DEFINITIONS, LAWS, AND PRINCIPLES: PHYSICS (PAPER 1)
VECTORS IN TWO DIMENTIONS
Resultant
the vector sum of two or more vectors, i.e., a single vector having the same effect as two or more vectors
together.
NEWTON’S LAWS AND APPLICATION OF NEWTON’S LAWS
Normal force
the force or the component of a force which a surface exerts on an object in contact with it, and which is
perpendicular to the surface.
Frictional force
the force that opposes the motion of an object and which acts parallel to the surface.
Static frictional force
the force that opposes the tendency of motion of a stationary object relative to a surface.
Kinetic frictional force
the force that opposes the motion of a moving object relative to a surface.
Newton's first law of motion
a body will remain in its state of rest or motion at constant velocity unless a non-zero resultant/net force acts
on it.
Inertia
the resistance of an object to any change in its state of motion. The mass of an object is a quantitative measure
of its inertia.
Newton's second law of motion When a resultant/net force acts on an object, the object will accelerate in the direction of the force at an
acceleration directly proportional to the force and inversely proportional to the mass of the object.
Newton's third law of motion
When object A exerts a force on object B, object B simultaneously exerts an oppositely directed force of
equal magnitude on object A.
Newton's law of universal each particle in the universe attracts every other particle with a gravitational force that is directly proportional
gravitation
to the product of their masses and inversely proportional to the square of the distance between their centres.
ELECTROSTATICS
State Coulomb's law
The magnitude of the electrostatic force exerted by two point charges on each other is directly proportional
to the product of the magnitudes of the charges and inversely proportional to the square of the distance
between them.
Electric field
region in space in which an electric charge experiences a force. The direction of the electric field at a point
is the direction that a positive test charge would move if placed at that point.
Electric field strength
Ohm's law
Power
Faraday's law
the electric field strength at a point is the electrostatic force experienced per unit positive charge placed at
that point.
ELECTRIC CIRCUITS
The potential difference across a conductor is directly proportional to the current in the conductor at constant
temperature.
the rate at which work is done or energy is transferred.
ELECTROMAGNETISM
The magnitude of the induced emf across the ends of a conductor is directly proportional to the rate of change
in the magnetic flux linkage with the conductor
DEFINITIONS, LAWS, AND PRINCIPLES: CHEMISTRY (PAPER 2)
Chemical bond
Lewis dot diagram
Valence electrons
Covalent bond
Bonding pair
Lone pair
Electronegativity
Non-polar covalent bond
Polar covalent bond
Bond energy
ATOMIC COMBINATIONS: MOLECULAR STRUCTURE
mutual attraction between two atoms resulting from the simultaneous attraction between their nuclei and the
outer electrons.
a structural formula in which valence electrons are represented by dots or crosses. It is also known as an
electron dot formula, a Lewis formula, or an electron diagram.
outer electrons are the electrons in the highest energy level of an atom in which there are electrons.
the sharing of electrons between two atoms to form a molecule.
a pair of electrons that is shared between two atoms in a covalent bond.
a pair of electrons in the valence shell of an atom that is not shared with another atom.
a measure of the tendency of an atom in a molecule to attract bonding electrons.
a bond in which the electron density is shared equally between the two atoms.
a bond in which the electron density is shared unequally between the two atoms.
a compound as the energy needed to break one mole of its molecules into separate atoms.
Bond length
Boiling point
Melting point
Vapour pressure
Solubility
Boyle's law
Mole
Molar mass
Avogadro's Law
Concentration
Heat of reaction
Exothermic reactions
Endothermic reactions
Activation energy
Activated complex
Arrhenius theory
Lowry-Brønsted theory
Ampholyte
Oxidation
Reduction
the average distance between the nuclei of two bonded atoms.
INTERMOLECULAR FORCES
the temperature at which the vapour pressure of a substance equals atmospheric pressure.
the temperature at which the solid and liquid phases of a substance are at equilibrium.
the pressure exerted by a vapour at equilibrium with its liquid in a closed system.
the property of a solid, liquid, or gaseous chemical substance (solute) to dissolve in a solid, liquid, or gaseous
solvent to form a homogeneous solution.
IDEAL GASES AND THERMAL PROPERTIES
the pressure of an enclosed gas is inversely proportional to the volume it occupies at constant temperature.
REPRESENTING CHEMICAL CHANGE
the amount of substance having the same number of particles as there are atoms in 12 g carbon-12.
the mass of one mole of a substance measured in g·mol-1.
one mole of any gas occupies the same volume at the same temperature and pressure.
as the amount of solute per litre of solution.
ENERGY AND CHEMICAL CHANGE
energy absorbed or released per mole in a chemical reaction.
reactions that release energy.
reactions that absorb energy.
the minimum energy needed for a reaction to take place.
the unstable transition state from reactants to products.
TYPES OF REACTION
an acid is a substance that produces hydrogen ions /hydronium ions when it dissolves in water. A base is a
substance that produces hydroxide ions when it dissolves in water.
An acid is a proton donor. A base is a proton acceptor.
a substance that can act as either acid or base
A loss of electrons. /An increase in oxidation number.
A gain of electrons. /A decrease in oxidation number.
Reducing agent
Oxidising agent
A substance that is oxidised/that loses electrons/whose oxidation number increases.
A substance that is reduced/that gains electrons/whose oxidation number decreases.