he emission spectrum of Hydrogen has a bright blue-green line at 486 ??. This electron ends in the ?? = 2 energy level. What is the initial energy of the electron that produced this photon? (Find the energy of the electron in its excited state, ??).

Q: An electron in an excited energy state of the Hydrogen atom has an energy En = 0.85 eV which is…

A: Energy of an electron in the n th orbit is  En=-13.6n2 ev And radius of n th electronic orbit is…

Q: Given that the energy of an electron in the He+ ion is Z²RH En n² what is the energy of a photon…

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Q: What is the frequency of light (in Hz) of a photon emitted when an electron in a hydrogen atom…

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Q: Tellurium has a work function of 4.95 eV. What is the minimum frequency of light needed to eject…

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Q: he blackbody radiation emitted from a furnace peaks at a wavelength of 2.5 10-6 m (0.0000025 m).…

A: Use Wein displacement law

Q: Light that has a frequency of about 4.43 1014 Hz (a wavelength of about 683 nm) appears red to our…

A:

Q: An electron is trapped in a one-dimensional box that is 501 nm wide. Initially, it is in the n = 3…

A:

Q: 1. Rank these photons in terms of decreasing energy: (a) IR (v = 6.5 x 1013 s'); (b) microwave (v =…

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Q: 16). How much energy is generated when a frequency of 2.74 e 14 Hz is created in an electron loss.

A: The energy E of a photon is given by E = hf where h the Planck's constant f is the frequency

Q: Ionizing a hydrogen atom in its electric ground state requires 13.6 eV of energy. What is the…

A: The ionization energy of a hydrogen atom in its ground state is 13.6 eV.The task is to find out the…

Q: To excite an electron in a one-dimensional box from its first excited state to its second excited…

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Q: An electron in hydrogen absorbs a photon and jumps from orbit n = 2 to n = 4. Using the energy level…

A: An electron jumps from n=2 to n=4

Q: Determine the maximum wavelength of the photon that hydrogen in the excited state ni = 6 can absorb.…

A: Given- Ni = 6 The energy of ground state oh hydrogen (E) = -13.6 eV Speed of light (c) =  2.99792 ×…

Q: In an photoelectric effect 0.500 moles of electrons are accelerated with the total speed of 3.61 x…

A: The photoelectric effect is a phenomena in which light causes electrons to be expelled from a…

Q: A hydrogen atom has its electron in the n = 2 state. (a) How much energy would have to be absorbed…

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Q: For potassium, find the critical frequency fo of the incident light below which no electrons are…

A: Work function (is constant for a metal) of potassium, W = 2.30 eV = 2.30×1.6×10-19 J From Einstein…

Q: Potassium and gold cathodes are used in a photoelectriceffect experiment. For each cathode, find:a.…

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Q: What is the energy of an electron with wavelength 680 nm?

A: Form the De Broglie equation, the momentum of the electron can be calculated if its wavelength is…

Q: Ex. 20: Find the value of energy of electron in eV in the third Bohr orbit of hydrogen atom.…

A: To find-E3=?Given-R=1.097×107 m-1h=6.63×10-34 Jsc=3×108 m/sn=3

Q: An electron in an excited energy state of the Hydrogen atom has an energy En = 0.85 eV which is…

A: Energy of excited state En = - 0.85 eV Energy of ground state Eo = - 0.85 eV - 12.75 eV = - 13.6 eV…

Q: An electron in the n = 4 level of an H atom emits a photon of wavelength 97 nm. To what energy level…

A: Wavelength of photon is Initial energy state of electron in hydrogen atom is Note:Rydberg's constant…

Q: Calculate the energy of an electron in the 1s energy level in a hydrogen atom.

A: Atom = hydrogen level = 1 sradius of 1s = 5.3 * 10-11 m to find : energy of electron in 1 s level

Q: The so-called Lyman-? photon is the lowest energy photon in the Lyman series of hydrogen and results…

A: a) Energy of Lyman photon, E= 13.6 eV × (1n22-1n12) = 13.6 eV × (122-112)   = 10.2 eV

Q: According to Bohr's model, what is the diameter of hydrogen in its first excited state

A: Bohr's model  To find = diameter of hydrogen in its first excited state .

Q: Protons are accelerated from rest by a potential difference of 3.80 kVkV and strike a metal target.…

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The Bohr model

Students often get confused between Rutherford’s model and Bohr model of an atom. They interpret the postulates of both these models to be the same, which is incorrect. Rutherford’s model differs from Bohr’s model in the following ways: