Bonding Flashcards
Define ionic bonding
Ionic bonding is the electrostatic attraction between oppositely-charged ions.
Give the 5 key compound ions you need to know.
Sulfate: SO4^2-
Carbonate: CO3^2-
Hydroxide: OH-
Nitrate: NO3-
Ammonium: NH4+
Define covalent bonding.
An electrostatic force of attraction between the nuclei and the shared pair of electrons.
Define a co-ordinate/ dative covalent bond.
A shared pair of electrons that came from one atom
Is there a difference in the chemical reaction of covalent and dative bonds?
No, a dative bond is treated as a standard covalent bond and reacts the exact same way.
Define metallic bonding.
The electrostatic attraction between a ‘sea’ of delocalised electrons and positive ions in a lattice.
What are trends in metallic bonding?
As the charge on the positive ion increases, the greater the metallic forces because of greater number of electrons.
As atomic radius of ions increase, the force of the metallic bonding.
What are the 4 types of crystal structures?
- Ionic
- Metallic
- Macromolecular
- Molecular
What is an example of an ionic crystal?
Sodium Chloride
What is the structure of an ionic crystal?
Ionic Lattice
Why do ionic crystals have a high melting/boiling point?
High mp/bp because the electrostatic forces between oppositely charged ions require a lot of energy to overcome.
Why can ionic crystals conduct electricity only when molten or as a liquid?
Cannot as a solid. When molten or as a liquid, can conduct electricity as ions are seperate and free to move and carry charge
What are 3 properties of ionic crystals?
- High melting/boiling point.
- Conducts electricity when molten/dissolved.
- Brittle
Why are ionic crystals brittle?
When a force is applied, distorting the layers of the lattice, like charges repel, breaking the crystal into fragments.
