Chemistry paper 2 Flashcards
(34 cards)
what is group 1
alkali metals
what are the properties of group 1 metals
- all have one outer shell electron
- low melting and boiling points
- very soft
- form ionic compounds (+1 ion)
why don’t group 1 elements form covalent bonds
they lose their outer shell electron so easily that sharing is necessary
what happens with reactivity in group one
as you go down the group, they get more reactive because the outer electron is more easily lost because its further from the nucleus so there is a larger atomic radius so is less strongly attracted to the nucleus and less energy is needed to remove it
what happens when the alkali metals are put in water
they react vigorously
the reaction produces hydrogen gas and a hydroxide of the metal
lithium will move around the surface fizzing
sodium and potassium do the same and also melt in the heat of the reaction. Potassium even gets hot enough to ignite the hydrogen gas being produced
caesium and rubidium do the same but explode
what are the group seven elements known as
the halogens
what do the halogens exist as
diatomic molecules
what are the properties of group 7 elements
as you go down melting and boiling points increase
what is the state and colour of chlorine, bromine and iodine at room temperature
chlorine - fairly reactive poisonous green gas
bromine - poisonous red-brown liquid which gives off an orange vapour at room temperature
iodine - a dark grey crystalline solid which gives off a purple vapour when heated
what is the test for chlorine
damp blue litmus paper will turn red then bleach white
what happens to reactivity in group 7
reactivity decreases as you go down because there is a larger atomic radius and therefore more electron shielding so it is harder for the atom to attract the one electron it needs because the force of electrostatic attraction between the nucleus and new electron is weak
they form 1- ions
what happens when the halogens react with metals
they form a salt called a metal halide
e.g sodium + chlorine -> sodium chloride
what happens when halides react with hydrogen
form hydrogen halides
they are soluble (can dissolve in water) to from acidic solutions
e.g HCL forms hydrochloric acid in water
what are the halogen displacement reactions
redox reactions
the halogens gain electrons (reduction) whilst halide ions lose electrons (oxidation)
how would you do a displacement reactions to show the reactivity trend of the halogens
1) start by measuring out a 5ml of halide salt solution in a test tube
2) add a few drops of halogen solution to it and gently shake tube
3) if you see a colour change then a reaction has happened - the halogen has displaced the halide ions from the salt
4) repeat the process using the different combinations of halide salt and halogen
what is group zero
the noble gases
what are the properties of the noble gases
- colourless gas at room temperature
- monatomic (single atoms not molecules)
- more or less inert - they don’t react with much at all because they have a full outer shell of electrons so they don’t give up or gain electrons easily
- non-flammable
- hard to observe so took a long time to discover
what are the everyday uses of the noble gases
- provide an inert atmosphere
- argon in filament lamps because it is non-flammable it stops the very hot filament from burning away
- flash photography uses the above principle with argon, krypton and Zenon to prevent high temperature flashes in filaments
- argon and helium can be used to protect metals that are being welded as the inert atmosphere stops the hot metal reacting with oxygen
- helium is used in airships and party balloons because it has a lower density than air so it floats and is non-flammable so safer to use than hydrogen gas
what are the properties of the noble gases
- boiling, melting point and density all increase as you go down the group
what is the rate of reaction
how quickly a reaction happens, how quickly a product is formed or the reactants are used up
what is the formula for rate of reaction
amount of reactant used or product formed / time
what are three ways that you can measure the rate of reaction
- precipitation
- change in mass (usually gas given off)
- the volume of gas given off
how does precipitation measure the rate of reaction
- mixing two see-through solutions produces a precipitate which clouds the solution
- you mix the two reactant solutions and put the flask on a piece of paper that has a mark on it
- observe the mark through the mixture and measure how long it takes for the mark to be obscured. The faster it disappears, the faster the reaction
why is using precipitation to measure the rate of reaction not accurate
because the result is subjective - different people might not agree on exactly when the mark disappears