Structure And Bonding Flashcards
Ionic bonding occurs between
A metal and a non-metal
Ionic compounds have a
Giant lattice structure of alternating positive and negative ions
They have high melting points because
Al large amount of energy is needed to break the strong electrostatic attraction between oppositely charged ions
They cannot conduct as a solid because
The ions are fixed in place in a rigid lattice and cannot move
They can conduct as a solution/molten because
The ions are free to move and carry charge
A covalent bond is
A shared pair of electrons
Covalent bonding occurs between
Non-metal atoms
Covalent compounds cannot conduct electricity because
They have no delocalised electrons/ ions to carry a charge
Giant covalent structures have high melting points because
A large amount of energy is needed to break all the strong covalent bonds between atoms
Simple molecular compounds have low melting points because
A small amount of energy is needed to overcome the weak intermolecular forces
Graphite can conduct electricity because
Each carbon atom only used 3 of its electrons in bonding which means the remaining electrons are delocalised between layers of carbon atoms
Covalent bonds can have either
A simple molecular structure or a giant structure
Metallic bonding is
An electrostatic attraction between positive metal ions and a surrounding sea of delocalised electrons
Metals have high melting points because
A large amount of energy is needed to break the strong electrostatic attraction between positive ions and delocalised electrons
Metals have a giant structure consisting of
Layers of positive metal ions and a sea of delocalised electrons
