bonding

• define "alloy"


  an alloy is a mixture of 2 or more elements atleast 1 in which is a metal
• what are the features of a giant metalic lattice

  1.cations are fixed in place and cannot move

  2.delocalised electrons are free to move

  3.high melting and boiling points because of the strong metalic bond

  4.do not dissolve in water and instead react
• what are the key properties to diamond a giant covalent structure

  1.high melting and boiling point due to the large amount of energy required to break the covalent bonds

  2.diamond does not conduct electricity because every electron is in a covalent bond and there are no delocalised electrons to act as charge carries

  3.insoluable, because solvents cannot disrupt the large numbers of strong covalent bonds

  4.contain 4 covalent bonds
• how many covalent bonds does diamond have

  4
• what are the key properties to graphite in a giant covalent structure

  1.excellent conductor of thermal energy, as more energy is transferred to the delocalised electrons they move around faster and rapidly transfer the energy along the layers

  2.contain delocalised electrons which allow them to move freely and allow graphite to conduct electricity

  3. arranged in layers which makes graphite soft to the touch
• what properties does fullerene have

  1.high tensile strength

  2.high electrical conductivity
• what is the structure of fullerene

  hexagonal rings of carbon
• what can fullerene be used for

  drug delivery in the body, used as lubricants and catalysts because of their big surface area to volume ration of nanoparticles
• what is the structure of graphene

  a single sheet of graphite which is so 1 atom thick
• what are the properties of graphene

  1.excellent conductor of thermal energy and electricity

  2.low density

  3. most reactive form of carbon
• why did scientists call fullerene "bucky ball"

  because of the cage like structure
• why are alloys harder than pure metals


  within an alloy all the atoms are different sizes making it harder for them to slide upon each other compared to in a regular pure metal because their layers are disorted by atoms
• what is ionic bonding


  a metal bonds with a non metal
• what is covalent bonding

  when 2 non metals bond