# Question #c9f53

Aug 2, 2016

$\text{_(color(white)(a)6)^14"C}$

#### Explanation:

The problem gives you the isotope's atomic number, which means that you know how many protons it contains in its nucleus.

In this case, your isotope has an atomic number

$Z = 6$

which tells you that you have $6$ protons inside the nucleus. You also know that the isotope has $8$ neutrons, which means that you have all the information that you need in order to calculate its mass number, $A$

$\textcolor{b l u e}{| \overline{\underline{\textcolor{w h i t e}{\frac{a}{a}} A = Z + \text{no. of neutrons} \textcolor{w h i t e}{\frac{a}{a}} |}}}$

In this case, you have

$A = 6 + 8 = 14$

Now, grab a periodic table and look for the element that has an atomic number equal to $6$. You'll find it located in period 2, group 14 $\to$ carbon, $\text{C}$.

You know that you're dealing with an isotope of carbon that has $8$ neutrons. To write it using isotope notation, add the mass number to the upper left of the chemical symbol and the atomic number to the lower left. You will have

$\text{_(color(white)(a)6)^14"C} \to$ carbon-14