Transcript Ch. 1-- Matter and Change

Ch. 1—Chemistry: An Introduction
What is chemistry?
• Chemistry is the study of the ___________________
composition
of substances and the changes they undergo.
alchemy
• It began from “_______________”...
the attempts of alchemists to
change common metals into _________
through trial and error.
gold
Divisions of Chemistry
There are several divisions or branches of chemistry:
1) _________
Organic chemistry: the study of substances that contain ________
carbon
Example: how gasoline is produced from oil
Inorganic
without
2) _______________
chemistry: the study of substances __________
___________
carbon
Example: how table salt reacts with different acids
Click below for the link to the
lecture
• http://danreid.wikispaces.com/file/view/Ch.
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Divisions of Chemistry (continued)
3) _______________
Analytical
chemistry: the study of the _______________
quantitative
composition of substances
Example: how much chlorine is in a sample of tap water
Biochemistry
living
4) ____________________:
the study of the chemistry of _________
__________________
organisms
Example: how sugar in the blood stream of cats affect
insulin production
The Scientific Method
•
The scientific method is way to solve a scientific problem. It is an
approach to a solution (using mostly common sense.)
Example: Your flashlight doesn’t work. (Not necessarily a
“scientific problem.”)
Steps to the Scientific Method
observations
(1) Make _________________-Use your 5 senses to gather
information.
hypothesis
(2) Propose a ______________-Make an “educated guess” for what
is happening.
experiments
(3) Perform _______________-This tests your hypothesis. Many
experiments are sometimes needed to test a hypothesis. The same
experiment must give similar results if the experiment is to be
reliable.
Steps to the Scientific Method (continued)
(4) Make a _____________-theory
This should explain the results of your
experiments. Theories may ___________
or be ___________
change
rejected
over time because of results from new experiments.
Scientific Laws
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Laws describe ____________
natural
___________________.
phenomena
why the
A law tells what happens. It does not attempt to explain _____
phenomena occurs. (That is the job of a theory.)
math
equation
Laws can often be summarized by a _____________
__________.
Ideal
Gas ______”)
Law
Example: PV = nRT (The “_________
______
This equation is used in Ch. 12. The law shows the
relationship between the pressure, volume and
temperature of a given quantity of gas in a
container.
Chapter 2--Matter & Change
Matter vs. Mass
•
mass and takes up ___________.
space
Matter is anything that has _________
solids __________,
liquids and ________...
gases
Examples: ________,
(the three
phases of matter)
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light
Things that are NOT matter: __________,
heat, emotions
________, sound...
Mass is the amount of ___________
in an object.
matter
The standard metric unit for mass is the ______________.
kilogram
Plasma
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Plasma is a high energy electrically charged mixture of ions and
electrons. __________
are made of plasma.
Stars
While plasma is the most abundant phase of matter in the universe,
on earth it only occurs in a few limited places:
– Lightning bolts
– Flames
– Fluorescent lights
– Aurora Borealis (Northern Lights)
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Bose-Einstein Condensate
Predicted in 1924 and created in 1995, the BEC is a small group of
atoms clumped together when taken down to a few billionths of a
degree above absolute zero.
This group of atoms takes up the same place, creating a "super
atom." There are no longer thousands of separate atoms.
They all take on the same qualities and for our purposes become one
blob.
Einstein
Bose
http://www.colorado.edu/physics/2000/bec/
400 nanoKelvins
200 nK
50 nK
States of Matter
phase
fixed shape
fixed volume
compressible
solid
YES
YES
NO
liquid
NO
NO
YES
NO
NO
YES
gas
Particle Motion
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vibrate
Solids-- particles ____________
back and forth in fixed positions
slide past each other in the container
Liquids-- clumps of particles ______
fly all over the place and collide
Gases-- individual particles _____
_________
Vapor is a term used for a gaseous substance that is normally a
________
solid or _______
liquid at room temperature.)
Example: _______
water vapor
States of Matter
Physical Properties and Physical Changes
•
Physical properties can be determined/measured without changing
the substance’s composition.
Examples: _______,
color odor, __________,
taste
mass, ________,
density
_________
point, hardness,
boiling point, ____________
melting
solubility, etc.
•
Physical Changes alter a substance without changing its
composition.
Examples: crushing, ripping, breaking, and any _________
phase
changes…(boiling, freezing, melting, etc.)
•
Most physical changes just alter the size of the particles and are
usually reversible.
Physical Properties
Physical Changes: Names of the Phase Changes
Solid
Gas
Liquid
SolidAqueous = ___________
dissolving
Aqueous  Solid = ___________
crystallizing
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Mixtures
Mixtures are a physical blend of two or more substances mixed
together.” The parts can be separated by _____________
means or
physical
____________
changes.
physical
There are 2 types of mixtures:
(1) _________________
Heterogeneous Mixtures: the parts mixed together can still be
distinguished from one another...NOT uniform in composition.
Examples: chicken soup, fruit salad, _____,
dirt sand in water
Homogeneous
(2) _________________
Mixtures: the parts mixed together cannot be
distinguished from one another...completely uniform in
composition.
Examples: ______,
Air Kool-aid, ________,
Brass salt water, milk
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solution
Another term for a homogeneous mixture is a “______________.”
Heterogeneous Mixtures
Homogeneous Mixtures
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Distillation
One way to separate a _________
solid from a ___________
liquid
in a
solution is by distillation. There are 2 steps to the process:
Step 1: _________
Boil the solution.
Condense
Step 2: ________________
the vapor as is escapes and collect it.
Distillation Animation
•
Chemical Properties and Chemical Changes
Chemical properties cannot be determined/measured without
changing the substance’s composition
Examples: ____________,
burning
whether or not it reacts with an
acid or a base.
Chemical Changes
•
Chemical changes will alter a substance and change its composition.
rusting
Examples: burning, ___________,
rotting or decomposing,
fermenting
__________________,
and other chemical
reactions.
•
Most, but not all, chemical changes are irreversible.
– You can’t “reverse” the burning of paper.
– _____________
use a reversible chemical reaction
Rechargeable ____________
batteries
Indications of Chemical Reactions
1) ________
Heat is produced: (________)
matches
Light is produced: (_____________
lightning
fireflies
2) ________
bugs/_____________)
Electricity
3) ______________
is produced:
(______________)
batteries
Indications of Chemical Reactions
4) ___________________
Precipitate
forms: (_______
soap ________)
scum
Two liquids chemically
react to form a solid.
5) gas/smoke/odor/bubbles produced:
soda
fizz
(________
______)
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Elements vs. Compounds
An element cannot be ___________
broken
down or _____________
changed
into
simpler substances by chemical means.
Elements are the _________
simplest forms of matter that can exists in
normal laboratory conditions.
Examples: _______,
Gold Helium, __________
Mercury
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2 or ________
more different elements
A compound is made up of ____
______________
chemically bonded together.
Compounds can only be broken down into simpler substances by
____________
chemical ____________.
reactions
Water Sand, _______________
NaCl (table salt)
Examples: _______,
Classification of Matter
Classification of Matter
Classification of Matter
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Chemical Symbols
Chemists use chemical symbols for the elements involved in a
chemical reaction. The symbols are a shorthand way of representing
the ______________.
(See the Periodic Table for a list of all the
elements
symbols.)
The first letter of the chemical symbol for an element is always
capitalized
_________________.
The next letter, if needed, is _______________.
Each capital letter
lowercase
in a formula, therefore, represents another element.
H ____,
Ne Hg, ___,
S NaBr, ________,
H2O LiC2H3O2
Examples: ____,
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Some symbols come from _______
Latin names: Au=Aurum (Gold)
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Chemical Reactions
When writing chemical reactions, the substances that ___________
react
with each other are written on the _______
left and are called
“reactants”.
The substances that are ____________
produced are written on the _______
right
and are called the “products.”
Reactants  Products
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yields or “reacts to
The “ ” symbol can be read as “_______”
produce.”
Example: two
2Hhydrogen
2H2O
2 + O2  molecules
plus one oxygen
which
means
“____________________________________
molecule
yields
two water molecules
________________________________________________.”
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Conservation of Mass
During chemical (or physical) reactions, mass (or matter) is neither
_____________
nor _________________.
created
destroyed
The mass of all the reactants _________
equals the mass of all the products.
number of each kind of atom is the same.
The ___________
Sometimes it appears that the reactant and product masses are not
gas was probably a reactant or product in the
equal, but a _______
reaction, and that is making the difference!
Example:
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2H2 + O2  2H2O
If 4 grams of hydrogen reacted with oxygen to produce 36 grams of
32
water, how many grams of oxygen were used? _______
# of H’s and O’s on each side is __________!
constant
Notice that the ____
Conservation of Mass
CaCl2 + Na2SO4  CaSO4 + 2NaCl
mass before = mass after
# atoms before = # atoms after