Ionic Bonding
- Created by: Ella Clark
- Created on: 02-01-13 13:46
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- Ionic Bonding
- Ionic Bonds
- Electrons are transferred from the metal atom to the non-metal atom
- An ionic bond is the electrostatic attraction between oppositely charged ions
- The metal ion = +ve, the non-metal ion = -ve
- E.g. Ionic bonding in sodium chloride, Na2O
- The compound is formed from the +ve sodium atoms and the -ve oxygen atom
- An Na atom has 1 e- in it's outer shell
- One e- is transferred:
- From each of the two sodium atoms
- to one oxygen atom
- With the formation of two Na+ ions and one O2- ion
- One e- is transferred:
- An O atom has 6 e- atoms in its outer shell
- One e- is transferred:
- From each of the two sodium atoms
- to one oxygen atom
- With the formation of two Na+ ions and one O2- ion
- One e- is transferred:
- An Na atom has 1 e- in it's outer shell
- The compound is formed from the +ve sodium atoms and the -ve oxygen atom
- Giant Ionic Lattices
- A giant iconic lattice is a three-dimensional structure of oppositely charged ions, held together by strong ionic bonds.
- All ionic compounds exist as giant atomic lattices in their solid state
- Each ion attracts oppositely charged ions from all directions
- Each ion is surrounded by oppositely charged ions
- Properties of Ionic Compounds
- High melting and boiling points
- Ionic compounds are solid at room temp.
- Therefore a large amount of energy is needed to break the strong electrostatic forces that hold the oppositely charged ions together in the solid ionic lattic.
- Ionic compounds are solid at room temp.
- Electrical conductivity
- In a solid ionic lattice:
- The ions are in a fixed position and no ions can move
- The ionic compound is a non-conductor of electricity
- When an ionic compound is melted or dissolved in water:
- The solid lattice breaks down and the ions are free to move
- The solid compound is now a conductor of electricity
- In a solid ionic lattice:
- Solubility
- The ionic lattice dissolves in polar solvents, such as water
- The polar water molecules break down the lattice surrounding each ion to form a solution.
- E.g. When NaCl is dissolved in water, the giant ionic lattice breaks down
- Water molecules attract Na+ and Cl- ions, the ionic lattice breaks down as it dissolves. water molecules surround the ions.
- Na+ attracts (delta-) charges on the O atoms of the water molecules and Cl- attracts (delta+) charges on the H atoms of the water molecules
- Water molecules attract Na+ and Cl- ions, the ionic lattice breaks down as it dissolves. water molecules surround the ions.
- The ionic lattice dissolves in polar solvents, such as water
- High melting and boiling points
- Ionic Bonds
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