Do electrons go to even lower ground states after exothermic reactions?What is meant by electrons moving to lower potential energy?Why do we use dG < 0 to describe a spontaneous process?Relationship between thermodynamic reversibility and reactionsWhat is the difference between convection and conduction?(Energetics) Potential Energy and Kinetic EnergyEnthalpy of a reaction changes with temperature, does this mean bond strengths change with temperature?What is the mechanism by which reactants in endothermic reactions absorb energy from their environments?Is enthalpy the same thing as potential energy?Why does ATP has a lower entropy than ADPWhy does standard reduction potential get multiplied by the change in oxidation state and not by the number of electrons transferred?What is meant by excess energy in exothermic reaction?
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Do electrons go to even lower ground states after exothermic reactions?
What is meant by electrons moving to lower potential energy?Why do we use dG < 0 to describe a spontaneous process?Relationship between thermodynamic reversibility and reactionsWhat is the difference between convection and conduction?(Energetics) Potential Energy and Kinetic EnergyEnthalpy of a reaction changes with temperature, does this mean bond strengths change with temperature?What is the mechanism by which reactants in endothermic reactions absorb energy from their environments?Is enthalpy the same thing as potential energy?Why does ATP has a lower entropy than ADPWhy does standard reduction potential get multiplied by the change in oxidation state and not by the number of electrons transferred?What is meant by excess energy in exothermic reaction?
$begingroup$
I am a bit confused about what happens to the energy levels during an exothermic reaction.
I understand that during an exothermic reaction, the energy of the electrons decreases.
Is the potential energy of electrons related to the energy level diagram, shown below?
So if the potential energy decreases, does that mean the ground state for the new molecules formed will be different from the old molecules?
thermodynamics
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
add a comment |
$begingroup$
I am a bit confused about what happens to the energy levels during an exothermic reaction.
I understand that during an exothermic reaction, the energy of the electrons decreases.
Is the potential energy of electrons related to the energy level diagram, shown below?
So if the potential energy decreases, does that mean the ground state for the new molecules formed will be different from the old molecules?
thermodynamics
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
$begingroup$
Related: chemistry.stackexchange.com/questions/114347/…
$endgroup$
– Karsten Theis
3 hours ago
add a comment |
$begingroup$
I am a bit confused about what happens to the energy levels during an exothermic reaction.
I understand that during an exothermic reaction, the energy of the electrons decreases.
Is the potential energy of electrons related to the energy level diagram, shown below?
So if the potential energy decreases, does that mean the ground state for the new molecules formed will be different from the old molecules?
thermodynamics
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
I am a bit confused about what happens to the energy levels during an exothermic reaction.
I understand that during an exothermic reaction, the energy of the electrons decreases.
Is the potential energy of electrons related to the energy level diagram, shown below?
So if the potential energy decreases, does that mean the ground state for the new molecules formed will be different from the old molecules?
thermodynamics
thermodynamics
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 6 hours ago
Mason RileyMason Riley
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 6 hours ago
Mason RileyMason Riley
61
asked 6 hours ago
Mason RileyMason Riley
61
61
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
New contributor
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
Mason Riley is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$begingroup$
Related: chemistry.stackexchange.com/questions/114347/…
$endgroup$
– Karsten Theis
3 hours ago
add a comment |
$begingroup$
Related: chemistry.stackexchange.com/questions/114347/…
$endgroup$
– Karsten Theis
3 hours ago
$begingroup$
Related: chemistry.stackexchange.com/questions/114347/…
$endgroup$
– Karsten Theis
3 hours ago
$begingroup$
Related: chemistry.stackexchange.com/questions/114347/…
$endgroup$
– Karsten Theis
3 hours ago
add a comment |
1 Answer
1
active
oldest
votes
$begingroup$
Yes, electron energy levels are like that, especially for single atoms.
Yes, forming molecular bonds creates different electron energy levels, with exothermic reactions leading to chemical bonds with lower ground levels then the reagents had.
Much more info you can get reading about
molecular orbitals
molecular orbitals diagrams
molecular orbital theory
on Wikipedia.
answered 6 hours ago
PoutnikPoutnik
1,599311
$endgroup$
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
add a comment |
Your Answer
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1 Answer
1
active
oldest
votes
1 Answer
1
active
oldest
votes
active
oldest
votes
active
oldest
votes
$begingroup$
Yes, electron energy levels are like that, especially for single atoms.
Yes, forming molecular bonds creates different electron energy levels, with exothermic reactions leading to chemical bonds with lower ground levels then the reagents had.
Much more info you can get reading about
molecular orbitals
molecular orbitals diagrams
molecular orbital theory
on Wikipedia.
answered 6 hours ago
PoutnikPoutnik
1,599311
$endgroup$
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
add a comment |
$begingroup$
Yes, electron energy levels are like that, especially for single atoms.
Yes, forming molecular bonds creates different electron energy levels, with exothermic reactions leading to chemical bonds with lower ground levels then the reagents had.
Much more info you can get reading about
molecular orbitals
molecular orbitals diagrams
molecular orbital theory
on Wikipedia.
answered 6 hours ago
PoutnikPoutnik
1,599311
$endgroup$
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
add a comment |
$begingroup$
Yes, electron energy levels are like that, especially for single atoms.
Yes, forming molecular bonds creates different electron energy levels, with exothermic reactions leading to chemical bonds with lower ground levels then the reagents had.
Much more info you can get reading about
molecular orbitals
molecular orbitals diagrams
molecular orbital theory
on Wikipedia.
answered 6 hours ago
PoutnikPoutnik
1,599311
$endgroup$
Yes, electron energy levels are like that, especially for single atoms.
Yes, forming molecular bonds creates different electron energy levels, with exothermic reactions leading to chemical bonds with lower ground levels then the reagents had.
Much more info you can get reading about
molecular orbitals
molecular orbitals diagrams
molecular orbital theory
on Wikipedia.
answered 6 hours ago
PoutnikPoutnik
1,599311
answered 6 hours ago
PoutnikPoutnik
1,599311
answered 6 hours ago
PoutnikPoutnik
1,599311
answered 6 hours ago
PoutnikPoutnik
1,599311
1,599311
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
add a comment |
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
$begingroup$
So when the exothermic reaction finishes, will the electrons end up at the ground energy level?
$endgroup$
– Mason Riley
3 hours ago
1
1
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
$begingroup$
Usually yes, even if sometimes they can even temporarily stay excited.
$endgroup$
– Poutnik
2 hours ago
add a comment |
Mason Riley is a new contributor. Be nice, and check out our Code of Conduct.
Mason Riley is a new contributor. Be nice, and check out our Code of Conduct.
Mason Riley is a new contributor. Be nice, and check out our Code of Conduct.
Mason Riley is a new contributor. Be nice, and check out our Code of Conduct.
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Related: chemistry.stackexchange.com/questions/114347/…
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– Karsten Theis
3 hours ago