created by Mr. Nuetzel, 12/2012
sciencenuetzel@gmail.com
Physical Science Core Standard
Describe how atomic structures determine chemical
properties and how atoms and molecules interact.
Periodic Table Shortcuts
 The period is the horizontal row that also tells how
many energy levels the atom has.
 The group is the vertical column that also tells how
many valence electrons there are.
 The charge of an ion can be found by seeing how many
columns it is from Group 8.
 (Group 1 = +1, Group 5 = -3, etc.)
Vocabulary Terms

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Element
Atom
Compound
Molecule
Nucleus
Proton
Neutron
Electron
 Group
 Valence Electrons
 Reactivity or Chemical Properties
 Period
 Energy Levels
 Charge
 Positive

 Mass Number
 Isotope
 Atomic Number
 Element Symbol
 Subscript
Loose Electrons = Positive
 Negative
 Gain Electrons = NEGATIVE
 Ion (positive or negative)
 Bond
 Ionic
 Covalent
Names for Matter
 An element is a pure substance, meaning it is made
up on only one type of atom.
 Gold, Copper, aluminum, etc.
 A compound is a mixture of multiple elements
 Carbon Dioxide, Water (H2O), etc.
 A molecule is a group of multiple elements and can
either be pure, or made up of multiple elements.
 An atom is the smallest ‘complete’ particle of one type
of element
 All matter is made up of different combinations of
elements and compounds.
 There are about 100 or so atoms which make up all of
the natural world, but a few are much more common
than others.
 We could actually create a lot more elements if we
wanted, but they are not normally stable (or useful).
Subatomic Particles
 All atoms are composed of three subatomic particles:
 Protons

Positive charge, found in the nucleus
 Neutrons

Neutral charge, found in the nucleus
 Electrons

Negative charge, found in electron cloud
Atomic Pictures
Atomic Pictures
Scale and Structure
Location
 Protons and neutrons are located in the center, densely
packed together.
 Penny on second base of Baseball diamond
 Electrons orbit the nucleus in different energy levels in
the electron cloud.
 Flying around the outside of the stadium
Scale and Structure
Mass
 Protons and neutrons are very similar and size
 Electrons are much, much smaller than the others
particles
 Fly vs. Garbage Truck
Writing Elements
M
A
C
R
R = Chemical Symbol
M = Mass Number
A = Atomic Number
C = Charge
Isotopes
 NOT all atoms in an element are EXACTLY
the same.
GENERAL RULES
 Protons determine the IDENTITY of an
atom
 Neutrons determine the ISOTOPE.
 Electrons determine the CHARGE
Elements and Numbers
 Atomic Number
 This tells the number of Protons in an atom
 This is also the basic number of Electrons in an atom

Atoms do not gain or lose protons, but ONLY electrons. When this
happens the charge on the atom will change. If an atom were to lose
a proton it would become a different type of atom
 Mass Number
 This tells the number of Neutrons + Protons in an isotope
Isotopes
12
6
C
13
6
C
14
6
C
Charges
 a Proton = +1 charge
 a Neutron = 0 charge
 an Electron = -1 charge
 When an atom gains electrons
 It becomes MORE negatively charged
 When an atom loses electrons
 It becomes MORE positively charged
 When an atom is a different Isotope
 It doesn’t affect the charge
The Periodic Table
of Elements
Periodic – appearing or occurring at intervals
 The number of outer electrons
equals the group.
 The number of energy levels equals
the period.
 Group = Vertical Column
 Period = Horizontal Row
Periodic Table Shortcuts
 The period is the horizontal row that also tells how
many energy levels the atom has.
 The group is the vertical column that also tells how
many valence electrons there are.
 The charge of an ion can be found by seeing how many
columns it is from Group 8.
 (Group 1 = +1, Group 5 = -3, etc.)
Group 5, Period 3
Group 5, Period 3
Group 5, Period 3
Group 5, Period 3
Group 5, Period 3
Period 5, Group 8
Period 5, Group 8
Period 5, Group 8
Period 5, Group 8
Period 5, Group 8
Periodic Table Shortcuts
 The period is the horizontal row that also tells how
many energy levels the atom has.
 The group is the vertical column that also tells how
many valence electrons there are.
 The charge of an ion can be found by seeing how many
columns it is from Group 8.
 (Group 1 = +1, Group 5 = -3, etc.)
Essential Questions
from Atomic Structure Notes
 #1 - What is the relationship between an atom and an
element?
 #2 - How are protons and neutrons different from and
similar to each other?
 #3 - How do electrons differ from both protons and
neutrons?
 #4 - How are protons, neutrons, and electrons
arranged to form an atom?
EQ#1 - What is the relationship
between an atom and an element?
 An element is a pure substance made up of one type of
matter or one kind of atom. The atom is the smallest
possible complete or ‘unique’ piece of matter. When
you completely break that pure compound element
into smaller pieces they are not specific to one type of
substance. For example, 2 protons, 2 neutrons, and 2
electrons is helium, but if you break that in half you
get a different atom, hydrogen (with an extra neutron)
which isn’t easily broken apart without large sums of
energy.

EQ#2 - How are protons and neutrons
different from and similar to each other?
 Protons and neutrons are both located inside of the
nucleus and they both have equal one atomic mass
unit. They are different because they have different
charges, the proton being positively charged, and the
neutron being negatively charged. The number of
protons determines the identity of the atom, but the
number of neutrons determines which isotope of a
certain element it is.
EQ#3 - How do electrons differ
from both protons and neutrons?

The electron is much smaller in mass than either a
proton or neutron. It is located in a different place
within the atom, and it has a negative charge, unlike
the other sub-atomic particles. The electrons do not
determine the type of atom, but they do have an effect
on the properties of an element. Elements with the
same number of valance electrons generally bond like
each other.
EQ#4 - How are protons, neutrons, and
electrons arranged to form an atom?

The protons and neutrons are located in the
nucleus, the very dense center of the atom. Almost all
of the mass of the atom is located in this small center.
On the outside, in different energy levels electrons
speed around the atom, pulled near by the electrostatic force between positive and negative charges.
The electrons orbit at a relatively far distance within
the atom. Most of the atom is empty space.
Element Families
 Noble Gases
 Do Not React With Others
 Happy / Stable = Full Outer Energy Level!
 Alkali Metals
 Hoping to lose 1 electron
 Halogens
 Greedy for electrons
Glencoe Ch. 6 Vocab and Terms
Section 1
 Neutral
 Electron Cloud
 Energy Levels
 2, 8, 8…
 Groups
 Electron Dot Diagram
 Valence Electrons (8*)
 Chemical Bond
Section 2
 Ions
 Ionic Bonds
 Compound
 Covalent Bond
 Molecule
 Polar Bond
 Uneven Sharing
 Chemical Formulas
Glencoe Science Ch. 6 Summary
The protons determines the type of element, while
the electrons determine the reactivity of the element. If
the protons and electrons are the same, it is neutral. All
atoms would rather be stable, with 8* valence electrons as
shown in Electron Dot Diagrams. Elements with the same
number of valence electrons form the families on the
periodic table.
Ionic bonding involves gaining / losing electrons
forming compounds between metals and nonmetals.
Covalent bonding involves sharing electrons between
nonmetals forming molecules, which are either polar or
non-polar. In a polar bond, one atom pulls more on the
electron, giving it have positive and negative “pole”. Nonpolar bonds equally shared electrons and are symmetrical.
Counting Atoms in Formulas
 Subscript = this tells the number of each atom in a
compound. If there is no subscript we know that it is
one atom.
H2O
 Parenthesis + Subscripts = sometimes there will be a
parenthesis with a subscript after it. This means that
you need to multiply all of the atoms in the
parenthesis by the subscript outside of the parenthsis.
Fe3(PO4)2
* Superscript – shows the charge on an ion
Chemical Formulas
Symbols = the type of atom
Subscripts = the number of each atom
Sodium Chloride - NaCl
Methane - CH4
Ibuprofen – C3H8O2C10H10
Chemical Formulas
Symbols = the type of atom
Subscripts = the number of each atom
Plavix (heart medication) – C4H12ClC4NC4O2SC4H4
Thymaine - C5H4N2(OH)2
Ionic Bonding
We know that opposites attract, so oppositely
charged ions will join together to form
compounds.
Ionic Bonding occurs between Metals and
Non-metals
Ions
 Electrons have negative charges. Protons have positive
charges. An atom has no net charge while the protons
and electrons are equal.
 To form an ion, an element will gain or lose electrons
until it has a complete outer energy level (HAPPY)
 An element would rather be happy than neutral.
 Gain electrons = net negative charge.
 Lose electrons = net positive charge.
Compounds – opposites attract!
 Positive Ions will attract Negative Ions.
 A +1 ion will equally bond with a -1 ion.
 A +2 ion will equally bond with a -2 ion.
 What about when a +2 ion encounters a -1 ion?
Making Compounds = Making Elements Happy
Compound
E-Harmony
1. Draw EDD’s
2. Figure out the Charge that the 2 Ions will make.
3. Multiply the + ions and – ions until they cancel.
4. Write the formula with the correct subscripts.
Na +
Cl

Ionic Bonding Practice
Be +
O

Be +
Cl

Periodic Table Shortcuts
Table
Group #
1
2
3
4
5
6
7
8
Valence
1
Electrons
2
3
4
5
6
7
8
Ion
+1 +2
Formed
+4
+3
-3 -2 -1 Na
-4
More Ionic Bonding Practice

Na +
P
Al +
Se 
Periodic Table Shortcuts
 The period is the horizontal row that also tells how
many energy levels the atom has.
 The group is the vertical column that also tells how
many valence electrons there are.
 The charge of an ion can be found by seeing how many
columns it is from Group 8.
 (Group 1 = +1, Group 5 = -3, etc.)
You should also be able to fill out a table like this,
with your Periodic Table…
#
Element
Symbol
2
2
Atomic
Mass # Group Period
#
# of
Protons
# of
Neutrons
# of
Electrons
18
22
18
Valence Energy Electrons in Charge
Electrons Levels
Ion
on Ion
18
Argon
Ar
18
39.95
8
3
8
3
18
0