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Chapter 2: Problem 39

What is an ionic compound? How is electrical neutrality maintained in an ionic compound?

Short Answer

Expert verified
An ionic compound consists of positive and negative ions. It is formed when a metal loses electrons and becomes a positive ion (cation), and a nonmetal gains those electrons becoming a negative ion (anion). The electrical neutrality in an ionic compound is maintained by ensuring the total positive charge equals the total negative charge, imparted by equal numbers of positive (cation) and negative (anion) ions.

Step by step solution

01

Understanding Ionic Compounds

An ionic compound is a compound made up of ions. They are formed when a metal loses electrons, and a nonmetal gains those electrons. The metal becomes a positively charged cation, and the nonmetal becomes a negatively charged anion. Because the positive and negative charges attract each other, these ions bond together to create an ionic compound.
02

Explain Electrical Neutrality in Ionic Compounds

Electrical neutrality in an ionic compound is maintained by the equal numbers of positive and negative charges. This balance is due to the loss and gain of electrons that happens when the ionic compound is formed. In other words, for every electron that a metal atom loses, a nonmetal atom gains one. This ensures that the total positive charge from the cations equals the total negative charge from the anions, creating an electrically neutral compound.

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Most popular questions from this chapter

Elements whose names end with "-ium" are usually metals; sodium is one example. Identify a nonmetal whose name also ends with "-ium."

Fill the blanks in the following table. $$\begin{array}{|c|c|c|c|}\hline \text { Cation } & \text { Anion } & \text { Formula } & \text { Name } \\\\\hline & & & \text { Magnesium bicarbonate } \\\\\hline & & \mathrm{Sr} \mathrm{Cl}_{2} & \\\\\hline \mathrm{Fe}^{3+} & \mathrm{NO}_{2}^{-} & & \\ \hline & & & \text { Manganese(II) chlorate } \\\\\hline & & \mathrm{SnBr}_{4} & \\\\\hline \mathrm{Co}^{2+} & \mathrm{PO}_{4}^{3-} & & \\\\\hline \mathrm{Hg}_{2}^{2+} & \mathrm{I}^{-} & & \\\\\hline & & \mathrm{Cu}_{2} \mathrm{CO}_{3} & \\\\\hline & & & \text { Lithium nitride } \\\\\hline \mathrm{Al}^{3+} & \mathrm{S}^{2-} & & \\\\\hline\end{array}$$

The Group \(1 \mathrm{~B}\) metals, \(\mathrm{Cu}, \mathrm{Ag},\) and \(\mathrm{Au},\) are called coinage metals. What chemical properties make them specially suitable for making coins and jewels?

The formula for calcium oxide is \(\mathrm{CaO}\). What are the formulas for magnesium oxide and strontium oxide?

What are the empirical formulas of the following compounds? (a) \(\mathrm{Al}_{2} \mathrm{Br}_{6},\) (b) \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{4},\) (c) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\)
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