Question

Explain why metal oxides tend to be basic if the oxidation number of the metal is low and tend to be acidic if the oxidation number of the metal is high. (Hint: Metallic compounds in which the oxidation numbers of the metals are low are more ionic than those in which the oxidation numbers of the metals are high.)

Short answer

Low oxidation states lead to ionic, basic oxides; high states to covalent, acidic ones.

Step-by-step solution

Understanding Metal Oxides

Metal oxides are compounds consisting of metal cations from the periodic table and oxide anions \((O^{2-})\). They are formed when metals react with oxygen, and their properties can be classified broadly as basic or acidic.

Low Oxidation States and Ionic Character

When metals have low oxidation states, typically, their oxides are more ionic. Ionic bonds involve the transfer of electrons, creating charged ions that easily dissociate in water, forming hydroxide ions \((OH^-)\). This process is characteristic of basic solutions.

High Oxidation States and Covalent Character

Metal oxides with high oxidation states are generally more covalent. Covalent bonds involve the sharing of electrons, which does not easily dissociate in water. These oxides can react with water to form acids or dissolve to give acidic solutions.

Ionic vs. Covalent Nature Impact

Low oxidation numbers favor the formation of ionic compounds, leading to basic oxides because they readily generate hydroxide ions in solution. In contrast, high oxidation numbers increase covalent character, making oxides that tend to form acidic solutions.

Concluding the Trend

The trend shows that as the oxidation state of the metal increases, the nature of the metal oxide changes from ionic to covalent, which corresponds to a transition from basic to acidic properties.

Key concepts

Oxidation State

The oxidation state or oxidation number of a metal in an oxide plays a critical role in determining the oxide's chemical properties. Generally, the oxidation state is a measure of the degree of oxidation of an atom in a compound. But why does it matter so much in metal oxides?

When a metal exhibits a low oxidation state, it typically forms oxides that are more ionic. In an ionic bond, electrons are transferred from the metal to the oxide ion, creating a strong electrostatic attraction between the charged particles. Metals in lower oxidation states, such as alkali and alkaline earth metals, tend to form oxides that create basic solutions in water. This is because these ionic oxides can easily dissociate, releasing hydroxide ions \((OH^-\)).

Conversely, metals with high oxidation states often form more covalent bonds, where electrons are shared rather than transferred. These covalent compounds are less likely to dissociate in water, meaning instead of producing basic solutions, they usually contribute to acidic solutions. Therefore, the oxidation state gives a good indirect indication of whether a metal oxide will behave in a basic or acidic manner.

Basic and Acidic Properties

Metal oxides exhibit either basic or acidic properties, primarily depending on the oxidation state of the metal involved. Understanding thus helps predict the behavior of these compounds when mixed in an aqueous environment.

- **Basic Oxides**: These are typical of metals with low oxidation states. When dissolved in water, these compounds tend to dissociate and produce hydroxide ions. An example is calcium oxide \((CaO)\), which forms the basic solution calcium hydroxide \((Ca(OH)_2)\) when combined with water.

- **Acidic Oxides**: In contrast, metals with high oxidation states form oxides that behave as acids in water. They don't generate hydroxide ions but rather react with water or bases to produce acids. A classic example is sulfur trioxide \((SO_3)\), which forms sulfuric acid \((H_2SO_4)\) when reacted with water.

This behavior is also aligned with the nature of the bonds formed. Fresher, ionic oxides are typically basic, while more mature, covalent oxides contribute to acidity. Thus, by analyzing an oxide's basic or acidic properties, one can infer information about the oxidation state of its metal.

Ionic and Covalent Compounds

The distinction between ionic and covalent compounds offers insights into the nature of metal oxides. This plays a significant role in understanding their behaviors and properties.

**Ionic Compounds**:
- These compounds form when metals in low oxidation states transfer electrons to oxygen. Notable for their strong electrostatic forces between ions, they easily dissociate in water, generating solutions rich in hydroxide ions.
- Common examples include the alkali metal oxides like sodium oxide \((Na_2O)\), which dissolves in water to form sodium hydroxide \((NaOH)\).

**Covalent Compounds**:
- Predominantly formed by metals with high oxidation states, these compounds exhibit shared electrons between the atoms, resulting in a significant covalent character. Such compounds do not readily dissociate into ions.
- Their interaction with water results in acidic solutions. For instance, phosphorous pentoxide \((P_4O_{10})\) reacts with water to form phosphoric acid \((H_3PO_4)\).

In essence, whether a metal oxide behaves ionically or covalently hinges on the metal's oxidation state. This categorization helps anticipate whether a simple metal oxide will contribute more towards basicity or acidity in solution.