Pcat Inorganic Chemistry

Front 1

Electrons within the same orbital are represented as having parallel spins. This goes against what?

Back 1

Pauli exclusion principle

Front 2

What are the four quantum numbers and what do they refer to?

Back 2

n principal quantum #
l azimuthal quantum #
angular momentum quantum #
m_l magnetic quantum #
m_s spin quantum #

Front 3

No two electrons in a given atom can posess the same quantum numbers is stated by:

Back 3

Pauli exclusion principle

Front 4

principal quantum number (n) is defined by

Back 4

energy level
(0, 1, 2, 3...n)

Front 5

azimuthal quantum number (l) is defined by

Back 5

shape of orbitals. subshells
(0, 1, 2, 3, up to n-1)
(s, p, d, f)

Front 6

The maximum number of electrons in energy level n is

Back 6

2n^2

Front 7

The maximum number of electrons that can exist within a subshell is given by

Back 7

4l+2

Front 8

For any given principal quantum number (n), the value of the azimuthal quantum number (l) ranges from

Back 8

0 to n-1

Front 9

The greater value of ___, the greater energy of the subshell.

Back 9

l

Front 10

The ____ value of l, the greater energy of the subshell.

Back 10

greater

Front 11

The greater value of l, the greater ________.

Back 11

energy of the subshell

Front 12

The greater value of l, the ______ energy of the subshell

Back 12

greater

Front 13

magnetic quantum number (m_l) is defined by

Back 13

orientation of the orbital in space
all integers (-l to l) including 0

Front 14

The possible values of m_l are

Back 14

all integers (-l to l) including 0

Front 15

spin quantum number (m_s) is defined by

Back 15

the direction of spin
(-1/2, +1/2)

Front 16

How many electrons can be in the same orbital?

Back 16

2

Front 17

The Pauli exclusion principle states that whenever two electrons are in the same orbital, they must have ____ spins

Back 17

opposite

Front 18

Subshells are ranked by increasing energy by finding

Back 18

n+l

Front 19

The lower the value of ___, the lower the energy of the subshell.

Back 19

n+1

Front 20

The ____ the value of n+l, the lower the energy of the subshell.

Back 20

lower

Front 21

The lower the value of n+l, the ____ of the subshell.

Back 21

lower the energy

Front 22

Hund's rule states that

Back 22

in subshells that contain more than one orbital, the orbitals are filled so that there are a maximum number of half-filled orbitals with parallel spins

Front 23

In Bohr's model of the hydrogen atom the energy of an electron is directly dependent on

Back 23

principal quantum number (n)

Front 24

What describes the excitation exhibited when an electron jumps from its ground state to a higher energy level?

Back 24

atomic absorption spectrum

Front 25

The Heisenberg uncertainty principle states that

Back 25

it is impossible to determine the momentum and the position of an electron simultaneously

Front 26

This says it is impossible to determine the momentum and the position of an electron simultaneously

Back 26

Heisenberg uncertainty principle

Front 27

What is planck's constant

Back 27

6.62E-34J*s

Front 28

What is the speed of light

Back 28

3E8 m/s

Front 29

What is the final orbital of Ca

Back 29

4s^2

Front 30

How many electrons in Ca

Back 30

20

Front 31

What is the final orbial and # of electrons if an atom has 20 electrons

Back 31

4s^2

Front 32

If an atom's final orbital is 4s^2, how many total electrons does it have

Back 32

20

Front 33

An energy (x) corresponds to the energy of an electron in which principal energy level?

What formula?

Back 33

E = -R_H/n^2

x = E
solve for n
R_H is given

Front 34

In going from 1s2-2s2-2p6-3s2-3p6-4s1 to
1s2-2s2-2p6-3s2-3p5-4s2 an electron would

Back 34

absorb energy

Front 35

In going from 1s2-2s2-2p6-3s2-3p5-4s2 to
1s2-2s2-2p6-3s2-3p6-4s1 an electron would

Back 35

emit energy

Front 36

How do you find the amount of energy it takes to move an electron from one energy level to another?

Back 36

E = -R_H ((1/n_i)^2 - (1/n_f)^2)

R_H = 2.18E-18J/electron

Front 37

How to determine the energy of a photon given the photon frequency?

Back 37

E=hv

h=planck's constant 6.62E-34J*s

Front 38

How to determine the wavelength given a photon that carries an x amount of energy?

Back 38

E = hc/wavelength

h=planck's constant 6.62E-34J*s

Front 39

On the periodic table electronegativity increases this direction

Back 39

up and to the right

Front 40

On the periodic table ionization energy increases this direction

Back 40

up and to the right

Front 41

On the periodic table atomic radius increases this direction

Back 41

down and to the left

Front 42

dipole-dipole interactions and dispersion forces are known as

Back 42

van der Waals forces

Front 43

van der Waals forces are

Back 43

dipole-dipole interactions and dispersion forces

Front 44

dipole-dipole interactions are formed by

Back 44

polar molecules arranging so that positive sides of molecules get close to negative sides of other molecules

Front 45

polar molecules arranging so that positive sides of molecules get close to negative sides of other molecules is called

Back 45

dipole-dipole interactions

Front 46

dipole-dipole interactions are negligible in this state phase

Back 46

gaseous

Front 47

_____ species tend to have higher boiling points than _____ species of comparable molecular weight

Back 47

Polar
nonpolar

Front 48

Polar species tend to have ____ boiling points than nonpolar species of comparable molecular weight

Back 48

higher

Front 49

Substances with hydrogen bonding tend to have ______ boiling points compared with compounds of similar molecular formula without H bonding

Back 49

unusually high

Front 50

Substances with ____ tend to have unusually high boiling points compared with compounds of similar molecular formula without _____.

Back 50

hydrogen bonding

Front 51

the short lived formation of dipoles caused by the rapid polarization and counterpolarization of the bonding electron cloud

Back 51

dispersion forces
london forces

Front 52

These kind of molecules possess greater dispersion forces

Back 52

large

Front 53

Large molecules possess more of this intermolecular force

Back 53

london dispersion forces

Front 54

How many moles in (x)grams of XY_2

Back 54

mol = weight of sample (g)
_________________________
total molar weight (g/mol)

Front 55

For the general reaction
aA + bB --> cC + dD

rate= ?

Back 55

rate = k[A]^x[B]^y

Front 56

The concentration of radioactive substance A at time t is found by

Back 56

[A_t] = [A_o]e^-(kt)

***
ln(A_t) = ln(A_o)-k*e*t

Front 57

How is the first order halflife of a reaction found

Back 57

t_(1/2) = ln (2/k) = .693k

Front 58

___ enthalpy change indicates an endothermic reaction

Back 58

negative

Front 59

___ enthalpy change indicates an exothermic reaction

Back 59

positive

Front 60

Negative enthalpy change indicates an _____ reaction

Back 60

endothermic

Front 61

Positive enthalpy change indicates an _____ reaction

Back 61

exothermic

Front 62

If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the reactants compared to the products

Back 62

very large

Front 63

If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain

Back 63

very little of the reactants compared to the products

Front 64

If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the products compared to the reactants

Back 64

very small

Front 65

If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain

Back 65

very little of the products compared to the reactants

Front 66

If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain approximately equal amount of reactants and products

Back 66

close to 1

Front 67

If K_eq is close to 1 compared to 1 an equilibrium mixture of reactants and products will contain

Back 67

approximately equal amount of reactants and products

Front 68

In an exothermic reaction adding heat will cause the reaction to

Back 68

shift to the left

Front 69

In an endothermic reaction adding heat will cause the reaction to

Back 69

continue forward faster

Front 70

An adiabatic process occurs when

Back 70

no heat exchange occurs in a system

Front 71

An isothermal process occurs when

Back 71

temperature of the system remains constant

Front 72

Isobaric process occurs when

Back 72

pressure of the system remains constant

Front 73

An isolated system occurs when

Back 73

it cannot exchange energy or matter with its surroundings

Front 74

A closed system occurs when

Back 74

it can exchange energy but not matter with its surroundings

Front 75

An open system occurs when

Back 75

it can exchange energy and matter with its surroundings

Front 76

To find the heat moved in a given process

Back 76

q = m*c*dT

m=mass
c=specific heat
dT=change in temp

Front 77

Given:
Several reactions and their changes in enthalpy. Calculate change in enthalpy for another reaction based on this.

Back 77

Comine given reactions, multiply/factor to cancel needed compounds on either side after adding is complete so that the final reaction is the same as the one that must be calculated for. Add the reactions' dH's to find the dH for the answer.

Front 78

Change in entropy is given by

Back 78

dS=Sfinal-Sinitial
dS=q_rev/T

Front 79

Change in Gibbs free energy is found by

Back 79

dG = dH - TdS

Front 80

If dG is negative the reaction is _______

Back 80

spontaneous

Front 81

If dG is positive the reaction is _______

Back 81

not spontaneous

Front 82

If dG is zero the reaction is ______

Back 82

in a state of equilibrium

Front 83

If dH = TdS the reaction is ____

Back 83

in a state of equilibrium

Front 84

If dH > TdS the reaction is ____

Back 84

not spontaneous

Front 85

If dH < TdS the reaction is ____

Back 85

spontaneous

Front 86

If dG is ____ the reaction is spontaneous

Back 86

negative

Front 87

If dG is ____ the reaction is not spontaneous

Back 87

positive

Front 88

If dG is _____ the reaction is in equilibrium

Back 88

zero

Front 89

The heat of formation of any element in its elemental state is

Back 89

0

Front 90

P1V1=?

Back 90

P2V2

Front 91

V1/T1=?

Back 91

V2/T2

Front 92

n1/V1=?

Back 92

n2/V2

Front 93

PV=?

Back 93

nRT

Front 94

P1V1
____ = ?
T1

Back 94

P2V2
____
T2

Front 95

density = ?

Back 95

m/v

P(MM)
_____
RT

Front 96

KE=(1/2)mv^2=

Back 96

(3/2)kT

Front 97

KE=

Back 97

(1/2)mv^2
(3/2)kT

Front 98

r1/r2 = ?

Back 98

sqrt(MM2/MM1)

Front 99

Natural processes want to decrease ____ and increase ____

Back 99

enthalpy
entropy

Front 100

Natural processes want to ____ enthalpy and _____ entropy

Back 100

decrease
increase

Front 101

Any process that increases entropy and decreases enthalpy will be

Back 101

spontaneous at any temperature

Front 102

Any process that does this will be spontaneous at any temperature

Back 102

increase entropy
decrease enthalpy

Front 103

The higher the molecular mass, the ___ the gas will diffuse

Back 103

slower

Front 104

The ____ the molecular mass, the slower the gas will diffuse.

Back 104

higher

Front 105

To find bond order from a MO diagram:

Back 105

subtract antibonding(*) electrons from bonding electrons and divide by two

Front 106

What type of amine is found as an organic salt?

Back 106

quaternary

NH4

Front 107

What are the colligative properties?

Back 107

lowering vapor pressure
boiling point elevation
freezing point depression
osmotic pressure

Front 108

What functional group cannot be formed from carboxylic acids?

Back 108

ethers

Front 109

In proton NMR, a peak with a shift between 6.0 and 9.5PPM denotes which functional group

Back 109

aromatic

Front 110

In proton NMR, a peak with a shift between 9.5 and 10.5PPM denotes which functional group

Back 110

aldehyde

Front 111

In proton NMR, a peak with a shift between 2.1 and 2.6PPM denotes which functional group

Back 111

ketone

Front 112

In proton NMR, a peak with a shift between 3.3 and 3.9PPM denotes which functional group

Back 112

ether

Front 113

The smaller the K_sp the lower the ___

Back 113

solubility

Front 114

The smaller the _____ the lower the solubility

Back 114

K_sp

Front 115

The ____ the K_sp the lower the solubility

Back 115

smaller

Front 116

Whatever is being oxidized is the ____

Back 116

reducing agent

Front 117

Whatever is being reduced is the ____

Back 117

oxidizing agent

Front 118

A gain in charge is ____

Back 118

oxidation

Front 119

A loss in charge is ____

Back 119

reduction

Front 120

A gain in electrons is ____

Back 120

reduction

Front 121

A loss in electrons is ____

Back 121

oxidation

Front 122

this hybridization is linear

Back 122

sp

Front 123

this hybridization is trigonal planar

Back 123

sp2

Front 124

this hybridization is tetrahedral

Back 124

sp3

Front 125

this hybridization is trigonal bipyrimidal

Back 125

sp3d

Front 126

this hybridization is tetrahedral

Back 126

sp3d2

Front 127

the shape of sp3d2 is

Back 127

octahedral

Front 128

the shape of sp3d is

Back 128

trigonal bipyramidal

Front 129

the shape of sp3 is

Back 129

tetrahedral

Front 130

the shape of sp2 is

Back 130

trigonal planar

Front 131

the shape of sp is

Back 131

linear

Front 132

How would you determine which part of an organic compound caused a peak on a mass spectrograph at X amu

Back 132

Find which molecular mass adds up to the given amu

Front 133

Which thermodynamics property tends to increase in a spontaneous process

Back 133

entropy

Front 134

What is the most advanced theory of molecular bonding

Back 134

MO theory

Front 135

A broad peak at 3200-3550cm^-1 in an IR spectrograph is

Back 135

-OH group

Front 136

A peak at 1630-1780cm^-1 in an IR spectrograph is

Back 136

carbonyl

Front 137

A peak at 2220-2260cm^-1 in an IR spectrograph is

Back 137

nitrile

Front 138

A peak at 2853-2962cm^-1 in an IR spectrograph is

Back 138

C-H stretch

Front 139

When asked to find the coordination number of the coordination complex, do this

Back 139

count the number of coordinate covalent bonds on the central atom

Front 140

K_sp = ?

Back 140

[A]^x * [B]^y ...

Front 141

LeChatelier's principle states that

Back 141

when a stress (change in concentration, temperature, volume, or total pressure) is applied to a system, the equilibrium will shift to relieve that stress

Front 142

Which is the anode and which is the cathode. What do the double lines represent

Cu|Cu2+ || Ag+|Ag

Back 142

Cu side is anode
Ag side is cathode

the salt bridge

Front 143

Cu|Cu2+ || Ag+|Ag

Where does oxidation occur

Back 143

at the anode on the left

Front 144

Cu|Cu2+ || Ag+|Ag

Where does reduction occur

Back 144

at the cathode on the right

Front 145

Meta directors do this

Back 145

help stabilize a positive charge on the meta position

Front 146

What is the order of oxidation for functional groups from lowest to highest

Back 146

alkyne
alkene
alkane
alcohol
ketone/aldehyde
COOH
CO2

Front 147

The dehydration of -COOH with an -OH yields what functional group

Back 147

ester

Front 148

What is the order of stability for a Carbon free radical from lowest to highest

Back 148

methyl
primary
secondary
tertiary

Front 149

Which of the following functional groups will have the greatest partial positive charge in carbon on the beta position to the functional group? Why?

amine
aldehyde
alcohol
alkene

Back 149

aldehyde

O has a large electronegativity so it has an inducive effect on adjacent carbons

Front 150

What results in a free radical

Back 150

homolytic cleavage

Front 151

homolytic cleavage results in

Back 151

a free radical

Front 152

The solution of a salt with a cation of a strong base and an anion of a weak acid will form what type of solution

Back 152

basic

Front 153

The solution of a salt with a cation of a weak base and an anion of a strong acid will form what type of solution

Back 153

acidic

Front 154

The solution of a salt with a cation of a ___ base and an anion of a ___ acid will form a basic solution

Back 154

strong, weak

Front 155

The solution of a salt with a cation of a ___ base and an anion of a ___ acid will form an acidic solution

Back 155

weak, strong

Front 156

As temperature increases reaction rates increase was an idea from

Back 156

Arrhennius

Front 157

If a gas is only on the product side of the equation it means

Back 157

entropy has increased

Front 158

If a gas is only on the reactant side of the equation it means

Back 158

entropy has decreased

Front 159

A solute in a liquid will cause vapor pressure ____

Back 159

depression

Front 160

To find heat capacity do this

Back 160

mass x specific heat

Front 161

to find rate of effusion

Back 161

rate 1
______ = sqrt(MW2/MW1)
rate 2

Front 162

wavelength x frequency =

Back 162

c (speed of light)

Front 163

On the periodic table atomic radii tend to increase

Back 163

down and to the left

Front 164

To determine which solutes in water will raise the boiling temperature the most:

Back 164

determine which solute produces the most moles when dissolved

Front 165

Given the initial concentration of a reactant in a first-order reaction, a rate constant, find the molarity after t seconds

Back 165

ln([A0]/A]) = kt

Front 166

When _______, equilibrium shifts in the direction to produce a smaller gas volume.

Back 166

pressure increases

Front 167

When _______, equilibrium shifts in the direction to produce a larger gas volume.

Back 167

pressure decreases

Front 168

This can react with either an acid or a base and is formed by an amphoteric element, which is an element that can react as a metal or a nonmetal

Back 168

An amphoteric oxide

Front 169

The larger the value of the equilibrium constant, K_A,

Back 169

the stronger the acid/base

Front 170

The smaller the value of the equilibrium constant, K_A,

Back 170

the weaker the acid/base

Front 171

What are the solubility rules

Back 171

-All salts formed with alkali metals
-All ammonium salts(NH4+) and nitrate salts (NO3-)
-Many chlorides bromides and iodides
-Many sulfates (SO4 2-)

Front 172

When _______, equilibrium shifts in the direction to produce a smaller gas volume.

Back 172

pressure increases

Front 173

When _______, equilibrium shifts in the direction to produce a larger gas volume.

Back 173

pressure decreases

Front 174

This can react with either an acid or a base and is formed by an amphoteric element, which is an element that can react as a metal or a nonmetal

Back 174

An amphoteric oxide

Front 175

The larger the value of the equilibrium constant, K_A,

Back 175

the stronger the acid/base

Front 176

The smaller the value of the equilibrium constant, K_A,

Back 176

the weaker the acid/base

Front 177

What are the solubility rules

Back 177

-All salts formed with alkali metals
-All ammonium salts(NH4+) and nitrate salts (NO3-)
-Many chlorides bromides and iodides
-Many sulfates (SO4 2-)

Front 178

These are the three steps to forming a polymer

Back 178

initiation - formation of free radical
propagation - chain lengthening step
termination - when something bonds to the free radical and discontinues the chain growth

Front 179

What kind of reactant is most likely to react with an aromatic compound

Back 179

eletrophile

Front 180

What type of alcohol will most rapidly undergo a dehydration reaction? Why

Back 180

tertiary
it will have the most stable carbocation intermediate, tertiary

Front 181

To find functional groups this spectroscopy is best

Back 181

IR

Front 182

To find molecular fragments this spectroscopy is best

Back 182

MS

Front 183

To find bonding structure this spectroscopy is best

Back 183

NMR

Front 184

1 mole of electrons is symbolized as

Back 184

1 faraday

Front 185

This is the only kind of nuclear decay that can increase atomic number

Back 185

beta decay

Front 186

When an aldehyde is oxidized it becomes

Back 186

carboxylic acid

Front 187

How is singlet/doublet/triplet/etc determined?

Back 187

count the number of H on the desired C and any adjacent C

Front 188

What represents the energy gained by giving an electron to an element

Back 188

electron affinity

Front 189

Ag+ + I- <--> AgI

what can be added to remove more silver from the solution

Back 189

KI

Front 190

In oxyacids, the _____, the stronger the acid

Back 190

more oxygen present

Front 191

In oxyacids, the more oxygen present the ______

Back 191

stronger the acid

Front 192

In polyprotic acids, the more hydrogen bonds of oxygen lost hydronium ions, the ____

Back 192

stronger the acid

Front 193

In polyprotic acids, ____, the stronger the acid

Back 193

the more hydrogen bonds of oxygen lost hydronium ions

Front 194

In equilibrium equations, ____ is not included because its will remain almost constant

Back 194

H2O

Front 195

H2O is not included in _______ because its concentration will remain almost constant

Back 195

equilibrium equations

Front 196

H2O is not included in equilibrium equations because

Back 196

its concentration will remain almost constant

Front 197

This is the formation of a solid from a gas

Back 197

deposition

Front 198

Causing a reaction to occur by increasing the temperature increases the influence of this

Back 198

entropy

dG = dH - TdS

Front 199

What kind of isomer will rotate plane polarized light

Back 199

enantiomer

Front 200

This has chiral carbons that cancel the rotation of light out on each other

Back 200

diastereomer

Front 201

What type of amine is most alkaline in water

Back 201

tertiary

Front 202

A Claisen rearrangement yields what type of compound

Back 202

phenol derivative
o-substituted phenol

Front 203

Ether oxidizes to this

Back 203

CO2

Front 204

Alpha decay does this

Back 204

reduces atomic number by 2

Front 205

Beta decay does this

Back 205

increases the atomic number

Front 206

When naming a benzene ring, constituents on adjacent carbons go in this order (carbon 1, 2, 3)

Back 206

ortho, meta, para

Front 207

A Claisen condensation will produce what

Back 207

beta keto ester

Front 208

This is the reaction of esters in the presence of sodium ethoxide

Back 208

Claisen condensation

Front 209

These are created by a dehydration reaction with a carboxylic acid and an alcohol

Back 209

esters

Front 210

These are created by a dehydration reaction with a carboxylic acid and an amine

Back 210

amides