1. (5 points) An electron in a hydrogen atom is initially at n=2 energy level. When the atom is exposed to 434.2 nm...
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...
1)Determine the wavelength of light emitted or absorbed by a hydrogen atom when an electron transitions from n = 9 to n = 5. Give your answer in units of nm. 2)An electron in a hydrogen atom absorbs 51.09 x 10 -20 J of energy. If the electron originated at energy level 2, to what level was it excited?
1. A hydrogen atom with its electron in the n = 5 energy level emits a photon of IR light. (i)[3 marks] Calculate the change in energy of the atom and (ii) [2 marks] Calculate the wavelength (in nm) of the photon.
When an excited electron in a hydrogen atom falls from n = 6 to n=2, a photon of violet light is emitted. If an excited electron in an Het ion falls from n = 5, which energy level must it fall to (nı) for violet light of a similar wavelength to be emitted? ni =
Determine the wavelength of light emitted or absorbed by a hydrogen atom when an electron transitions from n = 6 to n = 9. Give your answer in units of nm. An electron in a hydrogen atom absorbs 2.66 x 10 -20 J of energy. If the electron originated at energy level 5, to what level was it excited?
20. Calculate the wavelength of light (nm) released when an electron in a hydrogen atom transitions from energy level n=5 to energy level n=2 (7 points) (see back page for formula)
An electron in the n=7 level of the hydrogen atom relaxes to a lower energy level, emitting light of 2166 nm. What is the value of n for the level to which the electron relaxed? Express your answer as an integer.
In a hydrogen atom, an emission line is observed at a wavelength of 486 nm. If the electron was excited to an energy state n = 4, from what state was the electron excited? What was the minimum energy of the excitation light source to cause the initial absorption event? Note: The Rydberg constant is 1.097373 × 107 m
An excited hydrogen atom emits light with a wavelength of 397.2 nm to reach the energy level for which n = 2. In which principal quantum level did the electron begin? It would be very helpful if the last step could be over explained, thats where my answer is going wrong.
The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 and 102.5 nm. What is the quantum number of the initial excited energy level from which the electron falls?