Chapter 1- matter and change
Bravo – 15,000 kilotons
Do Not Need
in your
Notebook
Introduction
• “It has been said that Chemistry is what connects
us to the world. Everything we see, taste, and
touch is matter. Matter is what makes the world a
real place. Chemistry is the study of matter: its
properties, composition, and how some types of
matter interact with other types of matter in new
and interesting combinations.
• Chemistry is heavily involved in many interesting
and fascinating jobs, from making perfumes to
investigating crime scenes, from preparing great
tasting and safe foods to developing life-saving
drugs.”
Section 1-1
• Chemistry a physical science, is the
study of the composition, structure,
and properties of matter and the
changes it undergoes.
• Chemical is any substance that has a
definite composition. Example water
is always H2O. Everything is made of
chemicals.
• Branches of chemistry. Chemistry is
divided into six main areas of study.
6 Branches of Chem
1. Organic Chemistry- The study of most
carbon containing compounds. Example
C6H12O6 Glucose
2. Inorganic Chemistry- The study of all
substances not classified as organic;
compounds that do not contain carbon.
Example H2O Water. High school
chemistry is mostly inorganic chemistry.
3. Physical Chemistry (P-Chem)- the study
of the properties, changes, and
relationship between energy and matter.
4. Analytical chemistry- the identification of
the components and composition of
materials.
5. Biochemistry- the study of substances and
processes occurring in living things.
Example Photosynthesis
6. Theoretical Chemistry- the use of
mathematics and computers to design and
predict the properties of new compounds.
Types of Research
1. Basic Research-how and why
2. Applied Research- solve a specific
problem. Example the depletion of the
ozone layer.
3. Technological Development-involves the
production and use of products that
improve our quality of life. Technology is
the application of scientific knowledge to
solve problems. Examples Computers and
biodegradable materials.
Section 1-2
• Mass is the measure of the amount of
matter.
• Matter is anything that has mass and
volume (occupies) space. Examples air,
smoke, water vapor.
• Atom is the smallest unit of an element
that maintains the properties of that
element.
• Element is a pure substance made of only
one kind of atom. Periodic Table.
• Compound is a substance that is made from
the atoms of two or more elements that
are chemically bonded.
• Physical properties can be observed or
measured without altering the identity of
a material. Example melting ice to find the
melting point.
• Extensive Physical Properties- depend on
the amount of matter present and include
mass, length, and volume.
• Intensive Physical Properties- do NOT
depend of the amount of matter. Examples
melting point, boiling point, Density,
ductility, malleability, color, crystal shape
• Physical change is any change that
does NOT result in a change in
identity. Examples cutting wire,
crushing a solid, gas expanding.
• Changes in state is a physical change.
Example melting, boiling, freezing.
• Chemical Properties relates to a
substances ability to undergo
changes that alters it identity.
Example a chemicals reactivity.
• Chemical change or reaction (Rxn)
when a substance is converted into
different substance. Examples milk
souring, leaves changing color in the
fall.
• Basic Chemical Formula
• A+BC
• A and B are called Reactants
•  is read as “yields”
• C is the product (s)
4 states of matter
1. Solids have definite shape and
volume. Particles are packed closely
together.
2. Liquids have definite volume but, no
shape
3. Gases have neither a definite
volume nor definite shape.
4. Plasma is a gaseous system of
charges particles. Found on the sun.
Weight vs. Mass
• Weight is the pull
of gravity on an
object.
• Mass is the
quantity of matter.
• Astronauts in
space.
• Law of conservation of mass states that
matter can NOT be either created or
destroyed by ordinary chemical or physical
changes. Examples burning wood, nuclear
reactions
• Law of conservation of energy states that
E can NOT be either created or destroyed
but it can be converted from one form to
another. Examples Kinetic & potential
energy.
Classification of Matter
•
Mixture is a blend of two or more kinds
of matter, each of which retains its own
identity and properties and can be
separated physically.
• 2 types of mixtures
1. Homogeneous (solutions) have uniform
composition throughout. Examples air,
sugar in water, stainless steel.
2. Heterogeneous not uniform. Examples
granite, wood, blood.
Do Not Need in
your Notebook
Matter
Can it be
separated?
YES
NO
Mixtures
Pure Substances
Is the composition
uniform?
Can it be decomposed by ordinary
chemical means?
YES
NO
YES
NO
Homogenous
Mixtures
Air, sugar in water,
stainless steel
Heterogeneous
Mixtures
Granite, wood, blood
Compounds
Water,
sodium chloride,
sucrose
Elements
Gold, aluminum,
oxygen
o A pure substance has a fixed
composition and differs from a
mixture by all pure substance have
exactly the same physical and
chemical properties and every sample
of given pure substance has exactly
the same composition.
o Pure substances can be classified as
either compounds or elements.
Pure substances
• Compound is a substance that is
made from the atoms of two or more
elements that are chemically bonded.
Examples water, sodium chloride,
sucrose. Can not be separated
physically.
• Element made of one pure substance
that cannot be decomposed by
chemical changes. Examples gold,
silver, hydrogen.
Section 1-3
• Periodic table of elements is divided
into small squares that have one
element in each square.
• Elements have been named from
their Latin meaning, places, famous
scientist and from mythology.
Nonmetals
F
A
M
I
L
Metals Lf of step
Period
N
O
B
L
E
y
• Family or groups- vertical columns (18)
• Period- horizontal rows (7)
• Metals- ductile, malleable, lustrous, conduct
heat and electricity, high tensile strength
• Nonmetals- brittle, dull, poor conductor
• Metalloids- have some characteristics of
metals and nonmetals. Are semiconductors
• Nobel gases- family #18 unreactive gases
as room temp. WHY???
Work Cited
• July 25, 2006. “Pigs in Space”. JPG.
http://www.porphyrios.it/index.php?m=20050718
• July 25, 2006. “Chemistry”.
http://www.aprenda.info/Chemistry.asp
• July 27, 2006. “Periodic Table illustration”.
http://www.physast.uga.edu/classes/phys1010/heil/announc
ement%20files/equations/unit_4_eqs/periodic_table_illust
r.png
• Holt, Rinehart and Winston. Modern Chemistry. Harcourt
Brace & Company. 1999.
• Title slide “Bomb picture”. July 25, 2006.
http://www.sciencegeek.net/Chemistry/Powerpoint/Unit1/U
nit1_files/frame.htm