Chemistry

Chemistry

1. Chemistry 1a

   • Atoms
     • Atoms contain a nucleus and electrons which form the outer layers. They are used to stabilize the atoms by creating a full outer shell.
     • Atoms consist only of one type of atom. Its the number of protons that determine the type of atom that it is.
     • The number of protons is equal to the number of electrons. Protons are positive and Electrons are negative and they are equal to keep the Atom neutral and to make sure it stays stabilised
     • Atoms are represented by their atomic symbols
     • Electron Shells
       • Electron Shell Rules: 1) Electrons always occupy shells. 2) The lowest energy levels are always filled first. 3) Only a certain amount of electrons are allowed in each shell, 1st shell - 2, 2nd shell - 8, 3rd shell - 8. 4) Atoms are more stable when they have a full shell. 5) In most atoms the outer shell is not full and this makes the atom want to react to fill the outer shell and become stable.
       • The outer 6 electrons of an oxygen atom are stabilized by the outer 2 electrons of 2 hydrogen atoms to create a fully stabilized H20 atom
       • Covalent Bonds
         • A compound formed of non metals each atom shares an electron with another atom which is called a covalent bond. Each atom has to make enough covalent bonds to fill up its outer shell.
       • Ionic Bonds
         • A compound which is formed of Metals and Non Metals consists of Ions. The metal atoms lose electrons to form positive ions and the non metals gain electrons to form negative ions. The opposite charges of positive and negative mean that they are strongly attracted to each other.
         • Balancing Equations
           • Equations that have an equal number of electrons on each side are balanced and therefore correct.
           • Atoms in chemical reactions are not lost or made and all inputs in an equation must be present in the outputs
   • Limestone
     • Limestone is mainly Calcium Carbonate
       • When Calcium Carbonate is heated it thermally decomposes into Calcium Oxide + Carbon Dioxide. Carbon dioxide is produced in the process of thermal decomposition with carbonates so when Magnesium carbonate is heated Magnesium oxide and carbon dioxide will be produced.
         • Calcium Carbonate also reacts with acid to make Calcium Salt, Carbon Dioxide and water
   • Extracting Metals
     • Getting Metals from Rocks
       • Some metals are extracted from rocks using displacement reactions that use more reactive metals to displace less reactive metals in a solution.
       • Some metals that are highly reactive ,and cannot be cheaply extracted using a displacement reaction with carbon, are extracted by the process of Electrolysis
     • Electrolysis
       • Electrolysis is the process of breaking down metals with electricity
       • This requires a liquid to conduct the electricity, called an Electrolyte.
         • Electrolytes are often metal salt solutions made from the ore being extracted or molten metal oxides.
       • The Electrolyte has free ions and these conduct electricity to make the whole process to work

2. Chemistry 1b

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