The First Transition Series and Group VIII

Oct 13, 2025 by miodeya.com 72 views

Introduction

In chemistry, the electronic configuration of an ion is a crucial concept that helps us understand the properties and behavior of elements. The electronic configuration of an ion is the arrangement of electrons in an atom's orbitals, which can be determined by the number of protons and electrons in the atom. In this article, we will explore the electronic configuration of an ion ${$ Y^{3+} $}$ for an element that exists in the first transition series and Group VIII.

The First Transition Series and Group VIII

The first transition series consists of elements from Scandium (Sc) to Zinc (Zn), which are located in the d-block of the periodic table. These elements have partially filled d-orbitals, which are responsible for their unique properties. Group VIII, on the other hand, consists of the noble gases, which are unreactive and have a full outer energy level.

Electronic Configuration of Yttrium (Y)

Yttrium (Y) is a member of the first transition series and is located in Group III of the periodic table. The electronic configuration of Yttrium is ${$ [Kr] 4d^1 5s^2 $}$. When Yttrium loses three electrons to form the ${$ Y^{3+} $}$ ion, its electronic configuration changes to ${$ [Kr] $}$.

Electronic Configuration of ${$ Y^{3+} $}$

The electronic configuration of ${$ Y^{3+} $}$ can be determined by removing three electrons from the electronic configuration of Yttrium. The resulting electronic configuration is ${$ [Kr] $}$. However, we are asked to find the electronic configuration of ${$ Y^{3+} $}$ for an element that exists in the first transition series and Group VIII.

Options A, B, and C

Let's analyze the options given:

A. ${$ [ \text{Ar} ] 3d^5 $}$

B. ${$ [ \text{Ar} ] 3d^6 $}$

C. ${$ [ \text{Ar} ] 3d^7 $}$

Option A: ${$ [ \text{Ar} ] 3d^5 $}$

Option A suggests that the electronic configuration of ${$ Y^{3+} $}$ is ${$ [ \text{Ar} ] 3d^5 $}$. This is a possible electronic configuration for an element in the first transition series and Group VIII. The ${$ [ \text{Ar} ] $}$ core configuration indicates that the element has a noble gas core, which is consistent with Group VIII. The ${$ 3d^5 $}$ configuration suggests that the element has five electrons in its 3d-orbitals, which is consistent with the first transition series.

Option B: ${$ [ \text{Ar} ] 3d^6 $}$

Option B suggests that the electronic configuration of ${$ Y^{3+} $}$ is ${$ [ \text{Ar} ] 3d^6 $}$. This is also a possible electronic configuration for an element in the first transition series and Group VIII. The ${$ [ \text{Ar} ] $}$ core configuration indicates that the element has a noble gas core, which is consistent with Group VIII. The ${$ 3d^6 $}$ configuration suggests that the element has six electrons in its 3d-orbitals, which is consistent with the first transition series.

Option C: ${$ [ \text{Ar} ] 3d^7 $}$

Option C suggests that the electronic configuration of ${$ Y^{3+} $}$ is ${$ [ \text{Ar} ] 3d^7 $}$. This is not a possible electronic configuration for an element in the first transition series and Group VIII. The ${$ [ \text{Ar} ] $}$ core configuration indicates that the element has a noble gas core, which is consistent with Group VIII. However, the ${$ 3d^7 $}$ configuration suggests that the element has seven electrons in its 3d-orbitals, which is not consistent with the first transition series.

Conclusion

In conclusion, the electronic configuration of an ion ${$ Y^{3+} $}$ for an element that exists in the first transition series and Group VIII can be all the following except:

${$ [ \text{Ar} ] 3d^7 $}$

$The other options, ${$ [ \text{Ar} ] 3d^5 \$}$ and ${$ [ \text{Ar} ] 3d^6 \$}$, are possible electronic configurations for an element in the first transition series and Group VIII.<br/> **The Electronic Configuration of an Ion: Q&A**$

Q: What is the electronic configuration of an ion?

A: The electronic configuration of an ion is the arrangement of electrons in an atom's orbitals, which can be determined by the number of protons and electrons in the atom.

Q: What is the difference between the electronic configuration of an atom and an ion?

A: The electronic configuration of an atom is the arrangement of electrons in its orbitals, while the electronic configuration of an ion is the arrangement of electrons in its orbitals after it has gained or lost electrons to form a charged species.

Q: How do you determine the electronic configuration of an ion?

A: To determine the electronic configuration of an ion, you need to know the number of protons and electrons in the atom. You can then use the periodic table to determine the electronic configuration of the atom, and then adjust it to account for the gain or loss of electrons.

Q: What is the significance of the noble gas core in the electronic configuration of an ion?

A: The noble gas core in the electronic configuration of an ion indicates that the element has a full outer energy level, which is characteristic of the noble gases. This means that the element is unreactive and has a stable electronic configuration.

Q: Can an element in the first transition series have a noble gas core?

A: No, an element in the first transition series cannot have a noble gas core. The first transition series consists of elements that have partially filled d-orbitals, which means that they do not have a full outer energy level.

Q: What is the difference between the 3d and 4d orbitals in the electronic configuration of an ion?

A: The 3d and 4d orbitals are two different sets of orbitals in the electronic configuration of an ion. The 3d orbitals are located closer to the nucleus and have a higher energy than the 4d orbitals. The 4d orbitals are located farther from the nucleus and have a lower energy than the 3d orbitals.

Q: How do you determine the number of electrons in the 3d and 4d orbitals in the electronic configuration of an ion?

A: To determine the number of electrons in the 3d and 4d orbitals in the electronic configuration of an ion, you need to know the number of protons and electrons in the atom. You can then use the periodic table to determine the electronic configuration of the atom, and then adjust it to account for the gain or loss of electrons.

Q: What is the significance of the 3d and 4d orbitals in the electronic configuration of an ion?

A: The 3d and 4d orbitals are significant in the electronic configuration of an ion because they determine the chemical properties of the element. The number of electrons in the 3d and 4d orbitals affects the reactivity of the element and its ability to form bonds with other elements.

Q: Can an element in Group VIII have a partially filled d-orbital?

A: No, an element in Group VIII cannot have a partially filled d-orbital. Group VIII consists of the noble gases, which have a full outer energy level and are unreactive.

Q: What is the difference between the electronic configuration of an atom and an ion in Group VIII?

A: The electronic configuration of an atom in Group VIII is the same as the electronic configuration of an ion in Group VIII. This is because the noble gases have a full outer energy level and are unreactive, which means that they do not gain or lose electrons to form ions.

Q: How do you determine the electronic configuration of an ion in Group VIII?

A: To determine the electronic configuration of an ion in Group VIII, you need to know the number of protons and electrons in the atom. You can then use the periodic table to determine the electronic configuration of the atom, and then adjust it to account for the fact that the element is a noble gas.

Q: What is the significance of the noble gas core in the electronic configuration of an ion in Group VIII?

A: The noble gas core in the electronic configuration of an ion in Group VIII indicates that the element has a full outer energy level, which is characteristic of the noble gases. This means that the element is unreactive and has a stable electronic configuration.