J.R. S. answered • 05/29/18
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Ph.D. in Biochemistry--University Professor--Chemistry Tutor
If I understand your question correctly, the two sodium ATOMS would be bonded to each other by a metallic bond, and the two chlorine ATOMS would be bonded to each other by a covalent bond. The metallic bond is a bond that holds atoms of a metal together and results from the delocalization of electrons leaving a positive ion in a sea of electrons. The covalent bond is the sharing of valence electrons. Now, if these atoms were to reacts as in 2Na(s) + Cl2(g) => 2NaCl(s), then the bond between the Na+ and Cl- would, as correctly pointed out by Arturo O., would indeed be an ionic bond.
Charvi P.
Sir can you please explain me that how does that happens
Like does metallic bonding of sodium atoms and covalent bonding of chlorine breaks to form an ionic bond
Also i would ask that why chlorine breaks its bonds if it does
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05/29/18
J.R. S.
tutor
Yes. When sodium atoms find themselves in the presence of chlorine gas (Cl2), there is a chemical reaction with a relatively large release of energy (exothermic reaction). The sodium atom has 1 valence electron and chlorine has 7 valence electrons. When the sodium atom gives its electrons to the chlorine atom, the result is the sodium cation (Na+) and the chlorine anion (Cl-), which then are attracted by electrostatic forces. So, in order for all of this to happen, it is safe to say that the metallic bonds holding sodium atoms together and the covalent bonds holding chlorine atoms together must be broken.
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05/30/18
Charvi P.
So it means that it is necessary that chlorine atoms and sodium atoms break their bonds in presence of each other
Metallic bonding doesnt make sodium atoms stable and keep them inert to chlorine atoms
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05/30/18
J.R. S.
tutor
Correct. The sodium atoms (even though held together by metallic bonds) still have 1 electron the the outer shell, and are more stable when they can lose that electron. Chlorine has 7 electrons and is more stable when it can gain another one. Sodium metal is extremely reactive, i.e. not very stable.
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05/30/18
Arturo O.
J.R.S.,
Would this also apply to any alkali metal in the proximity of any Group 17 element?
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05/30/18
J.R. S.
tutor
Arturo,
I would say yes with the possible exception of astatine, which probably is too unstable to behave as other group 17 halogens.
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05/30/18
Charvi P.
05/29/18