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Mr. Fleming
 D.1
What are the effects adding
energy to matter in terms of the
motion of atoms and molecules,
and the resulting phase changes?
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All of the physical ‘stuff’ around us
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Solids, Liquids, Gases
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What are some examples of matter?
◦ Rocks
◦ Air
◦ Trees
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The smallest building blocks of matter
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All matter is composed of one or more atoms
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They cannot be created or destroyed, but
simply change form
Composed of three particles: Protons,
Neutrons and Electrons
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Blue: Protons (positive charge +1)
Red: Neutrons (neutral charge)
Black: Electrons (negative charge -1)
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Atoms can combine to form complex
molecules, which make up all matter.
They combine via their electrons, which try to
fill up all of the available spaces the atom can
hold.
The many different ways that atoms combine
form the multitude of different kinds of
matter we find on Earth.
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Study of how energy in the form of heat is
transferred to various types of energy within
a system.
Defined by laws
Conservation of Energy
Energy can neither be created nor destroyed
only transferred between different types of
energy.
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The ability to do
work or make
things move.
Many different
types of energy
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Heat- the total kinetic energy of the particles that
make up a substance.
 Units- joules or calories (cal)
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When you add heat to an object, you are adding
energy to that object.
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The increase in kinetic energy causes the object
to expand.
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Heat flows from warmer to cooler materials.
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Contraction
◦ Lose Heat=atoms/molecules come together
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Expansion
◦ Gain Heat=atoms/molecules move further apart
What is heat a measure of?
The total amount of kinetic energy of the
particles that make up a substance.
What happens to the speed of the particles in a
substance as heat is taken away?
Slow Down
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Matter is made of particles (atoms and
molecules).
These particles are constantly in motion.
The speed that these particles are moving
determines the temperature of an object.
Temperature- a measure of the average
kinetic energy of the particles in an object.
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Three Scales:
Fahrenheit (˚F)
Celsius (˚C)
Kelvin (K)- Absolute
zero
Conversion Formulas:
˚C = (˚F - 32) x 5/9
˚F = (C x 1.8) + 32
˚K=(F+255.372)
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Heat
◦ Total Amount of Kinetic Energy
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Temperature
◦ Average Amount of Kinetic Energy
Beaker A and B have equal volumes. Beaker A
has particles moving faster than Beaker B.
Which beaker has the higher temperature?
Beaker A
Which beaker contains more heat?
Beaker A
Why does it get easier to open a jar when you
add hot water to lid?
Particles expand when heat is added to it.
Metal in lid expands causing it to loosen from
jar.
Are heat and temperature the same
measurement? Explain.
No, temperature is the average amount of
kinetic energy and heat is the total amount of
kinetic energy.
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Specific Heat- the amount of heat that is
needed to raise the temperature of 1kg of a
material by 1˚C.
This measurement determines how things
conduct heat.
Example- Plastic has a higher specific heat
than metal which is why we use plastic
spoons when we cook.
Specific Heat Demo
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Heat – the total KE of a material.
Temperature – the average KE of a material.
Specific Heat - the amount of heat that is
needed to raise the temperature of 1kg of a
material by 1˚C.
True or False:
For any two objects, the one with the higher
temperature always has more thermal energy.
False, glass could have higher temperature
than pool, but pool will have higher thermal
energy.
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Describe how the thermal energy of an object
changes when the object’s temperature
changes.
Thermal energy increases along with
temperature of object.
When heat flows between two objects, does the
temperature increase of one object equal the
temperature decrease of the other?
No, heat could be lost to air surrounding
object.