c4 | Mind Map

testing water purity
1. test 4 sulfate
  1. add hydrocloric acid
    1. add barium chloride solution
      1. if whie precipitate there is
2. test 4 halide ions
  1. add dilute nitric acid
    1. add 10 drops of silver nitrat solution
      1. if precipitate fors yes there is
elements
1. isotopes
  1. different form of the same element
  2. same number of protons
  3. different number of nutrons
  4. same atomic number different mass number
  5. eg carbon 12 and carbon 14
    1. carbon 12
      1. 6 protons
      2. 6 electrons
      3. 6 nutrons
    2. carbon 14
      1. 6 protons
      2. 6 electrons
      3. 8 neutrons
  6. the number of nutrons is mass - atomic number
2. group number of electrons in outer shell
metals
1. crystal structure
  1. same properties
  2. special bonding that is in metals
  3. held together with metalic bonding
  4. outer electron moves freely
  5. this creates a sea of free electrons
2. high
  1. very hard dense and shiney
  2. strong atraction between
    1. positive ions
    2. delocalised electrons
  3. high melting and boling point
    1. large energy needed to break the metallic bonds
  4. strenght of the metallic bond decreases as atomic radious increases
    1. and melting point
3. strong
  1. hard to break
    1. high tensil streangth
  2. hammered into different shapes
    1. malleable
4. good conducters
  1. the delocolised electrons carry the electrical curent
  2. they also carry heat energy
5. use
  1. sausepan
    1. stainless steal
      1. good heat conducter
  2. electric wiring
    1. copper
  3. aeroplane
    1. aluminium
  4. bridge
    1. steel
ion and ionic componds
1. ions
  1. charged particals
2. ou have to balance the + and -
  1. 2K+
    1. k20
      1. the potassium ion 1+ and the oxygen 2- balance because you need 2 positive to the 2 negetive
  2. O2-
3. dot and cross diagram
  1. show what happens in ionic bonding
  2. arrows to
electron shells
1. shells
  1. 2nd = 8
  2. 3rd =8
  3. 1st =2
2. electronic configeration
  1. eg. 12= 2,8,2
superconducters
1. at low teperatures
  1. all have some resistance
  2. mean some eletrical energy turns to heat
  3. if cold enough
    1. it disdsapears
  4. dont loose any current
2. the catch
  1. you can make
    1. powet cables with no lose
    2. fast electronic circuites
    3. strong electromagnets
  2. has to be colder than -265 c
    1. hard and expencive
3. transition metals
  1. catalysts
    1. iron
      1. harbor process
    2. nickel
      1. hydrogenation
  2. colorful
    1. copper often blue
    2. iron (ll) often light green
    3. iron (lll) often orange or brown
  3. middle of the table
    1. have typical metallic propities
atoms
1. the nucleus
  1. positive protons
  2. netrule neutrons
  3. the nucleus it positive
2. electrons
  1. negitivly charged
  2. the electronic shell
  3. virtually no mass
3. atomic number and mass
  1. mass top number
  2. mass total of protons and nutron
  3. atomic number
    1. number of protons
    2. bottom number
    3. number of electrons
ionic bonding
1. transfering electrons
  1. atom loses or gains an electron
  2. forms a charged partical
    1. ions
  3. strongley atracted to each other
    1. +
      1. join together
    2. -
2. one electron on a shell got to go
  1. they like to hace a full outer shell
  2. once they get rid thy become positivley charged
  3. they will leapat the chance to stick to a negativ ion
3. nearly full shell wants an extra
  1. gain an electron to fill the shell
  2. become negetivly charged
4. eg
  1. sodium gives up an electron
    1. NA+
  2. chlorine picks p an atom
    1. CL-
      1. forms ionic bond
5. giant ionic lattice
  1. made from metals and non metals
  2. strong chemical bonds in all ions
groups
1. group 1 alkali metals
  1. oxidation
    1. loss of electrons
    2. the more reactive the happier to lose
  2. cold water
    1. produces hydrogen gas
    2. eg sodium
    3. they fizz
    4. reactivity increases the lower down the group
      1. potasium get hot enough to ignight
      2. sodium and potasium melt
    5. alkali forms
      1. 2 Na + 2 H2O > 2 NaOH + H2
  3. burn with charicteristic colors
    1. lithium =red
    2. sodium =yellow
    3. potassium = lilac
  4. key facts
    1. they all have one outer electron
    2. low melting point
    3. low density
    4. very soft
    5. they always form ionic
      1. NEVER COVALENT
2. group 7 halogens
  1. key facts
    1. they all have 7 outer electrons
    2. as you go down they become less reactive
      1. melting point increase
    3. at room tempreature
      1. chlorine
        poisonoius
        dense green gas
        fairley reactive
      2. iodine
        dark gray crystlline solid
      3. bromine
        poisonous
        orange liquid
  2. reduction
    1. keenn to gain an electron
      1. become a 1- ion
      2. stabel electronic structure
    2. the more reactive the happier it i to gain
    3. gain of electrons is called reduction
  3. form salts
    1. react with alkli metals
      1. makes salt called METAL HALIDES
    2. reactions eg
      1. 2 Na + Cl2 > 2 NaCl
        Sodium + Chlorine > sodium chloride
      2. 2 K + Br2 > 2 KBr
        potassium + bromine > potassium bromide
  4. displace
    1. more reactive halogen dispalce less reactive ones
      1. eg
        Chlorine + potassium iodide > iodine+ potassium chloride
covalent bonding
1. sharing electrons
  1. non metals combine to for convalent bonds
  2. both atoms have a full outer shell
  3. each provides one extra electron
2. dot and cross
  1. overlap
3. simple molecular substances
  1. covalent bods usely have simple molucal structures
    1. eg H2O and CO2
  2. held together with very strong covalent bonds
  3. force between them is very weak
    1. low boiling point
    2. lowmelting point
  4. at room tempreture gases and liquids
  5. the dont conduct electricity
    1. no free electrons
water purity
1. sea water
  1. very expersive
  2. in dry contrey r=they distill sea water
  3. needs alot of energy
2. limited resorcesd
  1. industrial coolent
  2. homes for washing
  3. ground water
    1. aquifers
      1. rocks trsp water
    2. upto 70% of water comes from underground
  4. ground water
    1. eg lakes rivers reservoirs
      1. run dry in summer
3. tap water
  1. still contains in puritys
  2. nitrate residue
    1. fertalizer running off fields
  3. lead compounds
    1. from old pipes
  4. pesicide residue
    1. spraying to near lakes
4. tretment plants
  1. filteration
    1. wire mesh
    2. takes out large twigs
  2. sedimentation
    1. iron sulphate is added
      1. makes small particals clump together
  3. chlorination
    1. bubbled through to kill harmfull bacteria
thermal decomposition
1. hydroxide tests
  1. copper (lll) = blue solid
  2. iron (ll) = gray/green solid
  3. iron (ll) = orange/brown solid
2. solid forms in solution
  1. 2 solution react and make a solid in the solution
  2. called a precipitate
3. breaking down with heat
  1. breaks into at leat 2 other substances
  2. break down into metal oxide and carbon dioxide
    1. eg. copper oxide
  3. check for carbon dioxide = lime water
history
1. theories backed up
  1. so that it can be checked for errors
  2. so other scientists can use it to develope there own work
2. time line
  1. john darlton
    1. jj thomson
      1. rutherford
        gold foil experimenthe came up with the thery of the nuclear atom found that the plum pudding was wrong
        bohr
        electrons can only exist in fixed orbits
        it was pretty clos to our current accepted verrsion
      2. found the charges and mass whch showed they wernt solid spheres new thery was called the plum pudding
    2. described them as solid spheres and said that different spheres made different elements

Next up

c4

Description

Resource summary

Similar

	Created by zoetoffee almost 11 years ago