It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. It does not adequately predict the line spectrum of hydrogen. It does not adequately predict the ionization energy of the 1st energy level electrons for one-electron species for elements other than hydrogen. It shows the electrons to exist outside of the nucleus. E. None of these 5.
Atomic radius decreases across a row and increases down a period.
F must be the smallest, as it is at the upper right hand corner of the periodic table. S is lower in Group VI than O, so it is larger. The statement that the 1st ionization energy for an oxygen atom is lower than the first ionization energy for nitrogen is A. consistent with the general trend relating changes in ionization energy across a period from left to right because it is easier to take an electron from an oxygen atom than from a nitrogen atom. B. consistent with the general trend relating changes in ionization energy across a period from left to right because it is harder to take an electron from an oxygen atom than from a nitrogen atom. C. inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that the oxygen atom has two doubly occupied 2p orbitals and nitrogen has only one.