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You sound like you've half got it already. A compound that doesn't
dissolve in water is probably not an ionic substance since water solvates
most (but not all) ionic substances. The final proof that the compound is
not ionic is that its molten form does not conduct electricity. Molten ionic
compounds are composed of mobile, electically charged particles, and thus
conduct electrical current.
Non-ionic substances have much lower melting points on average than
ionic compounds. Organic ionic compounds, such as sodium acetate, usually
decompose before they melt. That gives you an idea of just how stable ionic
compounds are. Since the question seems to be about ionic vs covalent
bonding, the answer should probably be that it would have a relatively low
melting point.
Hope this helps,
MikeKL5
"hii
It's a textbook question...but i don't understand it
A chemist analyzes a white, solid compound and finds that it does not
dissolve in water. When the compound is melted, it does not conduct
electricity.
(a.)What would you expect to be true about this compound's melting point?
[Does the conductivity of the compound have a relationship to if it was
melted or not?] -- If the compound melted, does it mean it has a low melting
point?
(b.)Are the atoms that make up this compound joined with covalent or ionic
bonds? Explain.
[I think it covalent because the compound isn't soluble and it does not
conduct electricity]
Thank you once again!"
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