Structure 1.3 : Electron configurations Structure 1.3.1 : Qualitatively describe the relationship between colour, wavelength, frequency and energy across the electromagnetic spectrum. Distinguish between a continuous and a line spectrum. Structure 1.3.2 : Describe the emission spectrum of the hydrogen atom, including the relationships between the lines and energy transitions to the first, second and third energy levels. Structure 1.3.3 : Deduce the maximum number of electrons that can occupy each energy level. Structure 1.3.4 : Recognize the shape and orientation of an s atomic orbital and the three p atomic orbitals. Structure 1.3.5 : Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to deduce electron configurations for atoms and ions up to Z = 36. Structure 1.3.6 : Explain the trends and discontinuities in first ionization energy (IE) across a period and down a group. Calculate the value of the first IE from spectral data that gives the wavelength or frequency of the convergence limit. Structure 1.3.7 : Deduce the group of an element from its successive ionization data.

Structure 1 / IB Chemistry / Structure 1.2 Structure 1.2 : The nuclear atom Structure 1.2.1 : Use the nuclear symbol A Z X to deduce the number of protons, neutrons and electrons in atoms and ions. Structure 1.2.2 : Perform calculations involving non-integer relative atomic masses and abundance of isotopes from given data. Structure 1.2.3 : Interpret mass spectra in terms of identity and relative abundance of isotopes.

Structure 1 / IB Chemistry / Structure 1.5 (Including worksheets) Structure 1.5- Ideal gases Structure 1.5.1 - An ideal gas consists of moving particles with negligible volume and no intermolecular forces. All collisions between particles are considered elastic. Structure 1.5.2 - Real gases deviate from the ideal gas model, particularly at low temperature and high pressure. Structure 1.5.3 - The molar volume of an ideal gas is a constant at a specific temperature and pressure. Structure 1.5.4 - The relationship between the pressure, volume, temperature and amount of an ideal gas is shown in the ideal gas equation PV = nRT

Chemistry IB _ Grade 11 and 12 Topic 3 : Periodicity

Structure 2.3 : The metallic model Structure 2.3.1 : A metallic bond is the electrostatic attraction between a lattice of cations and delocalized electrons. Structure 2.3.2 : The strength of a metallic bond depends on the charge of the ions and the radius of the metal ion. Structure 2.3.3 : Transition elements have delocalized d-electrons. Structure 2.4 : From models to materials Structure 2.4.1 : Bonding is best described as a continuum between the ionic, covalent and metallic models, and can be represented by a bonding triangle. Structure 2.4.2 : The position of a compound in the bonding triangle is determined by the relative contributions of the three bonding types to the overall bond. Structure 2.4.3 : Alloys are mixtures of a metal and other metals or non-metals. They have enhanced properties. Structure 2.4.4 : Polymers are large molecules, or macromolecules, made from repeating subunits called monomers. Structure 2.4.5 : Addition polymers form by the breaking of a double bond in each monomer.Structure 2.4.6 : Condensation polymers form by the reaction between functional groups in each monomer with the release of a small molecule.

Atoms, Elements, Compounds, and mixtures

Structure 1 / IB Chemistry / Structure 1.4 Structure 1.4—Counting particles by mass: The mole Structure 1.4.1 Structure 1.4.2 Structure 1.4.3 Structure 1.4.4 Structure 1.4.5 Structure 1.4.6

Structure 2 / IB Chemistry / Structure 2.2 (lesson / Worksheets / Tests/ Tables / Figures) Structure 2.2—The covalent model Structure 2.2.1—A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei. Structure 2.2.2—Single, double and triple bonds involve one, two and three shared pairs of electrons respectively. Structure 2.2.3—A coordination bond is a covalent bond in which both the electrons of the shared pair originate from the same atom. Structure 2.2.4—The valence shell electron pair repulsion (VSEPR) model enables the shapes of molecules to be predicted from the repulsion of electron domains around a central atom. Structure 2.2.5—Bond polarity results from the difference in electronegativities of the bonded atoms. Structure 2.2.6—Molecular polarity depends on both bond polarity and molecular geometry. Structure 2.2.7—Carbon and silicon form covalent network structures. Structure 2.2.8—The nature of the force that exists between molecules is determined by the size and polarity of the molecules. Intermolecular forces include London (dispersion), dipole-induced dipole, dipole–dipole and hydrogen bonding. Structure 2.2.9—Given comparable molar mass, the relative strengths of intermolecular forces are generally: London (dispersion) forces < dipole–dipole forces < hydrogen bonding. Structure 2.2.10—Chromatography is a technique used to separate the components of a mixture based on their relative attractions involving intermolecular forces to mobile and stationary phases.

Chemistry IB _ Grade 11 and 12 Topic 1 : Stoichiometric relationships

All the worksheets for IB chemistry topic 1 to 11 1 - Stoichiometrics 2 & 12 - Atomic Structure 3 & 13 - Periodicity 4 & 14 - Bonding & Structure 5 & 15 - Energetics 6 & 16 - Kinetics 7 & 17 - Equilibrium 8 & 18 - Acids & Bases 9 & 19 - Redox Processes 10 & 20 - Organics 11 & 21 - Measurements & Data

Chemistry IB _ Grade 11 and 12 Topic 10 : Organic chemistry

Chemistry IB _ Grade 11 and 12 Topic 7 : Equilibrium

Chemistry IB _ Grade 11 and 12 Topic 8 : Acids and bases

Chemistry IB _ Grade 11 and 12 Topic 6 : Chemical kinetics

Chemistry IB _ Grade 11 and 12 Topic 2 : Atomic structure

Chemistry IB _ Grade 11 and 12 Topic 5 : Energetics/thermochemistry

Chemistry IB _ Grade 11 and 12 Topic 11 : Measurement and data processing

MYP chemistry Grade 9 and grade 10 year 8 and year 10

1 - Particle Theory _ changes of State and Gas Pressure 2 - Diffusion and Investigating Diffusion

Structure 1 / IB Chemistry / Structure 1.1 Structure 1.1 : Introduction to the particulate nature of matter Structure 1.1.1 : Distinguish between the properties of elements, compounds and mixtures. Structure 1.1.2 : Distinguish the different states of matter. Use state symbols (s, , g and aq) in chemical equations. Structure 1.1.3 : Interpret observable changes in physical properties and temperature during changes of state. Convert between values in the Celsius and Kelvin scales.