CHEM 211 Lecture Notes - Lecture 1: Molecular Orbital Theory, Irreducible Representation, Atomic Orbital

• School: Queen's University
• Department: Chemistry
• Course: CHEM 211
• Professor: Philip G Jessop

Document Summary

Groups 13 boron: b al; makes sense that atomic radius increases, al ga; atomic orbital remains constant; less shielding since added e- go into d orbital. Therefore, feeling the nucleus positive charge and it doesn"t get easier to pull e- off (ionization energy barely changes) In ti; another stall, because we are adding the f orbital. Boron allotropes: different forms of the same element (eg. carbon, most common is -rhombohedral boron, pure bh3; no lone pairs. Interacts with other bh3 bonds it is desperate for e- Looking at h"s: get reducible representation; must break them down, get 2 lgos (since 2 hydrogens, 12e- total; 8 e- used up in terminal ends of b---h bonds so 4 e- leftover in mo diagram.