Giant Covalent Structures + Giant Metallic Structures

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Diamond+Silicon Dioxide Properties
Hard, high boiling point + high melting point
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Bonding in Diamond +Silicon Dioxide
1) 1:4 carbons, 2) strong covalent bonds, 3) 3D giant structure, 4) bonds difficult to break
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Why can graphite conduct electricity???
delocalised electrons ---> carry charge
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Bonding in Graphite
1) 1:3 carbons, 2) no covalent bonds between layers, 3) arranged in giant hexagon layers, 4)layers can slide
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Thermosoftening
Tangled web, easy to separate
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Thermosetting
Chains fixed together by STRONG COVALENT BONDS + crosslinks
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Properties of metals
held together by a sea of DELOCALISED ELECTRONS, NEGATIVE CHARGE of electrons between POSITIVELY CHARGED ions HOLD them in position. Electrons able to MOVE through lattice
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Metals
1) closely packed layers, 2)can conduct electricity and heat, 3)layers can slide over eachother, 4)can be shaped or bent, 5) delocalised electrons ---> allow current & heat to flow through the metal
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Alloys
1) harder than pure metals, 2)mixture of metals, 3)more difficult to slide over eachother, 4) distorted layers
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Other cards in this set

Card 2

Front

Bonding in Diamond +Silicon Dioxide

Back

1) 1:4 carbons, 2) strong covalent bonds, 3) 3D giant structure, 4) bonds difficult to break

Card 3

Front

Why can graphite conduct electricity???

Back

Preview of the front of card 3

Card 4

Front

Bonding in Graphite

Back

Preview of the front of card 4

Card 5

Front

Thermosoftening

Back

Preview of the front of card 5
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