
+/- 1/2 |
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What is z-effective?
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# protons - core electrons, so how much positive charge is felt by the outer electrons from the nucleus
|
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What is shielding?
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When core electrons shield outer electrons from the nucleus' charge
|
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What does the Aufbau principle say?
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Electrons fill lower energy orbitals first
|
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What does the Pauli exclusion principle say?
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Only two electrons will go per orbital and they will have opposite signs
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What does Hund's rule say?
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One electron will go in each orbital until orbitals are 1/2 filled
|
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Atomic radius increases...
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Down and Left
|
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Ionization energy increases
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Up and Right
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Electron affinity becomes more negative
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Up and Right
|
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When metals ionize, where do they lose electrons from first?
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Their outer shell (highest n value)
|
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Energy of photon*frequency = binding energy
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hV = O
h=Planck's constant V = frequency (Hz) O = binding energy (J) |
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Core electrons
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# of electrons of previous noble gas; for group C elements add 10 to include transition metals
|
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Outer electrons
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Always number of electrons in the shell with the highest n value
|
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Valence electrons
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Number of electrons n the highest n value shell but add the d electrons in the orbital you're in the process of filling for transition metals
|
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Electronegativity
|
FONClBr
|
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How to draw resonance hybrid
|
Draw sigma bonds
Draw electrons common to all structures Draw dotted bonds for where pi bonds could be Partial charges |
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Electron pair geometries
|
2-Linear
3-Trigonal Planar 4-Tetrahedral 5-Trigonal bipyramidal 6-Octahedral |
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Molecular geometries
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2-Trigonal Planar-Bent
4-Tetrahedral-Trigonal pyramidal-Bent 5-Trigonal bipyramidal-seesaw-T-shaped-Linear 6-Octahedral-Square pyramidal-square planar-T-shaped-Linear |
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Combustion reaction format
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C,H,maybe O +O2 --> CO2 + H2O
|
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Arrhenius acid
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Produce H3O+ in solution
|
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Bronsted-Lowry acid
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Proton donor
|
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Lewis acid
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Electron pair acceptor
|
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Arrhenius base
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Produces OH- in aqueous solvent
|
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Bronsted-Lowry base
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Proton acceptor
|
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Lewis base
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Electron donor
|
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Conjugate acid/base
|
The acid - H
The base + H |
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What are the diatomic elements?
|
BrINClHOF
|
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What happens in organic chemistry reactions of alkenes, alkynes, ketones, and aldehydes?
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The pi bond reacts to create two new sigma bonds
|
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Which o-chem reaction is it if it's a benzene?
|
Substitution: substituted for H
|
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Which o-chem reaction involves an alkane, halide, and heat?
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Substitution
|
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Which o-chem reaction involves a strong acid or strong base as the solvent?
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Elimination (the reverse of addition)
|
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Which o-chem reaction involves alcohols -OH going to =O?
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Oxidizing
|
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Which o-chem reaction involves LiAl4, and =O going to -OH?
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Reduction
|
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Compounds of group I are
|
soluble :)
|
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Compounds of nitrates are
|
soluble :)
|
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Compounds of acetates are
|
soluble :)
|
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Compounds of chlorates are
|
soluble :)
|
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Compounds of the halogens with metals are
|
soluble, EXCEPT:
Ag Hg I Pb (HALI) |
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Compounds of sulfates are
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soluble, EXCEPT:
Ba2+ Sr2+ Ca2+ Pb2+ Ag+ Hg+ |
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Compounds of carbonates are
|
insoluble :(
|
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compounds of hydroxides are
|
insoluble :(
|
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compounds of oxides are
|
insoluble :(
|
|
compounds of silicates are
|
insoluble :(
|
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Compounds of phosphates are
|
insoluble :(
|
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Compounds of sulfides are
|
insoluble, EXCEPT:
Ba2+ Sr2+ Ca2+ Mg Na+ K+ NH4+ |
|
Coffee cup calorimeter
|
-q=m*Cs*deltaT
|
|
Bomb calorimeter
|
-q=C*deltaT(bomb) + m*Cs*deltaT(surr)
|
|
How do you get Erxn per mole of a particular reactant?
|
Divide qrxn by the number of moles that reacted
|
|
Hess's Law
|
Hrxn = Sum of Hfproducts*mol - Sum of Hfreactants*mol
|
|
Reaction coordinate diagram Delta H?
|
Delta H = Sum of bonds broken - Sum of bonds formed
|
|
1st order rate law
|
ln[A]t = -kt + ln[A]o
|
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2nd order rate law (integrated)
|
1/[A]t = kt + 1/[A]o
|
|
How do you know which step is the rate determining step?
|
Smaller rate constant, greater activation energy
|
|
What does a large K or a small K indicate?
|
Large K: high concentration of products, low concentration of reactants
Small K: low concentration of products, high concentration of reactants |
|
What does it mean for a reaction to be in dynamic equilibrium?
|
Rate of forward reaction = rate of reverse reaction
|
|
What does Keq equal?
|
[C]^c[D]^d/[A]^a[B]^b
|
|
When do you negate x?
|
When the k value is very small, or when the initial concentration divided by k is greater than 400?
|
|
If Q<K
|
Reaction goes to right
|
|
If Q>K
|
Reaction goes to left
|
|
If Q=K
|
Reaction is at equilibrium
|
|
Strong acids
|
HI
HBr HCl H2SO4 HNO3 |
|
Strong bases
|
LiOH
NaOH KOH |
|
Ka = ?
|
[H3O+][A-]/[HA]
|
|
pH = ?
|
-log[H3O+]
|
|
pKa = ?
|
-logKa
|
|
Ka x Kb = ?
|
Kw = 1x10^-14
|
|
Reduction happens at the _____, oxidation happens at the ______
|
cathode, anode
|
|
Which half of the electrochemistry reaction will be the reduction half which is spontaneous?
|
The half-reaction with a more + Ecell
|
|
Ecell (entire redox) =
|
E(1/2 cell cathode) - E(1/2 cell anode)
|
|
Delta G =
|
-nFEcell
|