| A | B |
|---|
| Bohr model | atomic model constructed by Neils Bohr that proposes all electrons can be found in orbitals or paths; electrons must gain or lose energy to jump from one orbital to another |
| Compound | two or more atoms of DIFFERENT ELEMENTS chemically combined; always the same ratio |
| Electron | virtually MASSLESS (teenie, tiny) NEGATIVELY CHARGED particle found OUTSIDE the nucleus |
| Electron Configuration | the arrangement of electrons in an atom or molecule |
| Electron spin | two electrons are paired within each orbital having opposite spins. |
| Excited state | when an atom absorbs energy and one or more of its electrons “jump” to an orbital further from the nucleus |
| Ground state | when all electrons within an atom fill the lowest energy orbitals; when the electrons are where they would “normally” be |
| Heisenberg’s Uncertainty Principle | it is impossible to know the position and momentum of particles exactly. |
| Hund’s Rule | the process of how electrons fill orbitals of equal energy to maximize the number of unpaired electrons. |
| Ion | a charged atom; an atom that gains or loses an electron |
| Isotope | an atom of an element with the same number of protons (atomic #) but a different number of neutrons |
| Kernel electron(s) | any electrons found inside the valence shell; the innermost electrons |
| Lewis Dot Diagram | representation of an atom or molecule using only the element symbol and the valence electron arrangement |
| Line spectra | a spectrum that contains only certain colors, or wavelengths. |
| Orbital | a region where electrons of an atom can be found. |
| Planck’s Theory | the relationship between the frequency and the wavelength of a particular radiation and the energy with which it is associated. There is a limited amount of energy that an object can absorb or emit in pieces called quantum. |
| Principal energy levels | one of a limited number of energy levels in an atom, quantum number (n). |
| Quantum Theory | used to describe the dual nature of matter; electrons behave like particles and energy |
| Sublevel | a division of principal energy level in an atom (s, p, d, and f). |
| Valence electron(s) | the outermost electrons in an atom; there can NEVER be more than 8 valence electrons (OCTET RULE) |
| Visible spectrum | an array of colors with different wavelengths and frequencies depending on the color. |
| Wave-mechanical model | states that electrons don’t travel in fixed orbits, but that we can use mathematic principals to predict where electrons are most likely to be found |
