Molecule #7 BrF4* Calculate the number of valence electrons Draw the three-dimensional structure of the molecule using the "wedge and dash" notation. Our logic for this choice is: Draw the Lewis Structure below The molecular geometry is: This molecule is polar nonpolar (Circle your choice.) The formal charge on Br is The hybridization of Br is The formal charge on F is Estimate F-Br-F bond angle

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Which statements about resonance are correct? Select all that apply When drawing resonance structures, it is okay to move atoms around as needed. New formal charges can be created when doing resonance, so long as the overall charge of the molecule is the same in all structures. • Hybridization of atoms can change when involved in electron movement Sigma bonds cannot be messed with in resonance Resonance occurs because it helps stabilize molecules ●

- Complete the table. Number of electron groups Bond angle Outer atoms/Lone pairs 2 ? 2/0 3 4 ? ? bond angle in a two electron group molecule: bond angle in a three electron group molecule: bond angle in a four electron group molecule: 3/0 2/1 4/0 3/1 2/2 Shape ? trigonal planar (planar triangular) ? tetrahedral ? bent The shape of a two electron group molecule is The shape of a three electron group molecule with two outer atoms and one lone pair is The shape of a four electron group molecule with three outer atoms and one lone pair is

Use the following information to determine the Lewis structure, find the electron and molecular geometry of the molecule, determine the angle of the molecule, and determine the polarity. If the atoms are not the same, you may assume that the difference in their electronegativities are between 0.4 and 2.0. Atom information: A: 8 valence electrons, CAN exceed the octet. Further from fluorine on the periodic table than X. X: 7 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic table than A. Molecule: AX4 Electron Geometry: [Select] Molecular Geometry: [Select] Bond Angle: [ Select ] Polarity: [ Select ]

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Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

A Lewis structure is a two-dimensional representation of a molecule that does not necessarily show what shape that molecule would take in three dimensions. Based on the Lewis structure and your knowledge of VSEPR theory, approximate the smallest bond angle in this molecule. XÿX smallest bond angle: O

Determine the number of electron groups around the central atom for each of the following molecules. OF2