37. One of the lines in the atomic hydrogen line emission spectrum falls in the visiblelight region and has a wavelength of 410 nm.a. Explain the meaning of line spectrum.b. Give the name for this spectrum series.c. Determine the transition of the electron involved.Answer:c. 6

(a). Meaning of Line Spectrum A line spectrum is a type of spectrum that consists of discrete lines,…

Answered: 37. One of the lines in the atomic…

Chemistry

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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D. Draw the full orbital energy diagram for a neutral atom with 25 total electrons. Place energy on the y-axis. E. What are the four quantum numbers for an electron in the highest energy sublevel of the atom from part d (based on filling)? If multiple values are degenerate for a quantum number, write all of them.
The quantum number which describes the nominal energy of an electron and also its average distance from the nucleus is the a. angular momentum quantum number b. magnetic quantum number c. principal quantum number d. spin quantum number
Using complete subshell notation, match the predicted electron configuration of each of the following atoms. (match one from the top (letter) to one at the bottom (number). a. Sb b. P c. Sm d. V e. C 1. 1s22s22p63s23p3 2. 1s22s22p63s23p63d104s24p64d105s25p3 3. 1s22s22p2 4. 1s22s22p63s23p63d104s24p64d105s25p66s24f6 5. 1s22s22p63s23p64s23d3
Provide the following information for a photon in the Ultraviolet region of the Electromagnetic Spectrum. a. Calculate the energy if the photon has a wavelength of 292 nm. b. Calculate the frequency if the photon has a wavelength of 298 nm.
6. Using the spdf notation, predict the electronic configuration of each of the following atoms: a. 8 O b. 16 S c. 40 Ca d. 71 Lu
Please don't provide handwritten solution ... Explain why the answer is C
9
What is the number of angular nodes in each case? a.) 1s (angular nodes) b.) 3s (angular nodes) c.) 3d (angular nodes)
5. An electron in a hydrogen atom makes a transition from ann= 2 orbital to an n = 5 orbital. a. For this electron transition, is energy being absorbed or released? Circle one. ABSORBED RELEASED b. Calculate the energy difference for this transition and the wavelength (in nanometers) of the photon involved in this transition.
а. For a hydrogen-like atom, how do the energies of the 2s and 2p subshells compare? Provide reasoning to support your answer (it will be helpful to list all of the interactions between subatomic particles). b. Write the ground-state electron configuration and draw an orbital diagram for a neutral atom containing 5 electrons. C. Explain what the orbital approximation is in the context of this 5 electron atom. d. For this atom with 5 electrons, how do the energies of the 2s and 2p subshells compare? Provide reasoning to support your answer (it will be helpful to list all of the interactions between subatomic particles). You should include references to shielding and penetration in your response. As the energies in multi-electron atoms must be approximated, explain how variational principle could be used to determine said energies. е.
The lowest energy level in an atom is a. the absolute zero temperature. b. the ground state. c. the ionization level. d. responsible for Doppler shifts. e. the energy level from which the Paschen series of hydrogen originates.
The AE for the electronic transition is H-atom from n=2 to n=3 is a. 12.11 eV b. 1.9 eV c. 10.21 eV d. 13.61 eV e. 3.40 ev

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37. One of the lines in the atomic hydrogen line emission spectrum falls in the visible light region and has a wavelength of 410 nm. a. Explain the meaning of line spectrum. b. Give the name for this spectrum series. c. Determine the transition of the electron involved. Answer: c. 6