Current position : HomeNews Center PRODUCTS

Introduction to isotope

Isotopes are different number of neutrons have the same number of protons, the different isotopes of the same element of each Isotope.

An isotope is one of two or more atoms of the same chemical element with the same atomic number, occupying the same place on the periodic table, having almost the same chemical behavior but different atomic weights or mass Numbers, resulting in differences in mass spectral behavior, radioactive transformation, and physical properties (such as diffusion power in the gaseous state). The isotopic representation is marked with the mass number (protons + neutrons) in the upper left corner of the element symbol, and the number of protons in the lower left corner. So for example, carbon-14, we're going to use 14C instead of C-14.

Many elements in nature have isotopes. Some isotopes are natural, some are manufactured, some are radioactive and some are not.

Although isotopes of the same element have different mass Numbers, their chemical properties are basically the same (e.g., chemical reactions and ion formation), and their physical properties are different (e.g., melting and boiling points). In nature, each isotope has a certain percentage of atoms.

The isotopes that exist naturally in nature are called natural isotopes, and the synthetic isotopes are called artificial isotopes. If the isotope is radioactive, it is called a radioisotope. Each element has a radioactive isotope. Some radioactive isotopes are found in nature, while others are created by bombarding stable nuclei with nuclear particles such as protons, A particles, or neutrons.

Email Message TOP