Questions
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| Beryllium - 4 Protons, 4 Neutrons, 5 Electrons |
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| Carbon - 6 Protons, 6 Neutrons, 6 Electrons |
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| Oxygen 8 Protons, 8 Neutrons and 8 Electrons |
1: What is the atomic number for each of your models?
Oxygen:8
Beryllium:4
Carbon: 6
2. What is the atomic mass number for each of your models?
Oxygen: 15.994
Beryllium: 5.01262
Carbon:12.0107
3. In your models, which two subatomic particles are equal in number?
Protons and neutrons have the same amount of particles in an atom.
4.How would you make an isotope for one of your models? What would change with the model?
You can make an isotope for any atom by changing the number of neutrons that the atom has. When creating an isotope the number of protons stays the same, while the number of neutrons changes.
5. Considering the overall volume of your element models, what makes up most of the volume of an atom?
The volume is mostly made up of the Electrons, the protons and neutrons in the nucleus are such a small part of the atom that they don;t take up much space; where as the electrons are essentially orbiting the nucleus because of a positive force. The greater the charge of the nucleus the smaller the volume of the atom will be because the electrons are being pulled in closer to the nucleus.
6. For one of your models show with another image what happens when energy excites an electron.
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| Excited oxygen, one of the electrons have moved to a higher level of energy. |
7. Once the electron is excited, what do we typically observe when the electron returns to the ground-state?
The electron jumps to a higher energy orbital level when they absorb energy they drop down to a lower orbital when the energy is released. The energy is given off is called a photon, or a particle that represents the light or other electromagnetic radiation. The photon or giving off of light helps the atom re-stabilize and get back to its regular energy level. So essentially the atom gives off some sort of energy as light or heat to get rid of the extra energy to get itself back to normal.
8. Why are some elements different colors when they are excited?
Each element has a different number of valence electrons, when an atom either takes in a photon or gets rid of a photon it is jumping energy levels. When a photon is being released the atom must release energy. Like stated in my answer to question 7, when an atom is trying to get rid of energy it emits some sort of light or heat. When an atom emits light it will show the color of their dominant wavelength. Different atoms will show the color of their dominant wavelength. Different atoms will show at different wavelengths.
9. With the Fourth of July coming up quickly, explain how the colors of fireworks arise.
To start, fireworks need an oxygen-producer, fuel, binder, and color producer. There are two main parts in the color production in fireworks; Incandescence and Luminescence. Incandescence is light produced from heat, which causes the substance to become hot and glow. When the temperature of a firework is controlled the glow of it can be manipulated to the color you want, depending on the temperature and the timing that you have. Different metals, such as aluminum, magnesium, and titanium burn very brightly and are useful for increasing the temperature of a firework. Luminescence in the light produced using energy sources other than heat. This is what we were talking about in previous questions with an atom becoming excited and giving light from releasing the photons to re-stabilize the energy. When the electron return to a lower energy state the energy is released as a photon, the energy of a photon determines the wavelength or color. Below is a chart that i found online of the different elements used to make the colors of fireworks.
| Color | Compound |
| Red | strontium salts, lithium salts lithium carbonate, Li2CO3 = red strontium carbonate, SrCO3 = bright red |
| Orange | calcium salts calcium chloride, CaCl2 calcium sulfate, CaSO4·xH2O, where x = 0,2,3,5 |
| Gold | incandescence of iron (with carbon), charcoal, or lampblack |
| Yellow | sodium compounds sodium nitrate, NaNO3 cryolite, Na3AlF6 |
| Electric White | white-hot metal, such as magnesium or aluminum barium oxide, BaO |
| Green | barium compounds + chlorine producer barium chloride, BaCl+ = bright green |
| Blue | copper compounds + chlorine producer copper acetoarsenite (Paris Green), Cu3As2O3Cu(C2H3O2)2 = blue copper (I) chloride, CuCl = turquoise blue |
| Purple | mixture of strontium (red) and copper (blue) compounds |
| Silver | burning aluminum, titanium, or magnesium powder or flakes |
10. Explain the overall organizational structure of the periodic table.
The structure of the periodic table starts by listing the elements in increasing atomic number. The main body of the table is 18 by 7, with gaps to keep elements with similar properties together, such as the halogens and the noble gases. The periodic table below shows areas of the table in different colors. The colors represent the different groups that they have in the table. The groups are there to help predict the properties of various elements and relations between properties.
11. List two example elements for each of these groups or classes: Alkali Metals, Alkaline Earth, Halogens, Noble Gases, Transition Metals, Non-Metals, and Metalloid.
Alkali Metals
1. Lithium
2.Sodium
Alkaline Earth
1.Calcium
2. Beryllium
Halogens
1.Florine
2.Chlorine
Noble Gases
1.Helium
2.Neon
Transition Metals
1.Iron
2.Nickle
Non-Metals
1.Carbon
2.Oxygen
Metalloid
1.Silicon
2.Polonium
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