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Definition
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| X-ray diffraction provides info into: |
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Definition
| atomic and molecular structure |
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Term
| if Hv *v = nu* is over the "yield arrow" in a reaction: |
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Definition
| The reaction is being hit with light |
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Term
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Definition
| the distance in meters between two crests (lambda) of a wave |
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Term
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Definition
| the number of crests and troughs that pass over a specific amount of time. (nu) |
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Term
| The speed of light in a vacume (C) is equal to: |
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Definition
| Wavelength mulitplied by frequency |
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Term
| The relationship between the electromagnetic spectrum and frequency vs. wavelength: |
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Definition
| The leftmost portion has the shortest wavelength and the highest frequency while the rightmost has the longest wavelength and the lowest frequency. |
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Term
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Definition
ROYGBIV
red has the longest wavelength and lowest frequency
violet has the shortest wavelength and the highest frequency. |
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Term
| When do atoms give off light? |
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Definition
| When they're electrically excited (heated) |
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Term
| When an atom gives off light, the color of said light is dependent upon what? |
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Definition
| The wavelength of the light emitted and the particular atom that is being struck. (each atom emitts specific light frequencies) |
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Term
| What are the two types of light that can be produced by the atoms? |
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Definition
| Balmer (visible light) and Liman (UV light) |
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Term
| How can the light frequencies produced by atoms be tested? |
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Definition
| Using an atomic line spectrum |
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Term
| What does the Balmer-Rydberg equation determine? |
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Definition
| Where the lines (using the "test") appear in the spectrum |
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Term
| What is the Balmer-Rydberg equation for hydrogen? |
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Definition
| 1/λ = R [(1/m2) – (1/n2)] |
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Term
| In the balmer-rydberg equation, R is equal to what? |
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Definition
| the rydberg constant: 1.097 x 10–2 nm-1 |
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Term
| What are the 3 conditions/properties for n and m in the balmer-rydberg equation? |
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Definition
1. n must be greater than m.
2. the smallest number n is three, you use this to determine the longest possible wavelength
3. when n equals infinity, 1/n2 is equal to zero...this is used to determine the shortest possible wavelength |
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Term
| In the balmer-rydberg equation, when m=2, the light emitted is...? |
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Definition
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Term
| In the balmer-rydberg equation, when m=1, the light emitted is...? |
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Definition
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Term
| What two experiments support the theory that light acts as particles, and by whom were they performed? |
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Definition
| The black body radiation experiment by Max Planck and the Photoelectric effect by Einstein |
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Term
| Explain black body radiation |
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Definition
| If any metal is heated up enough, it will glow with an inversely proportional relationship between wavelength and light intensity. If light is a wave, this would be a continuous relationship, but in reality, the graphed line will peak and then suddenly drop off (after a certain wavelength, the intensity will drop) |
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Term
| Explain the photoelectric effect: |
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Definition
| If you shine light on a metal, electrons are ejected off of the surface only if the irradiation acquires the correct threshold value before the emition. (in other words, a certain amount of energy is needed to emit electrons) |
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Term
| What does planck's eqution say? |
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Definition
| Energy is equal to planck's constant mulitplied by frequency. (E=hv) |
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Term
| How do wavelength, frequency and energy relate? |
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Definition
| If a light has a low wavelength, it has a high frequency and a high energy...and vice versa |
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Term
| What does the hisenburg uncertainty principle state? |
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Definition
| There is no way to know the precise location and pathway of an electron. |
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Term
| Do electrons retain properties of a particle? |
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Definition
| They're not just particles floating around a nucleus, they have wavelike properties as well. |
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Term
| What does the shrodinger equation describe? |
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Definition
| An atom mathematically. Solving gives a wave function (orbital). If this is squared, it equals the probability of finding an electron in a specific place. |
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Term
| What is the principle quantum number and what does it tell us about an electron? Give an example. |
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Definition
N. It can be any integer, and relates to the size of an orbital.
ex: if n=2, there are 2 shells |
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Term
| What does L stand for, what does it tell us about an electron, and how does it relate to n? |
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Definition
L is the angular momemtum quantum number. It gives the 3D shape of an orbital. The value of l=0 when n=1.
For example: if n=1, l=0. If n=2, l can = either 0 or 1...etc |
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Term
| How does the orbital name relate to the value of l? |
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Definition
When l=0, the orbital is called s
when l=1, the orbital is called p
when l=2, " " d
when l=3, " " f
when l=4, " " g |
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Term
| What does Ml stand for, how do you define it numerically, and how does it relate to electrons? Give an example. |
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Definition
The magnetic quantum #. It defines the orientation of the orbital in space. ml is equal to the range between -L and +L.
If L=0 then ml=0, if L=1 then ml= -1, 0 or +1...etc |
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Term
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Definition
| the place in an pathway that has no electrons |
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Term
| Describe the orientation of the P orbital. |
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Definition
Two balloons tied together, Py= up/down, Px=horizontal, Pz="coming out at you"
Node where "balloons" connect |
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Term
| Describe the orientation of the s orbital. |
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Definition
| Spherical. 1 s= no nodes, 2s= 1 node...etc |
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Term
| What does ms stand for, explain its relationship to electrons. |
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Definition
| Spin quantum number, always two possibilities for spin, (+1/2) or (-1/2) |
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Term
| What is the Pauli exclusion principle? |
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Definition
| no two electrons in the same atom can have the same four quantum numbers. |
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Term
| What is electron configuration? |
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Definition
| The description of the electrons in each element on the periodic table |
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Term
| What are the three rules of electron configuration? |
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Definition
1. Fill the lower levels before the higher levels
2. Two electrons per level, each w/ opp. spins.
3. Degenerate electrons: place one electron in each level (same spin) until each level is half-full, then place the rest of the extra electrons with an opp. spin. |
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