In qualitative terms, how does Bohr's model account for the atomic spectrum of hydrogen? More than one selection may be correct. O The energy released when an electron drops from a higher to lower orbit appears as a photon with the appropriate frequency. O The energy released when an electron drops from a higher to lower orbit appears as a photon with energy equal to the energy difference between the two orbits. O Electron moves around the nucleus along orbits. O When a hydrogen atom absorbs energy, as it does when an electric discharge passes through it, the electron stays in the orbit having n = 1. O Electrons are found in orbits of arbitrary energy. O The energy released when an electron drops from a higher to lower orbit appears as a photon with an arbitrary frequency. O When a hydrogen atom absorbs energy, as it does when an electric discharge passes through it, the electron is raised from the orbit having n = 1 to a higher orbit, to n= 2 or n = 3 or even higher.

Can you explain this question then give the correct answer?

Enter a numeric response. In the Bohr model, how many photons are emitted when an electron moves from the # = 4 to the n = 3 orbit, and then from the n=3 to the n = 2 orbit? When an electron moves from n = 4 to n = 3, and then from n = 3 to n=2, photons are released.

A B 2 3 n=4 Hydrogen Atom Use the Bohr model of the hydrogen atom to determine the properties of the photon that will be emitted by each of the above transitions (by completing the table below). Transition Photon Energy (J) Photon Frequency (Hz) Photon Wavelength (nm) A 1 2 C Which of these transitions would produce light that you could see with your eyes? What color would you see? Which of these transitions would produce light that would damage your skin and/or eyes?

A liquid is exposed to infrared radiation with a wavelength of 9.51 × 10-4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 40.32 J of heat? number of photons =

According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 2 to n = 3 is ________ the energy necessary to excite an electron from n = 3 to n = 4.

A liquid is exposed to infrared radiation with a wavelength of 3.10 x 10-4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 52.94 J of heat? number of photons =

> Question Completion Status: QUESTION 4 Roaches for sale | C... For Sale/Trade/Wan... * Tarantulas CSL Behring Hell Let Loose TR St... Indicate which three of the following statements about the electron in a hydrogen atom are true by checking the box in front of each true statement. The atom is in the ground state when the electron is in the n=1 level. Energy is released when the electron is excited from the n=1 level to the n=3 level. A shorter wavelength of light is emitted when the electron moves from the n=3 level to the n=2 level than when the electron moves from the n=4 level to the n=2 level. Energy is always released when an electron relaxes. A lower frequency of light is emitted when the electron moves from the n=3 level to the n=2 level than when the electron moves from the n=4 level to the n=2 level. The atom is stable when the electron relaxes to the n=2 level.

Rank the following transitions in a hydrogen atom in order from the smallest change in electron energy to the greatest change. Explain your answer. n=4 -> n=2 n=4 -> n=3 n=2 -> n=1

Students at College of the Canyons performed a hydrogen emission lab, using a simulator program. The simulator showed four different kinds of photons in a visible light spectrum: blue, orange, red, and yellow. (alphabetical order) Which photon shows the longest wavelength? Which light has the highest frequency? O longest wavelength: red light, highest frequency: blue light O longest wavelength: blue light, highest frequency: yellow light longest wavelength: blue light, highest frequency: orange light longest wavelength: red light, highest frequency: red light