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chemistry (c1 (group 0 (all have full outer shells (Making them extremely…
chemistry
c1
structure of an atom
Protons and neutrons in nucleus electrons in shells
group 0
noble gasses on the right hand side of the periodic table
colourless
electron shells increse
all have full outer shells
Making them extremely stable and highly unreactive
boiling point increase as you go down the group
group 7
the halogens
florine ,clorine,bromine
7 electrons in outer shell
as you go down the group melting and boiling points increase
reactivity decreases as you move down the group
more reactive halogens displace less reactive halogens
group 2
alkalie earth metals
group 1
called alkali metals
all have one electron in outer shell
have to be stored carefully as they react with oxygen
elements/periodic table
Large number is the mass number =neutrons+protons
small number is atomic number=protons
protons=electrons
c2
ionic bounding
between non metals and metals
non metal ions gain electrons
metal ions lose electrons
have high melting points -don't conduct electricity when solid but when moltern
ionic compounds
magnesium oxide
sodium chloride
high melting and boiling points
covalent bounding
non metal and non metal combine by sharing electrons
don't conduct electricity
low melting and boiling points as intermolecular forces are weak
giant covalent structures
made of lots of atoms held together by covalent bounds
they have lots of bounds making them extremely strong
examples are graphite,diamound and sillica
have extremely high boiling points
diamound
it has very high melting points
it doesn't conduct electricity
form of carbon which is very hard as each atom is held together with 4 bounds
silica
similar structure itstead of being made of carbon it is made of silican and oxygen atoms
graphite
form of carbon in which atoms form layers
these layers can slide over each other making it much softer than diamound
each layer is only connected by 3 bounds
it conducts electricty
metallic bounding
metallic bounds held together within a sea of delocialised electrons
strong so need alot of energy to break them so therefore have very high melting and boiling points
metal structures
c3
rfm
to find the rfm of a substance you need to add up all the mass numbers
conservation of mass
during a chemical reaction nothing is lost or gained the atoms are just rearranged
total mass of product at the begging of the reaction is equal to the reactants at the end
c4
reactivity series
potasium
sodiumn
calciumn
aluminum
zinc
iron
tin
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displacement reactions
electrolysis
is a process in which ionic structures are broken downin to simpiler ones using electricity
in order for this process to work the ions must be molten
positively charged ions move to negative ions and are reduced
negatively charged ions move to positive ions they lose electrons and are oxcidised
different substances are produced during electrons if the substance is more reactive than hydrogen hydrogen will be produced if the substance is less reactive than hydrogen the metal will be produced
c5
exo and endothermic reactions
exothermic reactions transfer heat to the surroundings
for example burning
make surrounding areas hotter
endothermic reactions take energy in from the surroundings .usally transferred as heat energy and causesthe reaction mixture and its surroundings to get colder
for example electrolosis
fuel cells
energy profiles
exo starts with high energy releases it into the atmosphere making end up with less energy