Isotopes

Hafnium is a rare element with rare applications:

- component of control rods for nuclear reactors

- component of some alloys

- getter in lamps and tubes

- electrode for plasma cutters

- hafnium dioxide was recently used as an electrical insulator in microprocessors

- hafnium carbide has a very great point of melting (the most refractory compound known today)

- possible use in weapons (USA)

The definitive answer is 'Isotopes have a different numbers of neutrons'.

Taking hydrogen as an example. Iy has three isotopes.

#1 ; protium ; 1 proto and 1 electron 0 neutrons (The commonest isotope)

#2 ; deuterium ; 1 proton , 1 electrons 1 neutron. (Used to make ;heavy water')

#3 ; tritium ; 1 proton , 1 electron, and 2(TWO) neutrons. (Very rare and radio-active).

Isotopes are atoms of the same chemical element that have different masses due to differing numbers of protons in the nucleus. These are all averaged out to give the "normal" atomic mass that's on the periodic table eg: Cl = 35.5 its abundancy is 75% Cl35 and 25% Cl37.

Unstable isotopes can spontaneously undergo changes, transforming them into other isotopes of the same or of different elements. Stable isotopes do not. Some isotopes are very unstable and exist for less than a second; others can exist for billions of years but still be unstable. Many elements consist of more than one isotope. One or more of these isotopes may be unstable.

In isotopes of an element, the nucleus contains different numbers of neutrons while the number of protons remains the same and determines how the atom behaves chemically. There are several types of instability (too few neutrons, too many neutrons) and several types of decay.

Technetium, Promethium, and all elements heavier then Bismuth.

An isotope is unstable because isotopes are only atoms with a change in the number of neutrons. For an atom to become stable, it should have the maximum number of electrons it can have in its outer most shell, but since isotopes only deal with neutrons, this problem is not dealt with in this case. When there is a change in the number of electrons, it is called a ion. It can become stable through ionic bonding, covalent bonding and metallic bonding, depending on the two elements that are meant to bond.

they have different numbers of electrons

I hope it works bye :)

No, carbon-14 is continually being produced in the atmosphere by cosmic rays. While individual carbon-14 atoms will decay over time, new ones are constantly being created. This creates a balance in the amount of carbon-14 in nature.

This is the time in which half the the atoms was disintegrated.

there are many isotopes of hydrogen. they are:-hydrogen -1 protium. hydrogeen - 2 deuterium.hydrogen - 3 tritium. hydrogen - 4 hydrogen - 5 hydrogen - 6 hydrogen - 7

In the nucleus of molybdenum, a neutron undergoes beta decay, transforming into a proton and emitting an electron and an antineutrino. This process converts the element into technetium by increasing the atomic number by one and maintaining the same mass number.

Isotopes (of hydrogen) differ in the number of neutrons in the nucleus of the atoms.

The formula is Atomic Mass (rounded to the nearest whole number) minus the Atomic Number.

This works because Protons and Neutrons have virtually the same mass, and electrons virtually none. As well as the Atomic Number being equal to the amount of Protons.

Essentially:

Protons + Neutrons - Protons = Neutrons. Basic Prealgebra.

So to find the amount of Neutrons in Erbium:

Erbium's Atomic Mass rounded (167) - Erbium's Atomic Number (68) = approx. 99 Neutrons

Carbon-12 (98.93%), Carbon-13 (1.07%), and Carbon-14 (1 PPT) all occur naturally. However, Carbon-14 is radioactive (halflife 5,730±40 years) and is being produced only high in the atmosphere by bombardment of nitrogen gas by cosmic rays.

1. Radium has 45 isotopes and nuclear isomers.

2. Radium has no known today allotropes.

Plutonium has no natural isotopes. All plutonium isotopes are artificially produced through nuclear reactions.

Barium has seven isotopes, with atomic masses ranging from 130 to 138. The most abundant isotope of barium is Barium-138, making up about 71% of naturally occurring barium. Barium-137 is a radioactive isotope with a half-life of about 2.5 minutes.

Yes, even though they do emit ionizing radiation. The amount of radiation emitted from a smoke detector is about 1 hundredth of a millirem per year. The background radiation from radioactive isotopes in the ground is about 300 millirem per year. So the ground your standing on right now is exposing you to more radiation then your smoke detector ever will.

An isotope of zirconium will have protons, neutrons, and electrons. Zirconium typically has 40 protons and varying numbers of neutrons in its isotopes. Electrons surround the nucleus of the atom, balancing the positive charge of the protons.

70Ge (21.23%) - 38 neutrons
72Ge (27.66%) - 40 neutrons
73Ge (7.73%) - 41 neutrons
74Ge (35.94%) - 42 neutrons
76Ge (7.44%) - 44 neutrons

See link below.

Candu reactors have traditionally used natural uranium, which contains 0.7 percent U-235, which is the fissile isotope that produces all the nuclear fission energy. Proposals have been made that Candus could use fuel that has been discharged from light water reactors and might still contain about 0.9 percent U-235, or could even use fuel made from depleted uranium (mostly U-238) together with fissile plutonium available from dismantled nuclear weapons, but I don't think such proposals have reached the stage of implementation. For one thing, Canada doesn't have any nuclear weapons, so it would require some fuel manufacture to be set up in the US to make this fuel, or to utilise US spent fuel. There is plenty of this in US storage but no route for using it to make Candu fuel, which is of different dimensions and assembly details. However this might conceivably be done in the future.

Frederick Soddy discovered isotopes through his collaboration with Ernest Rutherford in studying radioactivity. They observed that certain elements had multiple forms with different atomic weights but similar chemical properties, leading to the concept of isotopes. Soddy coined the term "isotope" in 1913 to describe these different forms of elements.

The stable isotope formed by the breakdown of a radioactive isotope is called a daughter isotope. This process is known as radioactive decay, where a radioactive isotope transforms into a stable daughter isotope through the emission of particles or energy.

Carbon 12 and Carbon 13 are stable. All other isotopes of carbon are unstable and radioactive