Complete the Lewis structures for COCI2 and SOCI, using the skeletal structure shown below, being sure to follow the procedure for minimizing the sum of the absolute values for the formal charges, where the octet rule need not be followed. Based on the complete structures, which statement below is true? a-c-a CI-S - CI Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. O The SOCI2 exhibits both formal charges and resonance hybrids, while the COCI2 exhibits resonance hybrids but no formal charges. O The SOCI2 exhibits formal charges but no resonance hybrids, while the COCI2 exhibits resonance hybrids but no formal charges. O The COCI2 exhibits formal charges but no resonance hybrids, while the SOCI2 exhibits both formal charges and resonance hybrids. O The formal charges on all the atoms are zero, and the molecules have no resonance hybrids. O The COCI2 exhibits both residual formal charges and resonance hybrids, while the SOCI2 exhibits formal charges but no resonance hybrid

Complete the Lewis structures for COCI2 and SOCI, using the skeletal structure shown below, being sure to follow the procedure for minimizing the sum of the absolute values for the formal charges, where the octet rule need not be followed. Based on the complete structures, which statement below is true? a-c-a CI-S - CI Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. O The SOCI2 exhibits both formal charges and resonance hybrids, while the COCI2 exhibits resonance hybrids but no formal charges. O The SOCI2 exhibits formal charges but no resonance hybrids, while the COCI2 exhibits resonance hybrids but no formal charges. O The COCI2 exhibits formal charges but no resonance hybrids, while the SOCI2 exhibits both formal charges and resonance hybrids. O The formal charges on all the atoms are zero, and the molecules have no resonance hybrids. O The COCI2 exhibits both residual formal charges and resonance hybrids, while the SOCI2 exhibits formal charges but no resonance hybrid

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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O Unit 3d - Polarity O Unit 3c - Molecular Geometry O Unit 3b - Lewis Structures O Unit 3a - Molecules s3.net/mod/quiz/attempt.php?attempt=31808328&cmid3D26593598&page=7 The following two Lewis structures may be drawn for a certain ion with a charge of -1. First, show the formal charge on each atom of each ion, then choose which structure is preferred. :C=N=ö: The formal charge on C is 2 + The formal charge on N is +1 + The formal charge on O is o + . EN-C=0: The formal charge on N is -2 : The formal charge on C is 0 : The formal charge on O is +1 : The preferred structure is the bottom + one.
a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of Cl04~. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of ClO3-. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:
Draw out the Lewis structures for H₂CO3, HCO3, and CO32-. Then determine the maximum number of equivalent resonance structures for each species. Note that carbon is the central atom in all three cases. If the molecule contains hydrogen atoms they are attached to oxygen atoms. Only count the best structures. For example, A structure with really bad formal charges should not be counted. The molecule H₂CO3 has The molecule HCO3 has The molecule CO3²- has equivalent Lewis structures. equivalent Lewis structures. equivalent Lewis structures.
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure -C=C:] H-C : 0: 0=0=0 [HO] : O OO Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* П Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,0".
The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. We can draw three inequivalent Lewis structures for the sulfite ion, SO3²-. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge S 01 Use the References to access important values if needed for this question. 02 03 S KNENEN :0: B A I 2- 2. The best Lewis structure for SO3²- is A :0: C Previous Next
Draw Lewis structure(s) for the acetate ion (CH2CO0). If there are equivalent resonance structures, draw all of them. • Draw one structure per sketcher box, and separate added sketcher boxes with the Do not include overall ion charges or formal charges in your drawing. • Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. symbol. CH3COO":
Pass a piece of paper around the group and ask each group member in turn to perform the next step in the process of determining a correct Lewis structure (including formal charges on all atoms and resonance structures, if appropriate) for the following molecules and ions: N2H4, CCl4, CO3 2-, and NH4 +.
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
An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of +1. Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges.
Part A The Lewis structure for the chlorate ion is Calculate the formal charge on the chlorine (CI) 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 e in the following Lewis structure. :O: Express your answers as integers separated by commas. View Available Hint(s) formal charge on 0,, O, O, = Submit
Draw resonance structures for thiazyl fluoride, F3NS. For the most stable resonance structure, what bond orders are present: For the most stable resonance structure, what formal charges are present: What is the number of electron groups present? What is the molecular shape (geometry): Draw the structure, showing and explaining any deviations from a perfect geometry.
Complete the Lewis structures for COCl₂ and SOCI₂ using the skeletal structure shown below, being sure to follow the procedure for minimizing the sum of the absolute values for the formal charges, where the octet rule need not be followed. Based on the complete structures, which statement below is true? [a_i_d] Cl—N—C Cl-Br Cl Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. O The NOCI₂ exhibits both residual formal charges and resonance hybrids, while the BrOCI₂+ exhibits formal charges but no resonance hybrids. O No answer text provided. The NOC₂ exhibits both formal charges and resonance hybrids, while the BrOCl₂ exhibits resonance hybrids but no formal charges. O At least one atom in each molecule exhibits formal charges, and the molecules have no resonance hybrids. O The BroCl₂ exhibits both formal charges and resonance hybrids, while the POCI₂ exhibits resonance hybrids but no formal charges. O The NOCI₂ exhibits…