Module 2 Recap Flashcards
Cations -
Positive ion
Anion -
Negative ion
Ionic Bonds:
- Formed between a metal and non-metal
- One atom loses electron(s) to the other.
Polyatomic ions:
A group of covalently bonded atoms that form a single ion.
Ionic Compounds:
- Formed from ions electrostatically held together.
- High melting and boiling points.
- Soluable in water.
- Conduct electricity when liquid or in a solution as the electrons are free to move.
- Form giant ionic lattices.
Covalent Compounds:
- Low melting and boiling points due to weaker intermolecular forces.
- Insoluable in water.
- Do not conduct electricity.
- Volatile.
- Lattice structure.
Metals and non-metals react to form __.
Ionic compounds.
Non-metals react to form _.
Covalent compounds.
Molecule:
A particle that consists of two or more atoms bonded together.
Compound:
A particle that consists of two or more DIFFERENT atoms bonded together.
- All compounds are molecules, but all molecules are not compounds for this reason.
Covalent bonds:
When two atoms share a pair of electrons to get a full outer shell.
Structure of Diamond:
Diamond is a giant covalent structure. It is formed from a repeating patter of a single carbon atom, bonded to 4 others. It has a tetraedral shape.
Structure of Graphite:
Graphite has a giant covalent structure. It is formed from hexagonal rings of 6 carbon atoms, that form layers. The layers are stacked ontop of each other and they can slide across each other, making graphite quite soft.
Metallic bonding:
The atoms are tightly packed together so to allow the valance electrons to delocalise. The bond is the electrostatic attraction between free electrons and posotive ions.
