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 (H 2 O).

 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 – CH 4, C 8 H 18 ◦ Chlorinated hydrocarbons – DDT, PCBs ◦ Chlorofluorocarbons – CFCs ◦ Simple carbohydrates – C 6 H 12 O 6

 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 H 2, CO 2, O 2, O 3, NaCl, NaOH, N 2, N 2 O, NO, NH 3, H 2 SO 4

 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. ◦ Height ◦ Chemical ◦ Nuclear forces  Kinetic – contingent on mass and velocity. ◦ 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.

 1 st Law – In all physical and chemical changes, energy is neither created nor destroyed, but it may be converted from one form to another.  2 nd 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.”  3 rd 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 C o  D-D = 1 billion C o

 High-throughput (high-waste) societies attempt to avoid the impact of the 2 nd 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.