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MCAT Quicksheets Page 14

Terms in this set (36)

molecular shape for 2 regions of electron density
linear
-180 degrees between electron pairs
molecular shape for 3 regions of electron density
trigonal planar
-120 degrees between electron pairs
molecular shape for 4 regions of electron density
tetrahedral
-109.5 degrees between electron pairs
molecular shape for 5 regions of electron density
trigonal bipyramidal
-90, 120, 180 degrees between electron pairs
molecular shape for 6 regions of electron density
octahedral
-90, 180 degrees between electron pairs
chelation
binding of the central cation can be bonded to the same ligand multiple times
coordinate covalent bond
a covalent bond in which one atom contributes both bonding electrons
Lewis acid
electron pair acceptor
Lewis base
electron pair donor
hydrogen bonding
The partial positive charge of the hydrogen atom interacts with the partial negative charge located on the electronegative atoms (F, O, N) of nearby molecules
dipole-dipole interactions
polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule
dispersion forces
weak forces that result from temporary shifts in the density of electrons in electron clouds
rate law equation
rate = k [A]^x [B]^y
*values of k, x, and y must be determined experimentally
mole
the amount of a substance that contains the same number of particles that are found in a 12,000 g sample of carbon-12
combustion reactions
a fuel, such as a hydrocarbon, is reacted with an oxidant, such as oxygen, to produce an oxide and water
combination reactions
two or more reactants form one product
decomposition reactions
A compound breaks down into two or more substances, usually as a result of heating or electrolysis
single-displacement reaction
an atom (or ion) of one compound is replaced by an atom of another element
double-displacement reaction
elements from two different compounds displace each other to form two new compounds
-also called metathesis reactions
net ionic equation
an equation for a reaction in solution showing only those particles that are directly involved in the chemical change
neutralization reaction
specific double-displacement reactions that occur when an acid reacts with a base to produce a solution of a salt (and usually water)
factors affecting reaction rates
-reactant concentrations
-temperature
-medium
-catalysts
catalysts
unique substances that increase reaction rate without being consumed by lowering the activation energy
K_c
equilibrium constant (c stands for concentration)
K_c for aA + bB ⇌ cC + dD
K_c = ([C]^c [D]^d)/([A]^a [B]^b)
K_eq >> 1
an equilibrium mixture of reactants and products will contain Very Little of the Reactants compared to the products
K_eq << 1
an equilibrium mixture of reactants and products will contain Very Little of the PRODUCTS compared to the reactants
K_eq ~= 1
an equilibrium mixture of products and reactants will contain approximately equal amounts of the two
Le Chatelier's Principle
States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
Conditions where:
A + B ⇌ C + heat
will shift to the right
*more A or B is added
*C is taken away
*pressure is applied (assuming A, B, and C are gases)
*volume is reduced (assuming A, B, and C are gases)
*temperature is reduced
Conditions where:
A + B ⇌ C + heat
will shift to the left
*more C is added
*A or B is taken away
*pressure is reduced (assuming A, B, and C are gases)
*volume is increased (assuming A, B, and C are gases)
*temperature increases
Law of conservation of energy
energy can be neither created no destroyed, but all thermal, chemical, potential, and kinetic energies are interconvertible
isolated system
no exchange of energy/matter with the environment
type of system created by a bomb calorimeter
isolated
closed system
can exchange energy but not matter with the environment
open system
can exchange both energy and matter with the environment
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