[C3H5N3O9]

I just thought I would let you know as you seem to be interested in chemistry, most of what you posted particularly the info on basic ionic bonding and poly atomic ionic bonding is mainly accurate, the info on orbitals and electronic structure is on the right track ,(sort of) , but far from correct.
Electrons are arranged in energy levels called shells there are 7 shells called, K,L,M,N,O,P,Q respectivley, K being the lowest energy level and Q the highest. Each shell is then divided into sub shells of similar energy ,(known as orbitals), each orbital can hold a maximum of 2 electrons.
There are 4 different types of orbitals, (though there is now discussion of a fifth), S, P, D, F, the first shell only has 1S orbital, the second 1S and 3P's the third shell has 1S, 3P's and 5D's the fourth shell has 1S 3P's, 5D's and 7F'sand as I mentioned, in the course I am doing at the moment we are discussing the possiblity of a G orbital, but I will not discuss that here, the tricky thing is the orbitals don't fill completely in order, because electrons will always fill lower energy orbitals before higher energy orbitals.
The first energy level, the K shell can only hold 2 electrons, therefore it only has 1 orbital, called 1S. Hydrogen having only 1 electron has an electron configuration of 1S1. Helium the first noble gas has a full first shell so its structure is 1S2.
Now we move into the second shell the L shell can hold up to 8 electrons therefore it has 1 S orbital, called 2S and 3p orbitals.
For an example of this shell look at Fluorine, as you pointed out it is 1 electron short of having a full valence shell, so its structure is 1S2, 2S2, 2P5 so 2 of its 3 P orbitals are full but it is lacking an electron. Now Neon the second noble gas has a full valence shell as do all noble gasses, so its structure is 1S2, 2S2, 2P6.
This fills the second shell, so we now move to the third, this is where it begins to get tricky, the 4S orbital has lower energy than the 3D orbital so let's take things up to the next Noble gas Argon, it has 3 shells, with a total of 18 electrons, but the third shell can hold up to 18 electrons by it'self, Argon's electronic structure is 1S2, 2S2, 2P6, 3S2, 3P6. So even though its third shell only has 8 electrons it is considerd full, now as I mentioned the 4S orbital has lower energy than the 3D orbital, so for Potassium, element 19 and the first element to use the fourth shell its electron structure is, 1S2, 2S2, 2P6, 3S2, 3P6, 4S1. Its valence electron is in the fourth shell in the 4S orbital, because as I mentioned electrons will always fill lower energy levels first.
Calcium continues to fill the 4S orbital before the 3D its structure 1S2, 2S2, 2P6, 3S2, 3P6, 4S2, then after Ca the 3D orbitals begin to fill.
The next element being Scandium has the electronic structure, 1S2, 2S2, 2P6, 3S2, 3P6, 3D1, 4S2. As the periodic table continues we keep going up 1 electron at a time but the orbitals continue to swap around.
Copper is the first element to have a completely full 3rd shell, its structure, 1S2, 2S2, 2P6, 3S2, 3P6, 3D10, 4S1, as you can see it has gone back to having only 1 electron in the 4S orbital.
Electron structure specificly the valence electrons can predict/explain which elements will react with which and also how they will behave,( to a degree).
However in its entirity it is a rather complex aspect of chemistry.
I also thought I would mention that many of the transition elements can have multiple valencies, for example Iron Fe 2+-3+ ; Manganese Mn 2+-4+; Tin Sn 4+- 2+. Also the ammonium ion is NH+ (1+), there's also a few mistakes with capitalization, like it's KNO3 not KN03. Also H2O isn't an ionic compound it is a molecule which forms by the 2 Hydrogens sharing their valence electrons with Oxygens 6 to make 8, this is a covalent bond.
Apart from that it's all good
Any way I hope that hasn't confused people further but if you are going to learn, you really need to have the fundamentals right.