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| Celsius to Fahrenheit conversion equation |
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| Celsius to Kelvin conversion equation |
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hypo ~ ite
Charge?
How many O atoms? |
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~ ite
Charge?
How many O atoms? |
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~ ate
Charge?
How many O atoms? |
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per ~ ate
Charge?
How many O atoms? |
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No charge
1 + ~ 1/1837 amu |
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No charge
1 + ~ 1/1837 amu |
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(A / Z) X
What do each stand for? (X is supposed to be very large, and A and Z should actually be over one another.) |
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A- mass number (protons + neutrons)
Z- atomic number (protons)
X- element symbol |
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| Formula for determining average atomic mass |
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| Average atomic mass = [(isotopic mass)(relative abundance %) + ...] |
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| How to Find An Empirical Formula (Given the Masses of Several Elements) |
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1. Find how many moles there are of each element
2. Divide all the mole amounts by the smallest mole amount.
3. The quotient for a given element is how many atoms of it are in the empirical formula. |
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| How to Find the Limiting Reactant |
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1. Get a balanced equation.
2. Using stoichiometry, determine which reactant produces fewer moles of one of the products. This is the limiting reactant.
3. To determine how much is left of the non-limiting reactant, find how much of the non-limiting reactant is required to fully react with the limiting reactant. Subtract this amount from the original amount of the non-limiting reactant. |
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| # hydrogens = 2(# carbons) + 2 |
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| # hydrogens = 2(# carbons) |
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| # hydrogens = 2(# carbons) - 2 |
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| polyatomic prefix + [(ate --> ic) or (ite --> ous)] acid |
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| (Group I or II Metal) + H20 --> |
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| 1 mole = 6.02E23 atoms/molecules |
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| 1 mole gas at STP = ___ L |
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| ___ torr = ___ atm = ___ kPa |
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| 760 torr (mmHg) = 1 atm = 101.325 kPa |
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PV = nRT
P (atm)
V (L)
n (mol)
R - .0821 L*atm / mol * K
T (K) |
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| Formula for the density of a gas |
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| density = P * molar mass / RT |
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| R - .0821 L*atm / mol * K |
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| rate 1 / rate 2 = SQUARE ROOT (molar mass 2 / molar mass 1) |
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| Equation for q (using specific heat) |
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| Equation for q (using the heat of fusion or vaporization) |
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| q = m * ΔH(fusion or vaporization) |
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| A + BX --> AX + B will occur if... |
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| A is more reactive than B. |
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| A double replacement reaction will only occur if... |
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| Equation to Calculate the Energy of a Photon |
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Principal Quantum Number
Integers
Determines which electron shell |
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Angular Momentum
From 0 to (n-1)
Determines which subshell |
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Magnetic Quantum Number
From -l to l (0 included)
Determines which orbital in the subshell |
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Magnetic Spin Number
1/2 or -1/2
Determines spin up or spin down |
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| Pauli Exclusion Principle |
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| No two electrons around the same nucleus can have the exact same combination of n, l, ml, and ms-- at least ms has to be different |
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| Fill lowest orbitals first |
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| Electrons prefer to be unpaired |
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| Electron Configuration of Cr |
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[Ar] 4s1 3d5
NOT [Ar] 4s2 3d4 |
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| Electron Configuration of Cu |
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[Ar] 4s1 3d10
NOT [Ar] 4s2 3d9 |
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same electron configuration, different elements
Example: F-, Ne, Na+ |
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| Effective nuclear charge; increases going down vertically, increases going right horizontally |
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| Increases going down vertically, increases going left horizontally |
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| Ability of atom to trade one electron; increases going down vertically, increases going left horizontally... however, the more negative the EA, the better the atom can trade one electron, which means the element with the smallest EA value (in the upper right-hand corner) is most able to trade one electron |
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| Energy required to remove one electron from an atom; increases going up vertically, increases going right vertically |
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| Ability of atom to attract an electron in a bond; increases going up vertically, increases going right vertically |
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no difference in EN
Example: F -- F |
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| polar covalent bond (dipole moment) |
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slight difference in EN
Example: H (~+) -- F (~-) |
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large difference in EN
Example: Li (+) -- F (-) |
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Electron Pairs (Total/Bonding/Lone):
2 / 2 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
3 / 3 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
3 / 2 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
4 / 4 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
4 / 3 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Definition
trigonal pyramidal
<109.5°
sp3
p |
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Electron Pairs (Total/Bonding/Lone):
4 / 2 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
5 / 5 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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trigonal bipyramidal
180° / 120° / 90°
sp3d
np |
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Electron Pairs (Total/Bonding/Lone):
5 / 4 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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see-saw
180° / <120° / 90°
sp3d
p |
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Electron Pairs (Total/Bonding/Lone):
5 / 3 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
5 / 2 / 3
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Electron Pairs (Total/Bonding/Lone):
6 / 6 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Definition
octahedral
180° / 90°
sp3d2
np |
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Electron Pairs (Total/Bonding/Lone):
6 / 5 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Definition
square pyramidal
180° / 90°
sp3d2
p |
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Electron Pairs (Total/Bonding/Lone):
6 / 4 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity? |
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Definition
square planar
180° / 90°
sp3d2
np |
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| The addition of solutes... |
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Definition
| Lowers the vapor pressure, which elevates the boiling point and depresses the freezing point |
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| Freezing or Boiling Point Equation |
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ΔT(b or f) = K(b or f) * m * i
K(b or f) --> a constant
m --> molality (moles solute / kg solvent)
i --> Van't Hoff Factor, or the number of particles the solute dissociates into in solution (i = 1 for hydrocarbons) |
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dipole - dipole
dipole - dipole induced
London Forces (up mass, up LF) |
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The Driving Force Behind Chemical Reactions!
(An Equation) |
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spontaneous
non-spontaneous |
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| ΔH = SUM(ΔH of products) - SUM(ΔH of reactants) |
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| Keq = [products]^coefficients / [reactants]^coefficients |
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| Raise the pressure and shift... |
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Definition
| To the side with fewer gas molecules |
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| Lower the pressure and shift... |
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| To the side with more gas molecules |
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| With acids, the equilibrium always shifts to the side with... |
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| John Dalton (Credit to RK) |
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Definition
"captain obvious" (he basically took the obscured findings of previous scientists/philosophers and mashed them into his encompassing theory)
THEORY... 1) all elements are composed of atoms (which are indivisible and indestructable), 2) all atoms of the same element are alike 3) atoms of different elements are different 4) compounds are formed by combinations of atoms in a whole # ratio
Model - single, solid, circular blob |
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| JJ Thomson (Credit to RK) |
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Definition
took Crooke's tube (cathode ray tube) and improved upon his findings to observe particles (later dubbed and therefore discovered as "electrons")
Model - "plum pudding" model (positively charged aura of sorts with electrons floating around inside) |
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| Robert Miliken (Credit to RK) |
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Definition
oil drop experiment; he ionized drops of oil and tried to suspend them against gravity and messed around with charges and stuff... he eventually discovered the charge of the electron (1.602E-19 but we don't have to know that)
Model - "plum pudding" model (positively charged aura of sorts with electrons floating around inside) |
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| Somethingfirstname Rutherford (Credit to RK) |
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Definition
gold foil experiment; he shot particles at a section of gold foil and observe their deflection... and concluded that they were bouncing off of a central, positively charged nucleus (and therefore discovered protons)
Model - planetary model (electrons encircling the positive nucleus) |
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| Neils Bohr (Credit to RK) |
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Definition
wondered why electrons weren't immediately attracted into the nucleus. He decided that there were shells surrounding the atom that electrons orbited in with different energy states. He quantized the atom with a gas discharge tube.
Model - Bohr - shell model (protons in center with orbits of electrons surrounding) |
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