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AP Chemistry 2018 Summer Assignment Ashwat Chidambaram (Equilibrium (ICE…
AP Chemistry 2018 Summer Assignment Ashwat Chidambaram
Acids and Bases
Values
ICE tables
Equilibrium Constant
anti-logarithms
pOH
pH
Type
weak acid/base
dissociate 5% or less
strong acid/base
dissociate completely
Models
Bronstead-Lowery model
Arrhenius model
Bases
denature proteins
release OH- ions in water solutions
taste bitter
turn red litmus to blue
neutralize acids
Acids
taste sour
turn blue litmus to red
release H+ ions in water solutions
corrode active metals
neutralize bases
Fundamentals
Electron Configuration
Aufbau's Principle
Hund's Rule
Pauli Exclusion Principle
Heisenberg Uncertainty Principle
Structure of the Atom
History
JJ Thomson's Model
The Bohr Model
The Quantum Model
Dalton's Atomic Theory
Modern Atomic Theory
present-day idea
densely packed protons + neutrons
at center nucleus of atom
lots of free space around
electrons flying around in "shells"
outside this gap, attracted by nucleus
Kinetics
Rate Laws
an equation that represents the
rate of a reaction, determined experimentally
rate = k [A]^x [B]^y ...
where k = some constant
aA + bB <----> cC + dD
reac. rate: -Δ[A]/aΔT = -Δ[B]/bΔT = Δ[C]/cΔT = Δ[D]/dΔT
Method of Initial Rates
method used to determine orders of reactants
test effects of varying reactant concentrations on reaction rate
used differences to find reactant orders
Equilibrium
K constant
K = ([C]^c [D]^d)/
([A]^a [B]^b)
Q value = the intermediate
current state of reaction
Q < K -- go right
Q > K -- go left
Q = K -- donezo
ICE Tables
C: change -- usually use 'x' to represent change to find
I: initial -- the starting state
E: equilibrium -- the state we want to attain
used for reversible equilibrium reactions
(weak acids and bases)
Le Chatlier's Principle
temperature
increase = right on endo, left on exo reaction
decrease = left on endo, right on exo reaction
pressure
increase = shift to other side
decrease = shift to current side
concentration
increase = shift to less concentrated side
decrease = shift to less concentrated side
Redox
oxidation state rules
group 1 = +1, group 2 = +2,
group 15 = -3, group 16 = -2,
group 17 = -1, group 18 = chillin
individual atoms = 0
fluorine = -1,
hydrogen = +1,
oxygen = -2
NOTE: it's sign first, value second
ex: +1 is for oxidation, 1+ is for charge
balancing acid solutions
separate reactions into half reactions
balance elements in reaction
add H+ ions from H2O to balance charged
add e- to half reactions as necessary
recombine both half reactions
double check/verify equation is fully balanced
Periodic Table
Trends
Electronegativity
increases from bottom-left to top-right
Atomic Radius
increases from top-right to bottom-left
Ionization Energy
increases from bottom-left to top-right
Ionic Radius
increases from bottom-left to top-right
Ions
cation
generally metals
lower electronegativity
lower ionization energy
anion
generally nonmetals
higher electronegativity
higher ionization energy
polyatomic ion
has multiple elements/atoms
monatomic ion
only has one element/atom
Chemical Reactions
Types of Reactions
Single Replacement
metal cation replace metal cation
nonmetal anion replace nonmetal anion
Synthesis (Combination)
reactions with oxygen/sulfur
reactions with oxides
reactions with halogens
Decomposition
binary compounds
metal carbonates
metal hydroxides
metal chlorates
Combustion
reactants
organic compound (with Carbon)
oxygen gas
products
carbon dioxide
water
Double Replacement
metal cation replace other, nonmetal anion replace other
Law of Conservation of Mass
balancing equations
no net change in mass or elements
non-nuclear reaction
Acids and Bases II
Calculate pH with salts
first determine if acidic, basic, neutral salt
utilize ICE table as instructed before
determine the value of Ka from Kb or vice versa
use -log_10(OH-/H+) to determine pH/pOH
Bonding
ionic
metal + nonmetal
donating electrons
held together by ionic charge attraction between elements
covalent
nonmetal + nonmetal
sharing electrons
octet rule
polarity
polar covalent
unequally share electrons
difference in electronegativity
non-polar covalent
equally share electrons
symmetrical structure and electronegativity
held together by sharing electrons
Lewis Dot Structures
octet rule
resonance structures
add up valence electrons
VSEPR (AXE Method)
X
single atoms bonded with central atom
E
lone pairs on central atom
A
central atom
hybridization
metallic
metal + metal
sea of electrons
held together within electrons surrounding it
Empirical Formulas
Combustion Analysis
hydrocarbon + O2 --> CO2 + H2O
weight CO2, H2O, O2; use values to
calculate amounts of C, O, H in reaction
Normal
essentially just like "simplifying" a compound
divide out "common factors" among element subscripts
ex: C6H12O6 --> CH2O; H2O2 --> HO; Na2SO3 --> Na2SO3