atomic theory review. where did the elements come from? hydrogen, a little helium and less lithium...
TRANSCRIPT
ATOMIC THEORY REVIEW
Where did the elements come from?
Hydrogen, a little helium and less lithium were created in the big bang. The universe is about 95% hydrogen. Clouds of hydrogen gas and dust are compressed by gravity into stars. When the star's core runs out of hydrogen, the nuclear reaction pauses, and gravity compresses the star, heating it up enough to fuse helium.
Where did the elements come from?
If the star is big enough, like a supernova, it can eventually create all the elements in the periodic table up to iron. If a giant star explodes as a supernova, it will releases enough energy to make all the elements heavier than iron. So stars created the first elements!
The most common Elements in the Earth’s CRUST
Element AmountOxygen 46.1 %
Silicon 28.2 %
Aluminum 8.23 %
Iron 5.63 %
Calcium 4.15 %
The most common Elements in the Earth’s OCEANS
Element AmountOxygen 85.84 %
Hydrogen 10.82 %
Chlorine 1.94 %
Sodium 1.08 %
Magnesium 0.1292 %
The most common Elements in the Earth’s ATMOSPHERE
Element AmountNitrogen 78.1 %
Oxygen 20.9 %
Argon 0.96 %
ATOMS !!! What are the 3 subatomic particles?
ProtonsNeutronsElectrons
What is ALL matter made of?
Subatomic Particle Charges
protons (+)positive
neutrons (0)neutral
electrons (-)negative
We know that there are the same number of p+ and e- in atoms on the Periodic Table… So What is the overall charge of any atom?
The overall charge of any atom is
NEUTRAL… the positive charge cancels out the negative charge = 0!!!
What are the masses (amu) of the subatomic particles?
p+ = 1amu
n = 1amue- = 0 amu
1.66 x 10-27 kg = 1 amu
What is this AMU stuff?????
Atomic mass unit (AMU)
2.2 lbs= 1 kg
What are the two areas of an atom?
Nucleus and electron cloud
P+ & No
e-
Where are the p+, n, and e- located in an atom?
p+ in the nucleus
no in the nucleus
e- in the electron cloud
NucleusWhere is ALL the mass in an atom located?
Where is most of the volume of an atom located?
Electron Cloud
The nucleus contains the p+ and n… while the electrons “orbit” the nucleus in the energy rings of the e- cloud.
What does a Bohr model of the atom look like?
So what are the charges of the different areas?
1. So what is the overall charge of the nucleus?
Positive
2. So what is the overall charge of the electron cloud?
Negative
(opposite charges attract)
QUICK REVIEW- ATOMSSub-atomic particles:.
particles charge amu location abbrev.
Protons
Electrons
e-
Neutral (0)
+ p+nucleus
0
1
1
neutrons
Electron
cloud_
nucleus
no
protons, neutrons, and electronsnucleus and electron cloudParts of the atom:
Energy Levels of the Atom
8 e- 2e- 32e-
8 e-
18 e-
18 e- 32e-
The Nucleus
P+ N0
1st
shell7th
shell2nd
shell3rd
shell4th
shell5th
shell6th
shell
Atoms can have several energy levels. Sometimes they are also called energy rings, shells or orbits.
Lets take a look at the Periodic Table!The periods equal the number of energy shells or rings in an atom.
Beginning with Bohr Models Let’s try a few easy bohr models:
Li
Be
Bohr Model Practice
1. Ca2. O3. Ne4. K5. Rb
6. P7. F8. Cl9. Br10. I
More Bohr Model Practice11. Fr 12. Te13. Sn
14. Cs15. Kr
16. At 17. Ga18. Rn19. Ag20. W
Cs Fr Sn Te Kr At Ga Rn W Ag
Bohr Model
H vs. He
Explain why we use helium filled balloons instead hydrogen filled balloons at Parties.
Hydrogen is unstable and flammable and helium is stable!
Energy rings are not filled
Energy rings are filled
Draw the bohr models for the following atoms.
Burning Hindenburg
Complete the Bohr Models for the following elements. Ne, Ar, Kr and Xe
What 4 patterns or trends did you notice they have in common?
“Predict” what you think Radon’s (Rn) bohr model would look like.
Six rings Full shell More massive
All of the rings or shell are full.
They are all in the same group (18)
They gain an energy ring as you go down a period.
They gain more subatomic particles as you go down.
Patterns from the Bohr Models.
Ne Ar Kr Xe
Radon Bohr Model
Even More Bohr Model Practice!
21. Os 22. Hf23. Cm
24. Sr25. Ho
26. Tc27. Ac28. Zr29. Po30. Np
“Life on the Edge” with Valence Electrons
Valence electrons are electrons in the outermost shell of an atom.
They determine whether the atom will bond with another atom.
How many valence electrons does lithium have here?
1 valence electronCircle the valence electronsFrom your warm up.
Valence electrons are electrons in the outermost shell of an atom.
They determine whether the atom will bond with another atom.
How many valence electrons does lithium have here?
1 valence electronCircle the valence electronsFrom your warm up.
Arrangement of the Periodic Table
1. What atom is this?
Oxygen2. Which subatomic “particle” helped
you to determine that this Bohr model was of oxygen?
Protons
Arrangement of the Periodic Table1. The periodic table is arranged according to
what?A. Atomic SymbolB. Atomic massC. Atomic numberD. Number of Energy Shells Do the elements on the periodic table all
increase according to their masses?
No!! Can you find where they are not? There are a few of them. Look carefully!
Periodic Table Card Sort Poster
Breaking the CodePurpose: This lesson will help you identify
many of the patterns that are contained in the periodic table of elements.Use the card sort poster to answer the following questions on your paper.
Do you notice any patterns hereas the elements move to the right?
Li Na K Rb
Can you “predict” how many energy rings a bohr model of Francium (Fr) would have?
Gaining more mass
Gaining more energy rings
Gaining more p+, no, and e-.
Francium (Fr) Bohr Model
Seven energy rings
1 valence electro
n
What Bohr model patterns are you starting to see develop? Periodic Table Patterns
The atomic number is the same number as the number of protons and electrons.
Atoms get larger as you move down and two the right on the periodic table.
As you move from left to right on the periodic table, you gain protons and electrons and neutrons.
As you go down from the periodic table, the atom gains another energy shell or orbit.
Element Atomic Number
Atomic Mass
# of Protons
# of Electrons
# of Neutrons
Zn 30 65
Xe 54 77
Au 79 118
Hg 80 121
I 127 53
30
54
197
8020180
79
54131
30 35
305353
79
Manganese
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 7
Yttrium
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 18
Fifth Energy Level: 3
P39N50
2e 8e 8e 18e 3e
P25N30
2e 8e 8e 7e
Yttrium Manganese
Krypton
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 18
Germanium
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 8
Fourth Energy Level: 14
Krypton Germanium
P36N48
2e 8e 8e 18e
P39N50
2e 8e 8e 14e
Metals vs. Non-Metals
Metals
Non-metals
Man made elements and Rare Earth metals
Stair steps
Metalloids on the Periodic Table
FA
MIL
IES
/ G
RO
UP
S
Periods/ Rows
Metalloids
Properties of Metals
Most elements are metals. 88 elements to the left of the stairstep line are metals or metal-like elements.
Tend to have Luster High density Ductile Malleable
(shininess) (heavy for their size)
(most metals can be made into thin wires)(most metals can be hammered into
thin sheets)
Properties of Non-metals
Nonmetals are found to the right of the stairstep line.
No luster Brittle Not ductile Not malleable
(dull) (breaks
easily)
Properties of Metalloids
Metalloids are elements on both sides of the stair step line. They have properties of both metals and nonmetals.
Solids Can be shiny or dull Ductile Malleable
Families on the Periodic Table
So where do the names come from?
Iron (Fe)………….……Ferrum
Sodium (Na)….. …….Natrium
Gold (Au)……………Aurum
Silver (Ag)………….Argentum
Potassium (K)………… Kalium
Copper (Cu) ………….Cuprum
Mercury (Hg) ……Hydragyrum
Antimony (Sb)………… Stibium
Tin(Sn)….………… Stannum Lead(Pb)
……………..Plumbum
Tungsten(W)………….Wolfran
These abbreviations are for there LATIN names of the elements.
Steps for creating a bohr model
1. Complete the particle inventory for the atom (protons, electrons and neutrons).
2. Draw your nucleus.3. Put the number of protons
and neutrons in the nucleus.
4. Circle how many electrons you need to use in the shells.
5. Know how many electrons and shells you will need.
6. Put 2 electrons in the first shell. If there are more than 2, begin to fill the next shell (maximum of 8).
7. You cannot begin to fill the next shell until the previous shell is filled.
8. Remember` how many electrons each shell can hold a maximum of.(2, 8, 8, 18, 18, 32, 32,)