Download Chapter 1 - Palm Beach State College

Chapter 1
So . . . Where’d it all come from?
The Home World

The Earth, and this entire
star system, formed
approximately 4.5 billion
years ago.

The earth, and everything else
in the solar system, condensed
out of a Nebula left behind
by an exploding star.
(Supernova)

(This is not to be confused
with the Big Bang. Which
happened about 14 billion
years ago.)
This, is a Nebula.
M16
the Eagle Nebula
It’s in layers

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As the earth condensed it formed into layers of different
densities.
Your textbook refers to these layers as the different “Spheres”
of the earth.
See page 19
The Geosphere and the Biosphere
The Geosphere is the solid earth. The Biosphere is all of the life on the earth.
All of the Earth’s “spheres” are
interconnected and they all affect
each other.
The Atmosphere and the Hydrosphere
The Cryosphere
All of the Earth’s “spheres” are
interconnected and they all affect each other.
Earth System Science
Melting Antarctic Ice Caps
Earth is the only planet
in this solar system
where water can exist
as a solid, and as a
liquid and as a gas, all
at the same time.
It really is a pretty neat
trick.
It’s often called the “Goldilocks Effect”
Because everything has to be “ . . . Just right.”
The scientific method
Galileo is credited for inventing the Scientific
Method that we use today.
 Question


Hypothesis – a tentative, unproven explanation.
 Observations
and experimentation
 Publish:
 'Nullius
in verba'
 “Take no ones word for it”
 Theory – A fact, here and now.
 A Scientific Theory is not a guess.
 Law – True everywhere in the Universe,
throughout all of time.
Feed back mechanisms

Positive – goes on and on and on and on . . .

Negative – Something steps in to stop the cycle.
Renewable and Non renewable resources

Truthfully, in the long term, everything is renewable eventually.

Everything on earth has always been here in one form or
another. We just keep using it over and over again.

Water, soil, every atom in your body.
Chapter 2: Atomic structure
I don’t want to spend too much time on this because you
have learned it all once before.





This is what you are responsible for from Chapter 2.
This will be on the midterm.
Where does an atom’s Atomic Number and Atomic
Mass come from? What do these number stand for?
How do you determine the number of protons,
Neutrons and Electrons in an atom?
What is the difference between an Ion and an
Isotope?
http://education.jlab.org/qa/pen_number.html
The Periodic Table

Invented by Dimitri Mendeleev.

Elements 1 – 92 are natural and were all constructed during the Supernova. Elements
93 and up are all man made.

Rules for placing elements on the periodic table.
New elements must be placed on the Periodic Table in order of their
Atomic Number.
 New elements must be placed on the Periodic Table according to
“Periodicity of Properties.”

 This
means similar elements must be grouped together.
 This
is what gives the Periodic Table it’s weird shape.
One of Mendeleev’s first Periodic tables
Chapter 2
Atomic structure and minerals

Atom - smallest part of an element which
retains all of the characteristics of that element.

Is there anything smaller than an atom?

Yes of course. But once you break apart the
atom, the element loses all of its physical
characteristics.
What are the parts of the atom and what do
they do?
Proton – Located in the nucleus and gives the
atom it’s physical characteristics. It is
probably the most important part of the atom.
 Neutron – Also in the neucleus, all it does is
add mass.
 Electron – Extraordinarily tiny. It is so small it
is not even counted when measuring the mass
of an atom. It is located outside the nucleus in
the Electron Cloud it is involved in bonding
atoms together to form compounds.

What does an atom look like?



No one really knows for sure.
Facts:
1) The Nucleus is very, very
small but very, very heavy. The
Nucleus accounts for only 1%
of an atoms size, but, 99% of an
atoms mass!
2) The electron cloud accounts
for 99% of the atom’s size, but
only 1% of the atom’s mass.
Using the Periodic table

The number of protons is always equal to the
atomic number.

The number of electrons is usually equal to the
number of protons.

Atomic Mass is the sum of Protons + Neutrons

The number of neutrons is equal to the Atomic
Mass minus the Atomic Number.
Using the Periodic table

How do you determine the number of protons, Neutrons and
Electrons in an atom?

The number of protons is the same as the Atomic number.

The number of protons can’t be changed. If it did the element
itself would change.
Neutrons

The Atomic Mass is the Sum of Protons plus
Neutrons in an atom’s nucleus.

The number of neutrons is calculated by
subtracting the Atomic Number from the
Atomic Mass.**
Electrons

The number of electrons is usually the same as
the number of protons.
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However, electrons are not held very tightly
and they can come and go quite freely.

When this happens the atom becomes
electrically charged. Either positive or
negative, like a magnet.
Ions and Isotopes

Ions are atoms with the wrong number of electrons.

Isotopes are atoms with the wrong number of neutrons.
Ions

Atoms gain and lose electrons quite easily.
When they do they become an Ion.

Ions attract each other

Since opposites attract, Positive and Negative
ions attract each other and this is how
Compounds are formed.
Compounds

Compounds are completely different from the
elements from which they are formed.**

Water is H2O, a compound of hydrogen and oxygen.

Water is nothing like hydrogen and it is nothing
like oxygen.
Most substances in nature are compounds. It is
rare to find elements in their pure form.
Isotopes
Isotopes are atoms with the wrong number of
neutrons.
 Isotopes are atoms of the same element with
different mass numbers.


Isotopes are usually radioactive and dangerous.

Hydrogen is one of the best examples of an
isotope.
Minerals

Atoms make
minerals

Minerals make
rocks

Rocks make the
Earth