Consider the following four transitions in ahydrogen atom:(i) ni = 2, nf = 6 (ii) ni = 2, nf = 8(iii) ni = 7, nf = 8 (iv) ni = 6, nf = 2Find (a) the longest- and (b) the shortest-wavelength photon thatcan be emitted or absorbed by these transitions. Give the valueof the wavelength in each case. (c) For which of these transitionsdoes the atom lose energy? Explain.

Q: a)  Calculate the energy of the emissive transition with the lowest energy possible for the Lyman…

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Q: The hydrogen emission spectrum exhibits a line at 5.0010×10-19 J. If the final quantum state is n =…

A: Energy of transition for an atom is given by: ΔE = R(1/nf2 - 1/ni2) where, ΔE = energy released R=…

Q: Using the n value solved in part(a), calculate the maximum speed of the photoelectron from…

A: Given: The threshold frequency of potassium is 5.464×1014 s-1. Introduction: The photoelectric…

Q: Kα X-ray lines are emitted from a target with atomic number Z when an electron jumps down from n = 2…

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Q: exact value of s for significant figure purposes, 24 x 103 eV n . nm (three $). If the electron in a…

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Q: An alkali metal atom is in the ground state. The orbital angular momentum equals zero and the spin…

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Q: An infrared spectroscopy study of a diatomic molecule XY has given the following information: We…

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Q: Compute the change in wavelength of the 2p → 1s photon when a hydrogen atom is placed in a magnetic…

A: Spectral lines are formed due to electron transitions inside an atom. It was observed that when the…

Q: v) A source emits ultraviolet light of wavelength 96 nm. Could light of this wavelength be emitted…

A: When an atom absorbs energy, its electrons move to a higher energy level. When the electrons return…

Q: Cesium has a work function of 2.14 eV. What is the wavelength (nm) of a photon with the threshold…

A: Work function (Wo) = 2.14 eVKinetic energy of ejected electron,      KE = 580.89 nm

Q: a) The Balmer series consists of transitions in hydrogen from higher states where n > 2 to the n = 2…

A: Given: Balmer series of hydrogen atom  To Find: (a) Equation: 1λ=R122-1n2 (b) Light emitted in Hα…

Q: How does the answer to the previous question change if instead of a single jump from state n= 6 to…

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Q: Consider the spectral line of shortest wavelength corresponding to a transition shown in the figure.…

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Q: (a) The L→ K transition of an X-ray tube containing a molybdenum (Z = 42) target occurs at a…

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Q: (a) The Lyman series in hydrogen is the transition from energy levels n = 2, 3, 4, ... to the ground…

A: a) Given For the Lyman series in a Hydrogen atom The energy of each level is En=-13.6eVn2 So when an…

Q: If the element in the last problem has energy levels E, = 2.54 x 10 18 J and E2 = 2.2 x 10 18 J,…

A: E1 = 2.54×10-18 J E2 = 2.2×10-18 J difference of energy levels = E1 - E2= 2.54×10-18 -  2.2×10-18 J=…

Q: 1. An orthorhombic crystal with lattice parameters a = 0.32 nm, b= 0.27 nm and c= 0.5 nm is…

A: First, we need to calculate the wavelength of the electron beam using the de Broglie equation, which…

Q: What is the energy of the photon that, when absorbed by a hydrogen atom, could cause an electronic…

A: Energy required (E) to jump a electron from n1 to n2 is given by E= Rhc(1/n1² - 1/n2²)    n1= 3…

Q: onsider the electron of a Li2+ ion that undergoes a transition from a higher energy state n to its…

A: Given: The threshold potential of potassium is 5.464×1014 s-1. Introduction: The photoelectric…

Q: = Find the energy of the photon released in the transition from n₁ for a hydrogen atom. (Note: Use…

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Q: A photon can excite a hydrogen atom makes a from the n = (2.0000x10^0) state to the n = (8.00x10^0)…

A: Have a look dear

Q: The energy difference between the 1st excited state (n = 2) and the 2nd excited state (n = 3) in the…

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Q: While most transition metals have work functions corresponding to photon frequencies that are larger…

A: The energy of a photon is given by, E=hcλ Here h is Planck's constant, c is the velocity of light,…

Q: In the Balmer series, for the Hydrogen atom, a weak transition is observed at 397nm. the value of…

A: Lambda = 397 nm Li2+Z=3 for Li2+

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: