Giant covalent structures, such as diamond, graphite, and silicon dioxide, are composed of atoms bonded in extensive networks. Diamond's unmatched hardness stems from a tetrahedral carbon lattice, while graphite's layered structure allows for electrical conductivity and lubrication. Silicon dioxide, found in quartz, is pivotal in industries from electronics to construction due to its durability and thermal stability. These materials showcase diverse applications and significant technological importance.
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Giant covalent structures are vast assemblies of atoms held together by covalent bonds in a continuous network
Diamond
Diamond is a prime example of a giant covalent structure, with each carbon atom bonded to four others in a three-dimensional lattice
Graphite
Graphite is distinctive among giant covalent structures due to its layered arrangement and delocalized electrons, allowing for electrical conductivity
Silicon Dioxide
Silicon dioxide, or silica, is a widespread giant covalent structure found in nature as quartz and is the main ingredient in sand and glass
Giant covalent structures have high melting and boiling points due to the strong covalent bonds that require significant energy to break
While most giant covalent structures are poor conductors of electricity, graphite is an exception due to its delocalized electrons
Giant covalent structures are typically insoluble in water and exhibit low chemical reactivity, making them stable and durable materials
Diamond's renowned hardness and optical properties make it valuable in both ornamental and industrial applications
Graphite's lubricating properties and electrical conductivity make it useful in applications such as electrodes and batteries
Silicon dioxide's high hardness and thermal stability make it essential in industries ranging from electronics to construction
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Substances like ______, ______, and ______ (SiO2) are examples of materials with a single, extensive molecule forming their structure.
diamond
graphite
silicon dioxide
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Melting/Boiling Points of Giant Covalent Structures
High due to strong covalent bonds needing significant energy to break.
02
Electrical Conductivity in Giant Covalent Structures
Generally poor, except for graphite which has delocalized electrons allowing conductivity.
