Question

Find three examples of ions in the periodic table that have an electron configuration of \(n d^{8}(n=3,4,5 \ldots) .\)

Short answer

Three examples of ions in the periodic table that have an electron configuration of \(n d^{8}(n=3,4,5 \ldots)\) are: 1. \(Pd^{2+}\) with a \(4 d^8\) electron configuration. 2. \(Pt^{2+}\) with a \(5 d^8\) electron configuration. 3. \(Ir^{-}\) with a \(5 d^8\) electron configuration.

Step-by-step solution

Recall the periodic table structure and electron configurations

In order to solve this exercise, we need to recall the structure of the periodic table, and the rules for writing electron configurations. The periodic table is divided into groups (columns) and periods (rows). The elements in the same group have the same number of valence electrons. The electron configuration determines the distribution of electrons in the atomic orbitals. The electron configuration follows Aufbau principle, Hund's rule and Pauli's exclusion principle, and can be written in the form of \(\text{Principal Quantum Number} (\text{Orbital})^{\text{Number of Electrons}}\), such as "1s²2s²2p²".

Find the elements with the corresponding electron configurations

Now we need to find the elements with electron configurations of \(n d^{8}(n=3,4,5 \ldots)\). In general, these configurations are common in the transition metals which are located in the d-block of the periodic table.

Determine the three ions with \(nd^8\) electron configuration

To obtain ions with given electron configurations, we need to focus on comparing the general electron configuration of their neutral state and the following given configurations: 1. \(3 d^{8}\) 2. \(4 d^{8}\) 3. \(5 d^{8}\) As our first example, consider the neutral palladium (Pd) atom, which has an electron configuration of [Kr] \(4 d^{10} 5 s^0\). If we remove two electrons from the 4d orbital, we get the \(Pd^{2+}\) ion with an electron configuration of [Kr] \(4 d^8\). For the second example, let's look at the neutral platinum (Pt) atom. It has an electron configuration of [Xe] \(4 f^{14} 5 d^{9} 6 s^1\). If we remove an electron from the 5d orbital and another from the 6s orbital, we get the \(Pt^{2+}\) ion with an electron configuration of [Xe] \(4 f^{14} 5 d^{8}\). For the third example, let's take the neutral iridium (Ir) atom. Its electron configuration is [Xe] \(4 f^{14} 5 d^{7} 6 s^2\). If we add an electron to the 5d orbital, we get the \(Ir^{-}\) ion with an electron configuration of [Xe] \(4 f^{14} 5 d^{8}\). These three ions are examples for the given electron configurations: \(Pd^{2+}\) with a \(4 d^8\) electron configuration, \(Pt^{2+}\) with a \(5 d^8\) electron configuration, and \(Ir^{-}\) with a \(5 d^8\) electron configuration.

Key concepts

Transition Metals

Transition metals are a group of elements found in the center of the periodic table. They are located in the d-block, which means their valence electrons are filling the d orbitals. This gives them unique properties, such as the ability to form a variety of different ions. These metals are known for their colorful compounds and are often used in industrial applications, such as catalysts.

One interesting aspect of transition metals is their variable oxidation states. This ability comes from their d orbital electrons that can be easily removed or shared.

• This adaptability allows transition metals to form complex ions and coordination compounds.
• For example, iron can exist as Fe²⁺ or Fe³⁺, forming different compounds.

Understanding the electron configuration of transition metals is crucial to predict their chemical behavior. This helps in determining how they combine to form ions and compounds.

Periodic Table

The periodic table is a visual representation of all known chemical elements. It's organized by increasing atomic number and arranged in rows called periods, and columns called groups.

The periodic table helps predict the properties of elements based on their position. Each element's electron configuration, including the type of orbital and the number of valence electrons, is influenced by where they are in the table.

• Elements in the same group have similar valence electron configurations, contributing to their chemical similarities.
• The transition metals are found between groups 3 to 12, characterized by their d-block electron configurations.

These principles make the periodic table an essential tool for chemists and students, aiding in the understanding of both elemental and ionic behaviors.

Ions in Chemistry

In chemistry, ions are atoms or molecules that have gained or lost electrons, resulting in a net charge. When atoms lose electrons, they become positively charged (cations), and when they gain electrons, they become negatively charged (anions).

Understanding ions is crucial in predicting the electron configuration of various chemical species. This is especially true for transition metals, which often form different ions based on their need to achieve a stable electron configuration.

• For example, a copper atom can be ionized to form either Cu⁺ or Cu²⁺.
• When an atom like palladium forms a Pd²⁺ ion, it loses two electrons, typically from its outermost s and d orbitals.

Through gaining or losing electrons, atoms achieve the configuration of a noble gas, resulting in a lower energy and more stable state.

Aufbau Principle

The Aufbau Principle is a rule used to determine the electron configurations of atoms. It states that electrons fill atomic orbitals starting with the lowest energy levels before moving to higher ones. The order of filling is defined by the increasing energy of the orbitals.

This principle is applied when writing the electron configurations of elements, ensuring that the electron structure is accurately represented.

• Electrons first fill the 1s orbital, followed by 2s, 2p, 3s, and so on.
• For transition metals, electrons fill the d orbitals only after s orbitals of the same principal quantum number have been filled.
• For example, in an ion like Pd²⁺, the electrons are removed first from the 5s orbital, and then from the 4d orbital.

By understanding and applying the Aufbau Principle, one can predict the arrangement of electrons in an atom or ion, which is essential for understanding its chemical reactivity and properties.