Isotopes

Yes, radioactive isotopes are largely used for the treatment of cancer.

An isotope has same number of protons but a different number of neutrons as the original element in the atomic nucleus; it has the same atomic number as the element which isn't an isotope, but will have a different mass number.

-atomic number

During some radioactive explosion/exposure the atoms combine and if they stay stable they from with extra amounts of protons. Isotopes are when two or more elements have the same number of protons, but different number of neutrons.

When two molecules have different configurations but the same atomic composition the two molecules cannot be said to have the same physio-chemical properties. In fact, a simple rearrangement, even with identical chemical formulas, can drastically change the properties of a substance.

Neon isotopes can be used in dating meteoric rock and to investigate the creation of some isotopes in space.

The two fundamental differences between two isotopes are its mass and its spin. This is because there is a difference in the number of neutrons in the atom, and neutrons have a both mass and spin (1.67493x10-27kg and 1/2, respectively).

This, in turn, causes a handful of changes, including stability, appearance in nuclear magnetic resonance spectra, frequency of intranuclear vibrations, and radioactivity.

Yes, all elements have at least one radioactive isotope. Hydrogen has two isotopes, Deuterium and Tritium. H3 has a half life of 12.3 years.

Not all isotopes are radioactive. About half way up the atomic mass table, Tin appears to have the greatest number of stable isotopes - ten out of about 124 isotopes in all.

Magnesium has an atomic number of 12, so there are 12 protons in any atom of this element. The number of protons do not change if it is an isotope of an element.

Radium has 7 "shells" and has 88 protons and 138 neutrons. it also has 88 electrons.

the electrons are arranged like:

2 (1st shell)

8(2nd)

18(3rd)

32(4th)

18(5th)

8(6th)

2(7th)

12C is a carbon atom with 6 neutrons, 13C has 7 neutrons. Each isotope contains 6 protons, so 6+6=12 and 6+7=13.

Iodine (I) has 53 protons and 74 neutrons.

Carbon-14 and Uranium-235, to name two.

You add or remove one or more neutrons from each atom.

The process is called decay, or sometimes nuclear decay. A link can be found below.

Half the original amount.

Go to the periodic table and look up the atomic number of iron (Fe). The atomic number of iron is equal to the number of protons in iron. Mass number is the number of protons plus the number of neutrons so add up the two values.

Rubidium has two natural isotopes (85Rb and 87Rb) and 30 artificial isotopes.

No, it is a compound. If you read the definitions of isotope and compounds, the difference should become quite clear.

No, it is a compound. If you read the definitions of isotope and compounds, the difference should become quite clear.

No, it is a compound. If you read the definitions of isotope and compounds, the difference should become quite clear.

No, it is a compound. If you read the definitions of isotope and compounds, the difference should become quite clear.

Carbon-14.

Interestingly, there are natural ways that differences in the abundance of isotopes can arise.

The obvious example is carbon, where the different abundances of carbon 14 are used to date archeological artifacts.

For most elements, the isotopes were determined billions of years ago when the Earth condensed out of the swirl of matter around the newly formed Sun, so the mix of isotopes then was what it is now and things were pretty well mixed then. Even if not, the process by which the isotopes were made is pretty much the same all over the universe so different stuff combined from different parts of the universe should still have about the same isotopic mix. (See related link to Nucleosynthesis.)

There are a couple of things that can cause the isotopic ratios to change. In the case of carbon, the cause is bombardment of the atmosphere by cosmic rays with enough energy to cause nuclear reactions. Carbon 14 and Iodine 129 are produced by this process and they are termed "cosmogenic nuclei." So, objects with old carbon, not having exchanged carbon with the atmosphere will have less carbon 14 because whatever was there decayed and was not replenished.

There is also the process of natural radioactive decay of things like uranium-235, uranium-238, and thorium-232 produce various elements. These elements will not necessarily have the same isotopic composition as the element that was naturally occurring at the time the Earth was created.

Of course, one might ask if materials that come to Earth from outer space, e.g. meteorites, count as "naturally occurring." One would not expect them to have the same isotopic composition exactly as what is on Earth originally.

There are other differences, such as the rate of diffusion that are different for different isotopes. A molecule of water with a deuterium diffuses at a different rate than one just a tiny bit lighter. Such processes may lead to depletion of lighter isotopes in samples.

Those are a few obvious mechanisms that may create different abundances of isotopes in different samples of the same element, but there are surely more. This answer has not given any indication of which might be the most common mechanisms, except for carbon 14.

isotopes of a given element differ in the number of neutrons they have.

Oxygen-18 has 8 electrons and protons; the number of neutrons is 10.

Hydrogen-1 isotopes have one proton and no neutrons. Hydrogen-2 isotopes have one proton and one neutron.