Expanded octets As mentioned previously, the octet rule works best for the elements in the second period Li through F of the periodic table. Some of the third-period elements Si, P, S, and Cl can bond to more than four atoms, and thus need to involve more than the four pairs of electrons available in an s2p6 octet.
Mon May 24 I am a Biology teacher assigned a chemistry class and I cannot find the answer to the questions posed above. I have a pretty good idea about drawing the Lewis structures for both of these ions, but I don't know how to determine which one has a coordinate covalent bond.
Lewis structures for almost anything can be found by following a few simple rules. The structures for ClO- hypochlorous ion and ClO2- clorous ion are quite simple and are shown above, left. Notice that these Lewis structures show all atoms with an octet.
One could, I suppose, use an "expanded octet" structure for chlorous ion as well; such a structure is shown at right.
Nevertheless, the structures which preserve 8-electron octets are more valuable for determining which compound has a "coordinate" covalent bond, because such a bond is defined as one formed from electrons "belonging" to only one of the atoms. You will also notice that in every case the electron donor atom is assigned a single formal positive charge for each pair of electrons donated.
So the clue to finding coordinate covalent bonds within Lewis structures is to look for formal positive charges: For more on this, see one of my recent answers.Dot structures and molecular geometry. Drawing dot structures. Practice: Counting valence electrons.
Formal charge and dot structures. Resonance and dot structures.
This is the currently selected item. VSEPR for 2 electron clouds. VSEPR for 3 electron clouds. More on the dot structure for sulfur dioxide.
Feb 12, · A simple method for drawing Lewis electron dot structures for chlorine dioxide clo2 is given in this post. A simple procedure for writing Lewis structures was given in a previous article entitled “Lewis Structures and the Octet Rule”.
Write Lewis structures that obey the octet rule (a) POCl3, SO, XeO4, PO, ClO4- (b) NF3, SO, PO, ClO3- (c) ClO2-, SCl2, PCl2- (d) Considering your answers to parts a, b, and c, what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons?
• Structures with lower formal charges can be.
achieved by forming an extended octet. Example: Write the Lewis structure of XeF4. ntot = 8(Xe) + 4×7(F) = nrem = 36 - 8 = 28 nneed = 0(Xe) + 4×6(F) = nneed.
ClO2, chlorine dioxide, can be illustrated in a Lewis structure by writing Cl with O on both sides, separated by double bond dashes.
Cl has two dots above with one below, and the Os have two dots on their tops, bottoms and outer edges in the basic version, though variants are possible.
A Lewis structure is a diagram showing the chemical components of a substance. Only one is required to show how CO2 bonds. CO2 contains 2 double bonded oxygen atoms o apart .