Q 6.14 - An Introduction to General, Organic, and Biological Chemistry

Question

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

a. $P^{3-}$ and  ${\mathrm{Cl}}^{-}$

b. ${\mathrm{Ca}}^{2+}$ and ${\mathrm{S}}^{2-}$

c. ${\mathrm{Li}}^{+}$ and $S^{2-}$

d. ${\mathrm{Rb}}^{+}$ and ${\mathrm{P}}^{3-}$

e. $C{s}^{{+}^{}}$and  $I^{-}$

Step-by-Step Solution

Answer

a. is the correct ionic formula for the chemical.

b. The compound's correct ionic formula is  .

c. is the proper ionic formula for the chemical.

d.  is the right ionic formula for the compound.

e. The compound's correct ionic formula is

Step 1 : Given information (part a)

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

a. ${\mathrm{Al}}^{3+}$ and ${\mathrm{Cl}}^{-}$

Step 2 : Explanation (part a)

(part a) The charge on the ${\mathrm{Al}}^{3+}$ ion is $3+$ while the charge on the ${\mathrm{Cl}}^{-i}$ ion is $1$ -. One ${\mathrm{Al}}^3$ ion and three ${\mathrm{Cl}}^{-}$ions are used to balance the charge $(3+)+3\times (1-)=0$. Write the positive ion first, then the negative ion in the ionic formula. ${\mathrm{AlCl}}_3$ is the correct ionic formula for the chemical.

Step 3 : Given Information (part b)

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

b. ${\mathrm{Ca}}^{2+}$ and ${\mathrm{S}}^{2-}$

Step 4 : Explanation (part b)

The charge on the ${\mathrm{Ca}}^{2+}$ ion is $2+$ while the charge on the ${\mathrm{s}}^2$ ion is $2-$.${\mathrm{S}}^{2-}$ with three  ${\mathrm{Ca}}^{2+}$ ions and two$(2+)+(2-)=0$ ions. Write the positive ion first, then the negative ion in the ionic formula. The compound's correct ionic formula is $\mathrm{CaS}$ .

Step 5 : Given information (part c)

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

c. ${\mathrm{Li}}^{+}$and ${\mathrm{S}}^{2-}$

Step 6 : Explanation (part c)

The fee for ${\mathrm{Li}}^{+}$ion is $1$, but the fee for ${\mathrm{S}}^{2-}$ is 2. Two ${\mathrm{Li}}^{+}$ ions and one${\mathrm{S}}^{2-}$ions $2\times (1+)+(2-)=0$ions are used to balance the charge. Write the positive ion first, then the negative ion, in the ionic formula. ${\mathrm{Li}}_2 \mathrm{S}$ is the proper ionic formula for the chemical.

Step 7 : Given information (part d)

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

d. ${\mathrm{Rb}}^{+}$and ${\mathrm{P}}^{3-}$

Step 8 : Expanation (part d)

The charge on the  ion is $1+$, while the charge on the ${\mathrm{p}}^{3-}$ ion is $3 -$. Three ${\mathrm{Rb}}^{+}$ions and one ${\mathrm{P}}^3$ ion are used to balance the charge $3\times (1+)+(3-)=0$. Write the positive ion first, then the negative ion in the ionic formula. ${\mathrm{Rb}}_3\mathrm{P}$ is the right ionic formula for the compound.

Step 9 : Given information (part e)

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

e. ${\mathrm{Cs}}^{+}$ and  ${\mathbf{I}}^{\mathbf{-}}$

Step 10 : Explanation (part e)

The fee for ${\mathrm{Cs}}^{+}$ion is $1+$, but the fee for ${\mathrm{I}}^{- }$is $1$. Two ${\mathrm{Cs}}^{+}$ions and three ${\mathrm{I}}^{-}$ ions $(1+)+(1-)=0$ ions are used to balance the charge ((1+)+(1-)=0$. Write the positive ion first, then the negative ion in the ionic formula. The compound's correct ionic formula is $Csl$