IBDP HL atomic structure
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Transcript of IBDP HL atomic structure
HL Atomic Structure
Sketch the graph of first ionisation energies.What other evidence do we have for electron
sub levels ?http://www.ptable.com/
Aims
• Show how successive ionization energy data is related to the electron configuration of an atom.
Trends in the PT
Sub Levels Evidence
Further Evidence
Problem
• Predict which element in each of the following pairs has the larger first ionization energy.
• (a) Na or Mg
• (b) Mg or Al
• (b) B or Al
• (c) F or Cl
Definitions
• Aufbau– Lowest energy filled first
• Hund– Same sub-shell – singly first
• Pauli– no two electrons in the same atom can be in the
same quantum state
s p d f shapes
http://lincoln.pps.k12.or.us/lscheffler/OrbitalShapesOverheads.htm
Picturing Electrons
Filling Orbitals
• http://www.youtube.com/watch?v=fv-YeI4hcQ4&feature=fvw
Orbitals
• Rules :-– Electrons are found in orbitals– 2 electrons in each orbital – with opposite ‘spin’– They will pair up only when all empty orbitals are
filled.– S can hold 2– P can hold 6 ( px, py and pz )– D can hold 10 – F can hold 14
Order of Filling of Orbitals
Order of Filling of Orbitals
Blocks in the PT
How To ….
• Use the Periodic Table to find the atomic number, and hence number of electrons.
• Fill up orbitals in the order 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p - until you run out of electrons. The 3d is the awkward one - remember that specially. Fill p and d orbitals singly as far as possible before pairing electrons up.
Task
• Write a ‘how to fill electronic orbitals help sheet’
• Include 10 elements with their full electron configuration 3 from s block – 3 from p block and 4 from d block.
HL Atomic Theory
• Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 54.
What is electron configuration of
• Ca
• C
• Zn
• S
Cu and Cr Chromium and Copper have electron configurations [Ar] 3d5 4s1 and [Ar] 3d10 4s1 respectively
Ions Notation
Sc - (Ar) 4s2 3d1Ti - (Ar) 4s2 3d2V - (Ar) 4s2 3d3Cr - (Ar) 4s1 3d5Mn - (Ar) 4s2 3d5Fe - (Ar) 4s2 3d6Co - (Ar) 4s2 3d7Ni - (Ar) 4s2 3d8Cu - (Ar) 4s1 3d10Zn - (Ar) 4s2 3d10
Plenary
• Questions 58 - 60
Starter
Let’s Balloon