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

Determine the number of protons and neutrons in each isotope.
(a) $\quad \frac{23}{11} \mathrm{Na}$
(b) $\quad \frac{266}{88} \mathrm{Ra}$
(c) $\quad \frac{208}{82} \mathrm{Pb}$
(d) $\quad \frac{14}{7} \mathrm{N}$

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Key Concepts

Atomic Number

The atomic number represents the number of protons in an atom's nucleus. It uniquely identifies an element and determines its position on the periodic table, thereby influencing its chemical behavior.

Mass Number

The mass number is the total count of protons and neutrons in an atom's nucleus. It is used to distinguish between different isotopes of the same element, as variations in the number of neutrons affect the mass number.

Isotopes

Isotopes are forms of the same element that have identical numbers of protons but different numbers of neutrons. This difference in neutron count can influence the stability and radioactive properties of the atom.

Nuclear Notation

Nuclear notation is a system of writing an element's isotopic composition where the mass number is shown as a superscript and the atomic number as a subscript next to the element symbol. This notation provides immediate insight into the number of protons and the total nucleons present in the nucleus.

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