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Carbon monoxide is a simple diatomic molecule that illustrates how two different atoms interact to form molecular orbitals (MO). The oxygen atom and the carbon atom have an s and three p orbitals each. For clarity, we draw the atomic orbitals of oxygen in red, and those on carbon in black (see below).
In order to be able to determine how many lone pairs are present in a carbon dioxide molecule, you need to draw its Lewis structure. Carbon dioxide has a total of 16 valence electrons, 4 from carbon and 6 from each of the two oxygen atoms. In order to give the central carbon atom a complete octet, you need to form two double bonds with the two oxygen atoms. These bonds will account for 8 of the 16 valence electrons the molecule has.