Copper has a work function (Φ) of 4.70 eV. What is the longest wavelength of light, in nm, that will cause the ejection of electrons? (1 eV=1.6 × 10⁻¹⁹ J)

Bohr's model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr's model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 2 to n = 1. Submit an answer to four significant figures ninitial Mfinal = R Rm = 1.09678 x 107 m-'

Is this set of quantum numbers possible? n = 2, l = 1, ml = 0, ms = +1/2

What is the maximum number of orbitals that can be identified by the following set of quantum numbers? Note that in cases where the set of quantum numbers is not "allowed," the answer will be zero. n= 4, l= 3, ml= +4 orbital(s) n= 4, l= 2, ml= –1 orbital(s)

Part 1 The electron in a hydrogen atom is initially located in the shell where n=1. (A) The hydrogen atom is illuminated with radiation that has a wavelength of 97.2 nm. What is the energy (in J) of a single photon from that radiation? (B) After absorbing the photon described in (A), the electron becomes excited and travels from n=1 to another shell. After this transition, the electron is in the shell where n= (Show all your work for (A) and (B) Part 2 In Part 1, the electron in the hydrogen atom left n=1 after absorbing a photon. In which direction did the electron travel? a) towards the nucleus b) away from the nucleus c) into the nucleus

Do number 5

According to the Bohr model for a hydrogen atom, what is the energy di erence between the ground state (n = 1) and each of the rst (n = 2), second (n = 3), and third (n = 4) excited states? (Note: the electron always starts in the ground state). What wavelength of light, in nanometers, is needed to cause each of these excitations

Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number (), the magnetic quantum number (m₂), and the spin quantum number (mg) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. oooooo ☐ n = 3₂ l = 2, me = 2, ms = + 1²/2 n = 4, l = 2, me = 3, mg = − 1/1/ n = 3, l = —2, m₂ = 2, mg = − ½/2 n = 5, l = 4, me = 1, ms = - 1²/22 n = 2, l = 1, mę = 0, ms = 0 n = 4, l = 4, m₂ = −1, ms = − 1/12

The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.Which of the following statements are true and which are false. 1. it takes less energy to ionize the electron from n=3 than it does from the ground state.2. The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.3. the electron is farther from the nucleus on average in the n=3 state than in the ground state.4. The first excited state corresponds to n=3.5. The wavelength of light emitted when the electron drops from n=3 to n=2 is shorter than the wavelength of light emitted if the electron falls from n=3 to n=1.

A hydrogen atom absorbs a photon with a wavelength of 1094 nm and causes an electron to make a transition from an unknown n1 to a final n2 = 6.   Part A Calculate frequency of the absorbed photon in units of s-1.       Part B Calculate the energy change in the atom (ΔEatom in J) upon absorption of the photon.     Part C Calculate the value of n1