Noble gases Group 1 Build an Group 18 1.008 4.003 H Alkaline earth He metals Halogens 1 Group 2 Periodic TableAtom SimulatorGroup 13 Group 14 Group 15 Group 16 Group 17 2 6.94 9.012 10.81 12.011 14.007 15.999 18.998 20.180 Li Be B C N O F Ne 3 4 5 6 7 8 9 10 22.990 24.305 26.982 28.085 30.974 32.06 35.45 39.95 Na Mg Transition metals Al Si P S Cl Ar 11 12 Group 3 Group 4 Group 5 Group 6 Group 7 Group 8 Group 9 Group 10 Group 11 Group 12 13 14 15 16 17 18 39.098 40.078 44.956 47.867 50.942 51.996 54.938 55.845 58.933 58.693 63.546 65.38 69.723 72.630 74.922 78.971 79.904 83.798 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 85.468 87.62 88.906 91.224 92.906 95.95 [98] 101.07 102.906 106.42 107.868 112.414 114.818 118.710 121.760 127.60 126.904 131.293 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 132.905 137.327 138.905 178.49 180.948 183.84 186.207 190.23 192.217 195.084 196.967 200.592 204.38 207.2 208.980 [209] [210] [222] Cs Ba La Hf Ta W Re Os TheseIr activitiesPt have been createdAu Hg Tl Pb Bi Po At Rn 55 56 57 72 73 74 75 76 by77 the Royal Society78 of Chemistry79 80 81 82 83 84 85 86 to help celebrate the International [223] [226] [227] [267] [268] [269] [270] [269] Year[278] of the Periodic[281] Table. [280] [285] [286] [289] [289] [293] [294] [294] Fr Ra Ac Rf Db Sg Bh Hs MtFind out moreDs at: www.rsc.org/iyptRg Cn Nh Fl Mc Lv Ts Og 87 88 89 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 Alkali metals 140.116 140.908 144.242 [145] 150.36 151.964 157.25 158.925 162.500 164.930 167.259 168.934 173.054 174.967 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Lanthanides 58 59 60 61 62 63 64 65 66 67 68 69 70 71 232.038 231.036 238.029 [237] [244] [243] [247] [247] [251] [252] [257] [258] [259] [262] Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Actinides Wall chart © Royal Society of Chemistry 2018 Registered charity number: 207890 90 91 92 93 94 95 96 97 98 99 100 101 102 103 www.rsc.org/periodic-table Why are elements in groups? The pupils will discover why elements are in groups. Learning outcome: The pupils will discover that number of outer shell electrons are an indication of the group for a neutral atom. Student outcome: The pupils will then write down their rules and be able to predict the next ten neutral elements for outer shell electrons and groups. This exercise is to allow the pupils to discover and to reinforce where the electrons, neutrons and protons are in the atom. It will also allow the pupils to discover how the electrons, neutrons and protons are linked to the different type of elements and the formation of ions or neutral atoms. Ask the pupils to add protons to observe how the name of the element changes when they are added. As more protons are added the pupils will discover that there are many changes; name of the element, the atomic number increases, the mass number (atomic mass) increases and the overall net charge changes. The pupils will also observe that the atom becomes unstable when we add protons only. Why are elements in certain groups? The positioning of the element in a group is based on evidence and understanding. Ask the pupils to make all the first ten elements with only protons and electrons (turn off the stability function to help reduce the formation of misconceptions). The pupils will need to use a periodic table with the suitable group numbers. A neutral hydrogen atom (Group I). There are one electron in the outermost used shell. Since there are only one electron in the outermost shell the element is placed in Group I. The pupils will have the opportunity to discover or reinforce the rules related to electron positioning. A neutral helium atom (Known as Group 8 or Group 0). This shell can only hold two electrons. The outer most shell, that contains electrons, is said to be a “full shell”. When more electrons are added then they must go into the next shell. A rule in chemistry states that when an outer shell is full then it becomes unreactive (KS3 and KS4). A neutral lithium atom (Group I). There are three electrons in this atom however there are only one electron is in the outermost used shell. Since there is one electron in the outermost shell the element is placed in Group I. The pupils will have the opportunity to discover or reinforce the rules related to electron positioning. Explain the relationship between the number of outer electrons in the neutral atom and its group. Beryllium: Explain the relationship between the number of outer electrons in the neutral atom and its group. Boron: Explain the relationship between the number of outer electrons in the neutral atom and its group. Carbon: Explain the relationship between the number of outer electrons in the neutral atom and its group. Nitrogen: Explain the relationship between the number of outer electrons in the neutral atom and its group. Oxygen: Explain the relationship between the number of outer electrons in the neutral atom and its group. Fluorine: Explain the relationship between the number of outer electrons in the neutral atom and its group. Neon: 1. Up to how many electrons can be fitted into the first shell and why? 2. Up to how many electrons can be fitted into the second shell? 3. What does the term “outer shell” mean? 4. What is the relationship between the number of outer electrons in a neutral atom and the group number of the element? 5. Complete the table. Neutral element Number of outer electrons Element Group Number Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine 6. What is the rule for these elements? 7. What is different with helium and neon with this rule? Why? SUMMARY POSTERS Periodic table: The number of subatomic Pupils will be able see the name particles will be highlighted and symbol of the element. They and counted here. will also see how they do/do not change when particles are added. Atomic structure: Net Charge: Pupils will be able to place Pupils will be able see the how the sub-atomic particles into net charge does/does not change the areas of the atom i.e. when particles are added. nucleus and shells Mass Number: Pupils will be able see the mass Sub-atomic particles: does or does not change when Pupils will be able to select particles are added. the type of sub-atomic particle they want to investigate. Variety of simulations: Pupils will be able see to choose the option of simulation. Knowledge based and assessment of knowledge through games. Key terms Protons: Are located in the centre (nucleus) and when a proton is added then the element changes. Hydrogen has one proton; when another proton is added the it is helium (two protons). Neutron: Are located in the centre (nucleus) of the atom. When neutrons are added, they will not change the element. Electron: Are located outside the nucleus in areas called shells or orbits. Sub-atomic particles: This is the group name for protons, neutrons, and electrons. Nucleus: This is at the “centre” of the atom. The main misconception is relating the word nucleus of the atom to the nucleus of a cell. The nucleus in the atom contains two types of sub- atomic particles only. Atomic number: This is the number of protons located in the nucleus. A proton has a relative mass of one (these are atomic units and are not measured in the normal units: kg, g, etc.) A periodic table will have a key that explains where to find the atomic number. Atomic mass: Atomic mass and mass number are the same concept however with different names. This the dual name is a common cause of confusion and creation of a misconception. Atomic mass (mass number) is the mass of the entire atom. A neutron has a mass of one, similar to the proton. However, the neutron will not change the element but only change the mass. The electron has a very small mass. It is 1/1840th the mass of a proton or neutron. The mass can be described as 1/1840 or negligible. It must never be described a zero or nothing. When looking at the periodic table and at the elements this is the larger number located at the element symbol. Charges: There are positive and negative charges in the atom. All the positive charges are in the nucleus (centre of the atom) and all the negative charges are in the shells/orbits outside the nucleus.