Question

Use the periodic table to identify the elements in the following list with unfilled \(4 d\) orbitals: rhodium, rhenium, ruthenium, rutherfordium, radium.

Short answer

Rhodium (Rh) and Ruthenium (Ru) have unfilled 4d orbitals.

Step-by-step solution

Understand the Problem

We need to identify which elements from the given list have unfilled \(4d\) orbitals. The elements in question are rhodium, rhenium, ruthenium, rutherfordium, and radium.

Locate Each Element on the Periodic Table

The elements rhodium (Rh), rhenium (Re), ruthenium (Ru), rutherfordium (Rf), and radium (Ra) should be located on the periodic table. Remember that \(4d\) orbitals start filling in the 4th period (row) of the transition metals section.

Determine the Electron Configuration

Determine the electron configuration for each element:- **Rhodium (Rh):** [Kr] \(4d^8 5s^1\)- **Rhenium (Re):** [Xe] \(5d^5 6s^2\)- **Ruthenium (Ru):** [Kr] \(4d^7 5s^1\)- **Rutherfordium (Rf):** [Rn] \(5f^{14} 6d^2 7s^2\)- **Radium (Ra):** [Rn] \(7s^2\)

Identify Unfilled 4d Orbitals

Compare the electron configurations to see which elements have unfilled \(4d\) orbitals. Elements that have unfilled \(4d\) orbitals will have less than 10 electrons in their \(4d\) configuration.

Conclude Which Elements Have Unfilled 4d Orbitals

Comparing the configurations:- **Rhodium (Rh):** \(4d^8\) has 8 electrons in the \(4d\) sublevel (unfilled)- **Ruthenium (Ru):** \(4d^7\) has 7 electrons in the \(4d\) sublevel (unfilled)Rhenium, rutherfordium, and radium do not have unfilled \(4d\) orbitals as their configurations involve other d sublevels.

Key concepts

Electron Configuration

Electron configuration is a way of representing how electrons are distributed in an atom. It is critical in determining the chemical behavior of an element. Each electron shell, such as the 1s, 2p, 3d, has a specific number of orbitals and each orbital can hold two electrons. Let's start by understanding the notations used in electron configurations:

• The numbers represent the energy levels (shells). For instance, "1" corresponds to the first shell, "2" to the second, and so on.
• The letters (s, p, d, f) correspond to the type of subshell, indicating the shape of the orbital.
• The superscript numbers show the number of electrons in that subshell.

For example, rhodium's electron configuration is written as [Kr] \(4d^8 5s^1\). This means it has eight electrons in the 4d subshell and one electron in the 5s subshell, after the 36 electrons accounted for by krypton (Kr). Understanding this helps us see which d orbitals are filled and which are not.

Transition Metals

Transition metals are elements found in the d-block of the periodic table, spanning groups 3 to 12. These metals are characterized by the filling of d orbitals in their electron configurations. A few properties of transition metals include:

• They often form colored compounds.
• They can exhibit multiple oxidation states.
• They are good conductors of heat and electricity.
• They have high melting and boiling points.

These elements are essential in forming the central block of the periodic table and, as such, they have unique filling patterns for d orbitals. For example, in the context of our exercise, rhodium and ruthenium are transition metals in the 4th period with specific d orbital configurations that are not fully filled, making them notable for their incomplete 4d orbitals.

4d Orbitals

4d orbitals refer to a specific set of d orbitals present in the fourth energy level of an atom. They start becoming relevant in the electron configurations of elements within the transition metals area of the periodic table.Let's break down what makes up 4d orbitals:

• The "4" indicates the fourth principal energy level.
• The "d" indicates the type of subshell, known for its cloverleaf shape.

When talking about "unfilled 4d orbitals," we refer to configurations with less than the maximum 10 electrons. In our example, both rhodium (Rh) with a configuration of \(4d^8\), and ruthenium (Ru) with \(4d^7\), have not fully populated their 4d subshells. This leaves room for chemical and physical properties that are distinct due to these unfilled 4d orbitals.

Unfilled Orbitals

Unfilled orbitals are significant because they affect the chemical and physical properties of an element. Orbitals can contain a certain number of electrons: the s orbital holds 2, the p holds 6, the d holds 10, and the f holds 14. If these orbitals are not full, it impacts how atoms bond with others.In the case of 4d orbitals:

• A fully filled 4d subshell has 10 electrons.
• An unfilled 4d subshell, such as those in rhodium (\(4d^8\)) and ruthenium (\(4d^7\)), means there are fewer than 10 electrons.

These unfilled states allow for potential bonding sites with other atoms or molecules, influencing magnetism, catalytic properties, and more. Therefore, understanding which orbitals are unfilled is important for studying these atoms' interactions and behaviors.