Write the Lewis structure for each molecule or ion. a. N₂H₂ b. N₂H₄ c. C₂H₂

Draw the Lewis structure for each organic compound from its condensed structural formula. a. C₃H₈ d. CH₃COOH

Draw the Lewis structure for each organic compound from its condensed structural formula. a. C₂H₄ b. CH₃NH₂ c. HCHO d. CH₃CH₂OH e. HCOOH

Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6% S and 30.4% N. Measurements of its molecular mass yield a value of 184.3 g/mol. The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (b) Write Lewis structures for the molecule, based on the information you are given. (Hint: You should find a relatively small number of dominant Lewis structures.)

Using Lewis symbols and Lewis structures, make a sketch of the formation of NCl₃ from N and Cl atoms, showing valence-shell electrons. (a) How many valence electrons does N have initially? (c) How many valence electrons surround the N in the NCl₃ molecule? (d) How many valence electrons surround each Cl in the NCl₃ molecule?

The gas-phase reaction of NO with F₂ to form NOF and F has an activation energy of Ea = 6.3 kJ/mol. and a frequency factor of A = 6.0 × 10⁸ M^-1 s^-1. The reaction is believed to be bimolecular: NO(g) + F₂(g) → NOF(g) + F(g) (b) Draw the Lewis structures for the NO and the NOF molecules, given that the chemical formula for NOF is misleading because the nitrogen atom is actually the central atom in the molecule.