, "monatomic" is a combination of the words "mono" and "atomic", and means "single atom
". It is usually applied to
: a monatomic gas
is one in which atoms are not bound to each other. Examples at standard conditions include the noble gases argon, krypton, and xenon, though all chemical elements will be monatomic in the gas phase at sufficiently high temperatures. The Thermodynamics
behavior of a monatomic gas is extremely simple when compared to polyatomic gases because it is free of any rotational or vibrational energy.
The only chemical elements that are stable single atom molecules
at standard temperature and pressure (STP) are the
. These are helium
, and radon
. Noble gases have a full outer valence shell making them rather non-reactive species.
While these elements have been described historically as completely inert, chemical compounds have been synthesized with all but neon and helium.
When grouped together with the homonuclear diatomic gases such as nitrogen (N2), the noble gases are called "elemental gases" or "molecular gases" to distinguish them from molecules that are also chemical compounds.
The only possible motion of an atom in a monatomic gas is translation (electronic excitation is not important at room temperature). Thus by the equipartition theorem, the kinetic energy
of a single atom of a monatomic gas at thermodynamic temperature T
is given by
, where kb
is Boltzmann's constant. One mole of atoms contains an Avogadro number
) of atoms, so that the energy of one mole of atoms of a monoatomic gas is
, where R
is the gas constant
In an adiabatic process, monatomic gases have an idealised γ-factor ( Cp/ Cv) of 5/3, as opposed to 7/5 for ideal diatomic gases where rotation (but not vibration at room temperature) also contributes. Also, for ideal monatomic gases:
[ Heat Capacity of an Ideal Gas] [ Heat Capacity of Ideal Gases] [ Lecture 3: Thermodynamics of Ideal Gases & Calorimetry, p. 2]
- the molar heat capacity at constant pressure ( Cp) is 5/2 R = 20.8 J K−1 mol−1 (4.97 Calorie K−1 mol−1).
- the molar heat capacity at constant volume ( Cv) is 3/2 R = 12.5 J K−1 mol−1 (2.98 cal K−1 mol−1).