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MCAT > General Chemistry > Flashcards

General Chemistry Flashcards

1
Q

what is the definition of % mass solution??

A

Mass solute/ ( mass solute + mass solvent = mass solution )

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2
Q

3 fold dilution

A
  • dilute to 3x less than initial

- 2 part water and 1 part solution

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3
Q

Oxidation

A

it loses electrons

mneumonic “ OIL RIG”

OIL - oxides it loses e-
RIG = Reduction it gains e-

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4
Q

reduction

A

gains electrons

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5
Q

Reducing agent

A

helps reduce other agents ( REDUCTANT) and it get oxidized

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6
Q

oxidizing agent

A

acts like an oxidant ( oxidizes other reagents) and gets itself redued.

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7
Q

Solubility Rules: Salts containing Alkali metals cation with ( Li+, Na+, K+, Cl-)

A

water soluble

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8
Q

Solubility Rules: Salts containing Nitrate( NO3-)

A

water soluble

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9
Q

Salts containing halide anion( Cl-, Br-, I-)

A

water soluble except Ag+, Pb2+

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10
Q

Solubility Rules: Salts containing (SO4) 2-

sulfate

A

water soluble except Ba2+, Pb 2+, Hg 2+, Ca2+

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11
Q

Solubility Rules: Salts containing ( OH-) hydroxide

A

are slightly water soluble.

  • KOH and NaOH are substantially soluble, while Ca(OH)2, Sr(OH)2, and Ba(OH)2 are fairly soluble
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12
Q

Solubility Rules: Salts containing Carbonate( CO3) 2-, chromate ( CrO4-), phosphate anion ( PO4) 3-, sulfide ( S2-)

A

Slightly soluble

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13
Q

MNEUMONIC FOR LIMITING REAGENT

mole ratio A/B > balanced mole ratio A/B
then what is the limiting reagent?

mole ratio A/B

A

mole ration A/B > balanced mole ration A/B

THEN B is the limiting reagent

mole ratio A/B

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14
Q

oxidation state of oxygen

A

-2 except with peroxide

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15
Q

oxidation state of hydrogen

A

+1

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16
Q

oxidation state of halide

A

-1

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17
Q

1/5=

A

0.2

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18
Q

1/6=

A

0.166

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19
Q

1/7=

A

0.143

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20
Q

1/8=

A

0.125

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21
Q

1/9=

A

0.111

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22
Q

1/10=

A

0.1

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23
Q

1/11=

A

0.091

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24
Q

1/12=

A

0.083

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25
Q

for molecular molecules, the number of hydrogens must be

A

it must be an even number

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26
Q

Does molality change with temperature?

A

NO , molality doesn’t change with temperature

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27
Q

Does molarity change with temperature

A

Yes, molarity changes with temperature

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28
Q

Does density change with temperature

A

Yes, density changes with temperature

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29
Q

Does specific gravity change with temperature

A

Yes, specific gravity changes with temperature

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30
Q

Lower pKa ->

A

stronger acid and weaker base

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31
Q

Higher pKa

A

weaker acid and stronger base

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32
Q

if pH >pka, the molecule is?

A

deprotonated

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33
Q

if pH

A

protonated

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34
Q

Solid >—solid/liq—-> Liquid—> lig/gas—> gas

is what kind of process

A

endothermic ( it absorbs energy to break the bonds and release the molecules)

mneumonic - it takes energy to break bonds

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35
Q

Solid

A

exothermic ( release energy as bonds are made)

Mneumonic - when bonds are made, everyone is happy and energy is released.

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36
Q

Name the types of systems in thermodynamics

A
  • isolated
  • closed
  • open
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37
Q

Define Isolated system

A

no exchange of hear, work, or matter with surroundings

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38
Q

Define closed system

A

exchange of heat and work, but no matter with the surrounding

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39
Q

Define open system

A

exchange of heat, mass, and work with the surroundings

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40
Q

Define a state function

A

a system that is path -independent and depneds only on the initial and final states

examples: 
delta H ( enthalpy) 
Delta S ( entropy) 
Delta G (  Gibbs free energy) 
delta U ( internal energy change)
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41
Q

Conservation of Energy

A
  • the total amount of energy in an isolated system remains constant.

total energy is neither gained nor lost, it is merely transferred between the system and its surrounding
.

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42
Q

define Endothermic reactions

A

Energy is ABSORBED by the reaction in the form of heat.
delta H is positive
MNEUMONIC : H STANDS FOR HEAT

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43
Q

Define exothermic reactions -

A

energy is RELEASED by the reaction in the form of heat

Delta H is negative
MNEUMONIC : H STANDS FOR HEAT

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44
Q

delta H is the change in heat content of a reaction

A

+ means heat is ABSORBED

  • means heat is RELEASED
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45
Q

Bond dissociation energy define

A

it is the energy nrequired to break bonds

Energy in the reactants - products

the sign is POSITIVE because energy is required to break bonds

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46
Q

define Entropy

A

a measure of disorder

measured in J/K

Entropy of gas>liqiud>solid

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47
Q

define free energy

A

Free energy is the energy available that can be converted to do work.

Delta G = Delta H - T delta S

T is in kelvin

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48
Q

Sponantenity of a reaction relies on what?

A

Gibbs free energy

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49
Q

Spontaneous reaction has what sign of delta G

A

NEGATIVE aka exogonic

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50
Q

NONSPONTANEOUS reaction has what sign of delta G

A

POSITIVE aka endogonic

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51
Q

NONSPONTANEOUS reaction has what sign of delta G

A

POSITIVE aka endogonic

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52
Q

First law of thermodynamics

Del U= Q+W

A

is based on the principle of conservation of energy, and it basiclaly says that the change in total internal energy of a system is equal to the contributions from work and heat.

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53
Q

what is the Q in the first law of thermo?

A

HEAT

Q is positive –> the heat is being absorbed
Q is negative –> the heat is being released

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54
Q

What is the W in the first law of thermo?

A

WORK

Work is positive - when work is being done ON the system
Work is negative - when work is being done BY the system.

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55
Q

Second law of thermodynamics Entropy

A
  • 2nd law states that the things like to be in a state of hihger entropy and disorder
  • an islolated system will increase in entropy over time
  • an open system can decrease in entropy, but only at the expense of a greater increase in entropy of its surroundings

The universe as a whiole is increasing in entropy.

delt S >= q/t

reversible systems Delt S=q/t
irreversible systems det D>q/T

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56
Q

define heat of fusion

A

del H fusion = energy input needed to melt something from solid to liquid and vice versa
latent heats are measured as Joules/mass

therefore Q=mL where m = mole and L= latent heat of vaoprization or fusion

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57
Q

define heat of vaporiation - delt H vap =

A

= del H vap= energy input needed to vaporize something from liquid to gas and vice versa.

latent heats are measured as Joules/mass

therefore Q=mL where m = mole and L= latent heat of vaoprization or fusion

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58
Q

Area of a PV diagram gives you what?

A

WORK!

PV diagrams depict thermodynamic processes by plotting pressure againsst volume

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59
Q

Name the types of processes in thermodynamics

A
  • adibatic process
  • isothermal processs
  • isobaric process
  • isovolumetric ( isochoric ) process
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60
Q

Define Adiabatic process

A
  • NO heat exchange

Q=0

Det U = W

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61
Q

Isothermal Process

A

no change in temperature aka delta U = 0

the change in work = change in heat

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62
Q

isobaric process

A

constant pressure

W=Pdet V

P=0

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63
Q

Isovolumetric process ( isochoric(

A

no change in volume.
work = P det V=0 because there is no change in volume.

det U = Q

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64
Q

Mole M = It/nF

A

Helps determine moles of element being depositied on a plate
“ moles of M” it is eNouF

65
Q

Electrons flow which way? Anode to cathode or cathode or anode?

A

Anode to Cathode ( negative charge flows away from Negative anode)

A—-> C

66
Q

Current ( +) Charge flows cathode to anode or anode to cathode

A

Cathode to anode ( posituve charge flows away from positive cathode)`

C—-> A

67
Q

Arrhenius Equation

A

k=Aexp(-EA/RT)

k=rate constant
A= frequency factor

EA=activation energy
R= Ideal Gas Constant
T= temerature

A decrease in EA or Increase in T will increase K

68
Q

Arrhenius Equation

A

k=Aexp(-EA/RT)

k=rate constant
A= frequency factor

EA=activation energy
R= Ideal Gas Constant
T= temerature

A decrease in EA or Increase in T will increase K

NOT DEPENDENT ON ENTHALPY

69
Q

Lower the pka=more acidic

A

Resonance can help stablize

  • relative aciditity of a acid can be judged on the stabilization of its conjugate base of that acid

the stronger the acid, the more stablized the base,

70
Q

Gibbs free energy formula

A

delt G=del H-T Del S

Del H=enthalpy
Del S= Entropy

  • del H - del S ( same sign temp dep) LOW T

+ del H + del S ( same sign temp dep) HIGH T

-del H + del S EXOTERHMIC

+delH - del S Endothermic

71
Q

Solubility of molecules in a solute depends on temperature and its nature of solute and solvent

A

example: N2O gas at 248 compared to 298

Gas in lower temperature will dissolve better in fluid - additionally since H2O is polar- it will dissolve polarity better than nonpolar.

72
Q

Atomic Number

A

Atomic Number identifies the atom –> will tell you the number of proton

73
Q

Mass Number

A

mass number will indicate the entire mass of the atom

Neutron + proton

74
Q

During a phase change, what is constant?

A

During a phase change, temperature is constant!!

75
Q

Convection is defined as ?

A

Convection is defined as the movement of heat through liquid and gas

76
Q

Hund Rule

A

Parallel spin 1st occupy degenerate orbital that are parallel spins

77
Q

Aufbau principle

A

fill up the lowest orbiral first

78
Q

Pauli exclusion principle

A

opposite spin and no atom can have the same quantum numbers

79
Q

Changes in del S, del H, and Del G are state functions

therefore it only depends on its initial and final states

A

independent of path

80
Q

pKa +pKb=14 only applies to compounds

A

pka of acid and pka of conjugate base OR

pkb of base with pka of its conjugated acid

81
Q

Bronsted lowry acid =

A

Donate H+

82
Q

Bronsted Lowrey Base

A

Accept H

83
Q

Lewis Acid

A

accept electrons

Mneuominc : Lewis - think lewis strucures and electrons
ACid = Acceptance

electron acceptance

84
Q

Lewis base

A

donate electrons

Mneuominc : Lewis - think lewis strucures and electrons

85
Q

Lewis base

A

donate electrons

Mneuominc : Lewis - think lewis strucures and electrons

86
Q

“Strong” and “Weak” is respect to acid and bases - in terms of the degree to which it dissociates

A

Strong acid = 100% complete dissociation

therefore how much of Acid present compared to its conjugate base

87
Q

rate law /constant = wht

A

rate=k[A][B]

is there is an increase in temperature, k increases and therefore the rate constant also increases

88
Q

thermodynamic properties are not involved with kinetics

A
  • it deals with equilibrium ( thermodynamics)

- kinetics = deals with how to get the reaction to where it needs to be.

89
Q

Exothermic reactions deals with thermodymanics or kinetics?

A

thermodynamics?

90
Q

if there is BOILING POINT question, look for HB

A

increase HB causes increase in BP

91
Q

TLC plates ( aka thin layer chromatrography) - are silica plates that are very polar aka the stationary phase is polar

mobile phase = nonpolar substance

A

molecule with affinity for polar phases will have a lower Rf

nonpolar molecules will have a greater Rf

Rf is calculated distance substance traveled / mobile phase line traveld.

92
Q

Which atom has the smallest radius?

K
K+
Ar
Cl-

A

K+, Cl- and Ar are all isoelectic - which means they al have the same number of electrons YET the K+ have more protons which increases the Zeff therefore making the radius the smallest

93
Q

Most ideal gases experience very WEAK intermolecular forces WHY ? it wants to reduce the pressure component

A

HCl + NaOH = polar
HF + NaOH = polar
HF + CH4 = polar

HCl + CH4 = both are nonpolar and they have very low intermolecular forces

94
Q

at the equilvance point

mole H + = mole OH -

A

Need to keep in mind of the molarity

NaVa= NbVb

95
Q

at the equilvance point

mole H + = mole OH -

A

Need to keep in mind of the molarity

NaVa= NbVb

96
Q

Potassium

K–> K+ e- exothermic reaction

A

Normally all the small alkali metals are spontaneously reactive

97
Q

Gram eq weight defintion

A

molar mass/ number of protons

98
Q

EMF = E red, red - E red, ox

A

Reduced = more positve Emf = therefore has the ability to do work since it agained Electrons and it gained ENERGY

99
Q

Gas –> solid is called what?

A

deposition

100
Q

SOlid –> gas

A

sublimiation

101
Q

Liquid -> gas

A

vaporization

102
Q

Gas –> liq

A

condensation

103
Q

Solid –> liq

A

meltilng

104
Q

liq- solid

A

freezing

105
Q

Hydrogen bonding only occues when?

A

only occures when molecules have F,O,N and directly bonded to hydrogen.

106
Q

inert gas has what type of molecular interaction?

A

london dispersion

107
Q

Absolute O is when?

A

0 Kelvin

108
Q

Isothermal occurs more slowly

adiabatic = occur quickly * therefore the graphs look more sleep ) ( no heat exchange(

A

when trying to determine if something is compressed or expanded, look at the volume ( final - initial )

109
Q

Lewis Acid -

A

Accepts electrons

Molecules with incomplete octet ( AlCl3, BF3)

  • simple cation except ( alkali + heavy alkaline earth metal )
  • smaller cation with high charge = more electropillic
110
Q

Lewic base

A

Donates electrons

111
Q

Bronsted Lowey Acid

A

DOnate proton

112
Q

Bronstred Lowry Base

A

Accept proton

113
Q

Arrehnis acid

A

Makes H+

114
Q

Arrenhenis base

A

makes OH

115
Q

Strong Acid Name them

A 
Hydroiodic Acid    HI 
HydroBromic Acid  HBr 
Hydriochloric Acid  HCl 
Nitric Acid                HNO3 
Percholoric Acid     HClO4 
Choloric Acid          HClO3
Sulfuric Acid             H2SO4
116
Q

Strong Base

A 
Sodium Hydroxide   NaOH 
Potassium Hydroxide KOH 
Amide Ion                   NH2 - 
Hydride                       H-
Calcium Hydroxide  Ca(OH)2
Sodium Hydroxide    NaOH
Calcium oxide            CaO
117
Q

Acid disscociation decreases with acid concentration

A

think about the le chatlier principle if too much protons around, less likely to move

118
Q

Hydride

basic / netral = Hydride + Metal ( NaH(=)

Acid/Neutral = Hydride = nonmetal

A

Acidity of a nomental hydride transds to increase going down a periodic table ( probably becayse it doesnt want to hang on to its protons any more )

H20 < H2S< H2Se< H2Te

119
Q

Hydride

basic / netral = Hydride + Metal ( NaH(=)

Acid/Neutral = Hydride = nonmetal

A

Acidity of a nomental hydride transds to increase going down a periodic table ( probably becayse it doesnt want to hang on to its protons any more )

H20 < H2S< H2Se< H2Te

120
Q

Strong acid titarte with weal base

A

Ph < 7

121
Q

Strong base with weak acid

A

pH > 7

122
Q

Weak acid and weak base

A

if pKa of acid is lower than pKb of base then ph of eq pt will be ph<7

if pkb of base is lower than the pka then the pH of the eq point will be greater than 7

123
Q

In galvanic cells EMF = +

In electrolytic Cells EMF = -

A

Reduction always occurs in the cathode

oxidation always occurs in the anode k

124
Q

In terms of electrochemistry, oxized element will have more negative potential than the one being reduced in an galvanic cell

A

In a galvanic cell- the reduaction potential of the cathode cannot be less the anode because

emf = Ered, cat- E red, anode and the EMF must be postive

125
Q

Metal gives up electrons

A

Nonmetals take electrons

126
Q

Acid ending in - ic makes anions ending in - ate

A

sulfuric acid –>sulfate

ate has more oxygens than ite

127
Q

acid ending in - ous makes anions ending it - ite

A

US we AIGHT

nitrous acid –> nitrite

128
Q

Affinity Chromatorgraphy -

A

coat beads with receptor and the ligand will bind. Once the protien is retained, elute by washing with free receptor adn it will release it off the bead

129
Q

Size exclusion chromatography

A

Bead with small poes - smaller the size, the more slowed down because small object get stick in a small pore.

130
Q

Ion exchange chromatography

A

column coated with charged substance so it will bind to compoung with opposite charge

131
Q

Extraction

A

Used to separate organic and aquaous phases

132
Q

Filtration

A

seperate solid from liquid

133
Q

name the types of distillation

A
  • simple
  • vacuum
  • fractional
134
Q

Simple distillation

A

when the boiling point is more than 25 degrees apart from each other

135
Q

fractional distillation

A

when the two boiling points are 25 degrees within each other

136
Q

vacuum filtration

A

when the boiling points are greater than 150 C and need to decrease boiling point and its vapor pressure

137
Q

vacuum filtration

A

when the boiling points are greater than 150 C and need to decrease boiling point and its vapor pressure

138
Q

Boiling point of a liquid= temperature at which the vapor pressure of the liquid = the surface pressure

A

normal boiling pressure point is measured at 1 atm pressure.

Vapor pressure increases with temperature.

if the surface pressure decreases then the boiling point decreases

therefore in a vacumm, the surface pressure is low therefore the boiling point is low.

if there is aleak in the system, the surface pressure will increase and therefore increase the boiling point

139
Q

When atoms have the same number of electrons, the number of protons ( greatest will have the smallest size)

A

this is because it has the greatest number of protons which will cause more pulling and the Zeff will be higher in this case

140
Q

More arrangement = entropy is decreased

A

entropy typically means disorder

141
Q

gamma rays = represent ionizating energy

A

that is why is it horrible for yu.

142
Q

formal charge =

A

of valence electrons - sticks-dots

143
Q

at side chain pka, 50% protonated and 50 % deprotonated

A

this is where the half eq point happens where conj Base = acid and the concentrations are the same

144
Q

pH+pOH= 14
Ka*Kb=Kw=10^-14

pKa + pKb = 14

A

pkb ( add base to water )
B- + h20 –> HB + OH -

kb= [HB][OH-]/[B-]

pka ( add acid to water )

HA + h20 —> A- + h3o+

pka = [A-][h3O+]/HA

145
Q

pH+pOH= 14
Ka*Kb=Kw=10^-14

pKa + pKb = 14

A

pkb ( add base to water )
B- + h20 –> HB + OH -

kb= [HB][OH-]/[B-]

pka ( add acid to water )

HA + h20 —> A- + h3o+

pka = [A-][h3O+]/HA

146
Q

During titrations, it is important to note if it is monoprotic or diprotic. it is also good to note if it starting as an acid or a base. A good way to determine this is see what the acidity or basicity is if there is no titrant added. this will tell you where you should start.

A

acid titraated with strong base = start acidic

base titrated with strong acid = start basic

note you can only titrate with strong acid and strong bases because it will fully dissociate

147
Q

During titrations, it is important to note if it is monoprotic or diprotic. it is also good to note if it starting as an acid or a base. A good way to determine this is see what the acidity or basicity is if there is no titrant added. this will tell you where you should start.

A

acid titraated with strong base = start acidic

base titrated with strong acid = start basic

note you can only titrate with strong acid and strong bases because it will fully dissociate

148
Q

galvanic cells and concentration cells do not use a battery. it is spontaneous. in terms of the line notation it goes anode || cathode

A

in concentration cells, the anode is less concentratied and the cathode is more concentrated.

149
Q

geometry / shape refers to the position of the atoms not the electrons

A

molecular geometry - where atoms are located

electron geometry - where elctrons are located.

150
Q

air bubbles are often inserted into a boiling system to prevent superheating.

A

acts similar to boiling chips.

151
Q

define first ionization energy

A

first ionization energy si the energy required to remove an electron from the outer shell of an atom.

for a given period, it is the loweest when the removal of the electron results in a complete shell or subshell, and the highest when the removal of the electron disrupts a full complete shell or subshell.

noble gases will have the highest ionziation energy and the alkali metals ( potasium for example) - will have the loweest highest ionization energy.

152
Q

define first ionization energy

A

first ionization energy si the energy required to remove an electron from the outer shell of an atom.

for a given period, it is the loweest when the removal of the electron results in a complete shell or subshell, and the highest when the removal of the electron disrupts a full complete shell or subshell.

noble gases will have the highest ionziation energy and the alkali metals ( potasium for example) - will have the loweest highest ionization energy.

153
Q

to determine the number of protons and neutrons an atom has - look at the mass number and its atomic number…. the atomic number will indicate the protins and you can substrae that from the mass number to get the number of neutrons

A

in order to determine the number of elecctrons, protons = electrons if the charge is neutral.

154
Q

to determine the number of protons and neutrons an atom has - look at the mass number and its atomic number…. the atomic number will indicate the protins and you can substrae that from the mass number to get the number of neutrons

A

in order to determine the number of elecctrons, protons = electrons if the charge is neutral.

155
Q

hydrogen = metal or nonmetal

A

nonmetal

156
Q

molecules that contain strongly electron withdrawing or electron donating substituents - are highly polae and posses high dipole moments

A

example glycine AA molecule. COOH and the NH3 groups make strong dipole

157
Q

rate constants must have units in inverse time ( s^-1)

A

0 order : not dependent on concentration
1st order : rate order unit is ( s^-1 )
2nd order : M^-1 * s^-1

158
Q

define coordination number

A

coordination number typically occurs in coordinated covalent bond such that it describes the numeber of moelcules are around the ion.

159
Q

Bond enthalthy

A

the amount of heat required to break a bond

therefore the smaller the bond, the stronger the bond and more energy required to break it.

MCAT (10 decks)

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