# Question cd962

Jul 5, 2017

$2.326 \times {10}^{-} 23$ $\text{g}$

#### Explanation:

I'll assume you meant a nitride ion...

We're asked to find the mass, in $\text{g}$, of one nitride ion, ${\text{N}}^{3 -}$.

This is simply a charged nitrogen atom, which has gained three electrons from bonding. Recall that electrons have negligible mass compared to nucleons (protons and neutrons). This, the atomic mass of a nitride ion is essentially the same as the mass of a lone nitrogen atom.

According to a periodic table, the relative atomic mass of $\text{N}$ is

color(red)(14.007 color(red)("amu"

One atomic mass unit is $\approx 1.660 \times {10}^{-} 24$ grams, so let's use dimensional analysis to find the mass in grams of a nitride ion:

14.007cancel("amu")((1.660xx10^-24color(white)(l)"g")/(1cancel("amu"))) = color(blue)(2.326 xx 10^-23 color(blue)("g"#