It takes such a high temperature to break the ionic bond when salt is heated, but in water, the ions separate easily, yes? Why is that? Why does the Na Cl still have the properties of salt when the Na and Cl ions are separate? I guess I thought that the NaCl was just in smaller clumps, but still bonded...
2007-03-07 17:04:16 · 4 answers · asked by hpagliughi 1 in Science & Mathematics ➔ Chemistry
Sir, it is not the ionic bond that holds solid NaCl together.
It is the lattice of NaCl particles as they fit with each other to create the cubic shape.
Because water is a polar subtance, the highly polarized NaCl can easy be pulled apart by the various H and OH particles in the water.
Melting salt is trying to use heat to break apart the lattice frame work and thus requires more energy.
2007-03-07 17:10:30 · answer #1 · answered by whatwouldyodado2006 4 · 0⤊ 0⤋
Because the water molecules are polar. The electrostatic attraction between the ions and the charged ends of the water molecule help the ions to break free. Non-polar solvents, such as heptane, do not attack salt.
2007-03-07 17:10:31 · answer #2 · answered by Anonymous · 0⤊ 0⤋
the ionic bonds are like magnets. water is a polar molecule, which pulls the bonds apart heating does not have the same effect
2007-03-07 17:09:21 · answer #3 · answered by Tom B 4 · 0⤊ 0⤋
THe bonds dont break in water they just just sort of go for shopping in their own confined space of water ..;...its not easy to break NaCl Bond
2007-03-07 17:12:17 · answer #4 · answered by akshai k 2 · 0⤊ 0⤋