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From Standard Grade

From Standard Grade. I f we exclude the metal elements. There are two types of bonding. Ionic. Covalent. Covalent molecular. Covalent Network. Covalent is divided into two parts. Covalent Molecular. In covalent molecular bonding the atoms are joined into discrete molecules.

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From Standard Grade

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  1. From Standard Grade If we exclude the metal elements There are two types of bonding Ionic Covalent Covalent molecular Covalent Network Covalent is divided into two parts

  2. Covalent Molecular In covalent molecular bonding the atoms are joined into discrete molecules The molecules can be represented by simple formula Eg. CH4 C6H12O6 C33H68C60 Covalent molecular compounds tend to be gases, Liquids or low melting point solids Covalent molecular solids do not conduct electricity

  3. Covalent Network Structure In a covalent network the atoms are all joined in one large 3-dimensional structure This type of bonding is rare, examples are Carbon as diamond Carbon as graphite Silicon dioxide Silicon All substances with covalent network bonding have extremely high melting points The only covalent network solid to conduct is graphite (it can conduct because it contains delocalised electrons)

  4. - + + - + - - + Ionic compounds Ionic compound tend to be formed when metals bond to non-metals The ions formed join together to form a 3-dimensional crystal lattice The ions are tightly held together and for this reason ionic compounds do not conduct electricity as solids

  5. - + + + - + - + - + - + - - + - When melted (or dissolved) the crystal lattice is broken and the ions are free to move The ionic compound can now conduct electricity As ionic bond are strong ionic compounds are high melting point solids

  6. + + + + + + + + + + + + + + + e- e- e- e- e- e- e- e- e- e- e- e- Metallic Bonding This is the type of bonding found in metals Positive ions are surrounded by delocalised electrons It is these delocalised electrons which allow metals to conduct as solids The larger the positive charge the more delocalised electrons, which gives a stronger metallic bond

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