CHM135H1 Lecture Notes - Lecture 4: Unpaired Electron, Lone Pair, Formal Charge
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CHM135H1 Full Course Notes
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Polar covalent bonds: when the electrons are equally shared between 2 nuclei: more electronegative atom- pulls the electrons closer. Electronegativity: intrinsic atomic ability to pull electrons to itself. Inductive effect: shifting of electrons to more electronegative atom. ** most chemical reactions wouldn"t occur w/o electronegativity differences b/w elements- they"d be too stable- never react with each other** En increases upward, and rightward: most electronegative compounds: f, o, n, cl, br. Electrostatic potential maps: show charge distributions within molecules. Ionic: en difference 2: red = electron rich (more electronegative, blue = electron poor (less electronegative) Arrow- indicate direction of electron shift (towards more electronegative element) Dipole moment: the net molecular polarity: symmetry cancels out dipole moments. Likes dissolve likes: polar solvents dissolve polar solutes, non-polar solvents dissolve non-polar solutes. Just a formality- there"s not a negative ionic charge on the molecule: helps to keep track of the number of valence electrons the atom. However, is helpful to figure out chemical reactivity/behaviour.
