2.4 Flashcards
Diamond and carbon are…. Of carbon
Allotropes
Diamond atom;
Each cargo;atom bonds with four other carbon atoms forming a tetrahedron
Bonds in Diamond are
Very strong and no intermolecular forces
Physical Properties of Diamond
Does not conduct electricity
Very high melting point
Extremely hard density of 3.51g/cm3
Why are there no freely moving charged particles in the current of diamonds
All outer shell electrons in carbon are held in 4 covalent bonds around each carbon atom
Why is there a very large amount of heat energy needed to break the lattice of diamonds
4 covalent bonds are very strong and extend in a giant lattice
How are the carbon structure
Carbon atom forms 3 covalent bonds to other carbon atoms forming. Layers of hexagons leaving one electron free per carbon atom
What do the freee electrons in graphite do
Free to move and carry charge, which is why graphite can conduct electricity
How are the covalent layers in graphite
Very strong, layers are attracted to each other by weak intermolecular forces, which is why layers can Slide Over each other, soft and slippery
Graphite physical properties
Conducts electricity and heat
Very high melting point
Soft and slippery less dense than Diamond 2.25g/cm3
Graphite has …… Inter molecular forces
Weak
What can graphite be used as
Pencils and industrial lubricant
What does graphene consist of
Single layer of graphite, 2D molecule, good at fabricating composite materials and electronics
Properties of graphene
Extremely strong but very light (would take an elephant to break a sheet of graphene)
Conducts heat and electricity
Transparent flexible
Why is graphene very strong
Unbroken latter and strong covalent bonds
