C2 0.0 / 5 ? ChemistryThe Periodic TableGCSEAQA Created by: sophielouise277Created on: 16-09-18 12:57 How did John Dalton organise elements? In order of their atomic weights 1 of 27 How did John Newlands organise elements? In order of mass but noticed the properties of every eighth element seemed similar 2 of 27 How did Mendeleev organise the elements? Atomic weights and a pattern in properties could be seen. 3 of 27 Why did scientists think Mendeleev's discovery was a scientific breakthrough? Because he left gaps for elements and predicted their properties. A few years later his predictions closely matched the real elements 4 of 27 What group are the noble gases? Group 0 5 of 27 What do atoms of metals tend to do? Lose electrons 6 of 27 What do atoms of non-metals tend to do? Gain electrons 7 of 27 Why are group 0 gases unreactive? Because of their electron arrangements 8 of 27 What are group 1 elements called? Alkali metals 9 of 27 What is the pattern for melting and boiling points in group 1? It decreases as you go down the group 10 of 27 Why do alkali metals have to be stored in oils? To stop them from reacting with oxygen in the air 11 of 27 Why does the shiny silvery surface of an alkali metal turn dull when mixed in air? It is oxidising with the oxygen in the air 12 of 27 Why are alkali metals really reactive? They have one electron they want to get rid of 13 of 27 When you add an alkali metal to water why does it float and fizz? Because the metal reacts with water to form hydrogen gas 14 of 27 What forms when alkali metals react with water? H+ ions to make ionic compounds. These are generally white and dissolve in water, giving colourless solutions 15 of 27 What are group 7 elements called? Halogens 16 of 27 What is the pattern for mp and bp in halogens? Increase as you go down the group 17 of 27 What is the pattern for reactivity in halogens? They get less reactive as you go down the group 18 of 27 What will a more reactive halogen do to a less reactive halogen? Displace it from solutions of its salts 19 of 27 The number of shells increases as you go down the periodic table, what effects does this have? Larger atoms lose electrons more easily, larger atoms gain electrons less easily 20 of 27 What does the electrostatic attraction depend upon? Distance between outer electrons and nucleus, No of shells and size of positive charge 21 of 27 What are transition metals? Metals in the middle of the periodic table 22 of 27 Name 4 physical properties of a transition metal Good conductors, hard and strong, high densities and high melting points (apart from Mercury) 23 of 27 How reactive are transition metals? Less reactive than group 1 24 of 27 Why are transition metals important in the industry? They can be used as catalysts 25 of 27 Do transition metals react vigorously with oxygen or water? No 26 of 27 What can a transition metal form? Ions with different charges, in compounds that are coloured 27 of 27
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