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Chemistry

Covalent Substances & Conductivity & Metals (Section 2)

QuestionAnswer
Give 3 examples of a giant covalent structure Diamond, graphite, silicon dioxide
We need __________ temperatures to melt or boil simple molecular substances low
Simple molecular substances have strong _________________ but weak _________________ covalent bonds, intermolecular forces
With halogens, the boiling point ___________ as you go down the group, as the molecules get ___________ increases, larger
Do simple molecular substances conduct electricity? No
Does diamond conduct electricity when molten? No
What state do most simple molecular substances exist in at room temperature? Gaseous
Chlorine is a _____ at room temperature. gas
Bromine is a _______ at room temperature. liquid
Iodine is a _______ at room temperature and gives off __________________ solid, purple fumes
What is an allotrope? Different structural forms of the same element in the same physical state
In a diamond, each carbon atom is covalently bonded to __ other carbon atoms 4
In graphite, each carbon atom is covalently bonded to __ other carbon atoms 3
Why can graphite conduct electricity? Because each carbon atom has one delocalised electron, which can move freely, and so is able to carry charge.
What is a single layer of graphite called? Graphene
Most metals are malleable, which means what? They can easily be bent or hammered into shapes
Are metals good conductors of electricity and heat? Yes
How do we make an alloy? By mixing two different metals or a metal and a non-metal. We generally use elements with different sized atoms
Why are alloys much harder than pure metal? The different sized atoms disrupt the regular structure, meaning layers can no longer slide over each other
Created by: JoeMather
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