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Doc Brown's
Chemistry Cambridge 0652 IGCSE
Physical
Science
Helps the
CHEMISTRY of the
Cambridge IGCSE Physical Science 0652 CIE
syllabus-specification
Cambridge International
Certificate of Education (ICE) For examination in November
2012 and November 2013
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CHEMISTRY 0652 Curriculum core
content and supplements
It is important that, throughout this section, attention should be drawn to:
the finite life of the worlds resources and hence the need for recycling and conservation
economic considerations in the chemical industry, such as the availability and cost of raw materials and energy the importance of chemicals in industry and in everyday life. C1.The particulate nature of matter 1 describe the states of matter and explain their interconversion in terms of the kinetic particle theory 2 describe diffusion and Brownian motion in terms of kinetic theory
C2. Experimental techniques 1 name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders 2 describe paper chromatography (including the use of locating agents) and interpret simple chromatograms 3 recognise that mixtures melt and boil over a range of temperatures 4 describe methods of purification by the use of a suitable solvent, filtration, crystallisation, distillation (including use of fractionating column. Refer to the fractional distillation of crude oil (petroleum section 11.2) and fermented liquor (section 11.6)
C3. Atoms, elements and compounds
3.1 Atomic structure and the Periodic Table
1 state the relative charge and approximate
relative mass of a proton, a neutron and an
electron
2 define proton number and nucleon number
3 use proton number and the simple structure
of atoms to explain the basis of the Periodic
Table (section 7.1 to 7.4), with special
reference to the elements of proton number
1 to 20
4 use the notation abX for an atom
5 describe the build-up of electrons in 'shells'
and understand the significance of the
noble gas electronic structures and of outer
electrons
The ideas of the distribution of electrons
in s- and p-orbitals and in d-block elements
are not required.
Note that a copy of the
Periodic Table, will be provided in Papers 1, 2
and 3.
6 define isotopes
3.2 Bonding: the structure of matter
1 describe the differences between elements,
mixtures and compounds, and between
metals and non-metals (section 7.1)
2 describe alloys, such as brass, as mixtures of a metal with other elements
3 explain how alloying affects the properties
of metals (see 3.2 (d))
3.2(a) Ions and ionic bonds
1 describe the formation of ions by electron loss or gain describe the formation of ionic bonds between the alkali metals and the
halogens
2 describe the formation of ionic bonds between metallic and non-metallic elements
3.2(b) Molecules and covalent bonds
1 describe the formation of single covalent
bonds in H2, Cl2, H2O, CH4 and HCl as the
sharing of pairs of electrons leading to the
noble gas configuration
2 describe the electron arrangement in more complex covalent molecules such as N2, C2H2, CH3OH and CO2
3 describe the differences in volatility, solubility
and electrical conductivity between ionic and
covalent compounds
3.2 (c) Macromolecules
1 describe the structure of graphite and of
diamond
2 relate these structures to melting point,
conductivity and hardness
3.2 (d) Metallic bonding
1 describe metallic bonding as a lattice
of positive ions in a 'sea of electrons'
and use this to explain the electrical
conductivity and malleability of metals
C4. Stoichiometry 1 use the symbols of the elements and write
the formulae of simple compounds 2 determine the formula of an ionic
compound from the charges on the ions
present 3 deduce the formula of a simple compound
from the relative numbers of atoms present 4 deduce the balanced equation of
a chemical reaction, given relevant
information 5 construct word equations and simple
balanced chemical equations 6 define relative atomic mass, Ar 7 define relative molecular mass, Mr , and
calculate it as the sum of the relative atomic
masses (the term relative formula mass or
Mr will be used for ionic compounds) 8 calculate stoichiometric reacting masses
and volumes of gases and solutions,
solution concentrations expressed in
g/dm3 and mol/dm3 Calculations
based on limiting reactants may be
set; questions on the gas laws and
the conversion of gaseous volumes to
different temperatures and pressures will
not be set.
C5. Chemical reactions
5.1 Production of energy
1 describe the production of heat energy by
burning fuels
2 describe hydrogen as a fuel
3 describe radioactive isotopes, such as
235U,
as a source of energy
5.2 Energetics of a reaction
1 describe the meaning of exothermic and
endothermic reactions
2 describe bond breaking as endothermic and
bond forming as exothermic
Notes on Energy changes-transfers in
Chemical Reactions -
Exothermic and
endothermic energy changes
5.3 Speed of reaction
1 describe the effects of concentration, particle size, catalysts (including enzymes) and temperature on the speeds of reactions
2 show awareness that light can provide the energy needed for a chemical reaction to occur
3 state that organic compounds that catalyse organic reactions are called enzymes
4 state that photosynthesis leads to the production of glucose from carbon dioxide and water in the presence of chlorophyll and sunlight (energy)
5 describe the application of the above factors to the danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. mines)
6 describe the use of silver salts in photography (i.e. reduction of silver ions to silver)
5.4 Redox
1 define oxidation and reduction in terms of
oxygen gain / loss
Introduction to
OXIDATION
and REDUCTION and their application to REDOX reactions
C6. Acids, bases and salts
6.1 The characteristics properties of acids and bases
1 describe the characteristic properties of acids
as reactions with metals, bases, carbonates
and effect on litmus
2 define acids and bases in terms of proton
transfer, limited to aqueous solutions
3 describe neutrality, relative acidity and
alkalinity in terms of pH (whole numbers
only) measured using Universal Indicator
paper
4 use these ideas to explain specified
reactions as acid/base
5 describe and explain the importance of the
use of lime in controlling acidity in soil
6.2 Types of oxides
1 classify oxides as either acidic or basic,
related to metallic and non-metallic character
of the element forming the oxide
2 classify other oxides as neutral or
amphoteric
6.3 Preparation of salts
1 describe the preparation, separation and
purification of salts as examples of some of
the techniques specified in section 2 and the
reactions specified in section 6.1
2 suggest a method of making a given
salt from suitable starting materials,
given appropriate information, including
precipitation
6.4 Identification of ions
1 describe the use of the following tests to
identify:
aqueous cations:
ammonium, copper(II), iron(II), iron(III)
and zinc, using aqueous sodium
hydroxide and aqueous ammonia as
appropriate. (Formulae of complex ions
are not required.)
anions:
carbonate (by reaction with dilute acid
and then limewater), chloride (by reaction
under acidic conditions with aqueous
silver nitrate), nitrate (by reduction with
aluminium to ammonia) and sulfate (by
reaction under acidic conditions with
aqueous barium ions)
6.5 Identification of gases 1 describe the use of the following tests to
identify: ammonia (using damp red litmus
paper), carbon dioxide (using limewater),
chlorine (using damp litmus paper), hydrogen
(using a lighted splint), oxygen (using a
glowing splint)
See also Appendix
below for sections 6.4 and 6.5
Appendix - Summary of test results for chemical identification
Tests for anions - anion test and results
carbonate (CO32) add dilute acid effervescence, carbon dioxide
produced
chloride (Cl)
[in solution]
acidify with dilute nitric acid, then add
aqueous silver nitrate
white ppt.
nitrate (NO3)
[in solution]
add aqueous sodium hydroxide, then
aluminium foil; warm carefully
ammonia produced
sulfate (SO42)
[in solution]
acidify with dilute nitric acid, then add
aqueous barium nitrate
white ppt.
Tests for aqueous cations
cation effect of aqueous sodium hydroxide (NaOH(aq)) and effect of aqueous ammonia (NH3(aq))
NaOH(aq) - ammonium (NH4+) ammonia produced on warming
NaOH(aq) - copper(II) (Cu2+) light blue ppt., insoluble in excess
NH3(aq) - copper(II) (Cu2+) light blue ppt., soluble in excess,
giving a dark blue solution
NaOH(aq)/NH3(aq) - iron(II) (Fe2+) green ppt., insoluble in excess
NaOH(aq)/NH3(aq) - iron(III) (Fe3+) red-brown ppt., insoluble in excess
NaOH(aq)/NH3(aq) - zinc (Zn2+) white ppt., soluble in excess, giving a
colourless solution
Tests for gases
gas test and test result
ammonia (NH3) turns damp red litmus paper blue
carbon dioxide (CO2) turns lime water milky
chlorine (Cl2) bleaches damp litmus paper
hydrogen (H2) pops with a lighted splint
oxygen (O2) relights a glowing splint
C7.The Periodic Table 1 describe the Periodic Table as a method of
classifying elements and describe its use in
predicting properties of elements
7.1 Periodic trends
1 describe the change from metallic to
non-metallic character across a Period
2 describe the relationship between
group number and the number of outer
electrons
7.2 Group properties
1 describe lithium, sodium and potassium
in Group I as a collection of relatively soft
metals showing a trend in melting point,
density and reaction with water
2 predict the properties of other elements in
the group given data, where appropriate
3 describe chlorine, bromine and iodine
in Group VII as a collection of diatomic
non-metals showing a trend in colour, and
state their reaction with other halide ions
4 predict the properties of other elements in
the group given data, where appropriate
5 identify trends in other groups given data
about the elements concerned
7.3 Transition elements
1 describe the transition elements as a
collection of metals having high densities,
high melting points and forming coloured
compounds, and which, as elements and
compounds, often act as catalysts
7.4 Noble gases
1 describe the noble gases as being unreactive
2 describe the uses of the noble gases in
providing an inert atmosphere (e.g. argon in
lamps and helium for filling weather balloons)
C8. Metals
8.1 Properties of metals
1 compare the general physical and chemical
properties of metals with those of
non-metals
8.2 Reactivity series
1 place in order of reactivity: calcium, copper,
(hydrogen), iron, magnesium, potassium,
sodium and zinc, by reference to the
reactions, if any and where relevant, of the
metals with
water or steam,
dilute hydrochloric acid (equations not
required)
the aqueous ions of other metals
2 account for the apparent unreactivity of
aluminium in terms of the oxide layer
adhering to the metal
3 deduce an order of reactivity from a given
set of experimental results
8.3 (a) Extraction of metals
1 describe the ease in obtaining metals from
their ores by relating the elements to the
reactivity series
2 describe the essential reactions in the extraction of iron from haematite
3 name metals that occur native, including
copper and gold
4 name the main ores of aluminium, copper
and iron
8.3 (b) Uses of metal
1 describe the idea of changing the properties
of iron by the controlled use of additives to
form steel alloys
2 name the uses, related to their properties,
of copper (electrical wiring and in cooking
utensils) and of aluminium (aircraft parts
and food containers)
3 name the uses of mild steel (car bodies and
machinery) and stainless steel (chemical
plant and cutlery)
4 name the uses of zinc for galvanising and
making brass
C9. Air and water 1 describe a chemical test for water 2 show understanding that hydration may be
reversible (e.g. by heating hydrated copper(II)
sulfate or hydrated cobalt(II) chloride) 3 describe, in outline, the purification of
the water supply in terms of filtration and
chlorination 4 name some of the uses of water in industry
and in the home 5 describe the composition of clean air as
being approximately 78% nitrogen, 21%
oxygen and the remainder as being a mixture
of noble gases, water vapour and carbon
dioxide 6 name the common pollutants in the air
as being carbon monoxide, sulfur dioxide,
oxides of nitrogen and lead compounds 7 state the source of each of these pollutants: carbon monoxide from the incomplete
combustion of carbon-containing
substances sulfur dioxide from the combustion
of fossil fuels which contain sulfur
compounds (leading to 'acid rain') oxides of nitrogen and lead compounds
from car exhausts
8 explain the catalytic removal of nitrogen
oxides from car exhaust gases 9 state the adverse effect of common
pollutants on buildings and on health 10 describe the separation of oxygen and
nitrogen from liquid air by fractional
distillation 11 name the uses of oxygen in oxygen tents in
hospitals, and with acetylene (a hydrocarbon)
in welding 12 describe methods of rust prevention: paint and other coatings, to exclude
oxygen galvanising
13 explain galvanising in terms of the reactivity of zinc and iron 14 describe the need for nitrogen-,
phosphorous- and potassium-containing
fertilisers 15 describe the formation of carbon dioxide: as a product of complete combustion of
carbon-containing substances as a product of respiration as a product of the reaction between an
acid and a carbonate
C10. Lime and limestone 1 describe the manufacture of calcium oxide
(lime) from calcium carbonate (limestone) in
terms of the chemical reactions involved 2 name some uses of lime and calcium
hydroxide (slaked lime) as in treating acidic
soil and neutralising acidic industrial waste
products
C11. Organic chemistry
11.1 Names of compounds
1 name, and draw, the structures of methane,
ethane, ethanol, ethanoic acid and the
products of the reactions stated in sections
11.4 to 11.6
2 state the type of compound present, given
a chemical name ending in -ane, -ene, -ol, or
-oic acid or a molecular structure
11.2 Fuels
1 name the fuels coal, natural gas and
petroleum
2 name methane as the main constituent of
natural gas
3 describe petroleum as a mixture of
hydrocarbons and its separation into useful
fractions by fractional distillation
4 name the uses of the fractions:
petrol fraction as fuel in cars
paraffin fraction for oil stoves and aircraft
fuel
diesel fraction for fuel in diesel engines
lubricating fraction for lubricants and
making waxes and polishes
bitumen for making roads
11.3 Homologous series
1 describe the concept of homologous series
as a 'family' of similar compounds with
similar properties due to the presence of the
same functional group
11.4 Alkanes
1 describe the properties of alkanes
(exemplified by methane) as being generally
unreactive, except in terms of burning
11.5 Alkenes
1 describe the properties of alkenes in terms
of addition reactions with bromine, hydrogen
and steam
2 describe the manufacture of alkenes and
of hydrogen by cracking
3 distinguish between saturated and
unsaturated hydrocarbons from molecular
structures, by simple chemical tests
4 describe the formation of poly(ethene) as
an example of addition polymerisation of
monomer units
11.6 Alcohols
1 name the uses of ethanol: as a solvent, as a
fuel and as a constituent of wine and beer
2 describe the formation of ethanol by
fermentation and by the catalytic addition
of steam to ethene
PHYSICS 0652 Curriculum Core Content and Supplements Throughout this section, attention should be paid to showing the relevance of concepts to the students
everyday life and to the natural and man-made world. P1. General physics
1.1 Length and time
1 use and describe the use of rules and measuring
cylinders to determine a length or a volume
2 use and describe the use of
a mechanical method for the
measurement of a small distance
3 use and describe the use of clocks and devices for
measuring an interval of time
4 measure and describe how to
measure a short interval of time
(including the period of a pendulum)
1.2 Speed, velocity and acceleration
1 define speed and calculate speed from
total time
total distance
2 distinguish between speed and
velocity
3 plot and interpret a speed / time graph
4 recognise linear motion for which
the acceleration is constant and
calculate the acceleration
5 recognise from the shape of a speed / time graph
when a body is:
at rest
moving with constant speed
moving with changing speed
6 recognise motion for which the
acceleration is not constant
7 calculate the area under a speed / time graph to
determine the distance travelled for motion with
constant acceleration
8 demonstrate some understanding that acceleration
is related to changing speed
9 state that the acceleration of free fall for a body near
to the Earth is constant
10 describe qualitatively the motion
of bodies falling in a uniform
gravitational field with and without
air resistance (including reference
to terminal velocity)
1.3 Mass and weight
1 show familiarity with the idea of the mass
of a body
2 demonstrate an understanding that mass is a property which 'resists' change in motion
3 state that weight is a force
4 calculate the weight of a body from its
mass
5 demonstrate understanding that weights
(and hence masses) may be compared
using a balance
6
describe, and use the concept of, weight as the effect of a gravitational field on a mass
1.4 Density
1 describe an experiment to determine the
density of a liquid and of a regularly shaped
solid, and make the necessary calculation
2 describe the determination of the density
of an irregularly shaped solid by the method
of displacement
1.5 Forces
1.5 (a) Effects of forces
1 state that a force may produce a change in
size and shape of a body
2 take readings from and interpret extension load graphs (Hooke's law, as such, is not required)
3 plot extension-load graphs and describe the
associated experimental procedure
4 recognise the significance of the term 'limit of proportionality' for an extension-load graph and use proportionality in simple calculations
5 describe the ways in which a force may
change the motion of a body
6
recall and use the relation between force, mass and acceleration (including the direction)
1.5 (b) Turning effect
1 describe the moment of a force as a
measure of its turning effect and give
everyday examples
2 perform and describe an experiment
(involving vertical forces) to verify that there
is no net moment on a body in equilibrium
1.5 (c) Centre of mass
1 calculate the moment of a force given the
necessary information
2 perform and describe an experiment to
determine the position of the centre of
mass of a plane lamina
3 describe qualitatively the effect of the
position of the centre of mass on the
stability of simple objects
1.6 Energy, work and power
1.6 (a) Energy
1 give examples of energy in different forms, its conversion and conservation and apply the principle of energy conservation to simple examples
2 describe energy transfer in terms of work done and make calculations involving F Χ d
3 show some understanding of energy of motion and energy of position (i.e. gravitational and strain)
4 use the terms kinetic and potential energy in context
5 recall and use the expressions:
k.e. = ½ mv2
p.e. = mgh
1.6 (b) Major sources of energy and alternative sources of energy
1 describe processes by which energy
is converted from one form to another,
including reference to:
chemical/fuel energy (a regrouping of
atoms)
energy from water (hydroelectric
energy, waves, tides)
geothermal energy
nuclear energy (fission of heavy atoms)
solar energy (fusion of nuclei of atoms in the Sun)
recall and use the mass/energy equation
E = mc2
2 express a qualitative understanding of
efficiency
1.6 (c) Work
1 relate, without calculation, work done to the
magnitude of a force and distance moved
2 recall and use the formula ΔW = F Χ d = ΔE
1.6 (d) Power
1 relate, without calculation, power to work
done and time taken, using appropriate
examples
2 recall and use the equation P = E / t in
simple systems
P2. Thermal physics
2.1 Thermal properties
2.1 (a) Thermal expansion of solids, liquids and gases
1 describe qualitatively the thermal expansion of solids, liquids and gases
2 show an appreciation of the relative order of magnitude of the expansion of solids,
liquids and gases
3 identify and explain some of the everyday
applications and consequences of thermal
expansion
2.1 (b) Measurement of temperature
1 appreciate how a physical property which varies with temperature may be used for the measurement of temperature and state examples of such properties
2 apply a given property to the measurement of temperature
3 demonstrate understanding of sensitivity, range and linearity
4 recognise the need for and identify a fixed
point
5 describe the structure and action of liquid-in-glass thermometers
6
describe the structure and action of a thermocouple and show understanding of its use for measuring high temperatures and those which vary rapidly
2.1 (c) Melting and boiling
1 describe melting and boiling in terms
of energy input without a change in
temperature
2 distinguish between boiling and evaporation
3 state the meaning of melting point and
boiling point
2.2 Transfer of thermal energy
2.2 (a) Conduction
1 describe experiments to demonstrate the
properties of good and bad conductors of
heat
2 give a simple molecular account of the heat
transfer in solids
2.2 (b) Convection
1 relate convection in fluids to density
changes and describe experiments to
illustrate convection
2.2 (c) Radiation
1 identify infra-red radiation as part of the
electromagnetic spectrum
2 describe experiments to show the
properties of good and bad emitters
and good and bad absorbers of infra-red
radiation
2.2 (d) Consequences of energy transfer
1 identify and explain some of the everyday
applications and consequences of
conduction, convection and radiation
P3. Properties of waves, including light and sound
3.1 General wave properties
1 describe what is meant by wave motion as
illustrated by vibration in ropes, springs and
by experiments using water waves
2 use the term wavefront
3 give the meaning of speed, frequency,
wavelength and amplitude
4 recall and use the equation c = f λ
5 describe the use of water waves to show
reflection at a plane surface
refraction due to a change of speed
6
interpret reflection, refraction and
diffraction using wave theory
3.2 Light
3.2 (a) Reflection of light
1 describe the formation, and give the
characteristics, of an optical image formed
by a plane mirror
2 perform simple constructions,
measurements and calculations
3 use the law
angle of incidence = angle of
reflection
3.2 (b) Refraction of light
1 describe the refraction, including angle of
refraction, in terms of the passage of light
through a parallel sided glass block
2 determine and calculate refractive index
using n = sin i / sin r
3.2 (c) Thin converging lens
1 describe the action of a thin converging
lens on a beam of light
2 use and describe the use of a single lens as
a magnifying glass
3 use the term focal length
3.2 (d) Electromagnetic spectrum
1 describe the main features of the
electromagnetic spectrum and state that
all e.m. waves travel with the same high
speed in vacuo
2 state the approximate value of the speed of
electromagnetic waves
3 use the term monochromatic
3.3 Sound
1 describe the production of sound by
vibrating sources
2 state the approximate range of audible
frequencies
3 show an understanding that a medium is
required in order to transmit sound waves
P4. Electricity and magnetism
4.1 Simple phenomena of magnetism
1 state the properties of magnets
2 give an account of induced magnetism
3 distinguish between ferrous and
non-ferrous materials
4 describe an experiment to identify the
pattern of field lines round a bar magnet
5 distinguish between the magnetic
properties of iron and steel
6 distinguish between the design and use of
permanent magnets and electro-magnets
4.2 Electrostatics
1 describe simple experiments to show the
production and detection of electrostatic
charges
4.2 (a) Electric charge
1 state that there are positive and negative
charges
3 state that unlike charges attract and that
like charges repel
2 state that charge is measured in coulombs
4.3 Electricity
1 state that current is related to the flow of
charge
2 show understanding that a current is a rate
of flow of charge and recall and use the
equation
I = Q / t
4.3 (a) Current
1 use and describe the use of an ammeter
4.3 (b) Electro-motive force (e.m.f.)
1 state that the e.m.f. of a source of electrical
energy is measured in volts
2 show understanding that e.m.f. is defined
in terms of energy supplied by a source in
driving charge round a complete circuit
4.3 (c) Potential difference (p.d.)
1 state that the potential difference across a
circuit component is measured in volts
2 use and describe the use of a voltmeter
4.3 (d) Resistance
1 recall and use the equation V = IR
2 recall and use quantitatively the
proportionality between resistance and
the length, and the inverse proportionality
between resistance and cross-sectional
area, of a wire
3 describe an experiment to determine
resistance using a voltmeter and an
ammeter
4 relate (without calculation) the resistance of
a wire to its length and to its diameter
4.3 (e) V/I characteristic graphs
1 sketch the V / I characteristic graphs for
metallic (ohmic) conductors
4.4 Electric circuits
1 draw and interpret circuit diagrams
containing sources, switches, resistors
(fixed and variable), ammeters, voltmeters,
magnetising coils, bells, fuses, relays
2 draw and interpret circuit diagrams containing diodes as rectifiers
3 understand that the current at every point
in a series circuit is the same
4 recall and use the fact that the sum of the p.d.'s across the components in a series circuit is equal to the total p.d. across the supply
5 give the combined resistance of two or
more resistors in series
6 state that, for a parallel circuit, the current
from the source is larger than the current in
each branch
7 recall and use the fact that the current from the source is the sum of the currents in the separate branches of a parallel circuit
8 state that the combined resistance of two
resistors in parallel is less than that of
either resistor by itself
9
calculate the effective resistance of two resistors in parallel
4.5 Practical electric circuitry
4.5 (a) Uses of electricity
1 describe the uses of electricity in heating,
lighting (including lamps in parallel), motors
2 recall and use the equations
P = I x
V and E = I x V x t
and their alternative forms
4.5 (b) Safety considerations
1 state the hazards of
damaged insulation
overheating of cables
damp conditions
4.6 Electromagnetic effects
4.6 (a) Electromagnetic induction
1
describe an experiment which shows that
a changing magnetic field can induce an
e.m.f. in a circuit
2 state the factors affecting the magnitude of
the induced e.m.f.
3 show understanding that the direction of
an induced e.m.f. opposes the change
causing it
4.6 (b) a.c. generator
1
describe a rotating-coil generator and the
use of slip rings
2 sketch a graph of voltage output against
time for a simple a.c. generator
4.6 (c) d.c. motor
1 state that a current-carrying coil in a
magnetic field experiences a turning
effect and that the effect is increased by
increasing the number of turns on the coil
2 describe the effect of increasing the current
3 relate this turning effect to the action of an
electric motor
4.6 (d) Transformer
1 describe the construction of a basic
iron-cored transformer as used for voltage
transformations
2 show an understanding of the principle of
operation of a transformer
3 use the equation
(Vp / Vs) = (Np / Ns)
4 recall and use the equation
Vp Ip = Vs Is (for 100% efficiency)
5 show understanding of energy loss in
cables (calculation not required)
6 describe the use of the transformer in
high-voltage transmission of electricity
7 advantages of high voltage transmission
4.7 Cathode rays and the cathode-ray oscilloscope (c.r.o.)
4.7 (a) Cathode rays
1 describe the production and detection of
cathode rays
2 distinguish between the direction of
electron current and conventional current
3 describe their deflection in electric fields
and magnetic fields
4 deduce that the particles emitted in
thermionic emission are negatively charged
5 state that the particles emitted in
thermionic emission are electrons
4.7 (b) Simple treatment of cathode-ray oscilloscope
1 describe in outline the basic structure,
and action, of a cathode-ray oscilloscope
(detailed circuits are not required)
2 use and describe the use of a c.r.o. to
measure p.d.s and short intervals of time
(detailed circuits are not required)
3 use and describe the use of a cathode-ray
oscilloscope to display waveforms
P5. Atomic physics
5.1 Radioactivity
5.1 (a) Detection of radioactivity
1 show awareness of the existence of
background radioactivity
2 describe the detection of alpha-particles,
beta-articles and gamma-rays
5.1 (b) Characteristics of the three kinds of emission
1 state that radioactive emissions occur
randomly over space and time
2 state, for radioactive emissions:
their nature
their relative ionising effects
their relative penetrating abilities
3 describe their deflection in electric fields
and magnetic fields
5.1 (c) Radioactive decay
1 state the meaning of radioactive decay,
using word equations to represent changes
in the composition of the nucleus when
particles are emitted
5.1 (d) Half-life
1 use the term half-life in simple calculations
which might involve information in tables or
decay curves
5.1 (e) Safety precautions
1 describe how radioactive materials are
handled, used and stored in a safe way
5.2 The nuclear atom
5.2 (a) Nucleus
1 describe the composition of the nucleus in
terms of protons and neutrons
2 use the term proton number, Z
3 use the term nucleon number, A
4 use the term nuclide and nuclide notation
AZX
5 use the nuclide notation in equations to
show alpha and beta decay
5.2 (b) Isotopes
1 use the term isotopes
2 give and explain examples of practical
applications of isotopes
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B C D
E F
G H I J K L M
N O P
Q R
S T
U V W
X
Y Z |
