Which of the following substances exist(s) as a resonance hybrid?
CO2 (g)
SO3 (g)
HCO2- (aq)
A. I only
B. II only
C. III only
D. I and II only
E. II and III only
Ans w/i 12 hrs please!!
Sorry.
Well, I know that CO2 has resonance forms, but SO3 and HCO2 have resonance forms too. So that's why I don't get which one is the answer because all of them have resonance forms. I guess I just don't understand the "hybrid" part of the question, which would point to a right answer.
But I thought that CO2 could be like O=C=O, O-C=-O, and O=-C-O. Thank you though, for your input. :) I'm sorry about just posting the questions again.
To determine which of the given substances exist as a resonance hybrid, we need to understand what a resonance hybrid is.
Resonance occurs when there are multiple ways to arrange the electrons in a molecule. In a resonance hybrid, the molecule is represented as a combination of different resonance structures. These resonance structures have the same arrangement of atoms but differ in the way the electrons are distributed.
Now, let's analyze each of the given substances:
I. CO2 (g): In carbon dioxide (CO2), the carbon atom forms a double bond with each oxygen atom. The double bonds can be represented in two equivalent ways, with one carbon-oxygen double bond on each side. Therefore, CO2 exhibits resonance, and it exists as a resonance hybrid.
II. SO3 (g): Sulfur trioxide (SO3) also exhibits resonance. The sulfur atom forms a double bond with one oxygen atom and a single bond with the other two oxygen atoms. However, the double bond can be rotated, resulting in all three oxygen atoms being equivalent. This allows the molecule to exist as a resonance hybrid.
III. HCO2- (aq): Formate ion (HCO2-) contains a carbon atom, two oxygen atoms, and a hydrogen atom, with a negative charge on the entire ion. The structure can be represented with a double bond between the carbon and one oxygen atom, and a single bond between the carbon and the other oxygen atom. However, the negative charge can be localized on both oxygen atoms, resulting in resonance. Therefore, HCO2- exists as a resonance hybrid.
Based on the analysis above, both CO2 (g) and SO3 (g) are resonance hybrids. Option D, "I and II only," is the correct answer.
Remember, to determine whether a molecule or ion exists as a resonance hybrid, you need to analyze the Lewis structure and see if there are multiple ways to arrange the electrons, resulting in different resonance structures.
I have answered two of these ASAP questions in which you want answers w/i a specified time; however, my answers have been complete w/o any work from you. You need to know that we try to HELP do homework; therefore, you should make an attempt at these questions, tell us what you think or why you are stumped. With this particular question, please post your thought as to the correct answer and why you think that. Someone will get back to you.
I think your problem may be that you didn't draw the Lewis structures. I found a CO2 structure and a SO3 one. For HCO2^- I looked up HCOOH. For that, just look at the Lewis structure and remove the H of the COOH group and you will have the HCOO^0 ion.
lewis structure CO2
lewis structure SO3
lewis structure HCOOH
The CO2 one is the one that has no resonance hybrids; i.e., that's about the only way you can draw CO2. However, for SO3 the double bond can move to ANY of the S-O bonds and for HCOOH the double bond can move to either of the C-O bonds. Therefore, SO3 and HCOO^- have more than one way of drawing them; hence, they have resonance forms.