C3 Structure And Bonding Flashcards
Covalent bonding
Electrostatic attraction between a shared pair of electrons and the nuclei of two atoms
Ionic bonding
Electrostatic attraction between oppositely charged ions
Atoms are transferred.
A giant lattice/structure is a result of
The ionic bonds between the charged particles
Ionic compound/lattice properties (solid)
High melting/boiling point as heat has to overcome all the electrostatic forces of attraction
Not a conductor because its ions are held in fixed positions in the lattice
Molten Ionic lattice properties
High temp provides enough energy to overcome the many strong attractive forces between ions. Ions are feee to move around in the molten compound making it a conductor
Ionic compound in solution
Water molecules seperate ions from the lattice. Ions are free to move around within the solution.
It does conduct elecrticity.
Metalic bonds
Electrostatic attraction between delocalised outer shell electrons and metal ions
Giant structures
All solids at room temperature
High melting points beacuse lots of energy is required to break many strong bonds
Simple molecular/monatomic properties
‘Soft’ soldis, liquids or gases at room temperature (25°C) with Low melting points and boiling points as not much energy is required to break weak intermolecular forces between molecules.
What are the properties of giant covalent structures ?
High mp and bp
They are insoluable in water
They are hard and don’t conduct electricity (except graphite)
Why does graphite conduct electricity ?
The delocalised electrons which can move freely through its structure.
Carbon atoms have 4 electrons for bonding in there outer shell, graphite only uses three bonds due to its hexagonal shape. This leaves one spare outer electron.
Why is graphite soft ?
There are no covalent bonds between layers, only weak intermolecular forces.
What are intermolecular forces
Forces between sperate molecules that hold the substance together.
