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Summary GCSE AQA Chemistry mindmaps
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GCSE AQA Chemistry revision summary mindmaps including everything on the specification for all topics 1-10 to guarantee the highest grades.
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Atomic structure and period table Mass and isotopes Relative mass of atoms The periodic tableo An atom is the smallest part of an element that o The mass number is the sum of the protons and o Proton: 1 o Elements are arra
can exist neutrons in the nucleus of an atom o Neutron: 1 atomic (proton) n
o Compounds are formed from two or more o Isotopes are atoms of an element with different o Electron: very small with similar prope
elements numbers of neutrons but the same number of known as groups
o An element is a type of matter that can not be protons Relative atomic mass o The table is called
broken down into a simpler substance o The relative atomic mass of an similar properties
o A mixture consists of two or more elements or element is an average value that intervals
Relative electrical charge of subatomic particles
compounds not chemically bonded takes account of the abundance o Element in the sam
o Protons: +1
o Mixtures can be separated by physical processes o Neutrons: 0 of the isotopes of that element periodic table hav
such as filtration, crystallisation, simple o Electrons: -1 of electrons in the
distillation, fractional distillation and
Electronic structure this gives them sim
o In an atom the number of electrons is equal to the o The electrons in an atom occupy
chromatography number of protons to balance out the charge, so properties
the lowest available energy
atoms have no overall charge levels
Development of the atom model
Chemistry 1
o Atoms were thought to be tiny spheres that Metals and non-metals
could not be divided o Elements that react to form positive ions
o Discovery of the electron led to the plum o Elements that do not form positive ions a
pudding model - the atom is a ball of positive
Group 0 (noble gases)
charge with negative electrons embedded
o Unreactive as they have a stable arrangem
o The result of the alpha scattering experiment
o The boiling points increase with increasin
led to the conclusion that the mass of the
Development of the periodic table mass
atom was concentrated at the centre and that
the nucleus is charged o Before the discovery of neutrons, protons and electrons, Group 1 (alkali metals)
o Niels Bohr adapted the nuclear model by scientists classified the elements by arranging them in o Single outer electron
suggesting that electrons orbit the nucleus at order of their atomic weight o Reactivity increases down the group
specific distances o The early periodic table was incomplete, elements were Group 7 (the halogens)
o Later experiments led to the idea that the placed in inappropriate groups, and arranged in atomic o 7 outer electrons
positive charge of any nucleus could be weight o Reactivity decreases going down the grou
subdivided into a whole number of smaller o Mendeleev overcame some of the problems by leaving o Melting and boiling point increases going
particles, each particle having the same gaps for elements he thought had not been discovered Transition metals
amount of positive charge, the name protons and changed the order based on atomic weight o Higher densities, boiling point, melting po
were given to these particles o Elements with properties predicted by Mendeleev were stronger than group 1 metals
o The experimental work of James Chadwick discovered and filled the gaps o Have ions with different charges, form co
provided evidence to show the existence of o Knowledge of isotopes made it possible to explain why compounds and are useful as catalysts
neutrons in the nucleus the order based on atomic weights was not correct
, Chemical bonds The three states of matter
Properties of ionic compounds
o For ionic bonding the particles are oppositely charged ions o Melting and freezing takes place at the melting point,
o Regular giant ionic lattice structu
o For covalent bonding the particles are atoms which share boiling and condensing takes place at the boiling
o Strong electrostatic forces of attr
pairs of electrons point
between oppositely charged ions
o For metallic bonding the particles are atoms which share o The amount of energy needed to change state
o They have high melting and boili
delocalised electrons depends on the strength of the forces between
the large amount of energy requ
particles of the substance
bonds
Ionic bonding o The stronger the forces between the particles the
o When melted or dissolved in wat
o Metal reacts with a non-metal higher the melting and boiling point of a substance
conduct electricity because the i
o Electrons from the outer shell of the metal atom are
Polymers and so charge can flow
transferred to the outer shell of the non-metal
o Metal atoms lose electrons to form positively ions o Very large molecules Properties of small molecules
o Non-metal atoms gain electrons to form negatively ions o Atoms in the polymer molecules are linked to other o Usually gases or liquids that have
atoms by strong covalent bonds boiling points
Ionic compounds o Weak intermolecular forces betw
o Giant structure of ions o The intermolecular forces between polymer molecules
are strong and so they are solid at room temperature o It is these intermolecular forces t
o Ionic compounds are held together by strong electrostatic
Chemistry 2
not covalent bonds, when the su
forces of attraction between oppositely charged ions
o The intermolecular forces increa
o These forces act in all directions in the lattice and this is
molecules, so larger molecules h
called ionic bonding
and boiling points
Covalent bonding o These substances do not conduc
o when atoms share pairs of electrons, they form covalent the molecules do not have an ov
Properties of metals and alloys
bonds, these bonds between atoms are strong Giant covalent structures
o Metals have giant structures of atoms with strong metallic
o Covalently bonded substances may consist of small o Solids with very high melting poi
bonds meaning they have a high melting and boiling point
molecules, with low melting and boiling points due to the o All of the atoms in this structure
o In pure metals, atoms are arranged in layers, which allow metals
weak intermolecular forces atoms by strong covalent bonds
to be bent and shaped
o Some covalently bonded substances have giant covalent o These bonds must be overcome
o Pure metals are too soft for many uses and so are mixed with
structures, like diamond and silicon dioxide substances
other metals to make alloys which are harder
Metallic bonding o Diamond, graphite and silicon dio
o Metals consist of giant structures of atoms arranged in a giant covalent structures
regular pattern
Metals as conductors
o The electrons in the outer shell of metal atoms are Nanoparticles
o Metals are good conductors of electricity because the
delocalised and so free to move through the whole structure o Uses include: applications in med
delocalised electrons in the metal carry electrical charge
o The sharing of delocalised electrons gives rise to many cosmetics, deodorants and as ca
through the metal
strong metallic bonds o Risks include: skin penetration, t
o Metals are good conductors of thermal energy because energy
damage skin cells
is transferred by the delocalised electrons
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