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Chem Test 3
| Question | Answer |
|---|---|
| Energy of one photon equation (v) | E=hv |
| Energy of one photon equation | E=hc/λ |
| Speed of light equation | c=λv |
| Planck's constant | 6.63*10^-34 |
| Photoelectric Effect | When electromagnetic radiation or light hits a metal at a high frequency and electrons are ejected from the surface of the metal. Einstein explained by saying light is a quanta of energy that are like particles (photons). ^ frequency of light = faster e^- |
| Light as a wave | Waves of electromagnetic radiation. Light can be reflected, refracted, and diffracted. |
| Light as a particle | Photoelectric effect, electromagnetic energy comes in packets/quanta called photons which is proportional to frequency bc the higher the frequency the faster the electron and the shorter the wavelength the more e^- ejected. |
| Difference between light as a wave and light as a particle | The wave nature of light states that light can behave as an electromagnetic wave, whereas the particle nature of light states that light consists of particles called photons. |
| Bohr Model | Using the structure of a solar system, Niels Bohr created an inaccurate model of an atom called the planetary model or Bohr model that shows fixed electrons revolving around a dense nucleus. |
| Quantum Model | A model of an atom made by Erwin Schrodinger that is the modern understanding of an atom. This uses atomic orbitals to explain the uncertain locations of electrons in the atom. |
| Differences between Bohr Model and Quantum Model | B: electrons behave as particles, Q: the electron has both particle and wave behavior. B: e^-s are in fixed locations, Q: e^-s have indefinite location in the electron cloud. B: can only be applied to the hydrogen atom, Q: can be applied to all atoms |
| Similarities between Bohr and Quantum Models | Both explain the structure of an atom, both consider a heavily charged nucleus and electrons revolving around it. |
| Heisenberg Uncertainty Principle | It is impossible to know both the velocity or momentum and the position of a particle, such as a photon or electron, at the same time. Doesn't apply for ordinary sized objects. |
| First Quantum Number | Principle QN: "n" is an integer that describes the energy level of an e^-. n=0,1,2,3,4...; first # in electron config. |
| Second Quantum Number | Angular QN: "l" describes the shape of a sublevel within an energy level (type of orbital). s sublevel: sphere l=0; p sublevel: peanut/dumbbell l=1; d sublevel: double peanut/two dumbbells l=2; f sublevel: flower l=3. 1st letter in electron config. |
| Third Quantum Number | Magnetic QN: describes the orientation of the orbital within a sublevel, -l<ml<l; count to the 2nd # in electron config following the 3 guiding principles. |
| Fourth Quantum Number | Electron Spin: ms=+-1/2 |
| Aufbau Principle | electrons occupy the lowest energy orbital first, then move to the next. first fill 1s, then 2s, then 2p, then 3s... |
| Pauli Exclusion Principle | Spin in one orbital must be different: up down not up up or down down. no two electrons can have the same 4 electronic quantum #s. |
| Hund's Rule | single before double, all singles have the same spin |
| Principle Number of Electrons | |
| Order of spdf | |
| Relationship between frequency and wavelength | |
| Relationship between energy and wavelength |
Created by:
undercoverkookie68
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