Chemistry - Covalent bonds

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10 Terms

1
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what types of compounds can form covalent bonds

non-metals

2
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covalent bonds can be simple molecular structures or what

giant covalent structures

3
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what is the strong electrostatic attraction between

the negatively charged electrons and positively charged nuclei

4
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why do simple molecular structures have low melting and boiling points

because the inter molecular forces are weak so less energy is needed to overcome them

5
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why are simple molecular structures poor conductors

there are no delocalised electrons

6
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why do giant covalent structures have a high melting and boiling point

the non-metal atoms are bonded together by strong covalent bonds, these structures can be called giant lattices

7
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what are two examples of giant covalents

diamond and graphite

8
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why is diamond a bad conductor

each carbon atom is bonded to four other carbon atoms therefore there are no delocalised electrons

9
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graphite forms layers of what shape

hexagons

10
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why is graphite a good conductor

because each carbon atom is bonded to only three other carbon atoms, leaving one electron free