Why Copper is a Better Heat Conductor than Iron

In summary: I've no idea :redface: …Metallic bonds are real s,p,d,f, and k,l,m,n. Covalent and electrovalent bonds are not real, they are just terms that we use to describe how two atoms interact.
  • #1
sankalpmittal
785
15
Hii , i am new in this forum . I am in class 10th and my name is Sankalp . I have a question :

Can you tell me why copper is better conductor of heat than iron ??
 
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  • #2
Welcome to PF!

Hi Sankalp! Welcome to PF! :smile:

In an insulator, there are no free electrons, and heat is conducted only by transfer of vibrations from one molecule to another.

In a conductor, these molecular vibrations also occur, but there is a far greater effect, of heat being conducted by movement of the electrons throughout the material (the "electron fluid").

For the same reason, the materials which are good conductors of heat are also good conductors of electricity … for example, silver is slightly better than copper at both :approve:, and iron is a lot worse. :redface:

See http://en.wikipedia.org/wiki/Conduction_(heat)#Overview" :wink:
 
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  • #3
I know this . The theory of electron fluid !
But if iron forms ions more readily than copper then iron must be better conductor of heat but its not so .

Whyy ?
 
  • #4
The heat conduction in solids may be due to both lattice (ions) vibrations and electron conduction.
So in general is not a simple matter to say which material is a better thermal conductor.
For metals both electric and thermal conduction is strongly related to the free electrons and less to ions.
 
  • #5
nasu said:
The heat conduction in solids may be due to both lattice (ions) vibrations and electron conduction.
So in general is not a simple matter to say which material is a better thermal conductor.
For metals both electric and thermal conduction is strongly related to the free electrons and less to ions.

Then what is it special in copper to make it better conductor than iron ?

Please do add me too .
 
  • #6
conductivity (both thermal and electrical) in metals depends on its resistance, and resistance comes mostly from the rigidity of the molecular structure (if molecules won't get out of the way of electrons, they slow down, so hard metals have higher resistance than soft metals) … see http://en.wikipedia.org/wiki/Copper#Physical" :wink:
This is because the resistivity to electron transport in metals at room temperature mostly originates from scattering of electrons on thermal vibrations of the lattice, which are relatively weak for a soft metal.​

the softness is caused by the weakness of the metallic bonds … in copper (and silver and gold), they are not covalent (because those elements have a complete d-shell and only one s-electron on top, see image at http://en.wikipedia.org/wiki/File:Electron_shell_029_Copper.svg" [Broken]) …
Contrary to metals with incomplete d-shells, metallic bonds in copper are lacking a covalent character and are relatively weak. This explains the low hardness and high ductility of single crystals of copper.

Copper, silver and gold are in group 11 of the periodic table, and they share certain attributes: they have one s-orbital electron on top of a filled d-electron shell and are characterized by high ductility and electrical conductivity. The filled d-shells in these elements do not contribute much to the interatomic interactions, which are dominated by the s-electrons through metallic bonds.​
 
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  • #7
tiny-tim said:
conductivity (both thermal and electrical) in metals depends on its resistance, and resistance comes mostly from the rigidity of the molecular structure (if molecules won't get out of the way of electrons, they slow down, so hard metals have higher resistance than soft metals) … see http://en.wikipedia.org/wiki/Copper#Physical" :wink:
This is because the resistivity to electron transport in metals at room temperature mostly originates from scattering of electrons on thermal vibrations of the lattice, which are relatively weak for a soft metal.​

the softness is caused by the weakness of the metallic bonds … in copper (and silver and gold), they are not covalent (because those elements have a complete d-shell and only one s-electron on top, see image at http://en.wikipedia.org/wiki/File:Electron_shell_029_Copper.svg" [Broken]) …
Contrary to metals with incomplete d-shells, metallic bonds in copper are lacking a covalent character and are relatively weak. This explains the low hardness and high ductility of single crystals of copper.

Copper, silver and gold are in group 11 of the periodic table, and they share certain attributes: they have one s-orbital electron on top of a filled d-electron shell and are characterized by high ductility and electrical conductivity. The filled d-shells in these elements do not contribute much to the interatomic interactions, which are dominated by the s-electrons through metallic bonds.​

ummm What are metallic bonds and how they differ from covalent or electrovalent bond ??

Which are real s,p,d,f or k,l,m,n ?
 
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  • #8
sankalpmittal said:
ummm What are metallic bonds and how they differ from covalent or electrovalent bond ??

oooh, that's chemistry, I've no idea :redface:

you'll have to look it up! :smile:
Which are real s,p,d,f or k,l,m,n ?

what's k,l,m,n ? :confused:
 
  • #9
tiny-tim said:
oooh, that's chemistry, I've no idea :redface:

you'll have to look it up! :smile:
what's k,l,m,n ? :confused:
You mentioned metallic bonds in thermal conductivity :confused:
Hey tim , you must have studied the 2n^2 rule by neils bohr .

1st shell : K
2nd shell : M
and so on .I don't have any idea of s,p,d,f .

Do you know any site which can teach chemistry from sheer basics to advanced level ?

:smile:
 
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  • #10
ratnesh dubey said:
we gave more energy to any object then it is heated

yes , you're right .
 
  • #11
sankalpmittal said:
Hey tim , you must have studied the 2n^2 rule by neils bohr .

1st shell : K
2nd shell : M
and so on .

I don't have any idea of s,p,d,f .

ahh, you seem to be using the special X-ray spectroscopy notation …

for everything else, we use s p d and f

K L M and N refer to the number of shells (the l quantum number)

s p d and f correspond to the subscripts 1 2 3 and 4 (the n quantum number), eg L1 L2 L3

see http://en.wikipedia.org/wiki/X-ray_notation" [Broken] for the conversion table

(now, why couldn't you have found that? :wink:)​

for a full explanation of s p d f, see http://en.wikipedia.org/wiki/Electron_configuration#Notation"
Do you know any site which can teach chemistry from sheer basics to advanced level ?

:smile:

see this forum's "Math & Science Learning Materials" at https://www.physicsforums.com/forumdisplay.php?f=151" :smile:
 
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  • #12
tiny-tim said:
ahh, you seem to be using the special X-ray spectroscopy notation …

for everything else, we use s p d and f

K L M and N refer to the number of shells (the l quantum number)

s p d and f correspond to the subscripts 1 2 3 and 4 (the n quantum number), eg L1 L2 L3

see http://en.wikipedia.org/wiki/X-ray_notation" [Broken] for the conversion table

(now, why couldn't you have found that? :wink:)​

for a full explanation of s p d f, see http://en.wikipedia.org/wiki/Electron_configuration#Notation"


see this forum's "Math & Science Learning Materials" at https://www.physicsforums.com/forumdisplay.php?f=151" :smile:




Are you from UK ??

In India we study the system like this :

The 2n^2 rule :

For eg . There is 1st shell then no. of electrons would be given by 2n^2 :

1. 2x1^2=2 electrons in K shell :
2. 2x2^2=8 electrons in L shell and so on .

Foe eg atomic number of hydrogen is 1 ie 1
and of magnesium is 12 : ie : 2,8,2 .
 
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1. Why is copper a better heat conductor than iron?

Copper is a better heat conductor than iron because of its molecular structure. Copper atoms are arranged in a way that allows for more efficient transfer of heat energy compared to iron atoms. This is due to the presence of more free electrons in copper, which can easily move and transfer heat energy.

2. How does the atomic structure of copper contribute to its superior heat conductivity?

The atomic structure of copper is characterized by its loosely bound electrons in the outermost energy level. These electrons are able to move freely and transfer heat energy through the material. In comparison, iron has a more tightly packed atomic structure which limits the movement of electrons and thus, reduces its heat conductivity.

3. Is copper a better heat conductor at all temperatures?

While copper is generally considered a better heat conductor than iron, its conductivity can decrease at higher temperatures. This is because as the temperature increases, the copper atoms start to vibrate more vigorously, hindering the movement of electrons and reducing its conductivity. However, even at high temperatures, copper still maintains a higher heat conductivity compared to iron.

4. Can the thickness of copper affect its heat conductivity?

Yes, the thickness of copper can have an impact on its heat conductivity. Thicker copper has more atoms and electrons available for heat transfer, making it more efficient at conducting heat. However, the difference in heat conductivity between thin and thick copper is not significant, as the molecular structure of copper is the main factor that determines its heat conductivity.

5. Are there any other factors besides molecular structure that contribute to copper's superior heat conductivity?

Yes, other factors such as purity, density, and surface finish can also affect the heat conductivity of copper. Pure copper has a higher heat conductivity compared to copper alloys, as impurities can disrupt the movement of electrons. A higher density of copper also allows for more atoms and electrons to be present, increasing its heat conductivity. Additionally, a smooth surface finish can minimize resistance and facilitate the transfer of heat energy through copper.

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