2 - Test: Bonding, Structure, Seperation, Testing Flashcards
What do compounds with ionic bonding always form?
A lattice structure.
Ionic compounds’ melting points are…
High - lots of thermal energy required to break strong electrostatic bonds.
Do Ionic compounds conduct electricity?
No when solid.
Yes when melted or dissolved in water.
Ionic bonding is the…
Transfer of electrons.
Covalent bonding is the…
Share of electrons.
Giant Covalent compounds’ melting points are…
High - lots of thermal energy required to break strong covalent bonds.
Simple Covalent compounds’ melting points are…
Low - weak intermolecular forces of attraction - not much energy required to break.
Does Diamond conduct electricity?
No - no free delocalised electrons because all 4 carbon-carbon bonds are in use.
What is diamond’s physical state and why?
Hard - rigid lattice structure.
Does Graphite conduct electricity?
Yes - one free delocalised electrons since only 3 out of 4 carbon- carbon bonds in use.
What is Graphite’s physical state and why?
Soft and slippery because layers are free to slide.
Do Fullerenes have a high melting point?
Yes - strong covalent bonds.
What is C-60’s physical state and why?
Weak intermolecular forces so can slide and move around.
Does C-60 conduct electricity?
Yes but is a poor conductor because the free electron can’t move that much.
What is metallic bonding?
Electrostatic attraction between positive ions and delocalised electrons.
Are metals a good conductor of electricity?
Yes - delocalised electrons.
Why are metals malleable?
Have layers that can slide.
Cations
Positive ions
