Atomic Structure & Ionisation Energy - A Level Chemistry

OCR H432 · 2.2.1 · 3.1.1(a)–(c)

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2.2.1(a) the number of electrons that can fill the first four shells 2.2.1(b) atomic orbitals, including:
(i) as a region around the nucleus that can hold up to two electrons, with opposite spins
(ii) the shapes of s- and p-orbitals
(iii) 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 2.2.1(c) filling of orbitals:
(i) for the first three shells and the 4s and 4p orbitals in order of increasing energy
(ii) for orbitals with the same energy, occupation singly before pairing 2.2.1(d) deduction of the electron configurations of:
(i) atoms, given the atomic number, up to Z = 36
(ii) ions, given the atomic number and ionic charge, limited to s- and p-blocks up to Z = 36. 3.1.1(a) the periodic table as the arrangement of elements:
(i) by increasing atomic (proton) number
(ii) in periods showing repeating trends in physical and chemical properties (periodicity)
(iii) in groups having similar chemical properties 3.1.1(b) (i) the periodic trend in electron configurations across Periods 2 and 3 (see also 2.2.1 d)
(ii) classification of elements into s-, p- and d-blocks 3.1.1(c) first ionisation energy (removal of 1 mol of electrons from 1 mol of gaseous atoms) and successive ionisation energy, and:
(i) explanation of the trend in first ionisation energies across Periods 2 and 3, and down a group, in terms of attraction, nuclear charge and atomic radius
(ii) prediction from successive ionisation energies of the number of electrons in each shell of an atom and the group of an element

Atomic Structure & Ionisation Energy

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