PHYSICAL SCIENCES REVISION

# NORTH WEST GRADE 12 DEFINITIONS (Collectable Marks) Paper 1: Physics Newton's laws and application of Newton's laws Normal force, N, is the force or the component of a force which a surface exerts on an object with which it is in contact, and which is perpendicular to the surface. Frictional force, f, is the force that opposes the motion of an object and which acts parallel to the surface. Static frictional is the force that opposes the tendency of motion of a stationary object relative to force, f s , a surface. Kinetic frictional is the force that opposes the motion of a moving object relative to a surface. force, f k Weight is the gravitational force the Earth exerts on any object on or near its surface. Newton's laws Newton's first law A body will remain in its state of rest or motion at constant velocity unless a non-zero of motion: resultant/net force acts on it. Newton's second When a resultant/net force acts on an object, the object will accelerate in the direction law of motion: of the force at an acceleration directly proportional to the force and inversely proportional to the mass of the object. Newton's third law When one body exerts a force on a second body, the second body exerts a force of motion: of equal magnitude in the opposite direction on the first body. Newton's Law of Each body in the universe attracts every other body with a force that is directly Universal proportional to the product of their masses and inversely proportional to the square of Gravitation: the distance between their centres. Momentum and Impulse Momentum i s the product of an object's mass and its velocity. Newton's second The resultant/net force acting on an object is equal to the rate of change of law of motion in momentum of the object in the direction of the resultant/net force. terms of momentum Impulse is the product of the resultant/net force acting on an object and the time the resultant/net force acts on the object. The impulse- F net Δt = mΔv. momentum theorem A closed/an a system on which the resultant/net external force is zero (A closed/an isolated system isolated system (in excludes external forces that originate outside the colliding Physics), bodies, e.g. friction. Only internal forces, e.g. contact forces between the colliding objects, are considered) The principle of The total linear momentum of a closed system remains constant (is conserved). conservation of linear momentum:

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https://ultradeep.co.za Projectile Motion in One Dimension (1D) A projectile an object upon which the only force acting is the force of gravity Work, Energy and Power Work The work done on an object by a constant force F is F Δx cos θ , where F is the magnitude of the force, Δx the magnitude of the displacement and θ the angle between the force and the displacement. The work-energy The net/total work done on an object is equal to the change in the object's theorem: kinetic energy OR the work done on an object by a resultant/net force is equal to the change in the object's kinetic energy. In symbols: W net = Δ K = K f - K i . A conservative i s a force for which the work done in moving an object between two points is force independent of the path taken. Examples are gravitational force, the elastic force in a spring and electrostatic forces (coulomb forces). A non-conservative is a force for which the work done in moving an object between two points depends force on the path taken. Examples are frictional force, air resistance, tension in a chord, etc. The principle of The total mechanical energy (sum of gravitational potential energy and kinetic energy) conservation of in an isolated system remains constant. (A system is isolated when the resultant/net mechanical energy: external force acting on the system is zero.) Power is the rate at which work is done or energy is expended Doppler Effect (relative motion between source and observer) The Doppler effect is the change in frequency (or pitch) of the sound detected by a listener because the sound source and the listener have different velocities relative to the medium of sound propagation. Electrostatics and Electric field and Electric Circuits Coulomb's law: The magnitude of the electrostatic force exerted by one point charge (Q 1 ) on another point charge (Q 2 ) is directly proportional to the product of the magnitudes of the charges and inversely proportional to the square of the distance (r) between them. An electric field. is a region of 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 The electric field at The electric field at a point is the electrostatic forceexperienced per unit positive a point charge placed at that point Ohm's law: The potential difference across a conductor is directly proportional to the current in the conductor at constant temperature. Rms for an The rms value of AC is the DC potential difference/current which dissipates the alternating voltage same amount of energy as AC or an alternating current https://tvetpapers.co.za

https://ultradeep.co.za Optical Phenomena and Properties of Materials Photo-electric effect The photoelectric is the process whereby electrons are ejected from a metal surface when light of effect suitable frequency is incident on that surface. Threshold as the minimum frequency of light needed to emit electrons from a certain metal frequency, f o , surface. Work function, W o is the minimum energy that an electron in the metal needs to be emitted from the metal surface. Emission and absorption spectra An atomic is formed when certain frequencies of electromagnetic radiation that passes through a absorption medium, e.g. a cold gas, is absorbed spectrum An atomic is formed when certain frequencies of electromagnetic radiation are emitted due emission spectrum to an atom's electrons making a transition from a high-energy state to a lower energy state Paper 2: Chemistry GENERAL THEORY Structure of functional group Homologous series Structure Name/Description Only C-H and C-C Alkanes C C single bonds Carbon-carbon Alkenes C C double bond C C Carbon-carbon Alkynes triple bond Halogen atom C X Haloalkanes bonded to a saturated C atom (X = F, Cℓ, Br, I) Hydroxyl group lcohols C O H bonded to a saturated C atom O Aldehydes Formyl group C H O Carbon l group Ketones C C C bonded to two C atoms O Carboxylic acids Carboxyl group C O H O Esters C O C https://tvetpapers.co.za

https://ultradeep.co.za Molar volume of 3 1 mole of any gas occupies 22,4 dm at 0 °C (273 K) and 1 atmosphere (101,3 gases kPa). Dfferent Dipole-dipole Forces between two polar molecules intermolecular forces: forces (Van Induced dipole Forces between non-polar molecules der Waal's forces or London forces): forces Hydrogen Forces between molecules in which hydrogen is covalently bonding bonded to nitrogen, oxygen or fluorine – a special case of dipole-dipole forces Boiling point The stronger the intermolecular forces, the higher the boiling point. Melting point: The stronger the intermolecular forces, the higher the melting point. Vapour pressure The stronger the intermolecular forces, the lower the vapour pressure. Rates and equilibrium ΔH > 0 for endothermic reactions, i.e. reactions in which energy is released. ΔH < 0 for exothermic reactions, i.e. reactions in which energy is absorbed. factors that nature of reacting substances, affect the surface area, rate of concentration (pressure for gases), chemical temperature reactions, , the presence of a catalyst catalyst increases the rate of a reaction by providing an alternative path of lower activation energy. It therefore decreases the net/total activation energy. the factors pressure (gases only), that influence concentration the position of temperature. an equilibrium + auto-ionisation the reaction of water with itself to form H 3 O of water - ions and OH ions. Definitions Organic Chemistry https://tvetpapers.co.za

https://ultradeep.co.za Boiling point The temperature at which the vapour pressure of a substance equals atmospheric pressure Melting point: The temperature at which the solid and liquid phases of a substance are at equilibrium. Vapour pressure The pressure exerted by a vapour at equilibrium with its liquid in a closed system. Organic molecules are molecules containing carbon atoms. Molecular formula A chemical formula that indicates the type of atoms and the correct number of each in a molecule. Structural formula A structural formula of a compound shows which atoms are attached to which within the molecule. Atoms are represented by their chemical symbols and lines are used to represent ALL the bonds that hold the atoms together. Condensed This notation shows the way in which atoms are bonded together in the molecule, structural formula but DOES NOT SHOW ALL bond lines. Hydrocarbon: Organic compounds that consist of hydrogen and carbon only Homologous series A series of organic compounds that can be described by the same general formula OR in which one member differs from the next with a CH 2 group Saturated Compounds in which there are no multiple bonds between C atoms in their compounds hydrocarbon chains. Unsaturated Compounds with one or more multiple bonds between C atoms in their compounds : hydrocarbon chains. Functional group A bond or an atom or a group of atoms that determine(s) the physical and chemical properties of a group of organic compounds. Structural isomer Organic molecules with the same molecular formula, but different structural formulae. Chain isomers Same molecular formula, but different types of chains Positional isomers Same molecular formula, but different positions of the side chain, substituents or functional groups on the parent chain Functional isomers Same molecular formula, but different functional groups Hydrohalogenation: The addition of a hydrogen halide to an alkene Halogenation The reaction of a halogen (Br 2 , Cℓ 2 ) with a compound Hydration The addition of water to a compound Hydrogenation The addition of hydrogen to an alkene https://tvetpapers.co.za

https://ultradeep.co.za Dehydrohalogenatio The elimination of hydrogen and a halogen from a haloalkane n of haloalkanes: Dehydration of Elimination of water from an alcohol alcohols: Cracking of alkanes: The chemical process in which longer chain hydrocarbon molecules are broken down to shorter more useful molecules. Hydrolysis The reaction of a compound with water Macromolecule A molecule that consists of a large number of atoms Polymer: A large molecule composed of smaller monomer units covalently bonded to each other in a repeating pattern Monomer: Small organic molecules that can be covalently bonded to each other in a repeating pattern Polymerisation A chemical reaction in which monomer molecules join to form a polymer Addition A reaction in which small molecules join to form very large molecules by polymerisation : adding on double bonds Addition polymer : A polymer formed when monomers (usually containing a double bond) combine through an addition reaction Condensation Molecules of two monomers with different functional groups undergo polymerisation condensation reactions with the loss of small molecules, usually water Condensation A polymer formed by two monomers with different functional groups that are polymer linked together in a condensation reaction in which a small molecule, usually water, is lost RATES AND EQUILIBRIUM heat of reaction the energy absorbed or released in a chemical reaction. (ΔH) exothermic reactions reactions that release energy. endothermic reactions that absorb energy. reactions activation energy the minimum energy needed for a reaction to take place. activated complex the unstable transition state from reactants to products. reaction rate the change in concentration of reactants or products per unit time. positive catalyst a substance that increases the rate of a chemical reaction without itself undergoing a permanent change a catalyst increases the rate of a reaction by providing an alternative path of lower activation energy. It therefore decreases the net/total activation energy. open system continuously interacts with its environment, while a closed system is isolated from its surroundings. https://tvetpapers.co.za

https://ultradeep.co.za reversible reaction: A reaction is reversible when products can be converted back to reactants. Chemical equilibrium a dynamic equilibrium when the rate of the forward reaction equals the rate of the reverse reaction Le Chatelier's When the equilibrium in a closed system is disturbed, the system will re- principle: instate a new equilibrium by favouring the reaction that will oppose the disturbance. Acids and Bases Arrhenius theory An acid + is a substance that produces hydrogen ions (H )/hydronium ions + (H 3 O ) when it dissolves in water. A base - is a substance that produces hydroxide ions (OH ) when it dissolves in water. Lowry-Brønsted An acid + is a proton (H ion) donor. A base + is a proton (H ion) acceptor. Strong acids + ionise completely in water to form a high concentration of H 3 O ion Weak acids + ionise incompletely in water to form a low concentration of H 3 O ions. Strong bases - dissociate completely in water to form a high concentration of OH ions. Weak bases - dissociate/ionise incompletely in water to form a low concentration of OH ions Concentrated contain a large amount (number of moles) of acid/base in proportion to acids/bases the volume of water Dilute acids/bases contain a small amount (number of moles) of acid/base in proportion to the volume of water. Conjugate acid-base - When the acid, HA, loses a proton, its conjugate base, A , is formed. pairs - When the base, A , accepts a proton, its conjugate acid, HA, is formed. ampholyte or a substance that can act as either a s a n acid or a s a base. amphiprotic substance Hydrolysis the reaction of a salt with water. Equivalence point of is the point at which the acid /base has completely reacted with the a titration base/acid. Endpoint of a titration is the point where the indicator changes colour. Kw the equilibrium constant for the ionisation of water or the ionic product of + - 14 water or the ionisation constant of water, i.e. K w = [H 3 O ][OH ] = 1 x 10 by 298 K. auto-ionisation of + - the reaction of water with itself to form H 3 O ions and OH ions. water https://tvetpapers.co.za

https://ultradeep.co.za Electrochemical Reactions Galvanic cell a cell in which chemical energy is converted into electrical energy. A galvanic (voltaic) cell has self-sustaining electrode reactions Electrolytic cell a cell in which electrical energy is converted into chemical energy. i.t o. e- transfer Oxidation a loss of electrons. Reduction a gain of electrons. i.t.o oxidation nrs: Oxidation An increase in oxidation number Reduction A decrease in oxidation number Oxidising agent A substance that is reduced/gains electrons. Reducing agent A substance that is oxidised/loses electrons. Anode The electrode where oxidation takes place Cathode The electrode where reduction takes place an electrolyte a solution/liquid/dissolved substance that conducts electricity through the movement of ions Electrolysis The chemical process in which electrical energy is converted to chemical energy OR the use of electrical energy to produce a chemical change. Chemical Industry The fertiliser industry (N, P, K) eutrophication is the process by which an ecosystem, e.g. a river or dam, becomes enriched with inorganic plant nutrients, especially phosphorus and nitrogen, resulting in excessive plant growth. As plant growth becomes excessive, the amount of dead and decaying plant material increases rapidly. https://tvetpapers.co.za

https://ultradeep.co.za 4. GENERAL INFORMATION 4.1 Quantities, symbols and units The most common quantities, symbols and SI units used in introductory Physics are listed below. A quantity should not be confused with the units in which it is measured. Preferred Alternative Unit Quantity Unit name symbol symbol symbol mass m kilogram kg position x, y metre m displacement  x,  y s metre m -1 velocity vx , vy u, v metre per second m∙s -1 initial velocity vi u metre per second m∙s -1 final velocity vf v metre per second m∙s -2 acceleration a metre per second per second m∙s acceleration due to -2 g metre per second per second m∙s gravity time (instant) t second s time interval t second s energy E joule J kinetic energy K Ek joule J potential energy U Ep joule J work W joule J work function W0 joule J power P watt W -1 momentum p kilogram metre per second kg∙m∙s force F newton N weight w Fg newton N normal force N FN newton N tension T FT newton N friction force f Ff newton N coefficient of friction μ, μ s , μ k (none) torque τ newton metre N∙m wavelength λ metre m frequency f ν hertz or per second Hz or s -1 period T second s -1 speed of light c metre per second m∙s refractive index n (none) focal length f metre m object distance s u metre m image distance s' v metre m magnification m (none) charge Q, q coulomb C -1 newton per coulomb or N∙C or electric field E -1 volt per metre V∙m electric potential at VP volt V point P potential difference  V, V volt V emf E ε volt V current I, i ampere A resistance R ohm Ω internal resistance r ohm Ω magnetic field B tesla T 2 2 T∙m or magnetic flux Φ tesla∙metre or weber Wb Copyright reserved https://tvetpapers.co.za