c2 Flashcards
in graphite how many covelant bonds does each carbon have
3
what is an alloy
an alloy is a mixture of 2 or more metals
what is a giant covalent structure
a structure in which all the atoms are made by strong covalent bonds
state graphenes uses
electronics
making composites
why does diamond have a high melting point
due to every single bond being held by strong covalent bonds
4 properties of graphene
high melting and boiling points
conducts electricity
very light
strong
what are the three types of chemical bonds
ionic
covalent
metallic
why are alloys harder than pure metals
- the different elements have different-sized atoms
2.this disrupts the regular layered structure - meaning the layers can slide over one another
4.this makes them less malleable and harder
why do atoms form ions
atoms form ions so they can gain full outer shells of electrons
why are metals good at conducting electricity and heat
this is because they have delocalised electrons so they can move around and transfer energy
why are metals malleable
the layers can slide over one another which allows the structure to bend
describe the structure of graphite
carbon is covalently bonded to 3 other carbon atoms forming a sheet of hexagonal rings
they’re held together by intermolecular forces
3 examples of giant covalent structures
diamond graphite silicon dioxide
what does malleable mean
a structure that can be hammered into shape
what do covalent bonds form between
2 non metal atom
