The first five energy levels of the hydrogen atom are at n = 1, − 13.6 eV; n = 2, − 3.4 eV;n = 3, − 1.51 eV; n = 4, − 0.85 eV; n = 5, − 0.54 eV. A hydrogen discharge lamp givesan infrared spectrum that includes a sharp line at a wavelength of 4 µm, coming from electronsexcited by the discharge to a higher level, and then jump down to a lower level. Determine theenergy lost by these electrons, and identify the higher and lower levels involved.

What is the frequency of light that allows an electron to be released from a metal that has a work function of 4.136. ev? 1 x 10^15 1.5 x 10^(-15) 2 x 10^12 0.9 x 10^14

Use the table to determine the energy in eV of the photon emitted when an electron jumps down from the n = 4 orbit to the n = 3 orbit of a hydrogen atom. Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n E 0.053 nm -13.60 ev 0.212 nm -3.40 ev 0.477 nm -1.51 eV 4 0.848 nm -0.85 ev

FINA Energles of the lowest electron levels in the sodium atom n = 6 n = 5 n = 4 n = 3 n = 2 n = 1 -1.10 eV -1.40 eV -1.60 eV -1.90 eV -3.00 eV -5.10 eV A photon with a wavelength of 393 nm enters a cool cylinder of sodium gas. This photon will cause the sodium's electron to jump from state 1 to 2 have no affect on the sodium atoms. cause sodium to emit a violet photon. cause the sodium's electron to jump from state 2 to 4.

n = 1 E = -13.6 ev n= 4 E = -0.85 ev n=5 n= 2 E = -0.54 ev E = -3.4 ev n= 3 E = -1.51 ev a) At what wavelength (in meters) does the n = 3 → 2 transition of hydrogen occur?

Angular momentum and Spin. An electron in an H-atom has orbital angular momentum magnitude and z-component given by L² = 1(1+1)ħ², Lz = m₁h, 1 = 0,1,2,..., n 1 - m₁ = 0, ±1, ±2, ..., ±l 3 S² = s(s+1) h² = =h²₁ 4 Consider an excited electron (n > 1) on an H-atom. The total angular momentum ] = L + Š, whose magnitude and z-component follow a similar dependence to some quantum numbers j and m; as J² = j(j + 1)ħ², Jz = mjħ 1 S₂ = m₂h = ± = h Where j and m; are quantum numbers which assume values that jumps in steps of one such that j is non-negative and −j ≤ m¡ ≤ j. For a given quantum number 1, what are the (two) possible values for j? Clue: we can use the vector sum relation of angular momenta, then consider the z-component only.

What amount of energy is needed for an electron to jump from n = 1 to n = 3? (h = 6.626 x 10-34,1 eV = 1.6 x 10-19 J)

A photon is absorbed by a hydrogen atom in the ground state. n=3 n=2 n=1 n=7 n=6 n=s n=4 n n 11=3 n=2 n=1 + E = 0 Es=-0.544 eV E4-0.850 eV E3 = -1.51 eV E2 = -3.40 eV E1-13.6 eV Ground state If the electron is boosted from to the n = 2, what was the energy of the photon? Give your answer in electron volts (eV). ev

Consider the following energy level diagram and determine the wavelength of line 1 and line 2 observed in the emission spectrum respectively. 10 eV 6.0 eV 2.0 eV 1 2 (a) 310 nm, 155 nm (b) 240 nm, 120 nm (c) 325 nm, 165 nm (d) 420 nm, 210 nm

An electron is orbiting around a nucleus in a hydrogen atom in Bohr 's model with kinetic energy of 8.64✕10-20 J. Determine the allowed orbit in this atom.