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Bonding - Coggle Diagram

- - - - car engines
    - - space rockets
  - - - uranium-235
- - - - 6.02X10^23 atoms in 1 mole
    - - 1 mole of every gas is 24dm^3 at rtp(20 celsius and 1 atm)
- - - - Electrons TRANSFERRED between atoms
      - Usually for metal and non-metal bonds. Metals donate and non-metals accept electrons.
      - Lattice shape
      - Diagram
      - Transition metal ions
        
        Based on oxidation state
        
        EXCEPT Zinc(Zn2+) and Silver(Ag+)
      - Compound ions
      - Properties
        
        High mp and bp. because Ionic bonds are very strong, and require lots of heat energy to overcome.
        
        Soluble in water. Water molecules are able to seperate ions and undergo ion-dipole force.
        
        Conduct electricity when dissolved of molten. Because ions are free to move.
    - - Giant covalent
        
        Diamond
        
        Very hard, held by 4 covaelnt bonds
        
        High mp and bp
        
        Cant conduct electricity
        
        Continuation of covalent bond many many times.
        
        Silica(SiO2)
        
        Quartz. main mineral in sand
        
        Very ahrd and high mp
        
        Graphite
        
        Soft and slippery. Sheets can slide over each other
        
        Conducts electricty.4th electron free to move about.
        
        uses
      - Atoms SHARE electrons
      - Usually for non-metal and non-metal bonding.
      - Diagram
      - Repulsion between electrons dictates shape of molecule
      - Properties
        
        low mp and bp. Because attration between molecules is low, requires lesser heat energy to overcome. many liquids are volatile.
        
        Insoluble in water
        
        Do not conduct electricity
    - - Metal ions surrounded by sea of electrons
      - Electrons are delocalised from atoms
      - Properties
        
        Usually high mp and bp. Requires a lot of heat energy to break metallic bonds
        
        Malleable and ductile. Because Layers can slide to form shapes.
        
        Good conductors of heat and electricity. Deloclised electrons carry charge and heat throughout the metal.
      - Diagram
    - - Van der waals forces. When atoms may become asymmetrical and become polar for a moment in time.
  - - - average mass of isotopes compared with carbon-12 atom
      - Isotopes; same proton number but different neutron number
        
        Same chemical rpoperties(because electrons number dont change), different phycial properties(because neutrons increase and cause change in mass, density, etc.)
    - - Elements always react in the same ratio to produce a compound
      - Total mass does not change during chemical reaction.
- - - - Higher temperature, favour endothermic reaction
    - - Higher pressure favours fewer moles
    - - Cause shift in amount
    - - Equilibrium achieves at a faster rate, but no shidt in equilibrium
- - - - neutralisation by alkalis
      - combustion of fuels
      - respiration
    - - Energy to break - energy to make = -ve
  - - - Thermal decomposition
      - Cooking
      - Photosynthesis
    - - Energy to break - energy to make = +ve
- - - - When product is gas
        
        Amount of product per unit time
        
        Mass loss per unit time
      - When got colour change
    - - Concentration
        
        Higher concentration, higher rate of reaction.
        
        Increased number of reactant particles to collide
      - Temperature
        
        Higher temperature, higher rate of reaction
        
        Increased movement of particles, increased collisions
      - Surface Area
        
        higher surface area exposed, higher rate of reaction
        
        Increased atoms exposed to reactant, increased collisions
      - Catalyst
        
        Substance that speeds up chemical reaction but not used and and remains unchanged.
        
        usually transition elements or their oxides
        
        lowers activation energy, increases number of collisions
        
        Biological catalysts = enzymes
        
        More catalyst, increased rate of reaction
      - Pressure(gas)
        
        Higher pressure, higher rate of reaction
        
        Decreased space, increased concentration and increased collisions
    - - Particles must collide
      - needs enough activation energy to break bonds for reaction to be successful