Manganese doesn't like to be in +5 and +6 O.S. and the acid form of hypomanganate and manganate anion cannot exist due to rapid disproportionation. So, they exist as salts of alkali metals. Manganese in +7 O.S. is quite stable and hence permanganic acid can still exist in aqueous solution although it can deproptonate or decompose in solution to manganese dioxide, oxygen, and water, with initially formed manganese dioxide catalyzing further decomposition.
Note that manganic acid can exist in a metastable form during the formation of manganate salts but decompose to permanganic acid as it has been noted in an old book(some of the terms are outdated):
Manganic acid in a state of purity has not as yet been obtained; it is known only in combination with bases. In order to obtain it, a strong base, for example, potash or the nitrates of such bases are exposed to a read heat in conjunction with peroxide of manganese (assume MnO2). Whether the operation be performed with or without the contact of air, a manganate is produced; with the contact of air, the peroxide of manganese absorbs oxygen and transformed into manganic acid; without the contact of air, according to Mitscherlich, the peroxide of manganese is decomposed into manganic acid and deuteroxide of manganese (assume Mn2O3)
[...]
The manganates in solid state are so intensely green that they often appear black. Their aqueous solution are intensely green also; manganic acid easily decompose to hypermanganic acid (assume HMnO4). All acids, even weakest, impart immediately an intense red color as the green solution of manganates convert into hypermanganic acid, which is accompanied by the formation of black precipitate of peroxide of manganese, with hypermanganic acid further decomposition (if further heat is applied)
Ref.: CHEMICAL ANALYSIS by H.Rose, W. Tegg Publ., 1848