the boring states of matter ch11. kinetic energy e k the energy an object has because of its motion....
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The Boring States of Matter CH11
Kinetic Energy EK
The energy an object has because of its motion.
Temperature is a measurement of average kinetic energy.
Kinetic Theory-
Tiny particles in all forms of matter are in constant motion.
Liquids vs. Gases
Liquids, the molecules are moving and touching.
They interact
They take up less space than gasses
They overall have less Ek
than a gas of the same substance
Gases, the molecules bounce off each other, but do not stay in contact
There is very little interaction between molecules
They take up a lot of space
Which of these 2 parts are compressible?
Can you “squish” the gas?
Can you “squish” the liquid?
gas
liquid
Evaporation: conversion of a liquid to a gas
At the surface, there are a few molecules that have enough Ek to escape to gas.
By increasing the temperature, more molecules will have the necessary Ek and evaporation will occur faster than before.
The vapor pressure increases with more heat/ Ek
Average kinetic energy
Temperature is a measurement of average kinetic energy.
If a beaker of water reads 20°C, do all molecules in the beaker have kinetic energy = 20⁰C? There is a broad range of kinetic
energies. Most of the molecules are “around 20C”, but there are some
significantly less energetic, and some significantly more energetic.
Solids Molecules in
solids only vibrate in place, they do not slide past each other
They interact in their FIXED position
More dense than gas, and most liquids
Salt crystal, atoms are in a set position
Heating a solid
The vibrations increase
If they vibrate enough, some of the bonds holding the solid together will break.
This is called the melting point.
S L melting
L S freezing
L G vaporization (or evaporation)
G L condensation
Evaporation vs. Boiling point Atm is pressing down on the surface
Solid to a Gas?…Sublimation
Solids also have a vapor pressure.
When vapor pressure is high enough, the solid will go to gas, without stopping at liquid.
This is called sublimation.
Gas to a solid – DEPOSITION
Dry ice, is a classic example of sublimation
Phase Transition names
SL
LS
L G
GL
S G
GS d
Melting Freezing
Vaporization Condensation
Sublimation deposition
Give the change of state for each term
Ionic Solids
Strong forces between oppositely charged ions.
HIGH melting points HIGH boiling points Non conductors as
solids, conductors while molten.
Often water soluble Depends upon attractive
forces for each other and other molecules.
Molecular Combination of 2 or more non metals
Molecular substances have 3 important types of weak intermolecular forces
1. Dispersion Forces
2. Dipole Forces
3. Hydrogen bonds
Inter-molecular (between molecule) forces are weak.
Therefore easy to separate:
Have low melting and boiling points Think Oxygen and Water They’re gases and liquids
at room temperature Non-Conductors of
electricity
Dispersion (London) Forces
Most common type of intermolecular force.
Caused by temporary induced- dipoles formed in adjacent molecules.
All molecules have dispersion forces, the strength depends on 2 factors: *The # of electrons in the
molecule
As molar mass increases, dispersion forces become stronger, the boiling pt of non-polar molecules increases.
Think of the electron cloud being agitated
F2 -188
Cl2 -34
Br2 59
I2 184
Dipole Forces
Electrically attractive forces between + and – end of adjacent polar molecules.
Boiling points of N2 -196C O2 -183C
NO -151C
The Nitrogen Monoxide is slightly polar and therefore has weak dipole forces. This explains the relatively higher melting points.
Hydrogen Bonding
Unusually strong DIPOLE forces.
This is due to the very small Hydrogen atom’s
Electronegativity difference with:
F fluorine
O oxygen
N nitrogen
The strongest of the ‘weak forces’
Water H2O bp = 100 C, H2S -61C
Putting it all togetherHow can you know if a substance will melt, or sublimate?
The transitions depend upon both pressure and temperature.
At a given Temperature T: At a low pressure, something might sublimate, at a
higher pressure it would likely melt
Phase diagram
solid
liquid
gas
Pressure
temperature
Triple point, all 3 phases exist simultaneously
Phase Diagram for Water
Triple point
.006 atm
.001C
4th state of matter: Plasma
Plasma
Occurs at super hot temperatures
Gas atoms are stripped of their electrons
Mix of loose electrons, and + gas ions is
called PLASMA
Hot plasmas make up the stars, and can be 10 million degrees
Not very relevant to HS Chemistry.
Maxwell-Boltzman Distrubution
At high T
More molecules are in a higher energy state