The configuration of these electrons follows from the principles of quantum mechanics. The chemical properties of the atom are determined by the number of protons, in fact, by number and arrangement of electrons. Knowledge of the electron configuration of different atoms is useful in understanding the structure of the periodic table of elements.Įvery solid, liquid, gas, and plasma is composed of neutral or ionized atoms. The electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals. The periodic table is a tabular display of the chemical elements organized on the basis of their atomic numbers, electron configurations, and chemical properties. It should be noted that all of these decay pathways may be accompanied by the subsequent emission of gamma radiation. Many other rare types of decay, such as spontaneous fission or neutron emission are known. Unstable isotopes decay through various radioactive decay pathways, most commonly alpha decay, beta decay, or electron capture. If there are too many or too few neutrons for a given number of protons, the resulting nucleus is not stable and it undergoes radioactive decay. As a result, as the number of protons increases, an increasing ratio of neutrons to protons is needed to form a stable nucleus. Neutrons stabilize the nucleus, because they attract each other and protons, which helps offset the electrical repulsion between protons. There are only certain combinations of neutrons and protons, which forms stable nuclei. These two forces compete, leading to various stability of nuclei. The neutron has a mean square radius of about 0.8×10−15 m, or 0.8 fm, and it is a spin-½ fermion.Ītomic nuclei consist of protons and neutrons, which attract each other through the nuclear force, while protons repel each other via the electric force due to their positive charge. It has no electric charge and a rest mass equal to 1.67493 × 10−27 kg-marginally greater than that of the proton but nearly 1839 times greater than that of the electron. In the universe, neutrons are abundant, making up more than half of all visible matter. 121Sb is the most common isotope, having a natural abundance of approximately 57%.Īntimony-121 is composed of 51 protons, 70 neutrons, and 51 electrons.Īntimony-123 is composed of 51 protons, 72 neutrons, and 51 electrons.Ī neutron is one of the subatomic particles that make up matter. Main Isotopes of AntimonyĪntimony occurs in 2 natural isotopes: 121Sb and 123Sb. Mass numbers of typical isotopes of Antimony are 121, 123. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.įor stable elements, there is usually a variety of stable isotopes. Neutron number plus atomic number equals atomic mass number: N+Z=A. The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10 -19 coulombs. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. Antimony is a chemical element with atomic number 51 which means there are 51 protons in its nucleus.
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