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Part A Find the excitation energy from the ground level to the third excited level for...
An electron in the hydrogen atom make a transition from the ground state to an excited...
An electron in the hydrogen atom make a transition from the ground state to an excited level by absorbing energy from a photon. The wavelength of the photon is 95.0 nm. What is the final level that the electron can reach?
9.6 A hydrogen atom in its ground state (n = 1) is excited to the n...
9.6 A hydrogen atom in its ground state (n = 1) is excited to the n = 5 level by absorbing photons. It then makes a transition to the n = 3 level and then from n = 3 level directly to the ground level. (a) What is the wavelength of absorbed photon? (b) What are the wavelengths of the emitted photons? [Answer: (a) 95 nm, (b) 1282 nm and 103 nm] Please show work and explain how. I do...
An electron in a 10.1-nm one-dimensional box is excited from the ground state into a higher-energy...
An electron in a 10.1-nm one-dimensional box is excited from the ground state into a higher-energy state by absorbing a photon of electromagnetic radiation with a wavelength of 13,950 nm. Determine the final energy state for this transition. 04 0 0 w Na Un 0 0 1 pts Question 24
4. An atom emits a photon with a wavelength of 872 nm when its electron moves from the n = 5 energy level to the n...
4. An atom emits a photon with a wavelength of 872 nm when its electron moves from the n = 5 energy level to the n = 4 energy level. From this fact, what can you can conclude? (Hint: drawing a diagram may be helpful) (A) This atom must emit lower energy light than the 872 nm light when moving from the n= 5 energy level to the n= 1 energy level (B) This atom's electron can transition from the...
A ground state hydrogen atom absorbs a photon of wavelength A. The atom's electron is excited...
A ground state hydrogen atom absorbs a photon of wavelength A. The atom's electron is excited to the orbital level n 6. What was the wavelength absorbed (in nm)?
1) If the electron starts out in the ground state and is excited to level E3...
1) If the electron starts out in the ground state and is excited
to level E3 by an incoming photon, what was the wavelength of that
photon (in nm)?
a) 95.4 nm
b) 102.5nm
c) 121.5nm
d) 136.7 nm
e) 182.3 nm
2) When the electron transitioned from E1 to E3 its orbital
radius increased by a factor of:
A) 1 (It didn’t change)
B) 2
C) 3
D) 4
E) 9
3) What is the longest wavelength the hydrogen...
tate energy Part A How much energy does the electron have initially in the nu4 excited...
tate energy Part A How much energy does the electron have initially in the nu4 excited state? Express your answer with the appropriate units. View Available Hint(s) E. = -1.36x10-19 J Submit Previous Answers ✓ Correct 7 of Part B ter What is the change in energy if the electron from Part A now drops to the ground state? Express your answer with the appropriate units. View Available Hint(s) AE = -2.04x10-18 J Son Previous Answers Correct MacBook Pro Q...
J 2 (1.2843x10 11. An electron absorbs energy to transition from the ground state to n...
J 2 (1.2843x10 11. An electron absorbs energy to transition from the ground state to n = 6. The electron then transitions to a lower energy level emitting a photon with a wavelength of 1094 nm. At this energy level the electron absorbs a photon with a frequency of 2.338x1014 Hz before transitioning back to the ground state and emitting a photon with a frequency of 3.156x1015 Hz (95 nm). What are the energy level transitions?
Suppose the radius of a particular excited hydrogen atom, in the Bohr model, is 0.212 nm...
Suppose the radius of a particular excited hydrogen atom, in the Bohr model, is 0.212 nm . What is the number n of the atom's energy level, counting the ground level as the first? n = When this atom makes a transition to its ground state, what is the wavelength λ in nanometers of the emitted photon? λ =
Suppose the radius of a particular excited hydrogen atom, in the Bohr model, is 1.32 nm
Suppose the radius of a particular excited hydrogen atom, in the Bohr model, is 1.32 nm. What is the number n of the atom's energy level, counting the ground level as the first? When this atom makes a transition to its ground state, what is the wavelength λ in nanometers of the emitted photon?
An electron in a 10.1-nm one-dimensional box is excited from the ground state into a higher-energy state by absorbing a photon of electromagnetic radiation with a wavelength of 13,950 nm. Determine the final energy state for this transition. 04 0 0 w Na Un 0 0 1 pts Question 24
4. An atom emits a photon with a wavelength of 872 nm when its electron moves from the n = 5 energy level to the n = 4 energy level. From this fact, what can you can conclude? (Hint: drawing a diagram may be helpful) (A) This atom must emit lower energy light than the 872 nm light when moving from the n= 5 energy level to the n= 1 energy level (B) This atom's electron can transition from the...
A ground state hydrogen atom absorbs a photon of wavelength A. The atom's electron is excited to the orbital level n 6. What was the wavelength absorbed (in nm)?
1) If the electron starts out in the ground state and is excited
to level E3 by an incoming photon, what was the wavelength of that
photon (in nm)?
a) 95.4 nm
b) 102.5nm
c) 121.5nm
d) 136.7 nm
e) 182.3 nm
2) When the electron transitioned from E1 to E3 its orbital
radius increased by a factor of:
A) 1 (It didn’t change)
B) 2
C) 3
D) 4
E) 9
3) What is the longest wavelength the hydrogen...
tate energy Part A How much energy does the electron have initially in the nu4 excited state? Express your answer with the appropriate units. View Available Hint(s) E. = -1.36x10-19 J Submit Previous Answers ✓ Correct 7 of Part B ter What is the change in energy if the electron from Part A now drops to the ground state? Express your answer with the appropriate units. View Available Hint(s) AE = -2.04x10-18 J Son Previous Answers Correct MacBook Pro Q...
J 2 (1.2843x10 11. An electron absorbs energy to transition from the ground state to n = 6. The electron then transitions to a lower energy level emitting a photon with a wavelength of 1094 nm. At this energy level the electron absorbs a photon with a frequency of 2.338x1014 Hz before transitioning back to the ground state and emitting a photon with a frequency of 3.156x1015 Hz (95 nm). What are the energy level transitions?
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