Question

Give three examples of +2 ions that have an electron configuration of \(n d^{10}(n=3,4,5 \ldots)\)

Short answer

Three examples of +2 ions with an \(n d^{10}\) electron configuration are: 1. Zinc ion (Zn+2) with electron configuration: \(3d^{10}\) 2. Cadmium ion (Cd+2) with electron configuration: \(4d^{10}\) 3. Mercury ion (Hg+2) with electron configuration: \(5d^{10}\)

Step-by-step solution

Understand the electron configuration of an \(n d^{10}\) ion

An ion with an electron configuration of \(n d^{10}\) has 10 electrons in its d subshell. Given that the value of n ranges from 3 to 5, we are looking at elements whose d subshell can be filled with 10 electrons after losing two electrons to form a +2 ion.

Identify elements that will have an \(n d^{10}\) electron configuration as +2 ions

For this step, we need to look at the periodic table and examine elements within the d-block, also known as the transition metals. Transition metals usually form positive ions by losing their valence electrons from the s-subshell before losing the d electrons. Here, we are looking for the elements that will achieve a fully filled d-subshell after losing two s electrons. Candidate 1: Zinc (Zn, atomic number 30) Zinc's electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2\). Upon losing 2 electrons (from the 4s subshell), Zinc's configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10}\), which is the \(n d^{10}\) configuration with n = 3. Candidate 2: Cadmium (Cd, atomic number 48) Cadmium's electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2\). Upon losing 2 electrons (from the 5s subshell), Cadmium's configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10}\), which is the \(n d^{10}\) configuration with n = 4. Candidate 3: Mercury (Hg, atomic number 80) Mercury's electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2 5p^6 4f^{14} 5d^{10} 6s^2\). Upon losing 2 electrons (from the 6s subshell), Mercury's configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2 5p^6 4f^{14} 5d^{10}\), which is the \(n d^{10}\) configuration with n = 5.

Provide the three examples of +2 ions with an \(n d^{10}\) electron configuration.

We found three examples of elements that, when forming a +2 ion, reach the \(n d^{10}\) electron configuration: 1. Zinc ion (Zn+2) with electron configuration: \(3d^{10}\) 2. Cadmium ion (Cd+2) with electron configuration: \(4d^{10}\) 3. Mercury ion (Hg+2) with electron configuration: \(5d^{10}\)

Key concepts

Transition Metals

Transition metals are elements located in the middle of the periodic table, specifically in the block known as the "d-block." These elements have partially filled d orbitals, which gives them unique properties. They often display a variety of oxidation states, typically forming multiple ions with different charges. This flexibility comes from their ability to lose different numbers of electrons depending on the chemical environment.

Transition metals are characterized by their ability to conduct electricity and heat, their high melting and boiling points, and their magnetic properties in some instances. They are crucial in many industrial processes and are found in everyday items like stainless steel and batteries. These metals can form complex ions, developing bonds with other ions or molecules that stabilize them or enhance their reactivity.

Understanding transition metals is essential in exploring their roles in catalysis, biological systems like hemoglobin in blood, and electronic applications.

D-Block Elements

D-block elements are found in groups 3 to 12 on the periodic table. These elements are distinguishable by their slowly filling d-orbitals. Each element in this block adds electrons to the d-orbital. As the period progresses across these groups, electrons in the d-subshell increase.

These elements are mostly metals and are known for forming colorful compounds, which is a consequence of d-d electron transitions. Moreover, exceptions in their electron configuration, like the half-filled or fully filled d-orbitals having extra stability, result in unique behaviors. For instance, the electron configuration for chromium ends in 4s^1 3d^5, deviating from the expected sequence to attain a half-filled stability.

In the context of ions, when a d-block element forms a positive ion, it generally loses electrons from the s-orbital first. That's why elements like Zn, Cd, and Hg are excellent examples. They lose their 2 s-electrons to become +2 ions with fully filled d-orbitals.

Ions

Ions are atoms or molecules with an unequal number of protons and electrons, resulting in a net charge. When atoms lose or gain electrons, they form positively or negatively charged ions, respectively.

For transition metals, forming cations (positively charged ions) involves the removal of electrons starting with those in the outer s-orbital. As a result, many transition metals form stable ions with an electron configuration where the d-orbitals are filled to 10 electrons. Examples are Zinc (\(Zn^{2+}\)), Cadmium (\(Cd^{2+}\)), and Mercury (\(Hg^{2+}\)) where their electronic configuration changes to fully occupied d-orbitals.

Understanding how ions form and behave is crucial, as they participate in reactions, conduct electricity in solutions, and are vital in various biological processes. For instance, iron ions are central in oxygen transport in the blood, while chloride ions contribute to nerve impulse transmission.