Find the binding energy of the hydrogen electron for states with the following principal quantum numbers. (Note the binding energy is just the absolute value of the Energy level, the energy required to remove the electron from that state to infinity.)

Draw to careful scale an energy-level diagram for hydrogen for levels with n=1, 2, 3, 4, inf. Show the following on the diagram: (a) the limit of the Lyman series, (b) theHb line, (c) the transition between the state whose binding energy (= energy needed to remove the electron from the atom) is 1.51 eV and the state whose excitation energy is 10.2 eV, and (d) the longest wavelength line of the Paschen series.

Chapter 39, Problem 044 A hydrogen atom in a state having a binding energy (the energy required to remove an electron) of -1.51 eV makes a transition to a state with an excitation energy (the difference between the energy of the state and that of the ground state) of 10.200 eV. (a) What is the energy of the photon emitted as a result of the transition? What are the (b) higher quantum number and (c) lower quantum number of the transition producing this emission? Use -13.60 eV as the binding energy of an electron in the ground state. (a) Number Units (b) Number Units (c) Number Units

Answer the following. (a) Write out the electronic configuration of the ground state for nitrogen (Z = 7). 1s22s22p11s22s22p2    1s22s22p31s22s22p41s22s22p51s22s22p6 (b) Write out the values for the set of quantum numbers n, ℓ, m, and ms for each of the electrons in nitrogen. (In cases where there are more than one value, enter the positive value first. Enter positive values without a '+' sign in front of them. Include all possible values.) 1s states n =   ℓ =   m =   ms =   ms =   2s states n =   ℓ =   m =   ms =   ms =   2p states n =   ℓ =   m =   ms =   ms =   m =   ms =   ms =   m =   ms =   ms =