Here's some of what you'll need to know in order to have an idea of what I'm talking about...

I can't relate all of the fundamentals of chemistry in a single post. A lot of what I'd like to get across would best be done with drawings, images, graphs, and such. I'm too used to using words, but I'll try to provide some images, starting with this very post. Well, let's introduce the periodic table.

I hope you've seen it before. And if you haven't, what is wrong with you? There a lot to say about this table. It's one of the most important developments in science. It's fascinating and I recommend learning about it, but if you find it intimidating now, you can take solace in the fact that I'll only be using a small portion of it for this blog. Here, I'll show you.

See? It's the same table, but I erased everything we don't really care about. Some of the elements I erased from the table will actually be important in the future, but not for a while. We'll cross that bridge when we come to it. I also shaded in the elements we care about most. And out of the ones I didn't shade in, each one is pretty similar to the ones it shares a column with. That means we're really looking at about eleven different things, rather than over a hundred.

Of course, there's the issue of what these elements actually mean and why they're placed on the table the way they are. Each element is a substance that has its own unique atom. Atoms have three building blocks: protons, neutrons, and electrons. Neutrons are the heaviest. They have some important properties, but for our purposes they don't do much besides sit there in the middle of the atom, a region called the nucleus. Right beside them are the protons. Every atom has a specific number of protons, which is its atomic number. The number of protons is what makes an atom have the chemical properties that it does. And the table organizes them according to this number. You can see that hydrogen (atomic symbol H) is the very first one. Hydrogen atoms each have one proton. Helium (atomic symbol He), which I erased in the second table, is second and has two protons. Lithium (atomic symbol Li) is third and has three protons. This continues for the whole table. Every proton has a positive charge, often represented as +1.

Atoms also have electrons. But electrons don't sit in the nucleus. They buzz around in an area surrounding the nucleus. Electrons are much smaller than protons, but each one has a negative charge that cancels out the positive charge from a proton, often represented as -1. This means, of course, that an atom with the same number of electrons as it has protons will have no charge (it's neutral). Electrons interact in three-dimensional geometric structures called "orbitals" that I happen to find very annoying to draw. I'll cover those at some point in the future. What's important is that these orbitals take up a lot of space. Even though the nucleus is much heavier than all of the electrons combined and would take up more space than all of them, the negatively charged area of the orbitals engulfs the nucleus. I've heard the size difference likened to a golf ball sitting in the middle of a stadium, with the golf ball being the nucleus (with almost all of the mass) and the walls of the stadium being the outermost electrons.

The electrons on the highest or outside orbital are valence electrons. They're the ones that form bonds to other atoms. Chemistry deals with the countless ways in which bonds interact, where they can form, what it takes to break them, etc. Electrons in this "valence shell" typically exist in pairs (there's a reason for this, but it's another thing that I'm skipping for now). With this in mind, I'll go over the interactions we expect to see in bonds with our important atoms.

The alkali metals:

The alkali metals we're worried about are lithium (Li), sodium (Na), and potassium (K). And really, they're all pretty similar to each other, which simplifies things for us. Alkali metals are very reactive. They'll typically form ions. Ions are like atoms, but with either fewer or more electrons than the number of protons in the nucleus. This happens because the atoms either lose or gain valence electrons. An atom that has lost valence electrons is called a cation and has a positive charge (because it has more protons than electrons). An atom that has gained valence electrons is called an anion and has a negative charge (it has more electrons than protons). Alkali metals all have one valence electron. When they react, they become +1 charged cations. The most famous example of an ionic compound is sodium chloride, common table salt. The sodium cations and the chloride anions (anions of chlorine) are attracted to each other because they're oppositely charged (you did know that opposites attract, I hope). We won't be dealing with metals much, because this is organic chemistry. But it is important to understand ions.

The alkaline-earth metals:

The alkaline-earth metals we're worried about are beryllium (Be), magnesium (Mg), and calcium (Ca). When I was taking organic chemistry, I dealt with them even less than the alkali metals (and I didn't deal with berylium at all). But like the alkali metals and some other metals, these can come up when we get into organometallic chemistry (which won't be for a while). The only important thing to keep in mind about these metals is that they have two valence electrons and will react to form cations by losing both. I used sodium chloride as an example above. The equivalent to that here would be magnesium chloride, which is less well-known, but it is used to make tofu and is sometimes used as a dessicant (it absorbs water from the air). Because it needs to lose both of its valence electrons to become a stable cation, magnesium chloride crystals actually have pairs of chloride ions attached to the magnesium ions so the ratio of anions to cations is 2:1, whereas in the case of sodium chloride, the ratio was 1:1. Enough about metals, though. We'll be dealing almost entirely with non-metals.

Boron:

Boron is of some importance. When I reach material that deals with boron, I'll give more details on boron. For now, just note that boron has three valence electrons (it has two other electrons in a lower orbital, and only valence electrons are used in bonding). So boron will form three bonds. When these bonds are to other non-metals, they're generally covalent bonds. Covalent bonds are links between atoms generated by sharing of valence electrons. Boron forms three.

Hydrogen:

Hydrogen is a very simple case. Hydrogen atoms can bond to only one atom each. That is, each hydrogen atom can form only one bond. If two hydrogen atoms are bound to each other, it's a molecule of hydrogen gas. But most of the bonds we'll be seeing between hydrogen and other elements will be with hydrogen and carbon, nitrogen, or oxygen. Again, the rule for hydrogen is simple: hydrogen can only form one bond. Hydrogen can also form ions, but we'll deal with those later.

Carbon:

Here's where things get more complicated. Carbon has four valence electrons and forms four bonds. That means any given carbon atom could easily be bonded to four other atoms. But that's using only sigma bonding. There's also pi bonding. Rather than worry about that for now, just remember that double and triple bonds are also possible. So a carbon atom can be bonded to two, three, or four other atoms. Two bonds would mean that is forming either a triple bond and a single bond or two double bonds. Three bonds would mean that the carbon is forming a double bond and two single bonds. Four bonds would mean that it has single bonds to four different atoms.

A double or triple bond to hydrogen is impossible. What I said earlier about hydrogen only forming one bond also excludes double and triple bonds (those require electrons too). But carbon is capable of forming bonds to other carbon atoms, single, double or triple. Long chains or rings are possible. It's this versatility that makes organic chemistry unique.

Nitrogen:

Nitrogen has five valence electrons. One pair will always stay with the atom, so it can form up to three bonds. A nitrogen atom with a triple bond to another nitrogen atom forms a molecule of nitrogen gas, and you should know that this gas makes up most of the air you breathe. Triple bonds between nitrogen and carbon are also possible, as are double and single bonds.

Oxygen:

Oxygen has six valence electrons. Two pairs will always stay with the atom, so it can form two bonds, either two single bonds or one double bond. No triple bonds are possible with oxygen. Oxygen double-bonded to oxygen forms a molecule of oxygen gas, which makes up most of the rest of the air you breathe (the part that isn't nitrogen).

The halogens:

The halogens (the only ones that matter, anyway) are fluorine (F), chlorine (Cl), bromine (Br), and iodine (I). The differences will eventually come up, but as far as the fundamentals go, they're all interchangeable and when using atomic symbols to represent atoms, "X" in organic chemistry means one of these elements. They have seven valence electrons. Three pairs will always stay with the atom. One electron can participate in covalent bonding.

Silicon:

We won't be using silicon much. For now, all you need to remember is that, like carbon, silicon is tetravalent. Again, this means that it forms up to four bonds.

Phosphorus, and sulfur:

These two get a bit tricky. Phosphorus behaves a lot like nitrogen and sulfur behaves a lot like oxygen, but they can do other things too. These elements can form more than four bonds. Even though phosphorus will usually form three like nitrogen and sulfur will usually form two like oxygen, both can, in certain situations, form several bonds. So while you should expect not to see a carbon with five bonds to it, this can totally happen with these two elements.

That's all for now. I should probably cover some more, but I want to post this now.