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Comprehensive IB Chemistry SL & HL Syllabus

Comprehensive IB Chemistry SL & HL Syllabus

Unit 1: Stoichiometric Relationships

Stoichiometric Relationships

Subtopic Subtopic Number IB Points to Understand
Introduction to the particular nature of matter and chemical change 1.1 (SL) Matter is defined as anything that has mass and takes up space (it has volume).

Properties of three states of matter (Solids, Liquids and Gasses)

Temperature is a measure of the average kinetic energy of the particles of a substance

Sublimation: When solid turns into a gas without first becoming liquid.

Condensation: When gaseous state changes into liquid state.

Melting and boiling are endothermic processes

Condensation and freezing are exothermic processes

Elements, Compounds and Mixtures

An ion is a charge species

Atom economy is the efficiency of chemical reactions by comparing the molecular mass of atoms in the reactants with the molecular mass of useful compounds

The Mole Concept 1.2 (SL) The mole is an SI unit, symbol mol, defined as a fixed amount, n, of a substance

The relative atomic mass Ar of an atom is a weighted average of the atomic masses of its isotopes and their relative abundances

The empirical formula of a compound is the simplest whole-number ratio of atoms or amount (in mol) of each element present in a compound.

The molecular formula is the actual number of atoms or amount (in mol) of elements in one structural unit or one mole of the compound, respectively.

Reacting masses and volumes 1.3 (SL) Chemical change is an expression of reactants combining in fixed ratios to form products.

The reactant that determines the quantity of product is known as the limiting reactant.

The theoretical yield refers to the maximum amount of product obtainable, assuming 100% of the limiting reactant is converted to product.

The kinetic theory of gasses is a model used to explain and predict the behavior of gasses at a microscopic level

Standard temperature (0 °C/273 K) and Standard pressure (100kPa)

Boyle’s Law: Relationship between volume and pressure

Charles’s Law: Relationship between volume and temperature

Gay-Lussac’s Law: Relationship between pressure and temperature

Ideal Gas Equation: PV = nRT

A solution is a homogenous mixture of a solute that has been dissolved in a solvent. Solute is usually a solid but it can be a gas or liquid too. 

Unit 2: Atomic Structure

Atomic Structure

Subtopic Subtopic Number IB Points to Understand
The nuclear atom 2.1 (SL) Dalton’s Atomic Theory

Compounds consist of atoms of more than one element and are formed by combining atoms in whole-number ratios

Atom is the smallest unit of an element

Thomson’s Plum Pudding model of the atom

Rutherford’s model of the atom

Bohr Model of the Hydrogen atom

Atoms consist of three types of subatomic particles: the proton, the neutron and the electron.

The atomic number (Z) is the number of protons in the nucleus of an atom of an element.

The mass number (A) is the number of protons + the number of neutrons in the nucleus of an atom.

Isotopes are different forms of the same element that have the same atomic number, Z, but different mass numbers, A

When atoms lose electrons, it is a cation. If atoms gain electrons, it becomes an anion.

The unified atomic mass unit is a non-SI unit of mass and is defined as one-twelfth of the mass of a carbon-12 atom in its ground-state

The mass spectrometer is an instrument used to determine the relative atomic mass of an element.

Electron configuration 2.2 (SL) Electromagnetic radiation: form of energy that is produced by the movement of electrically charged particles traveling through a matter or vacuum or by oscillating magnetic and electric disturbance.

The electromagnetic spectrum (EMS) is a spectrum of wavelengths that comprise the various types of electromagnetic radiation.

All electromagnetic waves travel at the same speed (c) but can be distinguished by their different wavelengths (λ)

The SI unit of energy is the joule, J; for wavelength the meter, m; and for frequency the hertz, Hz.

When white light is passed through hydrogen gas, an absorption line spectrum is produced with some colors of the continuous spectrum missing.

If a high voltage is applied to the gas, a corresponding emission line spectrum is produced

The hydrogen line emission spectrum consists of a series of lines of different colors in the visible region of the spectrum.

The energy needed to remove an electron from the ground state of an atom in a mole of gaseous atoms, ions, or molecules is called the ionization energy

Ways to illustrate electron configurations

Unit 3: Periodicity

Periodicity

Subtopic Subtopic Number IB Points to Understand
The periodic table 3.1 (SL) Vertical columns: Groups

The Horizontal rows of elements numbered from 1 to 7 are termed period

Period number is equal to the principal quantum number, n

Properties of metals

S, p, d, f and transition elements

Periodic trends 3.2 (SL) Effective nuclear charge

Atomic radius is the distance from the center of the nucleus to the outermost shell containing electrons

The formation of positive ions involves the loss of the outer shell. The formation of negative ions involves the addition of electrons into the outer shell.

The ionization energy, IE, is the minimum energy required to remove an electron from a neutral gaseous atom in its ground-state

The first electron affinity of an element (∆Hea) is the energy change when one mole of electrons is added to one mole of gaseous atoms to form one mole of gaseous ions

The Group 17 elements have incomplete outer energy levels and the Group 1 metals have the lowest effective nuclear charge

Electronegativity, symbol χ, is defined as the relative attraction that an atom has for the shared pair of electrons in a covalent bond

Group 1, 17 and 18 chemical properties

Unit 4: Chemical Bonding and Structure

Chemical Bonding and Structure

Subtopic Subtopic Number IB Points to Understand
Ionic Bonding and Structure 4.1 (SL) Electrons positioned outside the nucleus, are less tightly held and outer electrons, known as valence electrons, can be transferred when atoms react together

An ionic Bond refers to the electrostatic attraction experienced between the electric charges of a cation (positive ion) and an anion (negative ion)

Electrostatic forces: The oppositely charged ions resulting from electron transfer are attracted to each other and are held together by this force

Ionic compounds: These forces are known as an ionic bond, and ions held together in this way 

The term coordination number is used to express the number of ions that surround a given ion in the lattice

Physical properties of ionic compounds

Covalent Bonding 4.2 (SL) Covalent Bonding: atoms share electrons with each other in order to attain a noble gas electron configuration

In a Lewis symbol representation, each element is surrounded by a number of dots (or crosses), which represent the valence electrons of the element

Bond strength and bond length

Covalent structures 4.3 (SL) Bonding pairs of electrons (showing the covalent bond as single, double, or triple bonds) and

Non-bonding pairs of electrons, often called the lone pairs, which are pairs of electrons not involved in the bonding

Valence shell electron pair repulsion (VSEPR) theory can be used to deduce the shapes of covalent molecules

Molecules with two electron domains will position them at 180° to each other

Molecules with three electron domains will position them at 120° to each other

Molecules with four electron domains will position them at 109.5° to each other

Resonance involves using two or more Lewis structures to represent a particular molecule or ion

Difference between graphite, diamond, fullerene and graphene

Intermolecular forces 4.4 (SL) Weak forces of attraction, known as London (dispersion) forces, will occur between opposite ends of these two temporary dipoles in the molecules. 

Dipole Dipole attraction

When a molecule contains hydrogen covalently bonded to a very electronegative atom (fluorine, nitrogen, or oxygen), they are attracted to each other by a hydrogen bond

Metallic Bonding 4.5 (SL) Delocalized: when there is no other element present to accept the electrons and form an ionic compound, the outer electrons are held only loosely by the metal atom’s nucleus

An alloy is a mixture that consists either of two or more metals, or of a metal (or metals) combined with an alloying element composed of one or more nonmetals

Unit 5: Energetics and Thermochemistry

Energetics and Thermochemistry

Subtopic Subtopic Number IB Points to Understand
Measuring energy changes 5.1 (SL) Thermodynamics is the study of energy and how it is interconverted

The first law of thermodynamics states that energy can be converted from one form to another and that the total amount of energy for a given system will remain constant

Enthalpy (H) is a measure of the amount of heat energy contained in a substance. It is stored in the chemical bonds and intermolecular forces as potential energy

Exothermic reactions give out heat and result in a transfer of enthalpy from the chemicals to the surroundings and ∆H reaction is negative

A few reactions are endothermic as they result in an energy transfer from the surroundings to the system. In this case the products have more enthalpy than the reactants and ∆H is positive

The standard enthalpy change of combustion (∆Hc) is the enthalpy change for the complete combustion of one mole of a substance in its standard state in excess oxygen under standard conditions

The standard enthalpy change of formation, ∆Hf, of a substance is the enthalpy change that occurs when one mole of the substance is formed from its elements in their standard states.

Hess’s Law 5.2 (SL) Hess’s Law states that the enthalpy change for a chemical reaction is independent of the route taken. 
Bond Enthalpies 5.3 (SL) The bond enthalpy is the energy needed to break one mole of bonds in gaseous molecules under standard condition.

Unit 6: Chemical Kinetics

Chemical Kinetics

Subtopic Subtopic Number IB Points to Understand
Collision theory and rates of reaction 6.1 (SL) The rate of a reaction depends on how quickly the concentration of either reactant or
product changes with respect to time.A colorimeter or spectrophotometer works by passing light of a selected wavelength through the solution being studied and measures the intensity of the light transmitted by the reaction componentThe total electrical conductivity of a solution depends on the total concentration of its ions and on their chargeMaxwell-Boltzmann distribution curveIn order for a collision to lead to reaction, the particles must have a certain minimum value for their kinetic energy, known as the activation energy, Ea

Factors affecting rate of reaction

Unit 7: Equilibrium

Equilibrium

Subtopic Subtopic Number IB Points to Understand
Equilibrium 7.1 (SL) A state of equilibrium is when both the forward and reverse reactions occur simultaneously with products and reactants constantly being interconverted.

The law of chemical equilibrium states that at a given temperature the ratio of the concentration of products to the concentration of reactants is a constant, Kc

The effects of changing experimental conditions on the equilibrium constant

The ratio of concentration of product to reactants will not equal K. This ratio is called the reaction quotient Q and it helps determine the progress of the reaction as it moves toward equilibrium.

Unit 8: Acids and Bases

Acids and Bases

Subtopic Subtopic Number IB Points to Understand
Theories of acids and bases 8.1 (SL) An acid is any hydrogen containing substance that is capable of donating a proton

A base is a molecule or ion able to accept a hydrogen ion from an acid

Arrhenius theory: acids and bases states that “an acid generates H+ ions in a solution whereas a base produces an OH- ion in its solution”

The combination of an acid and base is well known as a neutralization reaction involving the combination of the hydrogen ion and the hydroxide ion

Bronsted-Lowry: the theory defines “an acid as a proton donor and a base as a proton acceptor”

Lewis theory: The Lewis definition of acids and bases describes “acids as electron-pair acceptors and bases
as electron-pair donors”

An amphiprotic substance is one which can act as both a proton donor and a proton acceptor

Properties of acids and bases 8.2 (SL) Physical properties of acids and bases

  • acid + metal → salt + hydrogen
  • acid + base → salt + water acid + metal
  • carbonate/metal hydrogen carbonate → salt + carbon dioxide + water

Neutralization reactions are used to calculate the exact concentration of an acid or an alkali when the other concentration is known.

The solution of known concentration is known as the standard solution.

The equivalence point is reached when the acid and the base exactly neutralize each other.

A good indicator is one that gives a distinct or sharp color change at the equivalence point.

The pH scale 8.3 (SL) The pH scale is a simple and effective way of representing the concentration of hydrogen ions, [H+] in a solution

Calculating the pH

A way to measure pH is with universal indicator paper, pH meter or solution

Ionization of water

The relationship between H+ and OH– is inverse

Strong and weak acids and bases 8.4 (SL) If the acid dissociates fully, it will exist entirely as ions in solution. It is said to be a strong acid

If the acid dissociates only partially, it produces an equilibrium mixture in which the undissociated form dominates. It is said to be a weak acid

Distinguishing between strong and weak acids and bases using electrical conductivity, rate of reaction and their pH

Acid deposition 8.5 (SL) Acid deposition is the process by which acid-forming pollutants are deposited on the Earth’s surface

Acid rain refers to solutions with a pH below 5.6, and which therefore contain additional acids. The main contributors to acid rain are the oxides of sulfur and nitrogen

Effects of acid deposition on building materials, plant life, water and human health

Pre and Post-combustion technologies

Unit 9: Redox Processes

Redox Processes

Subtopic Subtopic Number IB Points to Understand
Oxidation and Reduction 9.1 (SL) Oxidation describes a process in which the oxidation state increases and reduction describes a process in which the oxidation state decreases.

Oxidation and reduction will always occur together and reactions of this type are known as redox reactions.

Oxidation state is the apparent charge of an atom in a free element, a molecule, or an ion.

Half-equations can be very useful in balancing complex redox reactions. Each half-equation represents the separate oxidation and reduction processes.

The reactant that accepts electrons is called the oxidizing agent as it brings about oxidation of the other reactant. In the process it becomes reduced.

Likewise the reactant that supplies the electrons is known as the reducing agent, because it brings about reduction and itself becomes oxidized.

Electrochemical cells 9.2 (SL) Voltaic (or galvanic) cells – these convert chemical energy to electrical energy. Voltaic cells convert energy from spontaneous, exothermic chemical processes to electrical energy.

Electrolytic cells – these convert electrical energy to chemical energy, bringing about a non- spontaneous process.

An electrode is a conductor of electricity used to make contact with a non-metallic part of a circuit, such as the solution in a cell

The electrode where oxidation occurs is called the anode. The electrode where reduction occurs is called the cathode

Unit 10: Organic Chemistry

Organic Chemistry

Subtopic Subtopic Number IB Points to Understand
Fundamentals of Organic Chemistry 10.1 (SL) Organic chemistry is the field of chemistry that studies carbon-based compounds

A homologous series is a series of compounds that can be grouped together based on similarities in their structure and reactions

The alkenes and alkynes are two more hydrocarbon homologous series that contain carbon– carbon double and triple bonds, respectively.

Members of a homologous series can be represented by the same general formula

The empirical formula represents the simplest ratio of atoms present in a molecule.

The molecular formula describes the actual number of atoms present in the molecule

Other representations: Full structural formula, condensed structural formula and skeletal formula

There are two possible arrangements for atoms that correspond to different molecules with different properties. Molecules, having the same molecular formula but different arrangements of the atoms, are known as structural isomers

Primary, Secondary and Tertiary compounds

Arenes are a class of compounds that are derived from benzene, C6H6. They form a special branch of organic compounds known as the aromatics

Functional Group Chemistry 10.2 (SL) Alkanes are the simplest hydrocarbons. 

Common reactions studied in organic chemistry include substitution, addition, and elimination. 

Substitution is the replacement of individual atoms with other single atoms or with a small group of atoms.

In an addition reaction, two molecules are added together to produce a single molecule, while elimination is the removal of two substituents from the molecule.

Free-radical refers to a species that is formed when a molecule undergoes homolytic fission: the two electrons of a covalent bond are split evenly between two atoms resulting in two free-radicals that each have a single electron

Heterolytic fission of a bond creates a cation and an anion, as the electrons involved in the bond are unevenly split between the two atoms

Initiation, Propagation and Termination

Alkenes are unsaturated hydrocarbons that contain at least one carbon–carbon double bond

Test for unsaturation

Polymerization of alkenes: Addition polymerization is the reaction of many small monomers that contain a carbon– carbon double bond, linking together to form a polymer. 

The oxidation of a primary alcohol is a two-stage process that first produces an aldehyde followed by a carboxylic acid.

The oxidation of a secondary alcohol such as propan-2-ol results in the formation of a ketone

Esterification is a reversible reaction that occurs when a carboxylic acid and an alcohol are heated in the presence of a catalyst

The electron-deficient carbon is attacked by electron-rich species known as nucleophiles.

An electrophile is an electron-poor species capable of accepting an electron pair. It acts as a Lewis acid.

Unit 11: Measurement and data processing and analysis

Measurement and data processing and analysis

Subtopic Subtopic Number IB Points to Understand
Uncertainties and errors in measurement and results 11.1 (SL) Significant figures refer to the number of digits reflecting the precision of a given measurement.
Graphical techniques 11.2 (SL) Graphical techniques are an effective means of communicating the effect of an independent variable on a dependent variable

The slope of gradient of the line. 

Intercept is found using extrapolation or using the equation of a line

Best-fit line

Spectroscopic identification of organic compounds 11.3 (SL) The degree of unsaturation or index of hydrogen deficiency (IHD) can be used to determine from a molecular formula the number of rings or multiple bonds in a molecule.

The degree of unsaturation is used to calculate the number of rings and π bonds present in a structure

Electromagnetic Spectrum

Infrared spectroscopy: using this type of spectroscopy, various functional groups can be identified in a molecule. The vibrational transitions correspond to definite energy levels.

Proton nuclear magnetic resonance spectroscopy

Mass spectrometry

Unit 12: Atomic Structure

Atomic Structure

Subtopic Subtopic Number IB Points to Understand
Electrons in atoms 12.1 (HL) First and second ionization energy

Periodic trends in ionization energies

Unit 13: Periodicity

Periodicity

Subtopic Subtopic Number IB Points to Understand
First-row d-block elements 13.1 (HL) A transition element is an element that has an atom with an incomplete d-sublevel or that gives rise to cations with an incomplete d-sublevel.

Characteristics of transition elements

Transition metals are often found with different oxidation states

Compounds that contain transition elements and in which the central metal ion is bonded, via coordinate bonding, to a group of molecules or ions (termed the ligands) are termed transition metal complexes

Ligands classification: Monodentate and Polydentate

Transition metals work as catalysts in chemical reactions

Paramagnetic and Diamagnetic materials

Coloured complexes 13.2 (HL) The visible spectrum ranges from 400 nm to about 700 nm

Transition metals appear coloured because they absorb visible light

Transition metals absorb light because the d orbitals split into two sub-levels

Unit 14: Chemical Bonding and Structure

Chemical Bonding and Structure

Subtopic Subtopic Number IB Points to Understand
Covalent bonding and electron domain and molecular geometries 14.1 (HL) A single covalent bond consists of two electrons shared between two atoms A and B.

A double covalent bond consists of four electrons, two pairs, shared between two atoms A and B

A triple covalent bond consists of six electrons, or three pairs, shared between two atoms A and B.

Catalytic destruction of ozone

Hybridization 14.2 (HL) A hybrid orbital results from the mixing of different types of atomic orbitals on the same atom

When carbon forms four single bonds, it undergoes sp3 hybridization, producing four equal orbitals.

When carbon forms a double bond, it undergoes sp2 hybridization, producing three equal orbitals.

When carbon forms a triple bond, it undergoes sp hybridization, producing two equal orbitals.

Unit 15: Energetics and Thermochemistry

Energetics and Thermochemistry

Subtopic Subtopic Number IB Points to Understand
Energy cycles 15.1 (HL) The first ionization energy is the minimum energy required to remove one mole of electrons from one mole of gaseous atoms.

The first electron affinity is the enthalpy change when one mole of gaseous electrons is added to one mole of gaseous atoms.

Born–Haber cycle and enthalpy of formation

The lattice enthalpy is defined as the standard enthalpy change that occurs on the formation of 1 mol of gaseous ions from the solid lattice

The enthalpy of atomization ΔHat is the standard enthalpy change that occurs on the formation of 1 mol of separate gaseous atoms of an element

The ionization energy, ΔHIE, is the standard enthalpy change that occurs on the removal of 1 mol of electrons from 1 mol of atoms or positively charged ions in the gaseous phase.

Enthalpy change if solution and hydration

Entropy and spontaneity 15.2 (HL) The combination of enthalpy, entropy, and temperature of system can be used to define a new state function called Gibbs free energy

The Gibbs free energy change of formation, ΔGf, represents the free energy change when 1 mol of a compound is formed from its elements under standard conditions of 298 K and a pressure of 100 kPa

Unit 16: Chemical Kinetics

Chemical Kinetics

Subtopic Subtopic Number IB Points to Understand
Rate expression and reaction mechanism 16.1 (HL) A catalyst is a substance that increases the rate of a chemical reaction, but is not consumed in the reaction itself. A catalyst provides an alternative pathway for the reaction and lowers the activation energy, Ea

Reactions may occur by more than one step and the slow step determines the rate of the reaction. The slow step is termed the rate-determining step (RDS

Zero to third order reaction

Activation energy 16.2 (HL) The activation energy is the minimum amount of energy required for reaction to take place.

Arrhenius equation

Unit 17: Equilibrium

Equilibrium

Subtopic Subtopic Number IB Points to Understand
The equilibrium law 17.1 (HL) Calculating equilibrium constant using the ICE Method

The Gibbs free energy change ∆G for a given reaction is an indication of whether the forward or reverse reaction is favored.

Unit 18: Acids and Bases

Acids and Bases

Subtopic Subtopic Number IB Points to Understand
Lewis acids and bases 18.1 (HL) A Lewis acid is a lone pair acceptor.

A Lewis base is a lone pair donor

A nucleophile (‘likes nucleus’) is an electron-rich species that donates a lone pair to form a new covalent bond in a reaction

An electrophile (‘likes electrons’) is an electron-deficient species that accepts a lone pair from another reactant to form a new covalent bond

Calculations involving acids and bases 18.2 (HL) Calculating acid dissociation constant Ka and the base dissociation constant Kb

The relationship between the acid dissociation constant for a weak acid and the base dissociation constant of its conjugate base can be useful in calculation

The stronger the acid, the larger the Ka

The weaker the acid, the larger the pKa

pH curves 18.3 (HL) A buffer is a solution that resists a change in pH upon the addition of small amounts of a strong base or strong acid, or upon the dilution of the buffer through the addition of water

The change in pH does not show a linear relationship with the volume of base added, partly due to the logarithmic nature of the pH scale

    • Titration of a strong acid with a strong base: pH at equivalence = 7
    • Titration of a weak acid with a strong base: pH at equivalence > 7
  • Titration of a strong acid with a weak base: pH at equivalence < 7
  • Titration of a weak acid with a weak base: pH at equivalence – difficult to identify

An indicator is typically a weak acid or a weak base that displays a different color in acidic or alkaline environments

Different indicators must be used for different titrations, depending on the pH at the equivalence point.

Unit 19: Redox Processes

Redox Processes

Subtopic Subtopic Number IB Points to Understand
Electrochemical cells 19.1 (HL) Electroplating – It is a process of deposition of a thin layer of a metal over another using an electrolytic process.

A Standard Hydrogen Electrode (SHE) is an electrode that scientists use for reference on all half-cell potential reactions

A voltaic cell generates an electromotive force (EMF) resulting in the movement of electrons from the anode to the cathode via the external circuit. 

Unit 20: Organic Chemistry

Organic Chemistry

Subtopic Subtopic Number IB Points to Understand
Types of organic reactions 20.1 (HL) SN2 reactions and primary halogenoalkanes: Nucleophilic substitution in primary halogenoalkanes proceed in one step. The rate- determining step involves both the halogenoalkane and the nucleophile. 

Drawing mechanisms for SN2 reactions

SN1 reactions and tertiary halogenoalkanes: Tertiary halogenoalkanes undergo nucleophilic substitution reactions that involve two steps. The rate-determining step involves only the halogenoalkane. 

Drawing mechanisms for SN1 reactions

The rate of a nucleophilic substitution reaction depends on three main factors: Identity of the halogen, Classes of the halogenoalkane and the Choice of Solvent

The major products of the electrophilic addition of hydrogen halides to unsymmetrical alkenes can be predicted using Markovnikov’s rule.

Electrophilic addition of halogens to alkanes and interhalogens to alkenes

Interhalogens are compounds in which two or more halogens are combined in a molecule.

Electrophilic substitution reactions and its drawing mechanism

Carboxylic acids are reduced to aldehydes and eventually to primary alcohols while ketones are reduced to secondary alcohols, in reactions that are the reverse of the oxidation of alcohols.

Synthetic routes 20.2  (HL) Organic synthesis takes a starting material and converts it via a series of reactions into the desired product.

Retrosynthesis

Stereoisomerism 20.3  (HL) Stereoisomers have an identical molecular formula and bond multiplicity but show different spatial arrangements of the atoms. 

Stereoisomers can be subdivided into two major classes, conformational isomers and configurational isomers.

Conformational isomers therefore differ from one another in the arrangement of atoms around a single bond.

Configurational isomers can be interconverted only by the breaking of bonds or through the rearrangement of the stereocenters.

Cis–trans isomers are determined by the positions of substituents relative to a reference plane. 

Optical isomerism is a type of configurational isomerism determined by the presence of chiral carbon atoms.

Plane polarized light

Diastereomers and Enantiomers

Unit 21: Measurement and Analysis

 

Subtopic Subtopic Number IB Points to Understand
Spectroscopic Identification of organic compounds 21.1  (HL) A high-resolution 1HNMR spectrum can show further splitting of some absorptions.

Splitting patterns result from spin–spin coupling.

Single X-ray Crystallography is a scientific method used to determine the arrangement of atoms of a crystalline solid in three dimensional space.

OPTION A: Materials

Materials

Subtopic Subtopic Number IB Points to Understand
Materials science introduction A.1 (SL) Metallic substances exhibit metallic bonding. This makes them strong, malleable, and good conductors of heat and electricity. 

Ceramics are traditionally inorganic non-metallic solids formed between metals and non- metals. They have a crystalline structure

Polymers form a third classification of materials based on bonding. Plastics are covalently bonded long chain molecules

Composites are mixtures composed of two distinct phases: a reinforcing phase embedded in a matrix.

Bond triangle diagram

Metals and inductively coupled plasma (ICP) spectroscopy A.2 (SL) Reduction of iron ore in the blast furnace

Reduction by a more reactive metal

Alloys are homogeneous mixtures of metals with other metals or non-metals.

Paramagnetic materials are attracted to a magnetic field whereas diamagnetic materials create a magnetic field opposed to the applied field; and are therefore weakly repelled by an external magnetic field.

In a ferromagnetic material the electron alignment induced by the magnetic eld can be retained, making a permanent magnet.

Spectroscopic methods: atomic emission spectroscopy, optical emission spectroscopy, mass spectrometry

Catalysts A.3 (SL) A homogeneous catalyst is in the same phase as the reactants, takes the part of a reactant, and is reformed as a product at the end of the reaction.

A heterogeneous catalyst is in a different phase than that of the reactants.

The mechanism by which the activation energy is lowered varies between homogeneous and heterogeneous catalysts.

Nanocatalysts and Transition metal catalysts

Zeolites: They are microporous substances made of alumina silicate which has a cage-like structure providing a large surface area

Liquid crystals A.4 (SL) Liquid crystals are a state of matter intermediate between crystalline and liquid. 

Thermotropic liquid-crystal materials are pure substances that show liquid-crystal behavior over a temperature range between the solid and liquid states.

Lyotropic liquid crystals are solutions that show the liquid-crystal state at certain concentrations.

The nematic liquid-crystal phase is characterized by rod-shaped molecules that are randomly distributed but on average align in the same direction.

Forming LCD displays

Polymers A.5 (SL) A polymer is a molecule i.e. formed by joining many small molecules called monomers.

Polymers can be classified as thermoplastics and thermosets based on their behavior when heated.

Elastomers are flexible polymers that return to their original shape after being deformed.

Polyvinyl chloride (PVC), is a synthetic resin made from the polymerization of vinyl chloride (chloroethene).

Polystyrene (polyphenylethene, (C8H8)n) is a thermoplastic polymer made from the monomer styrene.

Isotactic, Atactic, and Syndiotactic addition polymers

Identifying monomers

Atom economy is the measure of the amount of starting materials that end up as useful/desired products.

Nanotechnology A.6 (SL) Nanotechnology deals with the manipulation and control of atoms, molecules, and objects with dimensions of less than 100 nm

Methods of producing nanotubes include arc discharge, chemical vapor deposition (CVD), and high pressure carbon monoxide disproportionation (HiPCO)

Arc Discharge using carbon electrodes and metal electrodes

Chemical vapor deposition

Environmental impact: Plastics A.7 (SL) Green chemistry, also known as sustainable chemistry, is the design of chemical products and processes that reduce or eliminate the use or generation of hazardous substances.

The name “dioxins” refers to a class of environmental pollutants that are POPs. Certain dioxin-like polychlorinated biphenyls (PCBs) with similar toxic properties are sometimes included in the term “dioxins”

Recycling of plastics

Superconducting metals and X-ray crystallography A.8 (HL) Superconductors are materials that offer no resistance to electric currents below a critical temperature.

The Meissner effect is the ability of a superconductor to create a mirror image magnetic field of an external field, thus expelling it.

Resistance in metallic conductors is caused by collisions between electrons and positive ions of the lattice.

The Bardeen–Cooper–Schrieffer (BCS) theory explains that below the critical temperature electrons in superconductors form Cooper pairs which move freely through the superconductor.

Type 1 superconductors have sharp transitions to superconductivity whereas Type 2 superconductors have more gradual transitions.

X-ray diffraction can be used to analyze structures of metallic and ionic compounds.

Crystal lattices contain simple repeating unit cells.

The number of nearest neighbors of an atom/ion is its coordination number.

Condensation polymers A.9 (HL) Condensation polymers are polymers formed through a condensation reaction where molecules join together, losing small molecules as byproducts such as water or methanol.

In condensation polymerization, many monomers are joined by condensation reactions to form the polymer.

The esterification reaction: Acyl chlorides react with amines rather than alcohols in a condensation reaction that forms an amide.

Phenol-methanol plastics, polyurethanes

Polymer properties

Environmental impact: Heavy metals A.10 (HL) “Heavy metals” is a term that refers to toxic metals which have cumulative effects on health.

Chelating agents are used to remove heavy metals such as lead, arsenic, and mercury from the body. 

Absorption of heavy metals

Option B: Biochemistry

Biochemistry

Subtopic Subtopic Number IB Points to Understand
Introduction to Biochemistry