A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm. Both of these transitions are to the same final state. Determine the energy of each emitted wavelength (in J). A E1 = 7.908 x 1019 J and E2 = 6.558 x10-19J B E1 = 5.908 x 1019 J and E2 = 5.558 x1o-19J E1 = 4.908 x 10-19 J and E2 = 4.558 x10-19) D E1 = 4.628 x 10-19 J and E2 = 4.968 x10-19J

< Question 12 of 65 Submit What is the energy of a photon with a frequency of 8.40 x 10¹4 s¹? (h = 6.626 × 10-³4 J. s)

Consider the following energy levels of a hypothetical atom:   E4   =   −1.0 × 10−19  J   E3   =   −5.0 ×10−19  J   E2   =   −1.0 × 10−18  J   E1   =   −1.5 × 10−18  J  When an electron drops from the E2 level to the E1 level, the atoms are said to undergo emission. Calculate the wavelength (in nm) of the photon emitted in this process.

A wave has a wavelength of 32.87 μm, determine its frequency. 9.121 x 1012 S-1 O 1.096 x 10-13 S-1 9.121 x 106 s-1 O 1.096 x 1013 S-1

52. Calculate the difference in energy (in joules) between a photon with λ= 687 nm and a photon with λ= 393 nm. Enter your answer in scientific notation.

A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm . Both of these transitions are to the same final state. Determine the energy of each emitted wavelength (in J).   E1 = 5.908 x 10-19 J and E2 = 5.558 x10-19 J   E1 = 7.908 x 10-19 J and E2 = 6.558 x10-19 J   E1 = 4.628 x 10-19 J and E2 = 4.968 x10-19 J   E1 = 4.908 x 10-19 J and E2 = 4.558 x10-19

When light of frequency 1.12 x 1015 s1 shines on the surface of cesium metal, electrons are ejected with a maximum kinetic energy of 4.04 x 10-19 J. Calculate the wavelength of this light (in nm). i 146 eTextbook and Media nm Calculate the binding energy of electrons to cesium metal (in J). i J Calculate the longest wavelength of light that will eject electrons (in nm). i nm

Using these data, find the experimentally determined value of Planck's constant, ℎh , and the threshold frequency, ?0ν0 , for silver.

4. A certain shade of green has a frequency of 530. THz. What is the energy of exactly one photon of light?

The energy of light photons varies with wavelength. Calculate the energy per mole of photons for each of the given colors of visible light. red light, A = 693 nm kJ mol green light, A = 547 nm E = kJ mol kJ blue light, A = 403 nm mol Splitting liquid water into hydrogen and oxygen requires an input of 286 kJ/mol. 286 kJ + H,O(1) – H, (g) + ¿O,(g)