Draw the lewis structure of XeCl4 showing all lone...

Question

Draw the lewis structure of XeCl4 showing all lone pairs.XeCl4 molecule isa. polar.b. nonpolar.What are the approximate bond angles in XeCl4?Select all that applya. 90 degreesb. 109.5 degreesc. 120 degreesd. 180 degreesIdentify the molecular geometry of XeCl4a. tetrahedralb trigonal bipyramidalc. T-shapedd. lineare. see-sawf. octahedralg. square pyramidalh. benti. trigonal pyramidalj. square planark. trigonal planar

Jules Bruno · Accepted Answer

For this problem, we need to do the following steps:Step 1: Determine the central atom in this molecule.Step 2: Calculate the total number of valence electrons present.Step 3: Draw the Lewis structure for the molecule.Step 4: Draw dipole arrows for each bond.Step 5: Determine the polarity of the molecule.Step 1: Xe is less electronegative than chlorine so chlorine is the central atom.Step 2: The total number of valence electrons present in XeCl4 is:            Group             Valence ElectronsXe        8A                   1 × 8 e– = 8 e–Cl         7A                   4 × 7 e– = 28 e–Total:  36 valence e–[readmore]Step 3: Halogens, when not the central atom, form only 1 bond, which means each of the chlorine form 1 bond. Xenon is bonded to 4 Cl The incomplete Lewis structure of XeCl4 is:A bond corresponds to 2 electrons shared between two atoms so we currently have 4 × 2 e– = 8 val. e–, which means we’re still lacking 28 e–. We can start adding the missing electrons to the atoms while following the octet rule. The complete Lewis structure is:Step 4: The electronegativity difference between Xe and Cl is 3.0 so the Xe–Cl bond is polar. Recall that dipole arrows point towards the more electronegative atom. Drawing the dipole arrows:Step 5: We can see that dipole arrows point in opposite directions so they cancel out. This means there is no net dipole in the molecule, making it nonpolar.Therefore, the  XeCl4 is a nonpolar molecule.Next is let's determine the approximate bond angles in XeCl4.Step 1: Determine the number of electron groups around the indicated atom.Step 2: Determine the electron geometry and bond angle using this:Electron Regions          Electronic Geometry          Bond Angles2                                      linear                                    180˚3                                      trigonal planar                      120˚4                                      tetrahedral                            109.5˚5                                      trigonal bipyramidal              90˚, 120˚, and 180˚6                                      octahedral                            90˚ and 180˚Step 1: Xe is surrounded by 6 electron groups: 4 bonds and 2 lone pairs.Step 2: Since there are 6 electron groups around xenon, the electron geometry is octahedral, whose ideal bond angles are 90° and 180°. Recall that lone pairs compress the bond angle, causing a deviation from the ideal bond angle.This means that the approximate bond angles in XeCl4 are a. 90 degrees and d. 180 degrees.Next is let's determine the molecular geometry of XeCl4.The shape of a molecule is based on its molecular geometry: when determining molecular geometry, atoms and lone pairs are treated differently. There are four atoms and two lone pairs around the central atom, which corresponds to AX4E2 or square planar.The molecular geometry of XeCl4 is square planar.

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