the periodic table Flashcards
before the 20th century, what could scientist measure regarding elements
relative atomic mass
what was noticed after arranging elements in order of mass
properties of elements where repeated at regular intervals
what are some problems with the early periodic tables
not all elements had been discovered so not compleate
ended up in the wrong group as they where placed in order of relative atomic mass
what did Dmitri Mendeleev do
1869
left gaps
mainly in order of atomic mass
but switched order of some elements
so elements with the same properties ended up in the same groups
the gaps allowed predictions to be made about undiscovered elements
what did the discovery of isotopes do
isopotops of the same elemnt have different atomic masses but the same chemical propeties so occopy the same place on the pt so mendeelev was right to leave gaps
what is the modern periodic table measured in
incresing atomic number
what does the period number tell you
how many electron shells
what does the group number tell you
how many electrons in the outer shell
what are metals
elements that form positive ions when they react
why cant non metals form positive ions
right of pt where they have lots of electrons to remove gto form a full outer shell or near the top where the outer shell elecrons have a strong force of attraction towards the nucleus.
physical properties of metals
strong
malible
great conductors of heat and elecricty.
high boiling and melting points.
physical properties of non metals
dull
brittle
lower bp and mp
lower density
what are the alkali metals and what are their properties
group 1: lithium, sodium, potassium, rubidium, caesium and francium
they are silvery solids that have to be kept in oil.
one elecron in their outer shells. low density and get more reactive down the group
why do alkali metels get more reactive down the group
elecron is further away from force of attraction of the nucleus
what happens to the boiling point going down group 1 elements
decreases down the group