NCVPS Physical Science Announcement Ideas
Modules 10-15: Chemistry
Mod 10 – Properties of Matter
Mon.– Reviewing States of Matter
Play this Matching Game at: http://www.neok12.com/quiz/STSMAT02
Tues– Changing States
http://www.youngstown.k12.oh.us/powpak/cgi-bin/wq_teacher_page.pl?id=youn_stp&wq=6
Wed– What is the 4th state of matter?
http://science.discovery.com/tv-shows/deconstructed/videos/deconstructed-plasmacutter.htm
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Thurs– Dr. Carlson’s Density Theatre
Click here to watch a video to find out how dense is Dr. Carlson?
http://web.ics.purdue.edu/~mjcarlso/ST/ST012_Density.m4v
Fri– Chemical Change Examples
Color Changes as in the case of autumn leaves indicate a chemical
change. Perhaps you have found a half-eaten
apple that turns brown. The reason is that a
chemical change has occurred when food spoils.
Another sign of a chemical change is the release
or gain of energy by an object. Many substances
absorb energy to undergo a chemical
change. Energy is absorbed during chemical
changes involved in cooking, like baking a cake.
Energy can be released during a chemical
change. Fireworks release energy in a form of light that you can see.
It only takes one experience with a rotten egg to learn that they
smell different that fresh eggs. When eggs and food spoil, they
undergo a chemical change. The change in odor is a clue to the
chemical change.
Learn more at: http://www.ric.edu/faculty/ptiskus/chemical/
Mod 11 – Atoms and the Periodic Table
Mon.– Principles of Modern Atomic Theory
Discovery Channel Video: http://dsc.discovery.com/tv-shows/othershows/videos/assignment-discovery-shorts-nuclear-basics.htm
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Tues– What are elements?
All matter is made up of elements which are fundamental substances which cannot be broken
down by chemical means. There are 92 elements that occur naturally. The elements hydrogen,
carbon, nitrogen and oxygen are the elements that make up most living organisms. Some other
elements found in living organisms are: magnesium, calcium, phosphorus, sodium, potassium.
By the late 1800's many elements had already been discovered. The scientist Dmitri
Mendeleev, a Russian chemist, proposed an arrangement of know elements based on their
atomic mass. The modern arrangement of the elements is known as the Periodic Table of
Elements and is arranged according to the atomic number of elements.
http://www.nyu.edu/pages/mathmol/textbook/atoms.html
Wed– All About Atoms at Jefferson Lab
http://education.jlab.org/atomtour/index.html
Thurs– Who Discovered What Game?
Scientific discoveries usually happen over decades of research by many people. The
modern atomic theory has been developing for well over a hundred years. Find out who
did what throughout history. http://www.neok12.com/quiz/ATOM0005
Fri– What does Bill Nye, the Science Guy have to say about Atoms
Find out at: http://teachertube.com/viewVideo.php?video_id=105573
Mod 12 – Chemical Bonding & Nomenclature
Mon. Most elements will gain or lose electrons to increase stability.
Learn about chemical bonds on Discovery Channel's "Assignment Discovery."
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Tues– Chemical compounds are formed by
the joining of two or more atoms.
A stable compound occurs when the total
energy of the combination has lower
energy than the separated atoms. The
bound state implies a net attractive force
between the atoms ... a chemical bond.
The two extreme cases of chemical bonds
are:
Covalent bond: bond in which one or more
pairs of electrons are shared by two atoms.
Ionic bond: bond in which one or more
electrons from one atom are removed and
attached to another atom, resulting in
positive and negative ions which attract
each other.
Wed– Still Confused? Try this Chemical Bonding Tutorial
http://bcs.whfreeman.com/thelifewire/content/chp02/02020.html
Thurs– HOW TO WRITE CHEMICAL FORMULAS
Use this flowchart to assist you in writing your chemical formulas.
http://www.woodrow.org/teachers/chemistry/links/chem1/writingformulas.html
Fri– Common Oxidation Numbers Chart
For basis chemistry think of this number as the charge of the atom.
http://www.lz95.net/mss/faculty/eschoo/PDF%20FILES%20SCIENCE/Science/Ch.%207
/Common%20Oxidation%20Numbers%20Chart.pdf
Mod 13 – Chemical Reactions
Mon. - Six Types of Chemical Reaction
http://misterguch.brinkster.net/6typesofchemicalrxn.html
Tues– Overview of Chemical Reactions video
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Wed– Don’t forget to use Chem4kids to learn and review
http://www.chem4kids.com/files/react_intro.html
Thurs– Symbols in Chemical Equations
http://www.harpercollege.edu/tm-ps/chm/100/dgodambe/thedisk/chemrxn/rxnintr2.htm
Fri– Balancing Chemical Equations: Review of the Rules
You may remember that the law of conservation of mass says that matter is neither
created nor destroyed during a chemical reaction. This means that all chemical
reactions must be balanced—the number of atoms, moles, and ultimately the total mass
must be conserved during a chemical process. Here are the rules to follow when
balancing equations:
1. Determine the correct formulas for all the reactants and products in the reaction.
2. Begin balancing with the most complicated-looking group. A polyatomic ion that
appears unchanged on both sides of the equation can be counted as a single
unit.
3. Save the elemental (single elements) reactant and products for last, especially if
it is hydrogen or oxygen. Keep your eye out for diatomic molecules such as
oxygen, hydrogen, and the halogens.
4. If you get stuck, double the most complicated-looking group and try again.
5. Finally, make sure that all coefficients are in the lowest-possible ratio.
6. Know when to quit! None of the reactions you will encounter will be that difficult.
If the coefficients are getting wild, double-check what you’ve done since you may
have a simple mistake.
When balancing reactions, keep your hands off the subscripts! Use only coefficients to
balance chemical equations. Now let’s try an example. When you solve it yourself,
make sure to follow the steps!
http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter6section1.rhtml
Mod 14 – Acids, Bases, & Solutions
Mon. - ChemTutor for Acids and Bases
http://www.chemtutor.com/acid.htm
Tues– ph Scale
Acids are substances with a pH of anything below 7 while bases are substances with a
pH of anything above 7, making them opposites in a sense. However, some
substances--such as distilled water--are neutral, which have a pH of exactly 7.
http://students.cis.uab.edu/ash13y/Acids%20and%20Bases.html
Wed– Overview of Acids/Bases video/interactive
http://player.discoveryeducation.com/views/hhView.cfm?guidAssetId=7b344c6b-0c934666-af58-7d118eb43d35
Thurs– Acid Rain and the pH Scale
The pH scale measures how acidic an object is. Objects that are not very acidic are
called basic. The scale has values ranging from zero (the most acidic) to 14 (the most
basic). As you can see from the pH scale above, pure water has a pH value of 7. This
value is considered neutral—neither acidic or basic. Normal, clean rain has a pH value
of between 5.0 and 5.5, which is slightly acidic. However, when rain combines with
sulfur dioxide or nitrogen oxides—produced from power plants and automobiles—the
rain becomes much more acidic. Typical acid rain has a pH value of 4.0. A decrease in
pH values from 5.0 to 4.0 means that the acidity is 10 times greater.
http://www.epa.gov/acidrain/education/site_students/phscale.html
Fri– Most Americans are Acid
What does the pH scale have to do with our bodies? Plant based foods, which are
mostly alkaline foods, are the principal ingredients that keep us healthy and work well
in this slow moving human digestive system. Diseases can flourish in an acid
environment. The human body is designed to be slightly alkaline instead of acid,
although the body is acid by function (breathing, digestion, dealing with acid foods and
drink). Some areas of the body have different pH values but the blood is the major
indicator that tells the overall wellness of our bodies.
http://www.choose-healthy-eating-for-life.com/pH-scale.html
Mod 15 – Nuclear Chemistry & Radiation
Mon.– Nuclear Basics
Discovery Channel Video: http://dsc.discovery.com/tv-shows/other-shows/videos/assignmentdiscovery-shorts-nuclear-basics.htm
Tues– Half-life example
In discussions of radioactivity, the half-life of an isotope refers to the time it takes for
one-half of the sample to decay. If we start with 100 g of a radioactive substance whose
half-life is 15 days, after 15 days 50 g of the substance will remain. After 30 days, 25 g
will remain, and after 45 days, 12.5 g remains, and so on.
Example
A radioactive substance has a half-life of 20 minutes. If we begin with a 500 g sample,
how much of the original sample remains after two hours?
Explanation
The easiest way to attack these questions is to start with the original amount of the
sample, then draw arrows representing each half-life. Two hours is 120 minutes, so
that’s six half-lives. At the end of the stated time period, 7.8 g remains.
500 g
250 g
125 g
62.5 g
31.25 g
15.625 g
7.8125 g
http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter4section3.rhtml
Mon.– Help with Nuclear equations
http://library.thinkquest.org/10429/low/nuclear/nuclear.htm
Nuclear Equations
Nuclear notations are used to represent the decay of one element into another. The
generic formula for a radioactive element is as follows:
Some examples of nuclear decay equations are:
http://library.thinkquest.org/10429/low/nucle
ar/nuclear.htm
Tues– Radioactive Decay
There are three types of natural radioactive decay. They are alpha emisson, beta
emission, and gamma emission.
Alpha emission results in releasing an alpha particle. An alpha particle has two
protons and two neutrons, so it has a positive charge. (Since it has two protons it is
a helium nucleus.) It is written in equations like this:
Beta emission is when a high speed electron (negative charge) leaves the nucleus.
Beta emission occurs in elements with more neutons than protons, so a neutron
splits into a proton and an electron. The proton stays in the nucleus and the
electron is emitted. Negative electrons are represented as follows:
Gamma Emission is when an excited nucleus gives off a ray in the gamma part of
the spectrum. A gamma ray has no mass and no charge. This often occurs in
radioactive elements because the other types of emission can result in an excited
nucleus. Gamma rays are represented with the following symbol.
http://library.thinkquest.org/10429/low/nuclear/nuclear.htm
Wed– Safe handling of radioactive material
Knowing about half-lives is important because it enables you to determine when a
sample of radioactive material is safe to handle. The rule is that a sample is safe when
its radioactivity has dropped below detection limits. And that occurs at 10 half-lives.
So, if radioactive iodine-131 (which has a half-life of 8 days) is injected into the body to
treat thyroid cancer, it’ll be “gone” in 10 half-lives, or 80 days.
This stuff is important to know when using radioactive isotopes as medical tracers,
which are taken into the body to allow doctors to trace a pathway or find a blockage, or
in cancer treatments. They need to be active long enough to treat the condition, but they
should also have a short enough half-life so that they don’t injure healthy cells and
organs.
http://www.dummies.com/how-to/content/nuclear-chemistry-halflives-and-radioactivedating.html
Thurs– Radiation Therapy for Cancer
Radiation therapy kills cancer cells by damaging their DNA (the molecules inside cells
that carry genetic information and pass it from one generation to the next). Radiation
therapy can either damage DNA directly or create charged particles (free radicals)
within the cells that can in turn damage the DNA. Cancer cells whose DNA is damaged
beyond repair stop dividing or die. When the damaged cells die, they are broken down
and eliminated by the body’s natural processes.
More questions answered at:
http://www.cancer.gov/cancertopics/factsheet/Therapy/radiation
Fri– How Nuclear Power Works
What happens inside a nuclear power plant to
bring such marvel and misery into being? Imagine
following a volt of electricity back through the wall
socket, all the way through miles of power lines to
the nuclear reactor that generated it. You'd
encounter the generator that produces the spark
and the turbine that turns it. Next, you'd find the
jet of steam that turns the turbine and finally the
radioactive uranium bundle that heats water into
steam. Welcome to the nuclear reactor core.
More info at: http://www.howstuffworks.com/nuclear-power.htm