The atomic number indicates the number of protons in an atom's nucleus, which defines the chemical element. It is always a crucial part of an isotope's notation.

The mass number, which represents the sum of protons and neutrons, is usually written as a superscript. This distinguishes it from the atomic number that is commonly placed as a subscript.

Isotopes are variants of the same element that have identical numbers of protons but different numbers of neutrons. This difference results in varying mass numbers but similar chemical properties.

The mass number is the combined total of protons and neutrons within the nucleus of an atom. This value is fundamental for identifying different isotopes of the same element.

In Carbon-14, the number 14 is the mass number, which is the sum of the protons and neutrons in the nucleus. The atomic number for carbon remains 6, indicating its proton count.

To find the number of neutrons, subtract the atomic number (number of protons) from the mass number. This basic calculation is key to understanding isotope differences.

Uranium has an atomic number of 92, and with 144 neutrons the mass number becomes 236. Thus, the correct isotope notation is ²³❶U, where the superscript represents the mass number.

Carbon has an atomic number of 6, so it has 6 protons. For ¹³C, the number of neutrons is calculated as 13 - 6, which equals 7 neutrons.

Chlorine-35 is one of the stable isotopes of chlorine. In contrast, isotopes like Carbon-14 and Plutonium-244 are radioactive, and Chlorine-36 is unstable.

The mass number indicates the combined total of protons and neutrons in an atom's nucleus. In the notation ²❰❸Pb, 208 is the mass number, while the atomic number (for lead) is provided separately.

The element symbol in isotope notation uniquely identifies the chemical element. While the mass and atomic numbers provide additional details about the nucleus, the symbol is key to the element's identity.

Magnesium has an atomic number of 12, which means it has 12 protons. The mass number 24 indicates the sum of protons and neutrons, but only the atomic number specifies the proton count.

In a neutral atom, the number of electrons equals the number of protons, which is given by the atomic number. Hence, with an atomic number of 19, the atom has 19 electrons.

Radioactive isotopes are commonly referred to as radioisotopes. This term distinguishes them from stable isotopes and highlights their propensity to undergo radioactive decay.

Neon-20 indicates that the mass number is 20, derived from the total of protons and neutrons, while neon's atomic number is 10. The proper notation is ²❰Ne, with the mass number presented as a superscript.

Subtracting the atomic number of uranium (92) from the mass number (235) gives 143 neutrons. The abundance of neutrons in Uranium-235 is critical for initiating and sustaining nuclear chain reactions during fission.

Deuterium is the hydrogen isotope that consists of one proton and one neutron. This distinguishes it from protium, which has no neutrons, and tritium, which contains two neutrons.

During beta decay, a neutron is converted into a proton with the emission of a beta particle, causing the atomic number to increase by one while leaving the mass number unchanged. This change is key to understanding nuclear reaction processes.

Isotopic notation provides the mass and atomic numbers, which allow for the calculation of the neutron-to-proton ratio. A balanced ratio is a key indicator of nuclear stability and can hint at the likelihood of radioactivity.

Subtracting the atomic number (17) from the mass number (37) gives 20 neutrons. This neutron count plays an important role in determining the isotope's nuclear characteristics and overall stability.