A Be3+ ion begins with an electron at n=3. Then one photon of light (λ = 68.38 nm) is absorbed. What is the new n value for the excited electron? ni=3 ni should equal 6. Not sure how to get there.
A Be3+ ion begins with an electron at n=3. Then one photon of light (λ =...
Be3+ is a one-electron ion. It is a beryllium atom that has lost 3 of its electrons. Minimum energy of a photon that would ionize this ion= -217.6 eV The wavelength of the photon that would excite Be3+ from its ground state to its first excited state= 7.56 nm Calculate the kinetic energy of the photoelectrons if radiation of 4.0 nm of wavelength falls on an ensemble of Be3+ ions.
Calculate the wavelength, in nm, of the light emitted when a Be3+ ion makes a transition from the n=4 to the n= 1 state. Hint: The atomic number of Be3+ is Z=4, and it has one electron.
The electron in a Be3+ ion is in an orbit with n=6. What is the energy of the electron in this orbit? Use k=2.179×10−18J. Your answer should have four significant figures.
The single electron on a Li2+(g) atom is excited to the n=7 orbital. When the electron falls to the n=3 orbital a photon of light is emitted by the atom. What is the wavelength of this photon of light? (a) 496 nm (b) 1005 nm (c) 112 nm (d) 91.2 nm (e) 4468 nm ** solutions says answer is (C) but not sure how they got that
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 =
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.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the ground state. What happens to the light and to the electron? Group of answer choices a. The light is not absorbed and the final energy of the electron is -1312 kJ/mol. b.. The light is absorbed and the final energy of the electron is −328 kJ/mol. c.. The light is not absorbed and the final energy of the electron is −1050 kJ/mol. d.. The...
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)
An electron confined to a box absorbs a photon with wavelength λ. As a result, the electron makes a transition from the n = 1 state to the n = 3 state. (a) Find the length of the box. (Use the following as necessary: c, h, me, and λ.) L = (b) What is the wavelength λ' of the photon emitted when the electron makes a transition from the n = 4 state to the n = 2 state? (Give...
4. An N'°ion has atomic number Z 7, one electron, and is in the - 7 state initially, a. What is the energy of this state in eV? b. A photon of energy E-13.056 eV is absorbed by this atom. What is the nevw energy of the atom? c. What is the value of n now?