1. The Periodic Table of Elements

2. DMITRI MENDELEEV (1834- 1907)- The originator of the modern periodic table What is the periodic table? What information is obtained from the table ? How can elemental properties be predicted base on the Periodic Table? 3. There are approximately 110 different known elements. Each element has its own symbol made up of one or two letters. The first letter is always a CAPITAL letter. If there is a second letter it is always a SMALL letter. Points to ReMeMbEr.. 4. As there are so many elements , it becomes necessary to classify them into those which have Similar physical and chemical properties. This classification by properties divides the elements into Chemical families or groups . Each element is arranged according to its atomic number. Classification of elements!!! 5. Families of the Periodic Table Families/Groups group I - Alkali metals group II - Alkaline Earth metals group III - Boron Family group IV - Carbon Family group V - Nitrogen Family group VI Oxygen Family group VII - Halogens group VIII - Noble Gases Transition Metals 6. Periodic Table: The three broad Classes Main (Representative), Transition metals, lanthanides and actinides (rare earth) 7. Across the Periodic Table Periods: Are arranged horizontally across the periodic table (rows 1-7) These elements have the same number of valence shells. 1 IA 18 VIIIA 1 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 2nd Period 6th Period 8. Down the Periodic Table Groups : Are arranged vertically down the periodic table These elements of the same group have the same number electrons in the outer most shells (the valence shell.) 1 IA 18 VIIIA 1 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 Alkali Family: 1 e- in the valence shell Halogen Family: 7 e- in the valence shell 9. Look at the next picture of the periodic table. Where are the metals found? Where are the non-metals found? 10. 1 IA 18 VIIIA 1 1 H 1.00797 2 IIA Periodic Table 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 He 4.0026 2 3 Li 6.939 4 Be 9.0122 5 B 10.811 6 C 12.0112 7 N 14.0067 8 O 15.9994 9 F 18.9984 10 Ne 20.179 3 11 Na 22.9898 12 Mg 24.305 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 13 Al 26.9815 14 Si 28.086 15 P 30.9738 16 S 32.064 17 Cl 35.453 18 Ar 39.948 4 19 K 39.102 20 Ca 40.08 21 Sc 44.956 22 Ti 47.90 23 V 50.942 24 Cr 51.996 25 Mn 54.9380 26 Fe 55.847 27 Co 58.9332 28 Ni 58.71 29 Cu 63.54 30 Zn 65.37 31 Ga 65.37 32 Ge 72.59 33 As 74.9216 34 Se 78.96 35 Br 79.909 36 Kr 83.80 5 37 Rb 85.47 38 Sr 87.62 39 Y 88.905 40 Zr 91.22 41 Nb 92.906 42 Mo 95.94 43 Tc [99] 44 Ru 101.07 45 Rh 102.905 46 Pd 106.4 47 Ag 107.870 48 Cd 112.40 49 In 114.82 50 Sn 118.69 51 Sb 121.75 52 Te 127.60 53 I 126.904 54 Xe 131.30 6 55 Cs 132.905 56 Ba 137.34 57 La 138.91 72 Hf 178.49 73 Ta 180.948 74 W 183.85 75 Re 186.2 76 Os 190.2 77 Ir 192.2 78 Pt 195.09 79 Au 196.967 80 Hg 200.59 81 Tl 204.37 82 Pb 207.19 83 Bi 208.980 84 Po [210] 85 At [210] 86 Rn [222] 7 87 Fr [223] 88 Ra [226] 89 Ac [227] 104 Ku [260] 105 106 107 108 109 11. In the periodic table, metals and non metals can be divided by a stair case line. 1 IA 18 VIIIA 1 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 12. Periodic Table: Metallic arrangement Metals vs Nonmetals 1 IA 18 VIIIA 1 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 Metals All elements underneath the staircase are metals 13. Periodic Table: Metallic arrangement Metals vs Nonmetals 1 IA 18 VIIIA 1 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 Metals The elements above the staircase are non metals 14. Reading the Periodic Table: Classification Nonmetals, Metals, Metalloids, Noble gases Elements close to the staircase line, Can have some properties of metals and non metals they are called Metalloids 15. i.e. Magnesium 2. 8. 2 Mg 1st energy level 2nd energy level 3rd energy level Magnesium atomic no. 12 It has 12 protons & 12 electrons. 16. Mg Mg Loses two electrons Mg+2 Metal forming a positive ion 17. i.e. Chlorine 2. 8. 7 Cl 1st energy level 2nd energy level 3rd energy level Chlorine atomic no. 17 It has 17 protons & 17 electrons. 18. Cl Cl Cl-1 Non-Metal forming a Negative ion 19. Metals Non-metals Usually solids at room temperature except mercury Often gases except: Bromine: liquid Sulphur: solid Phosphorus: solid Iodine: solid Carbon: solid Boron: solid Silicon: solid High melting and boiling points (except Group I) Low melting and boiling points (except B, C, Si) Good conductors of heat and electricity Poor conductors of heat and electricity (except carbon/graphite) Often shiny, ductile, malleable, and possess great tensile strength Normally dull, soft, cannot be drawn out into wires or made into flat sheets Differences between metals and non-metals 20. Most compounds are ionic Most compounds are covalent Oxides are usually basic or amphoteric Oxides are usually neutral or acidic Often form hydrogen gas with dilute acids Never form hydrogen gas from acids Always form position ions (cations) Always form negative ions (anions) Metals Non-metals 21. 1. On which side of the periodic table do you find gases? 2. On which side of the periodic table do you find non-metals? 3. How do alkali metal atoms achieve stability? 4. What is the charge on group II metallic ion? 5. What is the charge on group VI non-metallic ion? 22. Group I Elements THE ALKALI METALS called Alkali metals BECAUSE the metals react with water to form alkaline solutions: the solutions turn red litmus paper blue. 23. Properties Of Group 1 Elements 24. have one outer shell electrons 25. shiny, silvery solids 26. Soft, easily cut with scalpel 27. low densities and melting points 28. As the atomic radius increases, the charges are further apart and the electrical attractive force is reduced. This results a weaker metallic bond and little heat energy is needed to overcome the bond. Thus, the melting/boiling point decreases as we go down the group. 29. good conductors of heat and electricity reacts easily in air so they're kept in oil. chemically reactive - reactivity increases down the group Caesium most reactive of all metals 30. loses one outermost electron to form an ion of +1 charge eg. Li+, Na+, K+ react violently with air or oxygen, catching fire, and burning with characteristic flame colors to form white oxides. To avoid this, t he metals are stored under oil eg. 4K (s) + O2 (g) ----> 2K2O (s) 31. Write down the balanced chemical equations to show the reaction of Lithium, sodium, rubidium and caesium with air!! elements in same group form same formula. Note: 32. They also react vigorously with water, forming the alkaline hydroxide and releasing hydrogen gas eg. 2Na (solid) + 2H2O (liquid) ---> 2NaOH (aqueous) + H2 (gas) 33. Write down the balanced chemical equations to show the reaction of Lithium, potassium , rubidium and caesium with water !! 34. Because alkali metals are such reactive metals, they combine directly with reactive non-metals such as the halogens to form salts eg. 2Na (s) + Cl2 (g) ----> 2NaCl (s) 35. Write down the balanced chemical equations to show the reaction of Lithium, potassium, rubidium and caesium with fluorine !! 36. Alkali metal Flame color Li red Na yellow K lilac Rb - FLAME COLOUR OF SOME ALKALI METALS 37. Alkali metal Reaction with air (oxygen) Reaction with water Reaction with chlorine lithium burns with a red flame to give lithium oxide (white solid) 4Li + O2 ---> 2Li2O floats on water and reacts quickly to produce lithium hydroxide and hydrogen gas 2Li + 2H2O ---> 2LiOH + H2 burns with a bright flame to give a white solid of lithium chloride 2Li + Cl2 ---> 2LiCl sodium burns with a bright yellow flame to produce white sodium oxide 4Na + O2 ---> 2Na2O floats on water and reacts very quickly to produce sodium hydroxide and hydrogen gas 2Na + 2H2O ---> 2NaOH + H2 burns with a bright flame to give a white solid of sodium chloride 2Na + Cl2 ---> 2NaCl potassium burns violently with a lilac colored flame to produce white potassium oxide 4K + O2 ---> 2K2O floats on water and reacts violently to produce potassium hydroxide and hydrogen gas 2K + 2H2O ---> 2KOH + H2 burns vigorously in chlorine with a bright flame to give a white solid of potassium chloride 2K + Cl2 ---> 2KCl Summary Table of the reactions of the alkali metals 38. Group VII Elements THE HALOGENS The word halogen itself refers to "salt former" in Greek. Halogens such as chlorine, bromine and iodine have properties that enable them to react with other elements to form important salts such as Sodium Chloride -- Table Salt. 39. Properties Of Group VII Elements 40. have seven outer shell electrons 41. elements become darker and solidify down the group Halogen Colour State Fluorine pale yellow gas Chlorine yellowish green gas Bromine red brown liquid Iodine shiny black solid 42. reactivity decreases down the group most reactive is fluorine; least reactive is iodine 43. because of their atomic size, which increases down the group therefore it becomes more difficult for the nucleus to attract an electron to form an ion. Why??? 44. reactive non-metals poisonous low melting and boiling points increases down the group all halogens form ions with single negative charge eg F-, Cl-, Br- Exists as diatomic molecules eg F2, Cl2, Br2, I2 reacts vigorously with metals to form ionic salts 45. Any halogen above another in the group will displace it from a solution of its salt ----> displacement reactions . This means that the more reactive halogen can take the place of the less reactive halogen of its salt. When chlorine gas is bubbled through a colorless solution of potassium bromide, reddish brown color of bromine is seen. eg. Cl2 + 2KBr -----> 2KCl + Br2 When chlorine gas is bubbled through a colorless solution of potassium iodide, it turns brown and finally a black precipitate of iodine is formed. eg. Cl2 + 2KI ----> 2KCl + I2 46. Write any three physical properties of group 7 elements. 47. Group VIII Elements THE Noble / Inert Gases They are chemically inert because the outermost shell of the element is full. It does not tend to combine with other elements, either covalently or ionically, and so are chemically inactive 48. Exist as monatomic (single atom) least reactive elements in the gaseous state; do not form bonds low melting and boiling points have stable electronic configuration with full electrons on their shells 49. THE TRANSITION METALS Since they can have variable oxidation states ---> no fixed Valency. 50. often form colored compounds 51. less reactive than group I and group II metals. high melting and boiling points and densitities. Variable oxidation states ---- which means it can form more than one ion: for example, Fe2+ iron(II) Fe3+ iron(III) Cu+ copper(I) Cu2+ copper(II) 52. Industrial process Description Contact Process uses vanadium(V) oxide to help in the conversion to sulphur trioxide Haber Process uses an iron catalyst with iron oxide promoters to make ammonia gas Margarine manufacture uses nickel catalyst in the hydrogenation of alkene can have catalytic properties ie: they speed up the industrial reactions . 53. 1. Which property decides the order of the elements in the Periodic Table? a. masses of their atoms b. number of electrons in the outer shell c. number of neutrons in the nucleus d. number of protons in the nucleus 54. 2. A metal X forms oxides with the formulae XO and X2O3 Where is X in the Periodic Table? a. Group II b. Group III c. second Period d. transition elements. 55. 3. Which of the following is a property of aqueous potassium iodide? a. it does not conduct electricity b. it is decolorised by chlorine c. it reacts with aqueous bromine to form iodine d. it reacts with aqueous lead(II) nitrate to form a white precipitate. 56. 4. Which list contains 3 elements that all exist as diatomic molecules at room temperature? a. hydrogen, fluorine, neon b. nitrogen, chlorine, neon c nitrogen, oxygen, fluorine d. oxygen, chlorine, helium