Atomic structure
Chemistry · Unit 1 — Chemical fundamentals — structure, properties and reactions · Properties and structure of atoms
Learning objectives (39)
LO-1Analyse data for atomic radii, valencies, ionic radii, 1st ionisation energy and electronegativities to determine periodic trends, patterns and relationships. Introduction to bondingLO-2Analyse flame tests and atomic absorption spectroscopy (AAS) to identify elements and determine the concentration of metallic ions in solution. Chem istry 2025 v1.3 Periodic table and trendsLO-3Analyse mass spectrometry spectra, to determine the isotopic composition of elements, the relative atomic mass of an element and percentage abundances of the isotopes of an element.LO-4Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 36.LO-5Apply the nuclear symbol notation M𝑍 𝐴 to determine the number of protons, neutrons and electrons in atoms, ions and isotopes.LO-6atomic absorption spectroscopy (AAS) and the concentration of aqueous metallic ions.* *Note: Simulations may be used.LO-7Compare the metallic and non-metallic behaviours of elements, including group trends and the reactivity for the alkali metals (Li–Cs) and the halogens (F–I).LO-8Describe that atoms can be modelled as a nucleus surrounded by electrons in distinct energy levels.LO-9Describe that isotopes are atoms of the same element that have different numbers of neutrons.LO-10Describe the relationship between the structure of the periodic table and the electronic configuration of atoms.LO-11Determine full and condensed electron configurations for atoms and ions up to Z = 36, e.g. 1s2 2s2 2p6 3s2 3p5 and [Ne]3s2 3p5.LO-12Determine Lewis (electron dot) structure of molecules and ions showing all valence electrons for up to four electrons pairs for each atom.LO-13Determine the formula and IUPAC name of ionic and molecular compounds.LO-14Discriminate between absorption and emission line spectra.LO-15Discriminate between the terms atomic number (Z), mass number (A) and isotopes of an element.LO-16Discriminate between the terms empirical formula, molecular formula and the formula unit.LO-17Explain how successive ionisation energy data is related to the electron configuration of an atom. IsotopesLO-18Explain that chemical bonds are caused by electrostatic attractions that arise because of the sharing or transfer of electrons.LO-19Explain that elements of the periodic table show trends in chemical and physical properties across periods and down groups as exemplified by groups 1, 2, 13 –18 and period 3.LO-20Explain that flame tests and atomic absorption spectroscopy (AAS) rely on electron transfer between atomic energy levels.LO-21Explain that ions are atoms or groups of atoms that are electrically charged due to an imbalance in the number of electrons and protons.LO-22Explain that the ability of atoms to form chemical bonds, is related to the arrangement of electrons in the atom and the stability of the valence electron shell.LO-23Explain that the emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels (Bohr model), which converge at higher energies.LO-24Explain that the relative atomic mass of an element is the ratio of the weighted average mass per atom of the naturally occurring form of the element to 1/12 the mass of an atom of carbon-12. Analytical techniquesLO-25flame tests to identify elementsLO-26Identify that isotopes of an element have the same electron configuration and possess similar chemical properties but have different physical properties.LO-27Identify that oxides change from basic through amphoteric to acidic across period 3.LO-28Identify that the number of electrons lost, gained or shared is determined by the electron configuration of the atom.LO-29Identify that the periodic table is arranged into four blocks associated with the four sub -levels — s, p, d and f.LO-30Identify that the structure of the periodic table based on increasing atomic number.LO-31Identify that the valency is a measure of the number of bonds that an atom can form.LO-32Identify the electron configuration of Cr and Cu as exceptions.LO-33Identify the numbers of bonding and lone pairs of electrons around each atom in a molecule. Chem istry 2025 v1.3LO-34mass spectra and isotopes*LO-35State that elements are represented by symbols.LO-36State that isotopes can be represented in the form AX (IUPAC) or X-A.LO-37State that mass spectrometry involves the ionisation of substances and the separation and detection of the resulting ions. (The operation of the mass spectrometer is not required.)LO-38State that transition elements can form more than one ion.LO-39State the relative energies of the s, p and d orbitals.
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