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A) Chemistry > States Of Matter > Flashcards

States Of Matter Flashcards

0
Q

MmHg

A

Unit of measure for pressure based on barometer readings

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1
Q

Pressure

A

The distribution of a force across a designated area

P=Fn/A

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2
Q

Torr

A

Unit of pressure equal to 1mmHg

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3
Q

Pascal (Pa)

A

Unit of pressure

Pa= 1 N/m^2

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4
Q

atm

A 
Unit of pressure measure based on sea level
Generally accepted
=101,325 Pa
=29.92 mmHg
=14.7 psi
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5
Q

Manometer

A

Laboratory equipment used to measure pressure

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6
Q

Simple gas laws

A

1) boyles law
2) charles law
3) avogadros law

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7
Q

Boyles law

A

V1P1=V2P2

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8
Q

Charles’ law

A

V1/T1=V2/T2

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9
Q

Avagodro’s law

A

V1/n1=V2/n2

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10
Q

Ideal gas law

A

PV=nR*T

R=0.08206

atm, L, mol, K

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11
Q

Ideal Gas Constant

A

R=0.08206

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12
Q

Molar Volume

A

Volume occupied by one mole of a substance

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13
Q

Standard temperature

A

0 C = 273 K

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14
Q

Standard pressure

A

1 atm

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15
Q

Gas density

A

Density = (molar mass)/(molar volue)

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16
Q

Partial pressure

A

Presure exerted by an individual gas in a mixture

Pn=nn (RT/V)

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17
Q

Daltons law

A

The sum of all partial pressures is equal to the total pressure

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18
Q

Kinetic molecular theory

A

Gas is represented by a series of tiny particles

1) the size of a particle is negligably small
2) the kinetic energy of each particle is proportional to the temperature in Kelvins
3) The collision of one particle with another results in an exchange of energy

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19
Q

Work on the Kinetic molecular theory with the gas law

A

226

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20
Q

Avagadros number

A

NA= 6.022x10^-23

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21
Q

Mole

A

Avagodros number of atoms (or molecules) of a given substance

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22
Q

Kinetic energy of a given particle

A

KE=1/2 (m*v^2)

Lighter particles carry more kinetic energy

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23
Q

Average kinetic energy

A

KE=(3/2)RT

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24
Q

Mean free path

A

The average distance a particle travels between collisions

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25
Q

Diffusion

A

The process by which gas molecules spread out in response to a concentration gredient

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26
Q

Effusion

A

Process by which gas escapes from a container into a vacuum through a small hole

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27
Q

Graham’s law of effusion

A

Describes the relationship between effusion rates

RateA/RateB = sqrt(molar massB/molar massA)

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28
Q

Gas law correction for volume

A

V=nRT/P+ nb

b is a constant represented by individual gasses

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29
Q

Gas law correction for pressure

A

P=nRT/V- a(n/V)^2

a is a constant represented by individual gasses

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30
Q

Vanderwals equation

A

[P+a(n/V)^2]x[V-nb]=nRT

Product of Corrected gas volume and corrected Volume equals the rest of the ideal gas law

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31
Q

Pressure-Volume relationship to atom count

A

PV=NkT

N=number of atoms
k=boltzman constant=1.38x10^-23

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32
Q

Boltzman constant

A

1.38x10^-23

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33
Q

Liquid

A

Definite volume

Assumes the shape of a container

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34
Q

Solid

A 
Definite Volume
Definite Shape
High density
Particles packed closely together
Low kinetic energy
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35
Q

Gas

A 
No definite volume,
No definite shape
Low density
Maximum space between particles
High kinetic energy
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36
Q

Melting

A

Physical change from solid to liquid

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37
Q

Evaporation

A

Physical change from liquid to gas

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38
Q

Sublimation

A

Physical change from solid directly to gas

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39
Q

Condensation

A

Physical change from gas to liquid

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40
Q

Freezing

A

Physical change from liquid to solid

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41
Q

Deposition

A

Physical change from gas to solid

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42
Q

Intermolecular forces

A

Forces that hold condensed (non-gaseous) states together

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43
Q

Dispersion force

A

Result of fluctuations in the electron distribution within molecules and atoms

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44
Q

Dipole-dipole forces

A

In polar molecules, forces that keep maintain the molecular geometry of a molecule

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45
Q

Miscilibility

A

The ability to mix without separating into separate states

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46
Q

Ion-dipole forces

A

Result of a polar compound mixing with an ionic compound

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47
Q

Surface tension

A

Energy required to increase the area of the liquid by a given unit

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48
Q

Viscocity

A

The resistance of a liquid to flow

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49
Q

Capillary action

A

The ability of a liquid o flow against gravity up a narrow tube

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50
Q

Volatile

A

A liquid’s ability to vaporize easily

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51
Q

Nonvolatile

A

Refers to liquids that do not vaporize easily

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52
Q

Phase Diagram

A

Pressure/temperature chart in which the phases are mapped out with the fusion curve, sublimation curve, and vaporization curve with the triple point where they all meet

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53
Q

Critical point

A

The point of maximum temperature and pressure at which substances become a superficial liquid, neither liquid nor gas

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54
Q

Sublimation curve

A

The line on the phase diagram lowest on the pressure/temperature chart
Higher pressure yeilds solid
Higher temperature yeilds gas

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55
Q

Fusion curve

A

The line that separates liquids from solids on the phase diagram
Runs up from the ‘triple point’
High temperature yields liquid
Low temperature yields a solid

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56
Q

Vaporization curve

A

The line on the phase diagram that seperates liquid from gas
Splits right from the triple point
High pressure yields liquid
High temperature yields gas

57
Q

Triple point

A

The point at which the temperature pressure ratio is at a delacate balance, where the smallest change in either variable could change the phase of the substance

58
Q

Crystalline structure

A

A solid in which atoms molecules or ions are arranged in patterns with long range repeating order

59
Q

Solution

A

A homogeneous mixture of two substances

60
Q

Solvent

A

Majority component in a solution

61
Q

Solute

A

Minority component of a solution

62
Q

Aqueous Solutions

A

A solution in which water is the solvent

63
Q

Solubilty

A

The amount of a substance that will dissolve in a given amount of solvent

64
Q

Natures mixing tendency

A

The resulting solution will be the lowest energy level possible

65
Q

Entropy

A

A measure of energy dispersal within a system

66
Q

Properties of the ideal gas

A

Molar Volume 22.41L at STP
No adjustment for VP=nRT
(V/nRT)=1

67
Q

Miscible substances

A

Substances that are soluble in one another

68
Q

Exothermic

A

Heat is given off, feels hot

69
Q

Endothermic

A

Absorbs thermal energy, feels cold

70
Q

Solution prosses

A

1) Solute is broken into constituent particles (endothermic)
2) The solvent particles separate to make room for the solute particles (endothermic)
3) Solute are dispersed throughout solvent (exothermic)

71
Q

Enthalpy of solution

A

The sum of the enthalpies for each step in the solution process
ΔH=Δh-solute seperation+Δh-solvent seperation+Δh-mixture

72
Q

Heat of hydration

A

The sum of the heat of solvent separation (endothermic) and and the heat of the mixture (exothermic)

73
Q

Dynamic equilibrium

A

The point at which the rates of dissolution and recrystaization become equal

74
Q

Saturated solution

A

Solution in which the amount of dissolvable solute has already been reached,
If any more solute is added, it will not dissolve

75
Q

Nonsaturated solution

A

A solution that could still dissolve more solute

76
Q

Supersaturated solution

A

Solution containing more solute than could be disolved in that solvent

77
Q

Recrystalization

A

A purification technique by which a solid is added to water to create a saturated solution at a high temperature, as the solution cools, it becomes over saturated and produces crystals of the dissolved solid

78
Q

Factors in solubility

A

1) Volume
2) Temperature
3) Pressure

79
Q

Henrys law

A

Solubility of a gas (units of M) is equal to the product of henrys law constant (k sub-h, individual to each gas) and the partial pressure of that particular gas

S=k*P

80
Q

Dilute solution

A

Solution containing some small quality of solute relative to the amount of solvent

81
Q

Concentrated Solution

A

A solution containing a large quantity of solute, relative to the solvent

82
Q

Molarity (M)

A

(Moles of solute)/(volume of the solution in L)

83
Q

Molality (m)

A

(Moles of solute)/(mass of solvent in Kg)

84
Q

Percent by mass

A

Way of representing the saturation of a solution

(Solute mass)/(solution mass)x100%

85
Q

Parts per million (ppm)

A

(Mass solute/mass solution)x10^6

86
Q

Parts per billion (ppb)

A

(Mass solute/mass solution)x10^9

87
Q

Parts by volume

A

(Volume solute)/(volume solution)x(multiplication factor)

88
Q

Usage of parts by mass or volume

A

Find the mass or volume of the solution given the solute specifications (vice versa)

89
Q

Mole fraction

A

(Moles Solute)/(moles of solute and solvent added) x100%

90
Q

Colligative property

A

Any property that depends on the number of particles dissolved in a solution

91
Q

Raoult’s law

A

The vapor pressure of the entire solution is equal to the product of the mole fraction and the vapor pressure of the pure solvent

See page 571 for practice

92
Q

Ideal solution

A

When both the solute and solvent are volitile, contributing to the vapor pressure of the overall solution

93
Q

Freezing point depression

A

lowering the freezing point of a solution,
Colligative property

ΔTf=m*Kf
m-molality
Kf freezing point depression constant for the solvent

94
Q

Boiling point elevation

A

Ease of Raising the boiling point of a solution,

Colligative property

95
Q

Osmosis

A

The flow of a solvent from a solution of lower solute concentration

96
Q

Semipermeable membrane

A

A material that effectively filters some substances but not others

97
Q

Osmotic pressure

A

Equal to molarity times the gas constant times solution temperature

MRT

98
Q

Van’t Hoff factor

A

i=(moles of particles in solution)/(moles of formula units dissolved)

99
Q

Colloids

A

A substance in which fine particles (between 1nm 1000nm in size) are evenly dispersed,
ie Milk

100
Q

Micelles

A

Non-polar hydrocarbon trails crowd into the center of a shape to maximize their interactions with one another

101
Q

Tyndall effect

A

The scattering of light by colloidal dispersion

102
Q

Moles present

A

(mass present)/(substance molar-mass)

103
Q

Aqueous solution

A

A solution in which water acts as the solvent

104
Q

Dilution equation

105
Q

Electrolytes

A

Solutes that dissolve into ions that conduct electricity

106
Q

Strong electrolytes

A

Electrolytes that dissolve completely in water

107
Q

Non-electrolytes

A

Solutes whose ions do not conduct electricity

108
Q

Strong acid

A

An acid that completely ionizes in water

109
Q

Weak acids

A

An acid that does not completely ionize in water

110
Q

Weak Electrolytes

A

Electrolytes that that do not dissolve completely in water

111
Q

Solubility rules

A

1) Group1 and Amonia cations
2) Nitrates and acetates
3) Chlorides, Bromides, Iodines (Ag1, Hg2, Pb2)
4) Sulfate (Sr2, Ba2, Pb2, Ag1, Ca2)
5) But not hydroxide or sulfide (Unless rule 1 applies, Ca2, Sr2, or Ba2)
6) But not carbonates or phosphates (unless rule 1)

112
Q

Precipitation reactions

A

When a solid (precipitate) is formed by the mixing of two solutions

113
Q

Precipitate

A

Solid formed by mixing two solutions

114
Q

Acid solutions

A

Acids release H+ ions in the presence of water

115
Q

Basic Solutions

A

Bases release OH- in the presence of water

116
Q

Hydronium ions

A

H+(aq) ions released by an acid in water

117
Q

Titration

A

Substance in a solution of a known concentration is reacted with another substance in a solution of unknown concentration

118
Q

Equivilence point

A

In an acid base reaction, the Point at which moles of OH- equal moles of H+

119
Q

Indicator

A

A dye used that changes color based on acidic exposure, used to indicate equivalence point of a solution

120
Q

Structural Isomers

A

Atoms are connected to one another in a variety of ways

121
Q

Stereoisomers

A

Atoms are connected in the same way, with a variety of specially arrangements about the metal atom

122
Q

Coordination isomers

A

Occurance of a coordinated ligand exchanging places with an uncoordinated counterion

123
Q

Linkage isomers

A

Stereoisomers that have ligands that coordinate to the metal in different geometric orientations.

124
Q

Geometric isomers

A

A type of stereoisomerism that results from ligands bonding to metal in a variety of spacial arrangements

125
Q

Hydroscopy

A

The ability of a substance to pull moisture from the surrounding environment

126
Q

Crystallgraphic deffect

A

Interruptions in the regular pattern of fixed repeating order solids (crystals)

127
Q

Microcrystaline

A

A solid that contains crystals visible only through microscopic examination

128
Q

Cubic crystal system

A

A crystal system in which the unit cell is in the shape of a cube
Toms are arranged in cubic order

129
Q

Crystal family (lattice system)

A

Several classes of crystaline structures that have similar symmetries

130
Q

Is it polar (from the chemical formula)

A

Determine the molecular geometry

Is it has lone pair electrons, it is polar

131
Q

Cone shaped bond in complex molecules

A

Look it up

132
Q

Dashed bond in complex molecules

A

Look it up

133
Q

Complex molecular orbit calculations

134
Q

Disiccant

A

Hygroscopic material that induces dryness in surroundings

135
Q

Brauner-Emmet-Teller (BET) theory

A

Solids are capable of absorbing gas particles at their surface

136
Q

Langmuer Equation

A

Reated the quantity of gas molecules absorbed by the surface of a solid to the gas pressure

137
Q

Calculating Ph value from hydrogen ion activity

A

Ph=log(1/[H+])

Where h+ refers to the hydrogen ion activity of a solution

138
Q

Supercritical drying

A

Transitioning a material from a liquid to a gas by raising the temperature and pressure beyond the supercritical point, and then lowing the pressure until the substance become a gas

139
Q

Surface energy

A

The quantitive measurement of the bonds disrupted by the formation of a surface

140
Q

Excimer

A

‘Excited dimer’

A short-lived molecule, formed from two species, with a filled vallance shell (noble gas)

A) Chemistry (9 decks)

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