Labels on household cleansers caution against mixing bleach with ammonia because the reaction produces monochloramine (NH2Cl) and hydrazine (N2H4), both of which are toxic. The balanced equations are shown below.      Draw the Lewis structure for monochloramine, which is a covalent compound with the formula NH2Cl. Include all nonbonding electrons, such as lone pairs, and any nonzero formal charges. Draw the Lewis structure for hydrazine, which has the formula N2H4. Include all nonbonding electrons, such as lone pairs, and any nonzero formal charges.

Consider the following ion: BrO3−. a)  Show the full electron configuration for Br.  b)  Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct.  c)  If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why.  d)  What is the electronic geometry of BrO3−? What is its molecular shape?  e)  Does BrO3− have a dipole moment? Briefly justify your answer.  f)  On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer.  g)  Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice.  h)  What is the molecular formula for Compound C? What is the empirical formula for Compound C?  please answer c, d and e

Although carbon has four bonds in stable molecules, sometimes reactive carbon intermediates that contain carbon atoms without four bonds are formed for very short time periods. Examples of these unstable intermediates include the methyl carbocation (CH 3) + and the methyl carbanion (CH 3) −. Draw Lewis structures for both unstable ions and predict the shape around carbon.

Write the Lewis symbols for boron and sulfur.