The question is incomplete, the complete question is;
Draw Lewis structures for the following compounds/ions.
Decide if the compound/ion listed can satisfy the octet rule (duet rule for H), if so choose Satisfies Octet Rule from the drop down menu.
If the compound/ion cannot satisfy the octet rule for one of the atoms in the formula, choose one of the following three reasons why;
Too many valence electrons (more than eight), Too few valence electrons (fewer than eight), or Odd # of valence electrons.
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons KrCl2
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons PCl3
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons BeH2
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons NO3-
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons SeO22-
Satisfies Octet Rule Too many valence electrons Too few valence electrons Odd # of valence electrons SO2
Answer:
See explanation
Explanation:
Let us consider the number of valence electrons in each of the species. This will let us know whether the specie satisfies the octet rule or not.
KrCl2 has a total of 22 valence electrons. This implies that there are too many valence electrons hence the compound does not satisfy the octet rule.
For PCl3, there are 26 valence electrons. This compound satisfies the octet rule.
For BeH2, there are four valence electrons. This number of valence electrons is too few hence BeH2 does not satisfy the octet rule.
NO3^- has 24 valence electrons and is represented using resonance structures. Its resonance structures show that the specie satisfies the octet rule.
SeO2^2- has 20 valence electrons. This specie satisfies the octet rule.
SO2 has 18 valence electrons and is represented by resonance structures which satisfy the octet rule.
