4. Consider only the four following quantum levels for the H atoms (n=4, n=3, n=2, andn=1). The emission spectrum of an excited H atom will consist of transitionsbetween these levels.a. How many emission lines are possible, considering only the four quantumlevels above?plactgeinb. Photons of the highest energy will be emitted in a transition from the levelwith n=to the level with n=inU elste iqgieatealM aSes 1onori yn n0Inebute yilenevhow olmebes elri no ponc. The emission line having the longest wavelength corresponds to atransition from the level with n=to the level with n=

A) Total number of emission spectral line Total lines = n(n-1)/2 = 4 ×(4-1)/2 = 6

- many emission lines are possible, considering only the four quan ls above? otons of the highest energy will be emitted in a transition from the to the level with n= bypes anebute vilanovinU alste iqqleatealM how olmebeos elit no 26 1onori yn e emission line having the longest wavelength corresponds to a nsition from the level with n3D to the level with n=

- many emission lines are possible, considering only the four quan ls above? otons of the highest energy will be emitted in a transition from the to the level with n= bypes anebute vilanovinU alste iqqleatealM how olmebeos elit no 26 1onori yn e emission line having the longest wavelength corresponds to a nsition from the level with n3D to the level with n=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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

See similar textbooks

Similar questions

23. What is the energy change (in J) and wavelength (in nm) of light emitted when an electron transitions from n = 5 to n = 2 in the hydrogen atom? A: -4.578 x 10-1⁹; 434 Ins
The threshold frequency vo describes the smallest light frequency capable of ejecting electrons from a metal. Determine the minimum energy Eo of a photon capable of ejecting electrons from a metal with vo = 5.81 x 1014 s-1. Eo = What is the maximum kinetic energy KEelectron of electrons ejected from this metal by light with a wavelength of 265 nm? KEelectron
-21 This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10 You can find the meaning of any SI prefix in the ALEKS Data tab.) energy (zJ) 1400 1200 1000 800 600 400 200 0 UB If the electron makes the transition shown by the red arrow, from C to B, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. C -A Use this diagram to complete the table below. μm x10 X
When a hydrogen electron is excited from level n=3 to level n=4, a proton of wavelength ___ m is absorbed. Calculate E one for the n= 3 energy level
Which of the following transitions in the Bohr hydrogen atom model affords emission of the highest-energy photon? (R, = 2.18 x 10-18 J) %3D O ni = 6 → nf = 3 O ni = 6 → nf = 1 O ni = 1→ nf = 6 O ni = 3→ nf = 6
The energies, E, for the first few states of an unknown element are shown here in arbitrary units. 1 2 4 00 ... E -96 -45 -21 -15 A gaseous sample of this element is bombarded by photons of various energies (in these same units). Match each photon to the result of its absorption (or lack thereof) by an n = 1 electron. Photon Energy Result A 96 75 C 69 D 51 Answer Bank electron ejected n = 1 to n = 4 not absorbed n = 1 to n = 2 n = 1 to n = 3
g. Diagram the electron transition that occurs when photons having energy equal to 5.00 x 10-¹⁹ J are released n = 5 n = 4 n = 3 n = 2 n=1
In regards to Rhydberg's equation, which transition on Hydrogen atoms would you expect to have the SHORTEST wavelength? 3-->4 2-->3 2-->break free 1-->5
The energy of a photon emitted when an electron underwent a transition to n = 1 energy level was 2.043x10-18 J. What was the initial energy level for the electron?
The work function for uranium is 5.768 X 10-19 J. Determine the kinetic energy of an electron that has been emitted from uranium if light of wavelength of 249. nm is shown upon the metal. KE = X 10-18 J Formatting Note: Your Answer X 10-18 J <-- not type this part in your answer. 10-18 J is assumed. Do
What is the frequency of light emitted when a hydrogen electron drops from the n=2 energy level (E2= -5.5 x 10-19 J) to the n=1energy level (E1 = -22 x 10-19 J)?a. 16.5 x 10-12 Hzb. 3.0 x 1010 Hzc. 1.2 x 10-21 Hzd. 2.5 x 1015 Hze. 1.1 x 10-28 Hz
The energies, E, for the first few states of an unknown element are shown here in arbitrary units. 1 3 4 ... E -84 -36 -16 -12 ... A gaseous sample of this element is bombarded by photons of various energies (in these same units). Match each photon to the result of its absorption (or lack thereof) by an n = 1 electron. Photon Energy Result A 84 В 68 C 63 D 48 Answer Bank not absorbed n = 1 to n = 3 electron ejected n = 1 to n = 2 n = 1 to n = 4 100