Isotopes

A well-known method is C-14 dating. Carbon 14 is a radioactive isotope of carbon that has half-life of 5730 years, meaning that if you start with 1000 g of C-14, after 5730 years you would have 500 g left (the other half has decayed into N-14). C-14 is present in trace amounts in nature and living organisms would therefore maintain a near-constant level of C-14 in their bodies if they consume and interact with their surroundings. Dead organisms, however, can no longer eat and therefore cannot replenish their C-14 levels, and the C-14 levels would begin to fall due to decay. The amount of C-14 in a dead organism can be compared to a reference level to determine how much time has passed since it died by the formula T = -5730*log2(r/R) where T is the time since the organism's death, r is the remaining level of C-14, and R is the reference level of C-14.

An isotope like carbon-14 can be used to date dead organisms by counting the atoms with a machine.

They are all forms of a given chemical element. Example for sulfur:

- S6, S7, S7, S7, S12, S18, etc. are allotropes of sulfur; but the atomic number (number of protons and electrons) of the sulfur atoms is the same.

- sulfur has natural or artificial isotopes; but the atomic number (number of protons and electrons) of the sulfur isotopes is the same.

- an isomer is 43mS; but the atomic number (number of protons and electrons) of this sulfur isomer atoms is the same as for other isotopes.

The atomic number of uranium is 92; all the elements under uranium (under 92) were discovered.

Isotopes have the same number of protons as the element they represent, which determines the overall positive charge. They also have the same number of electrons as the neutral atom to maintain electrical neutrality, even though the number of neutrons may vary.

Half of a radioactive isotope is an atom that would have half of the atomic number of the radioactive isotope. In the case of radium-88 (88Ra), half of the radioactive isotope would be ruthenium-44 (44Ru). This assumes that the protons do not break down and that none are lost to additional reactions with other elements or compounds. Electrons can be lost along the radioactive chain, resulting in an ion of ruthenium rather than an electrically neutral atom.

The ideal properties of a radioactive isotope used as a medical tracer include a suitable half-life for the imaging procedure, emission of detectable radiation, minimal impact on biological tissues, and easy incorporation into the target compound. Additionally, it should decay by a mode that minimizes exposure to harmful radiation.

The abundance of an isotope is strongly correlated with its stability. Isotopes with longer half-lives are more abundant because they persist for a longer period of time without undergoing radioactive decay.

Uranium, atomic number 92, has several isotopes, and 238U is just one of them. Remember that a nucleon is one of the particles that make up the nucleus of an atom, and that means a proton or a neutron. In the case of this isotope of uranium, it has the 92 protons we'd expect for uranium, and it has 146 neutrons in its nucleus along with those protons. That's 238 necleons in the nucleus if 238U. Wikipedia has more information on uranium and on the nucleon, and links are provided.

all isotopes of uranium have 92 protons, that is what makes them uranium.

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. They are determined based on their atomic mass, which is the sum of protons and neutrons in the nucleus. Isotopes of an element have similar chemical properties but may have different physical properties, such as radioactive decay rates.

The isotope number refers to the total number of protons and neutrons in the nucleus of an atom of a specific element. It is used to distinguish between different isotopes of an element based on their atomic mass.

Uranium is a non metal element. Atomic number of it is 92.

A normal periodic table does not list isotopes, but elements, almost all of which occur in more than one isotope, and there is probably at least one radioactive isotope for every element. Instead of the periodic table, a table of nuclides is needed to answer this question.

In Beta- decay, a neutron is converted into a proton, and an electron and electron anti-neutrino are emitted. The Atomic Number goes up by one, and the Atomic Mass Number stays the same. For instance, 6C14 becomes 7N14 plus one electron and one electron anti-neutrino.

In Beta+ decay, a proton is converted into a neutron, and a positron and electron neutrino is emitted. The Atomic Number goes down by one, and the Atomic Mass Number stays the same. For instance, 6C11 becomes 5B11 plus one positron and one electron neutrino.

Isotopes that decay by Beta+ decay also tend to decay by Electron Capture, a process where an inner K shell electron is absorbed by the nucleus, changing a proton into a neutron and emitting a neutrino. The isotope conversion process would be the same as for Beta+, above.

In Alpha decay, a Helium nucleus (two protons and two neutrons) are emitted. The Atomic Number goes down by two, and the Atomic Mass Number goes down by four. For instance, 92U238 becomes 90Th234 plus one Helium nucleus

Tin is the element with the most stable isotopes, ten. Xenon is second with nine isotopes. Both Xenon and Cesium have 36 possible isotopes, but 27 of Xenon's and 35 of Cesium's isotopes are radioactive. This means that they decay over time and "shed" particles. Hydrogen has the smallest amount of isotopes, with three total and two stable isotopes.

It is an isotope that occurs in nature, and is not manmade. Isotopes, by the way, are atoms that have the same number of protons, but different number of neutrons. The atomic number is the same, but atomic weight (or mass) is different. For instance, Carbon can be Carbon 10, 11, 12, or 14. They are all carbon.

It is difficult to point to any one radioisotope and say that it has the shortest half-life. That's because there are a number of extremely unstable radionuclides that have been created in the high energy physics lab. These isotopes decay almost immediately, and the half-lives of some of some of them fall in the range of 10-3 seconds to 10-9 seconds or even shorter.

In reality, as the atoms gets decayed it gives out radiations such as alpha, beta and Gama. Alpha is a helium nucleus which is massive and beta is electron but fast moving and Gama is an electromagnetic radiation. So as the atom decays then its mass is likely to be reduced.

Rutherford's radioactive law deals with the number of atoms undecayed present at an instant 't' given in the form N = No e-lambda t

Here No is the total atoms present both decayed and undecayed in a sample.

N is the number undecayed present

lambda - the decay constant

t - the time elapsed

The mass number of an isotope tells you the total number of protons and neutrons in the nucleus of that atom. It is used to distinguish different isotopes of an element, as isotopes of the same element have the same number of protons but different numbers of neutrons.

Sodium does not have naturally occurring radioactive isotopes - as it has only 1 naturally occurring isotope, which has 11 protons and 12 neutrons, and is not radioactive. However, the 18 other known types of sodium isotopes are all radioactive, and sodium-22 (the most stable radioactive sodium isotope) has a half life of 2.6 years.

Regardless of element type, an isotope will have the same number of protons as the base element. The atomic mass changes due to the addition (or subtraction) of neutrons in the atom's nucleus. This in turn leads to an unstable atom and radiation.

A gas centrifuge is commonly used to separate isotopes of an element by exploiting the small mass differences between isotopes. By spinning at high speeds, the heavier isotopes migrate closer to the outer edge of the centrifuge, allowing for their separation.

Isotope chemistry is a branch of chemistry that studies the variations of elements based on the number of neutrons in their atomic nuclei, known as isotopes. Isotopes of the same element have the same number of protons but a different number of neutrons, leading to differences in atomic weight and properties. Isotope chemistry is important for understanding chemical reactions, studying geological processes, tracing the origin of compounds, and dating materials.