Final Exam Chem 1211 – Flashcards

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Hydrogen Peroxide
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H2O2
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Hydrogen Chloride
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HCl
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Sulfuric Acid
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HNO3
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Acetic Acid
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CH3COOH
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Ammonia
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NH3
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Sulfur Dioxide
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SO2
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Sulfur Trioxide
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SO3
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Carbon Monoxide
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CO
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Carbon Dioxide
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CO2
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Methane
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CH4
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Ethane
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C2H6
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Propane
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C3H8
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Butane
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C4H10
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Pentane
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C5H12
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Benzene
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C6H6
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Methanol
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CH3OH
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Ethanol
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CH3CH2OH
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Acetone
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CH3COCH3
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Ether
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CH3CH2OCH2CH3
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Avagadro's number
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6.022E23
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*C-->*F
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*F=(1.8x*C)+32
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heat energy
q=
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q=m x c x ^T
(^T=change in temp)
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mole/volume relation
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M1V1=M2V2
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Davy
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passed electricity through compounds
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Faraday
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amount of reaction during electrolysis is proportional the the electrical current
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Thompson
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Determined e/m ratio, "discoverer of electrons"
Cathode ray with positive and negative plates on either side
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Millikan
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Determined charge and mass of electron
Container with hole, electrons drop through
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Goldstein
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observed canal rays
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Geiger and Marsden
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Shot gamma rays at piece of foil, most went straight through, some bounced back
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Rutherford
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analyzed Geiger and Marsden's experiment, found that atoms have very small, dense (+) centers
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Chadwick
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discovered neutrons
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metallic characteristics
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|<---
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Ampere
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1A=1E-10m
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velocity/c/wavelength(~)
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V=c/~
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Energy/h/c/~
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E=(hc)/~
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Planck's constant
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h=6.626E-34 J*s
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how to find wavelength moving from one energy level to another
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(1/~)=R[{1/(n1)2}-{1/(n2)2}]
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Rydberg's constant
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R=1.097E7 m-1
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speed of light through a vacuum
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c=3.00E8 m/s
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s orbital
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l=0
m(l)=0
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p orbital
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l=1
m(l)=-1,0,+1
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d orbital
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l=2
m(l)=-2,-1,0,+1,+2
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f orbital
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l=3
m(l)=-3,-2,-1,0,+1,+2,+3
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electron capacity of subshell
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4(l)+2
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electron capacity of a shell
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2n^2
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atomic radii
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|<---
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first ionization energy
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^--->
except 3A<2A and 6A<5A
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electron negativity
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--->-
^
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Electronegativity-ionic/(non)polar covalent
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^EN>1.7 ionic
0.4<^EN<1.7 polar covalent
^EN<0.4 nonpolar covalent
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acidic
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--->
^
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Strong acids
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HCl HBr HI HNO3 H2SO4 HClO4
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Weak acids
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HF
CH3COOH
HCN
HNO2
H2CO3
H2SO3
H3PO4
(COOH)2
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Strong bases
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1A oxides 2A oxides
LiOH Ca(OH)2
NaOH Sr(OH)2
KOH Ba(OH)2
RbOH
CsOH
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2 ternary acids with same central nonmetal
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hypo-stem-ous=2 lower ox
-ous=1 lower ox
-ic=1 higher ox
per-stem-ic=2 higher ox
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covalent bond
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2 nonmetals
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ionic bond
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metal+nonmetal
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Ternary acids
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H+nonmetal+O
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acid+base
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-->salt +H2O
never redox
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Formal Charge
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group# - (#of bonds + #unshared e-)
the lewis dot structure with all closest to 0 is best
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linear e. geo
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AB2
nonpolar
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trig. planar e. geo
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AB3
nonpolar
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tetrahedral e. geo
nonpolar
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AB4
nonpolar
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tetrahedral e. geo
polar
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AB3U, AB3U2, UBU3
polar
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trigonal bipyramidal e. geo
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AB5, AB4U, AB3U2, AB2U3
nonpolar
no octet rule
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octahedral e. geo
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AB6, AB5U, AB4U2
nonpolar
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every double bond has...
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1o, 1pi
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every triple bond has...
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1o, 2pi
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every single bond has...
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1o, 0pi
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*C --> K
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K= *C+273
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combined gas law
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[(P1V1)/T1]=[(P2V2)/T2]
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STP
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0*C
1 atm
22.4 L
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pressure, temperature, volume equation
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PV=nRT
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universal gas constant
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R=0.0821 (Latm/molK)
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total pressure
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Ptot=P1+P2+P3...
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atm to torr
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1atm=760 torr
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diffusion
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mixing one substance with another
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effuse
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gas in container with porous walls
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van der Waals equation
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[P+{(n^2)a/v^2}*{V-nb)=nrt
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exothermic
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releases energy
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endothermic
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absorbs energy
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Thermochemical standards
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298.15 K
1 atm
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electron affinity equation
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x(g)+e(-) --> X(-)(g)
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strong acid-strong base reactions equation
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H+(aq)+OH-(aq) --> H2O(l)
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