Why Do Strongly Bonded Compounds Like HCl and NaCl Ionize in Water?

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Discussion Overview

The discussion centers on the ionization of strongly bonded compounds, specifically HCl and NaCl, in water. Participants explore the nature of bonding in these compounds and the mechanisms behind their dissociation in aqueous solutions, touching on concepts of acid strength and hydrolysis.

Discussion Character

  • Exploratory, Technical explanation, Debate/contested

Main Points Raised

  • One participant questions why HCl, which has strong bonds, readily ionizes into H+ and Cl- in water, suggesting that it seems counterintuitive for a strongly bonded compound to completely dissociate.
  • Another participant notes that HF, despite being strongly bonded, does not ionize in the same manner, leading to its classification as a weak acid.
  • A participant raises the point that NaCl, which is ionically bonded, also dissociates easily in water, questioning the energy dynamics involved in breaking these bonds compared to the interactions with water molecules.
  • One participant introduces the idea that during the hydrolysis of an acid, a strong covalent bond is formed between H and O in the hydronium ion (H3O+), which may play a role in the ionization process.
  • Another participant asserts that HCl is covalent, which may influence its behavior in water.

Areas of Agreement / Disagreement

Participants express differing views on the nature of bonding in HCl and its implications for ionization, as well as the comparison with HF and NaCl. The discussion remains unresolved regarding the underlying reasons for the observed behaviors of these compounds in water.

Contextual Notes

Participants have not fully explored the assumptions regarding bond strength, energy requirements for dissociation, or the definitions of covalent versus ionic bonding in this context.

krackers
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The bonds between H and Cl are strong, almost close to ionic, right? Thus if that is the case why does HCl readily ionize into H+ and Cl- upon contact with water? It doesn't make sense that such a strongly bonded compound should completely disassociate upon contact with water. Further, why does HF, another strongly bonded compound, not do the same thus making it a weak acid?

On a similar note, why does NaCl do the same? Na and Cl are very strongly ionically bonded, requiring lots of energy to break apart the bond. Yet on contact with water, they easily disassociate. Interactions between the Na, Cl, and the H2O dipole don't seem like they have enough energy to break it apart.
 
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You should also take in mind that in the process of hydrolysis of an acid there is a new and very strong covalent bond being formed namely between H and O in ##\mathrm{H_3O^+}##.
 
HCl is covalent.
 

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