* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download File
Survey
Document related concepts
Nuclear fission wikipedia , lookup
Nuclear fission product wikipedia , lookup
Gamma spectroscopy wikipedia , lookup
Nuclear magnetic resonance spectroscopy of proteins wikipedia , lookup
Isotope analysis wikipedia , lookup
Ionizing radiation wikipedia , lookup
Background radiation wikipedia , lookup
Technetium-99m wikipedia , lookup
Nuclear binding energy wikipedia , lookup
Isotopic labeling wikipedia , lookup
Radioactive decay wikipedia , lookup
Nuclear transmutation wikipedia , lookup
Transcript
Isotopes and Nuclear Chemistry We’ve learned that each element has its own unique atom which is made up of a specific number of protons. The number of protons determines the atomic number of the element. Each atom also has the same number of electrons as protons. Isotopes The three most stable isotopes of Hydrogen: are atoms that have the same number of Protium, the most common isotope of hydrogen, consists protons and electrons, but a different of one proton and one electron. ... number of neutrons. Changing the number A deuterium atom contains one proton, one neutron, and one electron. of neutrons does not affect the chemistry Tritium atom contains one proton, two neutrons and one of the element. It does, however, change electron. the mass of the element. Isotopes are identified by their mass, which is the total number of protons and neutrons. There are two ways that isotopes are generally written. They both use the mass of the atom where mass = (number of protons + number of neutrons). The first way is to put the mass as a superscript before the symbol of the element: 4He, 14C, 235U The other way is to write out the element and write the mass after a dash next to the element's name: Helium-4, Carbon-14, Uranium-238. Stable and Unstable Isotopes Some isotopes are stable and happy. These are the elements that we see around us and find in nature. Stable atoms generally have the same number of protons and neutrons. Some accommodate one to two additional neutrons in the nucleus and remain stable. However, when the nucleus of an atom possesses either too many or too few neutrons compared to the number of protons it becomes unstable. You see, positive charges repel each other – but the strong force overcomes this electric force at small distances. The strong force is what allows neutrons to “act like glue” keeping the right amount of spacing between the positively-charged protons, and keep them from pushing each other out of the nucleus. When there are too few neutrons, the protons are able to push each other from the nucleus. When there is too many neutrons, this causes too much spacing in between protons and the electric force overcomes the strong force. Unstable isotopes also known as radioisotopes emit energy in the form of radiation to restore the balance of protons to neutrons in the nucleus, this is known as radioactive decay. The unstable isotope will decay over time and eventually it will turn into another isotope or element. Different Types of Radioactivity There are three main types of radiation or radioactive decay depending on the isotope: alpha decay, beta decay and gamma decay. Alpha decay - Alpha decay is caused when there are too many protons in a nucleus. In this case the element will emit radiation in the form of positively charged particles called alpha particles. Alpha particles are considered not dangerous as it can be stopped by a sheet of paper Beta decay - Beta decay is caused when there are too many neutrons in a nucleus. In this case the element will emit radiation in the form of negatively charged particles called beta particles. Beta decay is moderately dangerous and can penetrate superficial layers of skin tissue. Gamma decay - Gamma decay occurs when there is too much energy in the nucleus. In this case gamma particles with no overall charge are emitted from the element. Gamma rays are the most dangerous, these rays have the most penetrating power. These extremely high energy photons can travel through most forms of matter because they have no mass. It takes several inches of lead -- or several feet of concrete -- to effectively block gamma rays. If you're exposed to gamma rays, they pass through your entire body, affecting all of your tissues from your skin to the marrow of your bones. What is the half-life of an isotope? The half-life of an isotope is the time on average that it takes for half of the atoms in a sample to decay. For example, the half-life of Carbon-14 is 5730 years. This means that if you have a sample of Carbon-14 with 1,000 atoms, 500 of these atoms are expected to decay over the course of 5730 years. Some of the atoms may decay right away, while others will not decay for many thousands more years. The thing to remember about half-life is that it is a probability. In the example above, 500 atoms are "expected" to decay. This is not a guarantee for one specific sample. It is just what will happen on average over the course of billions and billions of atoms. Why is radiation dangerous? Radiation can alter the structure of cells in our bodies causing mutations which can produce cancer. The more radiation exposure, the more dangerous it is. Is some radiation good? Despite the risks, a number of good ways that science has used radiation include X-rays, medicine, carbon dating, energy generation, and to kill germs.