The Periodic Table

  • Created by: fjhcab
  • Created on: 21-03-16 21:04
Early 1800s
Categorised by physical & chemical properties & by relative atomic mass
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Döbereiner grouped similar elements called triads
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Newlands arranged it by mass. Came up with law of octaves
3 of 18
Mendeleev arranged atoms by mass but left gaps
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Modern Periodic Table
Moseley in 1914. Arranged elements by increasing atomic (proton) number
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Nuclear Charge
The more protons , the more positively charged & stronger the attract for electrons
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Atomic Radius
Attraction falls off very rapidly with distance. An electron close to the nucleus will be much more strongly attracted than one further away
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As the number of electrons between the outer electrons & the nucleus increases the outer electrons feel less attraction towards the nuclear charge.Lessening the pull of the nucleus by inner shell electrons
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IE Down a Group
Decreases as its easier to lose electrons
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IE Across a Period
Increases as its harder to lose electrons
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Reactivity Increases Down Group 2
Due to increasing atomic radius & shielding affect
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Group 2 Element + Water
Forms a metal hydroxide and hydrogen
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Group 2 Element + Oxygen
Forms a solid white oxide
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Group 2 Element + Dilute Acid
Forms a salt & hydrogen
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Test For Carbonates
Add dilute acid. If present the carbon dioxide will be released, then do limewater test
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Test For Sulfates
Add dilute HCl, then barium chloride solution. If positive a white precipitate is formed
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Test For Halides
Add nitric acid, then silver nitrate solution. White precipitate if silver chloride, cream precipitate if silver bromide & yellow precipitate if silver iodine
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Test For Ammonium Compounds
Add sodium hydroxide & warm mixture. Use damp red litmus paper if positive it will turn blue
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Card 2




Döbereiner grouped similar elements called triads

Card 3




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Card 4




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Card 5


Modern Periodic Table


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