the atom and the periodic table from
TRANSCRIPT
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The Atom and the Periodic Table
From http://pvphysicalscience.weebly.com/notes-and-handouts.html
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Atoms
Everything in the Universe is made of stuff (also known as matter).
The building blocks are the same, whether we are looking at Stars or Starbursts. http://www.jakehowlett.com/tuckshop/wrappers/sweets/fruits/starburst.jpg
http://library.thinkquest.org/12659/media/solar_system/sun/sun.jpg
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Atoms
Matter is made up of Atoms. Atoms are the smallest particle of an
element. They are so small that:
1 sheet of paper = 10,000 atoms thick 1 drop of water has 2 trillion atoms of oxygen
and 4 trillion atoms of hydrogen. The three parts of an atom are:
Protons Neutrons Electrons
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Atoms – Protons
There are three types of particles that make up atoms
The first type of particle is called the PROTON.
Protons are found in the nucleus of an atom.
Protons have a positive (+) charge. Protons have a mass of 1 a.m.u.
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Atoms - Neutrons
Another particle is the NEUTRON. Neutrons are also found in the nucleus
of an atom. Neutrons have no charge. We call this
neutral. Neutrons have a mass of 1 a.m.u. Neutrons act like the glue that holds
the nucleus together.
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Atoms - Electrons
Electrons are the third type of particle inside of an atom.
They are very small, and exist outside of the nucleus in the electrons clouds or shells.
Electrons have a negative charge (-) and have almost no mass at all.
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Atomic Structure
Atoms are made up of three subatomic particles:
Subatomic = smaller than an
atom
Live where?
Have mass?
What charge?
Protons
Neutrons
Electrons
In nucleus
In nucleus
Outside nucleus
1 a.m.u
1 a.m.u
No, negligible
+
-
none
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Atomic Structure Video
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Elements
Substances made of only one type of atom
Identified by atomic number (protons!!!)
Can not be broken down into simpler substances
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Element Symbols
Shorthand name of the element Most are based on the Latin name
Ex: Gold = Au The symbol is either:
1. One capital letter-ex: Carbon = C
2. Two letters…one capitol, one lower case-ex: Krypton = Kr
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Atomic Number Top Number indicates Atomic
Number Atomic Number = Number of
Protons Hydrogen:
Atomic Number 1 = 1 proton Magnesium:
Atomic Number 12 = 12 protons Lead:
Atomic Number 82 = 82 Protons
IF YOU CHANGE THE NUMBER OF PROTONS OF AN ATOM, YOU CHANGE ITS IDENTITY!!!!!!!!
1
H12
Mg82
Pb
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Atomic Mass Bottom Number indicates Atomic Mass Atomic Mass = Total Mass (Number of Protons +
Number of Neutrons) Hydrogen:
1 (Protons + Neutrons) Magnesium:
24 (Protons + Neutrons) Lead:
207 (Protons + Neutrons) If we take the Atomic Mass and subtract the Atomic
Number, we can figure out the number of neutrons. Pb –
(Atomic Mass) 207 – (Atomic Number) 82 = 125
H1
Mg24
Pb207
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Atomic Structure (cont.)
Atomic Mass Average mass of an element,
based on amount of each isotope found in nature
Not a whole number because it is an average
Atomic number Number of protons in an
element Also, number of electrons
when it is neutral (has no charge)
7
N14.011
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Atomic Structure (cont.) For a lithium (Li)
atom: What is the atomic
number? How many protons? How many electrons
since it is neutral? What is the atomic
mass? How many
neutrons?
3
3
3
6.941 rounded to 7
Usually 4
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Atomic Structure (cont.)
Practice Problem #1
For a sodium atom: What is the atomic
number? How many protons? How many electrons
since it is neutral?
What is the atomic weight? How many neutrons?
11
11
11
22.99 rounded to 23Usually 12
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Atomic Structure (cont.)
Practice Problem #2
For a boron atom: What is the atomic
number? How many protons? How many electrons
since it is neutral?
What is the atomic weight? How many neutrons?
5
5
5
10.81 rounded to 11
Often 6
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Atomic Structure (cont.)Helium
Atomic Number: 2
Protons: 2
Electrons: 2
Atomic Mass: 4.003
Atomic Mass rounded to: 4
Neutrons: 2
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Isotopes
Is an atom of a given element that has different numbers of neutrons and a different mass number. It has gained or lost neutrons Examples: Carbon—12
Carbon—14 Mass
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Carbon-12
#p+ 6
#e- 6
#n0 6
Mass 12
Carbon-14
#p+ 6
#e- 6
#n0 8
Mass 14
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Radioisotopes
Is an isotope with an unstable nucleus Examples: uranium, Plutonium Isotopes of all elements above #83 are
radioactive producing radioisotopes
Ex. U-238 is naturally occuring
U-235 is a radioisotope
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Writing Isotope Symbols
Hyphen Notation- is the element symbol with the atomic mass hyphenated.
Example C-12 and C-14
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Writing Isotope Symbols continued
Atomic Symbol Notation:
Atomic Mass
Atomic # =
# protons
Chemical Symbol
of Element
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The Periodic Table
Organized by trends and patterns “periodic” means
repeating This allows you to
make predictions about the atoms’ behavior based on where they are on the table
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Periods The elements are arranged on the periodic table of
elements Going horizontal across the table are the PERIODS
(Left to right)
Period # = # of valence shells Starting from the left, the periods go from metals
metalloids nonmetals
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Periodic Table - History
Dimitry Mendeleev was a Russian (actually Siberian) scientist that lived in the late 19th Century.
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Periodic Table - History
When Mendeleev arranged them by Atomic Mass, he was able to predict the properties of elements that had not yet been discovered.
This is the basis of the Periodic Table that we use today.
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Periodic Table - History
Now the Periodic Table that we use is arranged by Atomic Number instead of Mass.
Henry Moseley reordered the
Periodic Table by Atomic Number
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Groups and Families
The columns on the periodic table are called groups and families.
The groups are the numbers; the families are the names
They are organized by the number of valence electrons
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Metals
Lose electrons to form positive ions
Ductile & Malleable What do these
words mean? Good conductors of
heat and electricity MOST are solid at
room temperature
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Nonmetals
Gain electrons to form negative ions
Brittle Good insulators Found as solid,
liquid, or gas at room temp
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Metalloids (semi-metals)
Found directly on either side of side-step line Except Al (this is a
metal!!!) Properties of both
metals and nonmetals Less conductive than
metals, but poorer insulators than nonmetals
Electrons held more tightly than metals, but can be freed with heat
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Alkali Metals
Group 1A Only one
valence electron VERY reactive!!!! Hydrogen is
NOT included +1 charge
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Alkaline Earth Metals
Group 2A Two valence electrons Not as reactive as the alkali metals Named because of where they are
found on Earth +2 charge
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Transition Metals
Found in the middle of the table
In the “B Groups” Can change their
number of valence electrons
Bottom Rows are also known as the Rare Earth Metals!!!
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Halogens
Group 7A Seven valence
electrons VERY reactive!!!! They react with
alkali metals to form salts
-1 charge
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Noble Gases
Group 8A 8 valence electrons
—outer energy level is full
Very UNREACTIVE—what do they need to be
0 charge
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+1
-3+3+4
-4+2-2 -1
0
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Electron Clouds
The different layers of clouds hold different numbers of electrons 1st cloud = 2 2nd cloud = 8 3rd cloud = 8
These cloud layers conveniently match the rows on the periodic
table:1st row = 2 elements2nd row = 8 elements
3rd row =8 elements…And then it gets complicated
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Electron Clouds (cont.)
To draw the electron clouds: Figure out how many total electrons Fill in the electrons starting with the first
cloud Sulfur has:
16 electrons
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Electron Clouds (cont.)
Practice Problem Draw the electron clouds for an Al atom
This is WAY too much
work…there must be a
simpler way!
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Lewis Dot Structures
A smart man named Gilbert Newton Lewis figured out an easier way!
For Lewis Dot Structures draw only the important electrons…are called the outer, or valence, electrons
Just draw the outer electronsaround the atomic symbol
S
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Lewis Dot Structures (cont.)
Practice Problem #4 Draw Lewis Dot Structures for:
A Calcium atom
A Chlorine atom
An Oxygen atom
Ca
O
Cl
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Octet Rule
Noble gases are what all elements aspire to be like electronically
These elements have 8 electrons in highest energy level
8 is GREAT
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Lewis Dot Structures (cont.)
All elements want to be full of electrons: So they gain or lose electrons until they
are full This gives the atom a charge
Negative charge if they gain electrons Positive charge if they lose electronsCharged atoms are called
ions: cations if they are positive and anions if they
are negative
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Atomic Number Continued Also equal to number of electrons if the
atom has no charge If the Element has a positive charge
Take the atomic number and Subtract the charge to find # of electrons K
(Atomic Number) 19 - (Charge) 1 = 18 Electrons
Ca ?
If the element has a negative charge Take the atomic number and Add the
charge to find the number of electrons Cl
17 + 1 = 18 Electrons
+1
K
+2
Ca
-1
Cl
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Ions How many valence electrons in Li?
Is it easier to gain or lose to become full?
How many will it gain or lose?
What charge will it become?
1
lose
1
+1
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Ions How many valence electrons in O?
Is it easier to gain or lose to become full?
How many will it gain or lose?
What charge will it become?
6
gain
2
-2
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Ions
Magnesium-24
+2
Sulfur-33 -2
Phosphorus-34
-3
Name Symbol Atomic # Mass # Protons Neutrons Electrons Charge
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Atomic Tables
Rules Name
Comes from Periodic Table WITH Mass Number
Symbol Comes from Periodic Table
Atomic Number Top Number, Same as number of Protons
Mass Number Equal to Number of Protons + Number of Neutrons (Usually Bottom Number of Periodic Table Rounded)
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Atomic Tables Continued
Protons Equal to Atomic Number (Top)
Neutrons = Mass Number – Number of Protons
Electrons If No Charge
Equal to Number of Protons If Has a Positive Charge
Subtract Charge from Number of Protons If Has a Negative Charge
Add Charge to Number of Protons
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Practice ProblemsName Symbol Atomic
NumberMass
NumberProtons Neutrons Electrons Charge
10 0
30 26 0
Na 23 +1
16 16 -2
Nitrogen-15 10
Neon-20 Ne
12
26 56 26
10 20 10 10
18
FeIron-56
Sodium-23 11 11 10
Sulfur-32 S 32 16
7N 15 7 8 -3