Download Notes. - Net Start Class

C. Smith
Fall 2016
Properties of Matter
Matter is any substance
that has mass and takes
up space (volume).
All objects contain
matter.
Extensive
properties are
properties that
depend on the amount
of matter present.
Mass
Length
Volume
Intensive properties
are used to identify a
substance (does not
changed based on
amount).
Density
Color
Crystalline shape
Melting and Boiling point
Refractive index
Solids
Solid particles occupy a
regularly fixed position
in relation to
surrounding particles.
Solid particle appears to
vibrate around a fixed
point.
Particles are closely
packed and travel a
distance equal to only a
fraction of their
diameter before
colliding.
Solid particles are
arranged in a definite
pattern and have
definite shape and
volume.
Liquids
Liquid particles do not
act independently of
each other - motion is
limited.
Liquid particle slips by
each other because the
particles have vibratory
type of motion.
The particles still
travel in a straight-line
path between collision.
Liquids have definitive
volume and assume the
shape of their
container.
Gases
Gas particles are
independent of each
other and move in a
straight line.
Change in direction
occurs only with
collisions.
Gases assume the
shape and volume of
their container.
Plasma
Plasma is a high energy electrically
charged mixture of ions and electrons.
Particles that have been ionized
(charged)
There exist at extremely high
temperatures.
Exist at naturally (stars) or man-made
(neon signs).
While plasma is the most abundant
phase of matter in the universe, on
earth it only occurs in a few limited
places.
Bose-Einstein condensate
Extremely dense form of matter.
Particle motion slowed down by
decreasing temperature to cease
motion.
Consider to be super unexcited and
super cold (approaching absolute zero, –
273K)
Physical changes are changes in the form of a
substance but not in the substance.
The substance remains the same after the
change but appears different. (Phase change)
Physical changes can be reversible (but not
always).
Examples of phase changes
Melting
Freezing
Boiling/Vaporization
Condensation
Evaporation
Sublimation
Chemical changes
are changes in
which a new
substance with
different
characteristics
from the original
substance is
produced.
There are several
examples of
chemical changes
Burning
Digestion
Fermenting
Corrosion
Chemical
properties
describe the
reaction of a
substance with
other material
or the reaction
within the
substance itself.
Lack of
chemical
reactivity is also
important.
The evidence of a
chemical reaction
Color Change
Formation of a gas
Temperatures change.
Odor
Precipitate (solid)
Heterogeneous means more than one type of
substance. Heterogeneous matter exists in the
form of mixtures.
A mixture is matter that consists of two or
more different materials.
Mixtures can be separated by physical means.
(distillation and filtration)
Mixtures have phases, which are any region
with a uniform set of properties.
The boundaries between these phases are
called interfaces.
Homogeneous means only one type of a
substance.
Homogeneous matter is matter that is
uniformly mixed and cannot be separated
easily.
Homogeneous matter exist in several
forms:
Pure Substances- Elements & Compounds
Solutions
Solutions consist of solute (dissolved
material) and solvent (dissolving material).
Solute particles are very small and are
scattered in the solvent and appear as
uniform.
Solutions are not always liquid.
Filtration
• Separates a solid from a liquid
• Often used in chemistry labs
Distillation
• A liquid is boiled into
vapor and then
condensed into a liquid.
• Used to separate water
from impurities in the
water
There are two types of pure
substances.
Elements
Compounds.
Substances made of only one kind of
atom are called elements.
Substances made of more than one kind
of substances are called compounds.
Elements are the building
blocks for all other
substances.
Cannot be broken down
into simpler substances.
All atoms of an element
have the same number of
protons.
There are 109 of these
currently listed and named
on the Periodic Table
Metals: found on the left and
center of the Table of Elements
Non-metals: found on the right
side of the Table of Elements
Metalloids: found along the
stair-step line
Synthetic: made in the
laboratory and not yet found in
nature – many of the Actinide
and Lanthanide series and very
large # elements.
Compounds
Compound- Made of
molecules- two or more
atoms
can be separated into
simpler substances only
by chemical means.
Molecules are the
smallest particle of a
compound that retains
its properties and it is
composed of 2 or more
atoms.
When they are
broken down, the
pieces have
completely
different
properties than
the compound.
Each element is represented
by one- or two- letter
chemical symbol.
The symbols for most
elements consist of the first
one or two letters of the
element’s name.
A chemical formula is a
combination of symbols that
represents the composition of a
compound.
A formula shows two things:
1.The elements present in
the compound
2. The relative number of
atoms of each element in the
compound.
Example H2O
Formulas often contain numerals
to indicate the ratio of elements
in the compound.
The numbers used in the
formula are called subscripts.
During a chemical reaction, the quantity of matter is
unchanged. The mass of products is always equal to
the mass of reactants. The same can be said for
physical changes.
This is known as the Law of Conservation of Mass.
The law states that mass can neither be created nor
destroyed, it is conserved. Some of the mass can be
in the form of energy or a gas.
Cannot be
separated
physically
Can be
separated
physically
Pure
Substance
Mixture
Can see
the parts
Cannot
see the
parts
Heterogeneous
Mixture
Homogeneous
Mixture
Can be
separated
chemically
Compound
Cannot be
separated
Element
Three types
suspension
Most impure
colloid
solution
Most pure


Nichols, Nancy : Klein Collins Science
specialist (Ret.)
Textbook: Chemistry , Wilbraham, Staley,
Matta, Waterman; Pearson Realize