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What is current?
the flow of charged particles.
What kind of bonding occurs between a metal and a non-metal?
Ionic bonding.
What is electrostatic attraction?
The attraction of positive ions to negative ions.
What is involved in ionic bonding?
the transfer of electrons.
Describe the structure of ionic compounds.
arranged in a lattice structure.
Why do ionic compounds have high melting / boiling points?
they have very strong electromagnetic forces that require more energy to break the bonds.
Can solid ionic compounds conduct electricity? Why or why not?
no because there are no delocalised electrons.
When can ionic compounds conduct electricity?
when melted or dissolved in water.
What is simple covalent bonding?
It is the sharing of electrons between non-metals
Why do Simple Covalent Molecules have low boiling points?
they have weak intermolecular forces that require little energy to break
Do Simple Covalent Molecules conduct electricity?
No, because there are no delocalised electrons
What are examples of giant covalent structures? (D)
diamond
What are examples of giant covalent structures? (N-T)
nano-tubes
What are examples of giant covalent structures? (F)
fullerenes
What are examples of giant covalent structures? (SD)
silicon dioxide
What are examples of giant covalent structures? (ene)
graphene
What are examples of giant covalent structures? (ite)
graphite
Can diamond and silicon dioxide conduct electricity? Why or why not?
No, they don’t have delocalised electrons
What is a key property of graphite and graphene? (conduction)
They can conduct electricity because they have delocalised electrons
Why do graphite and graphene have a high melting point?
they have strong covalent bonds that require a lot of energy to break
How is diamond structured?
a tetrahedron shape, making it very strong
What is the practical use of graphite as a lubricant?
the layers can slide over each other
Why are fullerenes effective as lubricants?
Because they are ball-shaped and can roll
What defines metallic bonding?
metals have giant structures with positive ions arranged in regular layers
What happens to outer electrons in metallic bonding?
They become delocalised and can easily move throughout the structure.
What creates strong electrostatic attraction in metals?
the attraction between negatively charged electrons and positive metal cations
What are the characteristics of pure metals regarding atomic size?
atoms are the same size and layers to slide over each other
What is the property of alloys compared to pure metals?
alloys are harder because the different sizes of atoms distort the layers, preventing sliding
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