Isotopes

1. Carbon-14
2. Hydrogen-2 (Deuterium)
3. Uranium-235
4. Oxygen-18
5. Technetium-99
6. Potassium-40
7. Iodine-131
8. Tritium
9. Radon-222
10. Lead-206

The mass number of plutonium isotopes can vary depending on the specific isotope. Common plutonium isotopes include plutonium-238, plutonium-239, and plutonium-240, with mass numbers of 238, 239, and 240 respectively.

One example of isotopes is carbon-12 (12C) and carbon-14 (14C). These isotopes have the same number of protons, but different numbers of neutrons. Carbon-12 is stable and commonly found in nature, while carbon-14 is radioactive and used for carbon dating.

Every individual atom is an isotope - it has a whole number of neutrons and a whole number of protons in its nucleus. The word isotope generally refers to a quantity of some material, where every atom in that portion has the same whole numbers as described above.

An isotope depends on the number of neutrons in the atom. If you consider various isotopes of a particular element, the proton number does not change.

Examples:

Carbon 12: 6n, 6p

Carbon 13: 7n, 6p

Hydrogen 1 (protium): 1p

Hydrogen 2 (deuterium): 1n, 1p

isotopes are nucleus having same atomic no but different mass no .hydrogen, duterium,tritium are examples

isodiaphers are the nucleus having same difference in no o f protons and no of neutrons .

isotopes are nucleus having same atomic no but different mass no .hydrogen, duterium,tritium are examples

isodiaphers are the nucleus having same difference in no o f protons and no of neutrons .

isotopes are nucleus having same atomic no but different mass no .hydrogen, duterium,tritium are examples

isodiaphers are the nucleus having same difference in no o f protons and no of neutrons .

Isotopes typically have neutral electrical charge, as they have the same number of protons and electrons. The electrical charge of an isotope can change if it gains or loses electrons, resulting in a positively or negatively charged ion.

A stable isotope is an isotope that does not undergo radioactive decay, meaning its nucleus is stable and does not change over time. These isotopes have a constant number of protons and neutrons, making them suitable for use in scientific studies like tracing biological processes or determining the age of rocks. Examples include carbon-12, oxygen-16, and nitrogen-14.

Isotopes are atoms that have the same number of protons and electrons. They have the same atomic number on the periodic table but they have a different number of neutrons and so they have different mass. Isotopes of the same element can have different chemical properties.

Radium has today 33 isotopes and 12 nuclear isomers.

Yes. Yes it does.


The element calcium has a known 24 Stable Isotopes. For more information, ask google

Potassium has three naturally occurring isotopes: potassium-39, potassium-40, and potassium-41. The most common isotope is potassium-39, which makes up about 93% of naturally occurring potassium.

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

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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.