Draw Lewis structures for bromine nitrate (BRONO2) and bromine monoxide (Bro). (Draw all major resonance forms. Copy the given template as many times as needed. Assign lone pairs, radical electrons, and atomic charges where appropriate.) bromine nitrate (BrONO2): Marvin JS O Help H N F CI bromine monoxide (BrO): Marvin JS O Help

Two major resonance structures are possible for the anion shown. One resonance form is given, but it is incomplete. Complete the given structure by adding nonbonding electrons and formal charges. Draw the remaining structure, including nonbonding electrons and formal charges. Omit curved arrows. Structure A: complete the structure by adding nonbonding electrons and formal charges. H H H I Structure B: draw the remaining resonance structure, including nonbonding electrons and formal charges. H- : z: H H

Draw all resonance structures for the nitryl fluoride molecule, NO2F. Explicitly draw all H atoms. • Include all valence lone pairs in your answer. • Do not include overall ion charges or formal charges in your drawing. ● • Do not draw double bonds to oxygen unless they are needed for the central atom to obey the octet rule. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. ● Separate resonance structures using the ↔ symbol from the drop-down menu.

4. Draw two other reasonable resonance structures of this compound. Label each resonance form, including the one provided, as either "major" or "minor." :O: H3C H H

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Which is these isn’t a resonance structure

1. a) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula H2O b)draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula AsF5

Column I: Draw the best Lewis structure. Label any atoms with nonzero formal charge. Column II: List the total number of major resonance contributors and draw at least two (if they exist). Column III: How many electron groups are around the central atom? Column IV: What is the electron geometry? Column V: What is the molecular geometry? Possible answers: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, bent, trigonal pyramidal, see-saw, T-shaped, square pyramidal, square planar). Column VI: Give values of the bond angles around the central atom. (for example, 109.5°, less than 109.5°, 120°, less than 120°, etc.). Column VII: Give the hybridization of the central atom. Column VIII: State how many sigma bonds and pi bonds are present in the molecule or ion. Column IX: Is the molecule polar or non-polar?

Consider the resonance structure below: Draw an arrow pushing pattern to represent the flow of electrons that converts the first resonance structure into the second resonance structure?

1.a)draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula OF2 b) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula CH2Cl2