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Chem Final Flashcards

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1
Q

Limiting reactant/reagant

A

the reactant that gets used up first and therfor limits amount of product that can be formed

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2
Q

KMT-Kinetic Molar Theory

A
  • Helps you understand what happens with a gass
  • is a model
  • Gasses consist of large #s of molecules that are in continuous random motion. Speed and direction can change
  • The Combined volume of all of the moleculed of the gas is negligible relative to the total volume in which the gass is contained.
  • attrative and repulsive forces between gas moleculed are negligible because they are going too fast
  • The average KE of the molecule is proportioanal to the absolute tem (kelivin)
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3
Q

elastic

A

no KE is lost

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4
Q

KE

A

KE=1/2mvsquare

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5
Q

slow molecules=____ temp

A

cooler

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6
Q

fast molecules=____ temp

A

warmer

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7
Q

Properties of gas-

A

expansion, fluidity, have minimal inter molecular attraction(moving too fast)

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8
Q

diffusion

A

the spread of one substance throughout a space or throughout a 2nd substance

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9
Q

effusion

A

the escape of gas molecules thorugh a tiny hole into an evacuated space

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10
Q

Light gas travles_____ than heavy gass

A

faster

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11
Q

heavy gas travels___ than light gas

A

slower

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12
Q

Grahms Law

A

the rate of effusion for a gas is inversely proportioal to the square root of its molar mass (also for diffusion)

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13
Q

pressure(def)

A

the amount of force applied on an area

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14
Q

Atmospheric pressure

A
  • the weight of air per unit of area

- 1.00 atm=760 torr

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15
Q

manometer

A

used to measure the difference in pressure between atmospheric pressure and that of a gas in a vessel

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16
Q

Standard pressure

A
  • normal atmospheric pressure at sea level

- 1atm/760torr/101.325 KiloPasals

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17
Q

Dalton’s law of partial pressure

A

-the total pressure of a mixture of a gas equals the sum of the pressures that each would exert if it were present alone
Ptotal=p1+p2+p3…..

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18
Q

intermolecular force

A

between molcules(weak)

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19
Q

intramolecular force

A

within a molecule

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20
Q

van der waal forces

A

the sum of the attractive or repulsive forces between molecules (intermolecular forces)

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21
Q

London Dispersion forces

A
  • weakest
  • for a sec most electrons are one one side which becomes more (-) that the other side
  • causes polarity
  • a near atom would become dipole b/c it would repel
  • everything has london
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22
Q

Polarizability

A
  • the tendancy of an electron to distort

- strength of force is related to molecular weight. more weight=more force

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23
Q

Larege atoms are ___ to polarize

A

easier

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24
Q

A shorter dipole moment vector means a ___ polar bond

A

less

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25
Q

a longer dipole moment vector means a ___ polar bond

A

higher

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26
Q

molecules that have permanent dipoles are ____ to eachohter

A

attracted

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27
Q

the more___ a molecule the higher its boiling point

A

polar

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28
Q

hydrogen bonding

A
  • extreme dipole
  • A hydrogen bond is a type of attractive (dipole-dipole) interaction between an electronegative atom and a hydrogen atom bonded to another electronegative atom. This bond always involves a hydrogen atom. Hydrogen bonds can occur between molecules or within parts of a single molecule. A hydrogen bond tends to be stronger than van der Waals forces, but weaker than covalent bonds or ionic bonds.
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29
Q

what elements bond during hydrogen bonding

A

H to (N,O, or F directly) because they are the most electronegative elements.

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30
Q

What is the fundimental differnece between states of matter?

A

distance between particles.

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31
Q

Fluid

A

substance that can flow and take its containers shape (gas/liquid)

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32
Q

what is the most dense state of matter

A

solid (liquid id a close 2nd)

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33
Q

what is the most compressible state of matter

A

gas

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34
Q

surface tension

A

results from the net inward force experienced by the molecules on the surface of a liquid

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35
Q

cohesion

A

attraction of a substance to itself

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36
Q

adhesion

A

attraction of a substance to a surface

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37
Q

crystaline sold

A

particles are in highly ordered arrangement

-a unit cell is the smalled arangement of atoms in a crystal that has the same symmetry as the whole crystal

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38
Q

amorphous

A

no particular order in the arrangement of particles (glass)

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39
Q

how many types of solids are there and what are their names?

A

2 different types
crystaline-ordered
amorphous-not ordered

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40
Q

ion crystal

A

metal-non metal
either S or P
Non-metal is usually P block or poly atomic
held together by ionic

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41
Q

covalent network

A

looking at one big molecule

held together by covalent

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42
Q

metalic crystals

A

not covalent bonds
too strond to be van der waals
held by metalic

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43
Q

covalent molecular crystals

A

in a molecular solid the molecules are held together by relativily weak intermolecular forces

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44
Q

as more molecules escape the liquid, the pressure they exert _____

A

increases

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45
Q

THe boiling pressure of a liquid is the temp at which___________

A

the vapor pressure equals atmospheric pressure

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46
Q

the normal boiling point is the temp when to vapor pressure is ____

A

760 torr

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47
Q

Heat of fusion

A

energy required to change a solid at its melting point to a liquid

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48
Q

does the temperature change change during a phase change?

A

no

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49
Q

molar heat

A

energy needed change 1 mol

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50
Q

tripple point

A

whare all 3 states are in equalibrium

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51
Q

gasses

A

expand to fill their container
highly compressible
have extremely low densities at normal atmospheric pressure at sea level

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52
Q

Boyle’s Law

A
  • the volume of a fixed quantity of gas at constant temp is inversely proportional to the pressure
  • P1+V1=P2=V2
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53
Q

hwo to convert kelvin to celsius

A

C+273.15

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54
Q

charles law

A

the volume of a fixed amount of gas at constant pressure is directly prportiolan to is absolute tem
V1/T1=V2/T2

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55
Q

Gay Lussac’s Law

A

the pressure of a fixed amount of gas at constant volume varies directly with temp
P1/T1=P2/T2

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56
Q

Avogadro’s Law

A

the volume of gas at constant temp and pressure is directly proportional to the # of moles of the gas

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57
Q

one mol of gas will occupy ____ volume as any other gas at the same temp and pressure

A

same

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58
Q

STP

A

standard temp and pressure

0 degrees celcius adn 1 atm

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59
Q

at STP one mol of gas occupies _____

A

22.4 L

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60
Q

IDeal gas law

A

PV=nRT

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61
Q

mixture

A

2 or more things put together

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62
Q

solution

A

2 or more things mixed together that you cant see the different things(homogeneous)

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63
Q

suspensions

A

a mix that contains particles large enough to be settled out by gravity

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64
Q

colloids

A

a mix where the particles are much larger than individual molecules, but still too small to settle out by gravity

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65
Q

how big are colloid particles typically?

A

1000 nm in diameter

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66
Q

tyndall effect

A

colloids ccan scatter light- how to tell a solution from a colloid

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67
Q

thixotropic mixture

A

kind of a solid/ kind of a liquid

ex: toothpaste

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68
Q

brownian motion

A

crazy erratic random motion of colloid particle

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69
Q

what causes brownian motion

A

the collisons of the colloid particles with the dispersing medium

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70
Q

Solvant

A

have the most of in a solution

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71
Q

solute

A

have the least of in a solution

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72
Q

immiscible

A

liquids that are no soluble

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73
Q

miscible

A

liquids that dissolve freely in one another in any proportion

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74
Q

soluble

A

a substance that disolves in a solvant

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75
Q

saturated

A

a solvant is holding as much as possible at that temp

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76
Q

unsaturated

A

less than saturated/ can hold more

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77
Q

super-saturated

A

holds more than is possible(unstable)

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78
Q

% by mass

A

(mass of solute/mass of solution)(100)

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79
Q

% by volume

A

(volume of solute/volume of solution)(100)

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80
Q

Molarity

A

M=mol of solute/L of Solute
M= mol of solution/ L of solution
M=mol/L
since volume is temp dependant molarity can change with temp

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81
Q

Molality

A

m=mol/L

not temp dependant

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82
Q

mole fraction

A

(moles of solute)/(mols of solute+moles of solvent)

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83
Q

dilution

A

the process of adding water to a concentrated of stock solution to achieve the molarity desired for a particular solution

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84
Q

does dilution change number of mols of a solvant/solution

A

no

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85
Q

like dissolve like

A

the intermolecular forces between solute and solvant particles must be strong enough to compete with those between solute particles and those between solvent particles

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86
Q

solvate

A

a solution forms the, the solvent pulls solute particles apart and surrounds them

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87
Q

ion dipole is ____ than hydrogen bonding

A

higher

88
Q

“hydrated”

A

bonded with water

89
Q

If an ionic salt is soluble in water it is because____

A

the ion-diole interations are strong

90
Q

____ is known as the universal solvent

A

water\

O-H bonds

91
Q

what three things have to happen for a solution to form

A

-separate solute particles (takes energy)
-seperate solvent particles (takes solvent particle)
-new interactions between solute and solvent (release energy)
the enthalpy change of the overall process depends on the change in H for each of these steps

92
Q

the more ___ the intermoleular attractions the more likely two substances are to be soluble with each other

A

similar

93
Q

what makes something soluble in water

A

having a lot hydrogen bonding

94
Q

polar disolves in ____

A

polar

95
Q

non polar disolves in ___

A

nonpolar

96
Q

in general the solubility of gas in water increases with increasing ___

A

mass

97
Q

the solubility of liquid and solid ____ change with pressure

A

doesnt

98
Q

gas solubility is ____ related to pressure

A

directly

99
Q

Henry’s Law

A

S1/P1=S2/P2
where S is the solubility of gas
and P is pressure

100
Q

Solubility rate increases with///

A

temp
agitation
surface area

101
Q

one mol of a soluble molecular compound will produce ____ mol(s) of a particle in the solution

A

1

102
Q

1 mol of a soluble ionic compound will produce _____ 1

mol of solution

A

more than

103
Q

Changes in colligative properties depend on _____

A

of particles, not type of particle

104
Q

colligative properties

A

properties of solutions that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the type of chemical species present

105
Q

the vapor ressure of a solution is ___ than that of the pure solvant

A

lower

106
Q

vapor pressure of solutions

A

because of solute-solvant intermolecular attraction, higher concentrations of nonvolatiles soluts make it hard for solvant to escape to the vapor phase

107
Q

nonvolitile

A

Nonvolatile refers to a substance that does not readily evaporate into a gas under existing conditions.

108
Q

boiling point elevation and freezing point depression

A

non volatile solute-solvent interactions also cause solutions to have higher boilng points and lower freezing points than the pure solvent
Δ T= K(m)
where Δ T is the boiling point K is a constant and m is molality

109
Q

Δ T= K(m) (x)

what is X

A

x is the number of particles that one solute particle actually produces in solution
for molecular compounds x=1

110
Q

osmosis

A

diffusion of a solvent through a semipermeable membrane

111
Q

Semi permeable membranes

A

are barriers that allow some particles to crossq

112
Q

vant hoff factor

A

reassociation is more likely at higher concentration there fore the # of particles present is concentation dependant

113
Q

energy

A

the ability to do work or transfer heat

114
Q

work

A

used to cause an object to move
energy used to move an object over some distance is work
w=f(d)

115
Q

heat

A

energy used to change the temp higher is heat

116
Q

heat flows from ____ to ____

A

warmer objects; cooler objects

117
Q

kinetic energy

A

energy an object posses by virtue of its motion

118
Q

temperature

A

measure of the average kinetic energy of the particles

119
Q

What is the SI unit of energy

A

Joule

120
Q

1 calorie is….

A

4.18 J

121
Q

law of conservation of energy

first law of thermodynamics

A

energy can be converted from one forme to another but it can be neither created nor destroyed

122
Q

system

A

part of the universe you are focusing on

123
Q

surrounding

A

everything that is not the system

124
Q

endothermic

A

heat goes in to your system from the surrounding

125
Q

exothermic

A

release energy/heat

126
Q

energy gained by the surrounding=

A

energy lost from the system

127
Q

freezing is an ____thermic process

A

exo

128
Q

heat capacity

A

energy required to raise the temp 1 K/1 C

129
Q

specific heat

A

the amount of heat per unit mass required to raise the temperature by one degree Celsius

130
Q

specific heat equation

A

q=mcΔt

131
Q

heat lost by hot=____

A

heat gained my cold

132
Q

enthalpy

A

the internal energy plus the product of pressure and volume of a system

133
Q

is there a way to tell the exact amount of enthalpy of a system?

A

no, but we can measures changes in enthalpy

Δ H

134
Q

how to determine Δ H

A

take the enthalpy of the products minus the enthalpy of the reactants
Δ H=H products-Hreactants

135
Q

when Δ H is (+)

A

a process is endothermic

136
Q

when Δ H is (-)

A

a process is exothermic

137
Q

enthalpy is extensive property

A

dependent on sample size

138
Q

the Δ H for the reverse reaction is _____

A

equal in size but opposite size than the forward reaction

139
Q

Δ H of a reaction depends on

A

the state of the products and reactants

140
Q

1000 cal= how many kcal

A

1 kcal

141
Q

1 k cal is how many kJ

A

4.184 kilo joules

142
Q

thermo chemical equations

A

a balanced equation that includes states of matter of all reactants and products and the energy change

143
Q

enthalpy (or heat) of combustion

A

the enthalpy change for the complete combustion of one mol of the substance

144
Q

standard conditions

A

NOT STP

1 atm and 25 celcius

145
Q

molar enthalpy of vaporization

A

the heat required to vaporize one mole of a liquid

146
Q

molar enthalpy of fusion

A

the heat required to melt one mol of solid

147
Q

Hess’s Law

A
  • if a reaction is carried out in a seried of steps Δ H for the overall reaction will be equal to the sum of the enthalpy changes for the individual step
  • because Δ H is a state function the total enthalpy change depends only on the initial state of the reactants and the final state of the products
148
Q

enthalpy for motion- Δ Hf

A

the enthalpy change for the reaction in which one mol of a compound is made from its constituent elements in their elemental forms
-for any element in its elemnetal for Δ Hf=0
measued under standard conditions

149
Q

driving forces of reaction spontaneity

A
  • enthalpy (the majority of cchemical reactions are exothermic. products are more stable than the reactants.
  • the tendancy of nature is to proceed in a direction that leads to lower energy
150
Q

are all spontanious reactions exothermic?

A

no

151
Q

entropy

A

can be though of as a measure of the randomness of a system

-related to moles of motion of molecules

152
Q

the 2nd law of thermodynamics

A

the entropy of the universe is always increasing

in any spontanious process ther is an increase in the entropy of the universe

153
Q

the number of microstates and the entropy tends to increase with increase in….

A
  • temp
  • volume
  • # of independantly moving molecules
  • increases with the freedon of motion of molecules
154
Q

what state has the highest entropy

A

G>L>S

155
Q

3rd law of thermodynamics

A

The entropy of a perfect crystal, at absolute zero kelvin, is exactly equal to zero

156
Q

free energy changes

A

ΔG=ΔH-TΔS

T is the temperature on the Kelvin scale. In introductory courses we make the assumption that DeltaHo and DeltaSo, do not change as the temperature changes.

when G is negatice the reaction is sponaneous.
ΔH is the enthalpy term
TΔS is the entropy term

157
Q

rate deifinition

A

how fast a reaction takes place

158
Q

factors effecting rate

A 
collision frequency
collision efficiancy
nature(where they are in the activity series)
surface area
presence of catalyst
conentration
159
Q

how is temperature related to reaction rate

A

is related to KE
Related to speed/velocity
the higher the temp the higher the KE
the higher the KE the easier it is to get over the energy barrier

160
Q

how is concentration related to reaction rate

A

increasing the reactant concentration results in…

  • more collisions
  • more collisions per second(higher conentration frequency)
  • Higher KE
  • more collisions per second
  • greater statistical chance
  • more reactant molecules with enough energy to happen
  • the actual affect must be measured experimentally
161
Q

Catalyst

A
  • do not change energy of reation
  • DO change the rate
  • heterogeneous=different state than reaction
  • homogeneous=same state
162
Q

Rate Law

A
  • an equation that related reaction rate and concentrations of reactants
  • only applicable for a specific reaction at a given
163
Q

order definition

A

the power to which a reaction oncentration is raised

164
Q

orders of rate law

A

0 order- has no effect as long as it is there
First order=directly
Second=square of coefficient of reactant
may or may not match the coefficients

165
Q

how does the rate law constant change with temp?

A

increases with temp

166
Q

order of the reaction

A

sum of all the orders

167
Q

Inhibitor

A
  • substance that slows down reactions

- opposite of a catalyst

168
Q

the rate (is conctant/changes) over the course of the reaction

A

changes

169
Q

reactions mechanism

A

the step-by-step sequence of reactions by which the overall chemical change occurs.
-consists of the complete sequene

170
Q

intermediates

A

species that appear in some steps but not in the net equation

171
Q

simple/elementary reaction

A

occurs in one step
-the reaction rate of that step is proportional to the product of the reactant concentrations, each of which is raised to its stoichiometric coefficient

172
Q

complex reaction

A

ours in 2 or more steps

  • the rate law is determined from the slowest step because it has the lowest rate.
  • rate determining step
173
Q

rate determining step

A

slowest rate step in a reaction

174
Q

can a reaction go backwards

A

yes

175
Q

if the reaction is exothermic in forward then it is ____ in the backwards

A

endothermic

176
Q

is the rate of a chemical reaction constant?

A

no

177
Q

equalibrium

A

whent the 2 reaction rates (both forward and backwards) become equal

178
Q

dynamic equalibrium

A

stoff is still goin on a equal rates

179
Q

equalibrium constant

A 
-Keq
aA+bB=cC+dD
rateforward=k[A]a[B]b
ratebackwards= k[C]c[D]d
in equilibrium ratef=rateb
so.. k[A]a[B]b= k[C]c[D]d
Or..
(Kf/Kr)=( [C]c[D]d/[A]a[B]b)=Keq
PRODUCTS OVER REACTANTS COEDDICIENTS BECOME EXPONENTS- SOLIDS AND LIQUIDS DON’T GO IN
180
Q

Keq is ___ the initial concentrations

A

independent of

181
Q

Keq is _____ to temp

A

dependant

182
Q

Keq is found_____

A

experimentally

183
Q

why are pure solids and liquids omitted from the Keq equation

A

their concentration cannot change

184
Q

Keq<10 to the (-3)

A

mostly reactants

185
Q

Keq>10 to the (3)

A

mostly products

186
Q

Keq between 10 to the -3 and 10 to the 3rd

A

balanced

187
Q

how many equalibrium positions are there for a single reaction?

A

many

188
Q

equalibrium positions

A

a set of concentrations that result in equalibrium

189
Q

le chateliers principle

A

if a system at equalibrium is distured by a change in tem. pressure, or concentration of one of the components the system will shift its equalibrium position so as to counteract the effect of the disturbance

190
Q

equalibrium will shift ___ from the side you add to

A

away

191
Q

equalirium will shift-___ the side you take from

A

towards

192
Q

gas equalibrium

A

increase pressure=decrease container volume
derease container volume=increase concentration of gas
high pressure favors the side with the lowest volume
with more reactant gas molecules, equalibrium shifts to the right
with more product gas molecules equalibrium shifts to the left

193
Q

solubility product constant

A

Ksp
-similar to Keq of a sparingly soluble salt
-the product of the molar concentrations of its ions in a saturate solution
–bassically the product of the ion concentrations
-raised to the power of their coeffs
Ksp=[A]a[B]b

194
Q

reaction quotient

A
  • Q

- basically Keq but not at equilibrium. Use same equation but with concentratiosn that do not result in Keq

195
Q

Q= Keq

A

at equilibrium

196
Q

Q<Keq

A

Shifts to the right(consuming reactants and forming products to attain equilibrium)

197
Q

Q>Keq

A

shifts to the right (consuming products and forming reactants to achieve equilibrium.

198
Q

Qsp

A

Qsp

-if you sub in initial concentrations in to Ksp equation you do not get the SOLUBILITY PRODUCT you will get Q

199
Q

Qsp=Ksp

A

saturated solutions and nothing happens

200
Q

Qsp<Ksp

A

Unsaturated and no precipitate forms

201
Q

Qsp>Ksp

A

A precipitate will form and reduce the concentrations of the ions until the products of their concentrations in Ksp expression equals the numerical value Ksp

202
Q

Common ion effect

A
  • Shift in equilibrium position that occurs because of
    the addition of an ion already involved in the
    equilibrium reaction.
     An application of Le Châtelier’sprinciple.
    The lowering of the solubility of a substance because of the presence of a commo ion is called the common ion effect.
203
Q

properties of acids

A
  • sour taste
  • ractive
  • burns
  • turns blue litmus paper red
  • ph less than 7
  • reacts with active metals to produce H2
  • reacts with carbonates
  • conducts electric currents
204
Q

properties of bases

A
  • bitter
  • slippery
  • turns red litmus paper blue
  • ph greater than 7
  • conducts electric current
205
Q

binary acids

A

countains only 2 elements
typically hydrogen plus one of the mroe elctronegative elemets
-ic

206
Q

oxy acids

A

omosed of hydrogen, oxygen and a third element

207
Q

acid naming

A

i ATE something ICky and it gave me and (ITE)(OUS)

208
Q

arrhenius

A

defined an aid as any electrolite that produces H+ ions when dissolved in water

defined a base as any eletrolye that produces hydroxide

209
Q

what do u get when you put base in acid

A

salt water

210
Q

bronsted lowry

A

acid=anything that gives an H+
base=anything that takes a H+
water acts as a bronstead lowry base and abstracts

211
Q

Lewis definition of base and acid

A

acid=e- pair acceptor

base=e- pair donor

212
Q

weak acid/bases

A

implies that little or only partial dissociation

213
Q

strong acid/bas

A

implies complete dissociation

-any soluble OH in a base is strong

214
Q

conjugate

A
  • means to join together
  • when you add an acid and a base you get conjigate aid and base
  • acid has more H+
  • the species that remains after a bronstead lowry acid has given up a proton in the onjugate base of that aicd
  • the species that is formed when a bronstead lowry base gains a proton is the conjugate acid of that base
215
Q

vaporization

A

solid/liquid to gas

216
Q

volitile

A

vaporizes easily

Chem 2 (10 decks)

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