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Chapter 9: Problem 143

Give a brief description of the medical uses of the following ionic compounds: \(\mathrm{AgNO}_{3}, \mathrm{BaSO}_{4},\) \(\mathrm{CaSO}_{4}, \mathrm{KI}, \mathrm{Li}_{2} \mathrm{CO}_{3}, \mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgSO}_{4}, \mathrm{NaHCO}_{3}\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{NaF}, \mathrm{TiO}_{2}, \mathrm{ZnO} .\) You would need to do a Web search of some of these compounds.

Short Answer

Expert verified
The ionic compounds are used in various medical applications, such as antiseptics (silver nitrate), contrast agents in X-ray imaging (barium sulfate), and bone cement (calcium sulfate). Other compounds, like magnesium hydroxide or sodium bicarbonate, are commonly used in antacids.

Step by step solution

01

Research \(\mathrm{AgNO}_{3}\)

Silver nitrate (\(\mathrm{AgNO}_{3}\)) is used in medicine for its antiseptic and astringent (tissue tightening) properties. It's often used for removing warts and treating skin ulcers.
02

Research \(\mathrm{BaSO}_{4}\)

Barium sulfate (\(\mathrm{BaSO}_{4}\)) is used in medicine as a contrast agent in X-ray imaging of the digestive system. When swallowed, it helps to highlight certain areas, so they can be seen more clearly on an X-ray.
03

Research \(\mathrm{CaSO}_{4}\)

Calcium sulfate (\(\mathrm{CaSO}_{4}\)) is used in medicine as bone cement and for setting broken bones. It's considered biocompatible and can be reabsorbed by the body over time.
04

Research Additional Compounds

Continue this research process for \(\mathrm{KI}\), \(\mathrm{Li}_{2} \mathrm{CO}_{3}\), \(\mathrm{Mg}(\mathrm{OH})_{2}\), \(\mathrm{MgSO}_{4}\), \(\mathrm{NaHCO}_{3}\), \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), \(\mathrm{NaF}\), \(\mathrm{TiO}_{2}\), and \(\mathrm{ZnO}\). Each compound may have specific uses in the medical field.

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Most popular questions from this chapter

Write Lewis structures for the following ions: (a) \(\mathrm{O}_{2}^{2-},\) (b) \(\mathrm{C}_{2}^{2-},\) (c) \(\mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.

For each of the following organic molecules draw a Lewis structure in which the carbon atoms are bonded to each other by single bonds: (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{C}_{4} \mathrm{H}_{10},\) (c) \(\mathrm{C}_{5} \mathrm{H}_{12}\). For (b) and (c), show only structures in which each \(\mathrm{C}\) atom is bonded to no more than two other \(\mathrm{C}\) atoms.

Draw reasonable resonance structures for the following ions: (a) \(\mathrm{HSO}_{4}^{-},\) (b) \(\mathrm{PO}_{4}^{3-},\) (c) \(\mathrm{HSO}_{3}^{-}\) (d) \(\mathrm{SO}_{3}^{2-}\). (Hint: See comment on Example \(\left.9.11 .\right)\)

Comment on the correctness of the statement, "All compounds containing a noble gas atom violate the octet rule."

Compare single, double, and triple bonds in a molecule, and give an example of each. For the same bonding atoms, how does the bond length change from single bond to triple bond?
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