Oxidation of the cyanide ion produces the stable cyanate ion, OCN-. The fulminate ion, CNO- , on the other hand, is very unstable. In fact, fulminate salts explode when struck; mercury(II) fulminate, Hg(CNO)2 , is used in blasting caps. Draw the Lewis structures and assign formal charges for the cyanate ion and the fulminate ion. ( C is the central atom in OCN- and N is the central atom in CNO-). Assign non-zero formal charges next to each atom. Include all valence lone pairs in your answer. 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. Do not use the square brackets tool in your answer.

The Lewis structure for the chlorate ion is :0: Calculate the formal charge on the chlorine (Cl ) atom. Express your answer as an integer. • View Available Hint(s) formal charge on Cl = Submit Part B Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure. :0: Express your answers as integers separated by commas. • View Available Hint(s) formal charge on Oa , Ob , Oc = Submit ormal charges to predict the most stable structure he interactive activity shows how to calculate the formal charge of atoms in a structure. These formal charges can be used to predict the resonance structure that contributes most to the stability of a molecule or ion. The struc enerally the most stable. Part C What are the formal charges on the sulfur (S), carbon (C ), and nitrogen (N ) atoms, respectively, in the resonance structure that contributes most to the stability of the thiocyanate ion, SCN¯ ? The possible resonance structures for the thiocyanate…

(b) The Murchison meteorite that landed in Australia in 1969 contained 92 different amino acids, including 21 found in Earth organism A skeleton structure (single bond only) of one of these extraterrestrial amino acids is shown below. Draw a Lewis structure, and identify any atoms having a nonzero formal charge. H3N. C ČH2 ČH3 (c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F, 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smaller going down the halogen group from HF to HI Describe these observations

A student proposes the following Lewis structure for the isocyanate NCO− ion. Assign a formal charge to each atom in the student's Lewis structure.

Draw the Lewis structure with lowest formal charges, and determine the charge of each atom in (a) IF₅; (b) AlH₄⁻

Consider the molecule QR3 , where Q has 7 valence electrons and R has 6 valence electrons. Both -1 elements are in the third period or below. (a) On your scratch paper, draw the BEST Lewis structure. Don't forget resonance, if applicable. (b) Show the formal charges for all elements.

Give detailed Solution

Consider the structure below for the [EO₂F ] ion. Note: E represents an unidentified element from the fifth period. :0: [A] (a) What is the formal charge on E? Number (b) Which element could E represent? (Enter the correct atomic symbol.)

Based on average bond enthalpies, would you expect a photon capable ofdissociating a C¬Cl bond to have sufficient energy to dissociate a C¬Br bond?

Two possible Lewis structures for the cyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for cyanate? FC: -1 0 0 FC: -1 +1 -1 |:0—C=N:1 STRUCTURE A STRUCTURE B Structure A Structure B Both are equally likely QUESTION 19 Two possible Lewis structures for the thiocyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for thiocyanate? FC: 00-1 FC: -1 +1 -1 Ec: STRUCTURE A STRUCTURE B O Structure A Structure B