Key People
Dalton (atomic theory)
Thompson (electrons)
Rutherford (Gold leaf experiment)
The Particles
Atomic
Protons= +1 charge
Neutrons= 0 charge
Electrons= -1 charge
Mass of the atom is centred in
the nucleus
structure Waters of Crystallisa
and isotopes
Atomic number= number of
protons in an atom 1. Weigh an emp
A= mass number 2. Add the hydrated s
Z= number of protons 3. Using a pipe clay triangle
Protons and neutrons are equal
in charge... electrons are tiny in salt in a crucible on a
comparison= 1/1840 minu
4. Leave the crucible to cool
and anhydr
Definitions
IOns Isotopes= Atoms of the same element with different
Metals lose electrons and number of neutrons and different masses... Same
form positive ions reactivity as normal atoms
Non- metals gain electrons
and form negative ions Ions= Charged particles that is formed when an atom loses
or gains electrons.
Ammonium= NH4+
Hydroxide= OH- Positive ions are called cations .
Nitrate= NO3- Negative ions are called anions.
Nitrite= NO2-
Hydrogencarbonate= HCO3-
Manganate(VII)= MnO4-
Carbonate= CO32-
CHEMISTRY
Sulfate= SO42-
Sulfite= SO32-
Dichromate= Cr2O72-
Phosphate= PO43-
Formulae
and
Formulae
For ions: make sure that the overall
charge is zero (the sum of the positive
charges are equal to the sum of the
equations MODULE 2
negative charges)
Diatomic molecules= H2, N2, O2, F2, Cl2, Br2, I2
State symbols-
Gas= (g)
Liquid= (l)
Solid= (s)
Aqueous= (aq)
Definitions
Empirical formula= Simplest whole number ratio
of atoms of each present in a compound Acid= a proton donor
Bases= a proton accept
Definition Alkalis= bases that can dissolve
Relative Atomic Mass= The weighted mean mass to form aqueous hydroxide
of an atom of an element compared with one
, Definitions
Periodicity- The repeating trends in chemical and
physical properties
First ionisation energy- The energy required to remove one electron
from each atom in one mole of the gaseous element to form one mole
of gaseous 1+ ions.
Ionisation energy
The periodic
Factors that affect ionisation energy-
Atomic Radius
Nuclear Charge
table
Electron Shielding
First ionisation decreases between the end of a period and the
beginning of a new one because there is an increase in atomic radius
and an increase in electron shielding.
First ionisation decreases down the group because shielding increases (weaker attraction), atomic radius
increases (weaker attraction), increased number of protons is outweighed by increase in radius and
shielding
Metals
Giant metallic lattice properties:
High melting and boiling points
Good electrical conductors
Malleability
CHEMISTRY
Ductility Boltzmann distribution
Definitions and equations
Rate(mol dm-3 s-1) = change in concentration/ time
MODULE 3
Catalyst= A substance that increases the rate of reaction but does not get used up itself (they
provide a an alternative pathway for the reaction)
Homogeneous catalyst= A catalyst that is in the same state as the reactants
Heterogeneous catalyst= A catalyst that is in a different state as the reactants
Catalytic convertors= They are present in vehicles to reduce toxic emissions and prevent photochemical smog
Activation energy- the minimum energy that particles must collide with for a reaction to occur
Reactions
In order for particles to react, they must collide with sufficent energy
Dalton (atomic theory)
Thompson (electrons)
Rutherford (Gold leaf experiment)
The Particles
Atomic
Protons= +1 charge
Neutrons= 0 charge
Electrons= -1 charge
Mass of the atom is centred in
the nucleus
structure Waters of Crystallisa
and isotopes
Atomic number= number of
protons in an atom 1. Weigh an emp
A= mass number 2. Add the hydrated s
Z= number of protons 3. Using a pipe clay triangle
Protons and neutrons are equal
in charge... electrons are tiny in salt in a crucible on a
comparison= 1/1840 minu
4. Leave the crucible to cool
and anhydr
Definitions
IOns Isotopes= Atoms of the same element with different
Metals lose electrons and number of neutrons and different masses... Same
form positive ions reactivity as normal atoms
Non- metals gain electrons
and form negative ions Ions= Charged particles that is formed when an atom loses
or gains electrons.
Ammonium= NH4+
Hydroxide= OH- Positive ions are called cations .
Nitrate= NO3- Negative ions are called anions.
Nitrite= NO2-
Hydrogencarbonate= HCO3-
Manganate(VII)= MnO4-
Carbonate= CO32-
CHEMISTRY
Sulfate= SO42-
Sulfite= SO32-
Dichromate= Cr2O72-
Phosphate= PO43-
Formulae
and
Formulae
For ions: make sure that the overall
charge is zero (the sum of the positive
charges are equal to the sum of the
equations MODULE 2
negative charges)
Diatomic molecules= H2, N2, O2, F2, Cl2, Br2, I2
State symbols-
Gas= (g)
Liquid= (l)
Solid= (s)
Aqueous= (aq)
Definitions
Empirical formula= Simplest whole number ratio
of atoms of each present in a compound Acid= a proton donor
Bases= a proton accept
Definition Alkalis= bases that can dissolve
Relative Atomic Mass= The weighted mean mass to form aqueous hydroxide
of an atom of an element compared with one
, Definitions
Periodicity- The repeating trends in chemical and
physical properties
First ionisation energy- The energy required to remove one electron
from each atom in one mole of the gaseous element to form one mole
of gaseous 1+ ions.
Ionisation energy
The periodic
Factors that affect ionisation energy-
Atomic Radius
Nuclear Charge
table
Electron Shielding
First ionisation decreases between the end of a period and the
beginning of a new one because there is an increase in atomic radius
and an increase in electron shielding.
First ionisation decreases down the group because shielding increases (weaker attraction), atomic radius
increases (weaker attraction), increased number of protons is outweighed by increase in radius and
shielding
Metals
Giant metallic lattice properties:
High melting and boiling points
Good electrical conductors
Malleability
CHEMISTRY
Ductility Boltzmann distribution
Definitions and equations
Rate(mol dm-3 s-1) = change in concentration/ time
MODULE 3
Catalyst= A substance that increases the rate of reaction but does not get used up itself (they
provide a an alternative pathway for the reaction)
Homogeneous catalyst= A catalyst that is in the same state as the reactants
Heterogeneous catalyst= A catalyst that is in a different state as the reactants
Catalytic convertors= They are present in vehicles to reduce toxic emissions and prevent photochemical smog
Activation energy- the minimum energy that particles must collide with for a reaction to occur
Reactions
In order for particles to react, they must collide with sufficent energy
