then undergo these transitions, among others: (a) n = 6 → n=5 (b) n = 6 → n= 4 (c) n = 5 → n= 3 (i) Which transition produces a photon with the least energy? (ii) Which transition produces a photon with the highest frequency? (iii) Which transition produces a photon with the shortest wavelength?

3. (i) Define the term photon. Then, (ii) state whether a photon of blue light or red light has higher energy and (iii) explain how you made your determination. Be sure to (iv) include an equation that can justify your answer.

Which one is false?

How many orbitals in an atom can have each of the following designations?(a) 7s (b) 5d (c) 6p (d) n = 1

Ozone in the stratosphere absorbs ultraviolet light of wavelengths shorter than 320 nm, thus filtering out the most energetic radiation from sunlight.  During this absorption, an ozone molecule absorbs a photon, which breaks an oxygen-oxygen bond, yielding an oxygen molecule and an oxygen atom: O3(g) + hν → O2(g) + O(g)  (Here, hν denotes a photon.)  Suppose a flask of ozone is irradiated with a pulse of UV light of wavelength 275 nm.  Assuming that each photon of this pulse that is absorbed breaks up one ozone molecule, calculate the energy absorbed per mole of O2 produced, giving the answer in kJ/mol.

What is the frequency of a photon if the energy is 7.81 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)

Which of the following atomic electron transitions would emit a photon of light with the longest wavelength (λ)?   Group of answer choices   (1) n = 4 to n = 5 (2) n = 3 to n = 1 (3) n = 2 to n = 1 (4) n = 5 to n = 4 (5) n = 3 to n = 2

Which of the following quantum transitions of an electron in a hydrogen atom would emit a photon with the shortest wavelength?  Group of answer choices (a) : n = 1 to n = 4 (b) : n = 4 to n = 2 (c) : n= 4 to n = 3 (d) : n = 4 to n = 1 (e)    n = 2 to n = 4

What is the frequency of a photon if the energy is 7.05 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)

What is the frequency of a photon if the energy is 7.33 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)