chapter 8-Reactivity series Flashcards
(23 cards)
what block are group 2 in
s-block
what are the propeties of group 2 metals
all reactive metals, have relatively low densities, in each reaction they are oxidised
what happens to reactivity as you go down the group and why
increases
total ionisation energy to remove 2 electrons decreases down group
electrons are lost more easily
elements become a stronger reducing agents
what are the first 2 ionisation equations
Mg= Mg+. +e-
Mg+=Mg2+. +e-
why does the first and second ionisation energy decrease down the group
atomic radius increases
more inner shells
less attraction
what happens when group 2 metals react with oxygen
they form metal oxides
what happens when group 2 metals react with water
they form metal hydroxides and hydrogen gas
what happens when group 2 metals react with dilute acid
they form salts and hydrogen gas
what are some uses of group 2
calcium hydroxide is used in agriculture to neutralise acid soils
magnesium hydroxide and calcium carbonate are used to help neutralise stomach acid
what are the propeties of halogens
all reactive non metals and in redox each halogen is reduced they are in p block
what are the physical properties of halogens
diatomic molecules
in solids they form simple molecular lattices with weak london forces
down group london forces increase in strength
more energy is required to break the forces
what are halogens in redox reactions
strong oxidising agents
what is the trend in reactivity in halogens
decreases
sheilding and atomic radius increases
attraction decreases
what does the reaction between halogens and halides show
to show reactivity decreases
how is the halogen and halide test carried out
mix halogen and halide together
if reaction takes place the halogen oxidised the halide ion
what happen if you add cyclohexan to the solution
it produces a colour which makes it easier to identify
what is a disproportionation reaction
when the element is both oxidised and reduced
how can chlorine be used
water treatment and household bleach
how do you identify carbonate ions
add dilute nitric acid
if bubbles are observed bubble gas through limewater if it turns milky it is co2
how do you identify sulfate ions
add aqueous barium chloride or barium nitrate
if a white precipitation forms of barium sulfate forms it contains sulfate ions
how do you identify halide ions
add silver nitrate to solution
if precipitate forms the solution contains halide ions
how do you analyse a mixture of ions
do it in order carbonate>sulfate>halide
how do you identify ammonium ions
add naoh to solution and warm it
test the gas with damp red litmus
if it turns blue the gas is ammonia
