Question

What is the highest oxidation state for each of the elements from Sc to \(\mathrm{Zn} ?\)

Short answer

The highest oxidation states are Sc (+3), Ti (+4), V (+5), Cr (+6), Mn (+7), Fe (+6), Co (+5), Ni (+4), Cu (+3), Zn (+2).

Step-by-step solution

Understanding the Concepts

The oxidation state of an element is commonly defined by how many electrons are added, lost, or shared during a chemical reaction in comparison to its most stable ground state. In the case of transition metals, they can exhibit several oxidation states.

Consider Transition Metals

Scandium (Sc) through Zinc (Zn) are transition metals located in the first row of the d-block in the periodic table. Usually, the highest oxidation state for these elements corresponds to the total number of electrons in their outer s and d sub-shells.

Determine Subshell Electron Counts

Each element from Sc to Zn is adding electrons to the 3d and 4s subshells. For example, Sc has the electron configuration \([\text{Ar}] 3d^1 4s^2\). The sum of these electrons gives the highest oxidation state.

Calculate Highest Oxidation States

The highest oxidation state is found by summing the electrons in 3d and 4s subshells. For Sc (1+2=3), for Ti (2+2=4), up to Zn (10+2=12).

List Highest Oxidation States

The highest oxidation states for the elements Sc to Zn are respectively: Sc (+3); Ti (+4); V (+5); Cr (+6); Mn (+7); Fe (+6); Co (+5); Ni (+4); Cu (+3); Zn (+2).

Key concepts

Transition Metals

Transition metals are a set of chemical elements found in the "d-block" of the periodic table, specifically from scandium (Sc) to zinc (Zn). These metals are known for their unique properties, such as their ability to form multiple oxidation states. This means they can lose or gain different numbers of electrons during chemical reactions, allowing them to form a wide variety of compounds. This characteristic is mainly due to the presence of electrons in both their outer s and d subshells.
These metals are essential in many industrial processes and biological systems. They are often good conductors of electricity and heat, due to their ability to allow electrons to move freely. In addition, transition metals can serve as catalysts, meaning they speed up chemical reactions without being consumed in the process.
Understanding transition metals and their oxidation states is crucial for predicting the behavior of these elements in different chemical reactions, as well as for designing new materials with desirable properties.

Electron Configuration

Electron configuration is a way to describe the distribution of electrons in an atom of an element. For transition metals, the electron configuration plays a key role in determining their chemical properties, including their oxidation states.
These configurations are represented by the arrangement of electrons in an atom's electron shells and subshells. For instance, transition metals from scandium to zinc have their electrons gradually added to the 3d and 4s subshells. The electron configuration of scandium is \([ ext{Ar}] 3d^1 4s^2\), showing the presence of three valence electrons that contribute to its highest oxidation state of +3.
The filling of the 3d subshell gives rise to complex behavior, allowing these elements to adopt various oxidation states through the loss or sharing of these d electrons. Understanding electron configurations is essential for grasping why transition metals can exhibit such diverse chemical reactions and binding properties.

D-block Elements

D-block elements, often referred to as transition metals, include elements located in the center of the periodic table in groups 3 through 12. These elements are characterized by the gradual filling of the d subshell, which contributes significantly to their unique chemical behavior.
The d-block elements are notable for a few key characteristics:

• They commonly form colored compounds, due to d-d electron transitions.
• Most elements in this block have high melting and boiling points.
• These elements exhibit magnetic properties.

As the d subshell is filled from Sc (3d^1) to Zn (3d^{10}), these elements display variability in their chemical and physical properties.
Understanding the role of the d-block in the periodic table helps in predicting and explaining the colorful and complex nature of transition metal chemistry. From catalysis to metallurgy, these elements play a vital role in numerous scientific and industrial areas.