models of atomic structure. dalton model unbreakable neutrally charged spheres
TRANSCRIPT
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Models of Atomic Structure
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Dalton Model• Unbreakable neutrally
charged spheres.
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Thomson’s Cathode Ray Experiment• Cathode rays originate
from neutrally charged atoms.
• Cathode rays have a negative charge and are deflected by electrical charges and magnetic fields.
• Cathode rays are electrons.
Cathode Ray Tube
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Cathode Rays = Electrons
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Cathode Rays = Electrons
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Cathode Rays = Electrons
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Plum Pudding Model• Negative electrons stuck
inside and on the surface of a positive pudding.
• Atom’s mass and positive charge is widely spread.
• Electrons might wander but mostly motionless unless kicked out by a lot of energy.
• Chocolate chips in ice cream.
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Plum Pudding Model• Negative electrons stuck
inside and on the surface of a positive pudding.
• Atom’s mass and positive charge is widely spread.
• Electrons might wander but mostly motionless unless kicked out by a lot of energy.
• Chocolate chips in ice cream.
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Rutherford’s Gold Foil Experiment – Predicted Results
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Rutherford’s Gold Foil Experiment – Predicted Results
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Rutherford’s Gold Foil Experiment – Actual Results
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Actual Results
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Rutherford’s Gold Foil Experiment• Most alpha particles
(42He) passed right
through the gold foil. • A few alpha particles
had very large deflections.
• The Plum Pudding model would predict only small deflections.
• The mass and positive charge of an atom is concentrated in a very small nucleus.
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Rutherford-Bohr Model• Nucleus takes up very
little space. • Electrons jump up to a
higher energy level when they absorb energy.
• Electrons falls down to a lower energy level when they emit energy.
• Electrons orbit in regular “planet-like” energy levels around the positive nucleus.
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Rutherford-Bohr Model• Nucleus takes up very
little space. • Electrons jump up to a
higher energy level when they absorb energy.
• Electrons fall down to a lower energy level when they emit energy.
• Electrons orbit in regular “planet-like” energy levels around the positive nucleus.
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Quantum Model• Electron clouds not
orbits. • Electrons are not found
in fixed locations, but rather probabilities to be in a location.
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s-orbitals
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p-orbitals
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Atomic ModelsAtomic Model Description
Dalton Solid, neutrally charged spheres.
Plum-Pudding Negatively charged electrons in a glob of positive charge. Like chocolate chips in vanilla ice cream.
Rutherford-Bohr
Negatively charged electrons orbit a positive nucleus. Like planets around the sun.
Quantum Electrons are in layers of clouds around the nucleus.
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Key11NaSodium22.99
Atomic Number•Number of Protons•Number of Electrons (when atom is neutrally charged)
•Property unique to each element
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Key
Average atomic mass*•Weighted Average number of Protons and Neutrons (approximately)
NaSodium22.99
11
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Subatomic Particlesthe particles that make up an atom
• Protons – high mass, positive charge. Found in nucleus.
• Neutrons – high mass, no charge. Found in nucleus.
• Electrons – low mass, negative charge. Found orbiting around nucleus. (abbreviated e– )
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Basic Electrical Charge Laws
+ and – : Attract(pull
together)
– and – : Repel(push away)
+ and + : Repel(push
away) Like charges repel and Opposites attract
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An Atom
Nucleus
1 proton = H = hydrogen
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Why doesn’t the electron fall into the nucleus?• It orbits because the electron is moving really
fast around the nucleus. • Because the electron has such a low mass,
even a small amount of energy makes it move very fast.
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An Atom
Nucleus
1 proton = H = hydrogen
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Another AtomSize of atom
Size of nucleus
2 protons = He = helium
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Cathode Rays = Electrons
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NeFONCBBe
He
Li
H
Kr
ArCl
Br
XeI
SPSiMg Al
Ca
Na
K
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4 e– in valence shell