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Chemistry
Communal knowledge
Pure substances and mixtures
The candidate can
sb1 indicate what is meant by:
• a pure substance;
• a mixture.
sb2 indicate what is meant by phase transitions:
• condensation and evaporation;
• deposition and sublimation;
• solidification and melting.
sb3 indicate in which way a mixture can be distinguished from a pure substance:
• melting point /boiling point;
• melting range / boiling range.
sb4 list a number of types of mixtures and indicate what their properties are:
• solution;
• suspension;
• emulsion;
• alloy.
sb5 list a number of separation techniques / purification techniques, indicate to which type of
mixture the technique can be applied and indicate on which principles these techniques
are founded:
• extraction;
• absorption;
• distillation, the concepts of distillate and residue;
• filtration, the concepts of filtrate and residue;
• centrifugation;
• precipitation;
• evaporation;
• paper chromatography.
Elements and compounds
The candidate can
sb6 indicate what is meant by:
• an element as atomic species;
• an element as a non-decomposable substance;
• a compound as decomposable substance.
sb7 give the symbols of the following elements when the name has been given and the other
way around and indicate whether the element is a metal or nonmetal:
• hydrogen, helium, carbon, nitrogen, oxygen, fluorine, neon, sodium, magnesium,
aluminium, silicon, phosphorous, sulfur, chlorine, argon, potassium, calcium, iron,
nickel, copper, zinc, bromine, silver, tin, iodine, barium, platinum, gold, mercury,
lead, uranium.
sb8 give the formulas of the following substances when the name has been given and the
other way around:
• ammonia, bromine, carbon dioxide, carbon monoxide, chlorine, 'fizz', fluorine,
glucose, hydrogen, hydrogen chloride, hydrogen peroxide, iodine, nitrogen,
oxygen, ozone, nitric acid, sulfur dioxide, sulfuric acid, water.
sb9 give and interpret names and formulas of salts that are composed from the following
ions:
• Ag+, Al3+, Ba2+, Ca2+, Cu2+, Fe2+ , Fe3+ , Hg2+ , K+ , Na+ , NH4+ , Mg2+ , Pb2+ , Sn2+ , Zn2+
• Br—, CH3COO—, Cl—, F—, HCO3—, I—, O2— , OH— , NO2—, NO3— , PO43— , S2— , SO42— ,
SO32—
sb10 interpret the following state symbols:
• (s);
• (l);
• (g);
• (aq);
Atom structure
The candidate can
sb11 describe the structure of atoms and ions, using the concepts of atom core, proton,
neutron, core charge, atomic number, mass number, isotope, electron, electron cloud,
ionic charge.
Reactions
The candidate can
sb12 indicate what is meant by a chemical reaction:
• reactants;
• reaction products;
• law of conservation of matter;
• law of conservation of mass.
sb13 indicate what is meant by a decomposition reaction:
• thermolysis;
• electrolysis;
• photolysis.
sb14 indicate what is meant by a combustion reaction:
• complete and incomplete combustion;
• ignition temperature.
sb15 indicate that chemical reactions are accompanied by a heat effect:
• exothermic;
• endothermic.
sb16 indicate for a number of substances how their presence can be detected:
• reagent;
• detecting the presence of oxygen, hydrogen, water, carbon dioxide, sulfur dioxide.
Acids and bases
The candidate can
sb17 recognise the following substances/solutions as an acid/acidic solution:
• hydrogen chloride/hydrochloric acid;
• sulfuric acid/sulfuric acid solution;
• nitric acid/nitric acid solution;
• carbon dioxide/carbon dioxide solution;
• ethanoic acid, acetic acid/vinegar.
sb18 recognise the following particles as bases:
• hydroxide ions;
• oxide ions;
• carbonate ions;
• ammonia molecules.
Domain B: Substances, structure and bonds
Subdomain B2: Processes/reactions
The candidate can describe the solution and precipitation of salts and indicate for which
purposes precipitation reactions can be applied.
The candidate can:
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using a solubility chart indicate how via precipitation reactions:
• ions can be removed from a solution;
• the presence of certain ions can be detected;
• a certain satt can be prepared;
• ions can react with each other in a solution.
describe the solution of salts in water as the disintegration of the crystal structure and the
hydration of ions.
Subdomain B4: Types of bonds and properties
For a number of bonds the candidate can indicate how they are formed and which properties
these bonds have.
The candidate can:
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indicate whether a substance consists of ions, atoms, or molecules.
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indicate how the following types of bonds are formed and indicate which of those bond
types is/are present in a salt, a molecular substance (both polar and nonpolar), a
substance with an atomic lattice, or a metal:
• atom bond or covalent bond;
• polar bond;
• hydrogen bond;
• van der Waals bond;
• ion bond;
• metallic bond;
• dipole-dipole bond.
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indicate that ions can form bonds with water molecules and that this process is
reversible;
• hydration;
• salt hydrates;
• crystallisation water, using the notation · n H2O.
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using data to explain which type of crystal lattice a substance will have:
• atomic lattice;
• molecular lattice;
• ionic lattice;
• metallic lattice.
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make a connection between bond types, lattice type, and the properties of a substance:
• melting point and boiling point;
• hardness and brittleness;
• absence or presence of electrical conductivity in the solid, liquid, and/or dissolved
state,
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indicate how the strength of intermolecular bonds corresponds to the melting point or the
boiling point respectively of a molecular substance:
• van der Waals bond;
• dipole-dipole bond;
• hydrogen bond.
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indicate which molecular substances dissolve and which do not, given that the structure
of the molecules and the bond type present generally mix well, using the concepts:
• nonpolar/polar;
• hydrophobic/hydrophilic;
• hydrogen bonds.
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make the connection between the spatial structure of a molecule and the single, double,
or triple atomic bonds present in the molecule:
• tetrahedron (bond angles . 109°);
• plane (bond angles . 120°);
• linear (bond angles . 180°).
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using sources and the concept of electronegativity, make a qualitative prediction about
the polarity of a bond.
Domain C: Carbon chemistry
Subdomain C2: Other applications of carbon bonds
Subdomain C3:
The candidate can indicate for a number of carbon bonds which types of reactions they can
undergo and which products are then formed.
The candidate can:
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describe the reaction of alkenes and other unsaturated compounds with the following
substances as an addition reaction, give the possible products of the reaction, and give
the corresponding reaction equations in structural formulas:
• hydrogen;
• water;
• hydrogen halides;
• halogens, either dissolved or undissolved.
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indicate how the suspected presence of an unsaturated compound can be detected.
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indicate which types of alcohols (primary, secondary, tertiary) can react with an oxidising
agent, which products can be formed, and give the corresponding reaction equations in
structural formulas.
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indicate that carboxylic acids and phenol react as an acid and amines as a base and that
amino acids are ampholytes.
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indicate that from an alcohol and an acid an ester and water can be formed and give the
corresponding reaction equation in structural formulas:
• equilibrium reaction;
• H+ as a catalyst;
• glyceryl trinitrate;
• fats.
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describe how the cleansing action of soap can be explained.
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indicate how esters can by hydrolysed, which products can be formed in this hydrolysis,
and give the corresponding reaction equation in structural formulas:
• equilibrium reaction.
48
indicate which two types of polymerisation can be distinguished and in what ways these
are different:
• chain-growth polymerisation;
• condensation polymerisation.
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in molecular and structural formulas of monomers and polymers describe the
polymerisation process of:
• ethene;
• vinyl chloride;
• propene;
• styrene;
• isoprene.
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distinguish polymers based an their behaviour in thermoplastics and thermosets.
Subdomain C4: Structures of carbon compounds
The candidate can apply the IUPAC nomenclature to a number of types of carbon compounds
and recognise different types of isomerism.
The candidate can:
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indicate what a structural formula is.
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derive a molecular formula from a structural formula.
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recognise and name a number of features of a structural formula:
• carbon chain
• carbon skeleton
• alkyl groups: methyl and ethyl;
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• functional group;
• substituent;
• single bond;
• double bond;
• triple bond;
• primary, secondary, tertiary carbon atom;
• asymmetric carbon atom.
recognise and name structural characteristics of a carbon skeleton:
• branched;
• unbranched;
• cyclic;
• acyclic;
• aliphatic;
• aromatic;
• saturated;
• unsaturated.
indicate in which cases the rotation of a bond between carbon atoms is restricted.
derive the special structure of molecules from the carbon skeleton:
• configuration;
• tetrahedron.
make a connection between the general formula of a homologous series and the
corresponding structural formulas.
derive from the systematic name (IUPAC) the structural formula of a number of carbon
compounds whose main chain in the molecules consists of a maximum of 6 carbon
atoms:
• alkanes;
• alkenes;
• cycloalkanes;
• alkynes;
• halogen alkanes;
• alkanols;
• alkoxy alkanes;
• alkanals;
• alkanones;
• alkanoic acids;
• alkylalkanoates;
• alkane amines.
derive from the systematic name (IUPAC) the structural formula of a number of carbon
compounds whose main chain in the molecules consists of a maximum of 6 carbon
atoms and the molecules contain 2 or more of the following groups:
• C=C (no more than 3 groups);
• halogen (no more than 4 halogen atoms);
• OH;
• C=O: aldehyde, ketone, carboxylic acid (no more than 2 groups);
• NH2.
indicate for carbon compounds to which super class of compounds these belong and
indicate the functional groups:
• hydrocarbons;
• saturated and unsaturated compounds;
• aliphatic compounds;
• ethers;
• primary, secondary, and tertiary alcohols/hydroxyl group;
• aldehydes;
• ketones;
• carboxylic acids;
• fatty acids;
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• esters;
• amines/amino group;
• amino acids.
derive the structural formulas from a number of aromatic compounds from the systematic
name (IUPAC):
• benzene;
• alkyl benzenes;
• halogen benzenes;
• benzenol/phenol;
• benzenecarboxylic acids.
indicate that substances can also have trivial names besides systematic names and use
these alongside each other.
derive the structural formula of the monomer from the structural formula or name of a
number of addition polymers and the other way around:
• polymers from alkenes and substituted alkenes;
• polybutadiene;
• natural rubber.
from the structural formula or name of a number of condensation polymers derive the
structural formulas of the components and the other way around:
• polyesters;
• polyamides.
indicate what is understood by different types of isomers, recognise these and give
examples of these:
• structural isomers;
• stereoisomers;
• cis-trans isomers;
• mirror image isomers.
give the structural formulas of structural isomers that satisfy a given molecular formula
with a maximum of 6 carbon atoms.
derive from information about a reaction if structural isomers can be produced and, if so,
which ones.
indicate similarities and differences in properties of isomers and relate these to their
structure:
• melting and boiling points;
• reactivity.
Domain D: Biochemistry
Subdomain D2: Metabolism
The candidate can describe a number of biochemical processes.
The candidate can:
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describe the photosynthesis of glucose as a process during which energy is stored:
• light;
• clorophyll;
• energy storage;
• binding of carbon dioxide;
• production of oxygen.
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name the main components of food:
• proteins;
• carbohydrates;
• fats.
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describe the function of enzymes in organisms;
• catalyst;
• substrate;
• key-lock hypothesis.
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indicate that the digestion of food starts with the enzymatic hydrolysis of carbohydrates,
fats, and proteins, and name the substances produced in this process:
• glucose;
• glycerol and fatty acids;
• amino acids.
indicate that proteins are polyamides:
• peptide bond.
explain what is understood by the concept of essential in essential amino acids and
essential fatty acids.
describe the significance of nucleic acids in the body:
• chromosome;
• gene;
• DNA;
• RNA;
• transcription;
• translation;
• genetic code.
Subdomain D3: Structures of biochemical substances
The candidate van describe the structure of a number of biochemical substances and indicate
the components that they consist of.
Specification
The candidate can:
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indicate for a number of types of natural condensation polymers the components that
they consist of and schematically represent the structure of such a polymer molecule:
• starch;
• cellulose;
• proteins;
• nucleic acids.
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indicate that in a protein molecule, the number, type, and order of the amino acids
molecules is characteristic:
• primary, secondary, and tertiary structure.
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indicate that during denaturisation of proteins the tertiary structure is damaged.
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indicate that nucleic acids consist of polyesters of phosphoric acid and ribose plus
nucleic bases.
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indicate that nucleic acids have a helix structure.
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indicate that carbohydrates can be classified as mono-, di-, and polysaccharides and
give one or more examples for each category:
• glucose;
• fructose;
• ribose;
• saccharose;
• glycogen;
• starch;
• cellulose.
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give the molecular formulas of glucose and saccharose.
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indicate that di- and polysaccharides consist of a series of monosaccharides with a ring
structure.
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indicate how the suspected presence of starch can be detected.
Domain E: Properties of reactions
Subdomain E1: Applications
The candidate can describe a few natural cycle processes and indicate for a number of reaction
and process types what their properties are and show them in equations.
The candidate can:
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calculate the efficiency of a process as a percentage or fraction of the theoretical yield
on the basis of complete conversion.
95
indicate that by affecting the reaction rate in (industrial) processes, a certain product can
be obtained or can be produced more cheaply.
96
describe how a certain product can be obtained or can be produced more cheaply using
measures that affect the equilibrium position in (industrial) processes:
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use concepts that are linked to toxicity:
• acute toxicity;
• chronic toxicity;
• mutagenicity;
• carcinogenicity;
• no toxic effect level;
• ADI value;
• MAC value,
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describe the natural carbon cycle as an example of conservation of matter:
• photosynthesis;
• conversion of glucose into organic substances;
• biodegradation of these substances;
• significance of this cycle in relation to the environment.
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describe the natural nitrogen cycle as an example of conservation of matter:
• nitrogen fixation;
• nitrate in plant nutrients (fertiliser);
• formation of nitrogen-containing organic substances (proteins);
• reduction of nitrogen-containing organic substances to simple molecules;
• significance of this cycle for the environment.
102 name types of reactions and indicate what the properties of those reactions are:
• substitution;
• addition;
• redox;
• acid-base;
• esterification;
• saponification;
• polymerisation;
• hydrolysis;
• cracking.
103 reproduce chemical processes, solution, and evaporation using formulas and reaction
equations:
• molecular formulas;
• structural formulas;
• ions.
104 derive from data to which type of reaction (see #102) a certain reaction belongs:
• from the equation of the reaction;
• from data about reactants and products.
105 identify the reactants and products from data about a reaction/process.
Subdomain E3: Reaction rate
The candidate can indicate what is meant by reaction rate and explain which factors influence
reaction rates.
The candidate can:
106 indicate that phase transitions, solution, reactions (often) are accompanied by an energy
exchange:
• exotherm;
• endotherm.
107 describe the progression of a chemical reaction using an energy diagram:
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• transition state;
• activation energy.
indicate what is meant by reaction rate.
describe the 'colliding particles model'.
using the 'colliding particles model', explain how the factors of concentration, dispersion,
and temperature affect the reaction rate.
using the concept of activation energy, explain how the nature of the substances, the
catalyst and the temperature affect the reaction rate.
indicate schematically what happens to the reaction rate and to the concentration of a
reactant:
• during an irreversible reaction;
• when equilibrium is being reached;
• in equilibrium.
Subdomain E4: Equilibria
The candidate can indicate how the position of an equilibrium can be influenced.
The candidate can:
118 indicate what is meant by:
• a dynamic equilibrium;
• a homogeneous equilibrium;
• a heterogeneous equilibrium;
• a dispersion equilibrium.
119 indicate how an irreversible reaction can be obtained in an equilibrium.
120 explain for a number of factors how these affect the speed at which the equilibrium is
established:
• catalyst;
• temperature;
• dispersion;
• pressure/volume/concentration.
121 using the equilibrium value explain how the equilibrium situation can be affected by:
• the concentration of partial pressure of one or more substances involved in the
equilibrium;
• the total pressure an the gas equilibrium system;
• the volume of the equilibrium system;
• the temperature of the equilibrium system;
• the presence of a catalyst;
• the dispersion ofthe substances involved in the equilibrium:
122 give the equilibrium value for a given equilibrium reaction:
• reaction quotient/partial pressure quotient;
• equilibrium constant.
123 indicate for a number of factors whether these affect the equilibrium value:
• temperature;
• pressure;
• concentration of substances;
• catalyst;
• dispersion.
Subdomain E5: Reaction caiculations
The candidate can perform chemical calculations.
The candidate can:
125 explain what is meant by the concepts:
• chemical amount of substance, mole unit;
• molar mass;
• molar ratio;
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• molar volume of a gas.
indicate for a number of quantities that are characteristic for a particle or substance what
they mean:
• average atomic mass;
• molecular mass;
• ion mass;
• molar mass.
for a number of concepts that are used to indicate a level, explain what they mean and
perform calculations with them:
• volume percentage;
• mass percentage;
• volume ppm;
• mass ppm;
• concentration in mol L—1, molarity.
perform chemical calculations:
• mass percentages in compounds;
• contents in mixtures;
• molar ratio and mass ratio in reactions;
• volume ratio of gases in reactions.
Domain F: Chemical engineering
Subdomain F3: Detecting the presence of substances
The candidate can list a number of methods used to detect the presence of substances and
interpret the results that are thus obtained.
The candidate can:
139 interpret paper and thin Iayer chromatograms for the purpose of recognising substances.
140 interpret gas chromatograms for the purpose of recognising substances.
141 indicate that characteristic patterns can occur in spectrograms and interpret these
patterns in order to recognise those substances or types of substances:
• absorption spectra (visual, UV, IR);
• mass spectra.
Subdomain F4: Techniques of analysis
The candidate can list a number of techniques used to determine the amount of a substance
and perform the corresponding calculations.
Specification
The candidate can:
142 describe the principle behind a titration:
• in acid-base titrations: titration curve, choice of indicator.
143 use gas chromatograms to determine the amount of a substance.
144 indicate how the amount of a substance can be determined colorimetrically.
145 determine amounts of a substance using data from experiments and the Beer-Lambert
law.
Subdomain F5: Process industry
The candidate can describe the large-scale execution of a chemical process.
The candidate can:
146 distinguish steps in the large-scale execution of a chemical process:
• supply and storage of resources;
• preparation (dosing, mixing, heating, compressing);
• reaction;
• separation/recycling;
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• purification/waste processing;
• storage and transport of finished products.
indicate in which cases a batch process is preferred over a continuous process:
• small-scale production;
• broad product range.
list the advantages of a continuous process over a batch process:
• better automation;
• no time wasted by filling, emptying, cleaning;
• simpler recycling.
produce the flow chart of a production process that has been described.
interpret the flow chart of a production process that has been described.
use a mass balance, element balance, and/or energy balance when performing
calculations on a large-scale chemical process.
Domain G: Acids and bases
Subdomain G3: Properties, reactions, and the Bronsted theory
The candidate can apply a number of concepts from the acid-base theory.
Specification
The candidate can:
163 indicate what an acidic, basic, and a neutral environment is.
164 describe an acid-base reaction using the Brønsted theory.
165 for a given reaction indicate whether it is an acid-base reaction and identify the acids and
bases.
166 indicate what is meant by a conjugate acid, a conjugate base, and an acid-base pair.
167 indicate what is meant by a strong acid and a weak acid, a strong base and a weak
base, a buffer, and an ampholyte.
168 using reaction equations show that water can react as an acid and as a base.
169 represent the equilibrium conditions of a few equilibria:
• the water constant, Kw; pKw;
• the acid constant, Ka; pKa;
• the base constant, Kb; pKb;
170 using a table with acid-base constants, predict whether an acid-base reaction can occur.
172 qualitatively explain how a buffer solution works.
173 explain what happens to the pH when a solution is diluted:
• strong and weak acids in solutions;
• strong and weak bases in solutions;
• buffers.
174 explain what happens to the pH when small amounts of an acid or base are added to a
buffer.
Subdomain G4: Calculations
The candidate can perform calculations on acidic and basic solutions and on buffer solutions.
The candidate can:
175 using a table of acidity and basicity constants, calculate the pH from the molarity of
olutions and the other way around:
• strong acids and monoprotic weak acids;
• strong bases and monoprotic weak bases;
• buffers.
176 give the value of the water constant AT 298 K.
177 give the values of [H+], [0H—] and pH at 298 K for water and for neutral solutions.
178 using the data of a neutralisation in which an acid is added to a base, or the other
around, calculate the molarity of the acid or the base.
Domain H: Redox
Subdomain H3: Reactions
The candidate can apply a number of concepts from redox theory and using a table of half
reactions make statements about the application of redox reactions.
The candidate can:
191 indicate what a reductant and an oxidant are.
192 list the names and formulas of some common reductants:
• carbon monoxide;
• metals;
• carbon;
• sulfite.
193 list the names and formulas of some common oxidants:
• nitric acid;
• iron[III) compounds;
• oxygen;
• halogens;
• hydrogen peroxide;
• ozone.
194 indicate what a half reaction is and which types of particles are involved in this:
• electrons;
• redox pair;
• reductant;
• oxidant;
• conjugate.
195 using a table indicate for a redox reaction between given substances/particles which half
reactions will take place and from this derive the equation of the total reaction.
196 using a table of half reactions and data about the strength of oxidants and reductants,
indicate which half reactions will take place in an electrochemical cell and from this
derive the equation of the overall reaction.
197 for a given reaction indicate whether it is a redox reaction, identify the reductant and
oxidant, and indicate how the electron transfer takes place.
198 using a table containing data about the strength of oxidants and reductants, predict
whether in a given situation a redox reaction can take place and identify its reductant and
oxidant.
201 indicate which reactions take place when a given metal corrodes/rusts using sources.
202 indicate how the suspected presence of the following can be detected:
• chlorine;
• iodine;
• sulfite;
• sulfur dioxide;
• hydrogen.