MISCELLANEOUS CHEMICAL INFORMATION 1 Conversion 2 Quantum 3 Gas Laws 4 fpt/Bpt 5 VSEPR 6 Solution 7 Solubility 8 Colligative 9 Equilibrium 10 Acid-base 11 Kinetics 12 Thermo/Electro 13 Inorganic 14 Organic 15 Periodic table 16 Ka acids 17 Electrochem 18 Themo 1 Conversion information: System Pressure: LENGTH: VOLUME MASS Temperature English: 760 mmHg = 14.7 psi 1 atm = 101.3 KPa 1 ft = 12 in 1 mile = 5280 ft 1 gal = 4 qt 1 qt = 57.75 in 3 1 lb = 16 oz 1 ton = 2000lb T F = 1.8T C + 32 SI- English: 1 atm = 760 torr 1atm = 760 mmHg 1 in = 2.54 cm 1 mi = 1.609 km 1 L = 1.057 qt 1 qt = 0.946 L 1 lb = 453.6 g 1 oz = 28.35 g T C = (T F − 32) 1.8 Misc. info 1 J = 1 kg m 2 / s 2 1 mole = 6.02•10 23 Density H 2 O: 1.0 g/ml 2 Quantum Equations Electromagnetic Radiation E = h • ν = h c λ , h = 6.63 • 10 -34 J • s , c = 3.0 •10 8 m/s Energy for H-like atom E = Z 2 R h 1 n 2 Rydberg Equation Δ E = R H 1 n i 2 - 1 n f 2 1 λ = R H ( λ ) 1 n i 2 - 1 n f 2 R H(E) = 2.18 • 10 -18 J R H (λ) = 1.097 • 10 7 m -1 3 Gas law equations: Ideal Gas Law PV = nRT Denstiy(D) = m • P n R T , m= mass R = 0.08206 L • atm mol • K Real Gas vander Waal Equation P+ a•n 2 V 2 V-n•b ( ) = nRT STP P = 1 atm, T = 0°C, 1mole = 22.4 L Dalton's Law of Partial Pressure P T = P a + P b + P c + ... P T = (n a +n b +n c +...)R • T V T . Pa = χ a • P T Pb = χ b • P T . χ a = n a / n T χ b = n b / n T Speed of Gas particles KE = 1 2 mu 2 u rms = 3 RT M R = 8. 314 J mol • K Graham's Law of effusion rate a rate b = time b time a = M b M a Calorimetry q p = ΔH = m C s ΔT where ΔT = T f - T i, C s (H2O) = 4.184 J/g•K 4 Boiling Points of Liquids Liquid Boiling Point (°C) 1 Acetone 56.5 2 Carbon disulfide 46.3 3 Carbon tetrachloride 76.8 4 Chloroform 61.3 5 Ethanol 78.5 6 Ether 34.6 7 Methanol 64.6 8 Water 100.0
9
Embed
MISCELLANEOUS CHEMICAL INFORMATIONfaculty.sdmiramar.edu/faculty/sdccd/fgarces/Links_Lib/... · 2009-04-30 · 5 Valence Shell Electron-Pair Repulsion Theory (VSEPR) : # e- Domain
This document is posted to help you gain knowledge. Please leave a comment to let me know what you think about it! Share it to your friends and learn new things together.
5 Valence Shell Electron-Pair Repulsion Theory (VSEPR) :
# e- Domain or
region
AEn
Electronic Geometry
Bond Pr [Cord #]
non-bond
AEnBm
Molecular Geometry
Bond angle Hybrid
Examples
2 AE2 EE A Linear
2 0 AB2 B A B Linear
180° sp
BeH2
CO2
3 0 AB3 B A
B
B
Trigonal Planar
120°
sp2
BF3 BCl3
3
AE3
EE
EA
Trigonal
2 1 AB2E A
B
B
..
Bent
< 120°
sp2
NO2
4 0 AB4
BA
BB
B
l
Tetrahedra
109.5°
sp3
CH4
NH4+
3 1 AB3E
BA
BB
..
Trigonal
Pyramidal
< 109.5°
sp3
NH3
H3O+
PH3
4
AE4
A EEE
E
Tetrahedral 2 2 AB2E2
AB
B..
..
Bent
< 109.5°
sp3
H2O
H2S
F2O
5 0 AB5
B A B
B
B
B
Trigonal Bipyramidal
180° 120° 90°
sp3d
P I5
4 1 AB4E
A B
B
B
B
..
See-saw
180° 90° <120°
sp3d
S F4
3 2 AB3E2
. .A BB
B
..
T-shape
180° 90°
sp3d
Cl F3
5
AE5
A EEE
E
E
Trigonal Bipyriamidal
2 3 AB2E3
... .A
B
B
..
Linear
180°
sp3d
Xe F2
6 0 AB6 B A B
B
B
BB
Octahedral
90°
sp3d2
S F6
5 1 AB5E B A B
BB
B
..
Square Pyramidal
90° < 90°
sp3d2
Br F5
6
AE6
E EEA
E
E
E
Octahedral 4 2 AB4E2
B A B
BB ..
. .
Square planar
90°
sp3d2
Xe F4
6 Solution and Concentration equations:
Concentrations M, molarity = moles solute / liter solution N , normality = eq solute / liter solution m , molality = moles solute / Kg solvent % m, percent by mass = (mass solute / mass solution)*100 χ , mole fraction = moles a / moles a + moles b ...
Solution Dilution C1V1 = C2V2 (moles before dilution = moles after dilution)
7 Solubility rules: Soluble substances with - Exceptions Insoluble substances with - Exceptions
(SO42-) Sr, Ca, Ba, Hg, Pb Soluble - dissolve, no precipitate (aq -phase)
Alkali & NH4+ None insoluble (or slightly soluble) - does not dissolve, precipitate forms. (s-phase)
Solubility Table
C2H3O2- AsO4 3- Br - CO3 2- Cl - CrO4 2- OH - I - NO3 - C2O4 2- O 2- PO4 3- SO4 2- S 2- SO3 2-
Al +3 S I S - S - I S S - I I S d - NH4 + S S S S S S S S S S S S S S S
Ba 2+ S I S I S I s S S I s S S S S Bi 3+ - s d I d - I I d I I s d I - Ca 2+ S I S I S S I S S I I I I d I Co 2+ S I S I S I I S S I I I S I I Cu 2+ S I S I S I I - S I I I S I - Fe 2+ S I S s S - I S S I I I S I s Fe 3+ I I S I S - I - S S I I S I - Pb 2+ S I I I I I I I S I I I I I I Mg 2+ S d S I S S I S S I I I S d s Hg 2+ S I I I S s I I S I I I d I - K + S S S S S S S S S S S S S S S Ag + s I I I I I - I S I I I I I I Na + S S S S S S S S S S S S S S S Zn 2+ S I S I S I I S S I I I S I I S = Soluble in water I = Insoluble in water (less than 1 g./100 g H2O) s = slightly soluble in water d = Decomposes in water
8 Solubility and Colligative Properties Pressure effects: Henry's Law P = χ / k where χ = solubility Raoult's Law Psolv = χsolvent • P°solvent ΔPsolv = P°solv - Psolv = χsolute • P°solv Boiling Point Elevation ΔTb = m Kb Freezing Point Depression ΔTf = m Kf Osmotic Pressure Π = MRT (R = 0.08206 L•atm / mol•K) Van't Hoff Factor
Rates of Reaction rate = Δ[A] /Δ t = - Δ [react] /Δ t = Δ [prod] /Δ t Rate laws (Order of reaction) initial rate = k [A]x [B]y [C]z ... Overall order = x + y + z + ...
Conc. vs. Time dependence
Zeroth Order rate = k
[A] = [A]o - kt Conc. vs. Time ➟ straight line. Half life; t1/2 = [A]o / 2 k
First Order rate = k [A]
[A]= [A]o exp{- kt) ln[A] = ln[A]o - kt
ln[Conc.] vs. Time ➟ straight line Half life; t1/2 = 0.693 / k
Second Order rate = k [A]2 or k [A] [B]
1/[A] = 1/[A]o + kt
1/[Conc.] vs. Time ➟ straight line Half life; t1/2 = 1 / k [A]o
Temperature vs. Rate dependence
k= A exp {-Ea /RT} ln k = ln A - (Ea/R)•1/T
ln(k) vs. 1/T ➟ straight line.
12 Thermo Electro Chemistry Equations
Thermodynamics Standard Conditions: 1 atm, 25°C Universe = surroundings + system State Function (X) where X = E, H, S or G ΔXrxn = Σ n ΔX°prod - Σ n ΔX°react w = -P ΔV ΔE = q + w ΔH = ΔE + P ΔV ΔH = qp