Nuclides that have the same neutron excess are called isodiaphers.

Isodiaphers are nuclides having the same neutron excess, i.e. number of neutrons minus number of protons.

This means that even-even nuclei, which have not a strong neutron excess or neutron deficiency, have higher binding energy than their odd-odd isobar neighbors.

One large family of isodiaphers has zero neutron excess, N = Z. It contains many primordial isotopes of elements up to calcium.

In nuclear physics, isodiaphers refers to nuclides which have different atomic numbers and mass numbers but the same neutron excess, which is the difference between numbers of neutrons and protons in the nucleus.

The Russian team's desire to use an element they could not access was due to the nature of the calcium beam: the isotope of calcium used in the beam, calcium-48, has 20 protons and 28 neutrons; it is the lightest stable or near-stable nucleus with such a neutron excess.

There is general agreement that the next magic neutron number is 184, he said.

Neutron number is primarily of interest for nuclear properties.

In general, most actinide isotopes with an odd neutron number are fissile.

The neutron number, symbol N, is the number of neutrons in a nuclide.

Nuclides that have the same neutron number but a different proton number are called isotones.

Neutron numbers for which there are no stable isotones are 19, 21, 35, 39, 45, 61, 71, 89, 115, 123, and 127 or more.

The number of neutrons is the neutron number and determines the isotope of an element.

The nuclear structure group studies the structural evolution of the atomic nucleus as a function of proton and neutron number.

They are arranged with increasing atomic numbers from left to right and increasing neutron numbers from top to bottom.

Odd neutron number

Neutron number is rarely written explicitly in nuclide symbol notation, but appears as a subscript to the right of the element symbol.

Only 57 stable nuclides have an odd neutron number, compared to 200 with an even neutron number.

the Neutron number

The neutron count (neutron number) may then be derived by subtracting the number of protons (atomic number).

Atoms having the same atomic number Z but different neutron number N, and hence different atomic masses, are known as isotopes.

To visualize this scientists use a plot called the "Belt of Stability" which is a plot showing the stable combinations of proton/neutron numbers.

Because of their odd neutron numbers, the even-odd nuclides tend to have large neutron capture cross sections, due to the energy that results from neutron-pairing effects.

Because positron emission decreases proton number relative to neutron number, positron decay happens typically in large "proton-rich" radionuclides.

Chemical properties are primarily determined by proton number, which determines which chemical element the nuclide is a member of; neutron number has only a slight influence.

Nuclei are made up of Z protons (the atomic number), which are positively charged, and N neutrons (the neutron number), which are electrically neutral.

The number of neutrons, N, is known as the neutron number of the atom; thus, A = Z + N (these quantities are always whole numbers).

A set of nuclides with equal proton number (atomic number), i.e., of the same chemical element but different neutron numbers, are called isotopes of the element.

Nuclei which have neutron number and proton (atomic) numbers each equal to one of the magic numbers are called "double magic", and are especially stable against decay.

A given atomic nucleus, defined by its proton and neutron numbers, is a quantized system with a set of characteristic higher energy levels that it can occupy as a nuclear isomer.

These isotope tables show all of the known isotopes of the chemical elements, arranged with increasing atomic number from left to right and increasing neutron number from top to bottom.