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(a) Determine the formal charge on the chlorine atom in the hypochlorite ion, ClO-, and the perchlorate ion, ClO4-, using resonance structures where the Cl atom has an octet. (b) What are the oxidation numbers of chlorine in ClO- and in ClO4-? (c) Perchlorate is a much stronger oxidizing agent than hypochlorite. Suggest an explanation.

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Hubert Koch
Hubert KochLv2
26 May 2020

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Related questions

Oxidation Numbers

The oxidation number of an element is the "charge" the element would have if all of its bonds were completely ionic; that is, if the electron pairs of each bond were transferred to the more electronegative atom.

For monatomic ions the oxidation number is simply the charge of the ion. For covalently bonded elements the oxidation number is a bookkeeping device and does not mean that the element carries an actual charge.

Determine the oxidation state for each of the elements below.

The oxidation state of chlorine in hypochlorite ion ClO- is______
The oxidation state of chlorine in chlorine pentafluoride ClF5 is_____
The oxidation state of sulfur in sulfur dioxide SO2 is_______

1) Which compound or ion below MUST expand the octet on thecentral atom. Select all that apply.

Select one or more:

A. carbon dioxide

B. sulfur dioxide

C. xenon difluoride

D. sulfur tetrafluoride

E. perchlorate

2) Draw the Lewis structure for SO2. How manyresonance structures have a zero formal charge on all atoms?

3)Draw the Lewis structure for carbonate such that all atomshave an octet. How many resonance structures does it have?

Select one:

A. 0

B. 1

C. 2

D. 3

E. 4

4)Which compounds or ions below MUST have an atom with fewerthan an octet? Check all that apply.

Select one or more:

A. NO

B. ammonium ion

C. chlorine dioxide

D. HBrO

E. HCCH

5. Draw the lewis structure of ammonium ion. What is the formalcharge on the N?

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