Lesson 4.2.3.1
4.2.3.1 Diamond Quiz: AQA Chemistry, Unit 2
20 questions
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Lesson 4.2.3.1, Diamond: 20 multiple choice questions for the AQA GCSE Chemistry (8462), Unit 2: Bonding, structure, and the properties of matter, written with Revision Ninja.
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The 20 questions
-
How many covalent bonds does each carbon atom form in diamond?
- One
- Four
- Two
- Three
-
What type of structure does diamond have?
- Giant covalent structure
- Simple molecular structure
- Giant metallic structure
- Giant ionic lattice
-
What geometric shape describes the arrangement around each carbon atom in diamond?
- Octahedral
- Hexagonal
- Linear
- Tetrahedral
-
Why does diamond have an extremely high melting point?
- Strong covalent bonds
- Weak forces
- Mobile electrons
- Ionic lattices
-
What is the electrical conductivity of diamond?
- Semi-conductor
- Good conductor
- Conducts when molten
- Does not conduct
-
Why are there no free charge carriers in diamond?
- Layers can slide
- Structure is liquid
- Atoms are ions
- All electrons bonded
-
What type of overall structure do both diamond and silicon dioxide share?
- Giant covalent
- Giant ionic
- Simple molecular
- Simple atomic
-
Why is diamond exceptionally hard in all directions?
- Layered structure
- Rigid 3D network
- Molecular lattice
- Flexible chains
-
Which element is diamond made from?
- Carbon
- Sulfur
- Oxygen
- Silicon
-
Which specific crystal system does the diamond lattice belong to?
- Cubic
- Triclinic
- Monoclinic
- Orthorhombic
-
How many carbon atoms are bonded directly to any single carbon in diamond?
- Four
- Three
- Two
- Six
-
What is the spatial arrangement of carbon atoms in diamond?
- Linear chains
- Three-dimensional
- Layered sheets
- Simple cubes
-
Why does diamond have a very high melting point?
- Delocalised electrons
- Weak intermolecular forces
- Ionic attractions
- Strong covalent bonds
-
What is the structural difference between diamond and graphite?
- Graphite is 3D
- Diamond is 3D
- Both are linear
- Both are layered
-
Why is diamond extremely hard?
- Rigid covalent network
- Mobile ions
- Free electrons
- Weak layer forces
-
Which physical property does diamond share with giant ionic lattices?
- Electrical conductivity
- High melting point
- Low boiling point
- Soft texture
-
What is absent in diamond that is present in metals?
- Delocalised electrons
- Rigid structure
- Carbon atoms
- Covalent bonds
-
Why is diamond unable to conduct electricity?
- Free electrons
- Delocalised nuclei
- No free charges
- Mobile ions
-
What is the overall shape category of the diamond crystal lattice?
- Metallic network
- Giant covalent
- Simple molecular
- Polymer chain
-
How many outer electrons are used for bonding by each carbon in diamond?
- Only one
- All four
- Only three
- Only two
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