Atoms combining

Describe the formation of ions by electron loss or gain
1. If an atom contains more electrons than protons the atom has a negative charge. If the atom contains fewer electrons than the protons the atom has a positive charge. Ions are a group of atoms that carry a positive or negative charge.
Describe the formation of ionic bonds between elements from Groups I and VII
Explain the formation of ionic bonds between metallic and non-metallic elements
1. Ionic bonds are the bonds that form between opposite charges. A metal reacts with non-metal to form an ionic-compound.The metal ions lose electron. The non-metal gain them. The ions form a lattice. The compound has no over all charge.
State that non-metallic elements form non-ionic compounds using a different type of bonding called covalent bonding
1. Same nuclei attract the shared electrons -this a strong force of attraction hold the 2 atoms together. The force of attraction is called covalent bonds.
Draw dot and cross diagrams to represent the sharing of electron pairs to form single covalent bonds
1. Single bonds
Draw dot and cross diagrams to represent the multiple bonding
Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds
1. Volatility
  1. Ionic bonds have high melting and boiling points.
  2. Covalent bonds have low melting and boiling points.
2. Solubility
  1. Ionic bonds tend to be soluble in water.
  2. Covalent bonds tend to be insoluble.
3. Electrical Conductivity
  1. Ionic bonds conduct electricity when melted or dissolved in water.
  2. Covalent bonds do not conduct electricity.
Describe the giant covalent structures of graphite and diamond
1. Graphite
  1. ~Each carbon attached to three other carbon atoms ~Hexagonal ring layered lattice structure ~Delocalised electrons within each layer ~Weak intermolecular forces between the layers.
2. Daimond
  1. ~Each carbon forms four covalent bonds with other carbon atoms ~Each carbon has a tetrahedral arrangement ~All electrons are localised in covalent bonds.
Relate their structures to the use of graphite as a lubricant and of diamond in cutting
1. DIamond
  1. ~Each atom is held place by 4 strong covalent bonds. It has a high melting point.It also cannot conduct electricity.
2. Graphite
  1. ~Each atom is held in place by 3 strong covalent bonds. It has a low melting points. It also can conduct electricity.
Describe the structure of silicon(IV) oxide (silicon dioxide)
1. Silicon is similar to diamond. Each silicon atom bonds covalently with 4 oxygen atoms. Each oxygen atoms bonds covalently with 4 silicon atoms and the result is a very hard matarial with a high melting point.

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Atoms combining

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