Method of drawing the Lewis Structures of N5+ - #29

A simple procedure for writing Lewis structures is given in a previous article entitled “Lewis Structures and the Octet Rule”. Relevant worked examples were given in the following articles: Examples #1, #2, #3 , #4, #5, #6,  #7,  #8, #9, #10, #11, #12, #13, #14,  #15, #16, #17, #18, #19, #20, #21, #22,  #23,  #24, #25, #26, #27 and #28.

Let us consider the case of  the pentazenium or pentanitrogen N₅⁺ cation. This highly explosive cation was first synthesized and isolated as a salt by K.O. Christie in 1999 by the reaction of  N₂F⁺     with HN₃ . The N₅⁺ cation was the first new all nitrogen species to be synthesized in isolable quantities in more than a century, and only the third ever produced. Prior to this nitrogen cation only molecular N₂ , isolated in 1772 and the azide ion N₃^- , first synthesized in 1890, had ever been isolated. The overall objective of Christie's research was the synthesis and characterization of polynitrogen, high-nitrogen and high-oxy gen energetic materials, useful as propellants or explosive ingredients.

Step 1: Connect the atoms with single bonds.

Fig. 1: Connecting the atoms of  the  N₅⁺ cation with single bonds

Step 2: Calculate the # of electrons in π bonds (multiple bonds) using  formula (1): 

Where n in this case is 5 since N₅⁺ consists of 5 atoms.

Where V = (5 * 5 ) - charge  = 25 – 1 = 24, V is the number of the valence electrons in the ion.

Therefore, P = 6n + 2 – V = 6 *5 + 2 – 24 = 8   \  there are: 1) either 4 double bonds   2)  or 2 triple bonds   3) or 1 triple and 2 double bonds.

Step 3 & 4: The Lewis structure of N₅⁺  is as follows:

Figure 2:  Lewis electron dot structures for the N₅⁺ ion.  The least plausible structures are #1 (+ charges adjacent to each other) and #3 (large charge separation).

Therefore, five resonance electron dot structures were derived for the N₅⁺ion.

Lewis Dot Structure Method: Example diphosphene P2H2 - #28

A simple procedure for writing Lewis structures is given in a previous article entitled “Lewis Structures and the Octet Rule”. Relevant worked examples were given in the following articles: Examples #1, #2, #3 , #4, #5, #6,  #7,  #8, #9, #10, #11, #12, #13, #14,  #15, #16, #17, #18, #19, #20, #21, #22,  #23,  #24, #25, #26 and #27.

Let us consider the case of diphosphene P₂H₂

 Step 1: Connect the atoms with single bonds. 

Fig. 1: Connecting the atoms of P₂H₂  with single bonds

Step 2: Calculate the # of electrons in π bonds (multiple bonds) using  formula (1): 

Where n in this case is 2 since P₂H₂ consists of 4 atoms but two of them are hydro gen.

Where V = (1 + 5 + 5 + 1 )  = 12  

Therefore, P = 6n + 2 – V = 6 *2 + 2 – 12 = 2    So there is one double bond and therefore the structure in Step 1  has one double bond.

Step 3 & 4: The Lewis structure of P₂H₂  is as follows:

Figure 2: Lewis structure for diphosphene, P₂H₄