Isotopes

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).

Isotopes have various benefits such as their use in medical imaging for diagnostics, tracing the origin of elements in scientific research, and serving as tracers in environmental studies to track the movement of substances. Isotopes also have applications in dating archaeological artifacts and monitoring geological processes.

Any given element has a specific number of protons, but the number of neutrons varies; an isotope has a specified number of nucleons (protons plus neutrons). Hydrogen 1 has no neutrons, hydrogen 2 (also known as deuterium) has one neutron, hydrogen 3 (or tritium) has two neutrons.

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No.IsotopeRelative atomic mass 1.217U217,024 368 791 ± 0,000 093 262 2.218U 218,023 535 671 ± 0,000 032 763 3.219U219,024 919 160 ± 0,000 060 946 4.*220U220,024 723# ± 0,000 215# 5.221U221,026 399# ± 0,000 110# 6.222U222,026 086# ± 0,000 108# 7.223U223,027 738 600 ± 0,000 076 347 8.224U224,027 604 778 ± 0,000 027 176 9.225U225,029 390 717 ± 0,000 012 42810.226U226,029 338 702 ± 0,000 013 99911.227U227,031 156 367 ± 0,000 018 10412.228U228,031 374 006 ± 0,000 016 05113.229U229,033 505 939 ± 0,000 006 39614.230U230,033 939 784 ± 0,000 005 11015.231U231,036 293 704 ± 0,000 003 24216.232U232,037 156 152 ± 0,000 002 36517.233U233,039 635 207 ± 0,000 002 90418. **234U234,040 952 088 ± 0,000 001 960

(natural isotope)19. **235U235,043 929 918 ± 0,000 001 957

(natural isotope)20. 235mU "21.236U236,045 568 006 ± 0,000 001 96022.237U237,048 730 184 ± 0,000 002 01923. **238U238,050 788 247 ± 0,000 002 044

(natural isotope)24. 238m1U " 25. 238m2U "26.239U239,054 293 299 ± 0,000 002 05227.240U240,056 591 988 ± 0,000 005 53328.241U241,060 330# ± 0,000 320#29.242U242,062 931# ± 0,000 215#30. ***243U243,067 36 (not surely identified)31. ***244U244,069 95 (not surely identified)

Studies of metabolism, drug utilization, and other reactions in living organisms can be done with stable isotopes such as 13C, 15N, 18O, and 2H. Molecular compounds are "spiked" with these isotopes, and the metabolizedhttp://www.answers.com/topic/metabolize products are analyzed by using a mass spectrometer http://www.answers.com/topic/spectrometerto measure the altered isotopic ratios. Also, isotopes that are unstable will emit radiation, which can be alpha particles , beta particles or gamma radiation. The radiation can be used to treat cancer in the case of cobalt-60, which emits gamma radiation. Cancerous cell are destroyed by directing a controlled beam of gamma radiation at the cells.

Every element provides a couple of isotopes which are of very different use.

For example, carbon has a radioactive isotope (14C).

You can, for example, grow bacteria on a modified substrate which contains the radioactive isotope instead of normal carbon.

The resulting generation will inherit carbon in it's cellular substance which is not only heavier (14 instead of 12 nucleons) but also emits measurable radiation.

These features can be used to reconstruate cellular growth processes, as well as in other organisms bodily functions and development.

Hydrogen has three isotopes, one of them deuterium (features one neutron), which makes it twice as heavy as normal hydrogen. D2O water is therefore much heavier than normal H2O water. As water is widely used in most metabolic pathways, "marking" with D2O can let you find the isotope in different parts of the organism and it's products. For example, a plant can be fed with D2O, afterwards you can see how much of it was metabolized and used for building biological substance, and how much of it was transpirated through the leaves.

They do not combine with or interact with most other elements or compounds. ... radioactive. No radioactive isotope of platinum has any commercial application.

Copper has natural isotopes of 63,67.

And other isotopes are known at least from 58 through 70. But these are unstable.

There are several isotopes of iron, the most frequent is Fe56 (92 percent). Suggest you look up Wikipedia for Iron. I do not understand your use of word 'resonante'. If you mean 'resonate' I still don't understand what your query really is.

Isotopes are known to exist because they are variants of a particular chemical element with the same number of protons but different numbers of neutrons, resulting in different atomic masses. These variations can be detected through techniques like mass spectrometry and nuclear magnetic resonance. The existence of isotopes has been confirmed through experimental evidence and scientific research.

Yes - they have many applications. One isotope of an element can be very stable and have one set of uses while another is unstable (radioactive) and have a completely different set of applications. Let me give 3 examples:

1. 1 proton is hydrogen. 1 p and 1 n is an isotope of hydrogen that is called deuterium (note, only hydrogen isotopes have their own names). Deuterium is widely used in "deuterated" compounds because how it interacts with a magnetic field is different than hydrogen. A 3rd isotope of hydrogen is called tritium - it is radioactive and in very low quantities in water.

2. Tc is a transition metal but not found in the earths crust. It is made in a reactor. Tc-99 (Technetium) is used in different types of nuclear medicine. Tc-98 or Tc-100 would not work for the same applications.

3. Uranium has a number of isotopes. Two of the most well known are U-25 and U-238. They different by 3 neutrons (all uranium has 92 protons). U-235 is very radioactive and is used in bombs and nuclear power plants. U-238 is more stable and is used in the tips of missiles that pierce armor. Uranium is very dense.

Remember - isotopes (i.e. H, D, T) all have the same number of protons but different number of neutrons - and the number of neutrons impacts nuclear stability.

Helium 3 and helium 4 are naturally occurring isotopes 5 thru 10 are exotic isotopes.

Radioisotopes emit radiations and although most of the time radiation is bad for your body cause it can encourage mutation and damage body cells but sometimes if used in controlled condition they can kill cancerous cells which is good

Isotopes must have the same atomic number, which is the number of protons. The atomic mass, which is the total number of protons and neutrons, varies for the different isotopes.

so it should have different mass numbers..