Predict the charge of an ion from the electron configuration of the atom, including transition elements.
Define an ionic bond and deduce the formula and name of an ionic compound from its component ions, including polyatomic ions. Interconvert names and formulas of binary ionic compounds. Recall the following polyatomic ions by name and formula: ammonium (NH4+), hydroxide (OH-), nitrate (NO3-), hydrogen carbonate (HCO3-), carbonate (CO32-) sulfate (SO42-), and phosphate (PO43-)
Describe the structure of ionic compounds and explain their physical properties, including: volatility, electrical conductivity, and solubility. Describe lattice enthalpy as a measure of the strength of the ionic bond in different compounds, influenced by ion radius and charge.
Covalent bonding and forces
Define a covalent bond and deduce the Lewis formula of molecules and ions for up to four electron pairs on each atom. Understand and use the octet rule in molecules containing atoms with fewer than an octet of electrons, in both organic and inorganic examples.
Define single, double, and triple bonds and explain the relationship between the number of bonds, bond length, and bond strength.
Define a coordination bond and identify coordination bonds in compounds, including transition element complexes.
Understand the valence shell electron pair repulsion (VSEPR) model and predict the electron domain geometry and the molecular geometry for species with up to four electron domains. Recall how non-bonding pairs and multiple bonds affect bond angles.
Deduce the polar nature of a covalent bond from electronegativity values.
Recall bond polarity and molecular geometry as the factors governing molecular polarity, and deduce the net dipole moment of a molecule or ion.
Describe the structures and explain the properties of silicon, silicon dioxide, and carbons allotropes (diamond, graphite, fullerene, and graphene).
Understand the key intermolecular forces, including: London dispersion, dipole-induced dipole, dipole-dipole, and hydrogen bonding. Deduce the types of intermolecular forces present from the structural features of covalent molecules. Understand the term van der Waals forces as an inclusive term to include dipole-diploe, dipole-induced dipole, and London dispersion forces. Explain the occurrence of hydrogen bonds.
Compare the relative strengths of intermolecular forces. Explain the physical properties of covalent substances to include: volatility, electrical conductivity, and solubility in terms of their structure.
Understand chromatography as a technique used to separate the components of a mixture based on their relative attractions involving intermolecular forces to mobile and stationary phases. Explain, calculate, and interpret the retention factor values,Rf.
Metallic bonds
Define a metallic bond. Explain the electrical conductivity, thermal conductivity, and malleability of metals. Relate characteristic properties of metals to their experimental uses.
Understand that the strength of a metallic bond depends on the charge of the ions and the radius of the metal ion. Explain trends in melting points ofsandpblock metals.