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Chemistry Test

Two types of magnetism Diamagnetic and Paramagnetic
Diamagnetic All electrongs are paired up,down
Paramagnetic Unpaired electrons
Values of S,P,D 0,1,2
4 Quantum #'s n,l,ml,ms
n Primary quatum # deal w/ energy lvl
l Deals w/ the shape of the orbital (s,p,d,f)
ml Deals with the orientation 1s,3p,5d,7f
s Deals with the spin +1/2 or -1/2
Exceptions to AuFBau Cr,Cu,Mo,Ag
Electron Affinity x + e- --> x- Best for lvl 17. Peaks a 1,14,17.
Ionization Engery M --> M+ + e Best for group 1. Minor peaks at 2,15
Periodic Properties Atomic Size, Ionic Size, Electron Affinity, and Ionization Energy
Bohr Harbor Cycle Sublimation + Ionization energy + 1/2 bond energy + Electron Affinity + Lattice energy = Overall Delta H
Exception to Lewis 8e Rule 6e, 10e, 12e, Odd #'s of e
Isoelectronic Series -2,-1,0,+1,+2
Calculating # Bonds E have (8 X # Atoms) - ehave(Group #-10 & correct for charge) / 2
Formal Charge Group # - 10 - (# Bonds) - (# of electrons)
Electronegativity Increase up and to the right.
Ionice size Increase down and to the left. Postive ions are smaller than neutral ions. Negative ions are larger than neutral ion.
Ionic Bond Greater than 1.5
Polar Covalent Bond Btwn .5 and 1.5
Pure Covalent Less than .5
Schrodinger Led to the theory of quantum physics
Lyman 1 Ultraviolet
Balmer 2 Visible and Untraviolet
Paschen 3 Infrared
Brackett 4 Infrared
JJ Thomson Measured e/m ration of electron/proton
Millikan Oil drop experiment measures e
Davisson & Germer Mass of a nuetron AMU
Rutherfordy Gold foil experiment. Led to planitary model.
Bohr Model of e. Explain H. Calculates emission spectrum of H.
Einstein Photoelectric effect light ---> pariticles and waves
Rydberg Study emission spectrum of H. Led to Rydber constant.
C degree to Kelvin= (C+ 273.15)=K
C to F (1.8 x C)+ 32 F
Avagardo's Number 6.022 x 10^23
# of moles of an element # grams have / AMU of element
Molecular weight Atomic mass of each atom added together.
a b NI C # of protons = b # of netrons = a-b # of electrons = b while correcting for C(the charge)
Group 1 , Group 2, Group 16, Group 17, Group 18 1 Alikali Metals, 2 Alkaline Earth, 16 Chalcogens, 17 Halogens, 18 Noble Gas
S, D, P, F S(1,2); D(3-12); P(13-18); F(lower two)
Lanthanides First row of F
Actinides Second row of F
isotope Same # of protons but different # of neutrons
nano- 10^-9
pico- 10^-12
micro- 10^-6
milli- 10^-3
centi- 10^-2
deci- 10^-1
tera- 10^12
giga- 10^9
mega- 10^6
kilo- 10^3
% yield actual yield/ theoretical yield
Boyles Law PV=nRT
Gas constant R= .08206
Titration CV=CV
Molarity Moles/Liter(M=n/V)
Charles Law P1V1/T1 = P2V2/T2
A gas is most ideal under... High pressure and low temperature
Stoichiometry moles of what u have x want/have x grams of what u want
Dalton's Law Pi=XiPt
Endothermic reaction absorbs heat, temperature decreases, sign is +
Exothermic reaction gives off heat, temperature rises, sign is -
A bomb calorimeter measures Delta E
A cup calorimeter measures Delta H
Delta E = q + w
Created by: hermis1986