04-Anatomy of an Atom Name: Lab Section 3· The Bohr model provided insight into
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04-Anatomy of an Atom Name: Lab Section 3· The Bohr model provided insight into an electron's behavior within an atom. Experimental results like the absorption or emission spectra of an element brought further credence to his theory. The figure below (see chapter 4 of lecture textbook), presents the result one would observe if a Barium (Ba) salt was burned in a flame. If the green light emitted from the flame were passed through a prism, and allowed to shine on a black screen, one would observe several discrete spectral lines that correlate with discreet wavelengths of light (each line having its own color . These "emitted" spectral lines are the end product of electrons releasing energy in the form of light (i.e. emission) after the electrons were initially "excited" by the flame ast electrons absorbed the heat energy (i.e. absorption). In lecture, we discuss the fact that electrons reside in certain "home" energy levels. If these electron absorb enough energy, they can temporarily transition to a higher energy levels. When these elevated electrons are ready to move to a lower energy level (or back to its "home" energy level, called its ground state), the electron needs to release this energy in the form of light (thus the emitted spectral lines). Electron transitions that release energy within the visual range of the light spectrum are the only transitions that can be observed by the human eye. Light passes through a slit Prism Film (14 spectral lines) Barium light spectrum Use the discussion above (and info in chapter 4 of your textbook), to answer the following questions: a) How many e transitions are presented in the barium light spectrum? b) Is the resulting Barium light spectrum absorbed or emitted energy? c) Why are there different color lines presented in the Barium light spectrum? d) What is the significance of the blue and red spectral lines, in terms or energy? What is the significance of the blue and red spectral lines in terms of an electrons movement between the energy level(s)? e) 3Explanation / Answer
a. Since the emission spectra has 14 lines, each line is a result of transition of an electron from excited state to ground state there are 14e- transitions
b. As the spectral lines are due to the emission of energy absorbed during the excitation the lines are due to emitted energy.
c. During the de excitation of electrons from higher energy levels to its ground state the emit energy that has been absorbed during excitation which will be of different wavelengths for different electron de excitation. hence they give different colors to the spectral lines.
d. The colors of spectral lines is because they are in vissible region of the light spectrum. The vissible region contains 7different colors like violet, indigo, Blue, green, yellow, orange, red. The energy of thes colors decreases as we move from violet to red. Hence blue color has higer energy than red.
e. The blue spectral lines indicate that the energy required for this excitation of electrons between the energy levels is high. I,e the energy gap between the two energy levels involved in the excitation is large. So electron movement requires more energy.
Red spectral lines indicate the energy required for this excitation of electron is small and hence the energy gap between the two energy levels involved in the excitation is small. So electron movement requires less energy.
f. O2- = 1s2 2s2 2p6
Si = 1s2 2s2 2p6 3s2 3p2
Ca2+ = 1s2 2s2 2p6 3s2 3p6 4s0
N = 1s2 2s2 2p3
N3- = 1s2 2s2 2p6
Ar = 1s2 2s2 2p6 3s2 3p6
Li+ = 1s2 2s0
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