The Bohr equation applies to any 1 electron atom or ion, though the Rydberg constant changes depending on nuclear charge, reduced mass and other factors. For an He* ion the Rydberg constant is R4He = 2.19176x10 18J. If a He+ ion with an electron in the n=4 level absorbs a photon of wavelength 2153 nm, in what energy level %3D does the electron end? 2 07 1

It is easy to understand how two electrons (one with spin up, one with spin down) can fill the 1s shell for a helium atom. How is it possible that eight more electrons can fit into the 2s2 p level to complete the 1s2s22p6 shell for a neon atom?

Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number (e), the magnetic quantum number (m,), and the spin quantum number (m,) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. n = 2, l = 1, mę = -1, mş = 1 n = 3, l = 1, mę = 1, mş = - Un = 2, l = 2, mẹ = 0, ms = - n = 5, l = 3, mẹ = -3, ms = - n = 4, l = 2, mẹ = 3, m, = + %3D O n = 3, l = -1, mẹ = 1, m, = -

What is the wavelength in nm of a photon emitted from an H atom if an electron transfers from n=6 to n=3   RH = Rydberg constant = 1.097 x 10 -2  nm-1