Isotopes

All isotopes of an element have the same number of protons, otherwise they would not be the same element. What varies is the number of neutrons, they can be more or less than in the stable isotope(s) of the element.

Chlorine is a non metal element. Mass number of it is 35.

Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, with two neutrons.

If you want to refer to a certain isotope, you write it like this: AXZ. Here X is the chemical symbol for the element, Z is the atomic number, and A is the number of neutrons and protons combined, called the mass number. For instance, ordinary hydrogen is written 1H1, deuterium is 2H1, and tritium is 3H1.

there are "preferred" combinations of neutrons and protons, at which the forces holding nuclei together seem to balance best. Light elements tend to have about as many neutrons as protons; heavy elements apparently need more neutrons than protons in order to stick together. Atoms with a few too many neutrons, or not quite enough, can sometimes exist for a while, but they're unstable.

No, there is only one possible configuration for a compound with the formula NH3.

An isomer is a substance for which there are more than one configurations for the same chemical formula.

Strontium-88 is an isotope of strontium that has 52 neutrons. It has an atomic number of 38, therefore the total number of neutrons (52) is obtained by subtracting the atomic number from the mass number.

Smoke detectors, the older ones, used radiation to detect the smoke.

Soil density testers use radiation. A lot of medical instruments use it--X-ray machines and radiation machines for cancer treatment.

The correct conventional representation of an isotope of copper includes the element symbol "Cu" followed by the atomic number (number of protons) which is 29. Isotopes are represented by adding the mass number (sum of protons and neutrons) as a superscript before the element symbol. One example is copper-63, written as ^63Cu.

Isotopes can be distinguished by a mass spectrometer based on their differing atomic masses. The mass spectrometer ionizes a sample, separates the ions based on their mass-to-charge ratio, and then detects the abundance of each ion. The relative abundance of each isotope gives a unique mass spectrum that can be used to identify and quantify isotopes in a sample.

The diagnostic test that injects radioactive isotopes into the bloodstream is called a nuclear medicine scan. This procedure allows healthcare providers to visualize and assess the function of specific organs and tissues in the body. The radioactive isotopes emit gamma rays that are detected by a special camera to create images for analysis.

Carbon-14 dating is commonly used to date ancient artifacts such as fossils. This method relies on the half-life of carbon-14, which isotope decays at a known rate, to estimate the age of the artifact by measuring the remaining carbon-14 in it.

Certain radioactive isotopes have an affinity or liking for certain body cells. Thus iodide given to a patient will bunch up and help machines "visualize" the thyroid so that a gland expert doctor can determine if there is something wrong. A drink called "Go Litely" can help doctors "see" what might be wrong with an intestinal tract. Merely diagnostic or fact-finding.

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.