Atomic Structure and Theories Dalton Chemistry with Doc.
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Transcript of Atomic Structure and Theories Dalton Chemistry with Doc.
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Atomic Structure and Theories
Dalton
Chemistry with Doc
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Dalton1.The atom is made up of identical
particles throughout2.Particles are indivisible3.Atom is made up of mostly (+) charge4.Solid Billiard Ball Model
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J. J. Thompson “Plum Pudding model”
1. Discovered Electrons2. Used the “Cathode Ray Tube” a.k.a. “Crookes tube”3. Shot particle beams through a magnetic field4. Concluded that the beams were made up of
particles with a negative charge…..called electrons
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Rutherford “Gold foil experiment”1. Shot alpha particles (+) through a gold (Au) foil2. Saw that most particles went through undeflected3. noticed some particles were deflected4. concluded that the atom is made up of
Small dense (+) charged particles and is mostly open space
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Bohr Model1. Places electrons outside the nucleus in specific locations called orbits2. Orbits = Energy levels (n) = Periods (Remember That!)
Energy Levels 1st
2nd
3rd
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Modern Atomic Theory “Wave Mechanical Theory, Electron Cloud”
1. Like the Bohr model but can’t place electrons in an exact location2. Show the Most Probable Location
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Atoms are composed of subatomic particles
Name Location Charge Mass
Protons (Nucleons)
Nucleus + 1 amu
Neutrons (Nucleons)
Nucleus 0 1 amu
Electrons Outside nucleus in orbits
- 1/1836 amu
AMU= Atomic Mass UnitBased on C12 as the standard, therefore a proton 1H1 = 1/12 the Mass of Carbon
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Calculating Protons, Neutrons and Electrons
6C12 atomic mass = protons + neutrons
atomic number = number of protons = which
identifies the element!
(+) , Nuclear ChargeAssume….since all elements on the periodic table areNeutral, this must also represent the # of electrons.
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When they form a bond
Form and Ion It is called a….
Metals Lose Electrons (+) Ca(t)ion
t=(+)
Non-Metals Gain electrons (-) A(n)ion
n=negative
IONS
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Isotopes1. different form of the same element2. Differ in the number of neutrons therefore, they have different masses
6C126C14
7X146X12
=P==n==e=
=P==n==e=
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Characteristics of Isotopes1. Tend to be unstable, therefore they emit energy which makes them radioactive2. There are no stable isotopes above element #82
Atomic Mass vs Mass #(the sum of the weighted avg. of all naturally occurring isotopes P + N
(Whole number)
6C12.0171
6C12
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Calculate the Atomic mass of carbon that is made up of80% Carbon 12, 15% Carbon 10 and 5% Carbon 14?
Change % to decimal, multiply by the mass, then add.
.80 X 12 = 9.6
.15 X 10 = 1.5
.05 X 14 = 0.7 11.5 amu
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Lewis Dot Diagrams1. show only valence electrons2. remember…group number = valence electrons 1 =1, 2 =2, 13 = 3, 14 = 4, 15 = 5 etc.3. remember the last number in the configuration also equals # of valence electrons
Cl 2-8-7 valence electrons
3 energy levels This tells you:
3 energy levels are occupied (Cl is in per. 3) 7 valence electrons (Grp 17)
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H He Li Be
B C N O
F Ne
XX
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Electron Configurations
1. remember all configurations are located under the elements symbol
2. configurations show you a. total number of electronsb. number of occupied energy levels = periodsc. # of valence electrons
Ca . . 2-8-8-2 2 valence electrons Ca 18 kernel electrons
4 energy levels occupied
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Remember, after element #20 (Calcium), we then start to fill in the d block which are the transitional metals.
(not so important)
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Ground State vs Excited State
• Ground State• Stable• Lower energy
• Lower Energy
• Excited State• Unstable• Higher Energy State
• Higher energyAbsorb energy
Release energy
Bundle of Energy called a Quanta Bright line Spectrum
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17Cl35
2-8-7
3 energy levels (period 3)Group 177 valence electrons
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Spectral lines – identify the unknown
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