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•What is a model?
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•Uses familiar ideas to explain unfamiliar facts observed in nature.
•It can be changed if you get new info.
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•Evidence you get about an object without actually seeing or touching the object.
•You get a mental picture or a model of the object.
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•In the 5th century BC, Democritus believed that matter could be divided into smaller & smaller pieces forever until you got to the smallest possible piece called an atom (uncuttable).
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•In 1803, Dalton published his atomic theory from studying weather & the composition of air.
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•1) All matter is made of atoms 2) Different elements have different kinds of atoms 3) Compounds are formed by joining atoms of 2 or more elements.
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•He discovered the electron & figured it was part of an atom.
•Invented the Plum Pudding Model•The atom was a positively charged ball with lots of negatively charged electrons stuck into it like “plums in pudding.”
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•In 1908, Rutherford discovered the nucleus.
•He stated that the atom was mostly empty space made up of a positively charged nucleus with negative electrons scattered around it.
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• In his experiment, Rutherford fired a stream of alpha particles at a sheet of gold foil and found that:
1. Most of the bullets passed right through the gold sheet without changing course which meant that the gold atoms were made up of empty space.
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2. Some bullets bounced back from the sheet which meant that like charges repel. The alpha particles were positive so the nucleus must then be positively charged.
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•Bohr fixed up Rutherford’s theory.
•He stated that electrons orbited the nucleus on definite paths like the planets around the sun.
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•Based on a prediction of where the electrons actually are using math formulas.
•Basic idea of waves.
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•Subatomic Particles- particles smaller than an atom
•3 Main Subatomic Particles: Protons, Neutrons, Electrons
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Nucleus•The tiny center of atom•99.9% of atom’s weight is the nucleus but it is 100,000 times smaller than the entire atom.
•Like a bee in Yankee Stadium
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Protons•Positively Charged particles (+)
•Found in nucleus•Weighs 1 AMU
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Neutrons•Neutral particles •Found in nucleus•Weighs 1AMU+
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AMU•ATOMIC MASS UNIT•Special unit used to measure the mass of subatomic particles.
•1 proton = 1AMU
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Atomic Number•Number of protons in nucleus of atom
•Determines what the element is
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•Hydrogen’s Atomic number is 1 = 1 proton
•Carbon’s Atomic Number is 6 = 6 protons
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Isotopes•Atoms of same element that have the same number of protons but a different number of neutrons
•C12- C14- difference-2 more neutrons
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MASS NUMBER•Sum of protons & neutrons
•distinguishes one isotope from another
•Carbon = Mass# 12 6P + 6N= 12 total.
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•Uranium238 146N + 92P = 238 Uranium235
143N + 92P = 235
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Atomic Mass •Average mass of all isotopes of that element, usually a decimal located on the bottom of each card.
•Atomic mass of carbon=12.011
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Electrons•Number of protons = number of electrons outside nucleus.
•Electron fills cloud. Electrons can be anywhere within the space around nucleus
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•Electrons are arranged in energy levels according to how much energy they contain
•Electrons with lowest energy are in level closest to nucleus.
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•Electrons with high energy are in levels farther from nucleus.
•Each level can only hold so many electrons: 1st-2 2nd-8 3rd-18 4th-32 5th-18
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Chemical makeup•Properties of elements depend on how many electrons are in the various energy levels.
•Bonding: some do/some don’t
•Quarks-3particles that make up protons & neutrons