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?
The electron in a hydrogen atom falls from an excited energy level to the ground state...
An electron in an excited state of a hydrogen atom emits two photons in succession, the first at 2624 nm and the second at 97.20 nm, to return to the ground state (n=1). For a given transition, the wavelength of the emitted photon corresponds to the difference in energy between the two energy levels. What were the principal quantum numbers of the initial and intermediate excited states involved?
A hydrogen atom is excited from its ground state to the n = 4 state. The atom subsequently emits three photons, one of which has a wavelength of 122 nm . What are the wavelengths of the other two photons? Enter your answers in ascending order separated by commas. Lambda1,Lambda2=??
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?
Electrons in an unknown atom(not hydrogen) are excited from the ground state to the n=3 energy level. As these electrons make quantum jumps back to the ground state, photons of three different energies are emitted. The most energetic photon has an associated wavelength of 62.2 nm and the least energetic photon has an associated wavelength of 207 nm. What is the associated wavelength of the other type pf photon? The answer is 3-1 (20 eV), 3-2 (6 eV) and 2-1...
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...
please show work on paper 1.1 (opts). When the electron in a hydrogen atom falls from an excited energy level to the third energy level, a photon with a wavelength of 1005 3 nm is emitted. What is the principle quantum number of the original state?
The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. How much energy does the electron have initially in the n=4 excited state?
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...
When an electron of an excited hydrogen atom descends, from an initial energy level (ni) to a lower (nf), characteristic electromagnetic radiation is emitted. The Bohr model of the H-atom allows the calculation of ?E for any pair of energy levels. ?E is related to the wavelength (?) of the radiation according to Einstein's equation ( ?E = [(hc)/?]). Distinct series of spectral lines have been classified according to nf: Lyman series:nf=1 (91<?<123 nm; near-UV). Balmer series:nf=2 (365<?<658 nm; visible)....