C4

• Group 1 Alkali metals

  • -ium
  • one outer electron - similar chemical properties
  • Low mp/bp
  • low density
  • very soft- Li, Na, K floats on water
  • Ionic compounds- lose one electron so don't form covalent bonds
  • Very reactive- lose outer electron to produce 1+ ions
  • more reactive as you got down group 1 as atomic radius is larger and less energy needed to remove electron due to weaker intermolecular attraction
• Alkali and water

  • vigorous reaction
  • produces hydrogen gas and a hydroxide of the metal

  Lithium - fizzing

  Sodium/Potassium- melt and potassium ignite hydrogen gas

  Rubidium and caesium reacts violently with water and explode
• Alkali + dilute acid -> Salt and hydrogen gas 


  e.g

  Sodium + hydrochloric acid -> sodium chloride and hydrogen
• Group 7 - Halogens

  • 7 elections in outer shell
  • diatonic molecule - covalent bonding to give full outer shell
  • mp/bp increases as you go down group 7

  Room temp

  Chlorine- green gas, reactive, poisonous, low mp

  Bromine- poisonous, red-brown liquid, orange vapour at room temperature

  Iodine- dark grey crystalline solid- purple vapour when heated
• Reactivity Group 7

  • goes down reactivity decreases
  • }Gain one electron to form 1- ions
  • easier too attract an electron- more reactive
  • Harder to attract extra electron to fill outer shell when its further away from nucleus
• Halogens + alkali metals

  • form a salt called metal halides
• Halogen displacement reaction

  • more reactive displaces less reactive element to form a compound
• Displacement showing reactivity trends

  1. measure halide salt solution
  2. Add few drops of halogen solution and shake
  3. see a colour change, reaction has happened- halogen has displaces halide ions
  4. repeat process using different hallide salt and halogen
• Group 0

  • noble gases
  • colourless at room temperature
  • Monatomic
  • Inert- don't react
  • Full outer shell
  • non-flammable
  • hard to observe
  • bp/mp, density increases as you go down
• Transition metals

  • hard, strong, shiny that conduct heat and electricity
  • high mp
  • high densities
  • good catalysts: iron for hater process, V2O5 in contact process
  • more than one iron
  • unreactive
• Metals react with water

  Metal + water -> metal hydroxide + hydrogen
• Test for carbon

  • bubbling it through limewater e
  • limewater turn cloudy then Co2 is present
• Test for hydrogen

  • Squeaky pop with a lighted splint
  • nouse comes from hydrogen burning with the oxygen in the air to form water
• Test for oxygen

  if gas will relight a glowing splint
• Test for chlorine

  • use damp blue litmus paper
  • turns it white
  • may turn red if chlorine is acidic
• Test for anions ( negative ion)

  test for halide ions using silver nitrate solution

  1. Cl- , Br- and I-
  2. Add dilute nitric acid
  3. and drops of silver nitrate solution

  Chloride - white precipitate of silver chloride

  Bromide - Cream precipitate of silver bromide

  Iodide- yellow precipitate of silver iodide
• test for carbonate

  1. Barium chloride solution
  2. Carbonate ions present = white precipitate of barium carbonate
  3. Add dilute hydrochloric acid
  4. if carbonate ions are present the mixture will fizz as carbonate reacts with acid to make Co2
  5. collect gas and pass through limewater to turn cloudy
  6. once barium carbonate has reacted it'll turn colourless
• Test for sulfate ions

  1. add barium chloride solution
  2. white precipitate of barium sulphate will form
  3. dilute hydrochloric acid to test the sample
  4. Barium sulfate will not react with dilute hydrochloric acid so white precipitate won't dissolve
• Flame test- metal ions

  Lithium - crimson red

  Sodium- yellow

  Potassium- lilac

  Calcium- orange- red

  copper - green
• Flame test

  1. Platinum wire loop, clean it by dipping it in dilute hydrochloric acid, rinsing in distilled water and then hating it up in buses burner
  2. dip wire in compound you want to test
  3. Hold wire loop in blue part (hottest part) of flame
• Metal ions and sodium hydroxide

  1. metal hydroxides are insoluble and precipitate out of solution formed
  2. some hydroxides have characteristic colours
  3. Add sodium hydroxide solution to mystery compound

  Calcium - white

  Copper - blue

  Iron (II) - Green

  Iron (III) - Brown

  Zinc - white at first then colourless
• Concentration


  mass of solute / volume of solution
• Titration to find concentration

  1. how much acid needed to neutralise an alkali
  2. use pipette to measure a set volume of the alkali into a flask- add a few drops of indicator - methyl orange
  3. Use burette to add the acid to the alkali a bit at a time
  4. Swirl the flask regularly
  5. indicator changes colour when all alkali has been neutralised

  Phenolphthalein pink in alkali, colourless in acid

  Methyl Lange- yellow in alkali, red in acid

  6. record volume of acid used to neutralise acid and repeat to get the mean
• Concentration = number of moles / volume of solution
• Molar volume 


  gas volume / number of moles
• at Room temperature pressure

  moles = 24 dm$^3$
• Percentage yield = ( actual yield / theoretical yield ) x 100
• Atom economy = (Total Mr of desired/ Total Mr of all product) x 100
• Rate of reaction =

  amount of reactant used or amount of product formed / time
• Rate of reaction experiment Hydrochloric acid and marble chips

  • closed system , gas syringe and flask

  1. measure volume of gas produced using a gas syringe- take readings at regular time intervals
  2. repeat experiment with same measurements
  3. but with marbles more crunched up
  4. repeat with the same mass of powdered chalk
• Finer particles of solid means greater RofR

  • larger surface area to volume ratio
• Magnesium metal and dilute HCL 


  measuring effects of changing the concentration

  gives off hydrogen gas so use mass balance
• factors that effect dynamic equilibrium

  • pressure (gas)
  • Temperature
  • Concentration
• Le chatelier's principle

  • change in temperature, pressure (gas), and concentration in a reversible reaction the equilibrium will move to help counteract the change
• Metals below hydrogen on reactivity will not react with dilute acids