periodic table Flashcards
definition of an element
a substance made up of 1 type of atom
who developed the modern periodic table
mendeleev
state the features of mendeleev’s periodic table which are different to the modern periodic table
- elements arranged in order of atomic mass
- no noble gases
- fewer elements (had gaps)
- no transition metals
- no actinides or lanthanides
name given to the vertical columes
groups
name given to the horizontal rows
periods
name given to group 1
alkali metals
name given to group 2
alkaline earth metals
name given to group 7
halogens
name given to group 0
noble gases
name a semi-metal
gernanium, silicon
state the properties of metals
- good conductor of electricity
- good conductors of heat
- shiny
- malleable
- ductile
- sonorous
state the properties of non-metals
- poor conductor of electricity
- poor conductors of heat
- dull
- brittle
- not ductile
- not sonorous
definition of sonorous
makes a ringing sound when hit
which 2 elements are liquids at room temp
mercury, bromine
what does group number equal
number of electrons in the outer shell
why do elements in the same groups have similar properties
they have the same number of electrons in the outer shell
how are group 1 metals stored
in oil
what colour are all group 1 componds when solid
white
what colour are group 1 compounds when in solution
colourless
what does tarnish mean
shiny to dull
how does the reactivity of metals change down a group
increases
why does the reactivity of metals increase down the group
outer elctron gets further from the nucleus and is less attracted to it
what type of solution is produced when an alkali metal reacts with water
alkaline
state the typical observations when an alkali metal reacts with water
- fizzes
- floats
- moves across the surface
- disappears
- heat is released
what products are formed when an alkali metal reacts with water
metal hydroxide + hydrogen
write a half equation to represent a sodium atom becoming an ion
Na -> Na+ +e-
how does the rate of reactivity of group 7 change down the group
decreases
why does the reactivity of group 7 dcrease down the group
outer shell gets further from the nucleus and the incoming electron is less attracted to it
half equation to represent a chlorine atom becoming an ion
Cl + e- -> cl-
half equation to represent a chlorine molecule becoming an ions
Cl2 +2e- -> 2cl-
what is it meant by diatomic
2 atoms covalently bonded in a molecule
describe the appearance of fluorine
yellow gas
describe the appearance of chlorine
green gas
describe the appearance of bromine
red-brown liquid
describe the appearance of iodine
grey-black solid
iodine sublimes. what does this mean
changes from a solid to a gas
describe the test for chlorine gas
damp universal indicator changes to red and then bleaches white
why does the following equation occur?
chlorine + sodium bromide -> sodium chloride + bromine
chlorine is more reactive than bromine
what observations occur in the following reaction?
chlorine + sodium bromide -> sodium chloride + bromine
solution changes from colourless to orange
what observations occur in the following reaction?
chlorine + sodium iodide -> sodium chloride + iodine
solution changes from colourless to brown
why are noble gases unreactive
they have a full outer shell of electrons which makes them stable
describe the apperance of noble gases
colourless gases
how does the boiling points of the noble gases change down the group
increases
what colour is copper (II) oxide
black
what colour is copper (II) carbonate
green
what colour is copper (II) sulfate
blue
what colour is copper (II) salts in solution (usually)
blue
state some differences between group 1 metals and transition metals
- group 1-low m.p, tm-high m.p
- group 1-very reactive with water, tm- low reactivity with watrer
- group 1- form 1+ ions, tm form ions with different charges
- group 1 compounds are white, tm compounds are coloured
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