CHEM 1040 Lecture Notes - Lecture 4: Xenon Tetrafluoride, Electronegativity, Stereochemistry

• School: University of Guelph
• Department: Chemistry
• Course: CHEM 1040
• Professor: Abdelaziz Houman

Document Summary

Chemical properties mostly determined by # of valence electrons. Lack of reactivity of inert gases is associated with filled outer s and p shells. Lewis convention: chemical symbol stands for nucleus and inner electrons, outermost electrons are represented by dots (a line represents an electron pair) Lewis diagrams only useful when only have s and p electrons. To draw a lewis diagram you need the electron configuration or position in the periodic table. Atoms tend to achieve a complete outer shell either by: losing or gaining electrons (ionic bond, sharing (covalent bond) If too few electrons to satisfy all use double bonds or triple bonds until each has 8. If too many, add extra to central atom as lone pairs. To deduce the formal charges of an atom: assign one electron from each shared electron pairs and then and add those to the number of unshared electrons.