CC3/4 – Atomic structure (p79-82) Periodic Table - add the following labels: group, group numbers, period, metals, non-metals, metalloids, atomic mass, atomic symbol, atomic (proton number) CC3/4 – Atomic structure (p79-82) Electronic configurations – complete the electronic configuration of sodium. Structure of Atoms 1. Add a key to the diagram. 2. Fill in the table to show the properties of each Sub-atomic particle. Name Charge Mass Location Relative Atomic Mass A sample of lead contains 26.5% 206Pb, 26.5% 207Pb and 47% 208Pb, what is the relative atomic mass? Why are there three different types of Pb atom? Using the periodic table Pair Reversal -which 2 elements here did Mendeleev swap places? Why did he do this? History of the atom – describe the previous atom models and the experiments which led to them.

CC3/4 – Atomic structure (p79-82) Periodic Table - add the following labels: group, group numbers, period, metals, non-metals, metalloids, atomic mass, atomic symbol, atomic (proton number) CC3/4 – Atomic structure (p79-82) Periods 8/0 1 2 3 4 5 6 7 Electronic configurations – complete the electronic configuration of sodium. Atomic mass 1 2 3 4 5 6 7 Atomic symbol Groups Atomic (proton) number Non-metals Structure of Atoms 1. Add a key to the diagram. 2. Fill in the table to show the properties of each Sub-atomic particle. Metaloids Metals Name Charge Mass Location Proton +1 1 Nucleus Neutron Electron -1 0.0005 Shells Relative Atomic Mass A sample of lead contains 26.5% 206Pb, 26.5% 207Pb and 47% 208Pb, what is the relative atomic mass? 207.205 Why are there three different types of Pb atom? They are isotopes (different numbers of neutrons) Using the periodic table Pair Reversal -which 2 elements here did Mendeleev swap places? Why did he do this? History of the atom – describe the previous atom models and the experiments which led to them. 11 2 9 8 12 3 23 4 19 16 24 7 11 2 9 8 12 3 11 2 9 8 12 3 12 2 10 8 4 He swapped Te and I. He did this because although they were no longer in mass order they better matched the properties of their new group. Later discovery of atomic number supported swapping them. Thomson’s plum pudding model. He proposed a ball of positive charge with negative electrons spread out. Rutherford’s nuclear atom. A central positive charge with negative electrons around it.