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Why is it that for some elements, you say that you need to break the intermolecular forces for it to boil or melt e.g. Chlorine but for others you have to break covalent bonds e.g. carbon. Does carbon not have any intermolecular forces?? or are the intermolecular forces only possible between molecules and a carbon atom isnt a molecule???
Please reply! got a mock tomorrow
Please reply! got a mock tomorrow
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#2
(Original post by fares22)
Why is it that for some elements, you say that you need to break the intermolecular forces for it to boil or melt e.g. Chlorine but for others you have to break covalent bonds e.g. carbon. Does carbon not have any intermolecular forces?? or are the intermolecular forces only possible between molecules and a carbon atom isnt a molecule???
Please reply! got a mock tomorrow
Why is it that for some elements, you say that you need to break the intermolecular forces for it to boil or melt e.g. Chlorine but for others you have to break covalent bonds e.g. carbon. Does carbon not have any intermolecular forces?? or are the intermolecular forces only possible between molecules and a carbon atom isnt a molecule???
Please reply! got a mock tomorrow
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#4
(Original post by fares22)
i understand the difference between inter and intra. i just want to know why you have to break the covalent bonds in carbon for it to boil and not intermolecular forces like Cl2. does carbon not have intermolecular forces?
i understand the difference between inter and intra. i just want to know why you have to break the covalent bonds in carbon for it to boil and not intermolecular forces like Cl2. does carbon not have intermolecular forces?
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(Original post by Spannerin'moi)
When you say carbon, do you mean just as an atom? Or would you mean graphite ?The intermolecular bonds are still present in the case of graphite it holds the layers together but these forces are weak as compared to strong intramolecular giant covalent bonds
When you say carbon, do you mean just as an atom? Or would you mean graphite ?The intermolecular bonds are still present in the case of graphite it holds the layers together but these forces are weak as compared to strong intramolecular giant covalent bonds
are intermolecular forces only possible with atoms that are diatomic??
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#6
(Original post by fares22)
i mean as an atom. carbon on its own is monatomic so this would mean it doesnt have any intermolecular forces. but chlorine is diatomic so it does?
are intermolecular forces only possible with atoms that are diatomic??
i mean as an atom. carbon on its own is monatomic so this would mean it doesnt have any intermolecular forces. but chlorine is diatomic so it does?
are intermolecular forces only possible with atoms that are diatomic??
Van der Waal intermolecular forces do exist between monoatomic substances...noble gases
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(Original post by Spannerin'moi)
http://intro.chem.okstate.edu/AP/Lec83101.html
Van der Waal intermolecular forces do exist between monoatomic substances...noble gases
http://intro.chem.okstate.edu/AP/Lec83101.html
Van der Waal intermolecular forces do exist between monoatomic substances...noble gases
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#8
May I?
When considering melting points why are you considering monatomic carbon? carbon doesn't exist like that other than under extreme lab conditions.
Elemental carbon is macromolecular whether you consider graphire or diamond. A pieve of elemental carbon is effectively a single molecule. So there aren't intramolecular forces to breakdown - all the attraction forces that require breaking down are intramolecular, they are covalent bonds.
Boiling point of carbon is high because you need to melt it first.
(Original post by fares22)
i mean as an atom. carbon on its own is monatomic so this would mean it doesnt have any intermolecular forces. but chlorine is diatomic so it does?
are intermolecular forces only possible with atoms that are diatomic??
i mean as an atom. carbon on its own is monatomic so this would mean it doesnt have any intermolecular forces. but chlorine is diatomic so it does?
are intermolecular forces only possible with atoms that are diatomic??
Elemental carbon is macromolecular whether you consider graphire or diamond. A pieve of elemental carbon is effectively a single molecule. So there aren't intramolecular forces to breakdown - all the attraction forces that require breaking down are intramolecular, they are covalent bonds.
Boiling point of carbon is high because you need to melt it first.
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(Original post by TutorsChemistry)
May I?
When considering melting points why are you considering monatomic carbon? carbon doesn't exist like that other than under extreme lab conditions.
Elemental carbon is macromolecular whether you consider graphire or diamond. A pieve of elemental carbon is effectively a single molecule. So there aren't intramolecular forces to breakdown - all the attraction forces that require breaking down are intramolecular, they are covalent bonds.
Boiling point of carbon is high because you need to melt it first.
May I?
When considering melting points why are you considering monatomic carbon? carbon doesn't exist like that other than under extreme lab conditions.
Elemental carbon is macromolecular whether you consider graphire or diamond. A pieve of elemental carbon is effectively a single molecule. So there aren't intramolecular forces to breakdown - all the attraction forces that require breaking down are intramolecular, they are covalent bonds.
Boiling point of carbon is high because you need to melt it first.
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#10
(Original post by fares22)
so carbon is always in a big structure. okay but how about other elements such as silicon? do they also only exsist as large structures so they dont have any intermolecular forces but covalent bonds
so carbon is always in a big structure. okay but how about other elements such as silicon? do they also only exsist as large structures so they dont have any intermolecular forces but covalent bonds
Learn your common macromolecules, you will need to know these to understand or predict melting point or boling point trends and more
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(Original post by TutorsChemistry)
Yes silicon is also macromolecular.
Learn your common macromolecules, you will need to know these to understand or predict melting point or boling point trends and more
Yes silicon is also macromolecular.
Learn your common macromolecules, you will need to know these to understand or predict melting point or boling point trends and more
Any element which is macromolecular will need covalent bonds to be broken when melted or boiled. this is because one of them is monatomic so there are no intermolecular forces
Thank you for your help!
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#12
(Original post by fares22)
just to make sure please.
Any element which is macromolecular will need covalent bonds to be broken when melted or boiled. this is because one of them is monatomic so there are no intermolecular forces
Thank you for your help!
just to make sure please.
Any element which is macromolecular will need covalent bonds to be broken when melted or boiled. this is because one of them is monatomic so there are no intermolecular forces
Thank you for your help!
There are many elements (metals, Si, C for example) for which we don't have a specific number of atoms in their molecules, but please don't consider them monatomic - they have an unlimited number of atoms in their molecules.
You are correct that macromolecular elements will need many covalent bonds breaking. Not just elements though, macromolecular compounds such as SiO2 also have many covalent bonds to break when you melt them.
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