Possible Evidence of Thermodynamic Activity in Dark Matter Haloes.
Chapter 3 Atoms: The Building Blocks of Matter. I. The Atom *Matter: anything that has mass and...
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Transcript of Chapter 3 Atoms: The Building Blocks of Matter. I. The Atom *Matter: anything that has mass and...
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Chapter 3
Atoms: The Building Blocks of Matter
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I. The Atom
*Matter: anything that has mass and volume
*Indirect Evidence: evidence you get without actually seeing or touching the object
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-Greek Model (Democritus)*atom: smallest particle of an
element that has the prop of the element
~atomos: meaning not to be cut
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-Dalton’s Atomic Theory1. All elements are composed
of atoms2. Atoms of the same element
are exactly alike
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3. Atoms of diff. elements are diff.
4. Compounds are formed by joining of atoms of 2 or more elements
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5. In Chem Rxn’s, atoms are combined, separated, or rearranged.
-Are exceptions:
1. Atoms are divisible
2. Given elements can have atoms with diff masses (isotopes)
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*Law of Conservation of Mass: pg 66
*Law of Multiple Proportions: pg 66
*Law of definite proportions: pg 66
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II. The Structure of the Atom
-Thomson’s Model:
~Plumb Pudding
*Electrons: - charge
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~Cathode Ray (pg 70)
*Cathode: conn to the neg
*Anode: conn to the pos
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-Rutherford’s Model
~Gold Foil Experiment
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~Inferences made about atomic struct1. e- small2. neg3. must have a + charge to make an atom neutral4. Atom mass must come from somewhere else??
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~the atom was mostly empty space with a dense, positively charged nucleus in the center.
*Nucleus: the center of the atom*Nuclear Force: hold nuclei together
Like charges “+/+”
*Electrostatic (Electromagnetic): holds opposite charges together “e-/+”
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-Bohr Model
~electrons move in definite orbits around the nucleus
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-Wave Model (Today accepted model)~electrons don’t move about in a definite path~probable location is based on how much nrg the electron has
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-Subatomic particles
*smaller than the atom
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• Electrons• Electrons orbit around
an atom. In this picture, they are the small yellow bits.
• They have a negative charge.
• They are lighter than protons or neutrons.
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• They are positively charged.
• Are located in the nucleus.
• In this picture, the protons are the blue pieces in the center of the atom.
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• Neutrons are neither positive nor negative.
• Neutrons are in the nucleus of an atom.
• In this picture, neutrons are the purple pieces in the center of the atom.
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mass (amu) charge location
~proton: 1 + nucleus
~neutron: 1 +/- nucleus
~electron: 1/1836 - e- cloud
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SEE HISTORY OF THE ATOM WEBSITE
http://web.neo.edu/rjones/Pages/1014new/Lecture/chemistry/chapter_8/pages/history_of_atom.html
http://www.emsb.qc.ca/laurenhill/science/models.html
http://www.absorblearning.com/chemistry/demo/units/LR301.html#J.J.Thomson
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III. Counting Atoms
*Atomic Mass Unit (amu): measures mass of subatomic part.
-?? Where does it come from??
1/12 mass of a C-12 atom
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-Atomic #
*number of + in the nucl
~identifies the element
~never chngs
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-Mass # and Atomic Mass*sum of the + and neutrons in its nucleus
-Isotopes*same # of +, but diff # of neutrons(same elem, diff mass)*Nuclide: any isotope of any element
EX: table 3-3 pg 77
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-Isotopes of H (pg 76)
1. Protium: most common
1+, 1e-, 0+/- mass# = 1
2. Deuterium:
1+, 1e-, 1+/- mass# = 2
3. Tritium:
1+, 1e-, 2+/- mass# = 3
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isotope notation
1. mass # H : Nuclear symbol
atomic#
pg: 77
2. Hydrogen - mass #
pg 80
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*Aver Atomic mass: aver of the masses of all the atoms in the sample.(that’s why Atomic mass is not a nice numb)
~mass # - atomic# = #of neutrons
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*Mole: # of particles in 12 grams of C-12
pg 81
*Avogadro’s #: # of particles in 1 mole of substance.
6.022 X 1023 atoms
mole
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*Molar Mass: mass of 1 mole of pure substance
units---- g/mole
-Gram/Mole Conversion Examples