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• | reduction with carbon

  • ore has metal & impurities
• • separating a pure metal from its ore is EXTRACTION
• • extraction can be by…
  • CARBON
  • ELECTROLYSIS
• • if metal is MORE reactive than carbon, use reduction with ELECTROLYSIS
  • if metal LESS reactive than carbon, reduce with CARBON
• | reduction w/ carbon

  1. react metal with carbon inside a BLAST FURNACE
  2. carbon will DISPLACE metal & remove impurities
  3. gives us a pure metal!
• | reactivity series

  most to least

  
  

  potassium

  sodium

  lithium

  calcium

  magnetism

  CARBON

  Zinc

  Iron

  Hydrogen

  Copper
• | aqueous electrolysis

  • water dissociates (breaks down) into HYDROGEN & HYDROXIDE
• | aqueous electrolysis

  • dc power supply
  • graphite conductors (positive = anode, negative = cathode)
  • P.A.N.I.C
• | aqueous electrolysis

  1. CATHODE: metals less reactive than hydrogen react w/ cathode first (copper, silver, gold) where it gets REDUCED
  2. ANODE: priority for group 7 ions (halide), otherwise its HYDROXIDE where it gets oxidised_ oxygen is produced which is seen as BUBBLES:

  • 4OH- -> O2 + 2H2O + 4e-
  • test for oxygen: re-light glowing splint ..
• | half equations

  • group 1: 1+
  • group 2: 2+
  • group 3: 3+
  • group 5: 3-
  • group 6: 2-
  • group 7: 1-

  
• | diatomic

  • two atoms joint together
  • Have
  • No
  • Fear
  • Of
  • Ice
  • Cold (Cl)
  • Biryani (Br)
• | redox half equations

  1. write atom (0 charge by default)
  2. then ion
  3. add electron to balance charge

  • eg: Na -> Na+ + e-
• | half equations for oxygen

  • O2 + 4e- -> 2O^2-
• | making salts

  • salt crystals made with ACIDS + INSOLUBLE BASE (oxide or carbonate)

  1. react base with acid to make salt, keep adding until you see excess which means the acid has fully reacted
  2. use FILTRATION to separate the excess so only what is SOLUBLE passes
  3. use CRYSTALLISATION- pour solution into evaporating dish, put over Bunsen burner and gently heat it, allow it to cool
• | reacting masses

  
• | limiting reactants

  
• | ionic equations

  • break down aq!!!

  
• | allotropes of carbon

  • allotropes are different STRUCTURES of the same element
• | allotropes of carbon

  • carbon has 4 main allotropes

  1. diamond
  2. graphite
  3. graphene
  4. fullerene
• | allotropes of carbon

  Diamond

  • each carbon has 4 bonds
  • hard
  • strong covalent bonds = HIGH melting point
• | allotropes of carbon

  graphite

  • each carbon atom has 3 bonds
  • delocalised electron
  • conducts electricity
  • layers that can slide & slippery
  • Strong covalent bonds = HIGH MELTING POINT
• | allotropes of carbon

  graphene

  • one layer of graphite
  • strong & lightweight
  • delocalised electron
  • conducts electricity
• | allotropes of carbon

  fullerenes

  • small hollow molecules
  • buckminister fullerenes
  • transports drugs around body
  • high SA:V so can be used catalysts
  • used as lubricant bc they can ROLL
  • carbon nanotubes
  • conducts heat & electricity
  • high tensile strength, can pull heavy weights
• | ionic bonding

  • dot & cross diagrams are only for outer shells
• | ionic compounds

  properties

  • giant regular lattice
  • high melting/boiling points bc lots energy needed to overcome strong attraction
  • DONT conduct electricity as solids due to ions being in fixed positions
• | metallic bonding

  • positive ions & sea of delocalised electrons
  • can conduct electricity as electrons carry charge
  • high melting point due to strong electrostatic force
  • pure metals arranged in layers; can SLIDE
  • malleable
• | metallic bonding

  • mixing metals with other elements creates ALLOYS which are stronger
  • due to different sizes which disrupts the layers
• | group 1 metals

  Physical properties

  • soft
  • low melting point due
  • low density (can float)
  • malleable
  • shiny when cut
• | group 1 metals

  reactivity with oxygen

  • quickly reacts with oxygen, forming an oxide layer which makes it dull
• | group 1 metals

  chemical properties

  • reacts with water = alkaline solutions (pH 8-14)
  • store in OIL to prevent reacting with MOISTURE in AIR
• | group 1 metals

  Reactivity

  • as you go down, the MORE REACTIVE

  1. size of atom increases as you go down
  2. outermost electron is further from the nucleus
  3. easier to lose outer electron
• | group 1 metals

  reactivity with water

  • reacts vigorously as you go down outermost electron
  • lithium, sodium & potassium float & fizz
  • produces hydrogen
  • forms hydroxides that dissolve to give alkaline solution
• | group 7

  halogens

  • exist as DIATOMIC molecules
  • boiling point INCREASES as you go down
  • larger molecules which need more energy to break
• | group 7

  physical properties

  • flourine = yellow gas
  • chlorine = green gas
  • bromine = brown liquid
  • Iodine = grey solid with purple vapours
• | group 7

  reactivity decreases down

  • size increases
  • distance from nucleus to outer shell increases
  • harder to gain electron
• | group 7

  displacement reactions

  • most reactive joins with metal
  • fluorine
  • chlorine
  • Bromine
  • Iodine
• | group 7

  displacement reactions

  • chlorine: colourless
  • bromine: orange
  • iodine: brown
• | group 7

  ionic equations for displacement

  • remove metal & put minus sign..
• | chromatography

  • use it to investigate how many different colours there are

  1. draw baseline with pencil near bottom
  2. Pippete transfer onto baseline
  3. put paper in beaker with solvent below baseline
  4. put lid so solvent not evaporate
  5. allow solvent to travel up
  6. take paper out & draw line at top
• Rf = dye distance / solvent distance

  Rf= NEVER MORE THAN 1!!!