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Chem 105 > Chem test 3 study deck > Flashcards

Chem test 3 study deck Flashcards

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1
Q

What is the 1st law of thermodynamics?

A

the law of conservation of energy

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2
Q

What does the law of conservation of energy state?

A

Energy can be neither created nor destroyed

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3
Q

What is the mathematical equation for the 1st law of thermodynamics?

A

delta E universe= delta E sys +delta E surr=0

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4
Q

________ is the part of the universe that is the focus of the thermodynamic study

A

system

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5
Q

A system can be
1.
2,
3.

A

Isolated
Open
closed

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6
Q

_______ is everything in the universe that is not of the system

A

surroundings

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7
Q

The ______ is system+ surroundings

A

universe

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8
Q

_____ systems exchange both energy and matter

A

open

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9
Q

______ systems exchange only energy

A

closed

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10
Q

_______ systems do not exchange energy and matter

A

isolated

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11
Q

______ and ______ functions describe how properties of a system depend on changes

A

path and state

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12
Q

_____ functions are properties that depend only on current state of a system and not on the path taken to reach that state

A

state

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13
Q

enthalpy, entropy, pressure, temperature, and volume are _____ functions

A

state

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14
Q

______ functions are properties that depend on the specific path taken to reach a particular state

A

path

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15
Q

heat (q) and work (w) are _____ functions

A

path

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16
Q

What is the equation for energy change to the system?

A

Delta E= q+w

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17
Q

______ is energy transferred between objects because of difference in their temperatures

A

heat

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18
Q

_____ is heat leaving the system

A

exothermic

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19
Q

______ is done when a force (f) moves and object through a distance (d)

A

work

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20
Q

What are the two equations for work?

A

w= F(d)
w= -Pdelta V

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21
Q

work done by the system is energy _____ by the system

A

lost

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22
Q

work done by chem system is ______ of gas

A

expansion

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23
Q

solid to gas is _____

A

endothermic

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24
Q

liquid to gas is ____

A

endothermic

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25
Q

solid to liquid is _____

A

endothermic

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26
Q

gas to solid is _____

A

exothermic

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27
Q

gas to liquid is _____

A

exothermic

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28
Q

liquid to solid is _____

A

exothermic

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29
Q

______ _____ ______ is energy required to change amount of something by 1 degree K

A

specific heat capacity

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30
Q

What is the equation for calorimetry?

A

q=mcdeltaT

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31
Q

____ is the heat absorbed or given off by the system

A

q

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32
Q

If the system has two or more components how do you find the energy?

A

delta E= m1c1deltaT +m2+c2Delta T ….

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33
Q

______ is the amount of heat necessary to raise the temperature of 1 g of water 1 C

A

calorie

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34
Q

_______ J = 1 cal

A

4.184 J

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35
Q

What is the equation for enthalpy?

A

delta H= delta sys+ P delta V

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36
Q

q(p) - heat to _____

A

system

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37
Q

exothermic has ______ delta H

A

negative

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38
Q

endothermic has ______ delta H

A

positive

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39
Q

(delta r) H, the subscript r denotes ___ _____ of ____

A

per mole of reaction

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40
Q

What are the three ways to calculate delta r H

A
  1. Hess’s Law
  2. Enthalpies of formation
  3. Bond dissociation enthalpies
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41
Q

If a reaction can be broken into a series of steps delta H for the overall reaction will be equal to the sum of the ______ changes for the individual steps

A

enthalpy

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42
Q

_______ ____: use of reactions with known enthalpies to find enthalpy of unknown reaction

A

Hess’s law

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43
Q

If reaction is reversed, the enthalpy of reaction changes _____

A

sign

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44
Q

If coefficients in a balanced reation are multiplied by an value, the value of ______ is multiplied by the same value

A

delta H

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45
Q

Magnitude of delta H is _______ proportional to the quantities of reactants and products in a reaction

A

directly

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46
Q

pure elements in their most stable form at 25 C and standard sate conditions are assigned a delt Hf value of ____

A

zero

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47
Q

What are the standard state conditions for delta H

A

1 bar pressure, (1 atm)
1 M concentration
25 C

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48
Q

What is the equation for delta H r with delta Hf

A

[ v[ delta Hf (prod)- [ Vr delta H f (react)

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49
Q

most thermodynamic quantities depend to some degree on _____

A

temperture

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50
Q

enthalpy changes as changes in ____ strengths

A

bond

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51
Q

Breaking bonds _____ energy

A

requires

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52
Q

Bond dissociation enthalpies are only applicable for reactions in which all components are _____

A

gases

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53
Q

all gas-phase DH values are _____

A

positive

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54
Q

What is the equation for bond dissociation enthalpies?

A

dletar H= [ DH react+ DH(prod)

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55
Q

______ the heat needed to convert 1 mole of a solid at its melting point to 1 mole of liquid

A

molar heat of fusion

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56
Q

what is the equation for molar heat of fusion

A

q=ndeltaH fus

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57
Q

________ is the heat needed to convert 1 mole of a liquid at its boiling point to 1 mole of vapor

A

molar heat of vaporization

58
Q

What is the equation for molar heat of vaporization?

A

q= ndelta Hvap

59
Q

_______ is a device used to measure the absorption or release of heat by a physical or chemical process

A

calorimeter

60
Q

______ is the distance between two peaks or troughs in a wave

A

wavelength (lambda)

61
Q

______ is the number of waves (cycles) per second that pass a given point in space

A

frequency (v)

62
Q

______ is the speed of light

A

speed (c)

63
Q

What is the value of c?

A

3.00 E * m/s

64
Q

The units of wavelength is _____

A

m

65
Q

v (frequency) has units of

A

s^-1

66
Q

What is the equation for c?

A

c= v (lambda)

67
Q

What are the two key observations in accordance to light and nature of matter

A

-blackbody radiation
-photoelectric effect

68
Q

In blackbody radiation objects heated strongly _______ light

A

irradiate

69
Q

In blackbody radiation, an ideal object is one which absorbs and emits all ______ of radiation

A

frequencies

70
Q

T or F: light acts like a particle and a wave

A

TRUE

71
Q

Energy can be gained or lost only integer multiples of _____

A

hv

72
Q

What is Plank’s constant?

A

h (6.626x10^-34 J(s)

73
Q

T or F: light only transferred in packets

A

TRUE

74
Q

What is a packet of light called?

A

quanta

75
Q

A _____ is a particle of light

A

photon

76
Q

What is the equation for the energy of a photon?

A

Ephoton= hv or Ephoton=hc/lambda

77
Q

As lambda increases, the energy of photons _______

A

decreases

78
Q

ejection of electrons when metal is subjected to ______

A

light

79
Q

The intensity increase of incoming light should increase ____ of electrons

A

KE

80
Q

If there is more intensity there are more _____

A

photons

81
Q

What is De Broglie’s equation for wavelength?

A

lambda= h/m (u)

82
Q

______ _______contains all the wavelengths of visible light

A

continuous spectrum

83
Q

______ spectrum, each line corresponds to a discrete wavelength

A

line

84
Q

Problems with classical physics:
The solution to blackbody radiation: classical physics that an idealized object should emit infinite energy at high frequency is…

A

energy is quantized and emitted in discrete packets called quanta

85
Q

Problems with classical physics:
The solution to photoelectric effect, that classical wave theory suggested that increasing the light’s intensity should provide enough energy to release electrons from a metal surface regardless of light frequency is…..

A

light behaves as both a particle and wave, with photons carrying quantized energy based on frequency

86
Q

Problems with classical physics:
The solution to electrons orbit a positively charged nucleus is…

A

Bohr proposed that electrons exist in specific quantized orbits with fixed energies, where they do not raidate light, only transitions between these orbitals involve energy exchange

87
Q

Problems with classical physics:
The solution to why atoms emit light at specific frequencies creating spectral lines is…

A

quantum mechanics explains that electrons occupy discrete energy levels, and light is emitted or absorbed only when elected transitions between these levels creating distinct spectral lines

88
Q

Problems with classical physics:
The solution to assuming that it is possible to know both the position and momentum of a particle precisely is….

A

Heisenberg principle, when position is certain, momentum is uncertain

89
Q

Problems with classical physics:
The solution to electrons being characterized as a particle or wave is

A

it being a particle that acts like a wave

90
Q

Problems with classical physics:
The solution to knowing an electrons locality is

A

entanglement” particle share quantum state

91
Q

In Bohr’s model, the atom consists of electrons revolving around nucleus in _____ orbits

A

circular

92
Q

What is the equation for calculating the energy associated with each orbital?

A

E= -2.178E-18 J (z^2/n^2)

93
Q

Electrons closer to nucleus have more _____ energy

A

negative

94
Q

T or F: more negative means strong attraction

A

True

95
Q

How can you calculate the energy from an electron changing orbitals?

A

E= -2.178E-18(1^2/ n^2 final - 1^2/n^2 initial)

96
Q

Bohr model works for calculating _____ (which element)

A

hydrogen

97
Q

As electron is brought closer to the nucleus, energy is _____ from the system

A

released

98
Q

What is the equation for Heisenberg Uncertainty principle/

A

deltaX deltamu >= h/ 4 pie

99
Q

What type of wave has
uncertainty in wavelength:0
uncertainty in p: 0
and uncertainty is delta X= infinite

A

monochromatic

100
Q

In what type of wave is
there:
uncertainty in wavelength: infinite
uncertainty in p= infinite
uncertainty in delta x=0

A

superposition of waves

101
Q

T or F: energies of electronic orbitals are not quantized

A

FALSE

102
Q

T or F: Electronic orbital can be described as a standing wave

A

TRUE

103
Q

True or False: in quantum mechanic there must be whole number of half wave lengths

A

TRUE

104
Q

______ describes the quantum state of a particle or system of particles

A

wavefunction

105
Q

With wavefunctions if wavelengths don’t match up they have ______ interference and therefore cancel out

A

destructive

106
Q

What is the Schrodinger equation?

A

H (weird y)= E (weird y)

107
Q

weird y^2 represents the probability of finding an ______ in specific point

A

electron

108
Q

Wavefunction describes an atomic _____

A

orbital

109
Q

_______ are regions where the probability of finding an electron is zero

A

nodes

110
Q

_____ nodes are spherical regions around the nucleus where the probability of finding an electron is zero

A

radial

111
Q

What is the equation for radial nodes?

A

n-l- 1

112
Q

______ nodes are flat planes where the probability of finding an electron is zero

A

planar

113
Q

What is the equation for planar nodes?

A

l

114
Q

increasing n means _____ orbital

A

larger

115
Q

n defines a ____

A

shell

116
Q

the angular quantum number is ___

A

l

117
Q

___ determines the shape of the atomic orbital

A

l

118
Q

What is the equation for l?

A

n-1

119
Q

what letter is
l=0

A

s

120
Q

what letter is
l=1

A

p

121
Q

what letter is
l=2

A

d

122
Q

what letter is
l=3

A

f

123
Q

what is the magnetic quantum number ?

A

ml

124
Q

ml is related to the _____ of the orbital

A

orientation

125
Q

ml has values between _ to _

A

-l to l

126
Q

The electron spin quantum number is ____

A

ms

127
Q

ms has values of
1.
2.

A

-1/2, 1/2`

128
Q

What principle says no two electrons in an atom can have the same 4 quantum numbers?

A

Paule exclusion principle

129
Q

What three quantum numbers define the orbital?

A

n, l, ml

130
Q

The number of orbitals in each subshell is determined by the possible ____

A

ml

131
Q

A larger n values means a _____ energy

A

higher

132
Q

T or F: electrons in the ground state have the lowest energy possible

A

TRUE

133
Q

All orbitals with the same principal quantum number have _____ energy

A

degenerate

134
Q

electrons form ions to _____ the shell

A

fill

135
Q

______ describes atoms/ ions having identical electron configurations

A

isoelectronic

136
Q

When electrons are lost lost to make cations they lose electrons from the orbitals with the highest ___ value first

A

n

137
Q

T or F: Half-filled and completely filled subshells tend to be more stable than partially filled

A

TRUE

138
Q

________ _____ is the energy required to remove e- from gaseous atom

A

ionization energy

139
Q

______ _____ is the energy released as atom accepts electron

A

electron affinity

140
Q

Potassium channels are selective for _____ because the inside of the channel is lined with oxygen atoms which have a partial negative charge

A

cations

141
Q

______ is the attraction of atom to electrons

A

electronegativity

142
Q

_______ energy is the energy released when solid ionic crystal formed from ions in gaseous state

A

lattice

Chem 105 (24 decks)

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