IB Chemistry Topic 2 Atomic structure 2.2 Electron configuration

IB Chemistry Topic 2 Atomic structure 2.2 Electron configuration Experimental evidence of electron configurations using the hydrogen emission spectra. How to determine electron configurations and draw orbital diagrams. PPTs and quizzes are available on www.mrwengibchemistry.com 0:06 Electromagnetic spectrum 0:35 Emission spectra 1:01 Continuous vs emission spectrum 1:43 Demonstration of the hydrogen emission spectra 2:17 Spectral line series Lyman, Balmer, Pashen 3:36 Convergence 5:42 Electron shells 6:02 Principle energy levels and sublevels 8:07 Electron configurations from the Periodic Table 8:23 Electron configurations from diagram 9:54 Electron configuration notation 10:08 How to write electron configurations 10:49 How to write the orbital diagrams 11:27 Aufbau principle 11:49 Exceptions to the Aufbau principle Cr Cu 13:50 Electron configurations for ions 14:23 Electron configurations for transistion metal ions 15:03 Condensed written forms 15:37 Orbitals and analogy demonstration numbers and shapes 18:10 Examples of how to fill in orbital diagrams ​ 2.2 Electron configuration • Emission spectra are produced when photons are emitted from atoms as excited electrons return to a lower energy level. • The line emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels, which converge at higher energies. • The main energy level or shell is given an integer number, n, and can hold a maximum number of electrons, 2n2. • A more detailed model of the atom describes the division of the main energy level into s, p, d and f sub-levels of successively higher energies. • Sub-levels contain a fixed number of orbitals, regions of space where there is a high probability of finding an electron. • Each orbital has a defined energy state for a given electronic configuration and chemical environment and can hold two electrons of opposite spin. • Description of the relationship between colour, wavelength, frequency and energy across the electromagnetic spectrum. • Distinction between a continuous spectrum and a line spectrum. • Description of the emission spectrum of the hydrogen atom, including the relationships between the lines and energy transitions to the first, second and third energy levels. • Recognition of the shape of an s atomic orbital and the px, py and pz atomic orbitals. • Application of the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 36. Connect with me: Facebook:   / ibchemistry2016