Chemistry highlights for Princeton Review Chem ch 1-3
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Plank's Constant (h) | 6.63x10^-34 J*s
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Speed of light (c) | 3x10^8 m/s
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Equation for the Energy of a photon | hf or h*(c/wavelength)
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Hund's rule | electrons in the same subshel occupy available orbitals singly, before pairing up
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Aufbau principle | Electrons opccupy the lowest energy orbitals available
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Pauli exclusion principle | no two electrons in the same atom can have the same set of four quantum numbers
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n,l,m(l),m(s) | n = shell numberl = subshell number (n-1)m(l) = orbital numberm(s) = +1/2; -1/2
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diamagnetic | has all electrons paired, repelled by magnetic field
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paramagnetic | not fully paired electrons; attracted to magnetic field
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H | Hydrogen, 1.0, 1
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He | Helium, 4.0, 2
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Li | Lithium, 6.9, 3
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Be | Berillium, 9.0, 4
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B | Boron, 10.8, 5
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C | Carbon, 12.0, 6
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N | Nitrogen, 14.0, 7
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O | Oxygen, 16.0, 8
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F | Fluorine, 19.0, 9
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Ne | Neon, 20.2, 10
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Na | Sodium, 23.0, 11
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Mg | Magnesium, 24.3, 12
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Al | Aluminum, 27.0, 13
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Si | Silicon, 28.1, 14
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P | Phosphorus, 31.0, 15
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S | Sulfer, 32.1, 16
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Cl | Chlorine, 35.5, 17
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A | Argon, 39.9, 18
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K | Potassium, 39.1, 19
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Ca | Calcium, 40.1, 20
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Cu | Copper, 63.5, 29
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Zn | Zinc 65.4, 30
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Fe | Iron, 55.8, 26
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Ag | Silver, 107.9, 47
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Au | Gold, 197.0, 79
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Pb | Lead, 207.2, 82
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Beta Decay (B-) | unstable nucleus contains too many neutrons; 1n-> 1p and 1e-; atomic number (z)increases by 1 but mass number stays the same [ex: 6C-> 7N + 1e-]; MOST COMMON FORM OF BETA DECAY
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Beta Decay (B+) | unstable nucleus contains too few neutrons; 1p-> 1positron + n; atomic number (z) decreases by 1 but mass number stays the same [ex: 9F-> 8O + 1e+]
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Alpha Decay (a) | nucleus becomes more stable by ejecting alpha particle (2p and 2n) {same as a helium molecule}; reduces atomic number (z) by 2 and the mass number by 4; Ex: (210, 84, Po) -> (206, 82 Pb) + (4, 2 alpha)
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Electron Capture | nucleus combines an e- with a p to make a neutron; atomic number (z)decreases by 1, atomic number remains the same
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Gamma Decay | an excited nucleus that has undergone beta or alpha decay relaxes by emitting energy in the form of 1 or more photons which have very high frequency and energy. Gamma decay penetrates matter most effectively, no mass, charge, or effect on z or n
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mass defect | the mass of the combined nucleus is less than the sum of the masses of all its nucleons individually, stable nucleus will always have a positive mass defect
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eV | electronvolts, 1eV= 1.6 x 10^-19 J,
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1kg = ?? Joules | 19 x 10^16 J
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1 amu = ??? kg | 1.66 x 10^-27 kg
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Equation for mass-energy equivalence | E=mc^2 (in joules); or E= m(in amu) x 931.5 eV
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Alkali metals | Group I ns^1
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Alkaline earth metals | Group II ns^2
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Halogens | Group VII ns^2np^5
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Transition metals | d block
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Representative metals | p block (except for Group VIII)
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Rare earth metals | f block
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Noble gases | Group VIII ns^2 np^6
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the horizontal row on the periodic table | period
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vertical column on the periodic table | group
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Metalloids | elements that contain properties of both metals and non metals: B, Si, Ge, As, Sb, Te, Po
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Atomic and Ionic Radius Trend | moving from left to right across a period, atomic radius decreases (b/c increasing numbers of protons pulls the electrons in stronger) going down a group atomic radii increases via increased shielding
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Ionization energy (energy needed to remove an electron) trend | left to right ionization energy increasesb/c valence e- are bound tighter
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Electron Affinity | halogens have large negative electron affinities, they readily accept electrons which causes E to be released
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Electronegativity | F>O>N>CL>Br>I>S>C>H {Foncl Brisch} is a measure of an atoms ability to pull electrons to itself when it forms a covalent bond increases from left to right
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Acidity | how well a compound donates protons, accepts electrons, or lowers pH. acidity increases from left to right, and increases as you go down a group
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Formal Charge | FC= Valence - 1/2(Bonded) - number of lone pair electrons
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coordinate covalent bond | one atom will donate both of the shared electrons in a bond
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Lewis Acid | Accepts a pair of electrons
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Lewis Base/Ligand | Donates a pair of electrons; must have a pair of nonbonding electrons to be a lewis base
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Linear, Trigonal planar, tetrahedral, trigonal bipyramid, octahedral | has no lone pairs of electrons on the central atom
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Bent, trigonal pyramid, see-saw, square pyramid | has 1 pair of electrons on the central atom
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Bent, T-shaped, Square planar | has 2 pairs of electrons on the central atom
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Hybridization of Linear | sp
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Hybridization of Trigonal Planar | sp^2
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Hybridization of Tetrahedral | sp^3
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Hybridization of Trigonal bipyramidal | sp^3 d
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Hybridization of Octahedral | sp^3 d^2
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Heat of Transition ΔH | amount of energy required to complete a transition
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q (heat) = n x ΔH{of a phase change} | If q and ΔH are positive heat is absorbed if negative heat is released
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1 Calorie = ??? Joules | 4.2 J ; is the amount of heat required to raise 1 g of water 1 degree
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q (heat) = mCΔT | ...
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specific heat | the higher the specific heat of a substance the better it holds on to absorbed heat
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Temperature change is proportional to the heat absorbed, but inversely proportional to heat capcity | ...
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During a phase transition tempature doesn't change the greater the value for the heat of transition the longer the flat line on a phase change diagram , Heat of Vap always > Heat of Fusion | ...
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Triple point | is the temperature and pressure at which all three phases exist simultaneouly in equilibrium
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critical point | marks the end of the liquid-gas boundary beyond this point a substance displays properties of both a liquid and a gas (supercritcal fluid)
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supercritcal fluid | no amount of pressure can force the gas back into a liquid state
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