Crazy Clue-What Element am I?
What do dogs do with their bones?
Storage space for cars
Half of a dime.
Lone Ranger’s Horse
Male member of the Ganese tribe
A prison inmate that does stand up comedy.
Superman’s weakness
What do you do to your clothes when they are
winkled?
9. What do you do to your clothes when they are
ripped?
10. If someone ate all the cookies on your plate, you
would cry, “They _______.”
1.
2.
3.
4.
5.
6.
7.
8.
Unit: Atomic Theory and
Structure
Elements-

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

Pure substances that are all made of the
same type of atom
Represented by chemical symbol
Most are solids at Room Temp.
Earth’s crust made of 92 naturally
occurring elements
Building blocks of matter
John Dalton’s Recommended Chemical
Symbols
Alum molecule
How symbols were determined:



1. Use first letter of Name of element
2. Where conflicts, First letter plus one
additional letter (only capitalize first letter)
3. Still conflicts, select symbol from Latin
Name
Elements with Latin Chemical Symbols
Element
Latin Name
Symbol
Gold
Tungsten
Aurum
Wolfram
Au
W
Silver
Lead
Potassium
Tin
Argentum
Plumbum
Kalium
Stannum
Ag
Pb
K
Sn
Sodium
Copper
Mercury
Natrium
Cuprum
Hydragyrum
Na
Cu
Hg
W = wolfram (tungsten)
Cu = cuprum (copper)
Au = aurum (gold)
Fe = ferrum (iron)
Pb = plumbum (lead)
Hg = hydragyrum (mercury)
K = kalium (potassium)
Ag = argentum (silver)
Na = natrium (sodium)
Sn = stannum (tin)
Sb = stibium (antimony)
Atom


Smallest piece of matter that still has the
properties of the element
All elements made of atoms
Atomic Structure



Protons - (p+)
Positive charge
Found in nucleus
Mass of 1 amu
amu

(atomic mass unit)** Unit of measurement
for atomic particles which is 1/12th the
mass of a carbon atom containing 6 protons
and 6 neutrons
Neutrons – (no)



No charge
Found in nucleus
Mass of 1 amu
Electrons – (e-)
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
Negative charge
Surround the nucleus,
electron cloud
No significant mass
“Sub-Subatomic Particles”:


Quarks – smaller
particles that make
up protons and
neutrons
Leptons – smaller
particles that make
up electrons
Atomic Number



The number of protons in an
atom
Number of protons also
identifies the element
Whole number on Periodic
table

Atomic
#10?
 Neon
No 2 elements have the same Atomic #9 ?
atomic number
 Fluorine
Number of electrons?
If the atom is neutral:
Positives = negatives
# of protons = # of electrons
Atomic # = # of electrons
How many Protons and electrons?

Carbon?

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Sodium?
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6 protons, 6 electrons
11 protons, 11 electrons
Iron?

26 protons, 26 electrons
Mass Number

What has mass in atom?
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Protons and neutrons
the sum of the number of protons and
neutrons in an atom
# neutrons = Mass # - Atomic # (protons)
Is a whole number for that atom.
How many p+, n0, e-?

Lithium –7?
 3 p, 4 n, 3 e

Aluminum –27?
 13 p, 14 n, 13 e
 40K?
 19 p, 21 n, 19 e
 80Br?
 35 p, 45 n, 35 e
Isotopes


Atoms of the same element with different
numbers of neutrons
Same atomic # but different mass #
3
isotopes of Hydrogen
Protium
Deuterium
Tritium
Isotopes:

Different Isotopes have
different properties

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Carbon – 12
Carbon – 14
Some are
unstable/radioactive
Use for Radioactive Isotopes:

Radioactive Dating

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Such as Carbon-14 dating
Tracers in Medicine I-123 (thyroid
imaging)
Radiation Therapy for Cancer
Irradiation of foodCobalt-60
Smoke Detectors Americium-241
Ions


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Charged atom
Different number of
protons and electrons
No longer neutral
Average atomic mass
On periodic table
 The weighted average mass
of an element’s isotopes
 Using Hydrogen
Is closest to the element’s most abundant
isotope’s mass number
(if you round the number)
Ex. Lithium – 6.941
 Lithium – 7 is most abundant
Electron Energy Levels / Orbits

each of the 7 energy level can hold a
maximum number of electrons
Energy
Level
1
2
3
4
Max. # of
Electrons
2
8
18
18
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Each energy level is a
different distance from the
nucleus
Atoms only have the
number of energy levels
that are needed for its
electrons
Levels closest to the
nucleus have lower
amounts of energy
Rules for filling energy levels
(atomic # 1-18) – Think of Stadium Seating!!

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1. electrons are
placed in lowest level
first
2. when level 1 is full
then use level 2
3. fill each shell to
capacity until you get
to 3rd level (then these
rules don’t apply)
Drawing Bohr Models
Oxygen
Sodium
Neon
Dmitri Mendeleev
Late 1800 devised the 1st periodic
table


Based on elements atomic
mass number
at the time only about 63
known elements


left spaces in table for
elements yet to be discovered
There were some problems
with his table
By arranging the elements in order of increasing atomic weight he
discovered that there existed a periodicity of the elemental
properties. He used this periodicity to create a table in which that
elements with similar properties were vertically aligned with each
other.
In making such alignments Mendeleev was able to determine that
several, as yet unidentified, elements should exist (the elements
with masses 44, 68 and 72 are examples). He went on to make
predictions about the properties of these missing elements which
aided in their discovery. The discovery of scandium (44), gallium
(68) and germanium (72) and examination of their properities
(which were very similar to those predicted by Mendeleev)
provided evidence for the validity of the periodic table.

Henry Moseley (1913) arranged elements
by atomic number rather than atomic mass
Modern Table – by increasing atomic #

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Vertical Columns 
“groups or families”
18 groups
Have similar properties
Elements have the same
number of electrons in
outer energy level
Calledvalence electron #
Horizontal Rows 
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“periods or series”
- 7 periods
- don’t share similar properties
- all elements in the same period have the
same number of electron energy levels
Electron Configurations:


1.Within energy
levels are orbitals or
smaller mini orbits
“s”  Spherically
shaped (2 e-)
“p”  dumbbell shaped (6 e-)
“d” double dumbbell (10 e-)
“f”  complex (14 e-)
Each orbital has a certain number of sub-orbitals that can
each hold up to 2 electrons (that spin opposite each other)

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-Rules for filling sub-orbitals:
1. - “s” ALWAYS fills first in any energy level
2. - If it has a “p” then fills after the “s”
3. If it has a “d” orbital, it is always skipped in favor of
the next levels “s”
4. -Then after “s” is filled, go back to the “d” one energy
level lower
6
10
2
6
2
6
2
2
The Periodic Table
Contains all the known elements