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KS4 Chemistry

KS4 Chemistry. The Periodic Table. Contents. The Periodic Table. Elements and atomic number. Arranging elements. Patterns of behaviour. Patterns and electron structure. Summary activities. What are all substances made of?.

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KS4 Chemistry

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  1. KS4 Chemistry The Periodic Table

  2. Contents The Periodic Table Elements and atomic number Arranging elements Patterns of behaviour Patterns and electron structure Summary activities

  3. What are all substances made of? There are millions of different substances in the world, but what are they all made of? • Elements– the building blocks of all substances. There are about 100 different elements in a variety of forms. From sodium, a reactive metal… …to gold, an unreactive metal. From chlorine, a poisonous gas… …to oxygen, a life-giving gas.

  4. Properties of elements What is a property of an element? A property is any characteristic of an element. For example, here are some properties of sodium: • metallic; • highly reactive; • solid but melts easily; • feels light (low density). It would be really useful to be able to predict properties of elements instead of having to remember them! Are there any patterns in the properties of elements?

  5. atomic number = the number of protons in an atom Properties and atomic number The properties of an element depend on its atomic number. What is the atomic number of an element? Atoms contain three types of particles: Where are these particles found in an atom?

  6. proton electron neutron What is atomic number? What are the particles in this helium atom? What is the atomic number of helium? 2

  7. Total charge = 0 atomic number = the number of electrons in an atom Atomic number, charge and electrons Atoms contain equal numbers of protons and electrons.This means that atoms are neutral. What is the charge of a fluorine atom? 9 protons = +9 9 electrons = -9 10 neutrons = 0 What links atomic number and the number of electrons?

  8. Atomic structure revisited

  9. Contents The Periodic Table Elements and atomic number Arranging elements Patterns of behaviour Patterns and electron structure Summary activities

  10. Periodic table timeline

  11. Na Ar O H He Li Be B N C Cl Ne K Mg Al Si P S F Atomic number and patterns of behaviour If the elements are arranged in order of increasing atomic number, patterns in their properties can be seen. reactive gases reactive metals unreactive gases

  12. F Al Li K Ar S P H He Cl Mg B C N Be O Si Ne Na Positions of similar elements Compare the positions of similar elements: reactive gases reactive metals unreactive gases How many elements from one reactive gas to the next? 8 How many elements from one reactive metal to the next? 8 How many elements from one unreactive gas to the next? 8

  13. Mendeleev and the periodic table Mendeleev created the first modern periodic table by grouping together elements with similar properties.

  14. cut here cut here cut here He Li Be B C N Ar O Na H Mg Al Si P S Cl F Ne Ar K K H He Li Be B C N Ne O Mg Al Si P S Cl F Na Arranging elements Divide the elements at set intervals into separate rows: Arrange these rows so elements with matching properties are together:

  15. hydrogen is a special case reactive metals reactive gases unreactive gases Ne He Li Be B C N O F Na Mg Al Si P S Cl Ar K H Arranging elements into columns When elements are arranged according to their properties what patterns do you see? Similar elements go into the same columns. Hydrogen is an exception – it is best positioned above the reactive metals.

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

  17. 44 8 118 1 10 87 88 89 104 105 106 107 108 109 110 111 112 113 114 115 55 116 57 39 9 56 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 37 38 40 41 117 29 53 45 46 47 38 49 50 51 52 54 27 19 20 21 22 23 24 25 26 28 42 30 7 43 2 31 32 33 34 35 36 11 12 14 15 16 17 18 3 4 5 6 13 Missing elements! In this periodic table the symbols are replaced by atomic numbers. Some of the numbers are missing – where? Two more rows of elements fit here. They are called the lanthanides and actinides and are only shown on some periodic tables.

  18. The elements in the periodic table

  19. 1 5 0 2 3 7 6 4 Db Rf Ac Ag Fr Ds Sg Ra Bh La Mt Rg Hf ? ? ? ? ? ? Hs W Mo Ru At Re Os Ir Pt Au Hg Tl Pb Rh Bi Rn Ta Rb Sr Y Zr Nb ? Tc Po Cs Cd Pd Sn Te I Xe K Ca Sc Ti As Cr Mn Fe Co Ni Cu Zn Ga Ge Sb V Ba Se He Na Li In Mg Al Si P S Kr Cl Be Br B C N O F Ne H Ar Columns of elements What are columns of elements called? groups

  20. 7 1 2 6 4 3 5 Ds Fr Ra Ac Rf Db Sg Bh Hs ? Rg Pd Hf ? ? ? ? ? ? Mt La Mo Ru Po Re Os Ir Pt Au Hg Tl Pb W Bi At Ta Rb Sr Y Zr Nb Cs Tc Rn Ba Kr Ag Ge Sn Sb Te I Xe K Ca Sc V Cr Mn Fe Co Ni Cu Zn Ga In Ti Rh Se He As Cd Na Mg Al Si P S Br Cl Li Be B C N O F Ne H Ar Rows of elements What are rows of elements called? periods

  21. Contents The Periodic Table Elements and atomic number Arranging elements Patterns of behaviour Patterns and electron structure Summary activities

  22. Metalloids aren’t a type of rock music fan! Metalloids have some properties similar to metals and other properties similar to non-metals. Patterns: metals and non-metals Where are these different types of elements grouped together in the periodic table? • metals on the left and centre • non-metals on the right (except hydrogen) • metalloids between metals and non-metals Can you name a metalloid element?

  23. Metals, non-metals and metalloids

  24. Only two elements are liquids at room temperature.What are they? Patterns: physical state Where are these elements of different states grouped together in the periodic table? • solids on the left, in the centre and on the right • liquids in the middle and on the right • gases on the far right (except hydrogen) • bromine and mercury

  25. Solids, liquids and gases

  26. increase in reactivity Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Sr Rb Y Fr Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn K Ca Be Ti Sc Cr Li Al Mg V Ga Na Cu Ni Co Fe Mn Zn increase in reactivity Patterns: reactivity of metals What happens to the reactivity of metals along a period? What happens to the reactivity of metals down a group? Which is the most reactive metal?

  27. Which metal is more reactive?

  28. unreactive increase in reactivity Se At Rn Sb Te I Xe Ge As Br Si Kr S Cl Ar B C N O F Ne He P increase in reactivity Patterns: reactivity of non-metals Group 0 elements are the most unreactive of all elements. For the remaining non-metals and metalloids, reactivity increases up a group and along a period from left to right. Which is the most reactive non-metal/metalloid?

  29. Which non-metal is more reactive?

  30. Contents The Periodic Table Elements and atomic number Arranging elements Patterns of behaviour Patterns and electron structure Summary activities

  31. Tc Mt Fr Ra Ac Rf Db Sg Bh Hs Ds H Rg ? ? ? ? ? ? ? Ba Mo Cs Nb Pb Ta W Re Os Ir Pt Au Hg Tl Po Bi La At Rn Rb Sr Y Zr Hf Ru He Zn Pd Ag Cd In Sn Sb Te I Xe K Ca Sc Ti V Cr Mn Fe Co Ni Cu S Ga Ge As Se Br Kr Na Mg Al Si P Cl Ar Li Be B C N O F Ne Rh Patterns, atomic number and electrons The periodic table shows that patterns in the properties of elements are linked to atomic number. What links atomic number and the properties of elements? electrons

  32. Atomic number and electrons The properties of elements are hugely influenced by the number and arrangement of electrons in the atom. What links atomic number and the number of electrons in an atom? atomic number = number of protons number of protons = number of electrons atomic number = number of electrons As atomic number increases by one, the number of electrons also increases by one. This means that the elements in the periodic table are also arranged in order of the number of electrons.

  33. 2nd shell holdsa maximum of8 electrons 1st shell holdsa maximum of2 electrons 3rd shell holdsa maximum of8 electrons Electron shells Electrons are arranged in shells around an atom’s nucleus. Each shell has a maximum number of electrons that it can hold. Electrons will fill the shells nearest the nucleus first. This electron arrangement is written as 2,8,8.

  34. 1 5 0 2 3 6 7 1 4 He H Electrons in period 1 Elements in period 1 only have electrons in the first shell. Why are there only two elements in period 1? 1 2 The first shell can only hold a maximum of two electrons, so period 1 only includes the elements hydrogen and helium. What is special about the outer shell of helium?

  35. 1 5 0 2 3 7 6 2 4 Li Be C B O N F Ne Electrons in period 2 Elements in period 2 all have a complete first shell. What happens to electrons in the second shell in period 2? 2,4 2,5 2,7 2,1 2,2 2,3 2,6 2,8 The second shell is completed one electron at a time going across the period from left to right. What is special about the outer shell of neon?

  36. 1 5 0 2 3 7 6 3 4 Na Mg Si Al S P Cl Ar Electrons in period 3 Elements in period 3 have complete first and second shells. What happens to electrons in the third shell in period 3? 2,8,4 2,8,5 2,8,7 2,8,1 2,8,2 2,8,3 2,8,6 2,8,8 The third shell is completed one electron at a time going across the period from left to right. What is special about the outer shell of argon?

  37. 1 5 0 2 3 7 6 1 2 3 4 4 Patterns of electron arrangements Consider the electron arrangements of the first 20 elements in the periodic table. 2 1 2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8 2,8,1 2,8,2 2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8 2,8,8,1 2,8,8,2 What is the pattern of outer shell electrons in a group? What is the pattern of outer shell electrons across a period? What is the pattern of full electron shells in a group?

  38. Trends across a period: Electron trends in the periodic table Trends down a group: • the number of outer shell electrons is the same; • the number of complete electron shells increases by one. The number of a group is the same as the number of electrons in the outer shell of elements in that group,except for group 0. • the number of outer shell electrons increases by one; • the number of complete electron shells stays the same. The point at which a new period starts is the point at which electrons begin to fill a new shell.

  39. Electrons and groups

  40. Groups and periods

  41. What’s the electron arrangement?

  42. Names of groups in the periodic table

  43. Contents The Periodic Table Elements and atomic number Arranging elements Patterns of behaviour Patterns and electron structure Summary activities

  44. Glossary • atomic number – The number of protons in an atom. Sometimes called the proton number. • electron arrangement – A shorthand way of writing the number of electrons in an atom’s electron shells. • element – A substance made up of only one type of atom. • group – A column in the periodic table containing elements with the same number of outer shell electrons and similar chemical properties. • period – A row in the periodic table containing elements with the same number of full electron shells. • periodic table – The table that lists all the elements in order of increasing atomic number, arranged into groups and periods. • property – Any characteristic of an element.

  45. Anagrams

  46. Matching elements and groups

  47. Multiple-choice quiz

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