C2 - Giant Covalent Structures 0.0 / 5 ? ScienceAtomsGCSEAQA Created by: maddiecorfieldCreated on: 25-11-15 19:20 What are the properties of simple covalent molecules? Low melting and boiling points, usually soft and brittle, shatter when hit, does not conduct electricity. 1 of 13 Why do simple covalent molecules have the properties they do? Weak intermolecular forces. 2 of 13 What is covalent bonding? The bonding of NON METALS. 3 of 13 Name some giant covalent structures. Silicone Dioxide (Sand), Diamond (Carbon), Graphite (carbon) Fullerines (carbon) 4 of 13 What are different forms of the same element called? Allotropes (Diamond and Graphite are allotropes) 5 of 13 What is diamond made of? Carbon 6 of 13 In diamond, each carbon is bonded to how many other atoms? 4/4 7 of 13 What are the properties of diamond? Strong, high melting and boiling points, very hard, can't conduct, because of strong covalent bonds 8 of 13 Why is graphite soft and slippery? Weak intermolecular forces. Bonded to 3 instead of four. Arranged in layers. 9 of 13 Can graphite conduct? Yes, due to having delocalized electrons. 10 of 13 Describe the structure of fullerenes (double covalent bonds) Carbon, with each carbon bonded to 3 others, strong covalent bonds, will not conduct, HMP, HBP. 11 of 13 Describe the structure and properties of Silicone Dioxide. Giant, made of silicon and oxygen, each silicon bonded to 4 oxygens, strong covalent bonds, does not conduct, HMP, HBP, hard. 12 of 13 Why is silicon dioxide a suitable material for lining furnaces? HMP HBP, strong covalent bonds, does not conduct, giant lattice structure 13 of 13
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