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C2 End of Year 10 - Coggle Diagram
C2 End of Year 10
C1 Content
The Noble Gasses (Group 0) are extremely unreactive because they all have a full outer shell of 8 electrons(excluding helium which has 2). The boiling points of the noble gasses increase as their atomic number does (down the group).
The Alkali metals (Group 1) are soft metals with low boiling points. The reactivity of group one metals increases down the group. At room temperature, oxygen reacts with these metals, forming a white oxide on the metals surface; when heated and placed in a jar of oxygen, these metals react vigorously and the oxide appears as a white smoke.
The group one metals react vigorously with chlorine, producing chlorides; in the form of white solids at room temperature. The chlorides dissolve in water to form colourless solutions.
When group one metals react with water, a hydrogen gas and a metal hydroxide are produced; the violence of these reactions increases as you move down the group.
When lithium reacts with water, it floats and steadily fizzes, eventually disappearing.
When sodium reacts with water, it forms a ball that floats on the surface, fizzing rapidly. Additionally, the hydrogen gas produced may burn with an orange flame before the sodium disappears,
When potassium is added to water, it melts and then floats on the surface, it moves very quickly while around the water's surface. The hydrogen produced ignites instantly, with the metal also setting on fire and producing sparks and a lilac flame. There is sometimes a small explosion at the end of the reaction.
The halogens (Group 7) are non metals and the elements within occur in diatomic molecules. They react with metals to produce salts. They become less reactive as you move down the group. They also react with hydrogen to produce hydrogen halides, these are gasses at room temperature and can dissolve in water to produce acidic solutions.
Dobereiner: Placed elements in group of 3, every third element shared similar properties.
Newland: Octave placement, every other 8th element was similar.
Mendeleev: Arranged elements by atomic mass, left gaps for undiscovered elements, predicted properties were proved true.
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L8 - Fullerenes
A fullerene is an allotrope (different structural form) of carbon, usually formed from graphene.
Graphene is a single layer of graphite, this means that graphene is not soft or slippery because it has no layers on which to slide on; it still, however, possesses free, delocalised electrons.
Carbon nanotubes are a cylindrical form of graphene. They are able to conduct electricity, are incredibly strong(tensile strength) and (like all fullerenes) have a very large surface area to volume ratio. These nanotubes can be used in the production of electronics and also in the strengthening of such products as tennis racket frames.
Buckminsterfullerene is an altered form of graphene with a very large surface area to volume ratio, they can be used to deliver drugs within the body because of their hollow shape; they can also be used as catalysts (speed up reactions). Additionally, they are able to roll because of their spherical shape(used in lubricants).
L10 - Nanoparticles
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Nanoparticles can be used as catalysts, in electronics and in medicine (in the form of buckminsterfullerene for example). Additionally, we can use silver nanoparticles for their antibacterial properties.
There are disadvantages to nanoparticles however: they are a relatively new advancement so the effects that they may have on our bodies are not yet fully understood. Some argue that products such as suncream should be labelled indicating that they contain nanoparticles. Some speculate that these particles could also damage the environment.
L1 - States of Matter
3 states of matter are gas, liquid and solid. Within gasses, particles are far apart (bonds are broken) and the particles move in random directions at random speeds; they can be compressed and move to fill the container they are in.
Within liquids, bonds are relatively weak and the particles within are free to flow and take the shape of the container they are in, they cannot be compressed.
Solids contain particles that are uniformed, reside in fixed positions and vibrate in those positions, they do not move to fill the container they are in and cannot be easily compressed.
L4 - Ionic Compounds
Ionic compounds are structured in giant ionic lattices, within these lattices, all ions within possess strong electrostatic attraction to the oppositely charged ions within the lattice. This, henceforth, means that these lattices have an extremely high melting and boiling point because of the strong ionic bonds.
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Ionic compounds do not conduct electricity when solid because all ions are held in place firmly, however they are free to move if the compound is molten or aqueous, meaning they can conduct electricity in this state.
L9 - Metallic Bonding
Metallic bonding occurs between metal atoms and delocalised electrons. The electrostatic attraction itself occurs between positive metal ions and the a "sea" of negatively charged electrons. This holds all the atoms together in a uniform, regular structure.
These bonds require a large amount of energy to overcome. Additionally, delocalised electrons allow the metallic substance to conduct electricity. These pure metals are maleable (layers can slide).
Alloys contain two or more different elements, they disrupt the homogeneous arrangement of pure metals, meaning that their layers cannot slide.
L3 - Ionic Bonds
Ionic bonds form between metals and non-metals. It is caused by the transferal of electrons from one element to another. Metals always form positive ions, non-metals form negatively charged ions. Attraction between these differing charges is known as electrostatic attraction.
When drawing dot and cross diagrams, one of the elements (typically the metal) will have their electrons depicted as dots while the other will have their electrons depicted as crosses. Usually only the outermost energy level is drawn. Square parenthesis are used to indicate the overall charge of each ion.
L6 - Polymers
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Because polymer chains are so long, they have a very large surface area and many intermolecular forces, this means that these polymers will be solid at room temperature. The M.P and B.P of polymers is lesser than that of ionic or giant covalent structures, although they are greater than that of simple covalent structures.
L5 - Covalent Bonds
When two non-metals share electrons, they form a covalent bond; these bonds are strong (strong intramolecular forces). These bonds are held together via the attraction of one atom's electron(s) to another's nucleus and vice-versa. Atoms bonded covalent-ly form molecules, the attraction between these compounds is relatively weak(intermolecular forces).