Bonding Flashcards
(12 cards)
What is an Ionic bond?
An ionic bond is the electrostatic force of attraction between oppositely charged particles. These bonds are formed when elements loose or gain electrons to achieve a full outer shell.
Properties of ionic compounds:
High melting and boiling point (because of the strong electrostatic bonds which require a lot of energy to break)
Can conduct electricity when molten or dissolved in a liquid (because when they are in a liquid form the delocalised electrons are now free to move and carry electric charge and around the structure)
What are covalent bonds?
When non-metal atoms share pairs of electrons, covalent bonds are formed. Non-metals share electrons to get a full outer shell.
Properties of covalent compounds:
Low boiling and melting point (because they have weak intermolecular bonds which don’t require a lot of energy to break)
Molecular structure cannot conduct electricity (because the molecules are neutral so there are no electrons to carry charge)
Properties of metals
Have high melting and boiling points (because the strong electrostatic attraction between positive ions and delocalised electrons form these strong metallic bonds which require a lot of energy to break)
Can conduct heat (because delocalised electrons can carry thermal energy through the structure)
Can conduct electricity (because delocalised electrons can carry electrical charge through the metal)
Malleable (can be hammered into shape) and ductile (can be stretched into wires)- because the ions are arranged in layers meaning they can easily slide over each other.
Why are alloys harder than pure metals?
Because alloys contain atoms of different sizes. The bigger atoms disrupt the layers meaning more energy is needed for these layers to slide over each other.
Name diamonds properties
Doesn’t conduct electricity because there are no free moving electrons. All four are used in bonding.
High melting and boiling point because it has strong covalent bonds meaning it requires a lot of energy to break
Hard substance because the carbons are arranged in a giant lattice with strong covalent bonds between the atoms
Properties of Graphite
Soft substance because it consists of layers that can slide over each other easily
Conducts electricity because it has delocalised electrons to carry electrical charge
Each carbon is bonded to three other carbon atoms meaning only 3/4 of atoms are used so last one is delocalised electron.
Properties of Graphene
Hard to melt because of strong covalent bonds- each carbon atom is covalently bonded to 3 other atoms
Conducts electricity
Graphene is hard because it has a giant lattice with strong covalent bonds which require a lot of energy to break.
Uses of Graphene
Shoes- Shoes use Graphene because they are flexible and strong
Electronics- Thin, strong, flexible
Explain why metals can be bent and shaped:
Because their ions are arranged in layers and can easily slide over each other.
What is metallic bonding?
The strong electrostatic attraction between positive metal ions and the delocalized electrons
