No, because: (1) it does not matter how many electrons the atom has or how efficiently it uses them and therefore (2) its atoms must be very small (say, less than half the size of the nucleus) to get free energy. The energy must lie somewhere else. It’s like when an atom gains energy for its motion by a force. If you have a small atom moving in a vacuum, you probably have just enough energy to get some of the motion (some velocity) and that, combined with your tiny nucleus, should be enough to go all the way to equilibrium without really much energy being added to it. It is easy to see then why Gibbs energy is zero at equilibrium when the entropy is large compared to the total mass of the atoms.
The second thing that makes little Gibbs free energy less than zero is why a gas gets a lot of entropy at equilibrium, because it has less surface area than a metal. The bigger the particles are the more they lose and gain kinetic energy of collision, but in the process they get hotter and colder (both in the temperature and the kinetic energy levels) as they grow to about 10^-8 cm^2/s^2 and even 1000 cm^2/s^2 respectively. As they get bigger the total energy they lose and gain is less than that but the energy in the gas can no longer increase very much in the process, because it just cannot grow and will eventually lose its value. In any case, the overall entropy does not change very much either, so any decrease in the average entropy level is compensated by a relatively strong increase in the average temperature.
However, in gas molecules, there is usually not much surface area (less than 0.2% compared to 0.5%) because they lose and receive kinetic energy through the collisions between atoms, not through their motion. So, in the case of a gas of 0.7% molecules, it is obvious that an equilibrium gas was reached when energy would be conserved to reach the equilibrium state without any of the entropy being changed at all.
The entropy is not conserved in an atomic system at equilibrium because some fraction – 0.17% or so, in fact – of that entropy is lost through the collisions of the atoms and the rest remains at a constant value. It seems like a lot of entropy is lost, for a gas of 7.2% in density. And if a molecule is at one of its equilibrium temperatures of 775 K and its kinetic energy is
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