1What are ionic bonds?
electrostatic attraction between two oppositely charged ions; they’re formed as a result of a metal atom transferring electrons to a non-metal atom, which forms cations (positively charged) and anions (negatively charged)
2What are the properties of ionic compounds?
High melting and boiling points due to the strong electrostatic forces between ions and soluble in water
3Why can ionic compounds carry a charge in liquid or molten form, but not as a solid?
in a solid, the ions can’t flow and don’t carry a charge; the opposite is true in liquid form
4What are covalent bonds?
bonds between atoms that are formed when electrons are shared to achieve a full outer shell
5What are examples of covalent structures?
Graphite and diamond
6What are the properties of covalent structures?
Simple covalent: unconductive and have low melting points due to weak forces of attraction
Giant covalent: high melting points due to strong covalent bonds and mostly unconductive
7What the properties of diamond?
high melting and boiling points, hard and poor conductor due to not having any delocalised electrons in the structure
8What are the properties of graphite?
high melting and boiling points, soft and good conductor due to having delocalised electrons in the structure
9What is diamond used in?
machinery
10What is graphite used in?
pencils and as a lubricant in engines due to the layers being able to slide over each other
11What other structures have the same properties as graphite?
Graphene and fullerenes
12How big is a nanometre?
1 x 10*-9
13What are the uses for nanoparticles?
used in sunscreams, tennis balls and anti-bacterial socks