Isotopes

Isotopes were not invented - they exist in nature. They were discovered when the atomic mass of Chlorine was measured at 35.5

istopes was discovered by joseph john and francis aston both discovered isotopes

-------------------

The first hypothesis on isotopes is from Frederick Soddy (1912); the practical confirmation is attributed to J. J. Thomson (1913).

An isotope is an element that has the same number of protons and a different number of neutrons, whereas a nuclide is a specifically defined isotope.

Quite literally, they refer to the exact same atom, but the difference lies in the definition. Nuclides are defined by many different aspects, such as half life, mode of decay, percent abundance, and so on. The Chart of the Nuclides is a very extensive reference for the characteristics of over 3000 different isotopes.

The term isotope is merely a way of differentiating between an atom that is the same element (same number of protons) but has varying numbers of neutrons.

The nucleus of an isotope with a specific atomic mass and number contains protons and neutrons. The number of protons determines the element, while the sum of protons and neutrons gives the atomic mass. The neutrons in the nucleus help stabilize it by balancing the repulsion between positively charged protons.

Typically, a nuclear bomb would use plutonium-239 as the primary isotope for fission. Plutonium-239 is preferred due to its high fissionability and ease of obtaining through processing in nuclear reactors. Small amounts of other plutonium isotopes, such as plutonium-240, may also be present due to the manufacturing process, but the majority would be plutonium-239.

Isotopes are atoms that have the same atomic number or number of portions, but a different number of neutrons and therefore a different atomic mass, they also buttrape orphans in africa.

Since isotopes are nearly chemically identical, the use of chemical processes to separate isotopes is impractical, but it is used to separate deuterium from normal hydrogen. The extreme mass differences of deuterium and hydrogen (being twice its mass), allows for a more noticeable chemical difference: when chemical equilibrium is established with water (H2O or HDO, with one deuterium replacing the hydrogen) with pure light hydrogen gas, there is 3 to 4 times more deuterium in the liquid compound than in the gas. Thus, this difference can be used to separate the heavier deuterium from light hydrogen.

But the use of chemical methods would only work if the mass of the isotopes are immensely different, which only occurs with lighter elements.

To separate other isotopes, the physical properties of the compounds are used since they directly relate with the slight difference in masses.

The most common example of separation by physical properties is the separation by effusion, which is commonly used to separate uranium-235 (used in weapons and power generation) and uranium-238. These mass differences result in a different effusion rate as predicted by the Kinetic Molecular Theory, thus the lighter U-235 effuses faster than U-238, and the process being repeated many times nearly pure U-235 results.

Isotopes of elements are atoms with the same number of protons but different numbers of neutrons. This causes isotopes of the same element to have different atomic masses. Isotopes can be stable or unstable, with unstable isotopes undergoing radioactive decay.

All isotopes of an element have the same number of protons. When they are not ionic, they have the same number of electrons. And, for all practical purposes, they behave identically as chemicals. share most of the same physical properties, and chemical properties. They have different number of neutrons.

Silver hastwo stable isotopes107Ag and 109Ag. 107Ag is the more abundant stable isotope. 28 radioisotopes have been characterized.

Isotopes are atoms of the same element with the same number of protons but different number of neutrons. Radioisotopes are isotopes that are unstable and undergo radioactive decay, emitting radiation in the process. They are commonly used in medicine, industry, and research.

If two atoms are isotopes, it means they have the same number of protons but different numbers of neutrons. Thus, they have the same atomic numbers, but different atomic masses.

Isotopes and isobars are very different. Isotopes are different atoms of the same element that have varying atomic masses (such as U-237 and U-235; i.e. they differ only in the number of neutrons contained within the nucleus), while isobars are a computed line through a variable region that all have the same value (think about the lines on a meteorological map). The specific line around a low pressure system where the pressure at every point on the line is the same atmospheric pressure is an isobar.

Isobars are nuclei of different elements having the same mass number but different atomic number.

No, fructose and glucose are not isotopes. Isotopes are variants of a chemical element with the same number of protons but different numbers of neutrons. Fructose and glucose are different carbohydrates with distinct molecular structures.

There are many elements that have only one naturally occurring isotope. When you get to transuranic elements the elements all have no naturally occurring isotopes. But all elements have isotopes, they just have to be created, maybe in a nuclear reactor or particle accelerator or a supernova explosion.

No, J.J. Thomson did not discover isotopes. Isotopes were discovered by Frederick Soddy and John William Strutt in the early 20th century. J.J. Thomson is known for his discovery of the electron.

1. Sodium has 20 isotopes and 2 isomers.

2. Only the isotope 23Na is stable.

3. The stable isotope 23Na and the radioactive isotopes 22Na and 24Na (these isotopes exist in traces) are natural isotopes.

Isotopes are atoms of the same element with different numbers of neutrons, resulting in different atomic masses. They have the same number of protons and electrons, giving them the same chemical properties. Isotopes can be used in various applications, such as radiometric dating and nuclear medicine.

Some examples of isotopes are carbon-12 (6 protons, 6 neutrons), carbon-13 (6 protons, 7 neutrons), and carbon-14 (6 protons, 8 neutrons). These isotopes have the same number of protons but different numbers of neutrons.

Xenon has nine naturally occurring isotopes: Xe-124, Xe-126, Xe-128, Xe-129, Xe-130, Xe-131, Xe-132, Xe-134, and Xe-136.

A half-life is the time taken for the radioactivity of a material to fall to half its original value. A material can undergo infinite half-lives because each time it falls to half the next half-life falls to half of that half:

No half-lives have elapsed when radioactivity is at the original amount; 1/1.

1 half-life is when radioactivity is at 1/2

2 half-lives is when radioactivity is at 1/4.

3 half-lives is when radioactivity is at 1/8.

4 half-lives is when radioactivity is at 1/16.

And so on.

The natural percent abundance of the heavier isotope of gallium, gallium-71, is approximately 39.892%.

look here:

http://chiralpublishing.com/Bishop_Isotope_Notation.htm

If you are using mastering chemistry make sure you are using the correct insert. It should not look like a division problem (no line between the numbers).