Q. 6.6 - An Introduction to General, Organic, and Biological Chemistry

Question

Write the symbols for the ions with the following number of protons and electrons:

a. $8$ protons, $10$ electrons

b. $19$ protons, $18$ electrons

C. $35$ protons,  $36$ electrons

d. $50$ protons, $46$ electrons

Step-by-Step Solution

Answer

(part a) The ion with $8$ protons and $10$ electrons has the symbol ${\mathrm{O}}^{2-}$.

(part b) The ion with $19$ protons and $18$electrons has the symbol ${\mathrm{K}}^{+}$.

(part c) The ion with $35$ protons and $36$ electron has the symbol ${\mathrm{Br}}^{-}$.

(part d) The ion with $50$ protons and $46$ electrons has the symbol $S{n}^{4+}$.

Step 1: Information (part a)

Write the element's symbol with the required number of protons. Add the total positive charge owing to the total number of protons and the total negative charge due to the entire number of electrons to get the ionic charge.

Step 2: Explanation (part a)

(part a)

The element with $8$protons has the symbol $\mathrm{O}$. Add the total positive charge owing to the total number of protons and the total negative charge due to the entire number of electrons to get the ionic charge:

$$\begin{gathered} ionic charge = (8+)+(-10) \\ =-2 \end{gathered}$$

Step 3: Information (part b)

${\mathrm{O}}^{2-}$ is the symbol for the ion with the estimated ionic charge. Thus, the ion with $8$ protons and $10$ electrons has the symbol ${\mathrm{O}}^{2-}$.

Step 4: Explanation ( part b)

(part b)

$\mathrm{K}$ is the symbol for the element with $19$ protons. Add the total positive charge owing to the total number of protons and the total negative charge due to the entire number of electrons to get the ionic charge:

$$\begin{gathered} ionic charge = (+19)+(-18) \\ =+1 \end{gathered}$$

Step 5: Information (part c)

${\mathrm{K}}^{+}$ is the symbol for the ion with the determined ionic charge. As a result, the ion with $19$ protons and $18$ electrons has the symbol ${\mathrm{K}}^{+}$.

Step 6: Explanation ( Part c)

(part c)

$\mathrm{Br}$ is the symbol for the element with $35$ protons. Add the total positive charge owing to the total number of protons and the total negative charge due to the entire number of electrons to get the ionic charge:

$$\begin{gathered} ionic charge = (+35)+(-36) \\ =-1 \end{gathered}$$

Step 7: Information (part d)

${Br}^{-}$ is the symbol for the ion with the estimated ionic charge. As a result, the ion with $35$ protons and $36$ electrons has the symbol ${Br}^{-}$.

Step 8: Explanation (part d)

(part d)

$\mathrm{Sn}$is the symbol for the element with $50$ protons. Add the total positive charge owing to the total number of protons and the total negative charge due to the entire number of electrons to get the ionic charge:

$$\begin{gathered} ionic charge = (+50)+(-46) \\ =+4 \end{gathered}$$

${\mathrm{Sn}}^{4+}$ is the symbol for the ion with the estimated ionic charge. ${\mathrm{Sn}}^{4+}$ is the symbol for the ion having $50$ protons and $46$ electrons.