Question

2. Consider the anion [ClO2] - and answer the following questions: a. Draw a reasonable lewis dot structure for [ClO2] - that obeys the octet rule for all atoms. Prove your drawing is reasonable by calculating the formal charges for each atom in the molecule. b. Draw a reasonable lewis dot structure for [ClO2] - that includes an expanded octet. Prove your drawing is reasonable by calculating the formal charges for each atom in the molecule. c. Evaluate the two structures drawn in 1a and 1b, are they resonance structures of one another? i. State your opinion as a claim and support it with evidence and scientific reasoning. ii. If you take the position that they are not resonance structures provide an example of what a resonance structure would be for either the drawing in 1a or 1b

          2. Consider the anion [ClO2] - and answer the following
questions:
a. Draw a reasonable lewis dot structure for [ClO2] - that obeys
the octet rule for all atoms. Prove your drawing is reasonable by
calculating the formal charges for each atom in the molecule.
b. Draw a reasonable lewis dot structure for [ClO2] - that
includes an expanded octet. Prove your drawing is reasonable by
calculating the formal charges for each atom in the molecule.
c. Evaluate the two structures drawn in 1a and 1b, are they
resonance structures of one another?
i. State your opinion as a claim and support it with evidence
and scientific reasoning.
ii. If you take the position that they are not resonance
structures provide an example of what a resonance structure would
be for either the drawing in 1a or 1b

Show more…

Added by Antonio L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Kranti S

01/14/2022

Step 1

- Chlorine will have 3 lone pairs and 1 bond with one of the Oxygen atoms. - Each Oxygen will have 2 lone pairs and 1 bond with Chlorine. - Formal charges: Chlorine = 0, Oxygen = -1 ** Show more…

Show all steps

lock

Thanks for your feedback!

2. Consider the anion [ClO2] - and answer the following questions: a. Draw a reasonable lewis dot structure for [ClO2] - that obeys the octet rule for all atoms. Prove your drawing is reasonable by calculating the formal charges for each atom in the molecule. b. Draw a reasonable lewis dot structure for [ClO2] - that includes an expanded octet. Prove your drawing is reasonable by calculating the formal charges for each atom in the molecule. c. Evaluate the two structures drawn in 1a and 1b, are they resonance structures of one another? i. State your opinion as a claim and support it with evidence and scientific reasoning. ii. If you take the position that they are not resonance structures provide an example of what a resonance structure would be for either the drawing in 1a or 1b

Play audio

Feedback

Powered by NumerAI

Kranti S and 54 other subject Chemistry 101 educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Recommended Videos

Recommended Textbooks

Transcript

00:01 The luce structure when each atom completed octate would be somewhat like this.

00:05 We will have oxygen, then chlorine and oxygen.

00:08 And since octet is complete, so we have 7 valence electrons for oxygen in this fashion.

00:15 It will be having.

00:19 Here there will be two.

00:20 Here there is two.

00:21 So here what will happen is this is going to complete it octate in this manner.

00:27 So chlorine has completed octet and oxygen has also completed the octet.

00:31 So we can say that loose structure with the whole, each atom is completed octet so formal charge formal charge so even this part is there so even this electron is being considered of the oxygen now the octet is complete completely so formal charge calculation we will do in this part chlorine the valence electron minus non -bonding electrons minus half the bonding electrons this is the formula for calculation of formal charge so if in the case of chlorine, the valence electron is 7, non -bonding electrons over here is 4 minus half times the bonding electrons, that is 2, that is going to come out to be equal to 7 minus 5 which is equal to, whereas in the case of oxygen it is going to be valence electrons is 6, number of bonding electrons is 1 and non -bonding electron is 6.

01:33 So 6 minus 6 minus 1 times 1 is equal to minus 1.

01:37 So, this is the formal charges.

01:40 Moving forward to the b part when expanded octet is there.

01:44 Expanded octet.

01:47 So the loose structure will be cl.

01:52 We will have total 8 electrons, then oxygen in this fashion, and here we will have oxygen over here.

02:04 So this is going to form like this...

Ace is your personal tutor. It breaks down any question with clear steps so you can learn.

Start Using Ace

Continue solving this problem

Create a free account to:

View full step-by-step solution
Ask follow-up questions with Ace AI
Save progress and study later