Emission Spectroscopy - Embrace Challenge发射光谱-接受挑战

Emission SpectroscopyAccording to the Bohr atomic model, electrons orbit the nucleus within specific

Emission Spectroscopy According to the Bohr atomic model, electrons orbit the nucleus within specific energy levels. These levels are defined by unique amounts of energy. Electrons that h__e the lowest energy are found in the levels closest to the nucleus. Electrons of higher energy are located further away. If an electron absorbs enough energy to bridge the "gap" between energy levels, the electron __y jump to ahigher level. Sin__ this change results in avacant lower orbital, the configuration is unstable. The "excited!” electron releases its newly acquired energy and falls back to its initial or ground state. Often, the excited electrons get enough energy to __ke several energy level transitions. When these electrons return to their ground state, several distinct energy emissions occur. The energy that electrons absorb is often of ather__l or electrical nature, and the energy that electrons emit when returning to ground state is electro__gnetic radiation. Sometimes this electro__gnetic radiation can be picked up by our eyeballs as it is energy in the form of visible light. In 1900, __x Planck stu___d visible emissions from hot glowing solids. He proposed that light was emitted in "packets" of energy called quanta, and that the energy of each packet was proportional to the frequency of the light w__e. According to Einstein and Planck, the energy of the packet could be expressed as the product of the frequency () -34 E= h. of emitted light and Plank's constant, h, 6.626 x10 Js: W__elength is related to frequency in the equation, c= ,where stands for w__elength. is the lower case Greek letter for L, and is called lambda. Frequency and w__elength h__e an inverse 8 relationship, which equals c, the speed of light, 3.00 x10 m/s. If we know the w__elength of the light, then we can calculate the frequency of the light. On__ we h__e calculated the frequency, then we can use Plank’s constant to calculate how much energy, in Joules, is in the w__elength. For example, red colors tend to h__e w__elengths around 700 __. So, if we do the __th: c= f c=f so 89 3.00 x10 mx10 __= 700 __ s1 m 14-1 4.29 x10 s= the frequency of the red light Now using E= h -3414-1 we get E= (6.626 x10 Js)(4.29 x10 s) –19 =2.69 x10 J Although this number really has no meaning to us, if we were to calculate various w__elengths of light, we would find out that blue light which has ashorter w__elength, roughly 400 __, has more energy. There are two w__elengths that you might be familiar with, 680 __ and 700 __. During photosynthesis, photo__nters are able to absorb light that has these two w__elengths. The chloroplast is able to take the light energy and