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Chemistry Paper 1, - - Coggle Diagram

- - - - Periodic Group Properties
        
        Group 0 - Noble Gases -> unreactive / inert -> mpt and bpt goes up as you go down the column -> low density and inertness means they are used in airships , light bulbs and advertising signs.
        
        Group 1 - Alkali Metals -> more reactive as you go down the column -> mpt and bpt goes down as you go down the column -> low density - float on water and can burn with a purple flame. Form ionic compounds with the charge of +1. Form compounds of white solids and dissolve in water. Forms hydroxides (dissolve to form alkaline solutions) and hydrogen gas
        
        Group 7 - Halogens -> less reactive as you go down the column -> mpt and bpt goes up as you move down the column -> non-metals, diatomic. React with metals to form ionic compounds. React with non-metals to form covalent compounds. Form halides which dissolve in water to form acidic solutions
        
        Group 4 metals - Transition metals -> less reactive water and air. > high mpt -> dense, ions with different charges e.g. Fe 2+ and Fe 3+. Form coloured compounds Cr 3+ purple, Fe 2+ green, Co 2+ red, Ni 2+ dark green, Cu 2+ light blue
        
        History of the Atom
        
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- - - - Dimond lots of very strong covalent bonds.
        
        Each carbon is bonded with 4 others (carbon's valency is 4).
        
        It is therefore hard and has a very high melting point.
        
        Graphite – Each carbon forms bonds with 3 (1 is
        delocalised) others to make layers of hexagonal rings.
        
        The layers are able to slide over each other because there are weak intermolecular bonds.
        
        Therefore conducts and used as lubricants
        
        Nanoparticles
        
        Graphene – single layer of graphite (carbon) one atom thick.
        
        Uses:
        
        Deodorants and fabrics to prevent growth of bacteria
        
        Development of catalysts for fuel cell materials
        
        Cosmetics and sun creams
        
        Controlled drug delivery
        
        Electronics
        
        Synthetic skin
        
        Lubricants
        
        Fullerenes – made of carbon atoms but have a hollow shape.
        
        Based on hexagonal rings of carbon but can have rings made with other numbers of atoms.
        
        They have high tensile strength, conduct
        
        Used for drug delivery, lubricants, reinforcing materials eg tennis rackets
        
        Metallic structure
        
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        Advantages in sun cream:
        
        Better skin coverage
        
        More effective protection from UV rays
        
        Disadvantages in sun cream:
        
        Potential cell damage
        
        Potential harmful effects to the environment
- - - - Cells and batteries:
        
        Contain chemicals which produce electricity. A typical cell consists of two different materials in contact with an electrolyte
        
        Current flows from the more reactive to the less reactive metal. Eg Zinc to copper.
        
        The voltage produced depends on:
        
        The type of metal used as the electrodes
        
        The chemical used as the electrolyte
        
        In non-rechargeable cells and batteries, such as alkaline batteries when one of the reacts have been used up the chemical reactions stop and electricity is no longer produced.
        
        Fuel cells:
        
        Fuel cells differ from cells in that they are supplied by an external source of fuel, for example hydrogen and oxygen or air.
        
        The overall reaction in a hydrogen fuel cell involves the oxidation of hydrogen to produce water.
        
        2H2 (g) + O2 (g) 🡪 2H2O (l)
        
        These are environmentally friendly as water is the
        only waste product.
        
        These do not run out provided they are constantly
        supplied with fuel and oxygen.
        
        Equations to learn
        
        Mr = mass / moles
        
        Concentration = mass / volume
        
        % yield = (mass actually made / mass theoretically) x 100
        
        Atom economy = Mr of desired product / sum of Mr of all reactants
        
        Concentration of solution = moles of solute (mol) / vol of soln (dm3)
        
        Moles of gas = volume (dm3) / 24
        
        Titration
        
        Use the pipette and pipette filler to add a measured volume of sodium hydroxide solution to a clean conical flask.
        
        Add a few drops of indicator and put the conical flask on a white tile.
        
        Fill the burette with hydrochloric acid and note the starting volume.
        
        Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.
        
        Stop adding the acid when the end-point is reached (when the indicator first permanently changes colour). Note the final volume reading.
        
        Repeat steps 1 to 5 until concordant titres are obtained. More accurate results are obtained if acid is added drop by drop near to the end-point.