WHy are ionic bonds intramolecular forces?

In summary, the conversation discusses the concept of intramolecular forces and how they apply to ionic compounds and mixtures. It is explained that intramolecular forces hold atoms together to form compounds or molecules. In the case of pure NaCl, the ionic bonds hold the ions together. However, in a mixture of molten NaCl and CaCl2, the ionic bonds hold together a random order of ions, making it more complex. It is also noted that in an ideal case, a cooled melt would create one crystal with no molecules, making the bonds still intramolecular. The discussion also brings up the question of whether ionic compounds have covalent contributions and how overlapping electron clouds play a role in this concept.
  • #1
sgstudent
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3
An intramolecular force is a force that holds atoms that form compounds or moleculues together. So if we have NaCl there are a large number of Na+ and Cl- so those ionic bonds hold the ions together so they are considered intramolecular.

But say we have a mixture of molten NaCl and CaCl2 and we let them cool together. So some parts of the NaCl and CaCl2 would be mixed together - the structure would have different parts to it like Na+Cl-Ca2+Cl-Ca2+Cl-Na+ all in a random order.

In this case how can we consider those ionic bonds intramolecular? Because now they do not hold just the ions that form the compounds but instead they hold ions that form a mixture that does not have a specific ionic structure like in pure NaCl. So what are they considered in this case?

Thanks in advance
 
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  • #2
When a melt is cooled, it creates (ideally) one crystal. There are no molecules as well as in NaCl crystal there are no molecules. It's "one big molecule", which means energy states are different for every single electron (that's the only Pauli exclusion principle option for a single particle). So the bonds are still intramolecular in an ideal case.

For distribution of electron energy states the electron clouds MUST be overlapping. For ionic compounds it's quite odd (so every ionic compound has some of covalent contribution? Or might there be an overlapping without covalent contribution?). I hope somebody will explain...
 
  • #3
Well, this seems well coresponding, because truly every ionic crystal has covalent contribution.
 

1. Why are ionic bonds considered intramolecular forces?

Ionic bonds are considered intramolecular forces because they occur within a molecule, between two or more atoms, rather than between separate molecules. These bonds are formed through the transfer of electrons from one atom to another, resulting in the formation of ions that are held together by electrostatic forces.

2. How do ionic bonds differ from other types of intramolecular forces?

Unlike covalent bonds, which involve the sharing of electrons between atoms, ionic bonds involve the complete transfer of electrons from one atom to another. This results in the formation of positively and negatively charged ions that are attracted to each other, creating a strong bond.

3. What types of elements are involved in the formation of ionic bonds?

Ionic bonds typically form between a metal and a nonmetal. Metals tend to have low electronegativity, meaning they have a tendency to lose electrons, while nonmetals have high electronegativity and tend to gain electrons. This difference in electronegativity is what drives the formation of ionic bonds.

4. How do ionic bonds affect the physical properties of a substance?

Ionic bonds result in the formation of a crystal lattice structure, where positively and negatively charged ions are arranged in a repeating pattern. This structure leads to substances with high melting and boiling points, as well as being brittle and non-conductive in their solid form.

5. Can ionic bonds be broken?

Yes, ionic bonds can be broken through the addition or removal of energy. This can be achieved through processes such as dissolving in water, where the polar water molecules can separate the ions, or through the application of heat or electricity, which can provide enough energy to overcome the electrostatic forces holding the ions together.

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