Question:
Diamond has low
Diamond has low
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Remember that diamond's properties are a direct result of its strong sp\(^3\) covalent network. This strong bonding leads to high hardness, high stiffness, and high thermal conductivity. The lack of free electrons leads to low electrical conductivity.
Updated On: Aug 31, 2025
- electrical conductivity
- modulus of elasticity
- hardness
- thermal conductivity
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept:
The question asks to identify a property for which diamond, a crystalline allotrope of carbon, exhibits a low value. This requires knowledge of the structure and bonding in diamond and how they influence its physical properties.
Step 2: Detailed Explanation:
Diamond consists of carbon atoms arranged in a face-centered cubic lattice, where each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral geometry (sp\(^3\) hybridization). These covalent bonds are extremely strong and rigid.
Let's analyze the properties listed:
- (C) Hardness: Due to the strong, directional covalent bonds throughout its structure, diamond is the hardest known natural material. It has a very high hardness.
- (B) Modulus of Elasticity: This property measures a material's stiffness or resistance to elastic deformation. The strong C-C bonds make diamond extremely stiff. It has a very high modulus of elasticity.
- (D) Thermal Conductivity: Although it is an electrical insulator, diamond is an excellent thermal conductor. The strong, rigid lattice is very efficient at transmitting heat via lattice vibrations (phonons). At room temperature, diamond has one of the highest thermal conductivities of any material, several times that of copper.
- (A) Electrical Conductivity: For a material to conduct electricity, it must have mobile charge carriers (like free electrons). In diamond, all four valence electrons of each carbon atom are localized in strong covalent bonds. There are no free electrons. The energy gap (band gap) between the valence band and the conduction band is very large (\(\sim\)5.5 eV), making it extremely difficult to excite electrons into the conduction band. Therefore, diamond is an excellent electrical insulator and has a very low electrical conductivity.
Step 3: Final Answer:
Among the given options, diamond has a low electrical conductivity.
Step 4: Why This is Correct:
Diamond is known for its extreme properties, being exceptionally hard, stiff, and thermally conductive. Its only "low" property on this list is its electrical conductivity, which makes it a classic electrical insulator.
The question asks to identify a property for which diamond, a crystalline allotrope of carbon, exhibits a low value. This requires knowledge of the structure and bonding in diamond and how they influence its physical properties.
Step 2: Detailed Explanation:
Diamond consists of carbon atoms arranged in a face-centered cubic lattice, where each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral geometry (sp\(^3\) hybridization). These covalent bonds are extremely strong and rigid.
Let's analyze the properties listed:
- (C) Hardness: Due to the strong, directional covalent bonds throughout its structure, diamond is the hardest known natural material. It has a very high hardness.
- (B) Modulus of Elasticity: This property measures a material's stiffness or resistance to elastic deformation. The strong C-C bonds make diamond extremely stiff. It has a very high modulus of elasticity.
- (D) Thermal Conductivity: Although it is an electrical insulator, diamond is an excellent thermal conductor. The strong, rigid lattice is very efficient at transmitting heat via lattice vibrations (phonons). At room temperature, diamond has one of the highest thermal conductivities of any material, several times that of copper.
- (A) Electrical Conductivity: For a material to conduct electricity, it must have mobile charge carriers (like free electrons). In diamond, all four valence electrons of each carbon atom are localized in strong covalent bonds. There are no free electrons. The energy gap (band gap) between the valence band and the conduction band is very large (\(\sim\)5.5 eV), making it extremely difficult to excite electrons into the conduction band. Therefore, diamond is an excellent electrical insulator and has a very low electrical conductivity.
Step 3: Final Answer:
Among the given options, diamond has a low electrical conductivity.
Step 4: Why This is Correct:
Diamond is known for its extreme properties, being exceptionally hard, stiff, and thermally conductive. Its only "low" property on this list is its electrical conductivity, which makes it a classic electrical insulator.
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