ࡱ> %` 0bjbjNN 4,,'S''''(dD8H)^)^)^)^)///7777777$69h;7/.///7^)^)q7c6c6c6/^)^)7c6/7c6c6^Jc6^)<) 4w5'124c6/780D8c6<e5<c6c6<w6//c6/////77S6///D8////@ @  C4 Revision C4.1 What are the patterns in the properties of elements? 1. recall that atoms of each element have different proton numbers; e.g. hydrogen 1 proton, helium 2 protons 2. understand that arranging the elements in order of their proton numbers gives repeating patterns in the properties of elements; 1 H 2 He 3Li 4 Be 5B 6C 7N 8O 9F 10Ne 11Na (He and Ne inert) 3. be able to use the Periodic Table to obtain the names, symbols, relative atomic masses and proton numbers of elements; Relative atomic mass 12 Symbol C Name carbon Proton number 6 4. recall that a group of elements is a vertical column in the Periodic Table and that the elements have similar properties; Group 1 Alkali metals All react with water 5. recall that a period is a row of elements in the Periodic Table;  6. be able to use the Periodic Table to classify an element as a metal or non-metal;   7. be able to use patterns in the Periodic Table to interpret data and predict properties of elements; Cl gas Br liquid I solid 8. recall and recognise the chemical symbols for the group 1 metals: lithium, sodium and potassium; Lithium Li, sodium Na, potassium K. 9. recall that the alkali metals tarnish rapidly in moist air but are shiny when freshly cut; Sodium is a shiny silver metal forming a white solid on its surface in air. 10. be able to use qualitative and quantitative data to identify patterns and make predictions about the properties of group 1 metals (for example melting point, boiling point, density, formulae of compounds and relative reactivity); Mp: Li 181oC, Na 98oC, K 68oC Density: Li floats, Na floats, K floats Formulae: Li2O, Na2O, K2O 11. describe the reactions of lithium, sodium and potassium with cold water; Bubbles of gas of increasing vigour down the group. Each reaction leaves a hydroxide e.g. sodium hydroxide 12. recall that alkali metals react with water to form hydrogen and an alkaline of a hydroxide with the formula MOH; 2Na + 2H2O ( 2NaOH + H2 13. recall that alkali metals react vigorously with chlorine to form colourless, crystalline salts with the formula MCl; 2K + Cl2 ( 2KCl 14. understand and be able to give examples to show that the alkali metals become more reactive as the group is descended; Li tarnishes slowly in air when cut, Na tarnishes quickly in air when cut, K tarnishes instantly as soon as it is cut C4.1 What are the patterns in the properties of elements? 15. recall the main hazard symbols and be able to give the safety precautions for handling hazardous chemicals (limited to harmful, toxic, irritant, corrosive, oxidizing, highly flammable); Harmful avoid contact use fume cupboard; toxic do not eat(ingest); irritant/corrosive wear gloves/safety glasses use fume cupboard; oxidizing do not mix with things that burn; flammable avoid naked flames e.g. lit Bunsen. 16 explain the precautions necessary when working with group 1 metals and alkalis; Store the metals under oil; treat alkalis as corrosive. 17. recall and recognise the chemical symbols for the atoms and molecules of the group 7 elements: chlorine, bromine and iodine; Atom/molecule Cl Cl2, Br Br2, I I2. 18. recall the states of the halogens at room temperature and pressure; F gas, Cl gas, Br liquid, iodine I 19. recall the colours of the halogens in their normal physical state at room temperature and as gases; Cl green/yellow, Br red, I grey/black 20. recall that the halogens consist of diatomic molecules; Diatomic two atoms joined Cl-Cl, Cl2, Br2, I2 21. recall that the halogens can bleach dyes and kill bacteria in water; Cl bleaches litmus from red to white. Cl is put in drinking water and swimming pools to kill bacteria. 22. be able to use qualitative and quantitative data to identify patterns and make predictions about the properties of the group 7 elements (for example melting point, boiling point, formulae of compounds and relative reactivity); Mp: Li 181oC, Na 98oC, K 68oC Density: Li floats, Na floats, K floats Formulae: Li2O, Na2O, K2O 23. recall and be able to give examples to show that the halogens become less reactive as the group is descended Iron burns with bright glow in Cl Iron burns with dull glow in Br vapour Iron reacts slowly with iodine vapour 24. explain the safety precautions necessary when working with the halogens; Pure Cl, pure Br and iodine vapour should always be handled in fume cupboard. 25. recall the formulae of: *hydrogen, water and halogen molecules; *the halides and hydroxides of group 1 metals; H2, H2O, Cl2, Br2, I2 NaCl, LiBr, NaOH, KOH 26. be able to balance unbalanced symbol equations; Write reactants and products Sodium + chlorine ( sodium chloride Write formulae Na + Cl2 ( NaCl Balance 2Na +Cl2 ( 2NaCl 27. be able to write balanced equations to describe the chemical reactions of group 1 metals with water and halogens; 2Li +2H20 ( 2LiOH +H2 28. recall and use state symbols: (s), (l), (g) and (aq) in equations. (s) is solid, (l) is liquid, (g) is gas, (aq) is aqueous (dissolved in water) 2Li(s) +2H20(l) ( 2LiOH(aq) +H2(g) C4.2 How do chemists explain the patterns in the properties of the elements? 1. describe the structure of an atom in terms of protons and neutrons in a very small central nucleus with electrons arranged in shells around the nucleus;  INCLUDEPICTURE "http://www.drbateman.net/gcse2003/gcsesums/chemsums/atstruc/partic3.gif" \* MERGEFORMATINET  2. recall the relative masses and charges of protons, neutrons and electrons; ParticleRelative massRelative ChargeProton1+1Neutron10Electron1/1840-1 3. recall that in any atom the number of electrons equals the number of protons; Potassium atomic number = 19, 19 protons, 19 electrons 4. recall that all the atoms of the same element have the same number of protons; 1 2 3 H H H 1 1 1 5. recall that the elements in the modern Periodic Table are arranged in order of proton number; 1 H 2 He 3Li 4 Be 5B 6C 7N 8O 9F 10Ne 11Na 6. recall that some elements emit distinctive flame colours when heated (for example lithium, sodium and potassium); Lithium red flame, sodium yellow flame, potassium lilac flame 7. understand that the light emitted from an element gives a characteristic line spectrum; Na | | H | | | 8. understand that the study of spectra has helped chemists to discover new elements; Unexpected yellow line a the spectrum of light from Sun led to discovery of helium. 9. understand that the discovery of some elements depended on the development of new practical techniques (for example spectroscopy); Spectroscopy splints light into line spectra using a spectroscope. Helium would not have been discovered art the time without this technique. 10. be able to use simple conventions (for example 2.8.1 or dots in circles) to represent the electron arrangements in the atoms of the first 20 elements in the Periodic Table; Li atomic no =3 electronic structure 2.1 or  Li 11. recall that a shell (or energy level) fills across a period; Na 2.8.1, Mg 2.8.2, Al 2.8.3 Si 2.8.4 etc 12. understand that the chemical properties of an element are determined by its electron arrangement, illustrated by the electron configurations of the atoms of elements in groups 1 and 7. Li 2.1, Na 2.8.1, K 2.8.8.1 all have 1 outer electron so all have the same properties. F 2.7, Cl 2.8.7, Br 2.8.18.7 all have 7 outer electrons so have similar properties. (but different from group 1) C4.3 How do chemists explain the properties of compounds of Group 1 and Group 7 elements? Li, Na and K atoms can all lose 1 outer electron to become a positive ion. This is a metal property. F, Cl and Br atoms can all gain 1 electron to form negative ions. This is a non-metal property. 1. recall that molten compounds of metals with non-metals conduct electricity and that this is evidence that they are made up of charged particles called ions; Lead bromide, PbBr2 contains lead ions Pb2+ and bromide ions Br-. These charged ions carry current when the compound is molten. 2. recall that an ion is an atom (or group of atoms) that has gained or lost electrons and so has an overall charge; Sodium atom Na, sodium ion Na+ (has lost electron) Iodine atom I, iodine ion I- (has gained electron) 3. account for the charge on the ions of group 1 and group 7 elements by comparing the number and arrangement of the electrons in the atoms and ions of these elements; Na 2.8.1, Na+ 2.8 (has lost electron) Cl 2.8.7, Cl- 2.8.8 (has gained electron) 4. work out the formulae of ionic compounds given the charges on the ions; Na+, Mg2+, F-, O2-. To balance charges formulae must be: NaF, Na2O, MgO, MgF2. 5. work out the charge on one ion given the formula of a salt and the charge on the other ion; For PbCl2 if one ion is Cl- then other ion must be Pb2+ to balance charges. 6. recall that compounds of group 1 metals and group 7 elements are ionic; LiF, NaCl, KI etc are all ionic 7. understand that solid ionic compounds form crystals because the ions are arranged in a regular lattice; Regular NaCl structure that forms crystal is: Na+Cl-Na+ Cl-Na+Cl- Na+Cl-Na+ 8. describe what happens to the ions when an ionic crystal melts or dissolves in water; Ions separate and move around. Na+Cl-Na+ Na+ Cl-Na+Cl- ( Cl- Na+ Cl- Na+Cl-Na+ Na+ Cl- Na+ Na+ Cl- 9. explain that ionic compounds conduct electricity when molten or when dissolved in water because the ions are charged and they are able to move around independently in the liquid. 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