Hydrogen atom: The normalized wave function for a hydrogen atom in the 1s state is given by ψ(r) = e-r/α0 where α0 is the Bohr radius, which is equal to 5.29 × 10-11 m. What is the probability of finding the electron at a distance greater than 7.8 α0 from the proton?

A) 2.3 × 10-5 B) 1.2 × 10-5 C) 1.7 × 10-5 D) 4.6 × 10-5 E) 3.5 × 10-5 A) 2.3 × 10-5 B) 1.2 × 10-5 C) 1.7 × 10-5 D) 4.6 × 10-5 E) 3.5 × 10-5 A

Multielectron atoms: A neutral atom has an electron configuration of 1s22s22p63s23p2. How many protons does it have in its nucleus?

A) 5 B) 11 C) 14 D) 20 E) 26 A) 5 B) 11 C) 14 D) 20 E) 26

Exam 32: Electromagnetic Waves Optics

Hydrogen atom: The normalized wave function for a hydrogen atom in the 1s state is given by ψ(r) = e^-^r/α₀ where α₀is the Bohr radius, which is equal to 5.29 × 10^-11 m. What is the probability of finding the electron at a distance greater than 7.8 α₀ from the proton?

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(Multiple Choice)

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Question 1

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Angular momentum: What is the greatest magnitude of the orbital angular momentum L for an electron in a state with principal quantum number

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(Multiple Choice)

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Question 2

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Zeeman effect: Electrons in the presence of a magnetic field transition from 4p energy states to 3d states. How many different spectral lines could be observed from these transitions?

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(Multiple Choice)

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Question 3

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Multielectron atoms: A neutral atom has an electron configuration of 1s²2s²2p⁶3s²3p². How many protons does it have in its nucleus?

(Multiple Choice)

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Question 4

Angular momentum: The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. What is the orbital quantum number l of the electron?

(Multiple Choice)

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Question 5

Multielectron atoms: Consider the n = 9 shell. (a) What is the largest value of the orbital quantum number, l, in this shell? (b) How many electrons can be placed in this shell?

(Essay)

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Question 6

Lasers: In a ruby laser, an electron jumps from a higher energy level to a lower one. If the energy difference between the two levels is 1.8 eV, what is the wavelength of the emitted photon? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

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Question 7

Zeeman effect: An alkali metal atom is in the ground state. The orbital angular momentum equals zero and the spin angular momentum is entirely due to the single valence electron. A magnetic field is applied that splits the ground state energy level into two levels, 65 μeV apart.A photon, absorbed by the atom, induces a transition between the two levels. What is the wavelength of the photon? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, Bohr magneton = μ_B = 9.27 × 10^-24 J/T, 1 eV = 1.60 × 10^-19 J)

(Multiple Choice)

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Question 8

Zeeman effect: An atom in a state with its orbital quantum number l = 1 decays to its ground state (with l = 0). A photon of wavelength 630.000 nm is emitted in the process. When the same process takes place in the presence of an intense magnetic field, the following change in the spectrum is observed. With the magnetic field present, one of the emitted lines observed now has a wavelength of 630.030 nm. Which of the following wavelengths would you expect to be also present?

(Multiple Choice)

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Question 9

Multielectron atoms: An atom has completely filled inner shells and a single valence electron in an excited p state. The filled inner shells have an orbital momentum equal to zero. A magnetic field is applied, defining the z-axis along the field. Which of the following sets of angles are possible angles between the magnetic field and the orbital angular momentum?

(Multiple Choice)

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Question 10

Lasers: How many photons per second emerge from a laser of power with wavelength (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

(Multiple Choice)

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Question 11

Multielectron atoms: How many electrons can be found with principal quantum number in a suitably heavy atom?

(Multiple Choice)

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Question 12

Multielectron atoms: What is the electron configuration for ground state Li, which has 3 electrons?

(Multiple Choice)

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Question 13

Quantum numbers: If the orbital quantum number is l = 4, which one of the following is a possible value for the principal quantum number n?

(Multiple Choice)

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Question 14

Multielectron atoms: An atom with 5 electrons is in its ground state. How many electrons are in its outermost shell?

(Short Answer)

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Question 15

Quantum numbers: Consider the four quantum numbers of an electron in an atom, n, l, m_l, and m_s. The energy of an electron in an isolated atom depends on

(Multiple Choice)

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Question 16

Multielectron atoms: What is the correct electronic configuration for ground state carbon, which has 6 electrons?

(Multiple Choice)

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Question 17

Lasers: You need 14 W of infrared laser light power with wavelength 1270 nm to bore a hole in a diamond. How many downward atomic transitions per second must occur in the laser if all of them result in light directed onto the diamond? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

(Multiple Choice)

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Question 18

Lasers: The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states involved in laser action? (c = 2.9979 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.6022 × 10^-19 J)

(Multiple Choice)

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Question 19

Multielectron atoms: How many possible sets of quantum numbers (electron states) are there in the 5f subshell?

(Multiple Choice)

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Question 20

Showing 1 - 20 of 53

Exam 32: Electromagnetic Waves Optics

Hydrogen atom: The normalized wave function for a hydrogen atom in the 1s state is given by ψ(r) = e-r/α0 where α0 is the Bohr radius, which is equal to 5.29 × 10-11 m. What is the probability of finding the electron at a distance greater than 7.8 α0 from the proton?

Angular momentum: What is the greatest magnitude of the orbital angular momentum L for an electron in a state with principal quantum number

Zeeman effect: Electrons in the presence of a magnetic field transition from 4p energy states to 3d states. How many different spectral lines could be observed from these transitions?

Multielectron atoms: A neutral atom has an electron configuration of 1s22s22p63s23p2. How many protons does it have in its nucleus?

Angular momentum: The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. What is the orbital quantum number l of the electron?

Multielectron atoms: Consider the n = 9 shell. (a) What is the largest value of the orbital quantum number, l, in this shell? (b) How many electrons can be placed in this shell?

Lasers: In a ruby laser, an electron jumps from a higher energy level to a lower one. If the energy difference between the two levels is 1.8 eV, what is the wavelength of the emitted photon? (c = 3.00 × 108 m/s, h = 6.626 × 10-34 J ∙ s, 1 eV = 1.60 × 10-19 J)

Lasers: How many photons per second emerge from a laser of power with wavelength (c = 3.00 × 108 m/s, h = 6.626 × 10-34 J ∙ s)

Multielectron atoms: How many electrons can be found with principal quantum number in a suitably heavy atom?

Multielectron atoms: What is the electron configuration for ground state Li, which has 3 electrons?

Quantum numbers: If the orbital quantum number is l = 4, which one of the following is a possible value for the principal quantum number n?

Multielectron atoms: An atom with 5 electrons is in its ground state. How many electrons are in its outermost shell?

Quantum numbers: Consider the four quantum numbers of an electron in an atom, n, l, ml, and ms. The energy of an electron in an isolated atom depends on

Multielectron atoms: What is the correct electronic configuration for ground state carbon, which has 6 electrons?

Lasers: You need 14 W of infrared laser light power with wavelength 1270 nm to bore a hole in a diamond. How many downward atomic transitions per second must occur in the laser if all of them result in light directed onto the diamond? (c = 3.00 × 108 m/s, h = 6.626 × 10-34 J ∙ s)

Lasers: The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states involved in laser action? (c = 2.9979 × 108 m/s, h = 6.626 × 10-34 J ∙ s, 1 eV = 1.6022 × 10-19 J)

Multielectron atoms: How many possible sets of quantum numbers (electron states) are there in the 5f subshell?

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Hydrogen atom: The normalized wave function for a hydrogen atom in the 1s state is given by ψ(r) = e^-^r/α₀ where α₀is the Bohr radius, which is equal to 5.29 × 10^-11 m. What is the probability of finding the electron at a distance greater than 7.8 α₀ from the proton?

Multielectron atoms: A neutral atom has an electron configuration of 1s²2s²2p⁶3s²3p². How many protons does it have in its nucleus?

Lasers: In a ruby laser, an electron jumps from a higher energy level to a lower one. If the energy difference between the two levels is 1.8 eV, what is the wavelength of the emitted photon? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.60 × 10^-19 J)

Lasers: How many photons per second emerge from a laser of power with wavelength (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

Quantum numbers: Consider the four quantum numbers of an electron in an atom, n, l, m_l, and m_s. The energy of an electron in an isolated atom depends on

Lasers: You need 14 W of infrared laser light power with wavelength 1270 nm to bore a hole in a diamond. How many downward atomic transitions per second must occur in the laser if all of them result in light directed onto the diamond? (c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s)

Lasers: The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states involved in laser action? (c = 2.9979 × 10⁸ m/s, h = 6.626 × 10^-34 J ∙ s, 1 eV = 1.6022 × 10^-19 J)