Determine the number of protons and the number of neutrons...

Determine the number of protons and the number of neutrons in each isotope. \begin{equation}\text { a. }^{14} \mathrm{N} \quad\quad\quad\quad\quad \text { b. }_{11}^{23} \mathrm{Na}\end{equation} \begin{equation}\quad\quad \text { c. }\frac{222 \mathrm{Rn}}{86} \mathrm{Rn} \quad\quad \text { d. } \quad \frac{208}{82} \mathrm{Pb}\end{equation}

Determine the number of protons and the number of neutrons in each isotope.
\begin{equation}\text { a. }^{14} \mathrm{N} \quad\quad\quad\quad\quad \text { b. }_{11}^{23} \mathrm{Na}\end{equation} \begin{equation}\quad\quad
\text { c. }\frac{222 \mathrm{Rn}}{86} \mathrm{Rn} \quad\quad \text { d. } \quad \frac{208}{82} \mathrm{Pb}\end{equation}

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Key Concepts

Isotopes

Isotopes are variants of a chemical element that share the same atomic number (number of protons) but have different mass numbers due to varying numbers of neutrons. This difference in neutron count can affect the stability and nuclear properties of the isotope.

Atomic Number

The atomic number is the number of protons in the nucleus of an atom. It uniquely identifies an element and is fundamental in determining the chemical properties and placement of the element in the periodic table.

Mass Number

The mass number is the sum of protons and neutrons in an atom's nucleus. It is used to differentiate between isotopes and plays a crucial role in calculating the number of neutrons present in a specific isotope.

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