(a) Draw the best Lewis structure for the chlorate...

Question

(a) Draw the best Lewis structure for the chlorate ion. Include any resonance structures.(b) What is the average bond order of the chlorine-oxygen bond in the molecule you drew above?

Jules Bruno · Accepted Answer

Determine the resonance structure that will contribute the most for chlorate ion (ClO3-) and the average bond of each O-Cl First, we will have to draw the Lewis Structure of ClO3- and follow the steps:Step 1: Determine the central atom in this molecule.Step 2: Calculate the total number of valence electrons present.  [readmore]Step 3: Draw the Lewis Structure for the molecule        Step 1: Cl (EN = 3.2) is less electronegative than O (EN = 3.5) hence Cl is the central atom.Step 2: Calculate the total number of valence electrons present.          ClO3-:            Group             Valence ElectronsO            6A                   3 × 6 e– = 18 e–Cl           7A                   1 × 7 e– = 7 e–                                               +1 e–Total:  26 valence e–Step 3: Draw the Lewis Structure for the molecule• O → prefers to have complete octet (8 e- around them)• Surround Cl with Os• Distribute extra electrons in each of the O atoms (since they prefer to have complete octet and O is more electronegative than Cl)• O can have up to 2 bondsFirst resonance structure will appear as:To calculate for Formal Charges:Formal charge = Group # - bonds - non bonding e-non-bonding electron = lone pair e-Cl▪ Formal Charge:        F. C. = 7 – (5 + 2)F. C. = 7 – 7F. C. = 0O (single bond) ▪ Formal Charge:        F. C. = 6 – (1 + 6)F. C. = 6 – 7F. C. = -1O (double bond)▪ Formal Charge:        F. C. = 6 – (2 + 4)F. C. = 6 – 6F. C. = 0Overall charge:Overall charge = -1 + 0 + 0Overall charge = -1The second and third resonance structure will appear as O-Cl having alternating bonds. Summarizing, the resonance structures are:To determine the main contributor, we have to find the structure where the negative charge is distributed to the most electronegative atomIn this case, O is the most electronegative atom in the molecule. This means we have to find the structure where O has a negative charge.Hence, any of the structure above will be considered as the major structureAverage bond order can be calculated as:average bond order of O-Cl = 2(# of double bond) + # of single bond3average bond order of O-Cl = 2(2) + 13Average bond order = 1.67Therefore, the average bond order of O-Cl is 1.67

Problem: (a) Draw the best Lewis structure for the chlorate ion. Include any resonance structures.(b) What is the average bond order of the chlorine-oxygen bond in the molecule you drew above?

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Problem: (a) Draw the best Lewis structure for the chlorate ion. Include any resonance structures.(b) What is the average bond order of the chlorine-oxygen bond in the molecule you drew above?

FREE Expert Solution

Problem Details

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