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THE PERIODIC TABLE

Explore the properties and patterns of elements in the periodic table. Discover the arrangement of metals, non-metals, and metalloids. Learn about atomic numbers, groups, and periods.

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THE PERIODIC TABLE

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  1. THE PERIODIC TABLE

  2. There are millions of substances in the world. All these substances are made from about 100 different building blocks called elements. These elements take a huge variety of forms: From poison gases like chlorine From reactive metals like sodium to unreactive metals like gold To the air we breathe Variety

  3. In science the word properties means, what the substance is like. E.g. Here are some properties of sodium: Metallic Highly reactive Solid but melts easily Low density (light) It would be really useful to be able to predict properties of elements instead of having to remember them! Properties of Elements

  4. Scientists found that the properties of elements seem to depend upon atomic number. Atoms contain three types of particles: Atomic Number • Atomic number = the number of protons in an atom.

  5. In elements the atoms contain equal numbers of protons and electrons. It follows that for an element the atomic number is equal both to the number of protons and to the number of electrons. Fluorine 9 protons 9+ 9 electrons 9- 10 neutrons 0 Total Charge 0 Atomic Number Symbol Atomic Mass Atomic Number and Electrons 9 F 19

  6. When scientists arranged elements in order of increasing atomic number (below) they found patterns in the properties. H Mg Al K He Li Be B C N O F Ne Na Si P S Cl Ar Reactive Metals Reactive Gases Unreactive Gases Atomic Number and Patterns

  7. Activity Do similar elements occur at regular intervals? Reactive Metals Reactive Gases H Mg Al He Li Be B C N O F Ne Na Si P S Cl Ar K 1 12 13 19 2 3 4 5 6 7 8 9 10 11 14 15 16 17 18 Count the number of elements to get from one reactive metal to the next? 8 Count the number of elements to get from one reactive gas to the next? 8

  8. If we divide the elements up and arrange them into a table we easily get patterns. H Mg Al He Li Be B C N O F Ne Na Si P S Cl Ar K 1 12 13 19 2 3 4 5 6 7 8 9 10 11 14 15 16 17 18 Cut here H He and here and here Li Be B C N O F Ne And arrange these strips below each other Mg Al Na Si P S Cl Ar Putting Elements in a Table K Mg Na

  9. When we rearrange the strips elements that are similar go into the same columns. H Mg Al He Li Be B C N O F Ne Na Si P S Cl Ar K 1 12 13 2 3 4 5 6 7 8 9 10 11 14 15 16 17 18 19 Reactive Metals Reactive Gases He Unreactive Gases F B C N O Be Li Ne Cl S Al Si P Mg Ar Na K Putting Elements in a Table Mg Na

  10. Carrying on building up the elements by atomic number led to the creation of the periodic table shown below. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Putting Elements in a Table Mg Na

  11. Downward columns are called groups. Group 1 Group 2 Group 5 Group 3 Group 4 Group 6 Group 7 Group 0 H He Transition Elements Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Groups – Columns of Elements Means in-between Mg Na

  12. Rows of elements are called periods. Period Number 1 H He 2 Li Be B C N O F Ne 3 Na Mg Al Si P S Cl Ar 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Periods – Rows of Elements

  13. Activity Gp 2 1 0 5 3 4 6 7 Pd H 1 He C 2 Li Be B C N O F Ne 3 Na Mg Al Si P S Cl Cl Ar Mg 4 K K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? K C Cl Mg What’s the group and Period? Group 7 Period 3 Group 1 Period 4 Group 2 Period 3 Group 4 Period 2

  14. Below the chemical symbol have been replaced by atomic numbers. You will see some are missing 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 26 19 20 21 22 23 24 25 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 87 88 89 104 105 106 107 108 109 110 111 112 Two further series of elements should go here but are only shown on some Periodic Tables. They are called the lanthanides and actinides. Missing Elements!

  15. Metals are on the left and centre. Patterns 1. Metals and Non-metals • Non-metals are mostly on the right • In between are metalloids – these are like metals in some ways and like no-metals in others.

  16. Patterns 1. Metals and Non-metals

  17. Activity Say whether these elements are metals, non-metals or metalloids H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Francium (Fr) Silicon (Si) Cobalt (Co) Scandium (Sc) Krypton (Kr) Metal Metalloid Metal Non-metal Metal

  18. Physical state means – is it a solid, liquid or gas. There are only 2 liquid elements. Notice how most of the gases are on the far right. Physical State

  19. Physical State

  20. Activity Say whether these elements are solids, liquids or gases. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Niobium (Nb) Krypton (Kr) Bromine (Br) Barium (Ba) Nitrogen (N) Gas Solid Liquid Solid Gas N Br Kr Nb Ba

  21. As a general, but not perfect, rule: the further to the left and the further down the table - the more reactive the metal is. Patterns 2. Reactivity of Metals More Reactive More Reactive

  22. Activity Which metal is most reactive? H Li Be Na Mg Al K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Potassium (K) or Lithium (Li) Calcium (Ca) or Iron (Fe) Calcium (Ca) or Magnesium (Mg) Copper (Cu) or Barium (Ba) K Ba Ca Ca

  23. This is more complicated. At the very end of the periodic table is the most unreactive group of elements in the table. Apart from that – the further up and the further right – the more reactive the non-metal. Unreactive Patterns 3. Reactivity of Non-Metals More reactive More reactive

  24. Activity Which non-metal is most reactive? He B C N O F Ne Si P S Cl Ar As Se Br Kr Te I Xe At Rn Neon (Ne) or Iodine (I) Fluorine (F) or Chlorine (Cl) Carbon (C) or Oxygen (O) Oxygen (O) or Silicon (Si) I O O F

  25. The physical and chemical properties of elements are hugely influenced by the number and arrangement of electrons in the atom. This is why patterns in properties are linked to atomic number. If the atomic number increases by one it means that the atom has one extra electron. Atomic number = number of protons 1 H 1 2 He 4 3 Li 7 4 Be 9 5 B 10 For atoms of an element it is also = number of electrons Each element has one more electron Patterns and Electron Structures

  26. The places where we start a new period is to do with the arrangement of the electrons. It is the point at which electrons start entering a new shell further from the nucleus. H Mg Al He Li Be B C N O F Ne Na Si P S Cl Ar K 1 12 13 19 2 3 4 5 6 7 8 9 10 11 14 15 16 17 18 Cut here and here and here Patterns and Electron Structures We shall look at these electron arrangements in the next few slides.

  27. We can imagine building up atoms by adding protons, neutrons and electrons as we cross the periodic table. 2 1 2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8 Sc Ti V Cr Mn Fe Co Ni Cu Zn 2,8,1 2,8,2 2,8,4 2,8,3 2,8,5 2,8,6 2,8,7 2,8,8 2,8,8,1 2,8,8,2 Electrons in 1st shell Electrons in 4th shell Electrons in 2nd shell Electrons in 3rd shell Patterns of Electron Arrangements 2,8,8,2

  28. Because electrons will fill up “shells” working outwards from the nucleus. The periodic table can be used to work out the electronic arrangements within atoms. 1 0 1 2 3 4 5 6 7 1 2 2 2,1 2,3 2,4 2,5 2,6 2,7 2,8 2,2 3 2,8,4 2,8,1 2,8,2 2,8,3 2,8,5 2,8,6 2,8,7 2,8,8 4 2,8,8,1 22 Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Deducing Electron Arrangements Group Number = number of outer shell electrons (Except for Gp 0) Period number = number of shells Atomic number (which can be obtained by counting boxes starting with the top left ) = number of electrons

  29. Activity Gp 2 1 0 5 3 4 6 7 Pd H 1 He C 2 Li Be B C N O F Ne 3 Na Mg Al Si P S Cl Cl Ar Mg 4 K K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Rf Db Sg Bh Hs Mt ? ? ? Mg C What’s the electron arrangement K Cl 2.8.7 2.8.2 2.4 2.8.8.1

  30. Arrangement of Electrons 1 2 3 4 5 6 7 8 1 2 3 Click on action buttons to reveal how electron configuration is built-up. The transition metals Skip this

  31. Electrons in Period 1 1 2 3 4 5 6 7 8 1 1 2 Skip this

  32. 2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8 Electrons in Period 2 Elements in the second period contain 2 electrons in the first shell (complete) and the second shell is completed one electron at a time as you cross the period from left to right. 1 2 3 4 5 6 7 8 2 This atom is special it has a complete outer shell Skip this

  33. Electrons in Period 3 Elements in the third period have complete first and second shells. The third shell is completed one electron at a time as you cross the period from left to right. 1 2 3 4 5 6 7 8 3 2,8,1 2,8,2 2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8 Skip this

  34. Group 1 Elements 1 Group 1 elements have 1 electron in the outermost shell which they lose in chemical reactions. The outer electron is further from the nucleus and so more easily lost as you go down the group. This is why reactivity increases going downwards 1 1 2 2,1 3 Skip this 2,8,1

  35. Group 2 Elements In chemical reactions metals tend to lose their outer shell electrons to form positive ions. So, these elements all form ions with a 2+ charge. The further the outer shell is from the nucleus the more easily electrons are lost. 2 2,2 2,8,2 Skip this

  36. Group 3 Elements 3 Metals lose their outer electrons to form ions. The charge on the ion produced by Group 3 metals will be +3. 2,3 Skip this 2,8,3

  37. Group 4 Elements 4 The elements at the top of Group 4 are non-metals. They bond covalently, i.e. by sharing electrons with another atom. 2,4 Skip this 2,8,4

  38. Group 5 Elements 5 The number of electrons in the outermost shell is the same as the group number. They need 3 more electrons to achieve a full electron shell. 2,5 Skip this 2,8,5

  39. Group 6 Elements The atoms in Group 6 form negative ions (2-) by the addition of two extra electrons. This completes their outer most shell. 6 2,6 Skip this 2,8,6

  40. Group 7 Elements Group 7 elements form 1- ions by the addition of 1 extra electron. They are most reactive at the top of the group because incoming electrons are pulled into shells that are closer to the nucleus. 7 2,7 Skip this 2,8,7

  41. Group 0 Elements 8 The elements in Group 8 (or 0) have complete outer shells. They are very unreactive and are called NOBLE (or inert) GASES. 2 2,8 Skip this 2,8,8

  42. The fact that in each group the number of outer shell electrons is the same leads to similar types of chemical reactivity. E.G. All group 1 elements react with water to give hydrogen and an alkali. The fact that the outer shell electrons get progressively further from the nucleus leads to trends (patterns). E.G. Group 1 elements get more reactive as you go down the group. Periodic Table and Reactivity

  43. Broad Types of Element

  44. In the Periodic Table elements are arranged in order of? Atomic mass Atomic number Density Boiling point

  45. Neutral atoms of an element contain? Equal numbers of protons and neutrons Equal numbers of electrons and neutrons Equal numbers of protons and electrons Equal numbers of protons, neutrons and electrons

  46. A vertical collection of elements in the Periodic Table are called? Groups Periods Columns Gases

  47. A horizontal collection of elements in the Periodic Table are called? Groups Periods Rows Gases

  48. In the Periodic Table gases occur? On the left On the left and middle On the right and middle On the Right

  49. In the Periodic Table metals occur? On the left On the left and middle On the right and middle On the Right

  50. The Group 7 Elements are also called? The halogens The transition elements The alkali metals The noble gases

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