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chemistry > flashcards > Flashcards

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1
Q

What is chemistry?

A

study of electrons, atoms and molecules that make up matter and the changes they undergo during some process

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2
Q

adding sig figs

A

stay the same exponent

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3
Q

multiplying sig figs

A

adding the exponents

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4
Q

how many sig figs in 0.31

A

2

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5
Q

sig figs in 12.0

A

3

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6
Q

in 0.310

A

3

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7
Q

sig figs in addition

A

lowest amount after decimal

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8
Q

multiplication/division

A

least amount of sig figs

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9
Q

converting between units

A

amount * (how much/in one unit)
2.46$ to pennies
2.46 * (100 pennies/1dollar) = 246

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10
Q

how much is 1 kg in g

A

1000

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11
Q

how much is 1 L in cm^3

A

1000 cm^3

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12
Q

law of conservation of mass

A

matter isn’t created or destroyed

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13
Q

dalton’s atomic theory (4):

A

1) all matter is made up of small, indivisible particles called atoms
2) atoms in same element have same mass (diff elements, diff properties)
3) atoms of diff elements combine in simple whole number ratios
4) chemical reactions result in separation, combination or rearrangement of atoms

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14
Q

dalton definition

A

atoms are small and indivisible

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15
Q

mass # = ?

A

a # protons + # neutrons

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16
Q

atomic # = ?

A

a # protons

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17
Q

isotopes

A

atoms having same # protons but diff # neutrons

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18
Q

atomic mass units (amu)?

A

masses of atoms = mass #

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19
Q

mass # ?

A

average of isotopic masses

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20
Q

molecular formula

A

exact # and ratio of each element
(H2O)

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21
Q

structural formula

A

how atoms are bonded together
(H-O-H)

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22
Q

empirical formula

A

simplest whole # ratio (H2O2 = HO)

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23
Q

avogadros number

A

6.022 x 10^23 = 1 mole

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24
Q

molar mass

A

mass in grams of 1 mole = mass #

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25
Q

molecular mass

A

average mass (amu)

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26
Q

molecular formula

A

some multiple of empirical formula

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27
Q

chemical reaction

A

process in which a substance is changed into one or more new substances

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28
Q

stoichiometry

A

study of quantitative aspects of chemical recations

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29
Q

what does the quantity of product formed from a reaction depend on?

A

amount of reactant available

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30
Q

limiting reagent

A

consumed reagent

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31
Q

excess reagent

A

leftover reagent

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32
Q

limiting reagent is the

A

substance is is not enough to consume other reactant

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33
Q

molarity (M)

A

moles solute/litres solution

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34
Q

Molality (m)

A

moles solute/kg solvent

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35
Q

mole fraction (Xa)

A

moles/ (moles a + moles b + moles c)

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36
Q

weight percent

A

(g solute/g solution) x 100%

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37
Q

what are the 2 methods to prepare solutions of a specific concentration?

A

1 - weight out a solid solute and dissolve in a given quantity of solvent
2 - dilute a concentrated solution to give one that is less concentrated

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38
Q

preparing solutions by dilution shortcut?

A

(Mi)(Vi)=(Mf)(Vf)

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39
Q

what are 3 characteristics of gases

A

1 - uniformly fill any container
2 - mix with any other gas
3 - exert pressure on its surroundings

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40
Q

pressure =

A

force/area (units of Pa = N/m^2)

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41
Q

1 atm = ?

A

101.325 kPa = 760 mm Hg

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42
Q

manometers?

A

finding pressure of enclosed gas

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43
Q

ideal gas law

A

pV=nRT (is emprirical)

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44
Q

gas density

A

d = (p(MM))/(RT)

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45
Q

for mixture if gases, overall pressure??

A

sum of all partial pressures (p1 + p2 + p3)

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46
Q

what is kinetic molecular theory?

A

theoretical model to explain macroscopic behaviours based on microscopic properties of atoms and molecules in gas

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47
Q

what are the assumptions of KMT?

A

1 - gas molecules are in straight line constant motion
2 - volume of individual particles is 0
3 - collisions cause pressure exerted by gas
4 - particles don’t attract to repel each other except during collisions
5 - average KE is proportional to temp of gas (K)

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48
Q

pressure exerted is proportional to?

A

1 - momentum w/ which gas particles hit the wall (momentum = mv)
2 - rate of collisions w/ the wall

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49
Q

p =

A

= = (Nmv^2)/V

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50
Q

3d p =?

A

= = (Nmv^2)/3V

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51
Q

KE = ?

A

(1/2)(mv^2)

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52
Q

particles travel faster…?

A

when they are light and at higher temperatures

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53
Q

diffusion

A

gradual mixing of molecules of diff gases

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54
Q

effusion

A

escape of gas from its container thru a small hole

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55
Q

graham’s law

A

(RateA)/(RateB)= sqrt(MMb/MMa)

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56
Q

do real molecules have volume

A

yes

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57
Q

gases will exhibit behaviour closest to ideal behaviour at?

A

high temperatures and low pressures

58
Q

thermochemistry

A

energy changes involved in chemical reactions

59
Q

energy

A

capacity to do wrok or to produce heat

60
Q

potential energy

A

= energy available to a system due to the position of system

61
Q

kinetic energy

A

energy available due to motion on object

62
Q

1st law of thermodynamics

A

total energy of universe is constant

63
Q

state function =

A

property of a system that can be defined by current state system (independent of pathway)

64
Q

what are examples of state functions

A

energy, pressure, volume and temperature

65
Q

universe =

A

system + surroundings

66
Q

when is change in energy positive?

A

when energy flows into system

67
Q

when is change in energy negative?

A

when energy flows out of system

68
Q

internal change

A

sum of KE and PE

69
Q

change in internal energy =

A

sum of heat produced/consumed by system and work done on or by the system (U = q + w)

70
Q

heat =

A

flow of thermal energy between susbatnace that are at diff temps (ttansfer of energy between 2 objects)

71
Q

work

A

movement against a force = f x d

72
Q

when is heat positive? negative?

A

+ = absorbed by system
- = absorbed by surroundings

73
Q

when is work pos? neg?

A

+ = work done on system
- = work done by system

74
Q

1 cal =

A

4.184 J

75
Q

temperature

A

property that reflects motions of particles in substance

76
Q

heat capacity (C) =

A

heat energy required to raise the temp of a given quantity of substance by a given temperature

77
Q

specific heat capacity =

A

heat absorbed/mass

78
Q

molar heat capacity =

A

heat absorbed/moles

79
Q

work done by a gas

A

expansion

80
Q

work done to a gas

A

compression

81
Q

w =

A

p(change in V)

  • pressure is external pressure = positive
  • change in V is pos = volume is inc
  • w is negative = work done by system

System = -p(change in v)

82
Q

what drives chemical reactions

A

thermodynamics and kinetics

83
Q

enthalpy of reaction =

A

heat given off or absorbed by a reaction at constant pressure (change in H)

84
Q

endothermic

A

heat flows into system

85
Q

exothermic

A

heat flows out of system

86
Q

reversing a chemical equation will reverse sign of enthalpy for reaction

A

true

87
Q

heat of solution?

A

heat generated/absorbed when a certain amount of solute dissolves in a certain amount of solvent

88
Q

reversible reaction is in equilibrium when (3)

A

1 - rates of forward and reverse reaction are equal
2 - the conc of reactants and products remain constant (but not equal to each other)
3 - molecules are in constant motion (dynamic)

REMEMBER NOT ALL REVERSIBLE REACTIONS ARE IN A STATE OF EQUILIBRIUM

89
Q

what is constant?

A

ratio of products to reactants raised as an exponent (K = products/reactants)

90
Q

Kp (pressures in atm)

A

gas-phase reactions

91
Q

Kc

A

solution reactions

92
Q

Ka

A

acid appears on left of reaction

93
Q

Kb

A

base appears on left of reaction

94
Q

Ksp

A

solid compound dissolves

95
Q

gases drive equilibria more than liquids or solids

A

true

96
Q

reversing = reciprocal of value of K

A

true

97
Q

multiplying coefficient by variables = multiply the equilibrium const to the corresponding power

A

true

98
Q

overall reaction is sum of 2 reactions

A

true

99
Q

sum of 2 more reactions = equilibrium const is product

A

true

100
Q

le chartaliers principle

A

in external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium

101
Q

external stress?

A

conc, temp, pressure/volume for gases

102
Q

reaction will shift away from added component to consume that component

A

true

103
Q

for gases which side will the side shift too? (pressure is inc)

A

side that decreases the number of moles of gas until equilibrium is established

104
Q

for gases which side will the side shift too? (pressure is dec)

A

side that increases the number of moles of gas until equilibrium is established

105
Q

as volume inc, what happens to pressure?

A

decrease

106
Q

why does temperature change and cause change in K?

A

because to consume any added heat

107
Q

If T inc… (endothermic)

A

K increases

108
Q

If T inc… (exothermic)

A

K decreases

109
Q

Arrhenius acids?

A

substances ionize in water to produce H+ ions

110
Q

arrhenius base?

A

substances that ionize in water to produce OH- ions

111
Q

bronsted acid

A

proton donor

112
Q

bronsted base

A

proton acceptor

113
Q

strong acids are… what in water?

A

completely ionized because they are strong electrolytes

114
Q

monoprotic acids

A

acids that have one ionizable proton

115
Q

diprotic acids

A

acids that has 2 protons that can be donated pr the formula

116
Q

polyprotic acid

A

acid that has more than 2 protons that can be donated per formula

117
Q

metal hydroxides are?

A

strong bases

NaOH = Na+ + OH-

118
Q

conjugate base

A

species that remains after a bronzed acid has lost its proton

119
Q

conjugate acid

A

protonated species that is formed after a bronsted base gains a proton

120
Q

how do conjugate acid/base pairs differ?

A

molecular formulas only differ by one proton

121
Q

in aqueous solutions containing acids… water acts as a

A

base

122
Q

in aqueous solutions containing bases… water acts as a

A

acid

123
Q

autoionization

A

pure water will ionize to a small extent

124
Q

pH =

A

pH = -log[H3O+]

125
Q

pOH =

A

-log[OH-]

126
Q

do stronger bases have large or small Kb

A

large

127
Q

do weaker bases have large or small Kb

A

small

128
Q

CH3OO- (aq) + H2O (l) = OH- (aq) + CH3COOH

A

yes

129
Q

Hydrolysis

A

reaction of the cation or anion of a salt with water to produce a change in the pH of solution

130
Q

which ones don’t undergo hydrolysis

A

group 1 and 2 metal

if an anion is conjugate base of a strong acid

if anion is the conjure base of a weak acid

if cation is the conjug acid of a weak base

131
Q

common ion effect

A

shift in equilibrium caused by addition of a compound having an ion in common w/ the dissolved substanvce

132
Q

buffer solution

A

relatively large concentrations of a weka acid and conjugate base or a weak base and its conjugate acid (resist changes in pH)

133
Q

molar solubility =

A

the max number of moles of solute that can be dissolved in a given volume of solvent at a specific temperatire (Ksp)

134
Q

solubility

A

max mass of solute that can be dissolved in a given volume of solvent at a specific temp

135
Q

saturated

A

Q = Ksp

136
Q

unsaturated

A

Q < Ksp

137
Q

superstaurated

A

Q > Ksp

138
Q

how to decrease solubility of a salt?

A

adding a common ion

139
Q

kinetics

A

how fast does a reaction proceed

140
Q

Cr

A

4s13d5

141
Q

Cu

A

4s13d10

chemistry (3 decks)

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