Chemistry 130 Formulas - Final
Chemistry 130 with Zhao at University of Tennessee - Knoxville
About this deck
By: Radha Patel
Textbook:
Chemistry: The Central Science (11th Edition)
Created: 2011-05-01
Size: 56 flashcards
Views: 386
Textbook:
Chemistry: The Central Science (11th Edition)Created: 2011-05-01
Size: 56 flashcards
Views: 386
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Mass Percentage
grams of solute
------------------------------------
grams of solution
Mole Fraction
moles of A
-----------------------------------
moles of A+B
Molarity
moles of solute
-------------------------------
L of solution
Molality
moles of solute
--------------------------------
kg of solvent
Vapor Pressure
(mole fraction of A)(vapor pressure of A)
Colligative Properties
Boiling Pt. Elevation
Freezing Pt. Depression
Vapor Pressure Lowering
Osmotic Pressure
Boiling/Freezing Point
Boiling Point = (Kb)(m)
Freezing Point = (Kf)(m)
Half Life
t = 0.693
------------
k
Arrehenius Equation
k = Ae^(-Ea/RT)
Calculate Rate Constant
ln k2 = - Ea ( 1 1 )
---- ----- ----- - -----
k1 R ( T2 T1 )
Intermediate
Formed in first equation, consumed in the next reaction
Freezing Point of Solution
= Freezing Pt. of Solvent - Freezing Point
Pressure Constant
Kp = Kc(RT)^Δn
Δn = moles of product - moles of reactants
Equilibrium Constant Equilibrium
Kc = products
-------------------
reactants
Reverse reaction...
1
-------
Kc
pH
- log [H+] ; [H+] = 10^-pH
Henderson Hasselbalch: pKa + log [base]/[acid]
pOH
- log [OH-]
[OH-] = 10^-pOH
Acid-Base Dissociation Constant
Kw= 1 * 10^-14
pKw
pKw = 14.00 = pH + pOH
pKa
- log (Ka)
Ksp
Only include products
Precipitation
Q < Ksp then ppt will not occur.
Q > Ksp then ppt will occur.
Internal Energy
ΔE = q + W
where q = heat and W = work
Δ in Enthalpy
amount of heat transferred into or out of the system @ constant pressure.
-ΔH = q
Henderson-Hasselbalch/pH of a Buffer
pH = pKa + log [base]/[acid]
Use for buffers.
Heat
q = Cs * m * ΔT
State Functions
Temperature, internal energy, and enthalpy
Entropy
ΔS = qrev
----------
T
Effect of Temperature on the Spontaneity of Reactions (ΔH is negative)
ΔH ΔS Reaction Characteristic
- + Spontaneous at all temperatures
- - Spontaneous at low T; nonspontaneous at high T
Effect on Temperature on the Spontaneity of Reactions (ΔH is positive)
ΔH ΔS Reaction Characteristic
+ - Nonspontaneous at all temperatures
+ + Spontaneous at high T; nonspontaneous at low T
Characteristics of Entropy Change
ΔS will be positive if increase in temperature, volume, or # of gas particles
Free Energy Change
ΔGº = ΔHº - TΔSº
ΔGº = -nFEº
ΔGº = -RTlnK
Under standard conditions, ΔGº = ΔHº - TΔSº = 0
H = enthalpy
S = entropy
Standard Entropy Change
ΔSº = ΣnSº(products) - ΣmSº(reactants)
n and m = number of moles
Anode
Electrons in the product
Reducing Agent
Oxidation Reaction
Cathode
Electrons in the reactants
Oxidizing Agent
Reduction Reaction
Strongest Reducing Agent
Lowest Eºred
Strongest Oxidizing Agent
Highest Eºred
Standard Cell Potential
Eºcell = Eºred(cathode) - Eºred(anode)
5 Types of Radioactive Decay
- Alpha Emission
- Beta Emission
- Gamma Emission
- Positron
- Electron Capture
Alpha Emission
4
e-
2
*in the products
Beta Emission
0
e-
-1
*in the products
Positron
0
e-
1
*in the products
Electron Capture
0
e-
-1
*in the reactants
Percent Ionization
% = dissociated [H+]
----------------------------------
initial
Magic Numbers
Protons: 2, 8, 20, 28, 50, 82
OR
Neutrons: 2, 8, 20, 28, 50, 82, 126
= Stable
Belt Stability
High neutron-proton ratio = beta emission
Low neutron-proton ratio = positron or electron capture
Atomic number ≥ 84 = alpha emission
First-Order Rate Law for Decay
Nt
ln ------ = -kt
No
Nt = # of nuclei remaining
No = initial 3 of nuclei
Einstein's equation
ΔE = Δmc^2
* c = (2.9979 * 10^8) m/s
* m has to be in kg.
* m(products) - m(reactants) = Δm
Trends in Elemental Properties
→
Increasing ionization energy
Increasing nonmetallic character and electronegativity
Decreasing atomic radius
Decreasing metallic character
↓
Increasing atomic radius
Increasing metallic character
Decreasing ionization energy
Decreasing electronegativity
π bonds
First elements in a group are more readily to form.
Ionic Hydrides
alkali and alkaline earths combine with hydrogen
Metallic Hydrides
transition metals combine with hydrogen
Molecular Hydrides
nonmetals and metalloids combined
Acidic Oxides
oxides with water → acids
Basic Oxides
oxides with water → bases
Amphoteric
oxides with water → substance with both acidic and basic properties
About this deck
By: Radha Patel
Textbook: Chemistry: The Central Science (11th Edition)
Created: 2011-05-01
Size: 56 flashcards
Views: 386
Textbook:
Chemistry: The Central Science (11th Edition)Created: 2011-05-01
Size: 56 flashcards
Views: 386
About StudyBlue
STUDYBLUE makes things that make you better at school.
Things like online flashcards with photos and audio.
Things like personalized quizzes and friendly reminders about when (and what) to study next.
Think of it as a digital backpack™: access to all of your study materials online and on your phone.
STUDYBLUE exists to make studying efficient and effective for every student, for free. Join us.
“I have been getting MUCH better grades on all my tests for school. Flash cards, notes, and quizzes are great on here. Thanks!”
Kathy
Kathy