for a reaction that is at equilibrium, it is not considered spontaneous because deltaG=0 and the rates of the forward and reverse reaction are running at the same speed, so to say. when you start with 100% of one product, it will only be spontaneous if the deltaG of that reaction is negative, and will reach equilibrium when deltaG=0.
the constants Q and K are just ratios of the amount of products/reactants. when you have a Q which is greater than 1 it means there are more products than reactants, not necessarily meaning that the reaction is spontaneous or not. the spontaneity of a reaction depends on the gibbs equation and the other energies associated with the reaction: temperature, entropy, and enthalpy.
Q is only used when something is added or taken away from a reaction already at equilibrium. when Q>K this means there are more products than there were at the true equilibrium and this the reaction will shift to make Q=K, or in the reverse direction. when Q<K it means there are more reactants than products and the equilibrium will shift to increase Q to make it = to K and run the forward reaction to equilibrium.
le chatlier's principle does not depend on the energies of any of the reactions, it just says that it will counter the effect on the system to make it reach equilibrium again.