Alkanes contain strong carbon-carbon single bonds and strong carbon-hydrogen bonds. The carbon-hydrogen bonds are only very slightly polar and so there aren't any bits of the molecules which carry any significant amount of positive or negative charge which other things might be attracted to.
For example, you will find (or perhaps already know) that many organic reactions start because an ion or a polar molecule is attracted to a part of an organic molecule which carries some positive or negative charge. This doesn't happen with alkanes, because alkane molecules don't have this separation of charge.
The net effect is that alkanes have a fairly restricted set of reactions.
burn them - destroying the whole molecule;
react them with some of the halogens, breaking carbon-hydrogen bonds;
crack them, breaking carbon-carbon bonds.
These reactions are all covered on separate pages if you go to the alkanes menu (see below).
Cycloalkanes are very similar to the alkanes in reactivity, except for the very small ones - especially cyclopropane. Cyclopropane is much more reactive than you would expect.
The reason has to do with the bond angles in the ring. Normally, when carbon forms four single bonds, the bond angles are about 109.5°. In cyclopropane, they are 60°.
With the electron pairs this close together, there is a lot of repulsion between the bonding pairs joining the carbon atoms. That makes the bonds easier to break.
The effect of this is explored on the page about reactions of these compounds with halogens which you can access from the alkanes menu below.