Module 2
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principal quantum number
shell number/energy level
shapes of orbitals in s and p subshells
s: sphere p: dumbbell
why are ionic compounds generally soluble in polar solvents?
• ion-dipole interactions between ions and polar molecules are stronger than the ionic bonds between ions • therefore the ionic lattice breaks down and polar molecules surround the ions (energy released in the formation of ion-dipole interactions is greater than the energy required to break ionic bonds)
how do ionic compounds act as electrical conductors when molten or aqueous?
ions act as mobile charge carriers
ionic vs covalent bonds
ionic: - attracts in all directions (in three dimensions) - stronger covalent: - localised attraction (solely between shared pair of e- and nuclei of bonding atoms) - weaker
which periods can expand their octet?
period 3+
electronegativity
the ability of an atom to attract an e- pair in a covalent bond
why is a molecule polar? (2 marks)
• difference in electronegativity between atom A and atom B causes a dipole • the dipoles are assymetrical/do not cancel out
factors affecting IMF strength between inorganic molecules
• number of e- • charge of atoms in molecule
state and explain two anomalous properties of ice. (4 marks)
• ice is less sense than water –> H bonds between water molecules form an open lattice structure • ice has a relatively high melting point –> strong H bonds require a lot more energy to overcome
two types of isomerism
• structural • stereoisomerism
types of structural isomerism
• branched • positional • functional
types of stereoisomerism
• cis/trans • E/Z • optical
what is meant by the term weighted mean mass
mean average mass taking into account the abundance of the isotopes
order molecular structures from highest to lowest melting/boiling point
• giant covalent • metallic • ionic • simple covalent
define electronegativity
a measure of attraction of an atom in a bonded pair for the pair of electrons in a covalent bond
define electron affinity
the ability of an atom to accept an electron e- + X –> X-