Stack #53440
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| aufbau | an electron occupies the lowest possible energy levvel in the ground state
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| polyexclusion principle | no 2 electrons can have the same set of 4 quantum numbers
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| hunds rule | orbitals of equal energy are each occcupied by one electron before any orbital occupied by a second electron and all electron in a singly occupied orbital equal
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| order of levels | 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
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| violet | 400nm
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| indigo | 430nm
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| blue | 460nm
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| green | 500nm
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| yellow | 580nm
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| orange | 620nm
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| red | 700nm
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| electromagnetic radiation | a form of energy that exhibits wave like behavior as it travels through space i.e.gamma waves radio waves
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| wavelength | distance between corresponding points on adjacent waves measured in meters
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| frequency | number of waves that pass a given point in a specific time measured in Hz
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| speed of light (equation) | =frequency x wavelength=3.0x10^8 meters per second
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| photoelectric effect | mission of electrons from a metal when light shines on the metal
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| quantum | minnium quantity of energy that can be lost or gained by an atom
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| equasion of energy | energy equals plancks constant x frequency
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| ground state | lowest energy state of an atom, most stable
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| excited state | state in which an atom has a higher potential energy than it has in the ground state
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| when an excited atom returns to the ground state... | it gives of the energy it gained in the form of electromagnetic radiation
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| the energy of a photon | trhe difference in energy between an atoms initial state and its final state
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| lyman | uv
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| balmear | visible
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| paschen | infrared
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| electrons can only circle the nucleus | in allowed paths circles or energy levels
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| orbits are numbered from | 1 to 7
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| electrons must move to an excited state when | they absorb energy
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| excited state is unstable | (blank)
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| heisenberg uncertaintity principle | it is impossible to simultaneosly determin both the position and velocity of an electron or any other particle
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| quantum theory | mathematicaly describes the wave properties of electrons and other various small particles
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| orbital | 3d region around the nucleus that indicates the probable location of an electron
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| principle quantum number | n, indicates the main energy level total number of orbitals in a given shell equals n^2
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| egular momentum quantum number | indicates the shape of an orbital and number of possible orbital shapes in an energy level
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| magnetic quantum number | indicates the orientation of orbital around the nucleus
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| spin quantum number | has only 2 possible values which indicate spin status of an electron and they must have opposite spins if they are together
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| paramagnetic | an element that has atleast 1 unpaired electron they display magnetic properties
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| diamagnetic | an element with no unpaired electrons
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| a group | is a column
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| group 1 | alkalai
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| group 2 | alkalain/earth
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| group 17 | halogens
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| group 18 | noble gases
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| group 3b - 12b | transition metals
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| s block elementsa | group 1 and 2 valence electrons in s orbital
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| p block elements | group 13 - 18 last electron in p orbital
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| d block elements | 3b to 12b last electron in d orbital
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| f block elements | l and a last electron in the f orbital
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Created by:
lilee256