Q. 6.17 - An Introduction to General, Organic, and Biological Chemistry

Question

6.17 Write the correct ionic formula for the compound formed between each of the following pairs of ions:

a. ${\mathrm{Na}}^{+}$and ${\mathrm{O}}^{2-}$

b. ${\mathrm{Al}}^{3+}$ and $\mathrm{Br}$

c. ${\mathrm{Mg}}^{2+}$ and $\mathrm{F}$

d. ${\mathrm{Ml}}^{3+}$ and ${\mathrm{S}}^{2-}$

e. ${\mathrm{Ba}}^{2+}$ and ${\mathrm{N}}^{3-}$

Step-by-Step Solution

Answer

(part a) ${\mathrm{Na}}^{+}$ and ${\mathrm{O}}^{2-}$ is Oxide of aluminium (III), Calcium chloride (II),

(part b) ${\mathrm{Al}}^{3+}$  and $\mathrm{Br}$ is  Oxide of sodium (II),

(part c) ${\mathrm{Mg}}^{2+}$ and  $\mathrm{F}$ is Phosphide of magnesium (II), 

(part d) ${\mathrm{Ml}}^{3+}$ and ${\mathrm{S}}^{2-}$  is Iodide of potassium (I), 

(part e) ${\mathrm{Ba}}^{2+}$ and ${\mathrm{Ba}}^{2+}$ is Fluoride of barium (II).

Step 1 : Introduction (Part a)

To write the compound's name with the formula ${\mathrm{Al}}_2{\mathrm{O}}_3$, follow the steps below.

Write the ion generated by the non-metal first. $O$. The ion produced by non-metals $O$ is $O^{2-}$ to determine the charge on the cation now. $3{\mathrm{O}}^{2-ions}$ will be in command $3\times 2-=6-$. Two factors counteract this charge$\mathrm{Al}$ ions. The fee for each $\mathrm{Al}$ ion is $\frac{+6}{2}=+3$. As a result, the metal ion generated is ${\mathrm{Al}}^{3+}$.

Step 2: Explanation (Part a)

Write the cation's name. To do so, put the element name in parentheses and the charge in Roman numerals. The metal aluminium (III)

Write the anion's name. Use the initial syllable of the element's name, followed by Ide. Oxide.

Write the name of the compound first, then the cation, and finally the anion.

Oxide of aluminium (III).

Step 3 : Introduction (Part b)

To write the compound's name with the formula ${\mathrm{CaCl}}_2$, follow the steps below.

Write the ion generated by the non-metal first. $\mathrm{Cl}$. The ion produced by non-metals ${\mathrm{Cl}}^{-}{\mathrm{Cl}}^{-}$. One counterbalance Ca ion. The charge against Ca ion is $+2$. As a result, the metal ion generated is ${\mathrm{Ca}}^{2+}$.

Step 4 : Explanation (Part b)

Write the cation's name. To do so, put the element name in parentheses and the charge in Roman numerals. Calcium is an important mineral (II).

Write the anion's name. Use the initial syllable of the element name followed by $ide$. Chloride for this.

Write the compound's name first, followed by the cation, and then the anion.

Calcium chloride (II)

Step 5: Introduction (Part c)

To write the compound's name with the formula ${\mathrm{Na}}_2\mathrm{O}$, follow the steps below.

Write the ion generated by the non-metal first. $O$. The ion produced by non-metals $O$ is ${\mathrm{O}}^{2-}$. Two equal parts Na ions. The fee for each $N a$ ion is $\frac{+2}{2}=+1$. As a result, the metal ion generated is ${\mathrm{Na}}^{+}$.

Step 6 : Explanation (Part c)

Write the cation's name. Put the element name in parentheses and the charge in Roman numerals to accomplish this. Sodium is a mineral (I)

Write the anion's name. Use the initial syllable of the element's name, followed by Ide. Oxide.

Begin with the cation and end with the anion to write the chemical's name.

Oxide of sodium (II)

Step 7: Introduction (Part d)

To write the compound's name with the formula ${\mathrm{Mg}}_3{\mathrm{P}}_2$, follow the steps below.

Write the ion generated by the non-metal first. $P$. The non-metal ion produces $P$ is ${\mathrm{P}}^{3-}$. Three points of balance, ions. The fee for each $\mathrm{Mg}$ ion is $\frac{+6}{3}=+2$. As a result, the metal ion generated is${\mathrm{Al}}^{3+}.$

Step 8 : Explanation (Part d)

 Write the cation's name. To do so, put the element name in parentheses and the charge in Roman numerals. Magnesium is a mineral (II)

Write the anion's name. Use the element name's initial syllable followed by Ide. Phosphide for this.

Write the compound's name first, followed by the cation, and then the anion.

Phosphide of magnesium (II)

Step 9: Introduction (Part e)

Follow the instructions below to write the compound's name and formula$KI$.

Write down the ion produced by the non-metal $I$ first. The ion created by the non-metal $I$ is called ${\mathrm{I}}^{-}$. One $\mathrm{K}$ ion. The charge against $\mathrm{K}$ ion is $+1$. As a result, the metal ion generated is ${\mathrm{K}}^{+}$.

Step 10: Explanation (Part e)

Write the cation's name. To do so, put the element name in parentheses and the charge in Roman numerals. Potassium is a mineral (I)

Write the anion's name. Use the initial syllable of the element name followed by Ide. Iodide for this.

Write the name of the compound first, then the cation, and finally the anion.

Iodide of potassium (I).

Step 11 Introduction (Part f)

To write the compound's name with the formula ${\mathrm{BaF}}_2$, follow the steps below.

Write the ion generated by the non-metal first. $F$. The ion produced by non-metals $F$ is $F^{-}$. Determine the charge on the cation now. $2{ \mathrm{F}}^{-\text{ions will have charge }}2\times \mathrm{l}-=2-$. One $Ba$ ion balances this charge. The charge against $\mathrm{Ba}$ ion is $+2$. As a result, the metal ion generated is ${\mathrm{Ba}}^{2+}$.

Step 12: Explanation (Part f)

Write the cation's name. To do so, put the element name in parentheses and the charge in Roman numerals. Barium is a mineral (II)

Write the anion's name. Use the initial syllable of the element name followed by Ide. Fluoride for this.

Write the name of the compound first, then the cation, and finally the anion.

Fluoride of barium (II)