Three ???

Recently we did a lab on the light in fd and C blue dye in Gatorade. We look to see the percent transmittance between different variations of the stock solution and water mixture. In anatomy we have been learning about neurons and the brain and central nervous system. We watched a movie about the grain. It was really cool we saw how panic can produce hormones that distrubs the stimulus of the brain and makes it not be able to focus on its normal functions. I am stuck struggling with the stoichiometry. I just get confused on where to put the units over what. Overall I enjoyed this unit I find it fairly easy to understand I'm actually understanding the electron configuration and wavelength and frequency is in emission spectrum and its very relieving that I can actually understand something in AP chemistry. I am planning to keep up my practices with the math equations and stoichiometry so I can better my struggles and perform better on tests and quizzes and overall get a higher grade in this class.

Shell Activity Blog

• What is Coulomb's law? Coulombs law is the basic idea of electricity. It looks at forces created between two charged objects. As distance increases the forces of electric fields decrease. When there are two charged particle, an electric tone is created. If there are longer charges the forces will be longer. 

• Explain how distance and charge impact the energy to remove an electron.  Why do both 'charge' and 'distance' need to be included in your explanation? Distance and charge are inversely related to each other. The closer the electron is to the nucleus (closer distance) the stronger the force. So the closer the electron is the more energy is needed to overcome the force of attraction between electron and proton. The further the electron, there is less energy needed.

• Explain why removing an electron is an endothermic process.and why it isn't an exothermic process. Removing an electron is an endothermic process because energy is absorbed to break the bond between electron and proton.

• How is the amount of energy needed to remove an electron related to how electrons are organized within an atom? The amount of energy needed to remove an electron is related to how electrons are organized within an atom.When the electron jumps to a lower suborbital it emits a photon, emitting light, This absorbs energy which csuses the emission of a photn t make the atom stable. 

• How is the amount of energy needed to remove an electron related to, different than, or the same as, the energy to excite an electron? The energy needed to remove one or more electrons from a neutral atom to form a positively charged ion is a physical property that influences the chemical behavior of the atom. By definition, the first ionization energy of an element is the energy needed to remove the outermost, or highest energy, electron from a neutral atom. 

Light and Electons

• What is the relationship between wavelength, frequency and energy of light?

             As wavelength increases, frequency decreases. Both are inversely related to one another. And light of energy is                    inversely related to wavelength. So the longer the wavelength the lesser the energy

• How does light emission demonstrate electron transition?

              The color emitted corresponds to the frequency and wavelength  and energy. This results to a specific electron                      transition between different energy levels.

• What is significant about the different colors of light observed in spectral lines?

               All colors of light have different energies,When a electron moves from an excited state to a closer level to the                      ground state this jump emits photons which causes an emission in light. If the electron goes from the ground                        state to a more excited state it absorbs light causing a blacks space or line in the spectral line

• How can light be used to measure energy transitions of electrons?

              Light can be used to measure energy transitions of electrons by measuring the corresponding wavelengths.

Three Questions

Recently I have learned about the brain and its functions. I learned about the organize a shin of the central nervous system which includes the brain and spinal cord. The protection of the central nervous system . The disruption to neural functions, the metabolic processes, the layers of the cerebrum,and the sensory and motor areas of the cerebral cortex. In my AP Chemistry class I learned about light and electrons. Also a little brief review on frequency and wavelength. Recently we just completed a lab over the electrons and light in relate the white to the electron transition in the production of the light observed. Also I've recently completed a Play Doh brain model. I am planning to start to review my stoach and problem solving in my chemistry class so I can have a greater understanding of the whole concept and finally figure out what I need to learn and what I need to work on as the upcoming AP Chemistry test approaches, so I can get a good grade on that.

Light and Electrons

The higher the frequency the shorter the wavelength and the lower the frequency  the longer the wavelength. The longer the wavelength the lesser the energy . Wavelength and energy of light are indirect. Wavelength is also indirect with frequency. So frequency and energy of light are directly related.  light emission demonstrates electron transition by spectral lines. To produce these spectral lines you need to have an electron. Each electron produces one spectral line. For example a single atom of hydrogen cannot produce all for hydrogen spectral lines simultaneously. This is because hydrogen only contains one electron. Hydrogen gas can emit more than one spectral lines simultaneously because this is due to the multiple atoms used in your hydrogen gas example because there are more electrons there can be different spectral lines. The significance about the different colors of light observed in spectral lines are the wavelength. Each wavelength has its own unique color range. Red wavelength range range is from 625 to 740 nanometers, oranges range is from 592 to  625 nanometers, yellows range from 565 to 590 centimeters Greens range from 522 to 565 nanometers, blues range from 440 to 520 nanometers, and violets range from 382 to 440. There are different types of hues or shades of each color and they all each emitt different wavelengths. Every color has different energy; violets have the highest energy and the Reds have the lowest energy. So do to violet highest energy they have the shortest wavelength and red  has the longest wavelength because they have the lowest energy. During electron transition energy can either be released or absorbed. When energy is released they are returning to their lower energy levels as they get closer to the nucleus its "ground state." when energy is absorbed it goes to higher energy levels to do this it has to absorb enough energy to break the attraction between the nucleus and the electron. The spectral lines for atoms are unique, different wavelengths are emitted to different atoms. If an electron moves from energy level 5 to energy levels to this electron transition releases energy. The electron moves from a higher energy state to a lower energy state. In this electron transition light is released because the energy is absorbed. The longer the wavelength the lower the frequency the shorter the wavelength the higher the frequency wavelength and frequency are indirect. Light can be used to measure energy transitions of electrons by looking at the wavelength ranges. An example is hydrogen electron transition that involves light with a wavelength in the ultraviolet range which is it 10 to four hundred nanometers can be measured n= 6 to 1. A hydrogen electron transition that involves light with a wavelength in the infrared range which is a thousand 2106 nanometers can be directed as n equals 6 to n  equals 5. 

Three questions

Recently in my anatomy class we learned about muscles. And we took a test over the muscular system yesterday. In chemistry we are reviewing thermochemistry. I hope to not procrastibate in this next upcoming semester and finish my classes with all as.