Structure and bonding YEAR 10 Flashcards
Define ionic bonds
Electrostatic attraction between oppositely charged ions
Define Metallic bonds in terms of atomic structure
Electrostatic attraction between positive ions and delocalised electrons
Define intermolecular forces in terms of structure
Weak attraction between separate molecules
Ionic and metallic bonds are simple or giant?
GIANT
Why are ionic compound brittle
If ions shift and same charge ions are pushed together, they repel one another
Why are ionic compounds only conductors when molten or aqueous
This frees their ions allowing them to conduct electricity
Diamond is a _______ structure
Giant covalent
Why is diamond so strong
Each carbon atom is in 4 covalent bonds.
It is a giant covalent structure
Graphite is a ______ structure
Giant covalent
Why is graphite soft
Atoms are arranged in layers called graphene, which are only bonded with weak intermolecular forces
Why do ionic compounds have a high boiling point
Strong electrostatic attraction between ions
Why do covalent compounds have low melting points
the intermolecular forces of attraction between molecules are weak and easy to overcome.
Why is graphite used for electrodes
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct
What are fullerenes
Fullerenes are molecules. of carbon atoms with hollow shapes.
Cons of ball and stick diagrams
Don’t show movement of electrons
