Chemistry (ionic Bonding) Flashcards
Ionic bonding-
When a metal and a non-metal react together, the metal atom loses electrons to form a positive ion and the non-metal gains these electrons to form a negative ion. These oppositely charged ions are strongly attracted to one another by electrostatic forces.
Ionic compounds have a regular lattice structure
Ionic compounds always have giant ionic lattice structures. The ions form a closely packed regular lattice. These are very strong electrostatic forces of attraction between oppositely charged ions, in all directions.
Covalent bonds-
A covalent bond is a strong bond that forms when a pair of electrons is shared between two atoms. Simple molecular substances are made up of molecules containing a few atoms joined by covalent bonds.
Giant covalent structures-
- In giant covalent structures, all the atoms are bonded to each other by strong covalent bonds.
- They have a very high melting and boiling points as lots of energy is needed to break the covalent bonds.
- They generally don’t contain charged particles, so they don’t conduct electricity.
- They aren’t soluble in water.
- The following examples are all carbon-based giant covalent structures.
Electrical conductivity-
Ionic compounds conduct electricity when they are molten or dissolved in water. They do not conduct electricity when they are in the solid state.
Intermolecular forces-
Weak forces of attraction between molecules.
Polymers
Monomers are small, simple molecules that can be joined in a chain to form a polymer.
Allotropes-
Different structural forms of the same element
Metallic bonding-
Is the electrostatic attraction between the positive metal ions and the negative delocalised electrons.
Ionic properties:
High melting/boiling points
Many are soluble in water
Conduct electricity when liquid or in solution but do not when solid.
Simple molecular (covalent) properties:
Low melting/boiling points
A few are soluble in water
Most do not conduct electricity
Giant covalent properties
High melting/boiling points
Insoluble in water
Most do not conduct electricity (except in carbon as graphite)
Metallic properties:
High melting/boiling points
Insoluble in water
Conduct electricity when solid or liquid.