the periodic table

• what does group number tell us ?

  elements are arraged in groups of similar properties- group is also the number of electrons on the outer shell
• what does the period number tell us ?

  the period number tells us how many shells of electrons an atom has
• what increases down the group and why ?

  Atomic size increases aswell as reactivity (in some cases). the reactivity increases because it is easier for an electron to be lost as the electrostatic attraction between protons and electrons is weaker(but this is different when electrons need to be gained).
• what are group 7 elements known as ?

  halogens
• how does the reactivity of halogens change down the group?

  decreases (harder to gain an electron)
• what else increases down group 7 ?

  atomic/ relative atomic mass and higher melting and boiling points
• what are group 0 gases known as and why is it group zero not 8 ?

  Noble gases. They are called Group 0 because they have a full outer shell of electrons, making them stable and unreactive.
• why where group 0 elements hard to discover ?

  because of how unreactive they are
• what state and colour are the nobel gases at room temp ?

  gas + colourless
• why does the boiling + melting points increase down the group ?

  more electrons meaning more intermolecular force
• does xenon or neon have the higher BP ?

  xenon because it is lower down the group - greater intermolecular forces which need to be brioken
• why do group 7 elements get less reactive down the group ?

  • G7 elements react by gaining an electron to have a full outer shell
  • as you go down the group the electrons become futher away from the nucleus meaning less attraction
  • this makes it harder to gain so they become less reactive
• describe the reactivity of group 1 metals talking about shells


  -they are all reactive with one electron on its outer shell (which increases reactivity because Metals with one electron in their outer shell are highly reactive because they can easily lose that electron to achieve a stable, full outer shell, requiring low energy to do so.)
• describe the reactivity of group 1 metals and how it changes

  -reactivity increases down the group

  -all metals in group 1 have 1 electron on the outer shell
• what effect does having one electron on the outer shell do to the reactivity ?


  Metals with one electron in their outer shell are highly reactive because they can easily lose that electron to achieve a stable, full outer shell, requiring low energy to do so
• describe properties of group 1 elements


  -soft
• describe the properties of group 1 metals


  -soft metals , highly reactive, lower MP and BP compared to other metals
• what do group 1 metals typically react to form 


  ionic compounds
• describe the reactions of group 1 metals in water


  when group 1 metals are placed in water the react very intesly forming hydrogen gas and also metal hydroxides(the lower down the group the more intense the reaction)
• describe the reaction of sodium in water


  sodium reacts with water intensly forming hydrogen as it skips across the water which is then ignited to form purple sparks it also forms sodium hydroxide
• describe group 1 metals reacting with chlorine


  group 1 metals react with chlorine to form metal chloride salts eg :

  sodium chloride
• describe group 1 metals reaction with oxygen


  group 1 metals do not react vigoursly with oxygen however they do react forming metal oxides eg lithium oxide
• compare group 1 metals to transition metals


  transition metals are stronger with higher boiling points however less reactive than group 1 metals, they are also denser harder and heavier than group 1 metals