Games Like Binding Of Isaac, June 2019, Part 2 - PhysicsLAB!. About featured snippets•FeedbackQuestions & answersBrainlyQuestiona red photon in the bright line spectrum of hydrogen gas has an energy of 3.02 x10 ^-19 joule. what enegry levelAnswer · 0 votesThe energy level associated with the red photon in the bright line spectrum of hydrogen gas is approximately n = 2.68. The energy levels in the bright line spectrum of hydrogen gas are quantized and can be calculated using the equation: E = -13.6 eV/n^2 where E is the energy level, -13.6 eV is the ionization energy of hydrogen, and n is the principal quantum number. To determine the energy level associated with a red photon in the hydrogen spectrum with an energy of 3.02 x 10^-19 joule, we need to convert the energy from joules to electron volts (eV). The conversion factor is 1 eV = 1.6 x 10^-19 joule. Energy in eV = (3.02 x 10^-19 joule) / (1.6 x 10^-19 joule/eV) = 1.89 eV Next, we can equate the energy level equation with the calculated energy: 1.89 eV = -13.6 eV/n^2 To solve for n, we rearrange the equation: n^2 = -13.6 eV / 1.89 eV n^2 = 7.19 Taking the square root of both sides, we find: n = √7.19 n ≈ 2.68 The energy level associated with the red photon in the bright line spectrum…MoreBrainly.comQuestiona red photon in the bright line spectrum of hydrogen gas has an energy of 3.02*10^-19 joule what energy level transition does an electron in a hydrogen atom undergo to produce this photonAnswer · 0 votesThe electron in a hydrogen atom underwent a transition from the n=4 energy level to the n=3 energy level to produce the red photon in the bright line spectrum with an energy of 3.02 x [tex]10^{-19[/tex] joules.The line spectrum of Hydrogen gas is composed of a series of bright lines with distinct wavelengths. These lines are caused by the movement of electrons within the hydrogen atom, which causes photons to be emitted as the electrons drop from higher energy levels to lower energy levels. Each line in the hydrogen spectrum corresponds to a specific electron transition within the atom, with the lowest energy transition corresponding to the Lyman series and the higher energy transitions corresponding to the Balmer, Paschen, and Brackett series. The energy associated with each transition can be calculated using the equation: E = hc/λ, where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon. For a red photon in the brigh…MoreGauthmathQuestionz A red photon in the bright-line spectrum of hydrogen gas has an energy of 3.02 * 10-19 joule. What energy-level transition does an electron in a hydrogen atom undergo to produce this photon? A n=5 to n=2 B n=4 to n=2 C n=6 to n=2 D n=3 to n=2Answer · 100 votesAnswer to z A red photon in the bright-line spectrum of hydrogen gas has an energy of 3.02 * 10-19 joule. What energy-level transition does an electron in a hydMoreNumeradeQuestionWhich of the following statementsis TRUE for the following situation:A spectral line is simply a large number of photons having thesame wavelength. The violet line at 430 nm in the heliumspectrum is strong and intense, while the violet line at 430 nm inthe xenon spectrum is weak and faint.Group of answer choicesHelium has more atoms giving off more photons of violet lightthan xenon.Xenon has more atoms giving off more photons of violet lightthan helium.The electrons in helium are dropping more energy levels thanxenon.The electrons in xenon are dropping more energy levels thanhelium.Which of the following types of light has the highestfrequency?Group of answer choices400 nm visible light500 nm visible light600 nm visible light700 nm visible lightWhich of the following types of electromagnetic radiation hasthe highest energy?Group of answer choicesVisible light (wavelength = 500 nm) )Microwaves (wavelength = 10,000,000 nm)Infrared Radiation (wavelength = 10,000 nm)Radio Waves (wavelenght = 1,000,000,000,000 nm)Which of the following arrangements of the visible colors oflight is in the correct orderof increasing energy?Group of answer choicesred, orange, yellow, green, blue, indigo, violetviolet, indigo, blue, green, yellow, orange, redred, yellow, orange, green, blue, indigo, violetviolet, indigo, green, blue, yellow, orange, redWhich of the following statements best describes how the brightlines are generated when an element is energized?Group of answer choicesA unique bright line is generated when an electron drops fromone energy level to another giving off a specific amount (photon)of energy.A unique bright line is generated when an electron jumps up to ahigher energy level giving off a specific amount (photon) of energy.A unique bright line is generated when an alpha particle hitsthe nucleus of the atom giving off a specific amount (photon) ofenergy.A unique bright line is generated when an electron gives off aspecific amount of electrical energy.Answer · 2 votesin this uh problem or this submission. There is a collection of related problems dealing with with photons and energy transitions between energy levels and so on. So let's look at them one at a time. First one we're given a wavelength In the green 560 nm and we want the energy electron volts. So this is Planck's constant times the frequency may use a new greek letter Nu for frequency. Uh huh. But we also have this Hc over lambda for anyway V equals the wavelength times the frequency for anyway because Not mad. No. And so at this point we can just put in our values 6.63 Times 10 to -34 jewel second, three times 10 to the eight meters per second for C. And then 560 10 minus nine meters for the wavelength. And we can put in we could have calculated this but let me put in the conversion factor because this is going to lead us with jewels. So let's put the conversion factor to electron votes Well that time voters 1.6 It's 10 miles 19 jewels. And when all said and done, you get 2.2 electron …MoreQuoraQuestionHow is the bright line spectrum of an element produced?Answer · 10 votesIt’s produced by the electrons in the elements’ atoms jumping to lower energy states after being bumped upward by a collision with another atom or an incoming photon or electron or whatever.As they do so, they release their extra energy by radiating photons, usually one photon per transition. If a single photon, then the transition has a well-defined energy.The spectral lines are not infinitely thin, however. They are broadened by several causes:• The transition rate produces a broadening with a range of frequencies equal to that rate.• Something similar for collisions with other atoms and the like.• The atoms’ motions making Doppler shifts.MoreBartleby.comQuestionConsider the bright line spectrum of hydrogen shown in the figure below.Which line in the spectrum represents photons with the highest energy?410 nm 434 nm 486 nm656 nmHydrogen Line Spectrum. When excited hydrogen atoms return to lower energy states, they emit photons ofcertain energies, and thus certain colors. Shown here are the colors and wavelengths (in nanometers) of thephotons in the visible region that are emitted by excited hyárogen atoms.O 434 nmO 410 nm656 nmO 486 nmAnswer · 0 votesStep 1 Given line spectra of hydrogen atom is :Options are :a). 434 nmb). 410 nmc). 656 nmd). 486 nmPredict the line with highest energy = ? .MoreWeb 2.0 scientific calculatorQuestionthe bright red line from the emission spectrum of hyrogen has a wave lngth of 657 nm. what is the energy, in joules, of a single photon of this lightAnswer · 0 votesthe bright red line from the emission spectrum of hyrogen has a wave lngth of 657 nm. what is the energy, in joules, of a single photon of this lightWavelength=c/v, where c=speed of light, v=frequencyv=c/w=3 X 10^8/6.57 X 10^-7v=4.566 X 10^14 HertzE=hv, where h is Planck's constant, v is the frequencyE=6.63 X 10^-34 X 4.566 X 10^14E=3.0274 X 10^-19 Joules- the energy of a single photonMoreStudy.comQuestionWhat is the bright line spectrum?Answer · 0 votesA bright line spectrum is a class of spectra referred to as an emission spectrum. Electrons of an element (particularly valence electrons) are in an.More Feedback Gi Detox Binder, a red photon in the bright line spectrum of hydrogen gas .. 1 answerThe electron in a hydrogen atom underwent a transition from the n=4 energy level to the n=3 energy level to produce the red photon in the bright line . Purple Binder, Solved 13A red photon in the bright-line spectrum of. Question: 13A red photon in the bright-line spectrum of hydrogen gas has an energy of 3.02 * 10-19 joule. What energy-level transition does an electron in a . The Binding Of Isaac Rule 34, Modern Physics. PDFdiagram, ground state, orbital, relaxed state, excited state, bright-line spectra, . Visible red light has a higher frequency than infrared light, .7 pages Yu Gi Oh Binder, Emission spectrum of hydrogen (video) - Khan Academy. 10:50656 nanometers is the wavelength of this red line right here. 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