Elements other than carbon that can form many different compounds by bonding to themselves?












11












$begingroup$


My textbook says the following:




Unique among the elements, carbon can bond to itself to form extremely strong two-dimensional sheets, as it does in graphite, as well as buckyballs and nanotubes.




Is carbon the only element that can do this?



If not, then what are the other elements can also do this? Is there a term to describe such elements?



What is the chemical characteristic that allows this to occur?



I would greatly appreciate it if people could please take the time to clarify this.






bond elements







share|improve this question











$endgroup$








  • 2




    $begingroup$
    Catenation : self linking property of an element (atom).
    $endgroup$
    – glucose
    18 hours ago






  • 9




    $begingroup$
    The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
    $endgroup$
    – matt_black
    16 hours ago






  • 1




    $begingroup$
    I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
    $endgroup$
    – jeffB
    14 hours ago








  • 1




    $begingroup$
    Sulfur can also form rings and chains
    $endgroup$
    – porphyrin
    13 hours ago






  • 1




    $begingroup$
    What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
    $endgroup$
    – Mithoron
    8 hours ago


















11












$begingroup$


My textbook says the following:




Unique among the elements, carbon can bond to itself to form extremely strong two-dimensional sheets, as it does in graphite, as well as buckyballs and nanotubes.




Is carbon the only element that can do this?



If not, then what are the other elements can also do this? Is there a term to describe such elements?



What is the chemical characteristic that allows this to occur?



I would greatly appreciate it if people could please take the time to clarify this.






bond elements







share|improve this question











$endgroup$








  • 2




    $begingroup$
    Catenation : self linking property of an element (atom).
    $endgroup$
    – glucose
    18 hours ago






  • 9




    $begingroup$
    The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
    $endgroup$
    – matt_black
    16 hours ago






  • 1




    $begingroup$
    I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
    $endgroup$
    – jeffB
    14 hours ago








  • 1




    $begingroup$
    Sulfur can also form rings and chains
    $endgroup$
    – porphyrin
    13 hours ago






  • 1




    $begingroup$
    What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
    $endgroup$
    – Mithoron
    8 hours ago
















11












11








11





$begingroup$


My textbook says the following:




Unique among the elements, carbon can bond to itself to form extremely strong two-dimensional sheets, as it does in graphite, as well as buckyballs and nanotubes.




Is carbon the only element that can do this?



If not, then what are the other elements can also do this? Is there a term to describe such elements?



What is the chemical characteristic that allows this to occur?



I would greatly appreciate it if people could please take the time to clarify this.






bond elements







share|improve this question











$endgroup$




My textbook says the following:




Unique among the elements, carbon can bond to itself to form extremely strong two-dimensional sheets, as it does in graphite, as well as buckyballs and nanotubes.




Is carbon the only element that can do this?



If not, then what are the other elements can also do this? Is there a term to describe such elements?



What is the chemical characteristic that allows this to occur?



I would greatly appreciate it if people could please take the time to clarify this.






bond elements




bond elements






share|improve this question















share|improve this question













share|improve this question




share|improve this question








edited 5 hours ago









Karsten Theis

5,104644




5,104644










asked 19 hours ago









The PointerThe Pointer

1814




1814








  • 2




    $begingroup$
    Catenation : self linking property of an element (atom).
    $endgroup$
    – glucose
    18 hours ago






  • 9




    $begingroup$
    The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
    $endgroup$
    – matt_black
    16 hours ago






  • 1




    $begingroup$
    I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
    $endgroup$
    – jeffB
    14 hours ago








  • 1




    $begingroup$
    Sulfur can also form rings and chains
    $endgroup$
    – porphyrin
    13 hours ago






  • 1




    $begingroup$
    What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
    $endgroup$
    – Mithoron
    8 hours ago
















  • 2




    $begingroup$
    Catenation : self linking property of an element (atom).
    $endgroup$
    – glucose
    18 hours ago






  • 9




    $begingroup$
    The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
    $endgroup$
    – matt_black
    16 hours ago






  • 1




    $begingroup$
    I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
    $endgroup$
    – jeffB
    14 hours ago








  • 1




    $begingroup$
    Sulfur can also form rings and chains
    $endgroup$
    – porphyrin
    13 hours ago






  • 1




    $begingroup$
    What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
    $endgroup$
    – Mithoron
    8 hours ago










2




2




$begingroup$
Catenation : self linking property of an element (atom).
$endgroup$
– glucose
18 hours ago




$begingroup$
Catenation : self linking property of an element (atom).
$endgroup$
– glucose
18 hours ago




9




9




$begingroup$
The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
$endgroup$
– matt_black
16 hours ago




$begingroup$
The right question isn't whether an element can bond to itself. Plenty do that. The issue is whether an element can form a wide variety of stable structures when bonded to itself.
$endgroup$
– matt_black
16 hours ago




1




1




$begingroup$
I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
$endgroup$
– jeffB
14 hours ago






$begingroup$
I was also aware that boron sheets were recently synthesized, but did not realize that someone has even predicted nitrogen sheets that could be stable at room temperature!
$endgroup$
– jeffB
14 hours ago






1




1




$begingroup$
Sulfur can also form rings and chains
$endgroup$
– porphyrin
13 hours ago




$begingroup$
Sulfur can also form rings and chains
$endgroup$
– porphyrin
13 hours ago




1




1




$begingroup$
What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
$endgroup$
– Mithoron
8 hours ago






$begingroup$
What is the actual question here? Your citation does not say that bonding between identical atoms is something unique - every single element could do this even if transiently. The point is that carbon carbon allotropes are somewhat exceptional.
$endgroup$
– Mithoron
8 hours ago












3 Answers
3






active

oldest

votes


















10












$begingroup$


Is carbon the only element that can do this?




No, carbon is not the only element with such characteristics.




If not, then what are the other elements can also do this?




There is a whole number of elements such as silicon, arsenic, germanium.




Is there a term to describe such elements?




At least I'm unaware of such a term, which might be furnished by our far wiser community.




What is the chemical characteristic that allows this to occur?




Catenation.



More information:



According to the Molecular Orbital Theory, the condition for a compound to exist is that it should have more electrons in the bonding orbitals than in the anti-bonding orbitals. So, as long as you have the bonding orbitals filled more, you can have pretty anything, more than just chains of atoms.



Thus, the existence of a compound also depends on the precise conditions in which the compound is kept, for example sodium forms different types of chlorides under different conditions and that as pointed out by Poutnik in the comments, $ce{He2^1+}$ and a ton of others are discovered and still more awaiting discovery.






share|improve this answer











$endgroup$





















    0












    $begingroup$

    No, carbon is not the only one that can bond to itself. It's a unique property of some elements mainly the group 14 elements like silicon, germanium, arsenic etc. This phenomenon is called catenation. It might be mainly due to presence of four valence electrons in their outermost shell. A large number of carbon atoms are linked with each other with sigma and pi bonds. However catenation gets limited as we move down the group in group 14.






    share|improve this answer








    New contributor




    Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
    Check out our Code of Conduct.






    $endgroup$





















      -2












      $begingroup$

      So most of this has been answered, but the main elements that can bond to themselves are called diatomic atoms. This includes hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, and bromine. There are other elements that can do this as well, however these main elements occur naturally in their diatomic state as gases.






      share|improve this answer










      New contributor




      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
      Check out our Code of Conduct.






      $endgroup$









      • 4




        $begingroup$
        "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
        $endgroup$
        – andselisk
        9 hours ago










      • $begingroup$
        It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
        $endgroup$
        – Mark
        7 hours ago










      • $begingroup$
        The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
        $endgroup$
        – Karsten Theis
        1 hour ago












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      3 Answers
      3






      active

      oldest

      votes








      3 Answers
      3






      active

      oldest

      votes









      active

      oldest

      votes






      active

      oldest

      votes









      10












      $begingroup$


      Is carbon the only element that can do this?




      No, carbon is not the only element with such characteristics.




      If not, then what are the other elements can also do this?




      There is a whole number of elements such as silicon, arsenic, germanium.




      Is there a term to describe such elements?




      At least I'm unaware of such a term, which might be furnished by our far wiser community.




      What is the chemical characteristic that allows this to occur?




      Catenation.



      More information:



      According to the Molecular Orbital Theory, the condition for a compound to exist is that it should have more electrons in the bonding orbitals than in the anti-bonding orbitals. So, as long as you have the bonding orbitals filled more, you can have pretty anything, more than just chains of atoms.



      Thus, the existence of a compound also depends on the precise conditions in which the compound is kept, for example sodium forms different types of chlorides under different conditions and that as pointed out by Poutnik in the comments, $ce{He2^1+}$ and a ton of others are discovered and still more awaiting discovery.






      share|improve this answer











      $endgroup$


















        10












        $begingroup$


        Is carbon the only element that can do this?




        No, carbon is not the only element with such characteristics.




        If not, then what are the other elements can also do this?




        There is a whole number of elements such as silicon, arsenic, germanium.




        Is there a term to describe such elements?




        At least I'm unaware of such a term, which might be furnished by our far wiser community.




        What is the chemical characteristic that allows this to occur?




        Catenation.



        More information:



        According to the Molecular Orbital Theory, the condition for a compound to exist is that it should have more electrons in the bonding orbitals than in the anti-bonding orbitals. So, as long as you have the bonding orbitals filled more, you can have pretty anything, more than just chains of atoms.



        Thus, the existence of a compound also depends on the precise conditions in which the compound is kept, for example sodium forms different types of chlorides under different conditions and that as pointed out by Poutnik in the comments, $ce{He2^1+}$ and a ton of others are discovered and still more awaiting discovery.






        share|improve this answer











        $endgroup$
















          10












          10








          10





          $begingroup$


          Is carbon the only element that can do this?




          No, carbon is not the only element with such characteristics.




          If not, then what are the other elements can also do this?




          There is a whole number of elements such as silicon, arsenic, germanium.




          Is there a term to describe such elements?




          At least I'm unaware of such a term, which might be furnished by our far wiser community.




          What is the chemical characteristic that allows this to occur?




          Catenation.



          More information:



          According to the Molecular Orbital Theory, the condition for a compound to exist is that it should have more electrons in the bonding orbitals than in the anti-bonding orbitals. So, as long as you have the bonding orbitals filled more, you can have pretty anything, more than just chains of atoms.



          Thus, the existence of a compound also depends on the precise conditions in which the compound is kept, for example sodium forms different types of chlorides under different conditions and that as pointed out by Poutnik in the comments, $ce{He2^1+}$ and a ton of others are discovered and still more awaiting discovery.






          share|improve this answer











          $endgroup$




          Is carbon the only element that can do this?




          No, carbon is not the only element with such characteristics.




          If not, then what are the other elements can also do this?




          There is a whole number of elements such as silicon, arsenic, germanium.




          Is there a term to describe such elements?




          At least I'm unaware of such a term, which might be furnished by our far wiser community.




          What is the chemical characteristic that allows this to occur?




          Catenation.



          More information:



          According to the Molecular Orbital Theory, the condition for a compound to exist is that it should have more electrons in the bonding orbitals than in the anti-bonding orbitals. So, as long as you have the bonding orbitals filled more, you can have pretty anything, more than just chains of atoms.



          Thus, the existence of a compound also depends on the precise conditions in which the compound is kept, for example sodium forms different types of chlorides under different conditions and that as pointed out by Poutnik in the comments, $ce{He2^1+}$ and a ton of others are discovered and still more awaiting discovery.







          share|improve this answer














          share|improve this answer



          share|improve this answer








          edited 15 hours ago









          Martin - マーチン♦

          34.1k9112239




          34.1k9112239










          answered 19 hours ago









          user79161user79161

          17818




          17818























              0












              $begingroup$

              No, carbon is not the only one that can bond to itself. It's a unique property of some elements mainly the group 14 elements like silicon, germanium, arsenic etc. This phenomenon is called catenation. It might be mainly due to presence of four valence electrons in their outermost shell. A large number of carbon atoms are linked with each other with sigma and pi bonds. However catenation gets limited as we move down the group in group 14.






              share|improve this answer








              New contributor




              Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
              Check out our Code of Conduct.






              $endgroup$


















                0












                $begingroup$

                No, carbon is not the only one that can bond to itself. It's a unique property of some elements mainly the group 14 elements like silicon, germanium, arsenic etc. This phenomenon is called catenation. It might be mainly due to presence of four valence electrons in their outermost shell. A large number of carbon atoms are linked with each other with sigma and pi bonds. However catenation gets limited as we move down the group in group 14.






                share|improve this answer








                New contributor




                Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                Check out our Code of Conduct.






                $endgroup$
















                  0












                  0








                  0





                  $begingroup$

                  No, carbon is not the only one that can bond to itself. It's a unique property of some elements mainly the group 14 elements like silicon, germanium, arsenic etc. This phenomenon is called catenation. It might be mainly due to presence of four valence electrons in their outermost shell. A large number of carbon atoms are linked with each other with sigma and pi bonds. However catenation gets limited as we move down the group in group 14.






                  share|improve this answer








                  New contributor




                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.






                  $endgroup$



                  No, carbon is not the only one that can bond to itself. It's a unique property of some elements mainly the group 14 elements like silicon, germanium, arsenic etc. This phenomenon is called catenation. It might be mainly due to presence of four valence electrons in their outermost shell. A large number of carbon atoms are linked with each other with sigma and pi bonds. However catenation gets limited as we move down the group in group 14.







                  share|improve this answer








                  New contributor




                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.









                  share|improve this answer



                  share|improve this answer






                  New contributor




                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.









                  answered 15 hours ago









                  Charlie GogoiCharlie Gogoi

                  91




                  91




                  New contributor




                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.





                  New contributor





                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.






                  Charlie Gogoi is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                  Check out our Code of Conduct.























                      -2












                      $begingroup$

                      So most of this has been answered, but the main elements that can bond to themselves are called diatomic atoms. This includes hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, and bromine. There are other elements that can do this as well, however these main elements occur naturally in their diatomic state as gases.






                      share|improve this answer










                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.






                      $endgroup$









                      • 4




                        $begingroup$
                        "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                        $endgroup$
                        – andselisk
                        9 hours ago










                      • $begingroup$
                        It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                        $endgroup$
                        – Mark
                        7 hours ago










                      • $begingroup$
                        The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                        $endgroup$
                        – Karsten Theis
                        1 hour ago
















                      -2












                      $begingroup$

                      So most of this has been answered, but the main elements that can bond to themselves are called diatomic atoms. This includes hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, and bromine. There are other elements that can do this as well, however these main elements occur naturally in their diatomic state as gases.






                      share|improve this answer










                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.






                      $endgroup$









                      • 4




                        $begingroup$
                        "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                        $endgroup$
                        – andselisk
                        9 hours ago










                      • $begingroup$
                        It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                        $endgroup$
                        – Mark
                        7 hours ago










                      • $begingroup$
                        The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                        $endgroup$
                        – Karsten Theis
                        1 hour ago














                      -2












                      -2








                      -2





                      $begingroup$

                      So most of this has been answered, but the main elements that can bond to themselves are called diatomic atoms. This includes hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, and bromine. There are other elements that can do this as well, however these main elements occur naturally in their diatomic state as gases.






                      share|improve this answer










                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.






                      $endgroup$



                      So most of this has been answered, but the main elements that can bond to themselves are called diatomic atoms. This includes hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, and bromine. There are other elements that can do this as well, however these main elements occur naturally in their diatomic state as gases.







                      share|improve this answer










                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.









                      share|improve this answer



                      share|improve this answer








                      edited 9 hours ago









                      andselisk

                      19.9k667129




                      19.9k667129






                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.









                      answered 9 hours ago









                      Santiago ArellanoSantiago Arellano

                      12




                      12




                      New contributor




                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.





                      New contributor





                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.






                      Santiago Arellano is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
                      Check out our Code of Conduct.








                      • 4




                        $begingroup$
                        "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                        $endgroup$
                        – andselisk
                        9 hours ago










                      • $begingroup$
                        It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                        $endgroup$
                        – Mark
                        7 hours ago










                      • $begingroup$
                        The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                        $endgroup$
                        – Karsten Theis
                        1 hour ago














                      • 4




                        $begingroup$
                        "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                        $endgroup$
                        – andselisk
                        9 hours ago










                      • $begingroup$
                        It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                        $endgroup$
                        – Mark
                        7 hours ago










                      • $begingroup$
                        The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                        $endgroup$
                        – Karsten Theis
                        1 hour ago








                      4




                      4




                      $begingroup$
                      "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                      $endgroup$
                      – andselisk
                      9 hours ago




                      $begingroup$
                      "Diatomic atom" is a weird term, diatomic molecule makes way more sense. Besides, the way the answer is formulated, it appears to me that all elements that are capable of self-bonding are diatomic molecules, whereas in reality diatomic molecules is a tiny subset of the former.
                      $endgroup$
                      – andselisk
                      9 hours ago












                      $begingroup$
                      It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                      $endgroup$
                      – Mark
                      7 hours ago




                      $begingroup$
                      It's pretty clear that the question is asking about self-bonding beyond simple diatomic molecules.
                      $endgroup$
                      – Mark
                      7 hours ago












                      $begingroup$
                      The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                      $endgroup$
                      – Karsten Theis
                      1 hour ago




                      $begingroup$
                      The ability to make a stable diatomic molecule might be the reason for not observing chains or 2D structures for these elements.
                      $endgroup$
                      – Karsten Theis
                      1 hour ago


















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