Give the numbers of neutrons, protons, and electrons in the...

Give the numbers of neutrons, protons, and electrons in the atoms of each of the following isotopes: (a) radium-226, (b) ${ }^{206} \mathrm{~Pb},(\mathbf{c})$ carbon-14, (d) ${ }^{23} \mathrm{Na}$. (Use the table of atomic masses and numbers printed inside the front cover for additional information, as needed.)

Give the numbers of neutrons, protons, and electrons in the atoms of each of the following isotopes: (a) radium-226,
(b) ${ }^{206} \mathrm{~Pb},(\mathbf{c})$ carbon-14,
(d) ${ }^{23} \mathrm{Na}$. (Use the table of atomic masses and numbers printed inside the front cover for additional information, as needed.)

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Key Concepts

Neutron Calculation

The number of neutrons in an atom can be calculated by subtracting the atomic number from the mass number. This calculation is crucial when determining the specific properties of different isotopes.

Mass Number

The mass number is the total count of protons and neutrons in an atom's nucleus. It is used to differentiate isotopes within the same element by providing a measure of the overall mass of the nucleus.

Neutral Atomic Structure

A neutral atom contains equal numbers of protons and electrons. This balance ensures that the positive charge of the nucleus is exactly offset by the negative charge of the electrons, which is fundamental to the atom's stability.

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in distinct mass numbers, which are important for distinguishing among isotopes.

Atomic Number

The atomic number of an element represents the number of protons in its nucleus and uniquely identifies the element. In a neutral atom, the atomic number is also equal to the number of electrons, maintaining electrical neutrality.

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