Oxidation of the cyanide ion produces the stable cyanate ion, OCN⁻ . The fulminate ion, CNO⁻, on the other hand, is very unstable. Fulminate salts explode when struck;

 

Hg(CNO)₂ is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in OCN⁻ and N is the central atom in CNO⁻.)

 

Formic acid can lose the H bound to the oxygen atom as H', to give the conjugate base, format (CHO_2). Draw the resulting ion, and calculate the formal charge (show') of each atom. There is a second resonance form of format, in which the other oxygen atom has the negative charge. Draw the other resonance form, based on your first answer. Salts containing the fulminate ion (CNC^-) are used in explosive detonators. Draw three Lewis electron structures for CNO^- and use formal charges (show calculation) to predict which is more stable.

Draw a Lewis structure for the cyanate anion, OCN Show your work for counting electrons at each atom Assign formal charge at each atom Draw a resonance contributor for the above structure Assign formal charge at each atom Draw a Lewis structure for is cyanic acid. HNCO Show your work for counting electrons at each atom Assign formal charge at each atom Potassium cyanate and acetic acid were reacted together to form is cyanic acid and potassium acetate Write the reaction equation and label the acid-base/conjugate acid-conjugate base pairs. Look at the Lewis structures of the cyanate ion you drew in Question 1 (two resonance contributors) Protonation of the cyanate ion occurs at the N, not the O, to form HNCO, not HOCN. Explain why.

1. Which of the following in each pair has the larger bond angle? Why? a) CH4 and NHs b) OF2 and OCl2 c) NHs and NFs d) PHs and NHs 2. Predict the geometry (and draw, indicating approximate angles) and assign the point group to each of the following species: a) F2SeO b) SnCl2 c)I3 d) IO2F2 Write three reasonable Lewis dot structures for N20 (N is the central atom). Indicate which of the structures you have drawn is the most likely structure, and what is unfavorable with the others. 3. 4. Write a reasonable Lewis dot structure, assign formal charges and oxidation numbers, and predict the geometry and point group of each of the following: CIF, CIF3, ICl, HCIO