Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

Understanding the chemical reactions of oxides with water is crucial for grasping how different materials interact with water to form new substances. Oxides are compounds that include at least one oxygen atom bound to another element, like a metal or nonmetal. When oxides react with water, they typically form either a base or an acid.

Basic oxides, often formed by metals such as sodium (Na) and barium (Ba), will react to produce hydroxides. For example, when sodium oxide ((Na_2O)) reacts with water ((H_2O)), sodium hydroxide ((NaOH)) is formed, which is a strong base used in many industrial processes. Similarly, barium oxide ((BaO)) reacts with water to produce barium hydroxide ((Ba(OH)_2)), also a strong base.

On the other hand, acidic oxides are typically derived from nonmetals. Carbon dioxide ((CO_2)), for instance, reacts with water to produce carbonic acid ((H_2CO_3)), a weak acid. Other examples include nitrogen pentoxide ((N_2O_5)) which forms nitric acid ((HNO_3)) and sulfur trioxide ((SO_3)) forming sulfuric acid ((H_2SO_4)), both of which are stronger acids used commercially.

Examples of Reactions

• (Na_2O) + (H_2O) -> 2(NaOH)
• (BaO) + (H_2O) -> (Ba(OH)_2)
• (CO_2) + (H_2O) -> (H_2CO_3)
• (N_2O_5) + (H_2O) -> 2(HNO_3)
• (SO_3) + (H_2O) -> (H_2SO_4)

The byproducts of these reactions have various applications in everyday life, from fertilizers to cleaning agents, reflecting the importance of understanding these chemical processes.

Metallic and nonmetallic oxides display distinct physical and chemical properties that determine their reactivity and the types of compounds they form when reacting with water. Metallic oxides, or basic oxides, are typically solid at room temperature and will readily dissolve in water to form metal hydroxides which are alkaline solutions. These oxides are electrical conductors due to the presence of free electrons in their structure.

Nonmetallic oxides, on the contrary, are acidic and often form gaseous compounds such as carbon dioxide ((CO_2)) or liquids like sulfur trioxide ((SO_3)). They do not conduct electricity as their bonding does not allow for free-moving electrons. When dissolved in water, nonmetallic oxides produce acidic solutions, which can have corrosive properties and require careful handling.

Moreover, the solubility and strength of the acids or bases formed upon the reaction with water can vary. For instance, the base formed by sodium oxide is much stronger and more soluble than that formed by barium oxide. In the case of acidic oxides, sulfur trioxide forms a stronger acid than carbon dioxide when reacted with water.

The polarity and electronegativity of the elements also influence the properties of the oxides. Generally, the higher the electronegativity difference between oxygen and the other element, the more acidic the oxide. This concept is central in predicting and understanding the behavior of various oxides in chemical reactions.

Writing balanced chemical equations is a fundamental skill required for studying chemical reactions. These equations must follow the law of conservation of mass, meaning the number of atoms for each element must be the same on both sides of the equation. To write a balanced equation, one must first correctly identify the reactants and products involved in the chemical reaction and then apply coefficients to ensure equal numbers of atoms for each element on both sides of the reaction.

Referencing the reactions of oxides with water, we can examine the process of balancing chemical equations with one example: for the reaction between sodium oxide ((Na_2O)) and water, sodium hydroxide ((NaOH)) is formed. The unbalanced equation looks like this: (Na_2O) + (H_2O) -> (NaOH). To balance it, we observe that there are two sodium atoms on the left side, so we add a coefficient of 2 in front of (NaOH) on the right side, which gives us (Na_2O) + (H_2O) -> 2(NaOH).

Similarly, for the reaction of sulfur trioxide with water, we start with (SO_3) + (H_2O) -> (H_2SO_4). Since there is already one sulfur atom and four oxygen atoms on both sides, the equation is balanced.

Practice Tip

To improve skills in writing balanced equations, practice with various chemical reactions, use stoichiometry to verify the coefficients, and remember to balance the more complicated molecules first, as they often determine the coefficients for the simpler substances. This orderly approach simplifies the task and brings clarity to the process of balancing chemical equations.