chemistry unit 1 .3

1 understand the terms: • shells, sub-shells and orbitals • principal quantum number (n) • ground state, limited to electronic configuration 2 describe the number of orbitals making up s, p and d sub-shells, and the number of electrons that can fill s, p and d sub-shells 3 describe the order of increasing energy of the sub-shells within the first three shells and the 4s and 4p sub-shells 4 describe the electronic configurations to include the number of electrons in each shell, sub-shell and orbital 5 explain the electronic configurations in terms of energy of the electrons and inter-electron repulsion 6 determine the electronic configuration of atoms and ions given the atomic or proton number and charge, using either of the following conventions: e.g. for Fe: 1s2 2s2 2p6 3s2 3p6 3d6 4s2 (full electronic configuration) or [Ar] 3d6 4s2 (shorthand electronic configuration) 7 understand and use the electrons in boxes notation e.g. for Fe: [Ar] 8 describe and sketch the shapes of s and p orbitals 9 describe a free radical as a species with one or more unpaired electrons