Question #cd962

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Question #cd962

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Answer 1 · 2017-07-05T15:31:01

$2.326 \times 10^{- 23}$ $2.326xx 10^-23$ $g$ $"g"$

Explanation:

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

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

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 $N$ $"N"$ is

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

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

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

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Question #cd962

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