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ADV CHEM
Unit 3 Test 11/4
| Question | Answer |
|---|---|
| electromagnetic spectrum | distribution of electromagnetic radiation according to energy |
| does red have a long or short wavelength | long wavelength |
| does purple have a long or short wavelength | short wavelength |
| ROY G BV | red, orange, yellow, green, blue, violet |
| speed of light (c) | 3.00 x 10^8 m/s |
| wavelength | (lamda) the distance between corresponding points on adjacent waves |
| frequency | (nu) the given amount of waves passing a certain point in an certain amount of time, usually 1 second |
| what is wavelength expressed in (label) | meters |
| what is frequency expressed in (label) | s^-1, or Hz |
| 1 nm = ? meters | 10^-9 meters |
| photoelectric effect | emission of electrons from metal when light shines on metal |
| quantum | the min amount of energy gained or lost by an atom |
| Plancks Constant (h) | 6.626 x 10 ^-34 J/s |
| formula for energy | E = hv |
| when can photons release electrons from metal | when they have more energy |
| what did Einstien say about Planck's Theory | while light exhibits wave-like particles, it can also be thought of as a stream of particles |
| photon | a particle of electromagnetic radiation that has zero mass and is carrying an quantum of energy |
| ground state | lowest energy state of an atom |
| excited state | an atom has a higher energy state than its ground state |
| what happens when an excited state return back to its ground state | gives off energy in the form of light |
| formula for measure of light being let off when electrons change state | E= R (z^2/n^2)-(z^2/n^2) |
| relationship between wavelength and frequency | inverse |
| relationship between frequency and energy | direct |
| relationship between energy and wavelength | inverse |
| R = | -2.178 x 10^-18 |
| when energy is absorbed by electrons... | the energy will be negative |
| when energy is released by electrons... | the energy will be positive |
| electromagnetic system (order from short wavelength to long wavelength) | gamma rays, x-ray, ultraviolet light, visible, infrared light, microwaves, radio waves |
| in what order do final and initial energy level go in the Rydberg equation (n) | final then initial |
| n= | energy level |
| z= | atomic number |
| two things all electromagnetic radiation have in common | speed (3.00 x 10^8) and the ability to travel through a vacuum |
| quantum leap refers to | the jumping of electrons on energy levels |
| sublevels in an atom | s, p ,d ,f |
| shape of s sublevel | spherical |
| shape of p sublevel | peanut |
| shape of d sublevel | double peanut |
| shape of f sublevel | flower |
| orbitals in s sublevel | 1 |
| electrons in s sublevel | 2 |
| orbitals in p sublevel | 3 |
| electrons in p sublevel | 6 |
| orbitals in d sublevel | 5 |
| electrons in d sublevel | 10 |
| orbitals in f sublevel | 7 |
| electrons in f sublevel | 14 |
| electrons configuration | arrangement of electrons around an atoms nucleus |
| quantum mechanical model findings | electrons are located on very specific energy levels there is no exact path around the nucleus estimated the probability of finding electrons in a certain position |
| 3 terms that describe the location of an electron | energy level sublevel orbital |
| how many electrons can an orbital hold | 2 |
| Aufbau Principle | electrons occupy orbitals of lower energy first |
| Pauli Exclusion Principle | two electrons can occupy the same orbital only by having opposite spins (one up arrow, the other a down arrow) |
| Hund's Rule | in a set of orbitals, the electrons will fill the orbitals in a way that it would give the max amount of spins (fill all orbitals before doubling up) |
| valence electrons | outermost energy level |
| valence electrons determine | how an atom would react |
| positive electron (ion) | remove one electron for each positive charge |
| negative electron (ion) | add one electron for each negative charge |
| isoelectric | electron configurations are the same |
| exceptions to the Aufbau principle | d^4 and d^9 configurations |
| noble gas notation | use last novle gas located in periodic table before element. |
Created by:
stella_koe
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