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Chapter 1: Chemistry (right)
Standard 1
Atomic and Molecular Structure.
 The periodic table displays the elements in
increasing atomic number and shows how
periodicity of the physical and chemical properties
of the elements relates to atomic structure. As a
basis for understanding this concept students will
master 5 standards a-e.
4 pictures/4 color min.
1
2
(for the rest of the page)
3
4
Chemistry Vocabulary
CH. 4.1
On the left hand side, on the bottom HALF of p.
10, define the following words. (If you can answer
WITHOUT using your book, you are pro status!)
Nucleus
Proton
Neutron
Electron
Valence electron
Orbital
Molecule (105)
Parts of an Atom MUST HAVE COLOR! On Ch. 1 cover page box number 1
The Nucleus
Carbon
Proton (+)
EMPTY
space
++
++
++
Neutron
(neutral)
Electron (-)
Valence
electrons
Chemistry (what do you know?)
This goes on top ½ of p. 10 in NB (above 4.1 vocab words)
Write down anything you can think of or remember about
these subjects.
Chemical Bonding
Atoms
Chemistry
Chemical
Thermodynamics
Periodic Table
Chemistry Standard 1e

e. Students know the nucleus of the atom is much smaller
than the atom yet contains most of its mass.

What is the
definition of
“atom”?

Where is most of
the mass of an
atom located?


Atoms make up EVERYTHING you have ever
experienced!
“Atom” comes from a Greek word meaning
“unable to be divided”.

Most of the mass is located in the NUCLEUS,
other than that, atoms are mostly EMPTY space.
 If you compared the atom to a football
stadium, the nucleus would be the size of a
pea….

Balloons/empty space
This is 106,000 people!
Chemistry Standard 1e

e. Students know the nucleus of the atom is much smaller
than the atom yet contains most of its mass.

What is the
definition of
“atom”?
Where is most of
the mass of an
atom located?


What are the
main parts of an
atom?

“Atom” comes from a Greek word meaning
“unable to be divided”.

Most of the mass is located in the NUCLEUS,
other than that, atoms are mostly EMPTY space.



If you compared the atom to a football
stadium, the nucleus would be the size of
a pea….
Nucleus – the central part of the cell
 Protons (+) inside the nucleus
 Neutrons (neutral) inside the nucleus
Electrons (-) fly around OUTSIDE the nucleus at
tremendous speeds.
Chemistry Standard 1e

e. Students know the nucleus of the atom is much smaller
than the atom yet contains most of its mass.

What is the mass 
of a proton,
electron and
neutron?
Which
particle
is 
Particle
Charge
the smallest?

Proton
+1
Neutron
0
Electron
-1

DRAW this chart in your book. Under your notes.
Location
AnMass
electron(kg)
is 1,000 times smaller
than a
proton/neutron
and weighs about 10,000 times
-27
x 10 and neutrons
In Nucleus
less!1.67
Protons
are the same size.
1.67 x were
10-27 the size
In Nucleus
If a proton
and mass of a bowling
ball,9.11
thenxthe
electronMoving
would be
compared
to the
10-31
around
outside
size of…. well….. the of
period
on the end of this
Nucleus
sentence.
Chemistry Standard 1e

e. Students know the nucleus of the atom is much smaller
than the atom yet contains most of its mass.

Can the
subatomic
particles change?

ONLY the electrons and neutrons.

An Isotope is an element that has a different
number of NEUTRONS.

What is an
isotope?

What is an ion?

An ION is an element that has had a change in
the number of ELECTRONS
 Positive ions are called CATions.
 Negative ions are called ANions

Can the number
of p+ change?

NO, if you change the proton you change the
element into a different element!
Periodic Table / Atoms (cont)

How do electrons
move around the
nucleus?


Electrons are located in “shells”
Think of a spinning fan…


Only a certain number of e- can occupy
certain shells…



Draw and label
the different
electron shells

When scientists view e-, they see a blurry
cloud instead of a single electron.
Think of a roller coaster…
Only a certain number of people can sit in
the seats. If the seats fill up what happens?
The e- on the outer “shell” are called the
VALENCE ELECTRONS


“valence” means = outside
The VALENCE e-are the e- that bond with
other atoms to form molecules.
The atom
has different energy levels (draw this
The
Atom
under your notes must color!)
32
32
8
2
18
Nucleus
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
2
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
3
2
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
8
2
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
8
2
12
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
8
5
2
18
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
8
8
32
2
18
Pop
quiz hot shot!
Valence
electrons
How many valence electrons are there?
(Pop sticks)
8
2
2
What
happens aselectrons
more electrons are added and the
Valence
“shell/cloud” fills up?
8
10
2
18
Periodic Table / Atoms (cont)

How do we tell
atoms apart?

Based on their properties, we can tell a
lot about an atom.


Atoms have a “fingerprint”
 They show a certain “spectra”; the light
that they give off.
 They also give off a certain color when
burned.
Atoms are arranged in the periodic table
based on the number of PROTONS an atom
has in its nucleus (atomic #).
 Each atom/element has its own “element
card” with specific info about that atom.
 The number of protons and atom has will
NEVER change!


It tells us…
Periodic
Table
/ Atoms
What info
does
 The main families of elements
the Periodic
 The sub-families
of elements
= ATOMIC NUMBER
(the
 Which
Table give
us? of protons
number
an elements have the same properties
atom has.)
It also tells us specific info about each atom..
 Each “element card” tells me about the element.
 The number of protons (atomic number)
The number
of electrons (unless it is an ion).
= ATOMIC
SYMBOL
The number of protons and electrons will be
the SAME, because every atom wants to
have a charge of zero, or neutral.
 Tells me the atomic mass (p + n). I can figure
out the number of neutrons or protons by
subtracting it from the atomic mass (the
bigger number)
= (AVERAGE) ATOMIC
MASS
number
of AND
 DRAW
THIS(The
ELEMENT
SQUARE
LABEL
IT ON
THE LEFT
SIDE in your notes
protons AND neutrons
in the
nucleus
added
ADD COLOR! Should take up ¼ of your
together.)
page.

Periodic Table / Atoms

Every element
wants to be
balanced!




A balanced element will have the same
number of protons (+) AND electrons (-)
All elements in the periodic table are
balanced! Unless otherwise stated.
For the following element cards, give
me the name of the element, the
number of protons (atomic number),
electrons, neutrons and tell me its
total atomic mass.
Unless its an ion, why will the electrons
(-) equal the number of protons (+)?
A Guided Tour of the Periodic Table
a. Students know how to relate the position of an element in the
periodic table to its atomic number and atomic mass.
b. Students know how to use the periodic table to identify
metals, semimetals, non-metals, and halogens.
c. Students know how to use the periodic table to identify alkali
metals, alkaline earth metals and transition metals, trends
in ionization energy, electronegativity, and the relative
sizes of ions and atoms.
This is a new section. (write this on the right hand
side!) You will get a blank periodic table on which
you will color and write notes. Then it will be
TAPED into your notebook. DO NOT LOSE THE
COLORING! HIGHLIGHT/UNDERLINE THE
STANDARDS!
Periodic Table Coloring
Follow directions EXACTLY!
 Don’t Work AHEAD!
 Write the notes with your legend/key on the
BACK of your paper (write small, you will
need the room) Label everything!
 Copy the coloring exactly (outlining, coloring,
labeling…everything!)
 WRITE SMALL!!!!

The Write
Periodic
Table
these on
your chart!
G18
P1
G13
G1
G15
G14
G2
G17
G16
P2
P3
G10
G12
G11
G3 G4 G5 G6 G7 G8 G9
P4
P5
P6
P7
(Ve1) (Ve2)
(Ve6) (Ve8)
(Ve5) (Ve7)
(Ve4)
(Ve3)
The Periodic Table (on right hand side!)
Elements that follow the same patterns from
left to right are organized in horizontal rows or
periods. There are a total of 7 periods. Each
period also represents how many ELECTRON
SHELLS that period has…
 Elements that contain the same PROPERTIES
fall into groups. There are 18 groups of
elements. Think of them as friends that like to
hang out…
 Lanthanide/Actinide (inner transition metals)
are taken out so it is neater.

The Periodic Tabl
If the Lanthanide/Actinide series (inner transition metals) were
included in the table, it would be too wide.
So we take them out and put them on the bottom
The Periodic Table
Metals (outline in red)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= Metals are the largest group. FAMILY
REUNION! About 85 % of all known
elements are metals. Classified as metals
because they are shiny, good conductors of
heat and electricity and are malleable. That
means that they can be bent and shaped
without breaking. Within the metal family we
have 6 main sub families of elements.
The Periodic Table
ALKALI METALS (pink)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= Group 1 = Alkali metals. When you burn
alkali metals and mix their ashes with water it
became slippery. Alkali is an Arabic word that
means slippery. They make many soaps out of
alkali metals. They also make “alkaline”
batteries out of group 1 elements because they
readily lose their electrons.
And 3 things from video
1.
2.
3.
The Periodic Table
ALKALINE EARTH METALS (dark blue, NOT PURPLE!)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= Group 2 = Alkaline EARTH metals. The
second group is called the Alkaline earth
metals. Alkali earth metals share common
characteristics when placed in water with
alkali metals, they become somewhat
slippery, but they cannot burn. Have you
ever tried to light dirt on fire? It doesn’t work.
And 3 things from video
1.
2.
3.
The Periodic Table
TRANSITION METALS (red)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= Transition metals are the largest subfamily of elements. They tend to be harder
than the alkali metals and are used a lot for
structural purposes. Sheet rock, iron, cement
etc…
And 3 things from video
1.
2.
3.
The Periodic Table
Lanthanide (white), actinide METALS (gray)
(INNER TRANSITION)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The inner transition elements
(Lanthanide and Actinide) are taken out of the
graph and placed by themselves. They are all
rare earth metals meaning they occur very
rarely or were created in laboratories.
And 3 things from video (actinide)
1.
2.
3.
And 3 things from video (lanthanide)
1.
2.
3.
The Periodic Table
Other Metals
(light blue)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The 7 “other metals” do not have the
same properties as the transition metals.
They are solid, have a relatively high density
and are opaque (kind of see through).
And 3 things from video
1.
2.
3.
The Periodic Table
NON-METALS
(outline in
green)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The next big family is called the Non
metals. Nonmetals a poor conductors of
electricity and heat and may also be
transparent, meaning you can see through
them.
Non metals have 3 sub families: the noble
gases, halogens, and the “other non-metals”.
Hydrogen
The
Periodic
Table
(yellow)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
(yellow)= Hydrogen is the “lone ranger
element”. Technically a “non-metal” but is
placed by itself. Most abundant element in
the universe.
Three things from video…
1.
2.
3.
The Periodic Table
NOBLE GASES (purple)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The noble gases have a full outer energy
level so they don’t want to bond with
ANYONE. They got their name from the
earlier centuries where the “noble” people
would not associate with the peasants or
lower people. So the noble gases do not
want to associate with the lower class
elements. They are snobs!
Three things from video…
1.
2.
3.
The Periodic Table
HALOGENS (Brown)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The Halogens are “salt-forming”
elements. When mixed with other elements
they tend to form salts. Like our spectra lab
had NaCl (sodium chloride, chlorine is a
halogen and it bonds ionically to form a
“salt”)
Three things from video…
1.
2.
3.
The Periodic Table
OTHER NON-METALS
(green)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The other non-metals have no metallic
luster (not shiny) and do not reflect light, also
poor conductors of heat and electricity. They
exist as either a solid or a gas.
Three things from video…
1.
2.
3.
The Periodic Table
METALLOIDS /
semiconductors (orange)
The periodic Table (on the back of
the paper! Write small, this is your legend/key)
= The metalloids (also called
semiconductors) share properties of both
metals and non-metals, thus they are right in
between them. Semi-conductors are used a
lot in computers/calculators/electronics. The
“silicon” valley.
Three things from video…
1.
2.
3.
A Guided Tour of the Periodic
Table
1.
2.
3.
OBJECTIVES!
How do you find an elements # of valence
electrons?
Describe Ionization energy
Describe what happens to the size of an
atom as you go across the periodic table
and up or down the periodic table.
The Periodic Table
Elements that follow the same patterns from
left to right are organized in horizontal rows or
periods. There are a total of 7 periods.
 Elements that contain the same
PROPERTIES fall into groups. There are 18
groups of elements.
 In this case, as you travel from left to right the
ionization energy increases.
 Ionization energy is the amount of energy
needed to pull an electron away from the
outer shell or VALENCE electrons.

IONIZATION ENERGY INCREASES
The Periodic Table
1
1 2
1 2
1 2
1 2
1 2
As wecan
How
move
we from
easilyleft
figure
to right
the on
the periodic table it gets
valence electrons?
HARDER to pull away electrons.
The energy needed to pull away
electrons is called IONIZATION
ENERGY.
2
3 4 5 6 7 8
3 4 5 6 7 8
3 4 5 6 7 8
3 4 5 6 7 8
3 4 5 6 7 8
Relative sizes of atoms in the Periodic Table…
The Size of Atoms
Right = smaller Down = Larger
A Guided Tour of the Periodic
Table
1.
2.
3.
OBJECTIVES!
Describe an isotope.
Describe the difference between cations
and anions and how they became that way.
Describe the Octet Rule
The Atom
Ions and Isotopes
Nitrogen
An isotope is an element with
a different number of
NEUTRONS. YOU CANNOT
ADD OR TAKE AWAY
PROTONS
An ION is an element with a
charge, like a magnet. It loses
or gains electrons to become
positive or negatively
charged.
gain e- = negative (ANIONS)
lose e- = positive (CATIONS)
IONS! WRITE THIS SMALL!
1+,C
0
4+/4-2-=A
3+=C 3-=A 1-=A
2+=C
Valence electrons come from the
groups that each element is in.
Atoms form IONS when they
lose or gain electrons.
POSTIVE ions are CATIONS
NEGATIVE ions are anions.
4+ or 4- =polyatomic ion
2+
+ +
If I have 2 protons (+) and no
electrons, what is my “charge”?
Think of it like a magnet, if I have
MORE positives, do I have a positive
or negative charge overall?
0
2-
--
How many electrons (-) would I need
to BALANCE or have a charge of
zero?
------
+ + + +
What is my overall charge?
Did I ever change the +’s?
NO!
POSITIVES (PROTONS) CAN’T
CHANGE!
YOU JUST CREATED AN ION!!
Lithium
+ + +
Here I have 3 protons, which element
is this?
Can the number of protons change?
Charge = 0
+1
--
So,
lithiumelectrons
has one (-),
extra
friend,
Howifmany
does
lithium
how
many friends does it want to get
have?
rid of?
Is it balanced? What is its OVERALL
So
if I get rid of one friend, what is my
“charge”?
OVERALL charge?
How many electrons are in Lithium’s
FIRST shell?
How many VALANCE electrons does
lithium have?
+ + +
-Charge=
+
0
1
IONS!

What is the Octet
rule?




“oct” means eight, how many things can
you think of that have the word “oct” in
them that mean 8?
Every element wants to have 8 electrons
in their outer shell, thus being full.
When elements bond, they bond until
they have eight electrons to become full.
For example, water (H2O)
Why would helium be an exception?
Beryllium (Be)
If every atom wants to be full, would Be rather
gain or lose electrons?
Beryllium’s charge
is?
If I take away
electrons, what
+
+
does its charge
+
+
become?
2+
So it becomes
-
-
Be 2+
-
-
Sodium (Na)
Sodium’s charge
is?
If I take away
electrons, what
does its charge
become?
1+
So it becomes
Na 1+
-
-
-
+
+
+
+
+
+
+
+
+
+
+
-
Oxygen (O)
Oxygen’s charge
is?
If I ADD electrons,
what does its
charge become?
2So it becomes
O 2-
-
-
-
+
+
+
+
+
+
+
+
-
IONS!

What are the
different types of
ions?







Elements lose or gain electrons to
become ions
CATions are POSITIVE (+) ions
ANions are NEGATIVE (-) ions
How do you remember that?
I lost my CAT but it was a POSITIVE
thing because I got a dog.
I lost (electrons) my CAT (CATion) but it
was a POSITIVE (CATions are positively
charged) thing, because I got a dog.
METALS tend to become + and
NONMETALS tend to become -
Special Assignment
On (FULL) sheet of paper, you are going to
create for me a comic strip.
It must have 6 scenes, showing how you lost your
cat.
It must have 3 aspects
1. Title
2. Color
3. Paragraph explaining how your cartoon
relates or explains how atoms LOST electrons
to become CATions.
Title:

Go to Chemical Bond power point…
Chemistry Standard 1e





a. Students know how to relate the position of an element in the
periodic table to its atomic number and atomic mass.
b. Students know how to use the periodic table to identify
metals, semimetals, non-metals, and halogens.
c. Students know how to use the periodic table to identify alkali
metals, alkaline earth metals and transition metals, trends in
ionization energy, electronegativity, and the relative sizes of
ions and atoms.
d. Students know how to use the periodic table to determine the
number of electrons available for bonding.
e. Students know the nucleus of the atom is much smaller than
the atom yet contains most of its mass.