Isotopes

Because the isotopes do not appear in equal amounts.

This is hardly surprising since many isotopes experience radioactive decay and change to other elements after decay while stable isotopes persist - thus stable isotopes will usually dominate as the most common isotopes for individual elements with those with the longest half-lifes being more common than those with shorter half-lifes. Of course when you get into the heaviest elements there don't seem to be any stable isotopes so those with longest half life dominate.

Yes. There are isotopes of elements that are simply not found anywhere in the universe (and even if they did exist momentarily, their lifetime is so short that in the next moment they would have decayed into a different more stable isotope).

Some applications of americium are:

- smoke detectors

- source of neutrons, alpha particles, gamma rays

- nuclear densimeters

- calibration of gamma rays spectrometers

- initial reactant for nuclear reactions to obtain heavier isotopes

For score-keeping purposes, every defensive position is assigned a number. This number has nothing to do with the number on the back of a player's uniform. The scoring numbers are: 1 -- pitcher 2 -- catcher 3 -- first base 4 -- second base 5 -- third base 6 -- shortstop 7 -- left field 8 -- center field 9 -- right field so a scoredcard reading, for example, "E-6", would mean an error on the shortstop.

It sounds like they are elements on the periodic table of elements.

If you mean which isotope, then carbon-12 is the most abundant. If you mean where does the carbon come from, then it's atmospheric carbon dioxide for plants, and food for animals.

Pretty much any element is identified by its atomic number or number of protons; in the case of beryllium it has four of them in its nucleus. It's somewhat a matter of convention that it is beryllium by definition so long as it has those four protons; any element might be in a different oxidation state having gained or lost electrons, or be a different isotope by varying the number of neutrons, but the atomic number or number of protons is used to identify elements.

Radioactive minerals are unstable and emit radiation at a constant rate. They also have half lives and lose energy overtime. Nonradioactive minerals are stable, and by there own are incapable of emitting energy.

Example with the istope 235 of uranium:

- 235

92U (recommended) or

- U-235

The atomic particles of an isotope are the proton, electron and neutron

isotopes are atoms of an element with different #'s of neutrons (these are electrically neutral particles which change the weight of the atom); hydrogen has three isotopes; all three atoms have 1 proton and 1 electron but vary from no neutrons(the most common type of atom or isotope) to atoms with 1 neutron and 2 neutrons.

The nuclear reaction is: 242Cm + 4He = 245Cf + n

Same number of protons, different number of neutrons.

Oxygen consists of three stable isotopes: 16O, 17O, and 18O

omarion is currently dating rhinna

The most common isotope of osmium is 192 Os. All osmium isotopes contain 76 electrons.

Alloys

This is the gamma radiation.

Plutonium-238 is an alpha emitter.

The belt of stability is a graph which help to identify unstable isotopes.
See also this link.

Isotopes have a different number of neutrons but the number of protons and electrons is the same.

The answer is the atomic weight of the original element: It's the number on the top left of each element square of the Periodic Table.

An isotope is not really related to the number of electrons, but rather it is determined by the number of neutrons.

Isotopes of an atom does retain the properties of the atom. This is discrete in units of matter.