The shell of an atom is divided into subshells, or sublevels, identified by letters. For shell number n=1, the subshell is s; for n=2, it's s and p; for n=3, s, p, and d; and for n=4, s, p, d, and f. As n increases, the number of subshells also increases, but does not exceed f. Understanding these subshells is crucial for grasping electron configurations and the behavior of elements in chemical reactions.
Subshell designation gives the shape of an orbital within a subshell.
Electronic Structure:Subshells
1
concept
Electronic Structure: Subshells Concept 1
Video duration:
1m
Play a video:
Electronic Structure: Subshells Concept 1 Video Summary
The structure of an atom is organized into shells, which can be further divided into subshells, also referred to as sublevels. Each shell is associated with a principal quantum number, denoted as \( n \), which indicates the energy level of the electron. The possible subshells for each shell number are as follows:
For \( n = 1 \), the only subshell is s.
For \( n = 2 \), the subshells are s and p.
For \( n = 3 \), the subshells include s, p, and d.
For \( n = 4 \), the subshells are s, p, d, and f.
As the principal quantum number \( n \) increases, the variety of subshells available also expands. It is important to note that even at \( n = 5 \), the subshells remain limited to s, p, d, and f. Understanding these subshells is crucial for grasping the arrangement of electrons in an atom, which ultimately influences its chemical properties and behavior.
2
example
Electronic Structure: Subshells Example 1
Video duration:
53s
Play a video:
Electronic Structure: Subshells Example 1 Video Summary
In atomic structure, the principal quantum number \( n \) indicates the energy level of an electron, while the subshell letter denotes the type of orbital within that energy level. For an electron located in the third energy level, the principal quantum number \( n \) is equal to 3. When considering the subshells, the d subshell corresponds to the angular momentum quantum number \( l \), which for d orbitals is equal to 2. Therefore, the possible values for \( n \) and the subshell letter for an electron in the 3rd energy level and d subshell are:- \( n = 3 \)- Subshell letter: dThis means that the correct representation for an electron in this configuration is \( 3d \). Thus, the answer is option b, indicating that the electron is in the 3rd energy level and d subshell.
3
Problem
Provide all the possible values of the subshell for a 2 energy level.
A
0
B
0, 1
C
0, 1, 2
D
0, 1, 2, 3
E
1
4
Problem
How many sublevels are contained in the third shell (n = 3) for a given atom?
A
1
B
2
C
3
D
4
E
5
Do you want more practice?
We have more practice problems on Electronic Structure: Subshells
Here’s what students ask on this topic:
What are the subshells associated with each principal quantum number (n)?
The subshells associated with each principal quantum number (n) are as follows: for n=1, the subshell is s; for n=2, the subshells are s and p; for n=3, the subshells are s, p, and d; and for n=4, the subshells are s, p, d, and f. As the principal quantum number increases, the number of subshells also increases, but it does not exceed the f subshell. This pattern is crucial for understanding electron configurations and the behavior of elements in chemical reactions.
How do subshells relate to electron configurations?
Subshells are integral to electron configurations, which describe the arrangement of electrons in an atom. Each subshell (s, p, d, f) can hold a specific number of electrons: s can hold 2, p can hold 6, d can hold 10, and f can hold 14. Electrons fill subshells in order of increasing energy, following the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Understanding subshells helps predict the chemical properties and reactivity of elements.
Why do the number of subshells increase with the principal quantum number?
The number of subshells increases with the principal quantum number (n) because each shell can accommodate more complex electron arrangements as n increases. For n=1, only the s subshell is available. For n=2, both s and p subshells are available. For n=3, s, p, and d subshells are available, and for n=4, s, p, d, and f subshells are available. This increase allows for a greater number of electrons and more complex electron configurations, which are essential for the diverse chemical behavior of elements.
What is the maximum number of electrons that can occupy a subshell?
The maximum number of electrons that can occupy a subshell depends on the type of subshell: the s subshell can hold a maximum of 2 electrons, the p subshell can hold 6 electrons, the d subshell can hold 10 electrons, and the f subshell can hold 14 electrons. This is determined by the formula 2(2l+1), where l is the azimuthal quantum number corresponding to the subshell (0 for s, 1 for p, 2 for d, and 3 for f).
How do subshells affect the chemical properties of elements?
Subshells affect the chemical properties of elements by determining the distribution of electrons in an atom. The arrangement of electrons in different subshells influences an element's reactivity, ionization energy, and bonding behavior. For example, elements with similar electron configurations in their outermost subshells often exhibit similar chemical properties and are grouped together in the periodic table. Understanding subshells helps predict how elements will interact in chemical reactions.
