Describe the structure of diamond .

In diamond , each carbon atom is bonded to four others in a tetrahedral arrangement, forming a giant covalent lattice. There are no free electrons and no intermolecular forces — only very strong covalent bonds throughout.

In graphite, each carbon atom is bonded to ______ others, forming layers of ______ rings. One electron per atom becomes ______ .

In graphite, each carbon atom is bonded to three others, forming layers of hexagonal rings. One electron per atom becomes delocalised .

True or False? Graphite acts as a lubricant because the covalent bonds between its layers are broken, allowing the layers to slide.

False. The covalent bonds within each layer are strong and are not broken during lubrication. Graphite is slippery because the weak forces between the layers can be overcome easily, allowing the layers to slide over each other.

Why is graphite suitable for use as an electrode in electrolysis?

Graphite is suitable as an electrode because it is chemically inert (unreactive), has good electrical conductivity due to its delocalised electrons, and has a high melting point so it does not melt during use.

True or False? Silicon(IV) oxide (SiO 2 ) is found as an impurity in iron ore and is removed during the blast furnace process.

True. SiO 2 is present as an impurity in iron ore. In the blast furnace, it reacts with calcium oxide to form calcium silicate (slag), which is removed as a waste product.

Silicon(IV) oxide (SiO 2 ) has properties similar to diamond because both have ______ covalent structures with ______ covalent bonds throughout.

Silicon(IV) oxide (SiO 2 ) has properties similar to diamond because both have giant covalent structures with strong covalent bonds throughout.

True or False? Diamond and graphite are different elements because they have different structures and properties.

False. Diamond and graphite are both allotropes of the element carbon . They contain only carbon atoms but have different bonding arrangements, which gives them completely different properties.

O LevelChemistryCambridge (CIE)Flashcards2. Atoms, Elements & Compounds2.6 Giant Covalent Structures

2.6 Giant Covalent Structures (Cambridge (CIE) O Level Chemistry): Flashcards

Exam code: 5070

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FrontDiamond, Graphite & Silicon (IV) Oxide
Describe the structure of diamond.

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Cards in this collection (7)

Describe the structure of diamond.
In diamond, each carbon atom is bonded to four others in a tetrahedral arrangement, forming a giant covalent lattice. There are no free electrons and no intermolecular forces — only very strong covalent bonds throughout.
In graphite, each carbon atom is bonded to ______ others, forming layers of ______ rings. One electron per atom becomes ______.
In graphite, each carbon atom is bonded to three others, forming layers of hexagonal rings. One electron per atom becomes delocalised.
True or False?
Graphite acts as a lubricant because the covalent bonds between its layers are broken, allowing the layers to slide.
False.
The covalent bonds within each layer are strong and are not broken during lubrication. Graphite is slippery because the weak forces between the layers can be overcome easily, allowing the layers to slide over each other.
Why is graphite suitable for use as an electrode in electrolysis?
Graphite is suitable as an electrode because it is chemically inert (unreactive), has good electrical conductivity due to its delocalised electrons, and has a high melting point so it does not melt during use.
True or False?
Silicon(IV) oxide (SiO₂) is found as an impurity in iron ore and is removed during the blast furnace process.
True.
SiO₂ is present as an impurity in iron ore. In the blast furnace, it reacts with calcium oxide to form calcium silicate (slag), which is removed as a waste product.
Silicon(IV) oxide (SiO₂) has properties similar to diamond because both have ______ covalent structures with ______ covalent bonds throughout.
Silicon(IV) oxide (SiO₂) has properties similar to diamond because both have giant covalent structures with strong covalent bonds throughout.
True or False?
Diamond and graphite are different elements because they have different structures and properties.
False.
Diamond and graphite are both allotropes of the element carbon. They contain only carbon atoms but have different bonding arrangements, which gives them completely different properties.

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