I am currently teaching myself AP Chemistry, so am at a very basic level still.
I am studying chemical bonds now, but am wondering why the orbitals don't make a difference to the way atoms bond.
To explain further: Oxygen has 6 valence electrons, and so when drawing the Lewis dot structure, you would draw it with 2 pairs of electrons and two single electrons. This seems consistent with the orbitals of an Oxygon atom, because it has 1 pair of electrons in the 3s orbital, another pair in one of the 3p orbitals, and 2 single electrons in each of the remaining 3p orbitals. This also makes sense to me in terms of and Oxygen atom forming a covalent bond with another Oxygen atom, since the two single electrons in each of the remaining 3p orbitals will "hang out" together, completing the octet rule for the valence shell of both atoms.
But when I looked up the Lewis dot structure for Carbon, I felt confused. It seems to be drawn with 4 single electrons . This feels inconsistent with what we know about the orbitals of a Carbon atom. Given that there are 4 valence electrons, with 1 pair in the 3s orbital, and 2 more single ones in each of two of the 3p orbitals, surely we should draw it as: 1 pair of electrons, 2 single electrons.
But we draw it as 4 single electrons. I know I am probably being really daft and missing something obvious, but please can someone help explain a bit more about why we draw it this way? And why the orbitals' pairs don't seem to matter when it comes to bonds?
Thanks