Download Matter and Energy

Breaking it down and reviewing old material.
 SWBAT
identify the basic building
blocks of nature, describe the
common states of matter, discuss
atomic properties and nuclear
changes, as well as discern
between different societal use of
energy and matter.






Matter – anything that occupies space and
has mass.
Matter can be found in the form of elements
(distinctive building blocks) and compounds
(two or more elements bonded together).
Various elements, compounds, or both can be
found in mixtures.
Saltwater?
Silver bar?
Table salt?

Matter is found, essentially, in three states:
◦ Solid – atoms arranged in close proximity.
◦ Liquid – atoms arranged in a more dispersed
pattern.
◦ Gas – atoms widely spaced.


Atoms – the smallest component of an
element displaying all characteristics of that
element.
Sub-atomic particles –
◦ Protons – found in nucleus, + charge, 1 AMU
◦ Neutrons – found in nucleus, no charge, 1 AMU
◦ Electrons – found orbiting nucleus, - charge,
approximately 1/1836 AMU






Ions – charged atoms due to having gained or
lost electrons.
Why do ions form?
Examples of ions?
Isotopes – atoms with the same atomic
number but different atomic mass.
Why the difference in mass?
Examples of isotopes?




Ionic compounds are
compounds made up of
oppositely charged ions.
The classic example
would be table salt
(NaCl).
Covalent compounds
are formed from
uncharged atoms.
The classic example
would be water (H2O).


Based on carbon atoms bonded with one or
more other elements, such as: hydrogen,
oxygen, nitrogen, sulfur, phosphorus,
chlorine, and fluorine.
Types of organic molecules include:
◦
◦
◦
◦
Hydrocarbons – CH4, C8H18
Chlorinated hydrocarbons – DDT, PCBs
Chlorofluorocarbons – CFCs
Simple carbohydrates – C6H12O6


Composed of polymers of simple organic
molecules.
Examples include:
◦ Complex carbohydrates – formed from simple
carbohydrates
◦ Proteins – formed from amino acids
◦ Lipids – formed from excess carbohydrates
◦ Nucleic acids – formed from nucleotides
◦ Genes – composed of specific sequences of
nucleotides in a DNA molecule
◦ Chromosomes – combinations of genes


Basically, everything else.
Stuff like H2, CO2, O2, O3, NaCl, NaOH, N2,
N2O, NO, NH3, H2SO4



A measure of how useful a matter resource is,
based on availability and concentration.
High-Quality Matter is organized,
concentrated, usually found near the surface
of the Earth, and has great potential as a
matter resource.
Low-Quality Matter is disorganized, dilute,
usually found deep in the Earth or oceans,
and has little potential use as a resource.


The ability to do work (and transfer heat).
Forms of energy –
◦
◦
◦
◦
◦
◦
Light
Heat
Electricity
Chemical
Mechanical
Nuclear

Potential – stored and contingent on position.

Kinetic – contingent on mass and velocity.
◦ Height
◦ Chemical
◦ Nuclear forces
◦ Heat
◦ Temperature
◦ Electromagnetic Energy


Like Matter Quality, Energy Quality is
dependent on how useful it is to us.
High-Quality Energy –
◦ Gasoline
◦ Sunlight
◦ Uranium nuclei

Low-Quality Energy –
◦ Heat in the atmosphere or oceans
◦ Waste heat


Conservation of Matter – there is no “away”.
While we utilize resources and seem to
“consume” matter, we are really doing
nothing more than rearranging the atoms
involved.




1st Law – In all physical and chemical changes,
energy is neither created nor destroyed, but it
may be converted from one form to another.
2nd Law – When energy is converted from one
form to another, some of the useful energy is
always degraded to lower-quality, more
dispersed (higher entropy), less-useful energy.
Entropy is a measure of disorder. Therefore, it is
always increasing. “Entropy always wins.”
3rd Law – The entropy of a perfect crystal at
absolute zero is exactly equal to zero.
Zeroth Law – if two systems are both in thermal
equilibrium with a third, then they are in thermal
equilibrium with each other.



Physical – involves no change in chemical
composition. Examples include splitting wood,
mixing cake batter ingredients, and shaping
metal.
Chemical – involves a change to the chemical
composition of a substance. Examples include
burning wood, baking cake batter, and metal
rusting.
Nuclear – certain isotopes are so unstable they
are able to spontaneously rearrange themselves
and form new isotopes. These processes are
known as radioactive decay, fission, and fusion.




Radioactive decay occurs when unstable isotopes
rearrange their nuclei and release bursts of
energy in the form of high-energy particles that
are ionizing.
As they rearrange themselves, they become a
different, more stable isotope at a predictable
rate.
The amount of time it takes for 50% of a
substance to naturally degrade to a stable
isotope is expressed as its “half-life”.
Radioactive substances are deemed to be safe
after 10 half-life cycles.









Potassium-42 – 12.4 hours
Iodine-131 – 8 days
Cobalt-60 – 5.27 years
Tritium – 12.5 years
Strontium-90 – 28 years
Carbon-14 – 5,370 years
Plutonium-239 – 24,000 years
Uranium-235 – 710 million years
Uranium-238 – 4.5 billion years



Large, unstable isotope nuclei are struck by
neutrons and split into smaller nuclei.
When these nuclei split, energy and additional
neutrons are released.
A chain reaction will occur as long as
sufficient additional nuclei are present.



Two light elements, usually hydrogen
isotopes, are combined to form a larger atom.
D-T = 100 million Co
D-D = 1 billion Co



High-throughput (high-waste) societies
attempt to avoid the impact of the 2nd Law of
thermodynamics by utilizing increasing
amounts of energy and matter to sustain
themselves. Ultimately, they are
unsustainable.
Matter-recycling societies attempt to mitigate
their impact through recycling efforts. The
amount of energy becomes the limiting
factor.
Low-waste societies are sometimes referred
to as Earth-wisdom societies and attempt to
live in equilibrium with matter and energy
resources available.