Question 1

The complete electron configuration of chromium,element 24,is ________.

Accepted Answer

Chromium has an unusual electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹, due to the stability provided by a half-filled d subshell.

Question 2

What are the possible values of n and m_l for an electron in a 3d orbital?

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Question 3

What is the photoelectric effect?

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Question 4

Define diffraction.

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Question 5

How many orbitals are contained in the n = 2 level? Give thel and m_l values of each of them.

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Question 6

Which ion does not have a noble gas configuration in its ground state?

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Question 7

How are 3p orbitals different from the 2p orbitals?

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Question 8

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

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Question 9

Give an example of a p orbital.

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Question 10

For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?

Accepted Answer

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Question 11

What are the possible values of l if n = 6?

Accepted Answer

The possible values of l depend on the principal quantum number n according to the rule that l can range from 0 to n-1. Therefore, if n=6, the possible values of l are 0, 1, 2, 3, 4, or 5, which is option B.

Question 12

Give an example of a d orbital.

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Question 13

The element that corresponds to the electron configuration 1s²2s²2p² is ________.

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Question 14

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

Accepted Answer

The formula for calculating the wavelength of emitted photon is given by 1/λ = R[(1/nf^2) - (1/ni^2)], where λ is the wavelength, R is the Rydberg constant, nf is the final energy level, and ni is the initial energy level. 
In this case, the initial energy level is 4d and the final energy level is 2p. The corresponding values of ni and nf are 16 and 5, respectively (since the energy of an electron in a hydrogen atom is given by E = (-13.6 eV)/n^2). 
Substituting the values in the above formula, we get 1/λ = (1.097 × 10^7 m^-1) [(1/5^2) - (1/16^2)]. Solving for λ, we get λ = 486.2 nm. 
Therefore, the best choice is B, 486.2 nm.

Question 15

Why don't we observe the wavelength of everyday macroscopic objects?

Accepted Answer

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Question 16

How many orbitals are there in the fourth shell?

Accepted Answer

The fourth shell (n=4) has four types of orbitals: s, p, d, and f, with 1, 3, 5, and 7 orbitals respectively, totaling 16 orbitals.

Question 17

The de Broglie wavelength of an electron with a velocity of 9.00 × $10 ^ { 6 }$ m s^-1 is ________ m.The mass of the electron is 9.11 × $10 ^ { - 28 }$ g.

Accepted Answer

The de Broglie wavelength is calculated using the formula λ = h / (mv), where h is Planck's constant (6.626 × 10^-34 Js), m is the mass of the electron (9.11 × 10^-31 kg), and v is the velocity (9.00 × 10^6 m/s). Converting the mass from grams to kilograms and substituting the values, the wavelength is approximately 8.08 × 10^-11 m.

Question 18

How many subshells are there in the shell with n = 4?

Accepted Answer

The total number of subshells in a shell is equal to the value of n. Therefore, for n = 4, there are 4 subshells (l = 0, 1, 2, 3) which correspond to the s, p, d, and f sublevels.

Question 19

Describe how a neon light works.

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Question 20

Define constructive interference.

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Quiz 7: The Quantum-Mechanical Model of the Atom