CHM 230 Exam 2

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What is a model that uses electrostatics to explain electronics in complexes?

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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
<p>What are the values of h and s for line A</p>

What are the values of h and s for line A

h>0, s<0

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92
<p>What are the values of h and s for line B</p>

What are the values of h and s for line B

h<0, s <0

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93
<p>What are the values of h and s for line C</p>

What are the values of h and s for line C

h>0, s>0

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94
<p>What are the values of h and s for line <del>D</del></p>

What are the values of h and s for line <del>D</del>

h<0, s>0
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95
<p>under what conditions is the top line spontaneous</p>

under what conditions is the top line spontaneous

never spontaneous

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96
<p>under what conditions is the 2 line spontaneous</p>

under what conditions is the 2 line spontaneous

spontaneous at low temps

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97
<p>under what conditions is the 3rd line spontaneous</p>

under what conditions is the 3rd line spontaneous

spontaneous at high temps

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98
<p>under what conditions is the bottom line spontaneous</p>

under what conditions is the bottom line spontaneous

always spontaneous

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