(a) What is the wavelength of the photon needed to excite an electron from E₁ to E4? x 10 (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? x 10 m x 10 J (c) When an electron drops from the E3 level to the E₁ level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process. m

For light with a wavelength of 350 nm and with an intensity of /= 10-8 W/m², what is the number of photons/(m²s) in the light beam?

The quantum state of an electron in an atom is described by quantum numbers n = 6, ℓ = 5, and mℓ = 2. The z-component orbital angular momentum of the electron is measured to be x × h/2π, where h is Planck’s constant. What is the number x (remember to use the scientific notation)?

The energy levels of an electron in an atomic-like system are given by the expression En = -C/n^p C > 0, p > 0 n = 1,2,3... If the ionization energy for the electron in its ground state is 30 eV, and a photon of wavelength 50 nm is emitted when the electron makes a transition from the third level to the ground state, find C and p.

The ground state energy of hydrogen atom is -13.6 eV. (i) What is the potential energy of an electron in the 3rd excited state? (ii) If the electron jumps to the ground state from the 3rd excited state, calculate the wavelength of the photon emitted.

Based on your answer in Question 7, when light with a wavelength of 198 nm strikes the surface of tin metal, electrons are ejected with a maximum kinetic energy of 2.9 x 10-19  J. What is the binding energy of these electrons to the metal?

A photon with a wavelength of 4.16 nm strikes a surface and emits an electron with kinetic energy of 124.6 eV (electron volts). What is the binding energy of the electron in J?