C2- Bonding, structure and particles of matter

• Ionic, covenant and metallic

• Particles are oppositely charged ions - Metals and non metals

• Share pairs of electrons - most non-metallic and compounds of non metallic

• Particles are atoms which share delocalised electrons - Metallic elects and alloys

• Charged particles- can be single atoms or groups • Cations- positive • Negative- anions

• When metal and non metal react together, the metal atom loses electrons to form a positive ion and non metal gains these electrons to form negatively charged ion • Oppositely charged ions are strongly attracted to one another by electrostatic forces

• Dot and cross diagram

• Giant structure of ions • Held together by electrostatic forces between opposite charges • Act in all directions • Ionic compounds form giant ionic ionic lattice

• Ball and stock - colourful balls

• Share electrons to form full outer shell • Strong bonds • happens in non-metals

• dot and cross • Dispalyed forumla • 3d

• Hydrogen- Single • Chlorine - Single • Oxygen- Double • Nitrogen- tribble • Methane- four • water- single

• Usually those with covalent bonds have this • Held together with very strong bond- forces of attraction weak • Only need to break friable forces not bonds so melting points are low • No free electrons- don’t conduct

• High melting and boiling point • Due to many strong bonds that have to be broken • Cant conduct electricity when solid • When liquid they can conduct • Dissolve early in water

• Long chains of repeating units -lots of small units are linked to form long molecule • Draw repeated section • Joined by covalent • ## Loe boiling point

• Write down molecular formula and put brakes around and N on outside

• Giant covenant structures • All atom bonded by strong covalent • High melting points • Diamond dont conduct

• different structural forms of the same element in the physical state

• Diamond • Graphite • Graphene • Fullerne

• Allotrope of carbon • Very hard • Giant covalent • Four bonds • High melting point • doesn’t conduct

• Three bonds • Sheets in Hexagons • no bond between layers- move easily • High melting point • conducts as has one free

• One layer of graphite • One atom thick • Very strong • Can conduct

• Molecules of carbon atoms with hollow shapes • Hexagonal rings, however may also be five or seven • First was Buckminsterfullerene c60 which has a physical shape • cage other molecules

• Fullerene • Cylindrical very high length to diameter • Useful for nanotechnology, electronics and materials- strengthen without weight