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Exam 7: Quantum Theory and Atomic Structure

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Question 21

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In the quantum mechanical treatment of the hydrogen atom,the energy depends on the principal quantum number n but not on the values of l or m_l.

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B) False

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Question 22

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a.Use Bohr's equation to calculate how much energy (in J)is needed to promote an electron from the H-atom ground state to the n = 4 level. b.If a photon provides the energy in (a),what is its wavelength in nm?

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a.2.04 10...

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Question 23

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The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz.Find the wavelength of these waves.

What are the possible values for the following quantum numbers in an atom? a.n b.l c.m_l

The energy of an electron in the hydrogen atom is determined by

Use the Bohr equation to calculate the energy of a.the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom. b.the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

What is the speed of an electron in m/s if its wavelength is 0.155 nm?

The following combinations of quantum numbers are not allowed.Correct each set by changing only one quantum number,and write in an appropriate corrected value.

a.Calculate the wavelength in nm of a photon whose energy is 6.00 $\times$ 10^-19 J. b.Would the photon in (a)have enough energy to ionize a hydrogen atom in its ground state (i.e. ,to separate the proton and electron completely)? Use the Bohr equation to explain your answer.

Use the Rydberg equation to calculate the wavelength,in nm,of the least energetic (longest wavelength)line in the visible series (n₁ = 2)of the spectrum of atomic hydrogen.

A photon has an energy of 5.53 $\times$ 10^-17 J.What is its frequency in s^-1?

Line spectra are characteristic of atoms in the gas phase.

Contact lenses can focus light due to the ___________ of the waves.

For the following orbitals,state the values of n,l and m_l which apply,and draw a sketch showing the shape and orientation of the orbital. a.3s b.2p_x

Explain the context and meanings of the terms "orbit" and "orbital",making a clear distinction between them.

Who was the first scientist to propose that an object could emit only certain amounts of energy?

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

a.Use the Bohr equation to calculate the energy needed to ionize a hydrogen atom from its ground state. b.What is the minimum wavelength of a photon needed for it to have the energy needed in (a)?

Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom?

Line spectra from all regions of the electromagnetic spectrum,including the Paschen series of infrared lines for hydrogen,are used by astronomers to identify elements present in the atmospheres of stars.Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3.(R = 1.096776 $\times$ 10⁷ m^-1)