For most of organic chemistry reactions, octet rule is followed (notable exceptions are carbenes and nitrenes). The octet rule states that atoms are stable when they are surrounded by exactly 8 electrons (for hydrogen, it's two).
Oxygen has 6 valence electrons in atomic state. The net charge on the atom is zero.
Oxygen shares its electrons with other atoms to obtain an octet configuration. For example in a water molecule, water shares one of its electron with hydrogen. By doing so, oxygen can get the hydrogen atom's electron in return. There are 4 bonding electrons (2 $\ce{-OH}$ bonds) and 4 lone pairs on the oxygen. This gives oxygen an octet configuration around the atom. The oxygen owns 4 of its lone pairs and half of the bonding pairs (2 in this case). It has 6 electrons. A neutral oxygen atom owns 6 electrons.
Consider the case you have shown. There are 3 bond pairs (6 bonding electrons: two $\ce{-OH}$ bonds and one $\ce{-OC}$ bond) and one lone pair.
The oxygen has a total of 8 electrons surrounding it. The octet rule is satisfied. However, it does not own 6 electrons. It owns the lone pair (2 electrons) and half of the bonding electrons, i.e: 3. You get a total of 5 electrons. A neutral oxygen molecule owns 6 electrons. As the atom is one short of an electron, it is unit positively charged.