Anamalous behaviour of water

  • Thread starter djsourabh
  • Start date
  • #1
69
0

Main Question or Discussion Point

What is the exact scientific reason behind anamalous behavour of water?
Can the temperature range at which this happens be changed?
do any other substances also behave anamalously?
 

Answers and Replies

  • #2
662
307
mmm....what's anomalous?
 
  • #3
SteamKing
Staff Emeritus
Science Advisor
Homework Helper
12,798
1,666
No, no, the OP clearly said anamalous, whatever that is.
 
  • #4
2,463
97
He did say anamalous but that was probably just a typing error. He meant to write anomalous.
 
  • #5
Borek
Mentor
28,402
2,801
He wrote anamalous three times, it is not a typo.

To OP: please elaborate. In most cases water behaves as every other liquid. Sometimes it doesn't, but you need to explain what you mean if you want to get any help.

Besides, it looks like a HW question to me...
 
  • #6
69
0
Sorry for typing mistake.
I meant ' anomalous' only.
It's not a HW question.
 
  • #7
662
307
So what are you talking about Sourabh?
Large specific heat, expansion while freezing, inertness, or something else?
 
  • #8
69
0
The weird behaviour at 4 C to 0 C .
 
  • #9
662
307
Well, water is composed of three atoms two hydrogen and one oxygen. So a molecule looks likes this:
attachment.php?attachmentid=61616&stc=1&d=1378700879.gif

-When the temperature decreases the molecules start slowing down.
-This causes the volume to decrease and density to increase until 4°C while its still in liquid state.
-After this the molecules start crystallizing in a cage like structure by hydrogen bonding. Hydrogen bonding is a weak molecular interaction between the oxygen of one molecule and Hydrogen of another.
-In the crystallization process the density decreases and volume increases as the H-bonds push molecules apart to maintain a stable crystal lattice.
-The differences can be seen in this image [left is liquid and right is ice]:
320px-Liquid-water-and-ice.png

The temperature and pressure relationship of water is given by:
attachment.php?attachmentid=61615&stc=1&d=1378699692.gif
 

Attachments

  • #10
1,254
106
Bonds, bonds - Hydrogen bonds!
 
  • #11
Drakkith
Staff Emeritus
Science Advisor
20,799
4,537
Bonds, bonds - Hydrogen bonds!
Bond... hydrogen bond.
Shaken, not stirred.
 
  • #12
662
307
Bond... hydrogen bond.
Shaken, not stirred.
Nooo, supercool it and then shake it! The drink shall turn to Ice cream...
https://www.youtube.com/watch?v=DpiUZI_3o8s

The actual drink is a Vesper martini, it went like this:
"A dry martini," Bond said. "One. In a deep champagne goblet."
"Oui, monsieur."
"Just a moment. Three measures of Gordon's, one of vodka, half a measure of Kina Lillet. Shake it very well until it's ice-cold, then add a large thin slice of lemon peel. Got it?"
 
  • #13
69
0
Well, water is composed of three atoms two hydrogen and one oxygen. So a molecule looks likes this:
attachment.php?attachmentid=61616&stc=1&d=1378700879.gif

-When the temperature decreases the molecules start slowing down.
-This causes the volume to decrease and density to increase until 4°C while its still in liquid state.
-After this the molecules start crystallizing in a cage like structure by hydrogen bonding. Hydrogen bonding is a weak molecular interaction between the oxygen of one molecule and Hydrogen of another.
-In the crystallization process the density decreases and volume increases as the H-bonds push molecules apart to maintain a stable crystal lattice.
-The differences can be seen in this image [left is liquid and right is ice]:
320px-Liquid-water-and-ice.png

The temperature and pressure relationship of water is given by:
attachment.php?attachmentid=61615&stc=1&d=1378699692.gif
Thank you for such agood description.
My next query is "can the temperature range at which this phenomena occurs be changed by any means?"
 

Related Threads on Anamalous behaviour of water

  • Last Post
Replies
3
Views
25K
  • Last Post
Replies
6
Views
778
  • Last Post
Replies
1
Views
1K
  • Last Post
Replies
11
Views
2K
  • Last Post
Replies
0
Views
1K
  • Last Post
Replies
0
Views
2K
Replies
1
Views
1K
  • Last Post
Replies
2
Views
1K
Replies
5
Views
2K
  • Last Post
Replies
5
Views
1K
Top