ionic compounds Flashcards
ionic compounds
formed between metals donating their valence electron(s) to non-metal atoms to form cations and anions, they have no overall charge, aka salts
the bohr model shows
how ionic bonds are formed but not how they are arranged in 3d shape
what structure do anions and cations form
a 3 d crystal lattice when theyy combine as solids
the ionic model explains
the properties of ionic compounds do to the bonds between the cations and anions
properties of ionic compounds
brittleness, hardness, high melting point, no electrical conductivity
why do ionic compunds have a high melting point and hardness
the ionic bonds between the positive and negative ions in a crystal lattice are strong, meaning a large amount of force/energy is required to disrupt/break these bonds
why are ionic compounds brittle
when a strong force is applied, the positive cations llign and the negative anions allign, the repulsive forces between these ions of like charge is strong enough to shatter the lattice
why can’t solid ionicc compounds conduct electricity
there are no free floating charged particles, the ions are held in place, they cant move so can’t carry an electrical current
when do ionic compoundss conduct electricity
in a molten o=state or aqueous (dissolved in water)
empirical formula
a formula that shpws the simplest, whole number ratio of particles
electrolyte
a solution or molten substance that conducts electricity by mens of the movement of ions
how can an ionic compound conduct electricity in water
the ions break away from the ionic lattice and mix with the water molecules
whether an ionic compound is soluble or insoluble depends
the relative strengths of the forces of attraction between the positive and negative ions in the lattice and the forces of attraction between the water molecules and the ions
