Question

Name each ionic compound. $$ \begin{array}{l}{\text { a. } \mathrm{CaO}} \\ {\text { b. BaS }} \\ {\text { c. AlPO_ }} \\ {\text { d. } \mathrm{Ba}(\mathrm{OH})_{2}} \\ {\text { e. } \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}}\end{array} $$

Short answer

The names of the ionic compounds are: a. \(CaO\): Calcium oxide b. \(BaS\): Barium sulfide c. \(AlPO_4\): Aluminum phosphate d. \(Ba(OH)_2\): Barium hydroxide e. \(Sr(NO_3)_2\): Strontium nitrate

Step-by-step solution

Determine the Cation and Anion for Each Compound

First, we need to determine the cation (positively charged ion) and anion (negatively charged ion) for each compound. We will do this using the periodic table and remembering that the metal (usually on the left side of the periodic table) becomes the cation and the non-metal (usually on the right side of the periodic table) becomes the anion. a. CaO: Cation = Ca (calcium), Anion = O (oxygen) b. BaS: Cation = Ba (barium), Anion = S (sulfur) c. AlPO4: Cation = Al (aluminum), Anion = PO4 (phosphate) d. Ba(OH)2: Cation = Ba (barium), Anion = OH (hydroxide) e. Sr(NO3)2: Cation = Sr (strontium), Anion = NO3 (nitrate)

Name the Cations and Anions

Now that we have the cation and anion for each compound, we will name them according to their respective elements or groups. a. CaO: Cation = Calcium, Anion = oxide b. BaS: Cation = Barium, Anion = sulfide c. AlPO4: Cation = Aluminum, Anion = phosphate d. Ba(OH)2: Cation = Barium, Anion = hydroxide e. Sr(NO3)2: Cation = Strontium, Anion = nitrate

Combine the Names of the Cations and Anions

Finally, we will combine the names of the cations and anions to form the full name of the ionic compounds. a. CaO: Calcium oxide b. BaS: Barium sulfide c. AlPO4: Aluminum phosphate d. Ba(OH)2: Barium hydroxide e. Sr(NO3)2: Strontium nitrate

Key concepts

Ionic Bonds

Ionic bonds are fascinating and essential in the study of chemistry. They form when atoms transfer electrons between each other, typically between a metal and a non-metal. This electron exchange results in the formation of ions. A cation is a positively charged ion that has lost one or more electrons. In contrast, an anion is a negatively charged ion that has gained those electrons. The strength of ionic bonds comes from the strong electrostatic forces of attraction between the oppositely charged ions. Think of it as a powerful magnetic pull that keeps the ions tightly bound. This bond often results in the formation of a crystalline lattice, which is characteristic of many ionic compounds. Ionic compounds usually have high melting and boiling points due to the energy required to break these bonds. Another interesting property is their ability to conduct electricity when melted or dissolved in water, as their ions can move freely.

Cation and Anion Identification

Identifying cations and anions in a compound is crucial for naming ionic compounds. When you look at a formula like \( \text{CaO} \), you are seeing calcium (Ca) and oxygen (O). Here’s how you would typically determine each:

• Cations: These are generally metals and found on the left side of the periodic table. They lose electrons and have a positive charge. For instance, in \( \text{CaO} \), calcium acts as the cation.
• Anions: These are usually non-metals, found on the right side of the periodic table. They gain electrons and have a negative charge. In \( \text{CaO} \), oxygen is the anion.

To correctly name the ionic compound, you start with the cation, followed by the anion. For example, \( \text{CaO} \) is named calcium oxide. Always remember that the cation name is the same as the element, but for the anion, the ending changes to "-ide," unless it is a polyatomic ion such as phosphate (\( \text{PO}_4^{3-} \)).

Periodic Table

The periodic table is your best friend when it comes to identifying elements and understanding their properties for ionic compound naming. It is an organized chart that shows all known chemical elements arranged by increasing atomic number. Its layout is strategic: metals are on the left, and non-metals are on the right. This arrangement simplifies the process of identifying which elements can form cations and which can form anions.

• Groups and Periods: Elements in the same group have similar properties, as they have the same number of outer electrons. This can help predict the charge of the ions they form. For example, Group 1 elements (alkali metals) lose one electron to form cations with a charge of \( +1 \).
• Transition Metals: Often found in the middle of the periodic table, they can have variable charges, making naming slightly more complex as these require specific naming conventions (e.g., iron can be Fe\(^{2+}\), called ferrous, or Fe\(^{3+}\), known as ferric).

By understanding and using the layout of the periodic table, you can quickly determine the likely charges of ions and correctly name ionic compounds. Remember, practice makes perfect, and referring to the periodic table will help you reinforce this process.