Fill in this table: $$ \begin{array}{lcccc} & { }^{14} \mathrm{~N} & \frac{24}{12} \mathrm{Mg} & { }_{11}^{23} \mathrm{Na} & { }^{59} \mathrm{Fe} \\ \hline \text { Mass number } & ? & ? & ? & ? \\ \text { Atomic number } & ? & ? & ? & ? \\ \text { Number of protons } & ? & ? & ? & ? \\ \text { Number of neutrons } & ? & ? & ? & ? \\ \text { Number of electrons } & ? & ? & ? & ? \\ \hline \end{array} $$

First, let us identify the atomic number (Z), mass number (A), and chemical symbols for each element given in the question. 1) \({ }^{14} \mathrm{~N}\): Here, the chemical symbol is N (Nitrogen) with mass number (A) = 14. The atomic number is not given, so we will need to find the atomic number of Nitrogen from the periodic table, which is 7. 2) \(\frac{24}{12} \mathrm{Mg}\): Here, the chemical symbol is Mg (Magnesium), atomic number (Z) = 12, and mass number (A) = 24. 3) \({ }_{11}^{23} \mathrm{Na}\): Here, the chemical symbol is Na (Sodium), atomic number (Z) = 11, and mass number (A) = 23. 4) \({ }^{59} \mathrm{Fe}\): Here, the chemical symbol is Fe (Iron), with mass number (A) = 59. The atomic number is not given, so we will need to find the atomic number of Iron from the periodic table, which is 26.

Now that we have identified the atomic number, mass number, and chemical symbol for each element, we can fill in the table. $$ \begin{array}{lcccc} & { }^{14} \mathrm{~N} & \frac{24}{12} \mathrm{Mg} & { }_{11}^{23} \mathrm{Na} & { }^{59} \mathrm{Fe} \\\ \hline \text { Mass number } & 14 & 24 & 23 & 59 \\\ \text { Atomic number } & 7 & 12 & 11 & 26 \\\ \text { Number of protons } & 7 & 12 & 11 & 26 \\\ \text { Number of neutrons } & 7 & 12 & 12 & 33 \\\ \text { Number of electrons } & 7 & 12 & 11 & 26 \\\ \hline \end{array} $$ Remember that the number of neutrons can be calculated by subtracting the atomic number from the mass number (A - Z). Similarly, the number of electrons is equal to the number of protons (Z) for a neutral element.