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The flashcards below were created by user
victimsofadown
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3 types of isomerism
- Coordination isomers: ligand and counter ion exchange places
- Geometric isomers: differ in spatial orientation of ligands (cis/trans or fac/mer)
- Enantiomers: stereoisomers that are nonsuperimposable mirror images of eachother
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Strong field ligands vs weak field ligands, how do they fill? How can you determine the split d orbital delta?
- Strong field: CN- > NO2- > en > NH3. Fill the bottom 3 orbitals first then the top 2 afterward as two different energy levels
- Weak field: H2O > OH- > F- > Cl- > Br- > I-. Fill all 5 orbitals as a single energy level
- Ephoton = hν = hc/λ = Δ split d orbital [using wavelength of max absorption]
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3 Ways of radiation absorption by molecules w/ spectrum area
- Rotational transitions: microwave regions (causes molecules to rotate)
- Vibrational transitions: infared regions (causes molecules to vibrate)
- Electronic transition: visible and ultraviolet regions (move electron from lower to higher energy level within split d sublevels)
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Transmittance and absorption equations + Beer's law
- T = P/Po
- A = log(Po/P)
- Beer's Law: relationship between amt radiation absorbed and concentration of the analyte
- A = εbc [ε = absorptivity constant for each compound, b = length of cell, c = concentration (M)]
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Chemical kinetics general rate equation + difference btween avg rate and instantaneous rate
- Rate = Δ[product]/Δtime = -Δ[reactant]/Δtime
- Average rate: change in measured concentration in any particular time period (linear approximation of a curve)
- Instantaneous rate: change in concentration at any one particular time (slope at any one point of a curve)
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All integrated rate law functions for zero order reactions
- [A] = -kt + [A]i
- graph of [A] vs time is a straight line w/ slope -k and y-intercept [A]i
- t1/2 = [A]i/2k
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All integrated rate law functions for first order reactions
- ln[A] = -kt + ln[A]i
- graph of ln[A] vs time is a straight line w/ slope -k and y-intercept ln[A]i
- t1/2 = 0.693/k
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All integrated rate law functions for second order reactions
- 1/[A] = kt + 1/[A]i
- graph of 1/[A] vs time is a straight line w/ slope +k and y-intercept 1/[A]i
- t1/2 = 1/k[A]i
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Effect of temperature on k equations + Arrhenious equation + Arrhenious equation 2-point form
- k = A(e-Ea/RT)
- T = temperature in kelvin
- R = 8.314J/mol k
- A = frequency factor (# molecules that begin to form the activated complex in a given period of time)
- Ea = activation energy (amt energy needed to convert reactants into the activated complex)
- Arrhenious equation: ln(k) = -Ea/R(1/T) + ln(A)
- Arrhenious equation (2-point form): ln(k2/k1) = (Ea/R)(1/T1 - 1/T2)
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