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The Periodic Table - Coggle Diagram

- - - - They are good conductors of heat and electricity
      - But they are softer than most other metals, you can cut them with a knife.
      - They are lighter than most other metals, they have low density. So due to this, the elements can float on water, while reacting with it.
      - Have low melting and boiling points.
    - - We can´t see the table very clear but, as you go down there is a kind of increase or decrease for each property, doing a pattern that is called a trend.
    - - Comparing the reactions of lithium, sodium, and potassium.
        
        Reaction with water:
        
        There is a trend in reactivity, for sodium the reaction is: sodium+water ---->sodium hydroxide+hydrogen
        
        They three reacted violently with water, giving hydrogen and a hydroxide.
        
        The alkali metals react vigorously with water. Hydrogen bubbles off, leaving solutions of their hydroxides, which are alkalis.
        
        Reaction with Chlorine:
        
        If you heat the three metals, and plunge them into gas jars of chlorine they burst into flame. Burning, forming chlorides. Example: sodium+chlorine ----> sodium chloride
        
        Reaction with oxygen:
        
        When you heat them and plunge them into gas jars of oxygen, the three metals also burst into flame. Forming oxides, that dissolve in water to give alkaline solutions.
        
        In all three reactions the trend is clearly shown. Lithium is the least reactive and potassium is the most reactive of the three elements.
    - - Because they have the same number of valency electrons. (outer-shell electrons)
    - - Alkali metals are the most reactive.
      - Because they need to lose only one electron, to gain stability in the outer shell.
      - The alkali metals form ionic compounds, in which the metal ion has a charge of 1+.
      - Example: sodium chloride is made up of the ions Na+ and Cl-.
      - Have a strong drive to react with other compounds and elements, becoming ions.
      - Compounds are white solids, they dissolve in water to give colourless solutions.
  - - - Form coloured gases.
      - are poisononous
      - Form diatomic molecules. (containing two atoms) Example: CL2
    - - They are shown in the table. (unfortunaly we cant see clearly)
    - - The halogens are among the most reactive elements.
      - They react with metals to form compounds called halides, the example is in the following table.
      - Reactivity decreases as you go down Group VII.
    - - Because their atoms have 7 valency (outer-shell) electrons. Example below: Fluorine and chlorine.
      - Atoms with the same number of valency electrons react in a similar way.
    - - Because they only need one more electron to reach a stable outer shell of 8 electrons, so they have a strong drive to react with other elements or compounds.
      - When they react with metal atoms, halogen atoms accept electrons, forming halide ions.
        
        For example: reaction between iron + chlorine gives iron (III) chloride, made up of Fe3+ and Cl- ions.
      - With non-metal atoms like hydrogen and carbon, they share electrons, forming molecules with covalent bonds.
    - - For example: When chlorine water is added to a colourless solution of potassium bromide, the solution turns orange.
        
        Cl2 (aq) + 2KBr (aq) colourless ----> 2KCl (aq) + Br2 (aq) orange
      - A halogen will displace a less reactive halogen from a solution of its halide.
  - - - Non-metals
      - Courless gases
      - Monatomic (they exist as single atoms)
      - Unreactive
    - - Because the atoms of the noble gases already have a stable outer shell with 8 electrons, except for helium that has 2.
      - The atoms have no need to react in order to gain or lose electrons.
    - - The gases grow denser or heavier down the group, because the mass of the atom increases.
    - - The noble gases are unreactive or inert, which makes them safe tu use.
        
        Helium is used to fill baloons and airships
        
        Argon is used to provide an inert atmosphere.
        
        Neon is used in adversing signs.
        
        Krypton is used in lasers.
        
        Xenon is used in lighthouse lamps, light for hospital operating rooms, and car headlamps.
- - - - The zig-zag line divides the periodic table.
        
        The metals are to the left.
      - Over 80% of the elements are metals.
      - They have very different properties.
    - - Sits alone.
        
        Because it has an outer electron, and forms a positive ion. (H+)
      - It is a gas and usually reacts like a non-metal.
- - - - Block of 30 elements, that are metals, in the middle of the Periodic Table.
    - - Hard, tought and strong.
      - High melting points.
        
        But mercury is an exception, it is a liquid at room temperature.
      - Malleable (can be hammered into different shapes) and ductile (can be drawn out in wires).
      - Good conductures of heat and electricity.
        
        Silver is the best, copper is next.
      - High density. (heavy)
    - - They are much less reactive than the Group I metals.
        
        Transition elements do not corrode easily in the atmosphere. (iron being the exception)
      - They show no clear trend in reactivity, unlike the Group I metals.
      - 3: Most transition elements form coloured compounds.
      - Most can form ions with different charges.
        
        In this chart this elements show variable valency.
      - They can form more than one compound with another element.
        
        Because of variable valency.
        
        Example: copper(I) oxide, Cu2O
        
        Roman numeral in brackets tells you how many electrons the metal atom has lost, it is called its oxidation state.
      - Most transition elements can form complex ions.
    - - Structures such as bridges, buildings and cars. (Iron is the most widely used, usually in the form of alloys, called steels.)
      - In making alloys. Example: Chrominium+Nickel are mixed with Iron to make stainless steel.
      - As conductures of heat and electricity.
      - Some and their compounds act as catalysts.
        
        Speed up reactions, while remaining without changes.
- - - - Elements show periodicity
        
        Elements with similar properties appear at regular intervals.
      - Similar elements are arranged in columns.