Question

In an ion with an unknown charge, the total mass of all the electrons was determined to be 2.19 ✕ 10−26 g, while the total mass of its protons was 4.34 ✕ 10−23 g. What is the identity and charge of this ion? (Enter your answer in the form X^q±.)

Answer 1

`\large \boxed{\text{Fe$^{{2+}}$}}`

Step-by-step explanation:

1. Number of electrons

`\text{Number of electrons} = 2.19 * 10^(-26)\text{ g} * \frac{\text{1 electron}}{9.109 * 10^(-28)\text{ g}} = \text{24 electrons}`

2. Number of protons

`\text{Number of protons} = 4.34 * 10^(-23)\text{ g} * \frac{\text{1 proton}}{1.673 * 10^(-24)\text{ g}} = \text{26 protons}`

3. Identify the ion

An atom with 26 protons is iron, Fe.

A neutral atom of iron would have 26 electrons.

The ion has only 24 electrons, so it has lost two. The ion must have a charge of +2.

`\text{The symbol for the ion is $\large \boxed{\textbf{Fe$^{\mathbf{2+}}$}}$}`