Isotopes

an isotope is a different form of that element. They just have different mass numbers/ atomic mass. Therefore having the same characteristics of the atom except for an increased/decreased number of neutrons. Isotopes have the same atomic number as each other.

There are 33 protons and 41 neutrons in the atom arsenic.

An atom of Sodium weighs the same as 23 protons.

subtract the number of protons from the number of electrons.

The above answer does not answer the question!!

Radioactive substances in the environment can harm cells, damage DNA, and cause cancer. If we take gamma rays, they kill living cells upon contact as they have high penetration power. But this doesn't mean that they are totally dangerous and can't be used by living things. We have to see the level of radioactive isotopes used in order to say they are dangerous to others. Low levels of radioactive isotopes is used in a sample and it becomes a tracer by which to detect molecular changes. Melvin Calvin and his coworkers used Carbon 14 to detect all the various reactions that occur during the process of photosynthesis. Radioactive isotopes are being used largely in the medical field. The high level of radioactive isotopes (radiation) has been used to sterilize medicine and dental products for many years. Now, it can be used to sterilize the US mail and other packages to free them of possible pathogens such as anthrax spores. In addition to this, cancer treatment through radioisotopes to destroy only cancer cells, with little risk to the rest of the body is another important use of radioactive isotopes.

30,000

An isotope is an atom of a given element with a different mass. this means it must have a different number of neutrons, as changing the amount of protons would change the element. in short, an isotope is an atom with a special number of neutrons.

eg.

normal hydrogen-

1

H

1

deuterium (hydrogen with a neutron)

2

H

1

if you dont understand what im talking about just wiki it.

Isotopes are different forms of the element (they are therefore still elements).

For example - Carbon has 15 known isotopes, the stable ones being 12C and 13C.

All isotopes for the same element have the same number of protons, but a different number of neutrons. This means isotopes have different properties, such as different weights - but are all still the same element.

Isotopes are identified by their mass numbers.

Rutherford stated that electrons orbits the nucleus. Thus if the electrons were orbiting the nucleus then they must be accelerating due to the centripetal force acting on it. This proved to be a flaw, due to Maxwell theory that electrons accelerating produces EMR which in turns would mean the electrons would loose energy and crash into the nucleus leading to a unstable atom. Which is not the case.

Every atom, ion, and isotope of the same element will have the same number of protons. Hydrogen has one proton.

The chemical element is the same, only the number of neutrons is different.

Radioactivity stems from the instability of the nucleus of a given atom. Remember that in an atomic nucleus, protons and neutrons are held together with nuclear glue or binding energy (1H being the exception). Protons don't like each other to begin with. But under the most extraordinary conditions (like in a star), protons and neutrons can be forced together and fused (fusion) to create more complex nuclei. And in a supernova, elements heavier than iron (the heaviest "regular" element that a star makes during "normal" fusion) are created. In all this "creativity" and among all the products that result, some atomic nuclei that are formed aren't really happy with their arrangement. They are unstable, and at some time in the future they will spontaneously break apart. In some arrangements of nucleons (the particles that make up an atomic nucleus, the protons and neutrons), the ratio of the two types of particles, the ratio of protons to neutrons, is one that "strains" the combinational power that holds them together and other arrangements are possible. It is the number and type of nucleons that make up a nucleus that determines how stable it is. There are many stable nuclei. There are many combinations that are not possible - they will never form, they cannot form - and then there are the unstable nuclei. The different numbers of protons and neutrons that make up a nucleus make for a different "dynamic" in each atomic nucleus in which they are confined. Some are structures that will stay together, and in some of the structures formed, the nucleons can "shift" and break the structure of the nucleus, thereby allowing the nucleons to move to a lower energy level state. In radioactive decay, a shift in the nuclear structure and the release of a particle (or particles) and/or energy, allows the remaining nucleons to "rewrite" the terms and conditions of their "confinement" in the nucleus. This spontaneous transition is what radioactive decay is. The possibilities are why some nuclei are stable and some are not, and why some are more stable than others. It is impossible to say when any given unstable atom will decay, but over a large number of them, an "avarage" rate of decay can be quantified. That will allow us to know the half life of that radionuclide.

This is actually a very, very easy question to answer. Now, all atoms of the same element have the same number of protons. Otherwise, they wouldn't be the same element. For instance, if lead had one more proton, it would be bismuth, a non-toxic shiny metalloid. If it had one less, it would be thallium: a deadly poison which was only recently found. Lead has 82 protons.

When the number is given by an element name (e.g. lead-204), it is also showing the atom's nucleus' mass number. Natural lead contains lead-204, lead-206, lead-207, and lead-208. Each of these contains the same number of protons, but different numbers of neutrons, hence the mass difference. To find the number of neutrons, N, we subtract the number of protons, Z, from the mass number, A.

So, 204 - 82 = 122.

Lead-204 contains 122 neutrons.

A. Cobalt-60

-Castlearning.

Cobalt 60 is diagnosed into the patient due to the thyroid disorder, since cobalt 60 is known for its small radioactivity and short half life the patient would be treated then cured in approximately 25 days. Cobalt 60 is also unique since it is a selected radioisotope with a nuclide and decay mode of alpha(known to treat cancer and in this case thyroid disorder).

There are more than two isotopes....

if an isotope broke down the electrical energy would become balanced as the outer electron/s would be taken from the atom and the isotope would become like a noble gas. isotopes can be used for radiation aswell!

All have the same number of protons and electrons. They differ in the number of neutrons.

Radioactive phosphorus is used to treat abnormal cell proliferation, e.g., polycythemia (increase in red cells) and leukemia (increase in white cells). Radioactive iodine can be used in the diagnosis of thyroid function and in the treatment of hyperthyroidism. Since the iodine taken into the body concentrates in the thyroid gland, the radioaction can be confined to that organ. In research, radioactive isotopes as tracer agents make it possible to follow the action and reaction of organic and inorganic substances within the body, many of which could not be studied by any other means. They also help to ascertain the effects of radiation on the human organism (see radiation sickness ). In industry, radioactive isotopes are used for a number of purposes, including measuring the thickness of metal or plastic sheets by the amount of radiation they can stop, testing for corrosion or wear, and monitoring various processes.

Usually, the base element name followed by the mass number 'A', such as Carbon-12. You can also use the atomic symbol preceded by the mass number as a superscript. Some isotopes have special names and atomic symbols: Hydrogen-2: Deuterium (D) Hydrogen-3: Tritium (T) Helium-2: Diproton (Theoretical, not actually possible because of physics-y stuff)

Today are known approx. 3 000 radioactive isotopes, natural or artificial.

Atomic mass minus atomic number.

This is rather simplified but the atomic mass of an element is the total of all the protons, neutrons, and electrons in an atom. Each proton and neutron has an atomic mass of approximately 1 AMU (atomic mass units) while an electron has an atomic mass of about 0.0005 AMU. So, you don't need to worry about the electrons.

The atomic number of an element is simply the number of protons in the atom.

So, atomic mass (number of protons and neutrons) minus atomic number (number of protons) equals number of neutrons in an atom.

It is the neutron that makes changes in atomic nuclei to change them from one isotope to another. For any given element, that element will have a fixed number of protons. It is, after all, the number of protons that determine the elemental identity. But the number of neutrons in a given element can vary, and we use the term isotope to talk about which particular atom we're investigating. That is, we apply the term isotope to speak to an atom of a given element with a certain number of neutrons in its nucleus.

Isotopes have the same amount of protons but a different amount of neutrons.