First of all, all electrons of any atom are in orbitals. Second, an ionic bond can be defined as one which is depends only on distance between charges, NOT direction. So, in fact there are very few compounds which are 100% ionic. Most have some directional (covalent) characteristic to the bonds. A great example of this is HCl. In water, it is 100% ionized and most consider it ionic, but in the gas phase it is a covalent molecule. The hydrogen cation is just too small to be purely ionic in condensed phases (fluids, solids), so while I have no direct knowledge of what the HCl crystal structure is (as a solid), I can be confident that it exhibits mostly covalent character.
It is wrong to consider molecules as being un-ionized, just as it is wrong to consider ions as not having covalent bonds. The carbonate anion, CO3(-2) has three covalent bonds and ammonium hydroxide ("ionic") has 5 covalent bonds. On a more advanced level, the charge on an ion or on a molecule can either be localized to one atom or spread over many atoms (via covalent bonds). Carbonate has three equivalent oxygen atoms (in some environments), each having -⅔ charge. This doesn't make sense until you learn a bit about quantum mechanics (simplistically, you can consider these charges to be averages over time, although that is only approximately right). In other environments, the CO3 ion will behave like O=C(O⁻)₂ with two types of oxygen. So, how do you tell? First compare the electronegativity of the atoms, also consider the oxidation state the atoms are in and finally then consider the bonding between atoms as well as their stereochemistry and environment. Except for VERY simple examples, even the experts have to rely on x-ray crystallography (or now days on quantum mechanical calculations which might require supercompeters and a lot of time) to establish the location of charge centers. In other words, even the experts can't just figure it out based on any simple rules or on their experience (although these experts will already KNOW many many of these examples, having learned them on their way to becoming experts).
Oh, in case you haven't learned about orbitals, only the s (atomic) orbitals are "directionless" (spherically symmetric), so the fact that all electrons are in one orbital or another implies that their "directionality" depends on the orbital they are in. This is heavy duty quantum mechanics, so don't sweat it too much. A beginning student should be learning about the simple cases where these types of facts don't have to be discussed. But only for the most simple metal-nonmetal diatomic compounds is determination of their ionic nature easy. And as I already implied, ionicity depends on pressure, temperature, and other things in the environment, NOT just on the nature of the atoms.