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SCHS Chapter 5
Glencoe Chemistry Chp. 5
| Term | Definition |
|---|---|
| amplitude | of a wave is the wave's height from the origin to a crest, or from the origin to a trough |
| atomic emission spectrum | of an element is the set of frequencies of the electrospectrum consists of several individual lines of color, not a continuous range of colors as seen in a visible spectrum |
| atomic orbital | a three-dimensional region around the nucleus describing the electron's probable location |
| aufbau principle | states that each electron occupies the lowest energy orbital available.The aufbau diagram shows the energy of each sublevel |
| de Broglie equation | predicts that all moving particles have wave characteristics: wavelength equals h/ particle mass(m) x moving at velocity (v) |
| electromagnetic radiation | is a form of energy that exhibits wavelike behavior as it travels through space |
| electromagnetic spectrum | also called EM spectrum encompasses all forms of electromagnetic radiation with the only differences in the types of radiation being their frequencies and wavelengths |
| electron configuration | the arrangement of electrons in an atom with the low energy systems more stable than high energy systems. |
| electron-dot structure | consist of the elements's symbol represent the elements nucleus and inner level electrons surrounded by dots representing the atom's valence electrons. |
| energy sublevel | labeled s,p, d or f according to the shapes of the atom's orbitals and are contained in the principal energy levels |
| frequency | represent by v or the Greek letter nu. is the number of waves that pass a given point per second. Hz is the SI unit of frequency=1 wave per second represented as (1/s) or (s with the exponent -1) |
| ground state | the lowest allowable energy state of an atom. If an atom gains energy it is in an excited state....hydrogen has atom has many different excited states |
| Heisenberg uncertainty principle | states that it is fundamentally impossible to know precisely both velocity and position of a particle at the same time |
| Hund's rule | states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals. |
| Pauli exclusion principle | states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposites spins. |
| photoelectric effect | electrons are emitted from a metal's surface when light of a certain frequency shines on the surface (calculator powered by) |
| photons | is a particle of electromagnetic radiation with no mass that carries a quantum of energy |
| Planck's constant (h) | E= hv.......energy equals planck's constant times velocity h= 6.626 x 10 to the -34J times s. Joule is the SI unit of energy (J) |
| principal energy level | n specifies the atom's major energy levels. As n increases the orbital become larger the electron spends more time farther from the nucleus and the atom's energy level increases. |
| principal quantum number (n) | indicates the relative sizes and ergies of atomic orbitals. Range in values 1 to7 |
| quantum | is the minimum amount of energy that can be gained or lost by atom |
| quantum mechanical model of an atom | or wave mechanical model of an atom where the atomic model in which electrons are treated as waves and makes no attempt to describe the electrons party around the nucleus |
| valence electrons | electrons in the atom's outermost orbitals with the atom's highest principal energy level. |
| wavelength | the Greek letter lambda is the shortest distance between equivalent points on a continue wave. Measured from crest to crest or from trough to trough. In meters, centimes or nanometers ( very small...1nm=1x10 to the -9m) |
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