C3 Structure And Bonding Flashcards
How do particles move in a substance in the solid state
They vibrate in place
Why can a liquid flow
The particles can slide over each other
Why can a gas be compressed
There is a lot of space between the gas molecules
Why is energy transferred from the substance to the surroundings when a substance freezes
Bonds between atoms get stronger
How do metal atoms form ions
Metals loose electrons
What type of forces hold an ionic lattice together
Electrostatic
Why do ionic compounds have higher melting and boiling points
As a lot of heat energy is needed to break the strong electrostatic forces between oppositely charged ions
When can a ionic compound conduct electricity and why
When they’re molten or liquid or dissolved in a solution . This is Becuase the ions are free to move around in order to carry a charge
What is a covalent bond
Sharing a pair of electrons between 2 non - metals
When a substance made of small molecules boils what does the energy over come
Intermolecular forces
Why do simple covalent molecules have low boiling points
The intermolecular forces are weak and need little energy to overcome
Why can’t simple covalent molecules conduct electricity
As they have no overall charge meaning they can’t carry electrical charge
What does allotrope mean
Different types
How many covalent bonds does each carbon atom in graphene form
3
What’s the formula for buckminsterfullerene
C60
Why is graphene a good conductor of electicity
Each carbon atom makes 3 covalent bonds
Allowing 12 electron per carbon to be delocalised
And carry charge
Why does diamond have a higher melting point
Large amounts of energy needed to overcome the strong covalent bonds Allowing
Why is graphene soft and slippery
They have weak intermolecular forces betweeen the layer which require energy to overcome them
Why do giant covalent structures generally not conduct electricity
They have no delocalised electrons or free ions
How are the particles bonded together in metals
Electrostatic forces between positive ions and delocalised electrons
Why are metals good conducts of heat and electric
They have delocalised electrons which are free to move and carry charge
Why are metals good conducts of heat and electric
They have delocalised electrons which are free to move and carry charge
Why do metals have higher melting points
They have strong electrostatic attractions between positive ions and delocalised electrons
Why can metals be bent and shaped
As the layers of ions can easily slide over each other
