Organic Chemistry Some Basic Principles and Techniques
2022
chemistry
Diamond and graphite have two-dimensional network structures.
Diamond is covalent, and graphite is ionic.
Diamond is sp3 hybridized, and graphite is sp2 hybridized.
Both diamond and graphite are used as dry lubricants.
Explanation
To solve this problem, we need to analyze the structure and bonding of diamond and graphite.• Diamond and graphite are both allotropes of carbon, meaning they are different structural forms of the same element.• In diamond, each carbon atom is sp3 hybridized, forming a three-dimensional network. Each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral geometry.• In graphite, each carbon atom is sp2
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hybridized, forming a two-dimensional planar structure. Each carbon atom is covalently bonded to three other carbon atoms in a trigonal planar geometry, with delocalized electrons allowing for electrical conductivity.
Now, let's evaluate each option:
Option 1: Diamond and graphite have two-dimensional network structures.
• This is incorrect. Diamond has a three-dimensional network structure, while graphite has a two-dimensional planar structure.
Option 2: Diamond is covalent, and graphite is ionic.
• This is incorrect. Both diamond and graphite are covalent structures. Graphite has delocalized electrons, but it is not ionic.
Option 3: Diamond is
sp3
hybridized, and graphite is
sp2
hybridized.
• This is correct. Diamond is
sp3
hybridized, and graphite is
sp2
hybridized.
Option 4: Both diamond and graphite are used as dry lubricants.
• This is incorrect. Graphite is used as a dry lubricant due to its layered structure, but diamond is not used as a lubricant.