Question 1

Which of the following elements would you expect to have the lowest first ionization energy?

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Question 2

Arrange the following elements in order of increasing size: ₁₅P, ₂₀Ca, ₃₂Ge, ₃₇Rb, ₃₈Sr.

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Question 3

Radiation with a wavelength of ________ nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the ________ region of the electromagnetic spectrum.

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Question 4

How many electrons can be in the n = 3 shell of an atom? (Include all orbitals that have n = 3.)

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Question 5

Consider the radial distribution shown below for an electron in an s atomic orbital where r is the distance of the electron from the nucleus.  
Identify: (1) where the atomic nucleus is located; (2) a radial node; (3) the most probable distance of the electron from the nucleus; and (4) the principle quantum number for this orbital.

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Question 6

Write the electron configuration of Zn.

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Question 7

When the principle quantum number = 3, what values are possible for the other quantum numbers $$\ell$$ 
and m $\ell$ 
?

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Question 8

If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector? (1 eV = 1.60 *10^-¹⁹ J)

Accepted Answer

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Question 9

A light detector based on the photoelectric effect is made with cesium metal. Cesium metal has a work function of 3.40 *10^-¹⁹ J. What is the longest wavelength of light that one could expect to detect with this device?

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Question 10

De Broglie proposed that $\lambda$ = h/mv. Define the symbols in this equation and describe the significance of de Broglie's proposal.

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Question 11

Astronomers have detected hydrogen atoms in interstellar space in the n = 732 energy level. Suppose an atom in this excited state emits a photon and undergoes a transition from n = 732 to n = 721. How much energy does the atom lose as a result of this transition? What is the wavelength of the emitted photon? In which spectral region does this radiation lie?

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Question 12

What is the minimum energy that a photon must have to ionize a hydrogen atom from the n = 3 energy level?

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Question 13

Give the names of the three quantum numbers (n, $\ell$ 
, and m $\ell$ 
) that identify the mathematical functions (orbitals) that are solutions to Schrödinger's wave equation, and describe how the energy, size, shape, and orientation of the orbital varies with the relative values of these quantum numbers.

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Question 14

Which of the following elements would you expect to have the greatest first ionization energy?

Accepted Answer

Oxygen (O) has the greatest first ionization energy because it has a smaller atomic radius and higher effective nuclear charge than the other elements listed. This means that the outermost electron is held more tightly and requires more energy to remove.

Question 15

Astronomers have detected hydrogen atoms in interstellar space in the n = 732 energy level. Suppose an atom in this excited state emits a photon and undergoes a transition from n = 732 to n = 632. How much energy does the atom lose as a result of this transition? What is the frequency of this radiation? In which spectral region does this radiation lie?

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Question 16

Write the electron configuration of Zn²⁺.

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Question 17

Which sequence does not correctly arrange the elements in order of increasing energy released (electron affinity) upon formation of its monatomic anion?

Accepted Answer

Ar is a noble gas and does not readily form anions, so it should not be placed after S in terms of increasing electron affinity.

Question 18

Place these types of radiation in order of increasing energy per photon.
I. Yellow light from a street lamp.
II. X-rays from a dental X-ray.
III. Microwaves from your cell phone.
IV. Radio waves from your favorite FM station.

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Question 19

What is meant when two or more orbitals are said to be degenerate?

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Question 20

Copper forms a cation with a charge of 1+, but the element to the right of it in the periodic table (Zn) forms a cation with a 2+ charge. Use your knowledge of electron configurations to explain this observation.

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Quiz 7: A Quantum Model of Atoms: Waves and Particles

Which of the following elements would you expect to have the lowest first ionization energy?

Arrange the following elements in order of increasing size: ₁₅P, ₂₀Ca, ₃₂Ge, ₃₇Rb, ₃₈Sr.

Radiation with a wavelength of nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the region of the electromagnetic spectrum.

How many electrons can be in the n = 3 shell of an atom? (Include all orbitals that have n = 3.)

Write the electron configuration of Zn.

When the principle quantum number = 3, what values are possible for the other quantum numbers $\ell$ and m $\ell$ ?

If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector? (1 eV = 1.60 *10^-¹⁹ J)

A light detector based on the photoelectric effect is made with cesium metal. Cesium metal has a work function of 3.40 *10^-¹⁹ J. What is the longest wavelength of light that one could expect to detect with this device?

De Broglie proposed that $\lambda$ = h/mv. Define the symbols in this equation and describe the significance of de Broglie's proposal.

What is the minimum energy that a photon must have to ionize a hydrogen atom from the n = 3 energy level?

Which of the following elements would you expect to have the greatest first ionization energy?

Write the electron configuration of Zn²⁺.

Which sequence does not correctly arrange the elements in order of increasing energy released (electron affinity) upon formation of its monatomic anion?

Place these types of radiation in order of increasing energy per photon. I. Yellow light from a street lamp. II. X-rays from a dental X-ray. III. Microwaves from your cell phone. IV. Radio waves from your favorite FM station.

What is meant when two or more orbitals are said to be degenerate?

Copper forms a cation with a charge of 1+, but the element to the right of it in the periodic table (Zn) forms a cation with a 2+ charge. Use your knowledge of electron configurations to explain this observation.

Quiz 7: A Quantum Model of Atoms: Waves and Particles

Which of the following elements would you expect to have the lowest first ionization energy?

Arrange the following elements in order of increasing size: 15P, 20Ca, 32Ge, 37Rb, 38Sr.

Radiation with a wavelength of ________ nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the ________ region of the electromagnetic spectrum.

How many electrons can be in the n = 3 shell of an atom? (Include all orbitals that have n = 3.)

Write the electron configuration of Zn.

When the principle quantum number = 3, what values are possible for the other quantum numbers ℓ\ellℓ and m ℓ\ellℓ ?

If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector? (1 eV = 1.60 *10-19 J)

A light detector based on the photoelectric effect is made with cesium metal. Cesium metal has a work function of 3.40 *10-19 J. What is the longest wavelength of light that one could expect to detect with this device?

De Broglie proposed that λ\lambdaλ = h/mv. Define the symbols in this equation and describe the significance of de Broglie's proposal.

What is the minimum energy that a photon must have to ionize a hydrogen atom from the n = 3 energy level?

Which of the following elements would you expect to have the greatest first ionization energy?

Write the electron configuration of Zn2+.

Which sequence does not correctly arrange the elements in order of increasing energy released (electron affinity) upon formation of its monatomic anion?

Place these types of radiation in order of increasing energy per photon. I. Yellow light from a street lamp. II. X-rays from a dental X-ray. III. Microwaves from your cell phone. IV. Radio waves from your favorite FM station.

What is meant when two or more orbitals are said to be degenerate?

Copper forms a cation with a charge of 1+, but the element to the right of it in the periodic table (Zn) forms a cation with a 2+ charge. Use your knowledge of electron configurations to explain this observation.

Arrange the following elements in order of increasing size: ₁₅P, ₂₀Ca, ₃₂Ge, ₃₇Rb, ₃₈Sr.

Radiation with a wavelength of nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the region of the electromagnetic spectrum.

When the principle quantum number = 3, what values are possible for the other quantum numbers $\ell$ and m $\ell$ ?

If cesium, which has a work function of 2.1 eV, is used in a photodetector, what will be the kinetic energy of electrons produced by green light (540 nm) incident on the detector? (1 eV = 1.60 *10^-¹⁹ J)

A light detector based on the photoelectric effect is made with cesium metal. Cesium metal has a work function of 3.40 *10^-¹⁹ J. What is the longest wavelength of light that one could expect to detect with this device?

De Broglie proposed that $\lambda$ = h/mv. Define the symbols in this equation and describe the significance of de Broglie's proposal.

Write the electron configuration of Zn²⁺.