In the context of physical sciences, several forms of energy have been identified. These include:
Some entries in the above list constitute or comprise others in the list. The list is not necessarily complete. Whenever physical scientists discover that a certain phenomenon appears to violate the law of energy conservation, new forms are typically added that account for the discrepancy.
Heat and work are special cases in that they are not properties of systems, but are instead properties of processes that transfer energy. In general we cannot measure how much heat or work are present in an object, but rather only how much energy is transferred among objects in certain ways during the occurrence of a given process. Heat and work are measured as positive or negative depending on which side of the transfer we view them from.
Classical mechanics distinguishes between kinetic energy, which is determined by an object's movement through space, and potential energy, which is a function of the position of an object within a field, which may itself be related to the arrangement of other objects or particles. These include gravitational energy (which is stored in the way masses are arranged in a gravitational field), several types of nuclear energy (which utilize potentials from the nuclear force and the weak force), electric energy (from the electric field), and magnetic energy (from the magnetic field).
Other familiar types of energy are a varying mix of both potential and kinetic energy. An example is mechanical energy which is the sum of (usually macroscopic) kinetic and potential energy in a system. Elastic energy in materials is also dependent upon electrical potential energy (among atoms and molecules), as is chemical energy, which is stored and released from a reservoir of electrical potential energy between electrons, and the molecules or atomic nuclei that attract them. .
Potential energies are often measured as positive or negative depending on whether they are greater or less than the energy of a specified base state or configuration such as two interacting bodies being infinitely far apart.
Wave energies (such as radiant or sound energy), kinetic energy, and rest energy are each greater than or equal to zero because they are measured in comparison to a base state of zero energy: "no wave", "no motion", and "no inertia", respectively.
It has been attempted to categorize all forms of energy as either kinetic or potential, but as Richard Feynman points out:
Also, at relativistic speeds, defining kinetic energy is problematic because the energy due to the body's motion does not simply contribute additively to the total energy as it does at classical speeds.
Energy may be transformed between different forms at various efficiencies. Items that transform between these forms are called transducers.
Contents

Mechanical energy 1

Kinetic energy 2

Potential energy 3

Mechanical work 4

Elastic potential energy 5

Surface energy 6

Sound energy 7

Gravitational potential energy 8

Thermal energy 9

Chemical energy 10

Electric energy 11

Electrostatic energy 11.1

Electric energy 11.2

Magnetic energy 11.3

Electromagnetic energy 11.4

Nuclear energy 12

See also 13

References 14
Mechanical energy
General nonrelativistic mechanics
Mechanical energy (symbols E_{M} or E) manifest in many forms, but can be broadly classified into potential energy (E_{p}, V, U or Φ) and kinetic energy (E_{k} or T). The term potential energy is a very general term, because it exists in all force fields, such as gravitation, electrostatic and magnetic fields. Potential energy refers to the energy any object gain due to its position in a force field.
The relation between mechanical energy with kinetic and potential energy is simply

E = T + V \,\!.
Lagrangian and Hamiltonian mechanics
In more advanced topics, kinetic plus potential energy is physically the total energy of the system, but also known as the Hamiltonian of the system:

H = T + V , \,\!
used in Hamilton's equations of motion, to obtain equations describing a classical system in terms of energy rather than forces. The Hamiltonian is just a mathematical expression, rather than a form of energy.
Another analogous quantity of diverse applicability and efficiency is the Lagrangian of the system:

L = T  V \,\!,
used in Lagrange's equations of motion, which serve the same purpose as Hamilton's equations.
Kinetic energy
General scope
Kinetic energy is the work required to accelerate an object to a given speed. In general:

E_\mathrm{k} = \int \mathbf{F} \cdot d \mathbf{x} = \int \mathbf{v} \cdot d \mathbf{p}
Classical mechanics
In classical mechanics, for a particle of constant mass m, in which case the force acting on it is F = ma where a is the particle's acceleration vector, the integral is:

E_\mathrm{k} = \int \mathbf{F} \cdot d \mathbf{x} = m \int \frac{d\mathbf{v}}{dt} \cdot \mathbf{v} dt = m \int d\mathbf{v} \cdot \mathbf{v} = m \int \frac{1}{2} d (\mathbf{v} \cdot \mathbf{v} ) = \frac{1}{2}mv^2\,\!
Special relativistic mechanics
At speeds approaching the speed of light c, this work must be calculated using Lorentz transformations, and applying mass and energy conservation, which results in

E_\mathrm{k} = \left ( \gamma  1 \right ) m c^2 ,
where

\gamma = \frac{1}{\sqrt{1  \left ( \frac{v}{c} \right )^2}}
is the lorentz factor.
Here the two terms on the right hand side are identified with the total energy and the rest energy of the object, respectively. This equation reduces to the one above it, at small (compared to c) speed. The kinetic energy is zero at v=0 (when γ = 1), so that at rest, the total energy is the rest energy. So a mass at rest in some inertial reference frame has a corresponding amount of rest energy equal to:

E_0 = m_0 c^2 \,\!
All masses at rest have a tremendous amount of energy, due to the proportionality factor of c^{2}.
Potential energy
Potential energy is defined as the work done against a given force in changing the position of an object with respect to a reference position, often taken to be infinite separation. In other words it is the work done on the object to give it that much energy. Changes in work and potential energy are related simply,

\Delta U = \Delta W .
The name "potential" energy originally signified the idea that the energy could readily be transferred as work — at least in an idealized system (reversible process, see below). This is not completely true for any real system, but is often a reasonable first approximation in classical mechanics.
Mechanical work
Translational motion
If F is the force and r is the displacement, then the change in mechanical work done along the path between positions r_{1} and r_{2} due to the force is, in integral form:

\Delta W = \int_{\mathbf{r}_1}^{\mathbf{r}_2} \mathbf{F}\cdot\mathrm{d}\mathbf{r},
(the dot represents the scalar product of the two vectors). The general equation above can be simplified in a number of common cases, notably when dealing with gravity or with elastic forces. If the force is conservative the equation can be written in differential form as

\mathbf{F} = \nabla W .
Rotational motion
The rotational analogue is the work done by a torque τ, between the angles θ_{1} and θ_{2},

\Delta W = \int_{\theta_1}^{\theta_2} \left  \boldsymbol{\tau} \right  \mathrm{d}\theta.
Elastic potential energy
As a ball falls freely under the influence of
gravity, it accelerates downward, its initial
potential energy converting into
kinetic energy. On impact with a hard surface the ball deforms, converting the kinetic energy into
elastic potential energy. As the ball springs back, the energy converts back firstly to kinetic energy and then as the ball regains height into potential energy. Energy conversion to heat due to
inelastic deformation and
air resistance cause each successive bounce to be lower than the last.
Elastic potential energy is defined as a work needed to compress or extend a spring. The tension/compression force F in a spring or any other system which obeys Hooke's law is proportional to the extension/compression x,

\mathbf{F} = k\mathbf{x}\,\!,
where k is the force constant of the particular spring or system. In this case the force is conservative, the calculated work becomes

E_\mathrm{p,e} = \frac{1}{2}kx^2\,\!.
If k is not constant the above equation will fail. Hooke's law is a good approximation for behaviour of chemical bonds under stable conditions, i.e. when they are not being broken or formed.
Surface energy
If there is any kind of tension in a surface, such as a stretched sheet of rubber or material interfaces, it is possible to define surface energy.
If γ is the surface tension, and S = surface area, then the work done W to increase the area by a unit area is the surface energy:

\mathrm{d}W = \gamma \mathrm{d}S . \,\!
In particular, any meeting of dissimilar materials that do not mix will result in some kind of surface tension, if there is freedom for the surfaces to move then, as seen in capillary surfaces for example, the minimum energy will as usual be sought.
A minimal surface, for example, represents the smallest possible energy that a surface can have if its energy is proportional to the area of the surface. For this reason, (open) soap films of small size are minimal surfaces (small size reduces gravity effects, and openness prevents pressure from building up. Note that a bubble is a minimum energy surface but not a minimal surface by definition).
Sound energy
Sound is a form of mechanical vibration which propagates through any mechanical medium. It is closely related to the ability of the human ear to perceive sound. The wide outer area of the ear is maximized to collect sound vibrations. It is amplified and passed through the outer ear, striking the eardrum, which transmits sounds into the inner ear. Auditory nerves fire according to the particular vibrations of the sound waves in the inner ear, which designate such things as the pitch and volume of the sound. The ear is set up in an optimal way to interpret sound energy in the form of vibrations.
Gravitational potential energy
The gravitational force very near the surface of a massive body (e.g. a planet) varies very little with small changes in height, h, and locally is equal mg where m is mass, and g is the gravitational acceleration (AKA field strength). At the Earth's surface g = 9.81 m s^{1}. In these cases, the gravitational potential energy is given by

E_\mathrm{p,g} \approx mgh\,\!
A more general expression for the potential energy due to Newtonian gravitation between two bodies of masses m_{1} and m_{2}, is

E_\mathrm{p,g} = \frac{G m_1 m_2}{r}\,\!,
where r is the separation between the two bodies and G is the gravitational constant, 6.6742(10) × 10^{11} m^{3} kg^{1} s^{2}.^{[1]} In this case, the zero potential reference point is the infinite separation of the two bodies. Care must be taken that these masses are point masses or uniform spherical solids/shells. It cannot be applied directly to any objects of any shape and any mass.
In terms of the gravitational potential (Φ, U or V), the potential energy is (by definition of gravitational potential),

E_\mathrm{p,g} = \Phi m \,\!.
Thermal energy
General scope
Thermal energy (of some state of matter  gas, plasma, solid, etc.) is the energy associated with the microscopical random motion of particles constituting the media. For example, in case of monatomic gas it is just a kinetic energy of motion of atoms of gas as measured in the reference frame of the center of mass of gas. In case of molecules in the gas rotational and vibrational energy is involved. In the case of liquids and solids there is also potential energy (of interaction of atoms) involved, and so on.
A heat is defined as a transfer (flow) of thermal energy across certain boundary (for example, from a hot body to cold via the area of their contact). A practical definition for small transfers of heat is

\Delta q = \int_{T_1}^{T_2} C_\mathrm{v}\mathrm{d}T
where C_{v} is the heat capacity of the system. This definition will fail if the system undergoes a phase transition—e.g. if ice is melting to water—as in these cases the system can absorb heat without increasing its temperature. In more complex systems, it is preferable to use the concept of internal energy rather than that of thermal energy (see belowChemical energy).
Despite the theoretical problems, the above definition is useful in the experimental measurement of energy changes. In a wide variety of situations, it is possible to use the energy released by a system to raise the temperature of another object, e.g. a bath of water. It is also possible to measure the amount of electric energy required to raise the temperature of the object by the same amount. The calorie was originally defined as the amount of energy required to raise the temperature of one gram of water by 1 °C (approximately 4.1855 J, although the definition later changed), and the British thermal unit was defined as the energy required to heat one pound of water by 1 °F (later fixed as 1055.06 J).
Kinetic theory
In kinetic theory which describes the ideal gas, the thermal energy per degree of freedom is given by:

U = \frac{d_f}{2}k_B T
where d_{f} is the number of degrees of freedom and k_{B} is the Boltzmann constant. The total themeral energies would equal the total internal energy of the gas, since intermolecular potential energy is neglected in this theory. The term k_{B}T occurs very frequently into statistical thermodynamics.
Chemical energy
Chemical energy is the energy due to excretion of atoms in molecules and various other kinds of aggregates of matter. It may be defined as a work done by electric forces during rearrangement of mutual positions of electric charges, electrons and protons, in the process of aggregation. So, basically it is electrostatic potential energy of electric charges. If the chemical energy of a system decreases during a chemical reaction, the difference is transferred to the surroundings in some form (often heat or light); on the other hand if the chemical energy of a system increases as a result of a chemical reaction  the difference then is supplied by the surroundings (usually again in form of heat or light). For example,

when two hydrogen atoms react to form a dihydrogen molecule, the chemical energy decreases by 724 zJ (the bond energy of the H–H bond);

when the electron is completely removed from a hydrogen atom, forming a hydrogen ion (in the gas phase), the chemical energy increases by 2.18 aJ (the ionization energy of hydrogen).
It is common to quote the changes in chemical energy for one mole of the substance in question: typical values for the change in molar chemical energy during a chemical reaction range from tens to hundreds of kilojoules per mole.
The chemical energy as defined above is also referred to by chemists as the internal energy, U: technically, this is measured by keeping the volume of the system constant. Most practical chemistry is performed at constant pressure and, if the volume changes during the reaction (e.g. a gas is given off), a correction must be applied to take account of the work done by or on the atmosphere to obtain the enthalpy, H, this correction is the work done by an expanding gas,

\Delta E = p \Delta V \,\!,
so the enthalpy now reads;

\Delta H = \Delta U + p \Delta V \,\!.
A second correction, for the change in entropy, S, must also be performed to determine whether a chemical reaction will take place or not, giving the Gibbs free energy, G. The correction is the energy required to create order from disorder,^{[2]}

\Delta E = T \Delta S \,\!,
so we have;

\Delta G = \Delta H  T \Delta S \,\!.
These corrections are sometimes negligible, but often not (especially in reactions involving gases).
Since the industrial revolution, the burning of coal, oil, natural gas or products derived from them has been a socially significant transformation of chemical energy into other forms of energy. the energy "consumption" (one should really speak of "energy transformation") of a society or country is often quoted in reference to the average energy released by the combustion of these fossil fuels:

1 tonne of coal equivalent (TCE) = 29.3076 GJ = 8,141 kilowatt hour

1 tonne of oil equivalent (TOE) = 41.868 GJ = 11,630 kilowatt hour
On the same basis, a tankfull of gasoline (45 litres, 12 gallons) is equivalent to about 1.6 GJ of chemical energy. Another chemically based unit of measurement for energy is the "tonne of TNT", taken as 4.184 GJ. Hence, burning a tonne of oil releases about ten times as much energy as the explosion of one tonne of TNT: fortunately, the energy is usually released in a slower, more controlled manner.
Simple examples of storage of chemical energy are batteries and food. When food is digested and metabolized (often with oxygen), chemical energy is released, which can in turn be transformed into heat, or by muscles into kinetic energy.
According to the Bohr theory of the atom, the chemical energy is characterized by the Rydberg constant.

R_y= \frac{m_e e^4}{8 \varepsilon_0^2 h^2} = \frac{1}{2}\alpha^2 m_ec^2 = 13.605\;692\;53(30) \ \mathrm{eV}
(see Rydberg constant for the meaning of the symbols).
Electric energy
Electrostatic energy
General scope
The electric potential energy of given configuration of charges is defined as the work which must be done against the Coulomb force to rearrange charges from infinite separation to this configuration (or the work done by the Coulomb force separating the charges from this configuration to infinity). For two pointlike charges Q_{1} and Q_{2} at a distance r this work, and hence electric potential energy is equal to:

E_\mathrm{p,e} = \frac{1}
where ε_{0} is the electric constant of a vacuum, 10^{7}/4πc_{0}^{2} or 8.854188… × 10^{−12} F m^{−1}.^{[1]} In terms of electrostatic potential (ϕ for absolute, V for difference in potential), again by definition, electrostatic potential energy is given by:

E_\mathrm{p,e} = \phi q \,\!.
If the charge is accumulated in a capacitor (of capacitance C), the reference configuration is usually selected not to be infinite separation of charges, but vice versa  charges at an extremely close proximity to each other (so there is zero net charge on each plate of a capacitor). The justification for this choice is purely practical  it is easier to measure both voltage difference and magnitude of charges on a capacitor plates not versus infinite separation of charges but rather versus discharged capacitor where charges return to close proximity to each other (electrons and ions recombine making the plates neutral). In this case the work and thus the electric potential energy becomes

E_\mathrm{p,e} = \frac{Q^2}{2C} = \frac{1}{2}CV^2 = \frac{1}{2}VQ \,\!,
(different forms obtained using the definition of capacitance).
Electric energy
Electric circuits
If an electric current passes through a resistor, electric energy is converted to heat; if the current passes through an electric appliance, some of the electric energy will be converted into other forms of energy (although some will always be lost as heat). The amount of electric energy due to an electric current can be expressed in a number of different ways:

E = VQ = VIt = Pt = \frac{V^2 t}{R} = {I^2}Rt \,\!
where V is the electric potential difference (in volts), Q is the charge (in coulombs), I is the current (in amperes), t is the time for which the current flows (in seconds), P is the power (in watts) and R is the electric resistance (in ohms). The last of these expressions is important in the practical measurement of energy, as potential difference, resistance and time can all be measured with considerable accuracy.
Magnetic energy
General scope
There is no fundamental difference between magnetic energy and electric energy: the two phenomena are related by Maxwell's equations. The potential energy of a magnet of magnetic moment m in a magnetic field B is defined as the work of magnetic force (actually of magnetic torque) on realignment of the vector of the magnetic dipole moment, and is equal to:

E_\mathrm{p,m} = \mathbf{m}\cdot \mathbf{B}.
Electric circuits
The energy stored in an inductor (of inductance L) carrying current I is

E_\mathrm{p,m} = \frac{1}{2}LI^2.
This second expression forms the basis for superconducting magnetic energy storage.
Electromagnetic energy
Calculating work needed to create an electric or magnetic field in unit volume (say, in a capacitor or an inductor) results in the electric and magnetic fields energy densities:

u_e=\frac{\epsilon_0}{2} \left \mathbf{E} \right ^2 , \quad u_m=\frac{1}{2\mu_0} \left \mathbf{B} \right ^2 \,\!,
in SI units.
Electromagnetic radiation, such as microwaves, visible light or gamma rays, represents a flow of electromagnetic energy. Applying the above expressions to magnetic and electric components of electromagnetic field both the volumetric density and the flow of energy in EM field can be calculated. The resulting Poynting vector, which is expressed as

\mathbf{S} = \frac{1}{\mu} \mathbf{E} \times \mathbf{B},
in SI units, gives the density of the flow of energy and its direction.
The energy of electromagnetic radiation is quantized (has discrete energy levels). The energy of a photon is:

E = h\nu = \frac{hc}{\lambda}\,\!,
so the spacing between energy levels is:

\Delta E = E_2  E_1 = hc \left ( \nu_2  \nu_1 \right ) = hc \left ( \frac{1}{\lambda_2}  \frac{1}{\lambda_1} \right ) \,\!,
where h is the Planck constant, 6.6260693(11)×10^{−34} Js,^{[1]} and ν is the frequency of the radiation. This quantity of electromagnetic energy is usually called a photon. The photons which make up visible light have energies of 270–520 yJ, equivalent to 160–310 kJ/mol, the strength of weaker chemical bonds.
Nuclear energy
Nuclear potential energy, along with electric potential energy, provides the energy released from nuclear fission and nuclear fusion processes. The result of both these processes are nuclei in which the moreoptimal size of the nucleus allows the nuclear force (which is opposed by the electromagnetic force) to bind nuclear particles more tightly together than before the reaction.
The Weak nuclear force (different from the strong force) provides the potential energy for certain kinds of radioactive decay, such as beta decay.
The energy released in nuclear processes is so large that the relativistic change in mass (after the energy has been removed) can be as much as several parts per thousand.
Nuclear particles (nucleons) like protons and neutrons are not destroyed (law of conservation of baryon number) in fission and fusion processes. A few lighter particles may be created or destroyed (example: beta minus and beta plus decay, or electron capture decay), but these minor processes are not important to the immediate energy release in fission and fusion. Rather, fission and fusion release energy when collections of baryons become more tightly bound, and it is the energy associated with a fraction of the mass of the nucleons (but not the whole particles) which appears as the heat and electromagnetic radiation generated by nuclear reactions. This heat and radiation retains the "missing" mass, but the mass is missing only because it escapes in the form of heat or light, which retain the mass and conduct it out of the system where it is not measured.
The energy from the Sun, also called solar energy, is an example of this form of energy conversion. In the Sun, the process of hydrogen fusion converts about 4 million metric tons of solar "matter" per second into light, which is radiated into space, but during this process, although protons change into neutrons, the number of total protonsplusneutrons does not change. In this system, the radiated light itself (as a system) retains the "missing" mass, which represents 4 million tons per second of electromagnetic radiation, moving into space. Each of the helium nuclei which are formed in the process are less massive than the four protons from they were formed, but (to a good approximation), no particles are destroyed in the process of turning the Sun's nuclear potential energy into light. Instead, the four nucleons in a helium nucleus in the Sun have an average mass that is less than the protons which formed them, and this mass difference (4 million tons/second) is the mass that moves off as sunlight.
See also
References

^ ^{a} ^{b} ^{c} Mohr, Peter J.; Taylor, Barry N.; Newell, David B. (2008). "CODATA Recommended Values of the Fundamental Physical Constants: 2006".

^ Chemistry, Matter, and the Universe, R.E. Dickerson, I. Geis, W.A. Benjamin Inc. (USA), 1976, ISBN 0198551487
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