Calculate the energy when an excited electron in the hydrogen atom falls from the transitions below. What color of light is emitted?
a) n=5 to n=2
b) n=3 to n=2
Calculate the energy when an excited electron in the hydrogen atom falls from the transitions below....
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 =
4. When a hydrogen atom is bombarded, the atom may be raised into a higher energy state. As the excited electron falls back to the lower energy levels, light is emitted. What are the three longest-wavelength spectral lines emitted by the hydrogen atom as it returns to the n = 1 state from higher energy states? Give your answers to three significant figures. The lowest possible state, n = 1, corresponds to the electron in its smallest possible orbit; it...
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?
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. Consider a photon of light emitted from a hydrogen atom when an excited electron relaxes from n=6 to n=3; calculate the energy (5 pts), frequency (3 pts) and wavelength (3 pts) of this light. In what portion of the electomagnetic spectrum does this photon of light appear? (1 pt)
What wavelength (in nanometers) of light is emitted when an electron in a hydrogen atom falls from the n=4 to the n=3 energy level? What wavelength (in nanometers) of light is emitted when an electron in a hydrogen atom falls from the n=4 to the n=3 energy level? nm Check
21. Calculate the wavelength and frequency of light that is emitted when an excited electron in the hydrogen atom falls from n=5 to n=2?
An electron in an excited hydrogen atom makes two transitions. First the electron drops from the n=5 to the n=2 state, then the electron drops from the n=2 to the n=1 state. 1. Calculate the frequency of the photon emitted in the first transition. a) 2.91x1014 Hz b) 3.91x1014 Hz c) 4.91x1014 Hz d) 5.91x1014 Hz e) 6.91x1014 Hz 2. Calculate the momentum of the photon emitted in the second transition. a) 1.44x10-27 kg-m/s b) 2.44x10-27 kg-m/s c) 3.44x10-27 kg-m/s...
35. When the electron in a hydrogen atom falls from its first excited energy level to the ground state energy level, a photon with wavelength l is emitted. A proton having this same wavelength would have a velocity of a. 3.87 m/s. b. 5990 m/s. c. 1.21 ´ 10-7 m/s. D. 3.26 m/s. e. 5.99 m/s. answer is D
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?