Pearson Baccalaureate Chemistry Higher Level

Höfundar: Mike Ford; Catrin Brown (Útgáfa: 2)
Pearson Baccalaureate Chemistry Higher Level

Kaup valmöguleikar

Pearson Baccalaureate Chemistry Higher Level 2e

Nánar um bókina

Útgefandi
Pearson International Content
ISBN
9781292371559
Print ISBN
9781447959755
Format
Page Fidelity (PDF)
Útgáfa
2
Höfundar
Mike Ford; Catrin Brown
Tungumál
English
Útgefið
2020-07-20
Prent takmörkun á líftíma
100
Prent takmörkun
2
Afritunar takmörkun
2

Kaflar

  • Contents
  • Introduction
  • Chapter 1: Stoichiometric relationships
  • 1.1: Introduction to the particulate nature of matter and chemical change
  • Chemical elements are the fundamental building blocks of chemistry
  • Chemical compounds are formed from more than one element
  • Chemical equations summarize chemical change
  • Mixtures form when substances combine without chemical interaction
  • Matter exists in different states determined by the temperature and the pressure
  • Matter changes state reversibly
  • 1.2: The mole concept
  • The Avogadro constant defines the mole as the unit of amount in chemistry
  • Relative atomic mass is used to compare the masses of atoms
  • Relative formula mass is used to compare masses of compounds
  • Molar mass is the mass of one mole of a substance
  • The empirical formula of a compound gives the simplest ratio of its atoms
  • Percentage composition by mass can be calculated from the empirical formula
  • The molecular formula of a compound gives the actual number of atoms in a molecule
  • 1.3: Reacting masses and volumes
  • Chemical equations show reactants combining in a fixed molar ratio
  • The theoretical yield is determined by the limiting reactant
  • The percentage yield can be calculated from the experimental and theoretical yields
  • Avogadro’s law directly relates gas volumes to moles
  • All gases under the same conditions have the same molar volume
  • The gas laws describe pressure, volume, and temperature relationships for all gases
  • The ideal gas equation is derived from the combined gas equation and Avogadro’s law
  • Real gases show deviation from ideal behaviour
  • The concentration of a solution depends on moles of solute and volume of solution
  • Dilutions of solutions reduce the concentration
  • The concentration of a solution can be determined by volumetric analysis
  • Chapter 2: Atomic structure
  • 2.1: The nuclear atom
  • Dalton’s model of the atom
  • Atoms contain electrons
  • Rutherford’s model of the atom
  • Sub-atomic particles
  • Bohr model of the hydrogen atom
  • Atomic number and mass number
  • Isotopes
  • Ions
  • Relative atomic masses of some elements
  • Mass spectra
  • 2.2: Electron configuration
  • The electromagnetic spectrum
  • Atomic absorption and emission line spectra
  • Evidence for the Bohr model
  • The hydrogen spectrum
  • Wave and particle models
  • The Uncertainty Principle
  • Schrödinger model of the hydrogen atom
  • Atomic orbitals
  • Sub-levels of electrons
  • Aufbau Principle: orbital diagrams
  • The relative energy of the orbitals depends on the atomic number
  • Electron configuration of ions
  • Electronic configuration and the Periodic Table
  • 12.1: Electrons in atoms
  • Ionization energy
  • Patterns in successive ionization energies give evidence for the energy levels in the atom
  • A closer look at successive ionization energies gives evidence for the sub-levels
  • Trends in first ionization energy across periods accounts or the existence of main energy levels and
  • Chapter 3: Periodicity
  • 3.1: The Periodic Table
  • Periods and groups
  • Metals and non-metals
  • 3.2: Periodic trends
  • Physical properties
  • Chemical properties
  • Bonding of the Period 3 oxides
  • 13.1: First-row d-block elements
  • Transition elements have characteristic properties
  • Complex ions
  • Polydentate ligands act as chelating agents
  • Transition metals and their ions are important catalysts
  • The magnetic properties of the transition metals and their compounds
  • 13.2: Coloured complexes
  • The visible spectrum
  • Transition metals appear coloured because they absorb visible light
  • Transition metals absorb light because the d orbitals split into two sub-levels
  • Chapter 4: Chemical bonding and structure
  • 4.1: Ionic bonding and structure
  • Ions form when electrons are transferred
  • Ionic compounds form when oppositely charged ions attract
  • Ionic compounds have a lattice structure
  • The physical properties of ionic compounds reflect their lattice structure
  • Different ionic compounds have a different extent of ionic character
  • 4.2: Covalent bonding
  • A covalent bond forms by atoms sharing electrons
  • Atoms can share more than one pair of electrons to form multiple bonds
  • Short bonds are strong bonds
  • Polar bonds result from unequal sharing of electrons
  • 4.3: Covalent structures
  • Lewis diagrams are used to show the arrangement of electrons in covalent molecules
  • In coordinate bonds both shared electrons come from one atom
  • The octet rule is not always followed
  • VSEPR theory: The shape of a molecule is determined by repulsion between electron domains
  • Molecules with polar bonds are not always polar
  • Electrons in multiple bonds can sometimes spread themselves between more than one bonding position
  • Some covalent substances form giant molecular crystalline solids
  • 4.4: Intermolecular forces
  • London (dispersion) forces
  • Dipole–dipole attraction
  • Hydrogen bonding
  • The physical properties of covalent compounds are largely a result of their intermolecular forces
  • 4.5: Metallic bonding
  • Alloys are solutions of metals with enhanced properties
  • 14.1: Further aspects of covalent bonding and structure
  • Some molecules contain a central atom with an expanded octet
  • Summary of shapes of molecules predicted from VSEPR theory
  • Molecular geometry determines molecular polarity
  • Formal charge is a useful tool for comparing Lewis (electron dot) structures
  • Ozone: a case study in resonance, molecular polarity, and formal charge
  • Atomic orbitals overlap to form two types of covalent bond: sigma and pi
  • 14.2: Hybridization
  • The formation of covalent bonds often starts with the excitation of the atoms
  • Hybridization involves mixing atomic orbitals to form new hybrid atomic orbitals
  • Hybridization can also be used to predict molecular shape
  • Chapter 5: Energetics and thermochemistry
  • 5.1: Measuring energy changes
  • Energy and heat transfer energy
  • System and surroundings
  • The heat content of a system is its enthalpy
  • Exothermic and endothermic reactions
  • Standard enthalpy changes
  • Thermochemical equations
  • Temperature is a measure of average kinetic energy
  • Heat changes can be calculated from temperature changes
  • Enthalpy changes and the direction of change
  • Measuring enthalpy changes of combustion
  • Calculating enthalpies of reaction from temperature changes
  • Enthalpy changes of reaction in solution
  • 5.2: Hess’s law
  • Enthalpy cycles
  • Using Hess’s law
  • Standard enthalpy changes of reaction
  • Using standard enthalpy changes of formation
  • 5.3: Bond enthalpies
  • Breaking bonds is an endothermic process
  • Making bonds is an exothermic process
  • Using bond enthalpies to calculate the enthalpy changes of reaction
  • Ozone depletion
  • 15.1: Energy cycles
  • First ionization energies and electron affinities
  • Lattice enthalpies
  • Experimental lattice enthalpies and the Born–Haber cycle
  • Theoretical lattice enthalpies can be calculated from the ionic model
  • Lattice enthalpies depend on the size and charge of the ions.
  • Enthalpies of solution
  • The hydration enthalpy of an ion depends on the attraction between the ions and the polar water mole
  • The enthalpy change of solution is related to the lattice enthalpy and the hydration enthalpies of t
  • 15.2: Entropy and spontaneity
  • Entropy is a more complete direction of change
  • Predicting entropy changes
  • Absolute entropy
  • Calculating entropy changes
  • Spontaneity
  • Entropy changes of the surroundings
  • The change in entropy of the surroundings is proportional to – ΔH(system)
  • ΔS(surroundings) and an explanation of the units of entropy
  • Calculating total entropy changes and understanding endothermic reactions
  • Gibbs free energy is a useful accounting tool
  • Using ΔG(system) to predict the feasibility of a change
  • The effect of ΔH°, ΔS°, and T on the spontaneity of reaction
  • Calculating ΔG values
  • Gibbs free energy and equilibrium
  • Chapter 6: Chemical kinetics
  • 6.1: Collision theory and rates of reaction
  • Rate of reaction is defined as the rate of change in concentration
  • Measuring rates of reaction uses different techniques depending on the reaction
  • Collision theory
  • Factors affecting rate of reaction
  • 16.1: Rate expression and reaction mechanism
  • The rate law for a reaction is derived from experimental data
  • Units of k vary depending on the overall order of the reaction
  • Graphical representations of reaction kinetics
  • Determination of the order of a reaction
  • Reaction mechanism
  • The rate expression for an overall reaction is determined by the reaction mechanism
  • 16.2: Activation energy
  • The rate constant k is temperature dependent
  • The temperature dependence of the rate constant is expressed in the Arrhenius equation
  • Using the Arrhenius equation to calculate activation energy
  • Chapter 7: Equilibrium
  • 7.1: Equilibrium
  • Physical systems
  • Chemical systems
  • The equilibrium state has specific characteristics
  • The equilibrium constant Kc can be predicted from a reaction’s stoichiometry
  • The magnitude of Kc gives information on the extent of reaction
  • The reaction quotient, Q, enables us to predict the direction of reaction
  • Relationships between Kc for different equations of a reaction
  • When equilibrium is disrupted
  • Equilibrium theory is applied in many industrial processes
  • 17.1: The equilibrium law
  • Calculating the equilibrium constant from initial and equilibrium concentrations
  • Calculating equilibrium concentrations from the equilibrium constant
  • Free energy and equilibrium
  • Kc can be calculated from thermodynamic data
  • Kinetics and equilibrium
  • Chapter 8: Acids and bases
  • 8.1: Theories of acids and bases
  • Early theories
  • Brønsted–Lowry: a theory of proton transfer
  • 8.2: Properties of acids and bases
  • Acids react with metals, bases, and carbonates to form salts
  • Acids and bases can be distinguished using indicators
  • 8.3: The pH scale
  • pH is a logarithmic expression of [H+]
  • pH calculations
  • Measuring pH
  • The ionization of water
  • The relationship between H+ and OH– is inverse
  • 8.4: Strong and weak acids and bases
  • The strength of an acid or base depends on its extent of ionization
  • Weak acids and bases are much more common than strong acids and bases
  • Distinguishing between strong and weak acids and bases
  • 18.1: Lewis acids and bases
  • Lewis theory focuses on electron pairs
  • Nucleophiles and electrophiles
  • Comparison of Brønsted–Lowry and Lewis theories of acids and bases
  • 18.2: Calculations involving acids and bases
  • Kw is temperature dependent
  • pH and pOH scales are inter-related
  • Summary of the relationships between [H+], [OH–], pH, and pOH
  • Converting H+ and OH– into pH and pOH
  • Strong acids and bases: pH and pOH can be deduced from their concentrations
  • Dissociation constants express the strength of weak acids and bases
  • Calculations involving Ka and Kb
  • pKa and pKb
  • Relationship between Ka and Kb, pKa and pKb for a conjugate pair
  • 18.3: pH curves
  • Buffer solutions
  • Salt hydrolysis
  • Acid–base titrations
  • Indicators signal change in pH
  • 8.5: Acid deposition
  • Causes of acid deposition
  • Effects of acid deposition
  • Responses to acid deposition
  • Chapter 9: Redox processes
  • 9.1: Oxidation and reduction
  • Introduction to oxidation and reduction
  • Oxidation numbers enable us to track redox change
  • Strategy for assigning oxidation states
  • Interpreting oxidation states
  • Systematic names of compounds use oxidation numbers
  • Redox equations
  • Oxidizing and reducing agents
  • More reactive metals are stronger reducing agents
  • More reactive non-metals are stronger oxidizing agents
  • Redox titrations
  • 9.2 & 19.1: Electrochemical cells
  • Voltaic cells generate electricity from spontaneous redox reactions
  • Half-cells generate electrode potentials
  • Two connected half-cells make a voltaic cell
  • Different half-cells make voltaic cells with different voltages
  • Standard electrode potentials
  • Comparisons of half-cell electrode potentials need a reference point
  • The standard hydrogen electrode
  • Measuring standard electrode potentials
  • Standard electrode potentials are given for the reduction reaction
  • Using standard electrode potential data
  • A little caution about interpreting Eθ data
  • An external source of electricity drives non-spontaneous redox reactions
  • Redox reactions occur at the electrodes
  • Determining the products in electrolytic cells
  • The electrolysis of molten salts
  • Electrolysis of aqueous solutions
  • Factors affecting the amount of product in electrolysis
  • Electroplating: a widely used application of electrolysis
  • Summary of voltaic and electrolytic cells
  • Chapter 10: Organic chemistry
  • 10.1: Fundamentals of organic chemistry
  • Homologous series
  • Formulas for organic compounds: empirical, molecular, and structural
  • Nomenclature for organic compounds: the IUPAC system
  • Structural isomers: different arrangements of the same atoms
  • Primary, secondary, and tertiary compounds
  • Arenes
  • Trends in physical properties
  • 10.2: Functional group chemistry
  • Alkenes
  • Alcohols
  • Halogenoalkanes
  • Benzene
  • 20.1: Types of organic reactions
  • Nucleophilic substitution reactions: halogenoalkanes
  • Electrophilic addition reactions: alkenes
  • Electrophilic substitution reactions: benzene
  • Reduction reactions
  • Summary of reaction mechanisms
  • 20.2: Synthetic routes
  • Retro-synthesis: working backwards
  • 20.3: Stereoisomerism
  • cis–trans and E/Z isomers
  • Optical isomers
  • Chapter 11: Measurement and data processing and analysis
  • 11.1: Uncertainties and errors in measurement and results
  • Uncertainty in measurement
  • Other sources of uncertainty
  • Significant figures in measurements
  • Experimental errors
  • Percentage uncertainties and errors
  • Propagation of uncertainties in calculated results
  • Significant figures in calculations
  • Discussing errors and uncertainties
  • 11.2: Graphical techniques
  • Plotting graphs
  • The ‘best-fit’ straight line
  • Finding the gradient of a straight line or curve
  • Errors and graphs
  • Choosing what to plot to produce a straight line
  • The use of log scales
  • Sketched graphs are used to show qualitative trends
  • Using spreadsheets to plot graphs
  • 11.3: Spectroscopic identification of organic compounds
  • Analytical techniques
  • Mass spectrometry
  • The degree of unsaturation/IHD
  • Different regions of the electromagnetic spectrum give different information about the structure of
  • Infrared (IR) spectroscopy
  • Nuclear magnetic resonance (NMR) spectroscopy
  • Analytical chemistry depends on combining information
  • 21.1: Spectroscopic identification of organic compounds
  • Further NMR spectroscopy
  • Chapter 12: Option A: Materials
  • A.1: Materials science introduction
  • Materials are classifi ed based on their uses, properties, or bonding and structure
  • The properties of a material based on the degree of covalent, ionic, ormetallic character can be ded
  • There are four distinct classes of materials
  • Some physical properties of materials
  • A.2: Metals and inductively coupled plasma (ICP) spectroscopy
  • The method of extraction is related to its position in the activity series
  • The equations for the extraction can be deduced from changes in oxidation numbers
  • Aluminium is extracted from its ore (bauxite) by electrolysis
  • The amount of metal produced depends on the number of electrons supplied
  • Alloys are homogeneous mixtures of metals with other metals or non-metals
  • Paramagnetic and diamagnetic materials display different behaviour in magnetic fields because of the
  • Inductively coupled plasma (ICP) spectroscopy determines the identity and concentration of metals
  • A.3: Catalysts
  • Homogeneous and heterogeneous catalysis
  • Zeolites act as selective catalysts because of their cage structures
  • Nanoparticles are effective heterogeneous catalysts as they havea large surface area per unit mass
  • Catalytic activity can be modifi ed with the use of promoters and inhibitors or inactivated by poiso
  • Catalyst choice depends on selectivity for only the desired product and environmental impact
  • A.4: Liquid crystals
  • Thermotropic liquid crystals show liquid crystal behaviour over a temperature range
  • Lyotropic liquid crystals are solutions
  • The elasticity and electrical and optical properties depend on the orientation of the molecule to so
  • Biphenyl nitriles show liquid crystal behaviour
  • The use of biphenyl nitriles in liquid crystal display devices
  • Twisted nematic LCDs
  • A.5: Polymers
  • The density of poly(ethene) depends on the branching in the structure
  • Different orientations of side groups lead to isotactic and atactic forms
  • The properties of poly(vinyl chloride) are modified by using plasticizers
  • Expanded polystyrene is made by adding volatile hydrocarbons
  • Polymers can be classified based on their response to heat and applied forces
  • Atom economy is a measure of efficiency applied in Green Chemistry
  • A.6: Nanotechnology
  • Nanotechnology involves structures in the 1–100 nm range
  • Individual atoms can be visualized and manipulating using the scanning tunnelling and atomic force m
  • Self-assembly can occur spontaneously in solution due to intermolecular interactions
  • Nanowires are used in electronic devices
  • Carbon nanotubes aremade from pentagons and hexagons of carbon atoms
  • Single-walled carbon nanotubes (SWNTs) and multiwalled carbon nanotubes (MWNTs ) can be made
  • Graphene is a single atomic plane of graphite
  • Carbon nanotubes are made by arc discharge, chemical vapour deposition (CVD), and high-pressure carb
  • Implications of nanotechnology
  • A.7: Environmental impact: plastics
  • Health concerns of using volatile plasticizer in polymer production
  • Plastics do not degrade easily because of their strong covalent bonds
  • Incineration of plastics reduces bulk, releases energy but produces air pollution
  • Incomplete combustion of PVC produces dioxins
  • Polychlorinated biphenyls (PCBs) and polychlorinated dibenzofurans are dioxin-like substances and ar
  • House fires can release many toxins when plastic objects burn
  • Plastics require more processing to be recycled than other materials
  • Plastics can be identified from their IR spectrum
  • A.8: Superconducting metals and X-ray crystallography
  • Resistance in metallic conductors is caused by collisions between electrons and the positive ions in
  • Superconductors are materials that offer no resistance to electric currents below a critical tempera
  • The Meissner effect is the ability of a superconductor to create a mirror image magnetic field of an
  • Type 1 superconductors have sharp transitions to superconductivity whereas Type 2 superconductors ha
  • Type 1 and Type 2 superconductors
  • The structure of solids
  • The structure of solids is determined by X-ray diffraction
  • A.9: Condensation polymers
  • Condensation polymers can be formed from monomers with two functional groups
  • PET is a polyester
  • Nylon is a polyamide
  • Kevlar® is a polyamide
  • Phenol and methanal form a condensation polymer
  • Green Polymers
  • A.10: Environmental impact: heavy metals
  • Heavy metals are toxic
  • Ion exchange can be used to remove metal ions
  • Metal ions can be removed by chemical precipitation
  • Metal ions can be removed from solution by chelating agents
  • The solubility product is a measure of the solubility of an ionic compound
  • The common ion effect
  • Harmful hydroxyl free radicals can be formed in the body from hydrogen peroxide
  • The Haber–Weiss reaction generates free radicals naturally in biological processes
  • Chapter 13: Option B: Biochemistry
  • B.1: Introduction to biochemistry
  • Biochemical reactions are organized in metabolic pathways
  • Biomolecules are diverse organic molecules
  • Living cells transform energy
  • B.2 & B.7: Proteins and enzymes
  • B.2 Proteins and enzymes
  • B.7 Proteins and enzymes
  • The functions of proteins
  • The structure of proteins
  • Enzymes are globular proteins
  • Enzymes form a complex with the substrate
  • Analysis of proteins
  • B.3: Lipids
  • Functions of lipids
  • Structures of different lipids
  • Structure of triglycerides: fats and oils
  • Structure of phospholipids
  • Hydrolysis of fats and phospholipids
  • Structure of steroids
  • B.4: Carbohydrates
  • Functions of carbohydrates
  • Structure of carbohydrates
  • B.5: Vitamins
  • Vitamins are organic micronutrients
  • Vitamin deficiencies are a form of malnutrition
  • B.8: Nucleic acids
  • The role of nucleic acids
  • The structure of nucleic acids
  • DNA is expressed through protein synthesis
  • DNA replication makes a copy of the genetic information
  • DNA can be transferred between species
  • B.9: Pigments
  • Porphyrins
  • Carotenoids
  • Anthocyanins
  • Analysis of pigments
  • B.10: Stereochemistry in biomolecules
  • Stereochemistry in proteins
  • Stereochemistry in lipids
  • Stereochemistry in carbohydrates
  • Stereochemistry in vitamins
  • B.6: Biochemistry and the environment
  • Xenobiotics: strangers to life
  • Amelioration: responses to xenobiotics
  • Green Chemistry
  • Chapter 14: Option C: Energy
  • C.1: Energy sources
  • A useful energy source releases energy at a reasonable rate and produces minimal pollution
  • Renewable energy sources are naturally replenished
  • The energy density of a fuel is the energy produced per unit volume and the specific energy is the e
  • Energy conversions are never 100% efficient
  • C.2: Fossil fuels
  • Fossil fuels were formed by the reduction of biological compounds
  • Coal is the most abundant fossil fuel
  • Crude oil is a valuable fuel and chemical feedstock
  • Natural gas is mainly methane
  • The past and future of fossil fuels
  • Carbon footprint
  • C.3 & C.7: Nuclear fusion and fission
  • Some particles in the particles zoo
  • The mass defect is the difference between the mass of the nucleus and the sum of the masses of its i
  • Binding energy graphs can be used to understand nuclear stability
  • Light nuclei can undergo fusion reactions as this increases the binding energy per nucleon
  • The elements in the stars can be identified by their absorption spectra
  • Nuclear fusion as a possible source of energy
  • The advantages of nuclear fusion
  • Heavy nuclei can undergo fission reactions as this increases the binding energy per nucleon
  • Fuel enrichment involves the separation of different isotopes of uranium
  • Uncontrolled nuclear reactions are used in nuclear weapons
  • 23994Pu used as a fuel in ‘breeder reactors’ is produced from 23892U by neutron capture
  • Nuclear waste is still radioactive
  • The half-life of radioactive isotopes
  • Radioactive decay is a first-order process
  • Nuclear waste can be high level or low level
  • Comparison between fossil fuel and nuclear power stations
  • The dangers of nuclear energy are due to the ionizing nature of the radiation
  • C.4: Solar energy
  • Light can be absorbed by chlorophyll and other pigments with a conjugated electronic structure
  • Photosynthesis converts light energy into chemical energy
  • Ethanol can be used as a biofuel
  • The advantages and disadvantages of using biofuels
  • The energy content of vegetable oils
  • Transesterifi cation with ethanol or methanol produces oils with lower viscosity that can be used in
  • C.5: Environmental impact: global warming
  • Greenhouse gases absorb long-wave length IR radiation from the Earth
  • Greenhouse gases and their sources
  • Influence of increasing amounts of greenhouse gases on the atmosphere
  • There is a heterogeneous equilibrium between atmospheric carbon dioxide and aqueous carbon dioxide i
  • Ocean acidification affects shell-forming animals
  • Global dimming
  • Three strategies for reducing carbon dioxide levels
  • C.6: Electrochemistry, rechargeable batteries, and fuel cells
  • Electric circuits
  • The voltage of a battery depends primarily on the nature of the electrodes and the electrolytes
  • The Nernst equation can be used to calculate the potential of a half-cell under non-standard conditi
  • The electrodes in a concentration cell are the same
  • The total work that can be obtained from a cell depends on the quantity of materials used
  • Secondary cells can be recharged and so have longer life times than primary cells
  • Thermodynamic efficiency of a cell
  • Similarities and differences between fuel cells and rechargeable batteries
  • C.8: Photovoltaic and dye-sensitized solar cells (DSSC)
  • Silicon is a semiconductor
  • Comparing conductors and semiconductors
  • The conversion of light energy to electricity involves light absorption and charge separation
  • Solar energy can be converted to electricity in a photovoltaic cell
  • Dye-sensitized solar cells (DSSC)
  • Chapter 15: Option D: Medicinal chemistry
  • D.1: Pharmaceutical products an ddrug action
  • The human body has many natural systems of defence
  • Medicines and drugs: some terminology
  • Drugs can be administered in different ways
  • Bioavailability of drugs: the amount that reaches the target
  • Physiological effects of drugs are complex
  • Drug action depends on interactions with receptors
  • The development of new synthetic drugs is a long and costly process
  • D.2: Aspirin and penicillin
  • Aspirin: a mild analgesic
  • Penicillin: an early antibiotic
  • D.3: Opiates
  • The opiates bind to receptor sites in the brain
  • The structures and synthesis of opioids
  • Advantages and disadvantages of using strong analgesics
  • D.4: pH regulation of the stomach
  • Excess acidity in the stomach is potentially harmful
  • Some drugs work to prevent the production of excess acid
  • Antacids are weak bases which neutralize excess acid
  • D.5: Antiviral medications
  • Viruses: nature’s most successful parasites
  • The war against viruses
  • Flu viruses: a case study in antivirals
  • AIDS : a viral pandemic
  • D.7: Taxol: a chiral auxiliary case study
  • Optical isomerism: chiral drugs exist in two forms with different activities
  • Taxol is a powerful anti-cancer drug
  • Asymmetric synthesis: theproduction of a single enantiomer of Taxol
  • D.8: Nuclear medicine
  • Unstable atomic nuclei emit radiation
  • The main types of radiation are alpha, beta, and gamma
  • Radioactive emissions have an ionizing effect
  • Half-life of an isotope determines the rate of radioactive decay
  • Nuclear radiation in medical treatment
  • Diagnostic techniques in nuclear medicine
  • Radionuclide therapy
  • D.9: Drug detection and analysis
  • Drug isolation and purification
  • Drug detection
  • Organic structure analysis and identification
  • D.6: Environmental impact of some medications
  • Solvent waste: the major emission of the drug industry
  • Nuclear waste: an increasing problem in the drug industry
  • Antibiotic waste: are we killing the cures?
  • Obtaining the Tamiflu precursor: a Green Chemistry case study
  • Green Chemistry success stories in the pharmaceutical industry
  • Green chemistry
  • Experimental work in chemistry
  • Experimental work is an integral part of chemistry
  • Health, safety, and the environment
  • Practical skills
  • Assessment of experimental work
  • Internal assessment
  • The investigation
  • The assessment criteria
  • Making the most of your Internal Assessment opportunity
  • Theory of knowledge
  • Introduction
  • Ways of knowing: perception
  • Chemistry and technology
  • The scientific method
  • Ways of knowing: induction (reason)
  • Ways of knowing: deduction (reason)
  • Same data, different hypothesis
  • Are the models and theories that scientists use merely pragmatic instruments or do they actually des
  • Science and pseudoscience: alchemy and homeopathy
  • A web and hierarchy of disciplines
  • How does chemical knowledge change with time?
  • Paradigm shifts: phlogiston theory and the discovery of oxygen
  • Shared and personal knowledge
  • Ways of knowing: language
  • Measurement: the observer effect
  • Knowledge and belief
  • Chemistry and ethics
  • Ways of knowing: imagination
  • The knowledge framework in chemistry
  • Chemistry and TOK assessment
  • Some examples of prescribed essay titles for you to consider
  • Advice on the extended essay
  • Some advice
  • The assessment criteria
  • Bibliography and references
  • Viva voce
  • World Studies Extended Essay
  • Strategies for success
  • During the course
  • Preparing for the examination
  • In the examination
  • Index
  • Back Cover