Isotopes

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.

Gold is important because lot of people are going to lose their jobs because and if we run out of gold many people are going to be unemployed then there is going to be poverty in our country

The number of neutrons is the difference between the mass number and atomic number. For example U-235 means mass number equals 235. If we know that thge uranium atomic number is 92, then the number of neutrons for U-235 is 235-92 = 143 neutrons.

Beryllium-9 is a stable isotope.

Examples: 4120Ca, Ca-41, calcium-41; only the first is a scientific notation.

Each isotope has another type of decay but generally from californium are formed curium isotopes and an alpha particle.

The atomic number of the isotopes of an element is identical; the mass number is different.

n

The number of neutrons is different for each isotope.

One with a half-life close to the age of the object

ho

Tis is the isotope astatin-18.

The correct symbol is 2914Si.

You forgot to say that isotope is.

13

A "superscript" number before the symbol for the element - eg.

11C

12C

13C

14C

Denotes the four isotopes of the element Carbon.

The superscript number is a count of the total number of "nucleons" (protons and neutrons) in the atomic nucleus of the atom.

If you subtract the elements "atomic number" (which is the number of Protons that element has) from the Isotope (superscript) number you get the number of Neutrons in that isotope.

From this you will be able to deduce that isotopes of elements are caused by a variation in the number of neutrons in an atom of an element.

Carbon decay or carbon dating