CH1120 Liquids, Solids, and Intermolecular...
Transcript of CH1120 Liquids, Solids, and Intermolecular...
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CH1120
Liquids, Solids, and Intermolecular Forces
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The Three Phases of Matter(A Macroscopic Comparison)
State of Matter Shape and volume Compressibility Ability to Flow
Solid Retains its own shape and volume very low none
LiquidConforms to shape of container, but not
to volumelow moderate
GasConforms to shape
and volume of container
high high
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Particles packed close together and are fixed in position
(They may vibrate) Noncompressible
Retain shape and volume when placed in a new
container Do not flow
Particles closely packed Particles have some ability
to move around Noncompressible
Take the shape of their container
Flow, but don’t have enough freedom to escape or
expand
Particles have complete freedom of motion
There is a large amount of space between the
particles
Molecular View of Phases of Matter
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An important distinction !!
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Kinetic–Molecular Theory
Gases Kinetic energy overcomes attractions between particles.
Particles have complete freedom of motion.
Solids Kinetic energy cannot overcome attractive forces at all.
No translational or rotational motion. Particles may vibrate.
Liquids Kinetic energy can only partially overcome attractive forces. Particles have limited translational and rotational motion.
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Kinetic – Molecular Theory
What state a material is in depends largely on two major factors:
1. the amount of kinetic energy the particles possess 2. the strength of attraction between the particles
These two factors are in competition.
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Gas phase particles
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Attractive Forces
Particles are attracted to each other by electrostatic forces.
The strength of the attractive forces varies.
The strength of the attractive forces depends on the kind(s) of particles.
The stronger the attractive forces between the particles, the more they resist moving.
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Phase Changes
Gases can be condensed.
The amount of kinetic energy the particles have determines the state of matter.
Solids melt when heated.
Liquids boil when heated.
Liquids can be condensed.
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Special Properties of Liquids
Surface tension
Viscosity
Capillary Action
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Vaporization
Molecules in a liquid are constantly in motion; some molecules have more kinetic energy than
others.
If these high energy molecules are at the surface, they may have enough energy to
overcome the attractive forces
Therefore – the larger the surface area, the faster the rate of evaporation
This will allow them to escape the liquid and become a vapor.
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Condensation-The Opposite of Vaporization
Molecules of the vapor will lose energy through molecular collisions
Molecules get captured back into the liquid
Some may stick and gather together to form droplets of liquid
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Effect of Intermolecular Attraction on Evaporation and Condensation
Weaker attractive forces ➡ less energy needed to vaporize
Weaker attractive forces ➡ more energy will need to be removed from the vapor molecules before condensation
Weak attractive forces ➡ the faster the evaporation
Liquids that evaporate easily are said to be volatile.
Liquids that do not evaporate easily are called nonvolatile.
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Liquid FormulaNormal Boilng
Point(ºC)
Heat of Vaporization
(kJ/mol)
water H2O 100.0 40.7Isopropyl alcohol C3H8O3 82.3 39.9
acetone C3H6O 56.1 29.1
ethyl ether C4H10O 34.5 26.5
The amount of heat energy required to vaporize one mole of the liquid is called the heat of vaporization, ΔHvap, or the
enthalpy of vaporization.
Energetics of Vaporization
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1. Calculate the amount of heat needed to vaporize 90.0 g of C3H7OH at its boiling point (ΔHvap = 39.9 kJ/mol)
g mol kJ
39.9 kJ + C3H8O (liquid) C3H8O (gas)
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2. Calculate the mass of water that can be vaporized with 155 kJ of heat at 100 ° (ΔHvap = 40.7 kJ/mol)
kJ mol H2O g H2O
40.7 kJ + H2O (liquid) H2O (gas)
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What happens when you heat up a liquid ??
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Boiling As a liquid is heated, its temperature rises and the molecules move past each other more vigorously.
Once the temperature reaches the boiling point, the molecules have sufficient energy to overcome the attractions that hold them in contact with other
molecules and the liquid boils.
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ΔT
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Heating Curve of a Liquid
As you heat a liquid, its temperature increases linearly until it reaches the boiling point q = mass x Cs x ΔT
Once the temperature reaches the boiling point, all the added heat goes into boiling the liquid – the temperature stays constant
Once all the liquid has been turned into gas, the temperature can again start to rise. q = mass x Cs x ΔT
ΔT
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What happens when you heat up a solid ??
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Melting As a solid is heated, its temperature rises and the
molecules vibrate more vigorously.
Once the temperature reaches the melting point, the molecules have sufficient energy to overcome some of
the attractions that hold them in position and the solid melts.
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ΔT
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Heating Curve of a Solid
Once all the solid has been turned into liquid, the temperature can again start to rise. q = mass x Cs x ΔT
As you heat a solid, its temperature increases linearly until it reaches the melting pointq = mass x Cs x ΔT
Once the temperature reaches the melting point, all the added heat goes into melting the solid – the temperature stays constant ΔT
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Energetics of MeltingThe amount of heat energy required to melt one mole of the solid is
called the Heat of Fusion, ΔHfus or the enthalpy of fusion
Generally much less than ΔHvap
Liquid FormulaNormal
Melting Point(ºC)
Heat of Fusion(kJ/mol)
water H2O 0.0 6.02Isopropyl alcohol C3H8O3 -89.5 5.37
acetone C3H6O -94.8 5.69
ethyl ether C4H10O -116.3 7.27
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Quantitative Aspects of Phase Changes
Within a phase, a change in heat is accompanied by a change in temperature which is associated with a change in average kinetic energy of the molecules.
q = ( )(molar heat capacity)(∆T)quantity
ofmatter
J = g x x ºCJg ºC
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Quantitative Aspects of Phase Changes
During a phase change, a change in heat occurs at a constant temperature, which is associated with a change in average
rotational and translational energy of the molecules, as the average distance between molecules changes.
q = ( )(enthalpy of the phase change)quantity
ofmatter
kJ = mol x kJmol
No ΔT !!
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How much heat energy is required to raise the temperature of 1.0 mol of water
from -25ºC to 125ºC ??
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Heating Curve of Water
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Segment 1
Heating 1.00 mole of ice at −25.0 °C up to the melting point, 0.0 °C
q = mass x Cs x ΔTmass of 1.00 mole of ice = 18.0 g Cs = 2.09 J/g·°C
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Segment 2
Melting 1.00 mole of ice at the melting point, 0.0 °Cq = n·ΔHfus
n = 1.00 mole of ice ΔHfus = 6.02 kJ/mol
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Segment 3
Heating 1.00 mole of water at 0.0 °C up to the boiling point, 100.0 °C
q = mass x Cs x ΔTmass of 1.00 mole of water = 18.0 g Cs = 4.18 J/g·°C
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Segment 4
Boiling 1.00 mole of water at the boiling point, 100.0 °C
q = n·ΔHvapn = 1.00 mole of water ΔHvap = 40.7 kJ/mol
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Segment 5
Heating 1.00 mole of steam at 100.0 °C up to 125.0 °Cq = mass x Cs x ΔT
mass of 1.00 mole of water = 18.0 g Cs = 2.01 J/g·°C
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How much heat energy is required to raise the temperature of 1.0 mol of water
from -25ºC to 125ºC ??
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0.941 6.02 7.5240.7
0.904 56.085
56.1 kJ
12345
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Attractive Forces
Particles are attracted to each other by electrostatic forces
The strength of the attractive forces depends on the kind(s) of particles
The stronger the attractive forces between the particles, the more they resist moving
The strength of the attractions between particles of a substance determines its state.
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Kinds of Attractive Forces
Hydrogen Bonds between Molecules An especially strong dipole–dipole attraction resulting
from the attachment of H to an extremely electronegative atom
Dispersion Forces between Molecules Temporary polarity in molecules due to
unequal electron distribution
Dipole–Dipole Attractions between Molecules Permanent polarity in molecules due to their structure
Ion–Dipole Attractions - Not Intermolecular Between mixtures of ionic compounds and polar
compounds (esp. aqueous solutions)
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Some molecules are considered nonpolar because of the atoms which they contain and the
arrangement of these atoms in space.
CH4 BH3 C2H2 CO2
Nonpolarizedelectronclouds
But these molecules can all be “condensed.” !!
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Origin of Instantaneous Dipoles
δδ-δδ+
The δδ- charge repels electrons.
The δδ+ charge attracts electrons.
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Magnitude of the Induced DipoleThe magnitude of the induced dipole depends on several factors:
Polarizability of the electrons
Volume of the electron cloud
larger molar mass ⇒ more electrons ⇒ larger electron cloud ⇒ increased polarizability ⇒ stronger attractions
Larger molecules have more
electrons, leading to increased
polarizability.
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Gas Radius Molar Mass B.P.(K)
He 31 4 4.2
Ne 38 20 27
Ar 71 40 87
Kr 88 84 120
Xe 108 131 165
Rn 120 222 211
Effect of Molecular Sizeon Magnitude of Dispersion Force
As the molar mass increases, the number of
electrons increases. Therefore, the strength of
the dispersion forces increases.
The stronger the attractive forces
between the molecules, the
higher the boiling point.
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Boiling Points of Straight Chain Alkanes NonPolar Molecules
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Size of the Induced DipoleShape of the molecule
more surface-to-surface contact ⇒ larger induced dipole
⇒ stronger attraction
Molecules that are flat have more surface
interaction than spherical ones.
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Effect of Molecular Shapeon Size of Dispersion Force
n-pentane molar mass=72.15
b.p = 36.1 ºC
2-methylbutane molar mass=72.15
b.p = 27.9 ºC
2,2-dimethylpropane molar mass=72.15
b.p = 9.5 ºC
A larger surface-to-surface contact between molecules results in stronger dispersion force attractions and a
higher boiling point.
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Kinds of Attractive Forces
Hydrogen Bonds between Molecules An especially strong dipole–dipole attraction resulting
from the attachment of H to an extremely electronegative atom
Dispersion Forces between Molecules Temporary polarity in molecules due to
unequal electron distribution
Dipole–Dipole Attractions between Molecules Permanent polarity in molecules due to their structure
Ion–Dipole Attractions - Not Intermolecular Between mixtures of ionic compounds and polar
compounds (esp. aqueous solutions)
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Some molecules are inherently polar because of the atoms which they contain and the
arrangement of these atoms in space.
H2O NH3 CH2O HCl
δ− δ+ A crude representation of a polar molecule
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Dipole–Dipole Attractions
Polar molecules have a permanent dipole because of bond polarity and shape
1) dipole moment 2) as well as the always present induced dipole
The permanent dipole adds to the attractive forces between the molecules
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Name Formula Molar mass Structure Structure b.p. m.p.
formaldehyde CH2O 30.03 -19.5º -92º
ethane C2H6 30.07 -88º -172º
HH
H
H
HH
C
C
Effect of Dipole–Dipole Attraction on Boiling and Melting Points
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Hydrogen Bonding
When a very electronegative atom is bonded to hydrogen, it strongly pulls the bonding electrons toward it:
O─H, N─H, F─H
Because hydrogen has no other electrons, when its electron is pulled away, the nucleus becomes deshielded,
exposing the H proton.
The exposed proton acts as a very strong center of positive charge.
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Name Formula Molar mass Structure Structure b.p. m.p.
ethanol C2H6O 46.07 78.2º -114.1º
dimethyl ether C2H6O 46.07 -22º -138.5º
Effect of Hydrogen-Bonding on Boiling and Melting Points
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H-Bonds
Very strong intermolecular attractive forces
Stronger than dipole–dipole or dispersion forces
Substances that can hydrogen bond will have higher boiling points and melting points than similar
substances that cannot.
But hydrogen bonds are not nearly as strong as chemical bonds.
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One of these compounds is a liquid at room temperature (the others are gases). Which one and why?
MM = 30.03PolarNo H-Bonds
MM = 34.03PolarNo H-Bonds
MM = 34.02PolarH-Bonds
Because only hydrogen peroxide has the additional very strong H-bond additional attractions, its intermolecular attractions will be the strongest. We therefore expect hydrogen peroxide to be the liquid.
-19ºC -78ºC +150ºC b.p.
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All Molecules
Polar Molecules
Molecules containing O-H, N-H, or F-H
Bonds
Dispersion forces
Dipole forces
H-bonding
Hierarchy of Intermolecular Forces
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Comparison of Intermolecular Forces
H2, b.p. -253ºCweak attractions between molecules
HCl, b.p. -85ºCstrong attractions between
molecules
HF, b.p. +20 ºCvery strong attractions
between molecules
Dispersion forces:
Dipole-dipole forces:
Hydrogen bonding:
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0.05-40.0 kJ/mol
5-25 kJ/mol
10-40 kJ/mol
40-600 kJ/mol
Non-Bonding (Inter-Molecular) Forces
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Bonding Molecular Forces
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kJ/mol
Intermolecular Forces
Chemical Bonds
0 4000
Comparison of Strengths of Inter-Particle Forces
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Summary
Dispersion forces are the weakest of the intermolecular attractions. Present in all molecules and atoms Magnitude increases with molar mass
Dipole–dipole attractive forces - Polar molecules
Hydrogen bonds - the strongest of the intermolecular attractive forces
H directly bonded to either O , N, or F atoms
Ion–dipole attractions are present in mixtures of ionic compounds with polar molecules.
Ion–dipole attractions are especially important in aqueous solutions