CHM 230 Exam 2

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98 Terms

1
What is a model that uses electrostatics to explain electronics in complexes?
crystal field
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2
What is a model that uses molecular orbital approach in the structure of complexes?
ligand field
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3
What do colors in transition metal complexes come from
energy HOMO-LUMO gap
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4
What kind of coloration is glowing or light?
emissive coloration
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5
What kind of coloration is paint or clothes?
absorptive coloration
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6
We see the _____color of wavelengths absorbed
complementary
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7
In an octahedral field, what d orbitals are not point at the axis
dxy, dyz, dxz
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8
In an octahedral field, what d orbitals are affected most by electrostatic interaction?
dz2, and dx2-y2
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9
octahedral d1 through d 3 have all _______ electrons
unpaired
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10
octahedral d __ __through d_______ have both high and low spin states
4-7
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11
low spin means less _____ electrons
unpaired
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12
If delta O is less than repulsion between paired electrons than electrons ______ want to pair
don’t
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13
Ligands ____ the d-orbitals of transition metal complexes
split
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14
Electrons fill into the orbitals based of the size of what
delta O
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15
What influences the size of delta O
\-size of metal

\-charge of metal

\-nature of ligand
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16
big metals give a _____ delta O
larger
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17
as the charge on the metal increases, delta O ____-
increases
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18
Delta O increases as you go ___ __to__ _____ across a period
left to right
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19
What is the order of ligands from small delta O to large delta O
halogens< oxygen compounds< nitrogen compounds< carbon compounds
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20
What d orbitals are higher energy for tetrahedral complexes
dxy, dyz, dxz
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21
What d orbitals are lower in energy for tetrahedral complexes
dz2, dx2-y2
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22
Delta T is always ____- than delta O
less
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23
All tetrahedral complexes are ____ spin
high
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24
What square planar d orbitals have the lowest energy
dxz and dyz
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25
What square planar d orbital has the largest energy
dx2-y2
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26
What ions are mostly square planar
d8 (Ni2+, Pd 2+, Pt2+, Au3+, Rh +, Ir+)
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27
The delta SP is very ____-
large
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28
square planar are typically
diamagnetic
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29
What is beers law
absorbance= molar absorptivity x path length x molar concentration
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30
Molar absorptivity indicates how __ a species undergoes a ______
efficiently; transition
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31
a high molar absorptivity means
more photons absorped
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32
What impacts molar absorpitvity
selection rules and geometry
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33
The laporte rule is d-to-d transitions forbidden in ____ complexes
octahedral
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34
Transitions that require the spin of an electrion to change are
forbidden
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35
Tetrahedral complexes tend to be strongly
colored
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36
most transition metals show ___ main electronic transitions
3
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37
What is the equation for energy of transition?
energy= (hc/wavelength)
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38
When more energy is enetering a system than leaving or vise versa it is called a
dynamic system
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39
Enthalpy is hear flow measured at constant
pressure
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40
state functions are
\-size dependent

\-additive

\-value depends on the difference btwn 2 energentic states
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41
what is it called when gas goes to liquid
condensation
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42
what is it called when liquid goes to gas
vaporization
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43
What is it called when a solid goes to a gas
sublimation
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44
what is it called when a gas goes to a soild
deposition
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45
what is a solid going to a liquid
melting
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46
what is a liquid going to a solid
freezing
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47
What process of phase changes are endothermic
melting, vaporization, and sublimation
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48
What processes of phase changes are exothermic
freezing, condensation, and deposition
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49
what does combustion produce
co2 (g) and H20 (l)
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50
What is hess’s law
the summation of enthalpies
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51
What are the standard conditions
25 C, 1 atm pressure, 1 M solutions
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52
In enthalpy you assume that all elements have an enthalpy of _____ in their standard state
0
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53
for enthalpy of balanced thermochemcial reactions you can use the equation
h rxn= hf products - hf reactants
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54
What is the equation for estimating delta H using bond enthalpies?
Hrxn= h broken -h formed
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55
In bond enthalpies phases of matter _____ taken into account
are not
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56
What are the qualities common to spontaneous reactions?
\-release heat

\-form gases

\-form precipiates

\-form compounds with strong bonds
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57
What is the most convient and precise way to measure delta H
using Hf values
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58
What property of spontaneous reactions is hard to measure with enthlapy
forming gases
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59
A _____ is one of any possible configurations in a system
microstate
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60
What is the measure of the number of microstates available to the system being studied?
entropy
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61
entropy ___- with pressure
increases
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62
The _____ of particles increases the entropy of a system
mobility
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63
When a scoop of ice cream melts entropy ____
increases
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64
When a solid is turned into aqueous ions entropy ____
increases
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65
When a liquid and gas turn into a solid and gas entropy____
decreases
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66
What are the units of entropy
J/K
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67
Delta S =
n(S products)- n (S reactants)
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68
reactions that are spontaneous tend to be ___ and have an _______ in entropy
exothermic; increase
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69
What is the equation for delta G
delta G= delta H- (temp(K) x delta S)
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70
for a spontaneous process delta G has to be _____ zero
less than
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71
\-H and + S means the reaction is
spontaneous at all Temps
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72
\-H and -S means the reaction is
spontaneous at low temp
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73
\+H and +S means the reaction is
spontaneous at high temps
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74
\+H and -S means the reaction is
never spontaneous
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75
The best way to calculate delta G is using
free energies of formation
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76
When should you use delta G= delta H- (T x delta S)
when you need to determine TEMPERATURE of spontaneity and when entropy and enthalpy values are available
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77
When should you use delta G- (products)- reactants
when only delta G values are avaible and you only need to determine spontaneity
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78
What does Gibbs free energy have to be in order for a reaction to be spontaneous?
less than O (-)
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79
What state functions do elements in their standard state = 0
enthalpy and Gibbs Free Energy
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80
What are the units of delta G
kJ/mol
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81
The equilibrium constant is ( ) over ( )
products; reactants
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82
What drops out of the K expression
solids and liquids
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83
the molarity of gas is what
mols gas/ Volume container
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84
When reagents are added to a solution the equilibrium will shift
away from what was added
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85
If an endothermic reaction is warmed where will the equilibrium shift
to the right towards the products
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86
What are the top orbitals of an octahedral compound d orbital splitting diagram called?
eg
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87
What are the bottom orbitals of an octahedral compound d orbital splitting diagram called?
t2g
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88
What are the top orbitals of a tetrahedral compound d orbital splitting diagram called?
t2
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89
What are the bottom orbitals of a tetrahedral compound d orbital splitting diagram called?
e
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90
What is the order of square planar diagrams from bottom to top?
(dxz + dyz), dz^2, dxy, dx^2-y^2
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91
What are the values of h and s for line A
What are the values of h and s for line A
h>0, s
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92
What are the values of h and s for line B
What are the values of h and s for line B
h
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93
What are the values of h and s for line C
What are the values of h and s for line C
h>0, s>0
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94
What are the values of h and s for line ~~D~~
What are the values of h and s for line ~~D~~
h
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95
under what conditions is the top line spontaneous
under what conditions is the top line spontaneous
never spontaneous
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96
under what conditions is the 2 line spontaneous
under what conditions is the 2 line spontaneous
spontaneous at low temps
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97
under what conditions is the 3rd line spontaneous
under what conditions is the 3rd line spontaneous
spontaneous at high temps
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98
under what conditions is the bottom line spontaneous
under what conditions is the bottom line spontaneous
always spontaneous
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