First, it isn't very accurate to talk about a radioactive "element"; you should talk about radioactive isotopes. Different isotopes of the same element can have very different behavior in this sense. For example, hydrogen-1 and hydrogen-2 are stable, while hydrogen-3 is not (half-life about 19 years).
Individual atoms, in a radioactive isotope, will decay at a random moment. The half-life refers to how long it takes for half of the atoms in a given sample to decay (and convert to some other type of isotope).
[Radioactive half life is how long it takes for half the radioactive substance to decay. For example if something takes 100 years to decay, its half life is 50 years ^^]
That is a bit incorrect (it assumes a linear decay). Radioactive isotopes decay exponentially, so they never "completely" finish decaying. Half-life is indeed the time it takes for half of a sample to decay. If we have 100 isotopes and their half life is 1 year, then after 1 year we have 50 isotopes undecayed. After another 1 year, half of that will have decayed, so we have only 25 isotopes left undecayed. After another year, about 12-13 will be left, etc.
Depends on the isotope being used for dating.
There is some indication that Bismuth, normally considered stable, is actually radioactive with a halflife several times the age of the universe.
the halflife is 10 days
The length of time depends on the element and isotope, but the point at which half of the sample has decayed is known as the half-life.
There are several radioactive forms of carbon. The most familiar, used in carbon dating, is carbon-14. All of the others have very short half-lives.Isotopes of carbon range from carbon-8 to carbon-22. Carbon-12 and carbon-13 are stable and non-radioactive. Carbon-14 has a half-life of 5730 years. The longest lived beyond that is carbon-11 at 20.3 minutes.
radioactive decay
Over 99.999% of argon is not radioactive. A trace of radioactive argon-39 can be found in nature, but it is not significant. Synthetic radioactive isotopes of argon exist, as they do for all elements.
many. one example is lead-214 with a halflife of 26.8 minutes.
All atoms of a specific element have the same number of protons in their nucleus, but the number of neutrons in the nucleus may vary these are isotopes of that element.Hydrogen has several possible isotopes, only the first three of these are commonly referred to:hydrogen or protium or hydrogen-1, 1 proton 0 neutrons, stabledeuterium or hydrogen-2, 1 proton 1 neutron, stabletritium or hydrogen-3, 1 proton 2 neutrons, radioactive halflife 12.26 yearshydrogen-4, 1 proton 3 neutrons, radioactive halflife about 139 yoctosecondshydrogen-5, 1 proton 4 neutrons, radioactive halflife about 910 yoctosecondshydrogen-6, 1 proton 5 neutrons, radioactive halflife 290 yoctosecondshydrogen-7, 1 proton 6 neutrons, radioactive halflife 23 yoctosecondsetc.
halflife
no, halflife is a constant for each isotope's decay process.
my grandma
the halflife is 10 days
The basic idea is to compare the abundance of a naturally occurring radioactive isotope within a material to the abundance of its decay products; it is known how fast the radioactive isotope decays.
Uranium has the longest half-life element
The length of time required for half of a sample of radioactive material to decay
Half-life is the time it takes for one half of the radioactive material to decay. It is logarithmic, so after two half-lives, one quarter remains - then one eighth - etc.
Illadelph Halflife was created on 1996-09-24.
Making any change in the half-life of an isotope of any element is generally something that lies outside our abilities. A very few radioactive materials have demonstrated a change in their half-lives when bathed in intense magnetic fields. Generally, however, the half-life on a given radionuclide is not something that can be changed. A number of experiments have been conducted wherein investigators have deliberately sought to influence radioactive half-life, but in all but the rarest cases, radionuclides are sublimely resistant to having their half-lives changed.