how is the electron configuration consistent with Na3As,AsCl3,AsF5?
1 type s orbital → max 2 electrons 3 type p orbitals → max 6 electrons 5 type d orbitals → max 10 electrons 7 type f orbitals → max 14 electrons 9 type g orbitals → max 18 electrons The octet rule refers to the tendency of atoms to prefer to have eight electrons in their valence shellWhen atoms have less than eight electrons, they tend to react and form more stable compoundsThe main exception to the rule is hydrogen, which is at its lowest energy when it has two electrons in its valence shellHelium (He) is similar in that it, too, only has room for two electrons in its only valence shellOther notable exceptions are aluminum and boron, which can function well with six valence electrons, and some atoms beyond group three on the periodic table that can have over 8 electrons, including sulfurThese atoms have empty d sublevel orbitals in which more electrons can existAs [Ar] 3d^10 4s^2 4p^3 Thus, in the ground state, Arsenic lacks 3 valence electrons (from 4p orbitals)As a result, for every As atom there should be 3 sodium atoms(Na)Na [Ne] 3s1 sodium will lose 1 valence electron (from 3s orbital) to become stableThus, there will be 3 valence electrons gained by As from Na (x3) to achieve a full octet configuration (i.e8 electrons in the valence shells)it's the same with AsCl3 the halogen atom, chlorine lacks one valence electron; Cl [Ne] 3s2 3p5 (1 valence electron missing in the 3p orbital) F 1s2 2s2 2p5 (1 valence electron missing in the 3p orbital) thus, Cl will gain one valence electron from arsenic to become stable(octet)AsF5 is an exceptionHere, As loses 5 of its valence electrons (4s2 and 4p3) to 5 chlorine atoms F 1s2 2s2 2p5 (1 valence electron missing in the 3p orbital, thus 5 x Cl 5 valence electrons needed) hope this helps:-)
