Matter Unit Vocabulary
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Matter
Kinetic Theory
Solid
Liquid
Gas
Plasma
Phase change
– Freezing
– Melting
– Deposition
– Sublimation
– Condenstation
– Vaporization
Physical properties
– Ducility
– Malleability
– Melting point
– Boiling point
– Freezing point
– Solubility
– Reaction to light
– Electrical conductivity
Chemical properties
– Flammability
– Oxidation
– decomposition
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Physical change
Chemical change
Demoritus
John Dalton
JJ Thomson
Ernest Rutherford
Niels Bohr
Atomos
Bohr Model
Cloud Model
Valence Electrons
Energy Levels
– Shells
Properties of Water
– Universal solvent
– Adhesion
– Cohesion
– High specific heat
– Capillary action
– Surface tension
– Polarity
– States of matter
– Heat of vaporization
– pH
Matter
• Anything that has mass and occupies space
• The materials or “stuff” that all objects and
substances in the universe are made of
• 4 States of Matter = Solid, liquid, gas, and
plasma
Matter
• Because all matter takes up space (has
volume) and contains a certain amount of
material (has mass), all matter can be
detected and measured
Examples of Matter
• Rocks, water, trees, bicycles, lighting, animals,
stars, smoke, are all easily seen and observed
• Dust mites that live in your furniture and rugs
you may need a microscope to view
• Air maybe invisible but we can feel it when the
wind blows and see it bend the branches of
trees (oxygen, nitrogen, hydrogen, CO2)
What is not matter?
• Light
• Sound
• Gravity
• Friction
Matter
• Atoms are the building blocks of matter
• The elements in our periodic table make up all
matter
Kinetic Theory
All matter consists of tiny
particles that are in constant
motion.
Kinetic Theory
1. All matter is composed of small particles
(atoms, molecules, or ions). There is an
attractive force between them.
2. They are in constant, random motion.
The particles may collide with one another
or the sides of their container.
3. As the temperature increases the
speed of the particles increases. As the
temperature decreases the speed of the
particles decreases.
SOLIDS
•State of matter that
has a definite shape and
a definite volume.
•Particles of solids are
tightly packed, vibrating
about a fixed position.
•Particles are strongly
attracted to each other
LIQUID
 A state of matter that has
a definite volume but
takes the shape of its
container
 Liquids do not have a
definite shape
 Particles of liquids are
tightly packed, but are far
enough apart to slide over
one another, allowing it to
flow
GAS
 A state of matter that has no
definite shape and no definite
volume; expands to fill the
shape of its container
 Particles of gases are very far
apart and move freely.
 Attractive forces are very weak
• Contain mostly empty space –
because the particles are so far
apart
• Particles spread throughout a
given volume until distributed
equally – diffusion
Gas vs. Vapor
• Gas – a substance that
is naturally in the
gaseous state at room
temperature
• EXAMPLE: Helium
• Vapor – the gaseous
state of a substance
that is a solid or liquid
at room temperature
• EXAMPLE: Steam
PLASMA
 A state of matter that
does not have a definite
shape or volume and
whose particles have
broken apart
 Consists of + and –
charged particles
(electrons are knocked
off due to collisions)
 A plasma is a very good
conductor of electricity
and is affected by
magnetic fields.
• Plasma is the
most common
state of matter in
the universe
STATES OF MATTER
SOLID
LIQUID
GAS
PLASMA
Tightly packed, in a
regular pattern
Vibrate, but do not
move from place to
place, definite
shape and volume
Close together with
no regular
arrangement.
Move about, flow
and slide past each
other. Definite
volume, no definite
shape takes shape
of its container.
Well separated
with no regular
arrangement.
Move freely at high
speeds. No definite
shape or volume.
Easily
compressible.
Has no definite
volume or shape
and is composed of
electrical charged
particles
PLC-Unit 1B
STATES OF MATTER
SOLID
Tightly packed, in a
regular pattern
Vibrate, but do not
move from place to
place
LIQUID
Close together with
no regular
arrangement.
Vibrate, move
about, and slide
past each other
GAS
Well separated with
no regular
arrangement.
Vibrate and move
freely at high
speeds
PLASMA
Has no definite
volume or shape
and is composed of
electrical charged
particles
Phase Change
A transition of matter from one
state to another.
Some phase changes are more common and
easier for us to visualize.
For example, you have probably witnessed
freezing, melting, and vaporization just by
making ice, melting ice, and boiling water.
Condensation often occurs on the
outside of cold beverage containers. This is
when the humid air changes directly to a
liquid on the surface of the container.
Sublimation
Dry ice is actually solid carbon dioxide.
When it sits in the open or is placed in
water it rapidly changes directly from solid
to gas creating a foggy cloud.
Deposition
Frozen patterns of ice on your car windshield is
an example. Deposition involves a gas changing
to a solid. This occurs during winter months
when the humid air directly freezes into solid
ice.
Physical properties
• Characteristics that can be observed without
changing the makeup or identity of the matter
• Examples: color, size, state of matter, density,
ductility, malleability, boiling point, melting
point, freezing point, electrical conductivity,
solubility, reaction to light
Density
• The ratio of the mass of an object to its
volume
• Formula: d = m/V
• Units: g/mL or g/cm3
Ductility
• The ability to be pulled into a thin
strand
• EX: wire
Malleability
• The ability to be pressed or pounded into
a thin sheet
• EX: aluminum foil, sheet metal
Boiling Point
• The temp at which a substance changes
from a liquid to a gas
• EX: the boiling point of water = 1000C
Melting Point
• The temp at which a substance changes from
a solid to a liquid
• EX: the melting point of chocolate is 340C
Freezing Point
• The temp at which a substance changes
from a liquid to a solid
• EX: the freezing point of water = 00C
Electrical Conductivity
• How well a substance allows electricity
to flow through it
• EX: copper wires,
electrical lines
Solubility
• The ability to dissolve in another substance
• EX: sugar in water
Reaction to Light
• Reflection – to bounce off ( mirror)
• Refraction – to bend (water)
• Absorption – to take in (leaf)
Reaction to Light
• Transmission – allow to pass through
– Opaque – little to no light passes through
(blanket)
– Translucent – some light passes through
(sunglasses)
– Transparent- most light passes through ( glass
window)
Chemical properties
• The ability of matter to undergo a specific
chemical change, creating a different type of
matter with new properties
• Examples: flammability, decomposition,
oxidation
Flammibility
• To burn
• Must occur in the presence of oxygen
• EX: Flame tests help to identify metals by their
characteristic flame color
Decomposition
• To rot or breakdown
• Complex compounds breakdown to simpler
substances
• EX: CO2 breaks down to Carbon and Oxygen
Oxidation
• The process of losing electrons
• EX: iron rusts when exposed to oxygen
Physical Changes
• A process where a substance’s
chemical properties have not
changed
• Can be a change in size, color, shape, state of
matter
• EX: ice melting, salt dissolving in water, glass
breaking
Chemical Change
• Occurs when new substances or
materials are produced to have
different chemical properties from
the reactants
• EX: rust is the product
of iron and oxygen,
wood burning
Democritus
• Greek philosopher in 440 bc
• Was the first to proposed the
existence of atoms
• “Atomos” meaning “not to be cut”
John Dalton
• British chemist 1803
• Atomic Theory – He came
up with the theory that all
substances were made of
atoms
• Atoms were small, hard,
dense spheres that could
not be created, destroyed,
or altered
Dmitri Mendeleev
• Known as the father of the present day
periodic table
• Organized the elements (each type of atom)
by similar properties in 1869
J. J. Thomson
• British scientist 1898
• Proposed that atoms themselves were made
of smaller particles .
• He discovered that atoms contained
negatively charged particles, but did not know
their location
J. J. Thomson
• Theorized the negatively
charged particles were
spread evenly
throughout the
positively charged
material
• Thomson’s model of the
atom was called the
“plum-pudding” model
Ernest Rutherford
• 1911 a former
student of
Thomson's
• Proposed that atoms
had a dense,
positively charged
nucleus surrounded
by electrons
Niels Bohr
• 1913 Danish scientist
• Said that electrons
revolve around the
nucleus in circular
paths, called orbits
• And that electrons
could only exist in
certain orbits and at
certain energy levels
http://youtu.be/wCCz20JOXXk
Today’s model
electron cloud model
• Bohr’s model was an
important stepping stone
to today’s, which was
developed in the 1920’s
• Electrons surround the
nucleus, traveling not in
prescribed paths but in
regions of various
thicknesses called clouds
http://youtu.be/kYkD-dcupAU
Bohr Model
• Electrons orbit the nucleus
of an atom in set energy
levels
P = 20
N = 20
Energy Level
• The specific energies an electron in an atom
can have
• In the Bohr model used to describe the
different orbits or shells that the electrons
travel in around the nucleus
Valence Electrons
• The electrons in the highest or
outermost energy level
Polarity
• When electrons are not shared equally in a
covalent bond, causing one end of the water
molecule to have a positive charge while the
other has a negative charge
Each end of a water
molecule is attracted
to the opposite
charged end of
another water
molecule. Water's
polarity is
responsible for the
"stickiness" or
cohesion between
the molecules.
States of Matter
• The only known substance to naturally exist
on Earth in all three states of matter is water
Solid - Ice
Gas - Clouds
Liquid - Lakes
pH
• The measure of how acidic or
basic water is
Rainwater
Universal Solvent
• More
substances
dissolve in
water than in
any other
liquid
Cohesion
• Water molecules are attracted to more water
molecules so they stick to each other
Water ↔ Water
Adhesion
• Water molecules are attracted to and stick to
other substance
Water ↔ Other
Surface Tension
• Water molecules have a stronger attraction to
each other than to the air above, so the water
molecules cling tightly to each other forming
what’s like a skin at the surface
Capillary Action
• Movement of water within the spaces of a
porous material due to the forces of adhesion,
cohesion and surface tension
High Specific Heat
• The amount of energy required to raise the
temperature of water by one degree Celsius is
quite large, causing the temperature of water
to change slowly
Heat of Vaporization
• Water absorbs heat as it changes from a liquid
to a gas