Q) A hydrogen atom is initially in the groundstate, (i.e., n = 1 level), absorbed a photon, and asa result of this absorption, a transition occurredfor the electron and ended at the n = 4 level.A- What is the frequency of thephoton? *Your answerB- If the electron makes spontaneousemission and comes back to theground state by going through allenergy levels between them. Whatare the possible frequencies of thephotons emitted during this process?

"Since you've have asked more than one questions, we'll solve the first one for you. Please post the…

Q) A hydrogen atom is initially in the ground state, (i.e., n = 1 level), absorbed a photon, and as a result of this absorption, a transition occurred for the electron and ended at the n = 4 level. A- What is the frequency of the photon? *

Q) A hydrogen atom is initially in the ground state, (i.e., n = 1 level), absorbed a photon, and as a result of this absorption, a transition occurred for the electron and ended at the n = 4 level. A- What is the frequency of the photon? *

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter6: Electronic Structure And The Periodic Table

Section: Chapter Questions

Problem 66QAP: Consider the following transitions 1. n=3 to n=1 2. n=2 to n=33. n=4 to n=34. n=3 to n=5(a) For...

See similar textbooks

Related questions

Q: The frequency of a photon that has a wavelength of 7.98 × 1013 m is energy of this photon is The…

A: The frequency of a photon is defined as number of wavelengths a photon propagates each second. The…

Q: Which electron transition produces light of the highest frequency in the hydrogen atom? a. 3s --->…

A: To find Which electron transition produces light of the highest frequency in the hydrogen atom?

Q: What is the frequency of a wave with a wavelength of 30cm that travels with a speed of 6cm/s

A: The relation between the wavelength, frequency, and speed is given as- v= f. λ…

Q: A certain shade of blue has a frequency of 7.30×1014 Hz. What is the energy of exactly one photon of…

Q: . If a hydrogen atom in the excited n = 3 state relaxes to the ground state, what is the maximum…

A: For a Hydrogen atom, the maximum number of possible emission lines is given by the formula as shown…

Q: A 753 nm753 nm krypton laser puts out 4.00 W4.00 W of power with a beam 4.60 mm4.60 mm in diameter.…

A: Given: Wavelength of light = 753 nm Power of beam = 4.00 W Diameter of pinhole = 2.00 mm…

Q: An electron in the n=5 level of an H atom emits a photon ofwavelength 1281 nm. To what energy level…

A: Given information: Wavelength = 1281. nm Initial state of an electron = 5 Rydberg’s equation is…

Q: If an atom lies 4.49 × 10- J above the ground state, determine the wavelength of light (in nm) that…

Q: A hydrogen atom is excited to n initial=4. A 1875 nm photon is emitted as the electron falls to n…

Q: [Ref What is the energy of a photon corresponding to radio waves of frequency 1.116 x 10° /s? Energy…

Q: If a 755 nm photon travels in vacuum, what is the frequency of this photon? Recall that the speed of…

A: Given , speed of light ,c = 2.998 x 108 m/s Wavelength = 755 nm 1 nm = 10-9 m

Q: An instrument is sensitive to laser light packets that carry at least 2.78 × 10-15 J of energy. How…

A: Energy of 1 photon is calculated as follows,

Q: A photon of ultraviolet (UV) light possesses enough energy to mutate a strand of human DNA. What is…

Q: The energy emitted by a light is 286000 J. Calculated the wavelength of an emitted photon.

Q: A nitrogen laser puts out a pulse containing 27.0 m) of energy at a wavelength of 337.1 nm. How many…

A: Total Energy = (n × h × c)/√ √ = wavelength

Q: An electron in a hydrogen atom de-excites, emitting a photon with a wavelength in the visible region…

A: When an electron de excites from a higher energy level to a lower energy level, then it emits a…

Q: The absorption peaks of chlorophyll a are at 665 nm and 465 nm. Assume that a plant can convert all…

A: Energy of a radiation is affected by its frequency or its wavelength. The radiant energy (E)…

Q: A laser emits 2.13 * 1016 photons per second, each of which has wavelength 625 nm. Find (a) the…

A: A. Wavelength of photon = λ= 625 nm Energy of single photon is calculated by using formula, E=hcλ…

Q: Hydrogen atoms absorb energy so that the electrons are excited to the energy level n = 7. Electrons…

A: A photon is undergoing transition from n = 3 to n = 1, the relation used to calculate wavelength of…

Q: Determine the mass of a ball with a wavelength of 3.45 x 10-34 m and a velocity of 6.55 m/s.

Q: Calculate the energy of a single photon of red light with a wavelength of 750 nm. Calculate the…

A: The energy ‘E’ which is present in a photon is used to represent the smallest possible ‘packet’ of…

Q: An electron in a hydrogen atom transitioning from orbit n = 7 releases a photon whose frequency…

A: Given: Frequency = 6.44196×1013 s-1 Higher energy level =7

Q: A ground-state atom absorbs light of wavelength 400 nm to be promoted to an excited state. Find the…

A: The difference in energy between two states is related to wavelength of light absorbed by ground to…

Q: 1. The characteristic red color of blood is due to the very strong absorption of light at a…

Q: Determine the energy of 1.70 mol of photons for each of the following kinds of light. (Assume three…

A: Given :- A. infrared radiation (1440 nm ) B. visible light (480 nm) C. ultraviolet radiation (160…

Q: A watt is a unit of energy per unit time, and one watt (W) is equal to one joule per second (J-s-1).…

A: 40W Incandescent light bulbProduce 5% of its energy .E=n hCλ C=speed of light n=no…

Q: Calculate the energy for the transition of an electron from the n=1 level to the n=8 level of a…

A: when energy is given to any atom, the electrons absorb the energy and jumps to a higher energy…

Q: Calculate the energy for the transition of an electron from the n=5 level to the n= 4 level of a…

Q: Determine the energy, in J, of a photon with a wavelength of 333nm.

A: Given :- wavelength = 333 nm h = 6.626 × 10-34 J.s c = 3.00 × 108 m/s…

Q: What is the frequency of a photon if energy is 6.671 * 10^-19 J? (h= 6.626 * 10^-34 J. s)

Q: How many moles of photons are in a pulse if the pulse has a wavelength of 600 nm and a total energy…

Q: please fill out the blank line. Question: A ground-state H atom absorbs a photon of wavelength 93.78…

Q: The retina of a human eye can detect light when radiant energy incident on it is at least 4.0 ×…

A: Energy of the electromagnetic radiation (Ep) = hf Energy of the photon of blue light (Ep) = hc/ λ…

Q: Calculate the frequency (in s) of photons that have an energy of 89.11 kJ/mol.

A: E = h ν where E = energy 1 mol of photons = 89.11 KJ x 1000 J/1 KJ = 89110 J h = Planck's…

Q: Calculate the energy of a photon of electromagnetic radiation at each of the following frequencies.…

Q: Is it correct that all photons of the same frequency have the same energy?

A: Yes, all photons having same frequency would have same energy.The energy of photons is different…

Q: one of the emission lines of the hydrogen atom has a wavelenght of 93.07 nm. (a) in what region of…

A: The wavelength between 90- 400nm. It is ultraviolet region.Then the region of the electromagnetic…

Q: A ground-state H atom absorbs a photon of wavelength 97.25 nm. What higher energy level did the…

A: We need to calculate the value of the higher energy level for the transition with wavelength 97.25…

Q: A ground-state H atom absorbs a photon of wavelength 91.50 nm. What higher energy level did the…

Q: Determine the energy of 1 mol of photons for each kind of light. (Assume three significant…

A: 1 mol = 6.022×1023 atoms a) Wavelength = 1500 nm = 1500×10-9 m Energy of 1…

Q: a. Calculate the energy of one photon with a wavelength of 121.58 nm b. Calculate the energy for a…

A: (a) Energy of one Photon can be expressed as

Q: Knowing that it is a frequency of 4.76 x 10^14 Hz and once the light saber is running perfectly,…

A: Given data : Frequency of light = 4.76 x 1014 Hz We can use the Einstein equation, E=hνwhere E is…

Q: A photon has a frequency of 5.5 × 10⁸ Hz. What is the energy of this photon?

A: Given: Frequency of photon, f =5.5 × 10⁸ Hz. We know, Planck's constant , h = 6.626×10−34 Js

Q: An atom in its ground state absorbs a single photon of light and then relaxes back to the ground…

A: First, the total energy is calculated.

Q: A sample of electromagnetic radiation has a frequency of 1.7x10^6 Hz, what is the wavelength for…

Q: 4. An electron revolving in the fourth excited hydrogen atom drops into second state and then to the…

Q: Calculate the energy of a photon that has a wavelength of 91.1 nm. Recall that 1 m = 109 nm.

A: Energy = 2.18x10-18J

Q: Which of the following transitions for an excited electron satisfies the selection rule and could…

Q: Hydrogen atoms absorb energy so that the electrons are excited to the energy level n = 7. Electrons…

A: In the given question we have to calculate the frequency of a photon from the transition of n= 5…

Question

Q) A hydrogen atom is initially in the ground
state, (i.e., n = 1 level), absorbed a photon, and as
a result of this absorption, a transition occurred
for the electron and ended at the n = 4 level.
A- What is the frequency of the
photon? *
Your answer
B- If the electron makes spontaneous
emission and comes back to the
ground state by going through all
energy levels between them. What
are the possible frequencies of the
photons emitted during this process?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the difference between continuous and discrete spectra?
The following are sets of rotational quantum numbers (J,MJ,K). Label each indicated transition as either allowed or forbidden. Hint: Remember the rules for allowed values of the various quantum numbers. a (5,4,0)(3,6,0)b (8,2,2)(9,2,2) c (7,4,2)(7,4,2)d (4,2,5)(3,2,5)
The following are sets of rotational quantum numbers (J,MJ,K). Label each indicated transition as either allowed or forbidden. Hint: Remember the rules for allowed values of the various quatum numbers. a (0,0,0)(1,1,0)b (0,0,0)(1,0,0) c (3,2,1)(3,1,1)d (4,4,1)(2,4,1)
Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
Consider Figure 11.4 and choose the correct phrase: As the vibrational quantum number increases, the extension of the vibration increases/decreases/stays the same while the average length of the oscillator itself increases/decreases/stays the same. Explain your choices.
The maximum in the blackbody radiation intensity curve moves to shorter wavelength as temperature increases. The German physicist Wilhelm Wien demonstrated the relation to be max1/T . Later, Planck’s equation showed the maximum to be max=0.20hc/kt . In 1965, scientists researching problems in telecommunication discovered “background radiation” with maximum wavelength 1.05 mm (microwave region of the EM spectrum) throughout space. Estimate the temperature of space.
Draw the graphical representations see Figure 11.15 of the possible values for l and ml for the first four energy levels of the 3-D rigid rotor. What are the degeneracies of each state?
List some unexplainable phenomena from the classical science and describe what could not be explained about them at the time.
What is the physical explanation of the difference between a particle having the 3-D rotational wavefunction 3,2 and an identical particle having the wavefunction 3,2?
Use Hunds rules to predict the term symbol of the ground electronic state of an atom having a d6 electron configuration for its valence subshell.
Consider the following transitions 1. n=3 to n=1 2. n=2 to n=33. n=4 to n=34. n=3 to n=5(a) For which of the transitions is energy absorbed? (b) For which of the transitions is energy emitted? (c) Which transitions involve the ground state? (d) Which transition absorbs the most energy? (e) Which transition emits the most energy?
Which of the following is an acceptable wavefunction over the indicated interval? □ A. e¹: [0, +00] □B. e ; [0, +00] □ C. e ¹; 00, +00] □ D. e ¹: [ 00, 0]