Welcome to the Quiz!
This quiz contains 13 questions from a mix of 1 subtopics.
Select all the properties of diamond.
(Select all that apply).
high melting and boiling point
conducts electricity
weak
strong
low melting and boiling point
doesn't conduct electricity
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Do giant covalent structures have high or low melting points?
high
low
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Diamond and graphite are both made from the element , and are examples of covalent structures. Their atoms are arranged in a regular repeating structure with many multiple covalent bonds between each atom.
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Which of these is an example of a giant covalent structure?
diamond
ammonia
carbon dioxide
water
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Graphite is able to conduct . This is because each carbon atom has one electron, which can move freely, and so is able to carry charge.
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Unlike diamond, the carbon atoms in graphene each bond to other carbon atoms. This arranges the graphene into a single 2D layer made up of repeating hexagons.
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Which structure is shown in the image?
graphite
diamond
carbon
glass
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Which of the following statements are true of diamond?
each carbon atom is bonded to 4 other carbon atoms
it is made up of silicon and oxygen
each carbon atom is bonded to 3 other carbon atoms
it conducts electricity
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What do giant covalent crystals consist of?
small molecules held together by weak intermolecular forces
a network of atoms covalently bonded together
positive ions embedded in a sea of delocalised electrons
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Why graphite can conduct electricity?
carbon atoms can carry electrical charge
covalent bonds can carry electrical charge
ions within layers can carry electrical charge
delocalised electrons within layers can carry electrical charge
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What type of bonding is present in diamond?
metallic
ionic
covalent
hydrogen
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Giant covalent structures have high melting points because there are strong bonds between which require a lot of energy to break.
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What type of particle makes up giant covalent crystals?
ions
atoms
molecules
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