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Chemistry highlights for Princeton Review Chem ch 1-3

Quiz yourself by thinking what should be in each of the black spaces below before clicking on it to display the answer.
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Question
Answer
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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