Element – a substance consists of one type of atom.
Compound – a substance consists two or more
elements that are chemically bonded (molecule or ions).
Atom – smallest particle of an element.
Molecule – a group of two or more atoms.
Ion – a positively charged / negatively
charged particle.
Boiling point - Temperature at which liquid
changes to gas under standard pressure.
Melting point - Temperature at which solid
changes to liquid under standard pressure.
Isotopes – atoms of the same element with
same proton number but different nucleon numbers.
Matter(solid,liquid,gas)
Particles(atom,molecules,ions)
Subatomic particle – proton,neutron,electron
Number of neutron(√),neutron
number(×)
Proton number – the number of proton in its
atom.
Nucleon number – the total number of proton
and neutron in its atom.
Relative atomic mass of an element = the
average mass of one atom of an element/((1/12) x the mass of one carbon-12
atom).
Relative molecular mass of an element = the
average mass of one atom of an molecule/((1/12) x the mass of one carbon-12
atom).
Molecule formula – compound shows the
actual number of atoms of each element that are present in a molecule of the
compound.
Empirical formula – compound shows the
simplest whole number ratio of atoms of each element in the compound.
Mole – amount of substance that contains as
many particles as the number of atoms in exactly 12 g of carbon-12 the symbol
of mole is mol.
One mole – Avogadro constant – 6.02 x 1023
Group (Periodic Table) – vertical columns
of element (similar chemical properties).
Periods (Periodic Table) – horizontal rows
of element.
Valence electrons – electrons that occupy
the outermost shell.
Ionic bond – bond formed through the
transfer of electrons between atoms of metal and non-metal to achieve the
stable octet electron arrangement.
Ionic compound – consist of positive ions
and negative ions which are held by strong electrostatic forces of attraction.
Covalent bond – bond formed through the
sharing of electrons between atoms of non-metal to achieve the stable duplet or
octet electron arrangement.
Covalent compound (also simple molecular
structure) – consists of neutral molecules which are held by weak
intermolecular forces (Van der Waals).
Electrolysis – The process of breaking down
chemical compounds via the use of electric current.
Anion – Negatively charged ions.
Cation – Positively charged ions.
Halogen – salt former with metals.
Alkali (base) – chemical substance which
ionizes in water to produce hydroxide ions, OH-.
Acid – chemical substance which ionizes in
water to produce hydrogen ions, H+
or hydroxonium ions, H3O+.
pH – degree of acidity or alkalinity of a
solution. Scale ranges from 0 to 14.
pH value – measure of the concentration of
hydrogen ions, H+
/ hydroxide ions,OH-.
Strong alkali – ionises (dissociates)
completely in water to form high concentration of hydroxide ions, OH-.
Weak alkali – ionises (dissociates)
partially in water to form low concentration of hydroxide ions, OH-.
Strong acid – ionises (dissociates)
completely in water to form high concentration of hydrogen ions, H+.
Weak acid – ionises (dissociates) partially
in water to form low concentration of hydrogen ions, H+.
Neutralisation – the reaction between acid
and base to produce salt and water only.
Titration – a experiment used to determine
the volume of acid needed to neutralize a fixed volume and molarity of alkali
in a conical flask with the help of an acid-base indicator to detect the end
point of the neutralization.
Salt – a ionic compound formed when the
hydrogen ion , H+
from acid is replaced by a metal ion / ammonium ion , NH4+.
Alloy – The compound that is formed by
mixing metals with other elements.
Polymer – long chain molecules made up by
monomer (repeating unit).
Rate of reaction –speed at which reactant
are converted into products in a chemical reaction.
Effective collision (Collision theory) –
collision that results in a chemical reaction where the particles collide with
the correct orientation and are able to achieve the activation energy.
Catalyst – a chemical substances that
provide an alternative path to lower the activation energy and increase the rate of reaction.
Positive catalyst – increases the rate of
reaction & lower the activation energy.
Negative catalyst – decreases the rate of
reaction & higher the activation energy.
Homologous series – organic compounds
(families) with similar formulae and properties.
Organic compounds – carbon-containing
compound. Carbon atoms form covalent bonds.
Inorganic compounds – compounds from
non-living things which do not contain the element carbon.
Saturated hydrocarbons – hydrocarbons
containing only single bonds between all carbon atoms.
Unsaturated hydrocarbons – hydrocarbons
containing at least one carbon-carbon double or triple bond.
Isomer – Molecule that has same molecular
formula but different structural formula.
Esterification – esters are produced.
Vulcanisation – a process of hardening of natural rubber by adding sulphur compounds.
Redox reaction – chemical reactions
involving oxidation and reduction occurring simultaneously.
Exothermic reaction – chemical reaction
that release heat to the surroundings.
Endothermic reaction – chemical reaction
that absorbs heat from the surroundings.
Heat of precipitation – the heat change
when one mole of a precipitate is formed from their ions in aqueous solution.
Heat of displacement – the heat change when
one mole of a metal is displaced from its salt solution by a more
electropositive metal.
Heat of neutralisation – the heat change
when one mole of water is formed from the reaction between an acid and an
alkali.
Heat of combustion – the heat change when
one mole of a substance is completely burnt in excess oxygen.
Flavouring – improve the taste or smell of
food and restore taste loss due to food processing.
Stabilisers – help to mix two liquids that
usually do not mix together so that they form an emulsion.
Thickeners – substances that thicken food
and give the food a firm, smooth and uniform texture.
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