Chemical - Middle School Science - Mr Banks Home
Transcript of Chemical - Middle School Science - Mr Banks Home
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Chemical
reactionsMR. BANKS
7TH GRADE SCIENCE
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Atomic structure
Atoms are the smallest
things that can still be
considered a
chemical.
Atoms are made out
of small particles.
Protons and neutrons
in the nucleus at the
center.
Electrons orbiting
around the nucleus.
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Valence electrons
Electrons orbit the
nucleus at different
distances.
These different
distances are
known as energy
levels.
Electrons are held
onto more tightly
the closer you
move toward the
nucleus.
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Valence electrons
Electrons in the outermost energy level are held onto the loosest.
These outermost electrons are known as the valence electrons.
The valence electrons control the chemical bonding of the atom.
Valence electrons
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Valence electrons
An atom can have anywhere between 1 and 8
electrons in its valence.
The number of valence electrons an atom will
have is predicable and is seen on the periodic
table.
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Valence electrons
However, an atom
“wants” to have 8
electrons in its
valence.
Having 8 valence
electrons makes the
atom “stable”.
Hydrogen and
helium are the only
exceptions. They
each want two
valence electrons.
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Chemical bonds
There are only three ways for an
atom to get to 8 valence
electrons.
Take electrons from another
atom.
Give away electrons to another
atom.
Share electrons.
Each of these actions leads to
the formation of a chemical
bond between the atoms and
the creation of a compound.
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Chemical bonds
Electrons
given/taken
Electrons shared
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Chemical bonds
Two atoms can share
up to three pairs of
electrons at a time (six
electrons total).
Each pair of electrons
shared creates a new
bond.
The more bonds there
are between two
atoms the stronger
those atoms are stuck
together.
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Reactivity
Being close to having 8
electrons makes an atom
more “reactive”.
They will easily form bonds
with other atoms to
get/give away or share the
electrons they need.
They can even break apart
other compounds to get
what they need.
Atoms in groups 1a, 2a, and
7a are the most reactive.
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Physical property
Physical properties are characteristics of a substance that can be observed without changing the chemical identity of the substance.
Density, shape, texture, color, smell, taste, melting point, boiling point, hardness, solubility, flexibility, etc.
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A change where the form
of matter is altered, but
the chemical is not
transformed into a
different chemical.
Examples: cutting,
breaking, melting, and
freezing.
Physical changes
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Chemical properties
Chemical property – A
characteristic of a
substance that describes
its ability to chemically
change or react.
Can only be observed
when a substance
chemically changes.
Examples: Reactivity,
flammability, toxicity.
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Chemical changes
A process where one or
more substances are altered
into one or more new and
different substances.
A chemical reaction must
occur.
Burning, rusting, fizzing,
creating something new.
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Chemical properties
A chemical property of magnesium
is its ability to combine with oxygen
to form magnesium oxide.
Mg + O2 MgO
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Find an object in the room.
Describe that object in as many
ways as you can think of and
record your description in your
notebook.
Pair up with another student and
have them read your description
and try to guess your object.
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Chemical reactions
Signs of chemical reaction.
Bubbling (making gasses)
Changes in temperature
Production of an odor
Formation of a solid
Changes in color
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Compounds
The chemical and physical properties of compounds
are different from the properties of the elements they
are made of.
Soduim, Na Chlorine, Cl
Salt, NaCl
Na Cl
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Oxygen, O Hydrogen, H
Water, H2O
H
O
H
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1. A. Physical Change
B. Chemical Change
Rusting nails
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2. A. Physical Change
B. Chemical Change
Effervescent tablet
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3. A. Physical Change
B. Chemical Change
Cutting paper
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4. A. Physical Change
B. Chemical Change
Vinegar and Baking soda
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5. A. Physical Change
B. Chemical Change
Salt and water
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6. A. Physical Change
B. Chemical Change
Breaking glass
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7. A. Physical Change
B. Chemical Change
Burning wood
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8. A. Physical Change
B. Chemical Change
Ice melting
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9. A. Physical Change
B. Chemical Change
Sodium and water
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10. A. Physical Change
B. Chemical Change
Boiling water
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Changes in energy
When matter undergoes
a chemical change it
can either absorb or
release energy.
An exothermic reaction is
a reaction in which
energy is released.
This can be in the form of
sound, light, or most
commonly, heat.
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Changes in energy
An endothermic reaction
is a reaction in which
energy is absorbed from
the environment.
This can lead to a
decrease in temperature
or a reaction that has to
have energy constantly
added to it.
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Activation energy Activation energy is the
minimum amount of energy needed to start a chemical reaction.
All chemical reactions need some energy to get started.
Some reactions need very little and can get it from the environment.
Other reactions require an outside source to add energy, usually in the form of heat.
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