chem structure

structure of giant ionic crystal lattice structure

ionic compounds have a giant ionic crystal lattice structure with strong electrostatic attraction between the cations and anions

properties of GICLS

high melting and boiling points, hard and brittle, conduct electricity in liquid and aqueous state

why does GICLS have high melting and boiling points?

a large amount of energy is required to overcome the strong electrostatic attraction between the cations and anions.

why is GICLS hard?

a large amount of energy is required to overcome the strong electrostatic attraction between the cations and anions

why is GICLS brittle?

when sufficient force is applied, layers of regularly charged ions can slide, bringing ions of like charges next to each other, causing them to repel and the ionic lattice shatters

why can’t GICLS conduct electricity in solid state?

ions are held in fixed positions by strong electrostatic attraction between the cations and anions, hence the ions cannot move freely to conduct electricity.

why can GICLS conduct electricity in liquid and aqueous states?

the electrostatic attraction between the cations and anions are overcome. the ions are mobile and can move freely to conduct electricity.

structure of simple covalent structure

simple compounds have simple covalent structure with strong covalent bonds between each atom within each molecule, but weak intermolecular forces of attraction between the molecules

physical properties of SCS

low melting and boiling points, soft, no electrical conductivity

why does SCS have low melting and boiling points?

a small amount of energy is required to overcome the weak intermolecular forces between the molecules.

why is SCS soft?

a small amount of energy is required to overcome the weak intermolecular forces between the molecules

why can’t SCS conduct electricity

as the molecules exist as uncharged, neutral molecules, there is no mobile valence electrons and ions present to conduct electricity

structure of diamond

diamond has a giant covalent structure in which each C atom is joined to 4 other C atoms by strong covalent bonds.

structure of graphite

graphite has a giant covalent structure in which each C atom in the layer is joined to 3 other C atoms by strong covalent bonds. there are weak intermolecular forces of attraction between the layers of atoms.

properties of diamond

high melting and boiling points, hard, cannot conduct electricity

properties of graphite

high melting and boiling points, soft, can conduct electricity

why do diamond and graphite have high melting and boiling points?

diamond and graphite have a giant covalent structure. a large amount of energy is required to overcome the strong covalent bonds between the C atoms

why is diamond hard?

a large amount of energy is required to overcome the strong covalent bonds between the C atoms.

why is graphite soft?

a small amount of energy is required to overcome the weak intermolecular forces between the layers of atoms, allowing the layers to slide over each other easily

why can’t diamond conduct electricity?

all 4 valence electrons of each C atom are involved in covalent bonding. there are no mobile valence electrons and diamond cannot conduct electricity

why can graphite conduct electricity?

each C atom only used 3 valence electrons in covalent bonding. the 4th valence electron of each carbon atom is delocalised. the delocalised electrons can move freely along the layers to conduct electricity

structure of giant metallic lattice

metals have giant metallic structure with strong electrostatic attraction between the ions and the ‘sea’ of delocalised mobile valence electrons.

properties of GMLS

high melting and boiling points, malleable and ductile, good electrical conductor

why does GMLS have high melting and boiling points?

metal has a giant metallic lattice structure. a large amount of energy is required to overcome the strong electrostatic attraction between the ions and the ‘sea’ of delocalised mobile valence electrons.

why is GMLS malleable and ductile?

non-directional nature of metallic bonds allow layers of regularly arranged ions of the same size to slide over one another without breaking the strong electrostatic forces of attraction

why is GMLS a good conductor of electricity?

delocalised mobile valence electrons can move freely through the metallic structure to conduct electricity.