1. Protons: mass 1/ charge + Neutrons: mass 1/ charge 0
Atomic structure-
Protons: mass 1/ charge +
Neutrons: mass 1/ charge 0
Electrons: mass 0/ charge -
Ionic bonding-atoms like to have full outermost shells. Here an atoms gives away or receives an
electron to
achieve a
full shell.
The atoms attract
Because they
have a charge
(ions)
Metal + Non- Metal only
Covalent bonding- here atoms share electrons to gain a full outermost shell.
Non Metal + Non Metal only
Metallic bonding- Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move.
Metals are good conductors of electricity and heat, because the free electrons carry a charge or heat energy through the metal
Giant ionic lattice
Mass Number- number of protons + neutrons in the nucleus
Atomic number- number of protons or electrons
Carbon: 6p, 6n, 6e
Graphite
Diamond made of Carbon atoms
Nano particles- Nanoparticles range in size from about 100 nm down to about 1 nm. Working with nanoparticles is called nanotechnology. They are useful as
catalysts
to speed up
reactions
Calcium’s electronic structure
2,8,8,2
Conservation of mass- Mass is never lost or created
Electronic structure-
1st shell- up to 2 electrons
2nd shell- up to 8 electrons
3rd shell- up to 8 electrons
Relative Atomic Mass RAM-
Mass of each atom compared to Carbon (12). E.g. Magnesium has a mass of 24 (twice as heavy as carbon)
numerical format of this atom: 2,4
How much carbon is in CO2?
CO2 RAM is 44
Carbon mass is 12
(12/44) x 100 = ? %
Answer can’t be more than 100%!
Relative Formula Mass RAF-
Atomic mass of each atom added up.
Carbon = 12
Oxygen = 16
CO2 RAM= 44
Group 1 elements have 1 e- on their outer most shell
Group 2 elements have 2 e- on their outermost shell
Etc….
Isotopes are atoms of an element with the normal number of protons and electrons, but different numbers of neutrons. Isotopes have the same atomic number, but different mass numbers.
C2) Chemistry

2. Electrolysis is the process by which ionic substances are broken down into simpler substances using electricity. During electrolysis, metals and gases may form at the electrodes
Reversible reactions- you can get back to the original reactants
e.g. ammonium chloride ammonia + hydrogen chloride
Increased temperature = increased rate of reaction
the reactant particles move more quickly
more particles have the activation energy or greater
the particles collide more often, and more of the collisions result in a reaction
the rate of reaction increases
Exothermic reactions= gives off heat (feels hot)
Endothermic reaction= takes in heat (feels cold)
The Haber process- making ammonia gas
Nitrogen and hydrogen will react together under these conditions:
a high temperature - about 450ºC
a high pressure - about 200 atmospheres (200 times normal pressure)
an iron catalyst
Increasing concentration = increased rate of reaction there are more reactant particles in the same volume
there is a greater chance of the particles colliding
the rate of reaction increases
Increasing surface area= increased rate of reaction
its surface area is increased
more particles are exposed to the other reactant
there is a greater chance of the particles colliding
the rate of reaction increases
Acids- substances with a pH of 16
Neutral- substance with a pH of 7
Alkali/ Base- substance with a pH of 814
N2(g)       + 3H2(g) 2NH3(g)
Splitting up NaCl2
Neutralisation-
Acid + Alkali  Salt + Water
(Neutral)
Increasing pressure = increased rate of reaction.
Because there are more reactant particles in the same volume
there is a greater chance of the particles colliding
the rate of reaction increases
Acid + Metal  Salt + Hydrogen gas
Acid + metal carbonate salt + water + carbon dioxide
Catalysts increase the rate of reaction without being used up. They do this by lowering the activation energy needed. With a catalyst, more collisions result in a reaction, so the rate of reaction increases. Different reactions need different catalysts.
C2) Chemistry