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CHM 141 + 144 > CHM 141 final > Flashcards

CHM 141 final Flashcards

1
Q

conversion from one state of matter to another

A

Phase change

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2
Q

the change in enthalpy to melt a solid into a liquid

A

heat of fusion

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3
Q

the change in enthalpy to turn a liquid into a gas

A

heat of vaporization

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4
Q

the change in enthalpy to change a solid to a gas without passing through the liquid phase

A

heat of sublimation

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5
Q

vaporization + fusion =

A

sublimation

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6
Q

what equation should you use for the line B-C on a heating curve? (flat line)

A

q =m*heat of vaporization/ heat of fusion

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7
Q

what equation should you use for the line E-F on a heating curve? (increasing line)

A

q = mCs delta T

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8
Q

The temperature beyond which a gas cannot be compressed/ the highest temperature a liquid can exist as a liquid

A

Critical Temperature

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9
Q

Critical temperature—–with increasing intermolecular forces

A

increases

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10
Q

the pressure required to liquify a substance at critical T

A

Critical Pressure

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11
Q

occurs when critical T and P are surpassed and liquid and gas phases are indistinguishable from each other

A

Supercritical fluid

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12
Q

the pressure exerted by a vapor on the surface of a liquid during dynamic equilibrium,

A

Vapor Pressure

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13
Q

when two opposing processes are occurring simultaneously

A

dynamic equilibrium

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14
Q

True or false the relationship between vapor pressure and temperature is linear?

A

False, they do generally increase as the other increases but it is not linear

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15
Q

liquids that easily evaporate with high vapor pressures and low intermolecular forces

A

Volatile liquids

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16
Q

When the vapor pressure of a substance = the external pressures acting on the surface of the liquid where thermal E is enough to break intermolecular forces and create a gas

A

Boiling point

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17
Q

does boiling point increase or decrease at higher pressures?

A

Increases at higher pressures

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18
Q

the boiling point of a substance at 1 atm

A

normal boiling point

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19
Q

where all states of matter exist in equilibrium

A

triple point

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20
Q

solids with a ‘sea’ of delocalized valence electrons that conduct heat and electricity well

A

metallic solids

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21
Q

solids held together by cation and anion attractions, don’t conduct electricity well and are brittle

A

ionic solids

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22
Q

solids held together by a network of covalent bonds

A

covalent-network solids

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23
Q

individual molecules held together by weak intermolecular forces, soft with low melting points

A

molecular solids

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24
Q

chains of carbon bonded to adjacent chains held together by intermolecular forces, more flexible than other solids

A

polymers

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25
Q

solids where the dimensions have been reduced to 1-100 nm with unique properties

A

nanomaterials

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26
Q

solids with atoms in an arranged and orderly repeating pattern

A

crystalline solids

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27
Q

solids with random and cluttered atom arrangments

A

amorphous solids

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28
Q

a small repeating unit in a crystalline solid

A

unit cell

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29
Q

how is the structure of a crystalline solid defined?

A

by the shape and size of its unit cell
AND
by the arrangement of atoms in the unit cell

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30
Q

the blue print to fill in the unit cell, the arrangement of points that the unit cell will fill

A

crystal lattice

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31
Q

what are the five types of two-dimensional lattices

A

square lattice
rhombic lattice
hexagonal lattice
oblique lattice (most common)
rectagonal lattice

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32
Q

lattice cube with lattice points only at the points of a cube

A

primitive lattice cube

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33
Q

lattice cube with lattice points at the corners and one at the center of a cube

A

body-centered lattice cube

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34
Q

lattice cube with lattice points at the corners, center and on each face of a six-sided cube

A

face centred lattice cube

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35
Q

the arrangement of atoms on the lattice points in a unit cell

A

motif

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36
Q

material that contain more than one element and have properties of metals

A

alloy

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37
Q

a second element of similar size replaces a metal atom

A

substitutional alloy

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38
Q

a second atom of smaller size replaces a metal atom

A

interstitial alloy

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39
Q

compounds/ alloys with a specific order

A

intermetallic compound/ alloy

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40
Q

properties that depend on the amount of substance present

A

extensive properties

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41
Q

properties that are independent of the amount of substance present

A

intensive properties

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42
Q

M (mega)

A

10^6

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43
Q

k (kilo)

A

10^3

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44
Q

c (centi)

A

10^-2

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45
Q

m (mili)

A

10^-3

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46
Q

micro (little u thing)

A

10^-6

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47
Q

n (nano)

A

10^-9

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48
Q

p (pico)

A

10^-12

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49
Q

suffix for 4

A

tetra-

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50
Q

suffix for 5

A

penta-

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51
Q

suffix for 6

A

hexa-

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52
Q

suffix for 7

A

hepta-

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53
Q

if you are given the masses of two isotopes how do you find the abundance?

A

(atomic mass of element- istope mass 1)/ isotope mass 2 - isotope mass 1

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54
Q

if two isotopes are XYS 231 and XYS 233 and the original elements mass is 234 which is more abundant?

A

isotope 233 is more abundant because it is closer to the atomic mass of XYS

55
Q

E of a photon =

A

hc/ wavelength

56
Q

h=

A

6.62610^-34 Js

57
Q

c= speed of light

A

2.99*10^8 m/s

58
Q

how does effective nuclear charge change from left to right across the periodic table?

A

it increases as atoms become smaller

59
Q

how does ionization energy change across the periodic table from left to right?

A

it increases across the periodic table and decreases top to bottom

60
Q

the energy required to remove an electron from an atom

A

ionization energy

61
Q

is moving up on an energy emission and absorption graph an emission or absorption?

A

absorbtion (ex: 1-3 or 2-4)

62
Q

what is an allowed number for the quantum number l?

A

n-1 to 0

63
Q

what is an allowed quantum number for the quantum number m

A

-l to +l

64
Q

what are the allowed numbers for the magnetic spin quantum number?

A

+1/2 and -1/2

65
Q

the net charge experienced by an electron in a many-electron atom

A

effective nuclear charge

66
Q

are anions smaller or bigger than their neutral atom?

A

bigger, they have more electrons

67
Q

what is the Rydberg constant?

A

RH = 1.096776*10^7 m

68
Q

what is the rydberg equation?

A

1/ wavelength = RH (1/ n^2 2 - 1/n^2 1)

69
Q

how many s orbitals are there?

A

1

70
Q

how many p orbitals are there?

A

3

71
Q

how many d orbitals are there?

A

5

72
Q

how many f orbitals are there?

A

7

73
Q

lowest energy orbitals are filled first in an electron configuration

A

aufbau principle

74
Q

electron orbitals must all have at least one electron before pairing can begin

A

Hunds rule

75
Q

no more than 2 electrons (with opposite spins) can occupy the same orbital

A

pauli exclusion principle

76
Q

why are metals so closely packed together?

A

because of the sea of delocalized electrons that are shared by the metal cations, metals don’t have enough valence e for localized bonds

77
Q

how does the MO theory explain the trend in decreasing boiling/melting points after the 6th metal in transition metals?

A

Antibonding MOs decrease bond strength and bonding MOs increase bond strength. Initially in the transition metals bonding orbitals are filled but as antibonding orbitals are filled the bond strength decreases and decrease the melting/boiling point

78
Q

why are electron bands formed?

A

as link/chains of atoms increase the MOs grow closer together to form stacks of antibonding and bonding bands

79
Q

forms from bonding MOs

A

valence bands

80
Q

forms from antibonding MOs

A

conduction bands

81
Q

what is the most favorable/ stable arrangement of ionic solids?

A

those where cation-cation and anion-anion distance are maximized to reduce repulsion

82
Q

of cations/# of anions =

A

coordination of anion/coordination of cation

83
Q

are covalent network solids stronger or weaker than molecular solids?

A

stronger, covalent bonds are stronger than intermolecular forces

84
Q

non-metallic solids that can conduct well but not as well as metals

A

semi-conductors

85
Q

semiconductors with one type of atom (group 4A)

A

elemental semiconductors

86
Q

semiconductors with more than one type of atom

A

compound semiconductors

87
Q

the process of adding impurity atoms to semi conductors to affect conductivity

A

semiconductor dopping

88
Q

N-type semi conductors

A

negative, more electrons added

89
Q

p-type semi conductors

A

positive, less electrons (less electrons leaves holes in the valence bands)

90
Q

how do you name an ionic compound?

A

you keep the name of the cation and change the ending of the anion to ide

91
Q

how do you name a covalent compound?

A

use the prefixes unless the first atom has only one of it (never add mono- to the beginning) also change the ending of the second atom to -ide

92
Q

how do you name a binary acid (H+ one other atom)

A

add hydro to the beginning and ic to the end of the non-metal

93
Q

how do you name oxyacids? (with oxygen)

A

-ate endings change to -ic and -ite endings change to -ous + the word acid at the end

94
Q

chains of monomers together with a very high molecular weight

A

polymers

95
Q

soft, can be reshaped and typically can be recycled, no cross-links

A

thermoplastics

96
Q

formed by irreversible chemical processes so they typically cannot be reshaped, cross-links make them stronger

A

thermosets

97
Q

rubbery solids that re take their shape after being bent/folded

A

elastomers

98
Q

a kind of polymerization where multiple bonds are broken/ opened for monomers to join together

A

addition polymerization

99
Q

a kind of polymerization where monomers are joined by the removal of a smaller atom between them, usually H + OH-

A

condensation polymerization

100
Q

are polymers usually crystalline or amorphous? and why?

A

they are usually amorphous because they are made of monomers of different weights

101
Q

the degree of structure in a solid

A

crystallinity

102
Q

if a polymer is more dense will it have a high or low crystallinity?

A

it will have a high crystallinity (more dense = more regularity)

103
Q

materials where their dimensions have shrunk to 10-100nm

A

nanomaterials

104
Q

what makes metals more reactive when they are on the nanoscale?

A

the sea of electrons present in a metal meets the confines of the material as it has shrunk, or in other words it meets a “shore”

105
Q

Explain the trends in bonding atomic radii across and down the periodic table

A

Bonding atomic radii decreases from left to right across the table and increases down the periodic table

it increases down the periodic table because quntum number decides size

106
Q

what is lattice energy?

A

lattice energy is the energy required to turn one mol of a substance into a gas

107
Q

the ability for an atom to attract eletrons to itself

A

electronegativity

108
Q

what are the trends for electronegativity?

A

Increases (negatively) across the table

109
Q

the greater the difference in electronegativity the more — the bond is

A

polar

110
Q

the greater the difference in electronegativity the more — the bond is

A

polar

111
Q

energy is — when bonds are formed

A

released

112
Q

energy is — when bonds are broken

A

used

113
Q

q + w=

A

Change in internal energy

114
Q

system absorbs heat from the surroundings

A

endothermic (feels cold)

115
Q

system releases heat to the surroundings

A

exothermic (feels hot)

116
Q

a property whose value does not depend on the path taken to reach that specific value

A

state funcion

117
Q

H =

A

E + P*V

118
Q

how do you calculate work?

A

w = -p *change in volume

119
Q

formula for ammonia

A

NH4 +

120
Q

hypochlorite

A

ClO -

121
Q

chlorite

A

ClO2 -

122
Q

chlorate

A

ClO 3 -

123
Q

perchlorate

A

ClO4 -

124
Q

nitrite

A

NO2 -

125
Q

nitrate

A

NO3 -

126
Q

nitrate

A

NO3 -

127
Q

sulfate

A

SO4 2-

128
Q

Sulfite

A

SO 3 2-

129
Q

phosphate

A

PO4 3-

130
Q

what are the diatomics?

A

H2 N2 F2 O2 I2 Cl2 Br2

131
Q

what elements + compounds are always soluble?

A

Li +, K+, Na+, NH4 +, NO3 -

132
Q

what are Cl- , Br - and I- insoluble with?

A

Ag 2+, Hg2 2+, Pb2+

133
Q

what makes sulfate insoluble?

A

Ag, Pb, Ca, Sr, Ba

134
Q

what must hydrogen be bonded to to induce hydrogen forces?

A

O, N or F

CHM 141 + 144 (2 decks)

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