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| A quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles, proved to have wavelike properties in diffraction experiments. |  | |
| Group 1, 1 electron in outer level, very reactive, soft, silver, shiny, low density; Lithium, Sodium, Potassium, Rubidium, Cesium, Francium, react violently and vigourous with water. |  | |
| Most light appears to be one color, but if its put through a prism, its broken down into parts. Spectrum of all visible lines~ EX: A RAINBOW |  | |
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| A model of the atom developed by niels bohr that shows electrons moving in orbits around the nucleus of the atom, omly works and can be used to predict the motion of a hydrogen atom. | ||
| determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus | ||
| numbers that specify the properties of atomic orbitals and of their electrons | ||
| an atomic orbital may describe at most two electrons | ||
| A spinning electron that produces a magnetic field that makes the electron behave like a tiny magnet | ||
| The rule that electrons occupy the orbitals of lowest energy first | ||
| Atoms w. more than 1 e- (not H₂) | ||
| a horizontal row of elements in the periodic table | ||
| The energy required to remove one electron from a neutral atom of an element, Incrases across a perod and decreases going down a period. | ||
| 2 types covalent _________ , whicj is calculated by taking 1/2 the distance between the two atoms. For Example: (Br2, O2, F2), and metalic ________ formed from the average of ionic bonds radii. Decreases across(left to right) a period and increasesgoing down a period. | ||
| The energy change associated with the addition of an electron to a gaseous atom, usually negative. | ||
| the laws of mechanics concerning the interaction of matter and radiation at the atomic and subatomic level | ||
| Symbol for plank's constant = 6.626 x 10 ^-34 J/s | ||
| predicts that all moving particles have wave like characteristics and relates each particle's wavelength to its frequency, its mass and planck's constant m = h/wavelgth x velocity. | ||
| According to the Photoelectrical effect the excess intensity added to a light which exeeds the threshold frequency is converted to ______________. And the famous equation E= mc^2 comes from | ||
| (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) | ||
| occurs when an object causes a wave to change direction and bend around it | ||
| a series of bright spots on either side of the central bright spot; closest bright spots are called first order | ||
| Are formed when beams of light interfer constructively ( amplify) to produce a_____________> |  | |
| Occur when a beam of light interfers destructively (cancels out) therefor producing a __________ |  | |
| a series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism | ||
| Used to find the energy differnce that occurs between two different states. | ||
| A wave that appears to stand in one place, even though it is really two waves interfering as they pass through each other | ||
| regions of zero displacement in standing wave | ||
| the points of maximum amplitude on a standing wave | ||
| Predicts where each electron in an atom will probably be found, i.e. orbitals; quantization of electron energies is a natural outcome | ||
| these describe the statistical likelihood of the electron location at any time, part of Schrodingers equation. The square of this can be used to indicate the probability value near a given point in space. | ||
| states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle | ||
| A distrubution in which the intensity of the color is used to indicate the probability value near a given point in space | ||
| Total probability of finding an electron at any distance r from the nucleus, volume around the nucleus is divided into layers, add the probability densities in that layer to predict which layer has the electron | ||
| Symbolized by n, indicates the main energy level occupied by the electron | ||
| symbolized by l, indicates the shape of the orbital, has values from 0 to n-1. | ||
| m sub l, , the quantum number that indicates the orientation of an orbital around the nucleus, goes from - l to l | ||
| Orbitals of the same subshell are of the same shape and energy. p-orbitals are of the same subshell, while s-orbitals are of a separate subshell. Indicated by the angular momentum quantum number. |
