Intro to Chemistry
Chapter 1 and Chapter 2
A Preview of Coming Attractions
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RIGOROUS
ONLY INTENDED FOR MATURE STUDENTS!
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Taking
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words
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Main part for Notes
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Main Part for Notes
化学
S Chemistry in Japanese
S Literally means “change study.”
S Chemistry is the study of matter: the
composition of matter and the changes
matter undergoes.
S Did you start taking notes yet?
Quimica
S Chemistry in Spanish
S From Google Translate…
S La química es el estudio de la materia:
la composición de la materia y la
materia sufre cambios.
5 Branches of Chem
S Organic
S Contains Carbon (C)
S Inorganic
S Contains anything on the Periodic Table BUT
not C.
S Biochemistry (chemistry inside living things)
S Analytical (like on CSI)
S Physical (lots of math, including calculus)
8 Big Ideas
S Pg 4&5 lists 8 Big Ideas which the chemistry book
is organized around.
S Read these 2 pages tonight. You do not have to
MEMORIZE the Big Ideas, but you should be
familiar with them.
S Right now, we are in Big Idea 1. Using the Table
of Contents in the book, see if you can figure out
what chapters go with each Big Idea.
Accidental Chem
S Pg 12&13 lists 4 “accidents” which ended up
making millions of dollars or more.
S Sticky Notes were invented because a chemist
accidentally made some glue which didn’t stick
very well. If you pulled on the paper, it would
peel right off.
S His work sat on the shelf for about 6 years until
and idea popped into his head about how to use
it.
The Ancient Greeks
~ 400 BC
S Aristotle suggested that everything was composed of 4
elements:
S Water, Air, Earth and Fire
S He later added a 5th element which he called “aether” which
the stars and the heavens were made from.
S Aristotle also said that “cold” was a substance he called
primum frigidum, and that “cold” came from water.
S People actually believed this up until the middle ages (1500s at
least).
S Click on the next slide to see three of these “ancient elements.”
Earth Wind & Fire
(http://www.earthwindandfire.com/bio.html)
Yes, I’m “old school.” But I love these guys. And, I even saw them
in concert once, back in the 80’s. OK, back to chemistry on the
NEXT slide…If you don’t have these guys on your iPod or phone,
get some. Tonight. Seriously.
Antoine Lavoisier
(http://www.answers.com/topic/antoine-lavoisier)
Father of Modern Chemistry
Demonstrated experimentally the principle later
renamed “The Law of Conservation of Mass” in
Chapter 2 and later in this power point.
Turned chemistry from a series of observations
into a science of careful measurement that it is
today.
Wrote the first Chemistry textbook, which his
wife Marie Anne translated from French into
English.
Beheaded on 5/2/1794 by guillotine during the
French Revolution at age of 50.
The Scientific Method
Same one you’ve been studying
since elementary school.
S Observation
S Use your senses to make observations and
suggest questions.
S Hypothesis
S A testable “educated guess.”
S Experiment
S Supports and proves your hypothesis (or doesn’t
support and disproves)
Isn’t there MORE?
S Analysis of Data
S Analyze data collected during the experiment.
S Conclusion
S What happened?
S Was your hypothesis supported or not (try NOT to
think of it as success vs failure)?
S How could you improve your experiment?
S How could you expand upon your original
experiment?
Scientific Theory
S Theory
S A detailed explanation explaining why an experiment
works the way it does.
S A theory can never be PROVEN completely true.
S A theory can always be disproved if new data doesn’t
support the theory.
S If that happens, theory needs to be revised or discarded.
Scientific Law
S Law
S A law is a statement of fact, usually concerning a
natural phenomenon. Laws are always true, but it
doesn’t explain how or why.
S Theories explain why. Laws just tell you what it
is.
S Law of Gravity
S Theory of Evolution
S Lets talk about an important law in Chapter 2:
Variables in
Experiments
S Independent
S Variable “I” change and it is graphed on “x” axis
S Dependent
S Variable which “Depends” on independent variable
S Tested during experiment and it is graphed on “y”
axis
S Control
S Variables you control so they do not change and mess up
your experiment & NEVER GRAPHED
The Law of
Conservation of Mass
S In any chemical reaction or physical change, matter can
neither be created nor destroyed (page 50)
S The amount of matter (mass) doesn’t change.
S However, the identity of the matter (what type of
substance it is) could change.
S mass of the reactancts = mass of the products
Problem Solving
S Plan before you even TOUCH your calculator.
S This should take most of the time you spend on a
problem.
S Calculate (in other words, work your plan)
S This should be the quickest step.
S Evaluate your answer (most people skip this
step).
S Does it make any sense?
Chapter 2. Big Idea =
Chem as a Central Science
S Back to matter…matter has mass and volume.
S Intensive property—depends on the type of matter.
S Extensive property—depends on the amount of matter.
S Matter can be broken down into substances and mixtures.
S Substances are pure.
S Elements (smallest part of an element is an atom)
S Compounds (smallest part of a compound is a molecule)
S Mixtures of substances. NOT bonded together.
S Mixtures are either homogeneous or heterogenous.
Physical Properties
S Matter has both physical and chemical
properties.
S Physical properties can be observed without
CHANGING the type of matter.
S When solid water (ice) melts it becomes liquid
water. A change of state is a physical change (Δ or
delta means change).
S Physical changes are NOT permanent and are
reversible.
Chemical Properties
S Chemical properties can be ONLY be
observed BY CHANGING the type of
matter.
S Chemical properties are permanent and not
reversible.
S When salt is dissolved in water, a solution is
formed. That is a physical change. The salt is
still salt and the water is still water. You can
separate them easily by evaporating the water.
Chemical Properties
S But when sodium oxide (Na2O) is dissolved in water it dissolves, but
then a chemical reaction occurs. That is a chemical change. Sodium
oxide reacts with water to form sodium hydroxide (NaOH). If you
evaporate the water, you will have solid NaOH not Na2O.
S Sodium oxide has different chemical properties compared to salt, and so
it reacts differently.
S We write the reaction as
Na2O + H2O  2 NaOH
S That’s your first chemical “sentence.” The reaction describes a chemical
change. You need to be able to identify a property or change as being
either chemical or physical for the test next week!
Why does one react and the other
doesn’t?
S Well, that’s chemistry. It’s not all that
complicated but the answer won’t make
much sense right now.
S We still have a lot to learn.
S But, by the end of the course (Jan or June)
it should make a lot more sense.
States of Matter
S Solid *
S Liquid *
S Gas *
S A vapor is a substance that is generally solid or liquid at room temperature,
but is in the gaseous state (like steam or water vapor).
S Plasma
S Only observed at extremely high temperatures (several thousand degrees)
S Bose-Einstein condensates and Fermionic condensates
S Only observed at extremely low temperatures (within a degree or less of
absolute zero).
Substances vs mixtures
S Carbon is a substance.
S Water is a substance.
S Air is a mixture of substances (O2, N2, CO2,
etc)
S It is a homogenous mixture.
S What is the 3rd most abundant component of
air?
S A salad is a heterogeneous mixture.
Substances vs mixtures?
S You try some
S Methane (natural gas)
S Coffee
S Copper
S Salt
S Dirt
S Sand
What are physical separation
techniques? Techniques for
separating mixtures.
S Evaporation—can separate DISSOLVED solids from
the liquid.
S Filtration—can separate UNDISSOLVED solids from
the liquid.
S Decanting—can separate a dense solid from the liquid
(because the solid is on the bottom and you can pour
off the liquid).
S Distillation—can separate a mixture of liquids by
boiling them and condensing the vapors (check out the
distillation apparatus at the bottom of pg 40).
A physical separation technique
sometimes tested on the SOL.
S Chromatography
S Can be used to
separate a mixture of
solids dissolved in a
liquid.
S Ink
S Natural dyes
Substances: Elements
S Elements are on the Periodic Table. 90 occur naturally (1-92
except for 43Tc and 61Pm). 118 elements exist (but 113 Uut,
115 Uup, 117 Uus, 118 Uuo have not been named yet).
S Elements 93 and higher are man made (most of them by Dr.
Glenn Seaborg and his team at U. California @ Berkeley)
S 119 (Uue) and 120 (Ubn) are currently being worked on but
have not been synthesized as of yet.
S http://www.youtube.com/watch?v=cma-AjOUplU
S Do any still “undiscovered” elements exist anywhere in the
Universe?
Substances: Compounds
S Compounds are pure substances too. There are
literally millions of chemical compounds. Some
common compounds are:
S
S
S
S
S
S
S
S
Salt (sodium chloride or NaCl)
Sugar (sucrose or C12H22O11)
Baking Soda (sodium bicarbonate or NaHCO3)
Sand (silicon dioxide or SiO2)
Rubbing Alcohol (isopropanol or C3H7OH)
Carbon dioxide (CO2)
Ammonia (NH3)
Methane (CH4)
Distinguishing between:
Elements, Compounds, and
Mixtures?
S How can you tell if it’s an element or a compound or
mixture?
S An element cannot be broken down into anything simpler.
S A compound can be separated into smaller elements.
S But, you must use a chemical reaction to break down a
compound, because the elements in a compound are bonded
together.
S A mixture can be separated using physical separation
techniques.
S Check out the cool flowchart at the bottom of page 44.
Ionic Compounds vs
Molecular Compounds
S There are 2 types of compounds
S Ionic compounds have ionic bonds and are
composed of positive and negative ions.
S Ions are formed when atoms lose or gain
electrons.
S Molecular compounds have covalent bonds.
S Electrons are shared between atoms. There are
no ions or charges.
S We will study this more in Chapter 9.
Chemical Reactions
S Reactants  Products
S You need to start with 1 or more reactants and
You will produce 1 or more products
S How many you need and how much you produce
is characteristic of the specific reaction.
S We will study 5 major types of reactions starting
in Chapter 11.
S Chemical reactions are PERMANENT and NOT
reversible.
That’s Chemistry…
S That’s really all chemistry is…
S Atoms either take electrons from other atoms or
S Atoms lose electrons to other atoms or
S Atoms share electrons with other atoms
S Bonds are broken during that process and new bonds
are formed.
S Chemistry is the interaction of my electrons with your
electrons to form a bond. Electrons are involved, not
the protons or neutrons.
Should you Memorize the
Periodic Table?
S No!
S But learn the names of the symbols from 1-36 (OMG, vocabulary!)
S Some names are derived from Latin (Na and Au) or Greek (Hg),
German (W) and even mythology (Th). Some are even named after
real people (Cm and Es and Sg among others) or real places (like Y or
Ga or Ge) or planets (U, Np, Pu…and don’t start with me about
Pluto not being a real planet!). Each element has a definite story!
S The Element Song:
http://www.privatehand.com/flash/elements.html
S We will study the Periodic Table in greater detail beginning in Unit 2.
S Period = horizontal rows. There are 7 periods.
S Groups = vertical columns (also called “families”). There are 18
groups.
Remember: STUDY HARD!!
20-30 minutes every night! Have you started yet?
You should plan on studying hours for EVERY
chemistry test.
But it doesn’t all have to be
done the night before.
Students who just study 10 minutes before a test
usually don’t pass my test. Just saying!
Homework
1,2,6 due tomorrow!!
1. Answer the 6 questions on pg 20&21 about safety.
2. Pg 28-30, #55, 60, 67, 73, 75
3. You are also responsible for any vocab you don’t
already know on pg 27. Spelling does count.
4. More vocab on pg 54. If you don’t know those
words, make sure you learn them before the test (or
maybe start putting some into your notes).
5. There will be a vocab quiz this week!!
6. Pg 55-58, #43, 57, 63-66, 85, 86
The End