Question

Complete the following reactions: (a) \(\mathrm{Be}_{2} \mathrm{C}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (c) \(\mathrm{Mg}_{2} \mathrm{C}_{3}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (d) \(\mathrm{Al}_{2} \mathrm{O}_{3}+\mathrm{NaOH} \longrightarrow\) (e) \(\mathrm{BeCl}_{2}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OC}_{2} \mathrm{H}_{5} \longrightarrow\)

Short answer

The complete reactions are: (a) \(\mathrm{Be}_{2}\mathrm{C} + \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Be(OH)}_{2} + \mathrm{CH}_{4}\), (b) \(\mathrm{Mg}_{2}\mathrm{C}_{3} + 4 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Mg(OH)}_{2} + \mathrm{C}_{2}\mathrm{H}_{2}\), (c) \(\mathrm{Al}_{2} \mathrm{O}_{3} + 2 \mathrm{NaOH} \longrightarrow 2 \mathrm{NaAlO}_{2} + \mathrm{H}_{2} \mathrm{O}\), (d) \(\mathrm{BeCl}_{2} + \mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OC}_{2}\mathrm{H}_{5} \longrightarrow \mathrm{BeCl}_{2}\cdot (\mathrm{O \ C_{2} H_{5})_{2}\).

Step-by-step solution

Complete the reaction of \(\mathrm{Be}_{2}\mathrm{C}+\mathrm{H}_{2} \mathrm{O}\)

Beryllium carbide \(\mathrm{Be}_{2} \mathrm{C}\) reacts with water to form Beryllium hydroxide and Methane. The balanced reaction is written as: \( \mathrm{Be}_{2}\mathrm{C} + \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Be(OH)}_{2} + \mathrm{CH}_{4}\)

Complete the reaction of \(\mathrm{Mg}_{2}\mathrm{C}_{3}+\mathrm{H}_{2} \mathrm{O}\)

Magnesium carbide \(\mathrm{Mg}_{2}\mathrm{C}_{3}\) reacts with water to form Magnesium hydroxide and Acetylene. The balanced reaction is: \(\mathrm{Mg}_{2}\mathrm{C}_{3} + 4 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Mg(OH)}_{2} + \mathrm{C}_{2}\mathrm{H}_{2}\)

Complete the reaction of \(\mathrm{Al}_{2} \mathrm{O}_{3}+\mathrm{NaOH}\)

Aluminium oxide \(\mathrm{Al}_{2} \mathrm{O}_{3}\) reacts with Sodium hydroxide to form Sodium aluminate. The balanced equation is: \(\mathrm{Al}_{2} \mathrm{O}_{3} + 2 \mathrm{NaOH} \longrightarrow 2 \mathrm{NaAlO}_{2} + \mathrm{H}_{2} \mathrm{O}\)

Complete the reaction of \(\mathrm{BeCl}_{2}+\mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OC}_{2}\mathrm{H}_{5}\)

Beryllium chloride \(\mathrm{BeCl}_{2}\) reacts with Diethyl ether \(\mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OC}_{2}\mathrm{H}_{5}\) to form a complex compound. The reaction results in the formation of a coordination complex with the formula \(\mathrm{BeCl}_{2}\cdot \mathrm{(O \ C_{2} H_{5})_{2}}\), the balanced equation is: \(\mathrm{BeCl}_{2} + \mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OC}_{2}\mathrm{H}_{5} \longrightarrow \mathrm{BeCl}_{2}\cdot (\mathrm{O \ C_{2} H_{5})_{2}\)

Key concepts

Beryllium Carbide Reactions

Beryllium carbide, denoted as \( \mathrm{Be}_{2}\mathrm{C} \), undergoes a fascinating reaction with water. When \( \mathrm{Be}_{2}\mathrm{C} \) contacts water, it forms beryllium hydroxide and methane. This reaction is important because it highlights how certain carbides break down in the presence of water to create hydroxides and gaseous products.
The balanced equation is:

• \( \mathrm{Be}_{2}\mathrm{C} + 4 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Be(OH)}_{2} + \mathrm{CH}_{4} \)

Beryllium hydroxide formed here is a white solid that slowly settles in the solution. Methane, being a gas, escapes into the atmosphere.
This type of reaction is a typical example of a hydrolysis reaction where water plays a key role, breaking down complex compounds into simpler ones. Understanding these types of processes is critical for students studying inorganic chemistry, as similar reactions are fundamental in industrial and environmental chemistry processes.

Magnesium Carbide Reactions

Magnesium carbide, \( \mathrm{Mg}_{2}\mathrm{C}_{3} \), reacts differently compared to other carbides. In contact with water, \( \mathrm{Mg}_{2}\mathrm{C}_{3} \) forms magnesium hydroxide and acetylene, a flammable gas commonly used in welding.
This balanced chemical equation for this reaction is:

• \( \mathrm{Mg}_{2}\mathrm{C}_{3} + 4 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{Mg(OH)}_{2} + \mathrm{C}_{2}\mathrm{H}_{2} \)

This type of reaction is characteristic of acetylide compounds, which typically produce alkynes such as acetylene upon hydrolysis.
Acetylene is a gas that burns with a hot flame. The formation of the hydroxide adds a layer of complexity to this reaction, demonstrating how metallic carbides can be versatile in producing both solids and gases.
Understanding this reaction is essential in grasping the chemistry of metal carbides and their uses, as well as the production of important industrial products.

Aluminium Oxide Reactions

Aluminium oxide, \( \mathrm{Al}_{2} \mathrm{O}_{3} \), is an amphoteric oxide that can react with both acids and bases. When aluminium oxide is treated with sodium hydroxide (a base), it forms sodium aluminate. This reaction highlights aluminium oxide's dual nature in terms of reactivity.
The balanced chemical equation is:

• \( \mathrm{Al}_{2} \mathrm{O}_{3} + 2 \mathrm{NaOH} \longrightarrow 2 \mathrm{NaAlO}_{2} + \mathrm{H}_{2} \mathrm{O} \)

In this process, \( \mathrm{NaAlO}_{2} \) is formed as a colorless or white powder or gelatinous precipitate.
This kind of reaction is useful in various industries, such as water purification and manufacturing of building materials.
Allocating time to understand such reactions is crucial for students, as it underscores the versatility and importance of aluminium compounds in both laboratory and practical applications.

Coordination Complex Formation

The formation of coordination complexes is an intriguing area in inorganic chemistry. When beryllium chloride (\( \mathrm{BeCl}_{2} \)) reacts with diethyl ether (\( \mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OC}_{2}\mathrm{H}_{5} \)), it results in a coordination complex.
The complex formed, \( \mathrm{BeCl}_{2}\cdot (\mathrm{O \ C_{2} H_{5})_{2}} \), showcases the ability of certain compounds to surround a metal with ligands (in this case, the ether acting as a ligand). This is significant because it demonstrates how metals like beryllium can form stable compounds with non-metal atoms or molecules, enhancing their chemical stability and reactivity.
Coordination complexes are widespread in chemistry, with applications ranging from catalysis to materials science.
By studying these reactions, students can gain insight into how metals can be stabilized or activated through their interactions with surrounding ligands, opening up myriad opportunities for new materials and reactions.