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42 Cards in this Set
- Front
- Back
Aristotle
Continuous theory of matter |
matter can be subdivided
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Democritus
Discontinuous theory of matter |
get to a point where you can not further divide; "atomus"- indivisible
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John Dalton
Law of multiple proportion, law of definite proportion, amd law of conservation of mass |
1. all atoms of the same element are identical
2. atoms of different elements have different properties 3. each element is composed of indivisible particles called atoms 4. whole atoms combine in a definite ratio and in a different arrangement to form compounds 5. atoms are indestructable - can't be created or destroyed |
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atom
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smallest particle of an element that retains the properties of the element and can exist by itself or in combination with something else
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electron
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first subatomical particle discovered; never changed no matter the metal used in cathode ray tube experiment - fundamental particle
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JJ Thompson
electon: cathode-ray tube |
identified the electron in 1897
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Robert Milikan
oil drop experiment |
led to charge and mass of the electron
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JJ Thompson
proton |
discovered in 1899; always a multiple of what Hydrogen was
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James Chadwick
neutron |
discovered by accident; harder to discover because of neutral charge
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nucleus
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positive charge, 99.9% of the mass, very small radius, highly dense
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atomic number
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Z : number of protons in an atom
(bottom left subscript) |
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Mass number
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A; A = Z + N
-# of neutrons (top left superscript) |
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Atomic mass
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actual mass of the atom;
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Isotopes
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nuclides of same element - same Z, diff N
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Isobar
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same A, Diff Z
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Isotone
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same N, diff Z
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Isoelectronic
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particles with the same number of electrons
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atomic weight
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average of the atomic masses of the natural isotopes of an element based upon the proportion that are found in nature
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thermal emission
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when the electrons are emitted by some metals when the metals are heated to a high temperature
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photoelectric effect
Einstein |
light can behave as a particle and a wave; when elctrons are emitted from metals when they are exposed to light
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radioactivity
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the spntaneous decay of atoms of certain elements into other elements with the simultaneous production of rays or particels
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alpha particle
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helium nucleus, positive, most massive, least penitrative power
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beta particle
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an electron, negative, little mass, more penitrating
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gamma rays
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high energy electromagnetic radiation, no mass, travels at the speed of light, most penitrative
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nuclear reactions
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change in nucleus producing diff elements, diff isotopes have diff behavior, rate is unaffected by change in temp,etc, atom is essentially the same regardless if it is in a compound of by itself, great change in energy
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chemical reactions
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change in the distribution of the outer energy level electrons, diff isotopes have same behavior, rate is changed, less energy
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fission
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break up of a heavy nucleui into smaller ones
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fussion
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take lighter particles and make heavier
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nuclear transmutation
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process of converting one element to another
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beta emission
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wants to decrease ratio of n/p
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alpha emission
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increase n/p; add helium to product
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beta capture
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bombard nucleus with a beta particle; hydrogen atom to reactants
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binding energy
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energy that binds the nucleus together
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John Dalton
model |
atom is a hard, little, sphere that is indivisible
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JJ Thompson
"Raisin pudding model" |
electrons and protons embedded thru out the atom like raisins in pudding
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Rutherford
Alpha Particle Scattering Experiment |
lead to the discovery of the nucleus
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Bohr
Solar System model |
electron is moving around the nucleus in an orbit like planets
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Bohr's 4 postulates
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1. The e- are located in orbits (energy levels) around the nucleus. As long as it stays in a given orbit, it neither gains nor loses energy.
2. The e- in orbits closest to the nucleus are of lower energy. 3. Every e- in an atom may have only certain allowed energies. 4. The e- can move from one orbit to another. To do this, an e- must gain or lose a certain exact amount of energy |
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Planck
wave mechanical model |
when light is emitted, it is radiated in quanta, the amount of E radiated can be revealed by the wavelength of the light emitted
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light spectrum
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gamma, x-rays, ultraviolet, light, infared rays, microwaves, radar, tv, radio waves
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DeBroglie
Duality Nature of the electron |
light can behave like wave and particle
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Heisenberg
uncertainity principle |
impossible to know the exact position and momentum of a particle at a given time
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