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Chapter 3: Problem 1

Within one principal energy level, which subshell has the least energy? A. S B. P C. D D. F

Short Answer

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A. S

Step by step solution

01

Understand Principal Energy Levels

Principal energy levels, denoted by the principal quantum number (n), contain subshells (s, p, d, f). Each subshell represents a different shape of the region in which there is a high probability of finding an electron.
02

Subshel Energies Relation

Within the same principal energy level, subshells have different energy levels. The order of increasing energy within a principal energy level is: s < p < d < f.
03

Identify the Lowest Energy Subshell

Given the order of increasing energy (s < p < d < f), the s subshell has the least energy within a principal energy level.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Principal Quantum Number
The principal quantum number, denoted as *n*, is a fundamental concept in quantum mechanics. It signifies the main energy level occupied by an electron in an atom. The larger the value of *n*, the higher the energy level and the farther the electron is from the nucleus.

Principal energy levels are represented by integers (1, 2, 3, etc.). Each level can hold a certain number of electrons:

  • *n* = 1 can hold 2 electrons
  • *n* = 2 can hold 8 electrons
  • *n* = 3 can hold 18 electrons


These energy levels are composed of one or more sub-levels or subshells (s, p, d, f), which detail the electron's orbitals further.
Subshell Energy Order
Within any given principal energy level, subshells have different energy levels. The order of increasing energy is crucial for understanding electron configurations:

  • *s* subshell has the least energy
  • *p* subshell has more energy than *s*
  • *d* subshell has more energy than *p*
  • *f* subshell has the highest energy among these


Therefore, within a principal energy level, *s* subshells are the lowest in energy, making them the first to be filled by electrons. The order of filling of the subshells follows the Aufbau principle, which states that lower energy orbitals fill before higher energy orbitals.
Electron Probability Regions
Electrons do not orbit the nucleus in defined paths but exist in regions called orbitals where they are most likely to be found. These are electron probability regions. Each subshell has differently shaped orbitals where an electron is likely to be present:

  • *s* orbitals are spherical
  • *p* orbitals are dumbbell-shaped
  • *d* orbitals have more complex shapes
  • *f* orbitals are even more complex


The shape and size of these regions change with increasing principal quantum number *n*. The more complex the shape, the more energy the subshell has. This is why *f* orbitals have more energy than *d*, *p*, and *s* orbitals within the same principal energy level.

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Most popular questions from this chapter

Which of the following compounds possesses at least one ? bond? A. \(\mathrm{CH}_{4}\) B. \(\mathrm{C}_{2} \mathrm{H}_{2}\) C. \(\mathrm{C}_{2} \mathrm{H}_{4}\) D. All of the above contain at least one \(\sigma\) bond.

Which of the following hybridizations does the Be atom in BeH \(_{2}\) assume? A. \(s p\) B. \(s p^{2}\) C. \(s p^{3}\) D. \(s p^{3} d\)

Molecular orbitals can contain a maximum of: a. one electron. b. two electrons. c. four electrons. d. \(2 n^{2}\) electrons, where \(n\) is the principal quantum number of the combining atomic orbitals.

A carbon atom participates in one double bond. As such, this carbon contains orbitals with: A. hybridization between the s-orbital and one \(p\) -orbital. B. hybridization between the s-orbital and two \(p\) -orbitals. C. hybridization between the s-orbital and three \(p\) -orbitals. D. unhybridized s character.

Compared to single bonds, triple bonds are: a. weaker. b. longer. c. made up of fewer \(\sigma\) bonds. d. more rigid.
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