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Questions and Answers
What property makes diamonds particularly useful in cutting tools?
What property makes diamonds particularly useful in cutting tools?
Which aspect of diamond explains its inability to conduct electricity?
Which aspect of diamond explains its inability to conduct electricity?
What characteristic of graphite allows it to be used in pencil leads?
What characteristic of graphite allows it to be used in pencil leads?
Which property of graphite contributes to its use as a material for electrodes in electrolysis?
Which property of graphite contributes to its use as a material for electrodes in electrolysis?
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How do carbon nanotubes compare to graphite in terms of structure?
How do carbon nanotubes compare to graphite in terms of structure?
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What is a key feature of the covalent bonds in diamond?
What is a key feature of the covalent bonds in diamond?
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What distinguishes the electronic structure of graphite from that of diamond?
What distinguishes the electronic structure of graphite from that of diamond?
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Which of the following best describes the visual properties of diamond?
Which of the following best describes the visual properties of diamond?
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What characteristic of giant covalent structures leads to their very high melting points?
What characteristic of giant covalent structures leads to their very high melting points?
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Which of the following best describes the conductivity of graphite?
Which of the following best describes the conductivity of graphite?
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What distinguishes diamond from graphite in terms of atomic bonding?
What distinguishes diamond from graphite in terms of atomic bonding?
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Which property is NOT characteristic of diamond?
Which property is NOT characteristic of diamond?
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Why is graphite used as a lubricant?
Why is graphite used as a lubricant?
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What is a key feature of silica in relation to diamond?
What is a key feature of silica in relation to diamond?
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Which allotropes of carbon exhibit a similar structural property to diamond?
Which allotropes of carbon exhibit a similar structural property to diamond?
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What is the primary reason silicon is classified as a semiconductor?
What is the primary reason silicon is classified as a semiconductor?
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Study Notes
Giant Covalent Structures
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Giant covalent structures consist of many atoms held together by strong covalent bonds, forming a giant regular lattice structure.
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High melting points are a defining characteristic due to the extensive covalent bonds that need to be broken.
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Electrical conductivity varies, with some materials like diamond being non-conductive and others like graphite being conductive due to delocalized electrons. Silicon is a semiconductor.
Graphite
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Graphite is an allotrope of carbon with carbon atoms forming covalent bonds with three other carbon atoms.
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Each carbon atom has one delocalized electron, creating a layered structure enabling layer slippage and making graphite soft/easy to use as a lubricant.
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Delocalized electrons contribute to graphite's conductivity, making it suitable as electrodes.
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Despite softness, the strong covalent bonds within each layer give graphite high melting and boiling points.
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Graphite is black, shiny, opaque, and slippery.
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It is used in pencils and lubricants due to its layered structure.
Diamond
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Diamond is an allotrope of carbon where each carbon atom is bonded to four other carbon atoms.
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Diamond's rigid tetrahedral structure makes it very hard and has a very high melting point.
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It is insoluble in water and does not conduct electricity because there are no delocalized electrons.
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High hardness and high melting point make diamond suitable for cutting tools.
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Diamond is colourless, transparent, lustrous (sparkling).
Silica
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Silica (silicon dioxide) shares structural similarities with diamond and has similar properties like hardness and high melting points.
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Silica contains silicon and oxygen atoms instead of carbon.
Allotropes of Carbon
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Diamond, graphite, and fullerenes (including nanotubes and buckyballs) are different allotropes of pure carbon.
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Covalent bonds within their structures, however, the arrangements of atoms result in distinct properties.
Nanotubes
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Nanotubes are fullerene structures resembling graphite's layered structure.
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High melting point due to strong covalent bonds, similar to graphite and diamond.
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Conductivity due to delocalized electrons within the carbon structure.
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Description
Explore the fascinating world of giant covalent structures and understand the properties of graphite. This quiz covers the characteristics of covalent bonds, the unique attributes of graphite, and its applications. Test your knowledge about these essential materials in chemistry.
