Understanding Polar Molecules: Examples of XY and XY2

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Discussion Overview

The discussion revolves around the characteristics of polar molecules, specifically examining diatomic molecules like XY and triatomic molecules like XY2. Participants explore examples of real molecules, particularly CO2 and H2O, to illustrate the differences in polarity based on molecular geometry and bond characteristics.

Discussion Character

  • Exploratory
  • Conceptual clarification
  • Debate/contested
  • Mathematical reasoning

Main Points Raised

  • One participant asserts that a diatomic molecule XY with a polar bond must be polar, while a triatomic molecule XY2 with a polar bond does not necessarily have to be polar.
  • Several participants suggest CO2 as an example to illustrate the concept of molecular polarity.
  • Another participant expresses confusion about how CO2 demonstrates the characteristics of a polar molecule compared to H2O.
  • Participants discuss the molecular shapes of CO2 and H2O, noting that CO2 is linear while H2O is bent, which may affect their polarity.
  • One participant points out that H2O has polar covalent bonds and is a polar molecule, while CO2's structure leads to a different electron distribution.
  • There is a mention of the importance of locating partial charges in the molecules to understand their polarity.

Areas of Agreement / Disagreement

Participants generally agree on the need for examples to clarify the concept of molecular polarity, but there is no consensus on the implications of molecular geometry and bond characteristics, leading to multiple competing views on the topic.

Contextual Notes

Some participants express uncertainty about the method used to compare the molecular structures and their implications for polarity. There are also unresolved questions regarding the role of electron distribution and molecular shape in determining polarity.

Who May Find This Useful

This discussion may be useful for students or individuals interested in chemistry, particularly those studying molecular polarity and the effects of molecular geometry on chemical properties.

bjoyful
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A diatomic molecule XY that contains a polar bond must be a polar molecule. A triatomic molecule XY2 that contains a polar bond does not necessarily form a polar molecule. I need some examples of real molecules to help me explain the difference.

Thanks
 
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Look at CO2
 
concentration of hydrogen ions

oops...posted wrong message:(
 
Last edited:
so you are saying to look at CO2 as an example?
 
bjoyful said:
so you are saying to look at CO2 as an example?


That's what he/she said.
 
so I guess my question should become a little more specific...can someone tell me how (or give me a website) CO2 demonstates this?!
 
Look at CO2, compare it to H2O.
 
..
CO2 = :O::C::O:
..

H2O = H::O::H

So I compared them this way, but am I using the right method for this problem? I know that H2O is a polar covalent bonds forming a polar covalent molecule. But carbon is my center in CO2, not oxygen as it is in H2O. Help:(

edit: my dots are suppose to be over the carbon to represent non bonded pairs...
 
hint: CO2 is linear and H2O is bent

a molecule is polar when it has a side with a partial negative charge and the opposite side with a partial positive charge.

try to locate these partial charges on the molecules.
 
  • #10
H2O does not have any double bonds, BTW; its electron distribution is why it's a different shape to CO2 (as Kushal pointed out). Only vaguely related to the question, but an important concept.
 

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