Polarity and Intermolecular Forces Assignment.pdf

Polarity and Intermolecular Forces Assignment.pdf - Divya...

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Divya Dadar Polarity and Intermolecular Forces Assignment 1. Use the VSEPR theory to predict the shape of methane (CH4). Then indicate whether the bonds are polar. Will the molecule be polar? - The methane molecule is tetrahedral since there are four pairs of electrons and has no lone pairs. - CH4 has one carbon atom bonded to 4 hydrogen atoms. The four hydrogen atoms are placed at the vertices of tetrahedron. - There is an equal sharing of electrons and no lone pairs, the EN difference is less than 0.5 therefore, the bonds are nonpolar and the molecule is nonpolar as well - The bond angle is 109.5 - The molecular shape of CH4: (triangular faced pyramid) Figure 1: VSEPR diagram of methane(VibeThemes, 2018) 2. Using electronegativity values, determine bond polarities and the net dipoles in a molecule of PCl3 and indicate if the molecule will be polar. The electronegativity value of phosphorus is 2.1 and the electronegativity value of chlorine is 3.0 The EN difference is greater than 0.5 knowing that has polar bonds It contains one lone pair, four pairs of electrons and three bonding pairs → due to this structure, using VSEPR theory, it is identified with a geometrical arrangement of tetrahedron
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Divya Dadar However, due to its one lone pair its molecular shape is trigonal pyramidal, due to the fact that one corner is different from the others As chlorine is electronegative than phosphorus the dipole moment would all be towards chlorine, facing down in the molecule The dipoles do not cancel out as they are all in the same direction meaning the molecule is polar Figure 2:
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