Question

Match the following (a) Boron (p) Amphoteric oxide (b) Carbon (q) Acidic oxide (c) Silicon (r) Catenation (d) Phosphorous (s) Allotropy

Short answer

(a) Boron - p, (b) Carbon - r, (c) Silicon - q, (d) Phosphorous - s.

Step-by-step solution

Understanding the Terms

Before matching, it's important to understand the properties and definitions of each option provided. - **Boron**: Known for forming compounds showing amphoteric behavior. - **Carbon**: Well-known for its ability to catenate, forming long chains of molecules. - **Silicon**: Typically forms acidic oxides. - **Phosphorous**: Exists in several different structural forms, showing allotropy.

Match Boron with Its Property

Boron forms oxides that can behave as either acidic or basic under different conditions. This property is known as amphoterism. Therefore, Boron matches with __Amphoteric oxide (p)__.

Match Carbon with Its Property

Carbon's ability to form long chains by connecting with itself is known as catenation. Thus, Carbon matches with __Catenation (r)__.

Match Silicon with Its Property

Silicon typically forms compounds like silicon dioxide (SiO2), which act as acidic oxides. Therefore, Silicon matches with __Acidic oxide (q)__.

Match Phosphorous with Its Property

Phosphorous has different structural forms such as white, red, and black phosphorous, demonstrating allotropy. Thus, Phosphorous matches with __Allotropy (s)__.

Key concepts

Amphoteric Oxide

An amphoteric oxide is a type of oxide that can react both as an acid and as a base. This unique behavior allows the compound to neutralize both acids and bases, which gives it a versatile chemical profile. Amphoteric oxides typically occur in elements that are found in the middle of the periodic table, particularly the metalloids and some metals.
For instance, boron forms boron trioxide (B\(_2\)O\(_3\)), which can react with both acids, like hydrochloric acid, and bases, such as sodium hydroxide, to form different products. This dual reactivity makes amphoteric oxides particularly interesting, as they can participate in a wide range of chemical reactions.

• Common examples: Boron trioxide, aluminum oxide (Al\(\_2\)O\(\_3\)), zinc oxide (ZnO)
• Reacts with both acids and bases

This concept is particularly important in various applications, including metallurgy and the production of ceramics.

Catenation

Catenation is the ability of an element to form chains with its own atoms. This property is most pronounced in carbon, which can form stable, covalent bonds with other carbon atoms, allowing the formation of long chains and complex structures. This property is central to organic chemistry as it is the basis for the vast variety of organic compounds.
Carbon's unique ability comes from its tetravalency, allowing it to create four covalent bonds with other atoms including itself. This leads to the formation of various allotropes of carbon, such as diamond and graphite, each with different properties. Other elements, like silicon and sulfur, also exhibit catenation but to a lesser degree due to differences in their bonding abilities.

• Key element: Carbon
• Forms chains and rings: vital for organic molecules
• Essential for polymers and life-forms (e.g., proteins, DNA)

Acidic Oxide

Acidic oxides are oxides of non-metals that react with water to form acids or with bases to form salts. They are typically formed by the oxidation of nonmetals. Silicon, for instance, forms silicon dioxide (SiO\(_2\)), a classic example of an acidic oxide.
When acidic oxides interact with water, they tend to form oxyacids. For example, carbon dioxide (CO\(_2\)) reacts with water to produce carbonic acid. These oxides are important in understanding atmospheric chemistry and the behavior of pollutants.

• Formed by non-metals: often found in nature
• Reacts with water to form acids (e.g., CO\(_2\) forms carbonic acid)
• Neutralizes bases to form salts

Their role is significant in environmental science, particularly in the study of acid rain and pollution control.

Allotropy

Allotropy refers to the existence of two or more different forms of the same element in the same physical state. These different forms, known as allotropes, typically vary in structure and, consequently, exhibit different chemical and physical properties.
A well-known example of allotropy is phosphorus, which exists in several forms, including white, red, and black phosphorus. Each form has distinct properties; for instance, white phosphorus is highly reactive and toxic, while red phosphorus is more stable and less reactive. Other examples include the different forms of carbon, such as diamond (a hard, transparent structure) and graphite (a soft, opaque material).

• Occurs in some elements like phosphorus and carbon
• Different structural forms = different properties
• Applications range from industrial to daily-use materials

Understanding allotropy is crucial for material science and chemistry, particularly in synthesizing new materials with desired properties.