Using electrons and/or lone pairs in the following conjugated system, create a resonance form by moving electrons as far as possible. Modify the structure to show the resonance structure resulting from the movement of electrons. Be sure to include all lone pairs of electrons and charges. + + 0: ☑ ☐ :

Use this condensed chemical structure to complete the table below. OH The condensed chemical structure of phenol. Some facts about the phenol molecule: molecular formula: number of major resonance structures: number of carbon-hydrogen single (C-H) bonds: number of oxygen-hydrogen single (O-H) bonds: number of lone pairs: 0 0 0 0 0

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 three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond. b) The rightmost bond (between N and N) is a single bond. c) The formal charge on the leftmost (N) atom is -1. d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4. e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

Draw all reasonable resonance structures for the species shown below. Include arrows to show electron movement. Draw the resonance hybrid structures. ди [m]

Draw the resonance structure indicated by the curved arrows. Assign formal charges. H H/:O: H H-C-C-C-Ċ—H H H H Draw the molecule by placing atoms on the canvas and connecting them with bonds. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms in the correct structure.

Draw the Lewis structures for three resonance forms of the nitrate ion, NO−3. Include electron lone pairs, and any formal charges. Xenon can be the central atom of a molecule by expanding beyond an octet of electrons. Draw Lewis structures for the given xenon compound. Show all lone pairs: XeF2O Please answer both parts.

Draw two resonance structures of the given molecule/ion. Be sure to include all lone pairs. :Ö:

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) - H,O,(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. OH(g) H,O,(g) H H. : 0 H Question Source: MRG - General Chem about us privacy policy terms of use help contact us careers : :