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| 7579880100 | electromagnetic radiation | type of radiation that includes visible light, radio waves, infrared radiation, xrays | 0 | |
| 7579880101 | How fast does electromagnetic radiation move How does it move | moves at 2.998x10^8 m/s (speed of light) through a vaccum wave-like characteristics (similar to water waves) | 1 | |
| 7579880102 | speed of light | 3.00x10^8 m/s | 2 | |
| 7579880103 | What is meant by electromagnetic waves are "periodic" | water waves are *periodic* (patterns of peaks and troughs repeat at constant intervals) | 3 | |
| 7579880104 | define wavelength | distance between two adjacent peaks (or two troughs) | 4 | |
| 7579880105 | define frequency | number of complete wavelengths (cycles) that pass a specific point in a second | 5 | |
| 7579880106 | What do all electromagnetic wave characteristics rely on. | periodic oscillations in intensities of electric and magnetic fields associated with radiation | 6 | |
| 7579880107 | Wavelength and frequency are ___________ related | They are inversely related. the shorter the wavelength the higher the frequency and vise versa | 7 | |
| 7579880108 | formula that describes inverse relationship between wavelength and frequency UNITS FOR EACH | c = λν λ = wavelength (lambda), meters ν = frequency (nu), Hz c = light speed, m/s | 8 | |
| 7579880109 | what causes the differences between different types electromagnetic radiation | wavelength | 9 | |
| 7579880110 | the electromagnetic spectrum From left to right and direction of energy increase |  | 10 | |
| 7579880111 | what are Hertz (Hz) a unit for | unit for frequency expressed in cycles per second | 11 | |
| 7579880112 | ways of denoting hertz | MHz (mega-hertz) Hz (regular) s^-1 /s | 12 | |
| 7579880113 | The three phenomena that cannot be described by the wave model of light | Blackbody radiation - emission of light from hot objects photoelectric effect - emission of electrons from metal when light shines on it emission spectra - emission of light from electronically excited gas atoms | 13 | |
| 7579880114 | quantum | the smallest quantity of energy that can be emitted/absorbed as electromagnetic radiation The packets energy comes in | 14 | |
| 7579880115 | Energy equation in regards to the photoelectric effect ("energy of a photon") | E = hν the energy of a single quantum equals the constant times the frequency of the radiation ν = frequency h = Plank constant |  | 15 |
| 7579880116 | what is the value of the Plank Constant | 6.63x10^-34 | 16 | |
| 7579880117 | plank relation (for when you want to know E but arent given frequency) | This realationship works because of the energy inverse relationship of wavelength and frequency |  | 17 |
| 7579880118 | matter can only emit/absorb energy in whole number multiples of hν | ... | 18 | |
| 7579880119 | Energy of a photon | E = hv | 19 | |
| 7579880120 | How does the photoelectric effect work | phtotons striking a metal surface can transfer their energy to electrons in the metal If the photons have enough energy (work function) the electrons will overcome the attractive forces holding them in the metal. Excess energy from the photons are converted to kinetic energy of the electrons that are emitted | 20 | |
| 7579880121 | What is brightness dependent on | the number of photons hitting a surface in a unit of time. Not the energy intensity of the photons | 21 | |
| 7579880122 | So, is light a wave or a stream of particles? | Yes. And it can act like one more than the other depending on the circumstances. Buckle up kid's we're about to science. | 22 | |
| 7579880123 | define monochromatic | only emits a single wavelength (like a laser) | 23 | |
| 7579880124 | define polychromatic | contains many different wavelengths (like light and most other radiation sources) | 24 | |
| 7579880125 | define specrum (in context) | the result when a radiation source's wavelengths are separated | 25 | |
| 7579880126 | define continuous spectrum | no breaks in the spectrum. One color fades into the next | 26 | |
| 7579880127 | define line specrum | a spectrum of radiation that only contains specific wavelengths | 27 | |
| 7579880128 | the Rydberg equation |  | 28 | |
| 7579880129 | Bohrs 3 postulates | 1. Electrons in an atom can only occupy certain orbits (corresponding to certain energies). 2. Electrons in permitted orbits have specific, "allowed" energies; these energies will not be radiated from the atom. 3. Energy is only absorbed or emitted in such a way as to move an electron from one "allowed" energy state to another; the energy is defined by E = hv | 29 | |
| 7579880130 | will be given planks constant on the test will be given Bohr equation on the test. But still be familiar with it. what does k equal? | -hcR = k All three are constants nf = final energy level ni = initial energy level k = 2.18x10^-18 |  | 30 |
| 7579880131 | quantized | electrons can only exist at specific energy levels, separated by specific intervals(??) | 31 | |
| 7579880132 | Principle quantum number | symbolized by n, indicates the main energy level occupied by the electron orbit 1 = 1 orbit 2 = 2 etc... | 32 | |
| 7579880133 | The lower the orbit of the electron the more __________ the charge of the electron is, thus the more stable the atom | negative | 33 | |
| 7579880134 | define ground state | The lowest energy state of an atom (lowest orbit possible) | 34 | |
| 7579880135 | define excited state | any energy state higher than the ground state (higher orbit than the lowest possible orbit) | 35 | |
| 7579880136 | define radiant energy | radiation energy | 36 | |
| 7579880137 | does an electron release or absorb energy when it jumps up an orbit | absorbs because energy is positive it releases energy when it jumps down an orbit | 37 | |
| 7579880138 | delta E is positive when and electron jumps up and orbit or jumps down an orbit? | Jumps up because it's becoming less negative so the change in energy is positive | 38 | |
| 7579880139 | The sign of delta E tells whether the photon is _______ or _________ when an electron jumps from one orbit to another (up or down) | absorbed or emitted | 39 | |
| 7579880140 | The equation for the energy of a photon absorbed or emitted by an electron when it jumps/falls is equal to | Ephoton = hv = -deltaE | 40 | |
| 7579880141 | Most of Bohrs model only applies to hydrogen | ... | 41 | |
| 7579880142 | Two things that remain true about Bohrs model | Electrons only exist in discrete energy levels, and they are described by quantum numbers Energy is involved in transition of an electron between levels | 42 | |
| 7579880143 | Define matter waves | wave characteristics of material particles | 43 | |
| 7579880144 | wavelength of matter equation de Broglie relationship | h = plank constant mv = momentum Change mass to kilograms and velocity to m/s because J has kg as it's weight (J = kgm^2/s^2) |  | 44 |
| 7579880145 | what comprises momentum | mv Mass times velocity | 45 | |
| 7579880146 | The wavelength or regular size objects is so small that it is unobservable. That is not so for tiny objects (electrons) | ... | 46 | |
| 7579880147 | uncertainty principle | the principle that says it is impossible to simultaneously determine the momentum (mass times velocity) and the position of an electron with precision; either momentum or position may be precisely measured, but not both | 47 | |
| 7579880148 | define Schrodinger's wave equation | an equation that incorporates both the wave and particle behaviors of electrons | 48 | |
| 7579880149 | wave functions | The result of solving schrodinger's wave equation. They describe the electrons in an atom (electron density) The results are called Orbitals |  | 49 |
| 7579880150 | Probability density (electron density) | The probability that an electron will be found at that location Ψ^2 | 50 | |
| 7579880151 | define orbital | an area in which a electron may be found 90% of the time. Each orbital for an atom has a particular shape and energy. Orbitals are not Orbits. | 51 | |
| 7579880152 | The three quantum numbers that describe orbitals | n, l, and ml ml has the subscript of l | 52 | |
| 7579880153 | rules for n, l, ml | n - *positive integer value*.*Larger n means larger orbital* with *higher energy* and *more time spent farther from the nucleus* l - integer value from 0 to n-1. Defines shape of the orbital. letter designations for the values are s(0), p(1), d(2), f(3). After 3 is alphabetical ml - integer value from -l to l including zero. Describes orientation of the orbital in space | 53 | |
| 7579880154 | s, p ,d, f | Sharp Principal Diffuse Fundamental | 54 | |
| 7579880155 | names for n, l, ml | n = principle quantum number l = angular momentum quantum number ml = magnetic quantum number | 55 | |
| 7579880156 | unoccupied vs occupied orbitals | an occupied orbital is the current orbital an electron is in (the value of n) in any given instant. | 56 | |
| 7579880157 | Relationship between the quantum numbers Subshell vs orbital vs shell vs single electron |  | 57 | |
| 7579880158 | n, l, ml relationship | 1. Shell with n shells has n subshells 2. Each subshell consists of specific number of orbitals 3. total number of orbitals in said shell is n^2 |  | 58 |
| 7579880159 | Each orbital can have up to ____ electrons in it | 2 | 59 | |
| 7579880160 | The s orbital characteristics | they are all spherically symmetrical | 60 | |
| 7579880161 | s p d f orbital shapes/orientations |  | 61 | |
| 7579880162 | Degenerate orbitals | Orbitals with identical energies (same energy levels) | 62 | |
| 7579880163 | As number of electrons increase repulsion between them increases. What does this cause? | not all orbitals on the same energy level will be degenerate However sublevels of same level will still be | 63 | |
| 7579880164 | spin quantum number | not all electrons in the same orbital has the same energy. Spin describes an electrons magnetic field. Two electrons of opposite spins will attract each other to some degree. |  | 64 |
| 7579880165 | Radical probability function | 1.number of peaks 2. number of nodes (low points at which probability of electron being there = zero) 3.Spread (How large the orbital is) |  | 65 |
| 7579880166 | Contour representation | shapes | 66 | |
| 7579880167 | p orbitals | for every n (1,2,3???) Size and shape is the same but the orientation is different |  | 67 |
| 7579880168 | Pauli Exclusion Principle | No two electrons in the same atom can have exactly the same energy. • Therefore, no two electrons in the same atom can have identical sets of quantum numbers. • This means that every electron in an atom must differ by at least one of the four quantum number values: n, l, ml , and ms | 68 | |
| 7579880169 | orbital diagram |  | 69 | |
| 7579880170 | Electron configuration | The way electrons are distributed in an atom is called its electron configuration. • Each component consists of - a number denoting the energy level; - a letter denoting the type of orbital; - a superscript denoting the number of electrons in those orbitals. |  | 70 |
| 7579880171 | Aufbau principle | electrons fill lowest energy levels first | 71 | |
| 7579880172 | Hund's rule | when filling sublevel, one electron is added to each orbital (with same spin) before 2 are added to any (opposite spin) | 72 | |
| 7579880173 | valence electrons and group number on periodic table | each group has the same number of valence electrons | 73 | |
| 7579880174 | core electrons | filled shells below valence electrons | 74 | |
| 7579880175 | Abbreviated electron configuration | • We write a shortened version of an electron configuration using brackets around a noble gas symbol and listing only valence electrons. abbreviate the last noble gas |  | 75 |
| 7579880176 | correlations with periodic table doc in blackboard | ... | 76 | |
| 7579880177 | define Electron configuration exceptions | Half filled as well as fully filled sub-levels are stable Cr,Mo - [Ar] 4s¹3d⁵ Cu,Ag,Au - [Ar] 4s¹3d¹⁰ (The examples given apply to the first element listed) | 77 | |
| 7579880178 | define paramagnetic Substance | substance with one ore more unpaired electrons. are attracted t magnetic fields (find by looking at electron config) | 78 | |
| 7579880179 | define diamagnetic substance | substance with only paired electrons repelled by magnetic fields (find by looking at electron config) | 79 | |
| 7579880180 | anions (in regards to electron configuration) | Nonmetals gain enough electrons to have config like the noble gas just past them on the periodic table (8 valence electrons) | 80 | |
| 7579880181 | Cations (in regards to electron configuration | electrons are lost from outermost shell Group A ions will loose electrons to have config close to the the noble gas behind it. for group B elements (varied ion states) the concept is the same, you just have to know the charge you're dealing with (lose the electrons with the hight n value (highest shell)) if all the electrons that need dropping aren't in that highest n shell you can drop down to the next highest and take some of those | 81 |
