Homework Answers
Narrow lines means that the spectrum lines represent specific values of energy and not brad ranges that you would find on a band spectrum. This is agreement with Bohr's theorem that says energy levels are quantised meaning that all of the energy levels are integral values of the same value of energy. This along with the first statement tells us that Bohr's theory is a consequence of Line spectra
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3. Explain how the existence of narrow lines in atomic spectra is consistent with Bohr's theory...
4.66 Explain how the Bohr model of the atom accounts for the existence of atomic line...
4.66 Explain how the Bohr model of the atom accounts for the existence of atomic line spectra. 167 TATI. . 4.72 In order for hydrogen atoms to give off continuous spectra, what would have to be true? 4.56 It always takes energy to remove an electron from an atom, no matter what n shell the electron is in. Also, the higher the n, the more energy an electron starts out with (a) Explain why it takes energy to remove an...
Why are molecular absorbance spectra broad, while atomic absorbance spectra are narrow (“lines”)? What are the...
Why are molecular absorbance spectra broad, while atomic absorbance spectra are narrow (“lines”)? What are the major components of an absorbance instrument and what are their roles in spectral acquisition? Are absorbance measurements more qualitative or quantitative in nature (what useful information can we get from them)?
-obtain wavelengths for the hydrogen emission lines and then calculate the energy levels according to bohr's...
-obtain wavelengths for the hydrogen emission lines and then
calculate the energy levels according to bohr's theory
- determine wavelengths in nm associated with following
transitions of the H atom:
nf = 1 with ni = 2, 3, 4
nf = 2 with ni = 3, 4, 5
nf = 3 with ni = 4, 5, 6
Hydrogen יויויין יויויויויויויוי 400 500 600 700 Fig e: Hydrogen emission spectra for calculations 1 1 Rydberg Equation: -R, a n 1 1...
7. There are actually 2 purple lines in hydrogen's atomic spectra, one at 410 nm that...
7. There are actually 2 purple lines in hydrogen's atomic spectra, one at 410 nm that is very hard to see and one at 436 nm. What electronic transition do you think is responsible for the line at 410 mm? Explain
How are the lines in atomic emission spectra produced? Group of answer choices electrons absorb a...
How are the lines in atomic emission spectra produced? Group of answer choices electrons absorb a specific amount of energy and become excited electrons release a specific amount of energy, moving to a higher energy state electrons release a specific amount of energy, moving to a lower energy state electrons absorb a specific amount of energy, moving to a lower energy state
Please explain. 0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single elec...
Please explain.
0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single electron system well. But the energy level for orbitals change when as you add a second and more electron. In a single electron system, there are (a)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (b) sub-level(s) in the atom. In a multi-electron system, (c)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (d)sub-level(s) in the atom. Bohr was never...
Question 1 The atomic spectra of calcium and sodium were shown in experiment 9. These spectra...
Question 1 The atomic spectra of calcium and sodium were shown in experiment 9. These spectra help explain their color results for flame test. What feature(s) would you expect from the atomic spectra of potassium? Explain your reasoning. Question 1 options: Since the flame test for potassium is violet, there should be a significant number of emission lines toward the 500 nm end of the spectrum. Since the flame test for potassium is violet, there should be a significant number...
I was having trouble with some lab question on atomic emission spectra. Also answer the following...
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
Name: Christina Gonzalez PARTI - Hydrogen, energy levels, and atomic line spectra Lab Worksheet - Atomic...
Name: Christina Gonzalez PARTI - Hydrogen, energy levels, and atomic line spectra Lab Worksheet - Atomic Theory 1.a) Electrons in an atom are more stable than free electrons. This is why the energy levels of electrons in atoms are negative (free electrons are defined as having an energy of zero). Calculate the energy of a hydrogen electron in the 4th shell, in J. b) Calculate this energy in kJ/mole. 2. Calculate the energy for n=1, 2, 3, and 5 as...
Illustrate with a picture how a H 1s atomic orbital and a F2p a form bonding...
Illustrate with a picture how a H 1s atomic orbital and a F2p a form bonding and antibonding molecular orbitals in the HF m 3. mustrate 4. What is the bond order for HFT 5. Is the HF molecule predicted to be paramagnetic or diamagnetic? Use the MO diagram to predict where the electron density in the HF bond lies, closer to the H atom or closer to the F atom? Explain. 6. 7. Now draw the Lewis structure for...
4.66 Explain how the Bohr model of the atom accounts for the existence of atomic line spectra. 167 TATI. . 4.72 In order for hydrogen atoms to give off continuous spectra, what would have to be true? 4.56 It always takes energy to remove an electron from an atom, no matter what n shell the electron is in. Also, the higher the n, the more energy an electron starts out with (a) Explain why it takes energy to remove an...
-obtain wavelengths for the hydrogen emission lines and then
calculate the energy levels according to bohr's theory
- determine wavelengths in nm associated with following
transitions of the H atom:
nf = 1 with ni = 2, 3, 4
nf = 2 with ni = 3, 4, 5
nf = 3 with ni = 4, 5, 6
Hydrogen יויויין יויויויויויויוי 400 500 600 700 Fig e: Hydrogen emission spectra for calculations 1 1 Rydberg Equation: -R, a n 1 1...
7. There are actually 2 purple lines in hydrogen's atomic spectra, one at 410 nm that is very hard to see and one at 436 nm. What electronic transition do you think is responsible for the line at 410 mm? Explain
Please explain.
0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single electron system well. But the energy level for orbitals change when as you add a second and more electron. In a single electron system, there are (a)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (b) sub-level(s) in the atom. In a multi-electron system, (c)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (d)sub-level(s) in the atom. Bohr was never...
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
Name: Christina Gonzalez PARTI - Hydrogen, energy levels, and atomic line spectra Lab Worksheet - Atomic Theory 1.a) Electrons in an atom are more stable than free electrons. This is why the energy levels of electrons in atoms are negative (free electrons are defined as having an energy of zero). Calculate the energy of a hydrogen electron in the 4th shell, in J. b) Calculate this energy in kJ/mole. 2. Calculate the energy for n=1, 2, 3, and 5 as...
Illustrate with a picture how a H 1s atomic orbital and a F2p a form bonding and antibonding molecular orbitals in the HF m 3. mustrate 4. What is the bond order for HFT 5. Is the HF molecule predicted to be paramagnetic or diamagnetic? Use the MO diagram to predict where the electron density in the HF bond lies, closer to the H atom or closer to the F atom? Explain. 6. 7. Now draw the Lewis structure for...
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