Polarity in water molecule and electronegativity of oxygen in that molecule.

Click For Summary

Discussion Overview

The discussion centers on the polarity of water molecules (H2O) and the role of electronegativity of oxygen in this context. Participants explore the implications of atomic structure, electron sharing, and bond characteristics, delving into both theoretical and conceptual aspects.

Discussion Character

  • Exploratory
  • Technical explanation
  • Conceptual clarification

Main Points Raised

  • One participant states that H2O is polar due to oxygen's higher electronegativity compared to hydrogen, leading to shared electrons being closer to oxygen.
  • Another participant notes that oxygen has more protons, which contributes to its greater affinity for electrons than hydrogen.
  • A different viewpoint introduces the concept of ionization energies, suggesting that smaller atoms have electrons that are closer to the nucleus, requiring more energy to separate them.
  • One participant mentions the bond length and angle in water, indicating that the proximity of oxygen to hydrogen affects the molecular structure.
  • Another participant questions why oxygen's electrons are closer to the nucleus, seeking clarification on this point.
  • A participant explains that an atom's size is largely determined by its electron cloud, with more protons leading to a greater pull on electrons, thus affecting atomic size.
  • There is a repeated inquiry about the concept of "closeness" in relation to atomic structure.

Areas of Agreement / Disagreement

Participants express various viewpoints regarding the factors contributing to the polarity of water and the behavior of electrons in relation to protons. The discussion includes multiple competing explanations and remains unresolved on certain points, particularly regarding the nature of atomic size and electron proximity.

Contextual Notes

Some participants express confusion over the relationship between atomic structure and electron behavior, indicating potential gaps in understanding the underlying principles of electronegativity and atomic size.

AakashPandita
Messages
157
Reaction score
0
H20 is polar in nature.
It is fundamentally because oxygen is more electronegative than hydrogen and the shared electrons tend to be near oxygen.
This may be because the atomic number of oxygen is more than that of hydrogen.
But in the bond I don't understand how the 2 shared electrons experience more force from the oxygen side than they do from the hydrogen side.
As the 2 electrons are experiencing the force of 2 protons from both the sides.
Are you getting it, what I am trying to convey?
 
Chemistry news on Phys.org
AakashPandita said:
As the 2 electrons are experiencing the force of 2 protons from both the sides.

Oxygen has more than 1 proton. Because of this, the nucleus of oxygen has a greater affinity for electrons than hydrogen.
 
It is to do with ionization energies. When you go from left to right (and up) you encounter smaller atoms. Which means that the proximity of their electrons is a lot closer than a larger atom. Due to the fact that the Oxygen electrons are a lot closer to the nucleus of the atom a higher amount of energy is required to pull them apart. :) Hope this helped
 
Also, as Matt states, the oxygen is closer to each hydrogen atom than each hydrogen atom is to each other. Each OH bond in H2O is ≈95.84 pm. The bond angle is 104.45°, making the hydrogen atoms 177.38 pm apart.
 
MattA147 said:
Due to the fact that the Oxygen electrons are a lot closer to the nucleus of the atom
Why? This I am not able to understand.
 
Well, most of an atom's size is taken up by it's electron cloud. Having more protons means wanting more electrons. Oxygen's atomic number is 8, so it has 8 protons and 8 electrons in ground state. Hydrogen only has 1 proton, so it only has 1 electron. And more electrons means a larger atom.
 
why closer?
 
In short, so it doesn't get too confusing:

500px-Electron_shell_001_Hydrogen.svg.png
500px-Electron_shell_008_Oxygen.svg.png
 

Similar threads

Why are metals in aqueous solution basic, and non-metals acidic?
  • · Replies 1 ·
Replies
1
Views
3K
Group I/II Metal oxides always basic in aqueous solution -- why?
  • · Replies 3 ·
Replies
3
Views
2K
Non polar molecule with polar bonds?
  • · Replies 34 ·
2
Replies
34
Views
5K
Gamma Radiation and Electrolysis
  • · Replies 6 ·
Replies
6
Views
639
Negative Charge Stability: Oxygen vs. Carbon/Nitrogen
  • · Replies 7 ·
Replies
7
Views
4K
Q: What is the role of antibonding orbitals in CO bonding with metals?
  • · Replies 1 ·
Replies
1
Views
2K
Oxygen dip in ionization energy trend
  • · Replies 1 ·
Replies
1
Views
2K
Can elements replace Hydrogen in polar molecules & act similarly?
  • · Replies 1 ·
Replies
1
Views
3K
Why does an alkoxide steal H from water?
  • · Replies 11 ·
Replies
11
Views
4K
Why Do Water Molecules Attract Each Other Despite Complete Electron Shells?
  • · Replies 5 ·
Replies
5
Views
2K