Halflife
Number of halflives elapsed 
Fraction remaining 
Percentage remaining 


0  ^{1}/_{1}  100  
1  ^{1}/_{2}  50  
2  ^{1}/_{4}  25  
3  ^{1}/_{8}  12  .5 
4  ^{1}/_{16}  6  .25 
5  ^{1}/_{32}  3  .125 
6  ^{1}/_{64}  1  .563 
7  ^{1}/_{128}  0  .781 
...  ...  ...  
n  ^{1}/_{2n}  100/(2^{n}) 
Halflife (t_{1⁄2}) is the amount of time required for a quantity to fall to half its value as measured at the beginning of the time period. While the term "halflife" can be used to describe any quantity which follows an exponential decay, it is most often used within the context of nuclear physics and nuclear chemistry—that is, the time required, probabilistically, for half of the unstable, radioactive atoms in a sample to undergo radioactive decay.
The original term, dating to Ernest Rutherford's discovery of the principle in 1907, was "halflife period", which was shortened to "halflife" in the early 1950s.^{[1]} Rutherford applied the principle of a radioactive elements' halflife to studies of age determination of rocks by measuring the decay period of radium to lead206.
Halflife is used to describe a quantity undergoing exponential decay, and is constant over the lifetime of the decaying quantity. It is a characteristic unit for the exponential decay equation. The term "halflife" may generically be used to refer to any period of time in which a quantity falls by half, even if the decay is not exponential. The table on the right shows the reduction of a quantity in terms of the number of halflives elapsed. For a general introduction and description of exponential decay, see exponential decay. For a general introduction and description of nonexponential decay, see rate law. The converse of halflife is doubling time.
Contents
 Probabilistic nature of halflife 1

Formulas for halflife in exponential decay 2
 Decay by two or more processes 2.1
 Examples 2.2
 Halflife in nonexponential decay 3
 Halflife in biology and pharmacology 4
 See also 5
 References 6
 External links 7
Probabilistic nature of halflife
A halflife usually describes the decay of discrete entities, such as radioactive atoms. In that case, it does not work to use the definition "halflife is the time required for exactly half of the entities to decay". For example, if there are 3 radioactive atoms with a halflife of one second, there will not be "1.5 atoms" left after one second.
Instead, the halflife is defined in terms of probability: "Halflife is the time required for exactly half of the entities to decay on average". In other words, the probability of a radioactive atom decaying within its halflife is 50%.
For example, the image on the right is a simulation of many identical atoms undergoing radioactive decay. Note that after one halflife there are not exactly onehalf of the atoms remaining, only approximately, because of the random variation in the process. Nevertheless, when there are many identical atoms decaying (right boxes), the law of large numbers suggests that it is a very good approximation to say that half of the atoms remain after one halflife.
There are various simple exercises that demonstrate probabilistic decay, for example involving flipping coins or running a statistical computer program.^{[2]}^{[3]}^{[4]}
Formulas for halflife in exponential decay
An exponential decay process can be described by any of the following three equivalent formulas:
 \begin{align} N(t) &= N_0 \left(\frac {1}{2}\right)^{\frac{t}{t_{\frac{1}{2}}}} \\ N(t) &= N_0 e^{\frac{t}{\tau}} \\ N(t) &= N_0 e^{\lambda t} \end{align}
where

 N_{0} is the initial quantity of the substance that will decay (this quantity may be measured in grams, moles, number of atoms, etc.),
 N(t) is the quantity that still remains and has not yet decayed after a time t,
 t_{1⁄2} is the halflife of the decaying quantity,
 \tau is a positive number called the mean lifetime of the decaying quantity,
 \lambda is a positive number called the decay constant of the decaying quantity.
The three parameters t_\frac{1}{2}, \tau, and \lambda are all directly related in the following way:
 t_\frac{1}{2} = \frac{\ln (2)}{\lambda} = \tau \ln(2)
where ln(2) is the natural logarithm of 2 (approximately 0.693).
By plugging in and manipulating these relationships, we get all of the following equivalent descriptions of exponential decay, in terms of the halflife:
 \begin{align} N(t) &= N_0 \left(\frac{1}{2}\right)^{\frac{t}{t_{\frac{1}{2}}}} = N_0 2^{t/t_\frac{1}{2}} \\ &= N_0 e^{t\ln(2)/t_\frac{1}{2}} \\ t_\frac{1}{2} &= \frac{t}{\log_2(N_0/N(t))} = \frac{t}{\log_2(N_0)  \log_2(N(t))} \\ &= \frac{1}{\log_{2^t}(N_0)  \log_{2^t}(N(t))} = \frac{t\ln(2)}{\ln(N_0)  \ln(N(t))} \end{align}
Regardless of how it's written, we can plug into the formula to get
 N(0) = N_0 as expected (this is the definition of "initial quantity")
 N\left(t_\frac{1}{2}\right) = \frac{1}{2} N_0 as expected (this is the definition of halflife)
 \lim_{t\to \infty} N(t) = 0; i.e., amount approaches zero as t approaches infinity as expected (the longer we wait, the less remains).
Decay by two or more processes
Some quantities decay by two exponentialdecay processes simultaneously. In this case, the actual halflife T_{1⁄2} can be related to the halflives t_{1} and t_{2} that the quantity would have if each of the decay processes acted in isolation:
 \frac{1}{T_\frac{1}{2}} = \frac{1}{t_1} + \frac{1}{t_2}
For three or more processes, the analogous formula is:
 \frac{1}{T_\frac{1}{2}} = \frac{1}{t_1} + \frac{1}{t_2} + \frac{1}{t_3} + \cdots
For a proof of these formulas, see Exponential decay#Decay by two or more processes.
Examples
There is a halflife describing any exponentialdecay process. For example:
 The current flowing through an RC circuit or RL circuit decays with a halflife of RC\ln(2) or \ln(2)L/R, respectively. For this example, the term half time might be used instead of "half life", but they mean the same thing.
 In a firstorder chemical reaction, the halflife of the reactant is \ln(2)/\lambda, where λ is the reaction rate constant.
 In radioactive decay, the halflife is the length of time after which there is a 50% chance that an atom will have undergone nuclear decay. It varies depending on the atom type and isotope, and is usually determined experimentally. See List of nuclides.
The half life of a species is the time it takes for the concentration of the substance to fall to half of its initial value.
Halflife in nonexponential decay
The decay of many physical quantities is not exponential—for example, the evaporation of water from a puddle, or (often) the chemical reaction of a molecule. In such cases, the halflife is defined the same way as before: as the time elapsed before half of the original quantity has decayed. However, unlike in an exponential decay, the halflife depends on the initial quantity, and the prospective halflife will change over time as the quantity decays.
As an example, the radioactive decay of carbon14 is exponential with a halflife of 5730 years. A quantity of carbon14 will decay to half of its original amount (on average) after 5730 years, regardless of how big or small the original quantity was. After another 5730 years, onequarter of the original will remain. On the other hand, the time it will take a puddle to halfevaporate depends on how deep the puddle is. Perhaps a puddle of a certain size will evaporate down to half its original volume in one day. But on the second day, there is no reason to expect that onequarter of the puddle will remain; in fact, it will probably be much less than that. This is an example where the halflife reduces as time goes on. (In other nonexponential decays, it can increase instead.)
The decay of a mixture of two or more materials which each decay exponentially, but with different halflives, is not exponential. Mathematically, the sum of two exponential functions is not a single exponential function. A common example of such a situation is the waste of nuclear power stations, which is a mix of substances with vastly different halflives. Consider a sample containing a rapidly decaying element A, with a halflife of 1 second, and a slowly decaying element B, with a halflife of one year. After a few seconds, almost all atoms of the element A have decayed after repeated halving of the initial total number of atoms; but very few of the atoms of element B will have decayed yet as only a tiny fraction of a halflife has elapsed. Thus, the mixture taken as a whole does not decay by halves.
Halflife in biology and pharmacology
A biological halflife or elimination halflife is the time it takes for a substance (drug, radioactive nuclide, or other) to lose onehalf of its pharmacologic, physiologic, or radiological activity. In a medical context, the halflife may also describe the time that it takes for the concentration in blood plasma of a substance to reach onehalf of its steadystate value (the "plasma halflife").
The relationship between the biological and plasma halflives of a substance can be complex, due to factors including accumulation in tissues, active metabolites, and receptor interactions.^{[5]}
While a radioactive isotope decays almost perfectly according to socalled "first order kinetics" where the rate constant is a fixed number, the elimination of a substance from a living organism usually follows more complex chemical kinetics.
For example, the biological halflife of water in a human being is about 9 to 10 days, though this can be altered by behavior and various other conditions. The biological halflife of cesium in human beings is between one and four months. This can be shortened by feeding the person prussian blue, which acts as a solid ion exchanger that absorbs the cesium while releasing potassium ions in their place.
See also
References
 ^ John Ayto, "20th Century Words" (1989), Cambridge University Press.
 ^ "MADSCI.org". Retrieved 20120425.
 ^ "Exploratorium.edu". Retrieved 20120425.
 ^ "Astro.GLU.edu". Retrieved 20120425.
 ^ Lin VW; Cardenas DD (2003). Spinal cord medicine. Demos Medical Publishing, LLC. p. 251.
External links
 Nucleonica.net, Nuclear Science Portal
 Nucleonica.net, wiki: Decay Engine
 Bucknell.edu, System Dynamics – Time Constants
 Subotex.com, HalfLife elimination of drugs in blood plasma – Simple Charting Tool