s8p1 - weebly
TRANSCRIPT
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S8P1 Students will examine the
scientific view of the nature of matter.
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STOP
• In your own words describe what a cell
is and list it’s parts.
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Atoms • Atoms are the basic
building blocks of all matter.
• The smallest particle of matter.
• Like the bricks in a house.
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Parts of an Atom • An atom’s parts make it
different from other atoms.
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The Nucleus • At the center of an atom • Made up of two kinds of
particles –Protons –Neutrons
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Protons & Neutrons • Each have a mass of about 1 atomic
mass unit (amu) • Protons
–Carry a positive (+) charge • Neutrons
–Have no charge (neutral)
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Electrons • Move around in an area outside the nucleus called the electron cloud
• Carry a negative (-) charge • Have an insignificant mass compared to protons and neutrons
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STOP
• In your own words describe what an
Atom is.
• List the parts of an Atom, there location
in the Atom and their electrical charge.
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Elements • Each kind of atom is an element. • An element is a pure substance that cannot be
broken down into simpler substances.
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STOP
• What is an Element?
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Remember: The properties of an element are determined by the
structure of its atoms. • The main feature used to distinguish
the atoms of different kinds of elements is atomic number. – Atomic Number: the # of PROTONS in the
nucleus of an atom.
– It’s unique for each element.
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STOP
Describe what determines the properties
of an element?
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A more in depth look at an atom: • Does a carbon atom have a positive or negative
charge? – Hint: look at the # of subatomic particles.
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Atomic Mass • Protons + Neutrons = Atomic Mass
– The mass of a proton is 1 amu
– The mass of a neutron is 1 amu
– Electrons contribute no mass to an atom.
Proton
1 amu Neutron
1 amu
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Try a few… Element Protons Neutrons Electrons Atomic Mass
Carbon (C) 6 6 6
Oxygen (O) 8 8 8
Sodium (Na) 11 11 11
Potassium (K) 19 20 19
Iron (Fe) 26 29 26
12
amu
16
amu
22
amu 39
amu
55
amu
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Chemical Symbols
• A code, usually
one or two
letters, that is
used to
represent a
particular
element.
– Ex. – C=Carbon,
Ca=Calcium,
Fe=Iron, etc.
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Types of Matter
– Elements
– Compounds
– Mixtures
•All forms of matter can be classified into three groups based on how the atoms making up the matter are arranged.
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Mixtures • When two or more substances combine without joining together
chemically – The mixture’s parts retain their identity
• Heterogeneous – mixed unevenly • Homogeneous – mixed evenly • Mixtures can be separated more easily then compounds • Examples?
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STOP
• Describe what a mixture is.
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Pure Substances • Elements and Compounds
– Have a homogeneous composition • It’s properties and chemical makeup are the same throughout the sample
– Cannot be separated by physical means into the parts that make it up.
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STOP
• Describe what a pure substance is.
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Compound •Form when two or
more elements
join chemically.
–Join by
sharing
electrons
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STOP
• Describe what a Compound is.
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Example of a Compound • Table Salt
– Made up of Sodium (Na) and Chlorine (Cl) • Na – soft metal that explodes when combined with water
• Cl – poisonous gas
– Combine to form the edible, white solid: SALT!
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When elements combine to form
compounds, they DO NOT keep their
individual properties.
If they did, we wouldn’t be able
to eat salt!
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MATTER
Pure
Substances Mixtures
Heterogeneous
Mixtures
Homogeneous
Mixtures Elements Compounds
Made of one
type of atom
Made of more than
one type of atom
exists as
which include which include
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Molecules • The smallest unit of a compound that has all the
properties of the compound.
• Chemical Formula – uses chemical symbols and subscripts to identify the number and types of atoms of each element that make up a molecule of a compound.
Oxygen
Hydrogen Hydrogen H2O
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STOP
• Describe what a Molecule is.
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More with H2O • Chemical Symbol
for Hydrogen • Chemical Symbol
for Oxygen • What do you think
the “2” means? The # of atoms of that
element in the substance
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Subscript • Written to the right and slightly below a
chemical symbol to tell the number of atoms of that element in a substance.
• Water – H2O – Two molecules of Hydrogen – One molecule of Oxygen
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You Try! Common Name Formula How Many?
Dry Ice CO2 C- O-
Table Salt NaCl Na- Cl-
Fool’s Gold FeS2 Fe- S-
Cane Sugar C12H22O11 C- H- O-
Rust (Fe2O3)H2O Fe- O- H-
Asprin CH3CO2C6H4COOH C- H- O-
1 2
1 1
1 2
12 22 11
2 4 2
9 8 4