c2.3 p2 Flashcards
how many bonds can carbon form?
4
state properties of diamond (and explain why)
hint:
- its structure
- how many carbon atoms it bonds to
- melting point
- strength
- metal/non metal
- giant covalent structure (carbon atom is covalently bonded to four other carbon atoms)
- THEREFORE a high melting point
- very hard
- non metal (made of carbon atoms)
can diamond conduct electricity, and if so why?
it cannot, as all its outer electrons are shared when forming covalent bonds
what is a common use for diamond?
dental drills
state properties of graphite (and explain why)
- structure
- how many carbon atoms it bonds to
- can/cannot conduct electricity
- nonmetal/metal
- layered covalent structure
- bonds to three other carbon atoms
- can conduct electricity (one electron is delocalised as it does not form a bond)
- non-metal
what is the structure of graphite like? (4)
- giant covalent structure
- layered structure (which look like interlocking hexagons in a chicken wire)
- strong covalent bonds IN layer, weak intermolecular forces BETWEEN layers
- delocalised electrons able to carry charge
state a common use of graphite
pencil tip
crucibles
lubricants
polishes
what is graphene?
a single layer of graphite
properties of graphene
- almost transparent
- extremely strong
- conducts electricity
- almost 2D (one atom thick)
define fullerenes
a family of carbon allotropes where molecules are shaped like tubes or balls
in terms of forces of attraction what happens when a substance changes state
- forces of attraction between its particles are overcome
how do nanoparticles compare to fine particles
they are smaller
why do nanoparticles have different properties to the same material in bulk?
because of its high surface to volume ratio
this causes it to be more reactive
