да Using a 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. 2 Π x G さ C
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- 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: ☑ ☐ :None11. Which of the following statements about resonance is true? I. Resonance hybrids occur because a compound changes back and forth between two or more resonance structures. II. Resonance structures differ in the arrangement of electrons but not in the arrangement of atoms. III. Resonance hybrids contain delocalized electrons. IV. Resonance structures for a given compound always contribute equally to the resonance hybrid. V. Resonance structures occur when there are two or more valid Lewis structures for a given compound. VI. Resonance hybrids are a composite of resonance structures. a. I, II, V, VI b. I, II, V, VI c. II, III, IV, VI d. II, III, V, VI e. II, IV, V, VI 12. How many resonance forms will nitrate ion (NO3-) have? a. -1 b. 0 c. 1 d. 2 e. 3 13. A list of non-metals is given below. Which elements cannot exceed the octet rule? B Si N P O S F Cl a. Si, P, S, Cl b. B, N, O, F c. O, S, F, Cl d. B, Si, N, P e. All eight elements can exceed the octet…
- Draw one of the possible resonance structures for the chlorate ion (ClO3−). Be sure to include all lone pair electrons and nonzero formal charges.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 0Use this condensed chemical structure to complete the table below. CH, — С — О — С — CH, The condensed chemical structure of acetic anhydride Some facts about the acetic anhydride molecule: number of carbon-carbon single (C - C) bonds: number of carbon-hydrogen single (C - H) bonds: number of lone pairs:
- Draw an equivalent resonance structure that minimizes charge. Include all lone pairs in your structure. CH2 QDraw 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 three resonance structures for (a) the cyanate ion (NCO−) and (b) the isocyanate ion (CNO−). In each case, rank the resonance structures in order of increasing importance. Be sure to include all lone pair electrons and nonzero formal charges.a) NCO−Consider the resonance structures of formate. Y-Y > H. Select the true statements about the resonance structures. Each carbon-oxygen bond is somewhere between a single and double bond. Each oxygen atom has a double bond 50% of the time. The actual structure of formate is an average of the two resonance forms. The actual structure of formate switches back and forth between the two resonance forms.