The threshold frequency vo describes the smallest light frequency capable of ejecting electrons from a metal. Determine the minimum energy Eo of a photon capable of ejecting electrons from a metal with vo = 3.54 × 1014 s-1. E, = J What is the maximum kinetic energy KEelectron of electrons ejected from this metal by light with a wavelength of 285 nm? KEelectron = J

The element hydrogen, using the Rhydberg equation, can be  used to calculate the energy difference between n shells.   Calculate the FREQUENCY in Hz and the wavelength in nanometers for the emission of energy for the electron excited to n =425 and then emitting light to n = 1

Which of the following statements is FALSE regarding transitions (between electronic energy levels) of hydrogen atoms? The frequency of the n = 1 to 3 transition is А higher than that of the n = 1 to 2 transition. The wavelength of the n= 1 to 3 transition is В higher than that of the n= 1 to 2 transition Above a certain frequency, called the ionization frequency, electrons are emitted from hydrogen atoms. C Below a certain frequency, called the ionization frequency, transitions of hydrogen atoms occur at a discrete set of frequencies.

Enter numeric value The first ionization energy of a potassium atom is 0.696 aJ (attojoules). What is the frequency and wavelength, in nanometers, of photons capable of just ionizing potassium atoms? Values for constants can be found in the physical constants table. V = λ = Assuming an ionization efficiency of 68.0%, how many such photons are needed to ionize 1.00 × 10¹6 atoms? number of photons: 8-1 nm

Give the chemical symbol for the element with the ground-state electron configuration [Ne]3s?3p?. symbol: Determine the quantum numbers n and e and select all possible values for m, for each subshell of the element. 3s 3s The possible values of me for the 3s subshell are O-3,-2,-1,0, +1, +2, +3 -1,0,+1 -2,-1,0,+1,+2 3p 3p e = The possible values of me for the 3p subshell are -2,-1,0,+1, +2 -1,0,+1 O -3,-2, -1,0, +I,+2, +3

What is the energy (in J) of a photon required to excite an electron from n = 2 to n = 5 in a He⁺ ion?

What is the wavelength (in nm) of the photon emitted when the electron in a single-electron lithium atom in an excited state makes the transition from the n=7 state to the n=3 state?

What is the wavelength of the electromagnetic radiation emitted from a hydrogen atom when the electron undergoes the n=5 transition n=3 to ?

Calculate the ionization energy (eV) for a 'hydrogen-like' atom with one electron and Z=3 from the ground state. Submit an answer to three significant figures. eV 1 2 3 4 C 7 8 9 +/- х 100 +