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Ch 4 Eelctrons
| Term | Definition |
|---|---|
| electromagnetic radiation | an oscillating electric and magnetic wave that can move through space |
| wavelength | the distance from the peak of one wave to the peak of the next wave |
| frequency | the number of waves that pass a fixed point in one second (1 |
| Joule | a unit of energy |
| Hertz | the unit for frequency equal to one wave per second (1/s = Hz) |
| Planck's constant | the constant that results by dividing energy by frequency (E/f=Planck's constant) |
| quantum | the specific amount of energy that can be absorbed or released by an electron |
| ground state | the lowest possible energy level of an electron |
| excited state | an electron that has absorbed a quantum of energy, and as a result has moved outward to a higher energy level |
| line emission spectrum | an element's unique set of ER wavelengths that are produced as the electrons in an atom emit energy and fall back to ground state |
| quantum theory | the current atomic theory that describes the location of electrons in 3-D orbitals based on mathematical calculations |
| principal quantum number | a number used to describe the main energy level in which an electron is most likely found |
| n | the symbol used to represent the principal quantum numer |
| sublevel | this describes the shape and number of orbitals of an area within a given level; the number of sublevels is equal to the principal quantum number (n) |
| orbital | a 3-D area in which an electron has a high probability of being found |
| orbital diagram | a visual representation of an atom's electron configuration |
| electron configuration | the arrangement of an atom's electrons in energy levels, sublevels, orbitals, and spin of the electron |
| noble gas | a group of nonreactive elements whose out energy level is filled with the outer configuration of s2p6 |
| octet rule | main group elements will gain, lose, or share electrons to fill their outermost s and p sublevels minimizing energy |
| noble gas configuration | a shorthand method of writing an electron configuration by replacing the core electrons with a bracketed symbol of the nearest preceding noble gas |
| Coulombic attraction | The force of attraction between the positively charged nucleus and a valence electron |
| speed of light | The speed at which ALL electromagnetic radiation travels; equal to 3.00 x 10^8 meter/sec |
| Niels Bohr | the scientist who developed the planetary model of the atom in which electrons orbit the nucleus at fixed energy levels |
| Erwin Schrodinger | the scientist who developed the quantum theory of atoms by treating electrons as waves and using an equation to create a 3-D area of high probability for finding an electron |
| How is the line emission spectra created? | Already excited electrons give off energy in the form of light as they fall from a higher energy level to an energy level closer to the nucleus |
| Why is the line emission spectrum useful to scientiests? | Every element has a unique line emission spectrum; therefore it can be used to identify an element |
| Which electrons can be found closest to the nucleus? | Electrons with the lowest amount of energy are located closest to the nucleus |
| Can electrons have the same set of 4 quantum numbers? | No, every electron has a unique set of 4 quantum numbers. They can only share up to 3 of the same quantum numbers. |
| What "things" can behave as a wave and a particle? | electromagnetic energy and electrons |
Created by:
vcanfield
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