Bonding Unit 2 Chemistry

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  • Created by: Sunset
  • Created on: 05-01-14 13:21
Why do GIANT IONIC STRUCTURES have high melting and boiling points?
Lots of attraction required to overcome strong attraction
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Why don't SIMPLE COVALENT STRUCTURES conduct electricity?
They have no charge
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Why is DIAMOND hard?
Each carbon atom is bonded to 4 others by strong covalent bonds and there are no layers
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Why does GRAPHITE conduct electricity?
Each carbon atom is bonded to three others leaving one free electron which is delocalised and able to carry charge
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What type of atom does COVALENT BONDING happen between?
Non-metals
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Why are METALS malleable?
They are arranged in layers which can slide over one another
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Why do METALS have high melting and boiling points?
There is a strong electrostatic attraction between the positive ions and delocalised electrons which requires a lot of energy to break
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Why are ALLOYS harder than pure metals?
The different sized atoms disrupt the pattern preventing the layers from slidingw
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Why don't Thermosetting Plastics soften when heated?
They have strong covalent bonds which require a lot of energy to break
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What charged ion would a group 2 atom make?
+2
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Lithium has atomic number 12 and oxygen has atomic number 8. They are ionically bonded. What is the formula of the ionic compound that they form?
Li2O
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Other cards in this set

Card 2

Front

Why don't SIMPLE COVALENT STRUCTURES conduct electricity?

Back

They have no charge

Card 3

Front

Why is DIAMOND hard?

Back

Preview of the front of card 3

Card 4

Front

Why does GRAPHITE conduct electricity?

Back

Preview of the front of card 4

Card 5

Front

What type of atom does COVALENT BONDING happen between?

Back

Preview of the front of card 5
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