Consider the Bohr-model description of a hydrogen atom. (a) Calculate E2 - E1 and E10 - E9 . As n increases, does the energy separation between adjacent energy levels increase, decrease, or stay the same? (b) Show that En+1 - En approaches (27.2 eV)/n3 as n becomes large. (c) How does rn+1 - rn depend on n? Does the radial distance between adjacent orbits increase, decrease, or stay the same as n increases

Consider the Bohr-model description of a hydrogen atom. (a) Calculate E2 - E1 and E10 - E9 . As n increases, does the energy separation between adjacent energy levels increase, decrease, or stay the same? (b) Show that En+1 - En approaches (27.2 eV)/n3 as n becomes large. (c) How does rn+1 - rn depend on n? Does the radial distance between adjacent orbits increase, decrease, or stay the same as n increases

Similar questions

Answer question throughly and with much detail as possible.
Chapter 39, Problem 017 An electron in the n, state in the finite potential well of of Figure (a) absorbs 650 eV of energy from an external source. U U(x) Ug L. (a) Using the energy-level diagram of Figure (b), determine the electron's kinetic energy after this absorption, assuming that the electron moves to a position for which x > L.
Consider a Bohr model of doubly ionized lithium. (a) Write an expression similar to E, = -13.6/n² eV for the energy levels of the sole remaining electron. (Use the following as necessary: n.) 122.4 E, v ev n° (b) Find the energy corresponding to n = 5. (Enter your answer to at least one decimal place.) -4.89 ev (c) Find the energy corresponding to n = 3. (Enter your answer to at least one decimal place.) -13.6 ev (d) Calculate the energy of the photon emitted when the electron transitions from the fifth energy level to the third energy level. Express the answer both in electron volts and in joules. 8.71 V ev 1.395e-18 (e) Find the frequency and wavelength of the emitted photon. 6.2e15 Your response differs from the correct answer by more than 100%. Hz 48 Your response differs from the correct answer by more than 10%. Double check your calculations. nm (f) In what part of the spectrum is the emitted light? O visible light region O infrared region O gamma ray region O x-ray region…
In the Balmer series, for the Hydrogen atom, a weak transition is observed at 397nm. the value of the same transition for the Li2+ ion would correspond to an energy value of: a) 28.1 eV, b) 122.4 eV, c) 2.5 eV, d) 13.3eV, e) 119.9 eV
Suppose you recently discovered a hydrogen like element that has only one electron orbiting around a nucleus containing a proton and a neutron. You found the ground state energy of the electron to be -16 eV. What will be the energy of this electron when it is on the excited state shown in the sketch? Note that all other possible intermediate states are shown by dashed lines. Electron is here Ground state 1.0 eV 16 eV - 1.0 eV -4.0 eV 4.0 eV
Please answer (i), (v), and (vi). Thank you! (i) Using Bohr model for atomic hydrogen, obtain energy levels for the 2s, 3s and 3p states in the actual number with the unit of [eV]. We consider a transition that electron in the 3p state emits a photon and make a transition to the 2s state. What is the frequency v of this photon ? (ii) Now we do not include electron spin angular momentum, and just estimate an effect of a magnetic field B on this transition (Normal Zeeman effect) with orbital angular momentum. How many lines of optical transition do we expect ? What is the interval of the frequency in the field B = 0.1 Tesla ? (iii) In this situation, we do not expect transition from 3s to 2s state if the electron is initially in the 3s state, Explain the reason. (iv) We now consider an effect of magnetic field B to a free electron spin (not in Hydrogen, but a free electron). The magnetic field of B = 1.0 Tesla will split the energy level into two (Zeeman) levels. Obtain the level…
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 =