List These Electron Subshells In Order Of Increasing Energy: $6p$, $7s$, $4f$, $5f$.Note For Advanced Students: You May Assume These Subshells Are Part Of Typical Energy Level Configurations.

Introduction

In the realm of chemistry, electron subshells play a crucial role in determining the energy levels of electrons within an atom. The arrangement of these subshells is essential in understanding the electronic configuration of atoms and molecules. In this article, we will delve into the world of electron subshells, exploring their characteristics and how to list them in order of increasing energy.

What are Electron Subshells?

Electron subshells are the regions within an atom's electron cloud where electrons are likely to be found. These subshells are designated by a set of four quantum numbers: n, l, m_l, and m_s. The principal quantum number (n) determines the energy level of the subshell, while the azimuthal quantum number (l) specifies the subshell's shape and orientation.

Types of Electron Subshells

There are several types of electron subshells, each with its unique characteristics. The most common subshells are:

• s-subshells: These subshells have an orbital shape that is spherical in nature. They are typically found in the innermost energy levels of an atom.
• p-subshells: These subshells have an orbital shape that is dumbbell-like in nature. They are typically found in the outer energy levels of an atom.
• d-subshells: These subshells have an orbital shape that is four-leaf clover-like in nature. They are typically found in the higher energy levels of an atom.
• f-subshells: These subshells have an orbital shape that is complex and multi-lobed in nature. They are typically found in the highest energy levels of an atom.

Listing Electron Subshells in Order of Increasing Energy

Now that we have a basic understanding of electron subshells, let's move on to the main topic of this article: listing these subshells in order of increasing energy. The subshells given in the problem are $6p$, $7s$, $4f$, and $5f$. To determine the order of increasing energy, we need to consider the principal quantum number (n) of each subshell.

• $6p$: The principal quantum number (n) of this subshell is 6. The p-subshell is typically found in the outer energy levels of an atom.
• $7s$: The principal quantum number (n) of this subshell is 7. The s-subshell is typically found in the innermost energy levels of an atom.
• $4f$: The principal quantum number (n) of this subshell is 4. The f-subshell is typically found in the higher energy levels of an atom.
• $5f$: The principal quantum number (n) of this subshell is 5. The f-subshell is typically found in the higher energy levels of an atom.

Order of Increasing Energy

Based on the principal quantum number (n) of each subshell, we can determine the order of increasing energy:

1. $4f$: The principal quantum number (n) of this subshell is 4, which is the lowest among the given subshells.
2. $5f$: The principal quantum number (n) of this subshell is 5, which is higher than 4.
3. $6p$: The principal quantum number (n) of this subshell is 6, which is higher than 5.
4. $7s$: The principal quantum number (n) of this subshell is 7, which is the highest among the given subshells.

Therefore, the order of increasing energy is: $4f$, $5f$, $6p$, $7s$.

Conclusion

In conclusion, listing electron subshells in order of increasing energy requires a basic understanding of the principal quantum number (n) and the characteristics of each subshell. By considering the principal quantum number (n) of each subshell, we can determine the order of increasing energy. This knowledge is essential in understanding the electronic configuration of atoms and molecules, which is crucial in various fields of chemistry.

References

• Chemistry: An Atoms First Approach by Steven S. Zumdahl
• General Chemistry by Linus Pauling
• The Elements by Theodore L. Brown, H. Eugene LeMay, and Bruce E. Bursten

Further Reading

• Electron Configuration by Khan Academy
• Subshells by Chemistry LibreTexts
• Quantum Numbers by HyperPhysics
  Electron Subshells: A Q&A Guide =====================================

Introduction

In our previous article, we explored the world of electron subshells, discussing their characteristics and how to list them in order of increasing energy. In this article, we will delve into a Q&A format, addressing some of the most frequently asked questions about electron subshells.

Q: What is the difference between an electron shell and an electron subshell?

A: An electron shell is a region around the nucleus of an atom where electrons are likely to be found. It is designated by a principal quantum number (n). An electron subshell, on the other hand, is a specific region within an electron shell where electrons are likely to be found. It is designated by an azimuthal quantum number (l).

Q: What are the different types of electron subshells?

A: There are several types of electron subshells, including:

• s-subshells: These subshells have an orbital shape that is spherical in nature.
• p-subshells: These subshells have an orbital shape that is dumbbell-like in nature.
• d-subshells: These subshells have an orbital shape that is four-leaf clover-like in nature.
• f-subshells: These subshells have an orbital shape that is complex and multi-lobed in nature.

Q: How do I determine the order of increasing energy for electron subshells?

A: To determine the order of increasing energy for electron subshells, you need to consider the principal quantum number (n) of each subshell. The subshell with the lowest principal quantum number (n) will have the lowest energy, while the subshell with the highest principal quantum number (n) will have the highest energy.

Q: What is the significance of the azimuthal quantum number (l) in electron subshells?

A: The azimuthal quantum number (l) determines the shape and orientation of an electron subshell. It also determines the number of orbitals within a subshell. For example, an s-subshell has one orbital, while a p-subshell has three orbitals.

Q: Can you provide an example of how to list electron subshells in order of increasing energy?

A: Let's consider the following subshells: $3s$, $4p$, $5d$, and $6f$. To list these subshells in order of increasing energy, we need to consider the principal quantum number (n) of each subshell:

• $3s$: The principal quantum number (n) of this subshell is 3.
• $4p$: The principal quantum number (n) of this subshell is 4.
• $5d$: The principal quantum number (n) of this subshell is 5.
• $6f$: The principal quantum number (n) of this subshell is 6.

Based on the principal quantum number (n) of each subshell, we can determine the order of increasing energy:

1. $3s$: The principal quantum number (n) of this subshell is 3, which is the lowest among the given subshells.
2. $4p$: The principal quantum number (n) of this subshell is 4, which is higher than 3.
3. $5d$: The principal quantum number (n) of this subshell is 5, which is higher than 4.
4. $6f$: The principal quantum number (n) of this subshell is 6, which is the highest among the given subshells.

Therefore, the order of increasing energy is: $3s$, $4p$, $5d$, $6f$.

Q: What are some common mistakes to avoid when working with electron subshells?

A: Some common mistakes to avoid when working with electron subshells include:

• Confusing the principal quantum number (n) with the azimuthal quantum number (l): The principal quantum number (n) determines the energy level of an electron subshell, while the azimuthal quantum number (l) determines the shape and orientation of the subshell.
• Not considering the number of orbitals within a subshell: The number of orbitals within a subshell is determined by the azimuthal quantum number (l).
• Not listing subshells in order of increasing energy: Failing to list subshells in order of increasing energy can lead to incorrect conclusions about the electronic configuration of an atom.

Conclusion

In conclusion, electron subshells are a fundamental concept in chemistry, and understanding them is essential for understanding the electronic configuration of atoms and molecules. By addressing some of the most frequently asked questions about electron subshells, we hope to have provided a comprehensive guide to this complex topic.