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CHEM 1A: VSEPR Theory Now that we have an understanding of covalent bonding and how atoms share electrons to form molecules and polyatomic ions, we will use Lewis dot structures to predict electronic and molecular geometries.
According to the Valence Shell Electron Pair Repulsion (VSEPR) Theory, the areas of high electron density move as far apart from each other as possible, without leaving the atom. It is the repulsion of lone pairs of electrons that causes the geometry or molecular structure of the molecule.
The VSEPR (Valence Shell Electron Pair Repulsion) theory predicts the shape of a molecule based on the repulsion between electron pairs in the valence shell of the central atom. In CCl4 (carbon tetrachloride), the central carbon atom is surrounded by four chlorine atoms.
For each molecule below, (i) draw the Lewis structure with nonbonding electrons, (ii) determine the number of nonbonding lone pairs and bonding pairs on the central carbon atom, and (iii) predict the electron domain and molecular geometries using the VSEPR model.
Lewis Structures, VSEPR, Polarity, IM Forces - Answers For each of the following molecules, draw the Lewis structure (with any resonance structures, if applicable), indicate the molecular shapes and bond angles, indicate the molecular polarity (if any), and identify the major intermolecular force in each compound. Hint – in this worksheet, as in
Draw Lewis dot diagrams to represent valence electrons in elements and draw Lewis dot structures to show covalent bonding. Use valence shell electron pair repulsion (VSEPR) model to draw and name molecular shapes (bent, linear, trigonal planar, tetrahedral, and trigonal pyramidal).
VSEPR Worksheet 1) What is the main idea behind VSEPR theory? 2) For each of the following compounds, determine the bond angles, molecular shapes, and hybridizations for all atoms: a) carbon tetrachloride b) BH3 c) silicon disulfide d) C2H2 e) PF3
