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Why are reactions exo/endothermic?
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What is the difference between these two reactions (and please don't just say 'one gives out energy' 
) and what causes different reactions to behave in this way?
Edit - I know about bond enthalpies! That isn't my question!
) and what causes different reactions to behave in this way?Edit - I know about bond enthalpies! That isn't my question!
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#2
It basically describes heat change of a reaction under constant pressure.
So if you did an endo, you would feel the test tube getting colder
If you did an Exo, you would feel the test tube getting warmer
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So if you did an endo, you would feel the test tube getting colder
If you did an Exo, you would feel the test tube getting warmer
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(Original post by Tillsy)
It basically describes heat change of a reaction under constant pressure.
So if you did an endo, you would feel the test tube getting colder
If you did an Exo, you would feel the test tube getting warmer
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It basically describes heat change of a reaction under constant pressure.
So if you did an endo, you would feel the test tube getting colder
If you did an Exo, you would feel the test tube getting warmer
Posted from TSR Mobile
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#4
Bond breaking is endothermic which absorbs heat.
Bond formation is exothermic which releases heat.
If more bonds are made than broken, then the reaction is exothermic.
If more bonds are broken than made, then the reaction is endothermic.
Bond formation is exothermic which releases heat.
If more bonds are made than broken, then the reaction is exothermic.
If more bonds are broken than made, then the reaction is endothermic.
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#5
To break a bond energy has to be taken in so the energy of the reaction goes up and the energy (heat) of the surroundings goes down.
To make a bond energy is released making the energy of the reaction go up and the energy (heat) of the surroundings go up.
If more energy is taken in than given out (each bond requires a certain amount of energy to break/make) then the reaction is endothermic and vice versa.
To make a bond energy is released making the energy of the reaction go up and the energy (heat) of the surroundings go up.
If more energy is taken in than given out (each bond requires a certain amount of energy to break/make) then the reaction is endothermic and vice versa.
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#6
It's to do with the bonds being formed and broken in a reaction.
Bond breaking is endothermic
Bond forming is exothermic.
So if more energy is needed to break the bonds than is given out when the bonds are formed, the reaction is endothermic.
If more energy is given out when the new bonds are formed than is taken in to break the bonds, the reaction is exothermic.
Bond breaking is endothermic
Bond forming is exothermic.
So if more energy is needed to break the bonds than is given out when the bonds are formed, the reaction is endothermic.
If more energy is given out when the new bonds are formed than is taken in to break the bonds, the reaction is exothermic.
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(Original post by Petulia)
Bond breaking is endothermic which absorbs heat.
Bond formation is exothermic which releases heat.
Bond breaking is endothermic which absorbs heat.
Bond formation is exothermic which releases heat.
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming releases energy, apart from it being the reverse of bond breaking.
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#8
(Original post by Arithmeticae)
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
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#9
(Original post by Arithmeticae)
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
I don't think you need to know this in detail at AS though.
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#10
(Original post by Arithmeticae)
What is the difference between these two reactions (and please don't just say 'one gives out energy') and what causes different reactions to behave in this way?
What is the difference between these two reactions (and please don't just say 'one gives out energy'
) and what causes different reactions to behave in this way?
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#11
(Original post by Arithmeticae)
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
Why does bond formation release energy though?
Intuitively I've understood that bond breaking requires energy (because you need to split up the bonds), but never actually understood why bond forming requires energy, apart from it being the reverse of bond breaking.
So everything and has energy within it and when the bonds are MADE*, obviously it will be released and converted into other types of energy. It's pretty straightforward to be honest... I think you're looking into it too much and confusing yourself.
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#12
It's just common sense, some chemical reactions need more energy to break the bonds of the reactants, than the energy that is released when the bonds of the products are formed.
On the other hand, some chemical reactions don't require AS MUCH energy to break the bonds of the reactants, and more energy is released when the bonds creating the products are formed.
For instance if the bonds in the reactants of a chemical reaction are particularly strong, you'll need a lot of heat energy to break them, and when the bonds of the products are formed heat energy will be released but it won't be as much as the energy you had to provide for the breaking to happen.
And vice versa
On the other hand, some chemical reactions don't require AS MUCH energy to break the bonds of the reactants, and more energy is released when the bonds creating the products are formed.
For instance if the bonds in the reactants of a chemical reaction are particularly strong, you'll need a lot of heat energy to break them, and when the bonds of the products are formed heat energy will be released but it won't be as much as the energy you had to provide for the breaking to happen.
And vice versa
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(Original post by easyastau)
It's pretty logical if you think about it. You have to put in work or energy to make anything
It's pretty logical if you think about it. You have to put in work or energy to make anything
(Original post by Petulia)
Bond breaking takes in energy because energy is required to break the bonds. Bond making releases energy because the atoms are stable when in a bond.
I don't think you need to know this in detail at AS though.
Bond breaking takes in energy because energy is required to break the bonds. Bond making releases energy because the atoms are stable when in a bond.
I don't think you need to know this in detail at AS though.
(Original post by GCSEsitter)
The chemical explanation at igcse level is that making bonds is an ectothermic process, releasing heat energy and breaking bonds is an endothermic process, which requires energy. The amount of energy used to break bonds(-) and the amount of energy released to make them(+) is added(remembering that one is negative the other is positive). This give enthalpy change, if this value is negative then it's exothermic, if it's positive then it's endothermic.
The chemical explanation at igcse level is that making bonds is an ectothermic process, releasing heat energy and breaking bonds is an endothermic process, which requires energy. The amount of energy used to break bonds(-) and the amount of energy released to make them(+) is added(remembering that one is negative the other is positive). This give enthalpy change, if this value is negative then it's exothermic, if it's positive then it's endothermic.
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(Original post by saad97)
ENERGY IS NEVER CREATED NOR DESTROYED!
So everything and has energy within it and when the bonds are broken, obviously it will be released and converted into other types of energy. It's pretty straightforward to be honest... I think you're looking into it too much and confusing yourself.
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ENERGY IS NEVER CREATED NOR DESTROYED!
So everything and has energy within it and when the bonds are broken, obviously it will be released and converted into other types of energy. It's pretty straightforward to be honest... I think you're looking into it too much and confusing yourself.
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Bond breaking takes energy, it doesn't release it... :/
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#15
(Original post by saad97)
ENERGY IS NEVER CREATED NOR DESTROYED!
So everything and has energy within it and when the bonds are broken, obviously it will be released and converted into other types of energy. It's pretty straightforward to be honest... I think you're looking into it too much and confusing yourself.
Posted from TSR Mobile
ENERGY IS NEVER CREATED NOR DESTROYED!
So everything and has energy within it and when the bonds are broken, obviously it will be released and converted into other types of energy. It's pretty straightforward to be honest... I think you're looking into it too much and confusing yourself.
Posted from TSR Mobile
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#16
(Original post by Arithmeticae)
I said released and required, nothing in that post suggests that energy is created or destroyed.
Bond breaking takes energy, it doesn't release it... :/
I said released and required, nothing in that post suggests that energy is created or destroyed.
Bond breaking takes energy, it doesn't release it... :/
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#17
Imagine having two balls with opposite charges, kept at some distance. They attract each other, which means they have some potential energy. You allow them to get closer to each other - their potential energy gets lower. What happened to the rest of the energy? It was released - and one of the easiest ways of releasing energy is giving heat.
It is very similar for atoms, even if they are not necessarily initially charged. That's because the charges (electrons) are shifted to different positions and the net effect is very similar.
It is very similar for atoms, even if they are not necessarily initially charged. That's because the charges (electrons) are shifted to different positions and the net effect is very similar.
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#18
(Original post by Arithmeticae)
So the atoms change from a less stable state to a more stable state, because the electrons from the outer orbitals have a lower energy sum than the electrons of the atoms that form the bond?
So the atoms change from a less stable state to a more stable state, because the electrons from the outer orbitals have a lower energy sum than the electrons of the atoms that form the bond?
Exothermic = MORE energy given OUT forming bonds, than energy given IN while breaking bonds. Temperature increases.
Endothermic = MORE energy given IN to break bonds, than energy given OUT while forming bonds. Temperature decreases.
That's it. That's all you have to know. Now MOVE ON! This is only 0.00000001% of Unit 2
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(Original post by Borek)
Imagine having two balls with opposite charges, kept at some distance. They attract each other, which means they have some potential energy. You allow them to get closer to each other - their potential energy gets lower. What happened to the rest of the energy? It was released - and one of the easiest ways of releasing energy is giving heat.
It is very similar for atoms, even if they are not necessarily initially charged. That's because the charges (electrons) are shifted to different positions and the net effect is very similar.
Imagine having two balls with opposite charges, kept at some distance. They attract each other, which means they have some potential energy. You allow them to get closer to each other - their potential energy gets lower. What happened to the rest of the energy? It was released - and one of the easiest ways of releasing energy is giving heat.
It is very similar for atoms, even if they are not necessarily initially charged. That's because the charges (electrons) are shifted to different positions and the net effect is very similar.
So it's due to the Coulomb force between charged particles (and the polarization of the charges which still results in a force being created between the two)?
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(Original post by BarBaBaBaBarBaBaBa)
That's it. That's all you have to know. Now MOVE ON! This is only 0.00000001% of Unit 2
That's it. That's all you have to know. Now MOVE ON! This is only 0.00000001% of Unit 2
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