Chemistry 1.1
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Transcript of Chemistry 1.1
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ChemistryChapter 1 - Section 1
Why Do Atoms
Combine???
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First, we need to
know what an atom is?
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Atomic Structure
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Atomic Structure
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Atomic Structure
All matter, even solids, contain mostly e m p t y space.
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Atomic Structure
All matter, even solids, contain mostly e m p t y space.
How can this be?
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Atomic Structure
All matter, even solids, contain mostly e m p t y space.
How can this be?
Although there might be little or no space between atoms, a lot of empty space lies within each atom.
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Atomic Structure
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At the center of every atom is a nucleus containing protons
and neutrons.
Atomic Structure
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At the center of every atom is a nucleus containing protons
and neutrons.
The nucleus makes up most of the mass of an atom.
Atomic Structure
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At the center of every atom is a nucleus containing protons
and neutrons.
The nucleus makes up most of the mass of an atom.
The rest of the atom is empty except for the atom’s electrons,
which are extremely small compared with the nucleus.
Atomic Structure
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At the center of every atom is a nucleus containing protons
and neutrons.
The nucleus makes up most of the mass of an atom.
The rest of the atom is empty except for the atom’s electrons,
which are extremely small compared with the nucleus.
The exact location of an electron cannot be determined, the electrons travel in an area around the nucleus called the electron cloud.
Atomic Structure
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Atomic Structure
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Are you ready to be
amazed??
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WOW
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WOWAtoms are extremely small.
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WOWAtoms are extremely small.
One hydrogen atom is approximately 5x10-8mm in diameter.
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WOWAtoms are extremely small.
One hydrogen atom is approximately 5x10-8mm in diameter.
Think about a 1 mm line. It would take _______ hydrogen atoms lined up beside each other to make a line as long as the mark.
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WOWAtoms are extremely small.
One hydrogen atom is approximately 5x10-8mm in diameter.
Think about a 1 mm line. It would take _______ hydrogen atoms lined up beside each other to make a line as long as the mark.
20 million!!!! Monday, July 9, 2012
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Electrons and Our Solar System
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Electrons and Our Solar System
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Planets orbit the sun, just as electrons orbit the nucleus of an atom.
Electrons and Our Solar System
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Planets orbit the sun, just as electrons orbit the nucleus of an atom.
Some differences between electrons and plants are:
Electrons and Our Solar System
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Planets orbit the sun, just as electrons orbit the nucleus of an atom.
Some differences between electrons and plants are:Planets do not have a charge, electrons are negatively
charged
Electrons and Our Solar System
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Planets orbit the sun, just as electrons orbit the nucleus of an atom.
Some differences between electrons and plants are:Planets do not have a charge, electrons are negatively
chargedPlanets orbits are predictable, electron orbits are not
as predictable.
Electrons and Our Solar System
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Element Structure
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Element Structure
Each element has a different atomic structure and a different number of protons, neutrons, and electrons.
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Element Structure
Each element has a different atomic structure and a different number of protons, neutrons, and electrons.
The number of protons and electrons is always the same for a neutral atom.
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Electron Energy
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Electron Energy
All electrons in an atom are somewhere in the electron cloud.
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Electron Energy
All electrons in an atom are somewhere in the electron cloud.
Some electrons are closer to the nucleus than others.
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Electron Energy
All electrons in an atom are somewhere in the electron cloud.
Some electrons are closer to the nucleus than others.
The different areas for an electron in an atom are called energy levels.
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Electron Energy
All electrons in an atom are somewhere in the electron cloud.
Some electrons are closer to the nucleus than others.
The different areas for an electron in an atom are called energy levels.
Each level represents a different amount of energy and can hold a certain number of electrons.
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Electron Energy
All electrons in an atom are somewhere in the electron cloud.
Some electrons are closer to the nucleus than others.
The different areas for an electron in an atom are called energy levels.
Each level represents a different amount of energy and can hold a certain number of electrons.
The farther an energy level is from the nucleus, the more electrons it can hold.
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Energy Steps
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Energy Steps
Text
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Energy Steps
Text
Level Max. number of electrons1st 22nd 83rd 184th 32
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Energy Steps
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Energy Level 1 has the lowest amount of energy.
Energy Steps
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Energy Level 1 has the lowest amount of energy.
Electrons furthest away have the most energy.
Energy Steps
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Energy Level 1 has the lowest amount of energy.
Electrons furthest away have the most energy.
Electrons furthest away are the easiest to remove.
Energy Steps
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Energy Level 1 has the lowest amount of energy.
Electrons furthest away have the most energy.
Electrons furthest away are the easiest to remove.
How many electrons can occupy an energy level?
Energy Steps
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Energy Level 1 has the lowest amount of energy.
Electrons furthest away have the most energy.
Electrons furthest away are the easiest to remove.
How many electrons can occupy an energy level?
Use 2n2 (n represents the energy level).
Energy Steps
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Magnets & Paper Clips
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Magnets & Paper Clips
Removing electrons that are closer to the nucleus takes more energy than removing ones that are further away.
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Removing Part of the Balloon
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Removing Part of the Balloon
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What is being removed from the balloons atoms?
Removing Part of the Balloon
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What is being removed from the balloons atoms?
Electrons
Removing Part of the Balloon
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What is being removed from the balloons atoms?
ElectronsFrom what energy level?
Removing Part of the Balloon
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What is being removed from the balloons atoms?
ElectronsFrom what energy level?
Highest energy level
Removing Part of the Balloon
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Removing Part of the Balloon
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Our Wonderful and Perfect Periodic Table
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Horizontal Rows are called periods
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Our Wonderful and Perfect Periodic Table
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Horizontal Rows are called periods
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Period 1
Our Wonderful and Perfect Periodic Table
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Horizontal Rows are called periods
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Period 1
Period 2
Our Wonderful and Perfect Periodic Table
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Horizontal Rows are called periods
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Period 1
Period 2
Period 3
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Group 4
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Group 5
Group 4
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Group 5
Group 6
Group 4
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Group 5
Group 6
Group 7
Group 4
Our Wonderful and Perfect Periodic Table
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Vertical Rows are called Groups or Families
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Group 1
Group 2
Group 3
Group 5
Group 6
Group 7
Group 4
Group 8
Our Wonderful and Perfect Periodic Table
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Our Wonderful and Perfect Periodic Table
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Remember that the number of protons and electrons are the same in a neutral atom (which
is what is represented on the periodic table).
Our Wonderful and Perfect Periodic Table
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Remember that the number of protons and electrons are the same in a neutral atom (which
is what is represented on the periodic table).
The number of electrons increases by one as
you move across the period.
Our Wonderful and Perfect Periodic Table
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Our Wonderful and Perfect Periodic Table
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Our Wonderful and Perfect Periodic Table
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Our Wonderful and Perfect Periodic Table
A few things to notice....
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Our Wonderful and Perfect Periodic Table
A few things to notice....
Groups 3-12 are not pictured.
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Our Wonderful and Perfect Periodic Table
A few things to notice....
Groups 3-12 are not pictured.
Group 18 is complete, it is full. It has _____ electrons.
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Hydrogen is usually considered separately,
so the first element
family begins with lithium and sodium in the first column.
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Our Wonderful and Perfect Periodic Table
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Our Wonderful and Perfect Periodic Table
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Human family members often have similar looks and traits.
Our Wonderful and Perfect Periodic Table
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Human family members often have similar looks and traits.
Also, members of element families have similar properties, chemical properties, because they have the same number of electrons in their outer energy levels.
Our Wonderful and Perfect Periodic Table
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It was the repeating pattern of properties that gave Russian chemist Dmitri Mendeleev the idea for his first periodic table in 1869.
Our Wonderful and Perfect Periodic Table
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Why so Noble, Group 18?
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Why so Noble, Group 18?
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Noble Gases have energy levels that are complete. They have 8 electrons in their outer energy levels.
Why so Noble, Group 18?
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Noble Gases have energy levels that are complete. They have 8 electrons in their outer energy levels.
Do not combine well with other elements – originally thought they would not combine at all, but they will on rare occasion.
Why so Noble, Group 18?
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Noble Gases have energy levels that are complete. They have 8 electrons in their outer energy levels.
Do not combine well with other elements – originally thought they would not combine at all, but they will on rare occasion.
Because they are so stable they are used to protect filaments in light bulbs.
Why so Noble, Group 18?
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Noble Gases have energy levels that are complete. They have 8 electrons in their outer energy levels.
Do not combine well with other elements – originally thought they would not combine at all, but they will on rare occasion.
Because they are so stable they are used to protect filaments in light bulbs.
Also used as to produce coloured lights in signs…electricity causes the noble gases to emit a certain colour light. Neon – orange/red; Argon – lavender; Helium – yellowish white
Why so Noble, Group 18?
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Halogens From Halifax(Group 17)
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Halogens From Halifax(Group 17)
Monday, July 9, 2012
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Halogens only need one more electron, so they are very reactive.
Halogens From Halifax(Group 17)
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Halogens only need one more electron, so they are very reactive.
Fluorine is the most reactive because the electrons are so close to nucleus.
Halogens From Halifax(Group 17)
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Halogens only need one more electron, so they are very reactive.
Fluorine is the most reactive because the electrons are so close to nucleus. Remember that when electrons are close to the nucleus,
there is a stronger pull from the protons.
Halogens From Halifax(Group 17)
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Halogens From Halifax(Group 17)
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Halogens From Halifax(Group 17)
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Halogens From Halifax(Group 17)
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The further you go down group 17, the
reactivities decrease.
Halogens From Halifax(Group 17)
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The further you go down group 17, the
reactivities decrease.This is because there is more energy levels,
and so the electrons are further away from the pull of the protons.
Halogens From Halifax(Group 17)
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Halogens From Halifax(Group 17)
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Alkali Metals Have One Extra Petal
(Group 1)
Monday, July 9, 2012
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Alkali Metals Have One Extra Petal
(Group 1)
Monday, July 9, 2012
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Alkali Metals have one electron in outer most
energy level.
Alkali Metals Have One Extra Petal
(Group 1)
Monday, July 9, 2012
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Alkali Metals have one electron in outer most
energy level.
This electron will be removed when alkali metals reacts.
Alkali Metals Have One Extra Petal
(Group 1)
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Alkali Metals have one electron in outer most
energy level.
This electron will be removed when alkali metals reacts.
The easier it is to remove an electron, the more reactive the atom is.
Alkali Metals Have One Extra Petal
(Group 1)
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Alkali Metals Have One Extra Petal
(Group 1)
Monday, July 9, 2012
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Reactivities increase as you go down the group. Why?
Alkali Metals Have One Extra Petal
(Group 1)
Monday, July 9, 2012
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Reactivities increase as you go down the group. Why?
Alkali metals want to give away one of their electrons. That electron is further away from the pull of the proton as you move down group 1 in the periodic table.
Alkali Metals Have One Extra Petal
(Group 1)
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Electron Dot Diagrams
Monday, July 9, 2012
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Electron Dot Diagrams
An electron dot diagram is the symbol for the element surrounded by as many dots as there are electrons in its outer energy level.
Monday, July 9, 2012
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Electron Dot Diagrams
An electron dot diagram is the symbol for the element surrounded by as many dots as there are electrons in its outer energy level.
Only the outer energy level electrons are shown because these are what determine how an element can react.
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Electron Dot Diagrams
Monday, July 9, 2012
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Start by writing one dot on the top of the
element symbol
Electron Dot Diagrams
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Start by writing one dot on the top of the
element symbol
Then work your way around, adding dots to the right, bottom, and left.
Electron Dot Diagrams
Monday, July 9, 2012
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Start by writing one dot on the top of the
element symbol
Then work your way around, adding dots to the right, bottom, and left.
Add a fifth dot to the top to make a pair.
Electron Dot Diagrams
Monday, July 9, 2012
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Start by writing one dot on the top of the
element symbol
Then work your way around, adding dots to the right, bottom, and left.
Add a fifth dot to the top to make a pair.
Continue in this manner until you reach eight dots to complete the level
Electron Dot Diagrams
Monday, July 9, 2012
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Electron Dot Diagrams
Monday, July 9, 2012