ionic, metallic, covalent and compound ions Flashcards
(22 cards)
what is an ionic compound
- giant lattice structure
- of oppositely charged ions
- require large amounts of energy to break bonds
properties of ionic compounds
- height melting and boiling points
- can conduct when aqueous or molten
- always want to get a full outer shell
what is ionic bonding
electrostatic attraction between oppositely charged metal ions and negatively charged non metal ions
why do ionic compounds have high melting and boiling points
- strong forces of attraction
- between oppositely charged ions
- require large amounts of energy to break bonds
when do ionic compounds conduct
not when solid but when molten or aqueous
why are metals good conductors of electricity
- delocalized electrons
- which are free to move
- can carry charge from one end to the other
why are metals good conductors of heat
- ions are tightly packed
- arranged in regular patterns
why are they malleable
layers that can slide over each other
do covalent compounds conduct electricity
no
what is covalent bonding
- sharing of a pair of electrons
- between 2 non metal ions
- strong attraction between a shared pair of electrons and 2 nuclei
what is a covalent compound
- giant lattice structures
- strong covalent bonds
- which require a lot of heat energy to break
- weak intermolecular forces
why do so simple molecular substances have low boiling points
- weak intermolecular forces
- which require little energy to break
- due to weak forces of attraction between molecules
why does diamond have a high melting point
- though forces are weak they must be over come to melt diamond
- because larger molecule
- more mass
- also means more attractions to overcome
why do covalent compounds not conduct
no charges particles in covalent compounds
what are allotropes
différent forms of same element
eg. diamond, graphite, fullerene, (carbon)
why is diamond so hard
- giant covalent structure
- many strong covalent bonds
formula for hydroxide
OH^1-
carbonate
CO3^2-
nitrate
NO3^1-
sulphate
SO4^2-
ammonium
NH4^1+
why are metals good conductors
- sea of delocalised electrons
- electricity is the flow of electrons
- so it is east for electricity to flow
