Here is an energy level diagram that shows what happens when a photon of light is absorbed. Compare and contrast the energy level diagram with your representation in Q2.2. How does atomic structure change when a photon is absorbed? Energy Yu E5 (n=5) E4 (n=4) E3 (n= 3) E2 (n=2) E1 (n=1) Enter your answer here

Mark the following on the spectrum scale and indicate the region of the spectrum (IR, UV, etc) in which each lies. For each, find a more precise value for frequency and wavelength in standard units than you can read from the plot. (1) Bond vibration corresponding to a wavelength: 6.5 um (find E in J) (2) Energy required to break a CH bond: 413 kl/mol (Find A in nm) (3) Energy required to remove an inner electron from a C atom: 308 eV (Find 2 in nm) (4) One of the rotational frequencies of a molecule: 12 GHz 12,000 MHz (2in cmJ (5) lonization energy of hydrogen atom: 13.6 ev (a in nm, E in kF/mol) (6) Frequency of a radio station: 91.7 MHz (Find 2 in m) (7)The energy of the n=4 to n=2 transition in H atom (Find A in nm)

For each of the statements below, indicate whether it is true or false and explain your reasoning. (1-3 sentences) ( 1/ It takes more energy to ionize an electron from the 2s orbital than an electron from the 2p orbital in the Li2+ ion. 2/ The electron affinity of the Ne atom is larger than the electron affinity of the F atom. 3/ K* has a larger radius than Ar. 4/ For a diatomic molecule, in which the internuclear axis is the z-axis, the 3dz2 orbital cannot mix with the 2px orbital. 5/ The internuclear distance of O2 increases as it takes an additional electron to become O2.

This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: E energy C Which is the ground state? B A Use this diagram to complete the table below. How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the absorption line at the shortest wavelength? Which transition causes the absorption line at the longest wavelength? (pick one) 0 0 0 → 0 0-0