CHEM 105N 1st Edition Lecture 19 Outline of Last Lecture I. Polyatomic IonsOutline of Current Lecture I. ElectronegativityII. Non-Polar covalentIII. Polar covalentIV. Ionic bondsV. Valence-shell-electron-pair-repulsion-theoryVI. Bonding AnglesCurrent LectureI. Electronegativity:- Measure of an atom’s ability to attract bonding electrons- Nonmetals have a high ionization energy- Don’t like to lose electrons so they SHARE- The larger the atom, the smaller the electronegativity- As Group number decreases, so does electronegativity- As period number increases, so does electronegativity- Need a whole new periodic table when calculating electronegativity. Will not be shown on standard colorless tableII. Non-Polar covalent:- Equal sharing of electrons- Occurs between non-metals- Has almost NO electronegativity difference (0.0-0.4)III. Polar covalent:- Do NOT share equally- Moderate electronegativity difference (0.4-1.7)IV. Ionic Bonds:- Electron TRANSFER- Metal and nonmetal- LARGE electronegativity (1.7+)V. Valence-Shell-Electron-Pair-Repulsion-Theory:- Pairs are to be placed equally apart to minimize repulsion- Period #= # of valence electronsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Be- exception to octet ruleVI. Bonding Angles:-180⁰= linear-120⁰= trigonal planer- 109⁰=
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