Bonding & Intermolecular Forces Series - Covalent Bonding Mindmap
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?- Created by: Tommy1boy
- Created on: 15-02-16 11:50
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- Covalent Bonding
- Molecules form when two or more atoms bond together
- They can be the same or different atoms
- Covalent Bonds can be single, double or triple bonds
- They can be the same or different atoms
- Example
- Water
- Carbon Dioxide
- Nitrogen
- Simple Covalent Compounds
- Compounds that are made up of lots of individual molecules are called simple covalent compounds.
- Atoms in the molecules are held together by strong covalent bonds
- But the molecules within the compound are held together by much weaker forces called intermolecular forces.
- It is these intermolecular forces that determine the properties of a simple covalent compound.
- But the molecules within the compound are held together by much weaker forces called intermolecular forces.
- Atoms in the molecules are held together by strong covalent bonds
- Compounds that are made up of lots of individual molecules are called simple covalent compounds.
- Giant Covalent Compounds
- Giant covalent structures are a type of crystal strucure
- Graphite
- The carbon atoms in graphite are arranged in sheets of flat hexagons with three bonds each.
- The fourth outer election of each carbon atom is delocalised
- The sheets are held together by weak can der Walls forces (type of intermolecular force)
- Properties of Graphite
- The weak forces between the layers are easily broken so the sheets can slide over each other. Graphite feels slippery and is used as a dry lubricant in pencils
- The delocalised electrons in graphite are free to move along the sheets so an electric current can flow
- The layers are quite far apart compared to the length of the covalent bonds, so graphite has a low density and is used to make strong lightweight sports equipment
- Because of the strong covalent bonds in the sheets, graphite has a high melting point. The strong bonds also means it is insoluble in any solvent
- Diamond
- Diamond is made up of carbon atoms which are covalently bonded to four other carbon atoms
- This creates a tetrahedral shape. It has a crystal lattice structure
- Properties of Diamond. Because of its strong covalent bonds:
- Diamond has a very high melting point
- Diamond is extremely hard. It is used in diamond-tipped drills and saws
- Vibrations tavel easily through the stiff lattices, so it is a good thermal conductor
- It cannot conduct electricity. All the outer electrons are held in localised bonds.
- Diamond will not dissolve in any substance
- Diamond is made up of carbon atoms which are covalently bonded to four other carbon atoms
- Graphite
- They are sometimes referred to as macro-molecular structures
- Giant covalent structures are a type of crystal strucure
- Co-ordinate bonds (Dative Covalent bonds)
- In a dative covalent bond, one of the atoms provides both of the shared electrions
- These form when one of the atoms in the bond has a lone pair of electrons and the other does not have any electrons available to share
- Example - Hydroxonium Ion
- Molecules form when two or more atoms bond together
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