2015年5月2日 · When solving the lewis structure for the $\ce{ClO2-}$ ion, taking into consideration formal charges, the structure is represented as: A lewis model with 2 double bonds also fits the formal charge and lewis model requirements, however this time the negative formal charge would be on the chlorine atom.

2014年7月15日 · For "ClO"_2^"-", "Cl" is the less electronegative atom. So, "Cl" is the central atom The skeleton structure is "O-Cl-O". The trial structure is You have 20 valence electrons in your trial structure. The valence electrons you have available are: "1 Cl + 2 O + 1 e" = 1×7 + 2×6 + 1 = 20. Hence, the trial structure has the correct number of ...

The percentage value gives an estimate how close the given conformation is to an idealised Lewis structure. From this you could also derive how much such a structure would contribute to a resonance situation (in terms of Valence Bond theory). What we do see here is, that the electronic structure is better described with more formal charges.

2017年12月16日 · Well we has got..... 7_"Cl"+2xx6_"O"+1_"negative charge"=20*"valence electrons" to distribute across 3 centres...

2015年11月27日 · Both have a charge of -1. This is the nitrite ion, in Lewis structure form. Notice how one oxygen has 6 valence electrons and the nitrogen ion has 5 valence electrons and are paired with that many electrons, so they both have formal charges of 0. The other oxygen, on the other hand, is assigned 7 electrons so its formal charge is 6-7, or -1. This leaves the nitrite ion …

2016年10月8日 · These try to depict the electronic structure of ClO^- anion. In fact the given diagram is highly misleading and ambiguous. The valence electrons around the chlorine atom were depicted. Why should only the chlorine-based electrons be? As written, the chlorine atom is neutral. A similar depiction should have been given around oxygen, and here a formal …

2014年7月13日 · Yes, the chlorate ion has three major contributors to the resonance hybrid. We can write three important equivalent Lewis structures for the chlorate ion.

In class, we learned about the Lewis structure of some elements such as carbon, but we didn't learn how to do the Lewis structure of cations and anions. Do we just draw the number of electrons in the ion, or do we do something different? So for example, what would be the Lewis structure of $\ce{Li+}$ and $\ce{Li-}$? How would you draw it out?

2016年7月30日 · In both examples, the chlorine atom is neutral, and the charge is presumed to reside on oxygen. For Cl, and O, there are 7, and 6 valence electrons respectively associated with the neutral atoms. For hypochlorite ion, Cl-O^-, we have to distribute 7+6+1 electrons in the Lewis structure. There are thus 7 electron pairs. One of these electron pairs is conceived to form the …

Chlorite ion features a unusual III^+ oxidation state with respect to the chlorine, and a bent structure based on a tetrahedron (i.e. 2 lone pairs on Cl). As O=Cl-O^-, the doubly bound oxygen and the chlorine are neutral. The other O has a formal negative charge. From left to right, there are 8 electrons associated with the oxygen (6 valence and 2 inner core) and hence neutral as …