| pm_flame_test.pdf |
| am_flame_test.pdf |
33 Comments
AM! Christina, Hunter, and Abbey
9/18/2012 12:03:06 am
We believe that the flame changes colors from the electrons gaining energy from the heat, switching orbitals, cooling off, and then returning to their original position. While returning, they release photons which are seen in light rays, creating the different flame colors. The flame colors are determined by the amount of metal ions being burned.
Christina, Abbey, and Hunter.. Again
9/25/2012 12:05:25 am
When the electrons heat up, they move from lower energy levels to higher energy levels. When they move back to their original positions, they release electromagnetic radiation. This has different wavelengths, which determines the color of the flame.
Christina,abbey, and hunter
9/25/2012 12:23:19 am
The bigger the wavelength, the lower the energy and frequency. The smaller the wavelength, the higher the energy and frequency.
Jake and Allison (a.m.)
9/18/2012 12:03:36 am
The different colors of light are produced because when then electrons of the atom are heated, they gain and lose energy. This change in energy levels gives off the light.
Jake and Allison
9/25/2012 12:23:06 am
Color is the portion of the visible electromagnetic spectrum; it is radiant energy within the range of infrared and ultraviolet. We believe that the electrons inside the atom are emitting photoelectric energy when a light is shone on it. The enter guy from the eLements getting excited and changing their energy state causes the rays of color to be given off.
J and A
9/25/2012 12:25:32 am
*the energy from the electrons getting excited and grounded cause the rays of colors to be given off because of different wavelengths and frequencies.
Kayla, Andrew, Chris
9/18/2012 03:44:11 am
We believe that the amount of electrons an atom has affects the color of the flame because when the electrons are heated, they go into an excited state causing the flame to change colors. The transferred energy of the electron creates a photon (light particle) while going through the flame. When the atom comes out of the flame, it regains its energy and the flame goes back to its original color.
Andrew, Chris, Kayla
9/25/2012 03:43:27 am
Different atoms react differently with the color spectrums and spectral lines. Some atoms bring out different spectral lines than others do. This would give off the different colors that are seen with different elements.
Andrew Chris Kayla
9/25/2012 04:10:28 am
The hotter it gets, the faster the electrons move, causing there to be more energy.
Krista, Bailey, Davanna, Laurel
9/18/2012 03:48:21 am
We think that this happens becuase the electrons in each metal are heated so they gain energy when in the flame and lose the energy by releasing a photon when they exit the flame. Different colors are produced by different frequencys of light, so the different amount of electrons in each salt release a different amount of light (frequency of light), causing different colors.
Laurel Payne
9/24/2012 03:45:47 am
"Metals" change to "Salts"
Krista, Bailey Davanna, Laurel
9/25/2012 03:38:09 am
The change in the levels of the electrons each have spectral lines unique to the number of the electrons.
Laurel Payne
9/25/2012 03:49:07 am
Each spectral line corrisponds with a certain frequency/wavelength of light, leading to particular colors being seen for each element.
Krista, Laurel, Davanna, Bailey
9/25/2012 04:09:21 am
As wavelength increases, energy and frequency decrease. As energy increases, frequency increases and wavelength decreases. while frequency increases wavelength decreses and energy increases.
Amanda, Zeke,and Lee
9/18/2012 03:55:26 am
We believe that the color of the flame changes because the electrons give off a photo , a wave of light, when they lose energy and jumping back into their original orbit. The electron jumps to the next orbit because it gains energy from the heat of the flame. The wave color is different in each salt because different metals were used, potasium
Amanda, Zeke, and Lee
9/18/2012 04:01:48 am
We believe that the color of the flame changes because the electrons give off a photon, a wave of light, when they lose energy and jump back to their original orbit. The electron jumps to the next orbit because the heat of the flame gives energy to the electron. The color of the flame is different in each salt because different metals were used used, potassium, lithium, strontium, and copper.
Amanda, Zeke, and Lee
9/25/2012 03:47:11 am
The amount of energy given off when the electrons jump back down to their original level gives off a different color because the frequency of the photons differ. The more energy given off from the electron jump, the higher the frequency is, and the each color has a different frequency level.
Amanda, Zeke, and Lee
9/25/2012 04:10:34 am
The more energy the electrons give off the higher the frequency is going to be be while the wavelength is going to be smaller. The less energy the the electrons give off, the larger the wavelength is going to be while the frequency is going to be smaller.
Sara and DOUGLAS >:O
9/18/2012 05:19:56 am
When the chemical is sprayed into the flame, the electrons become heated. When heated, electrons become "excited," and need to move to a higher energy level. In order to do this, they move to an outer orbital (as orbitals farthest away have the most energy). However, when the electron needs to return to its ground state, it moves back to an orbital closer to the nucleus. When it moves, it releases the energy it had previously gained in the from of photons a.k.a. light waves. The wave has a specific wavelength which corresponds to a certain color on the color spectrum of light, resulting in the color difference we see when the flame is sprayed.
Sara and Megan
9/25/2012 12:04:40 am
When electric charges are sent through the tube, electrons become "excited," from this added energy, and need to move to a higher energy level. In order to do this, they move to an outer orbital (as orbitals farthest away have the most energy). However, when the electron needs to return to its ground state, it moves back to an orbital closer to the nucleus. When it moves, it releases the energy it had previously gained in the from of photons a.k.a. light waves. The wave has a specific wavelength which corresponds to a certain color on the visible light spectrum, resulting in the color difference we see when the gas's electron's are excited.
Sara and Megan
9/25/2012 12:28:20 am
When there is a low amount of energy, the wavelength tends to be large, but the frequency is low. When there is a large amount of energy, the wavelength is smaller but the frequency increases.
Brendan Bruce and Carly
9/18/2012 05:53:04 am
Brendan Bruce and Carly
9/25/2012 03:46:13 am
They get excited, not just from heat, but from anything that causes the electrons to jump rings, (i.e. electricity)
Bruce Brendan and Carly
9/25/2012 04:11:09 am
the energy varies from the mixture so therefor the wavelength and color do too
Ben and Katie
9/18/2012 08:59:59 am
As the number of electrons in each compound vary, different amounts of energy will be released on contact with the flame, thus producing various colors.
Ben and Katie
9/24/2012 11:54:36 pm
As the number of electrons in each compound vary, the form which excites them (heat, electricity) causes them to excite and release energy (photons), producing color.
Ben and Katie
9/25/2012 12:25:38 am
Wiith high frequency comes high energy and small wavelengths. With low frequency comes low energy and large wavelengths. Energy is needed to make the frequency higher.
Megan and Austen (a.m)
9/18/2012 09:04:32 am
We think that as the atoms are being heated, the electrons are becoming excited. This allows the electrons to move to different shells, gaining energy.Then, when the electrons return to thier original position (ground state), this energy is released in the form of light. Since each element has a different spectrum of colors that can be emitted in this situations, there will be a different color for each element heated.
Sara and Megan
9/25/2012 12:05:13 am
When electric charges are sent through the tube, electrons become "excited," from this added energy, and need to move to a higher energy level. In order to do this, they move to an outer orbital (as orbitals farthest away have the most energy). However, when the electron needs to return to its ground state, it moves back to an orbital closer to the nucleus. When it moves, it releases the energy it had previously gained in the from of photons a.k.a. light waves. The wave has a specific wavelength which corresponds to a certain color on the visible light spectrum, resulting in the color difference we see when the gas's electron's are excited! :)
Rachel, Faith, Dave
9/24/2012 03:46:10 am
The quantem jumps cause photons to be released. We know that red is the lowest color on the color spectrum, which explains why fire is naturally red/orange. (it takes less energy to make red.) The heat gives the energy to the electrons and the different levels of energy produce different colors.
Rachel, Dave, and Faith
9/25/2012 04:10:12 am
High energy produces high frequency and small wavelengths.
Madison, Nicole, Wyatt p.m.
9/24/2012 03:46:17 am
We believe the electrons become excited when the heat hits them, which causes them to emit a photon.
Madison, Nicole, Wyatt
9/25/2012 04:09:56 am
When the energy increases, the wavelength decreases and the frequency increases. Leave a Reply. | ArchivesSeptember 2013 Categories |
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