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