chemistry

Method for Lewis dot structures: The nitrate ion Home > Lewis structures and the Octet rule > Lewis Electron Dot Structure of nitric acid HNO 3 > Lewis Structures for nitrogen oxychloride NOCl > Method for Lewis dot structures: The nitrate ion lewis structures NO 3 -   Method for Lewis dot structures: The nitrate ion NO 3 -   A simple procedure for writing Lewis Dot Structures was given in a previous article entitled “Lewis Structures and the Octet Rule” . Several worked examples relevant to this procedure were given in previous posts please see the Sitemap - Table of Contents (Lewis Electron Dot Structures). Let us consider the case of the nitrate ion NO 3 - . What are the Lewis electron dot structures of NO 3 - ? Step 1 : Connect the atoms with single bonds.     Step 2 : Calculate the # of electrons in π bonds ( multiple bonds ) using  f...

A simple procedure for writing Lewis Structures was given in a previous article entitled “Lewis Structures and the Octet Rule”. Several worked examples relevant to this procedure were given in previous posts please see the Sitemap - Table of Contents (Lewis Electron Dot Structures). Let us consider the case of the allylic carbocation: C 3 H 5 + Step 1 : Connect the C atoms with single bonds and add H atoms so that an octet of electrons exists around each atom: Fig. 1:   The atoms connected with single bonds in the “initial” structure Step 2 :  Calculate the # of electrons in π bonds (multiple bonds) using   formula (1) : Where n in this case is 3, excluding the H atoms. Where V = (4 + 3 + 4 + 2 + 4 +2) – 1 = 18 , V is the number of valence electrons of the molecule. Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 18 = 2     So, there is one double bond in the molecule. Step 3 & 4 : The   resonance structures of the allylic carbocation are as fol...

Let’s consider the following carbocations and rank them in terms of their stability :   Fig. 1: Carbocation 1 is stabilized by the –OCH 3   substituent   since it is electron donating. The + charge is delocalized and the carbocation is stabilized. Carbocation 2 is destabilized by the electron withdrawing substituent NO 2 . By drawing the resonance structure we see that there are two adjacent positive charges. This resonance structure is highly unfavorable! The substituent (-OCH 3 ) stabilizes carbocation 1 by resonance and the resulting charge delocalization. The + charge is delocalized to the O atom. The substituent (-NO 2 + ) in carbocation 2 is electron-withdrawing and the carbocation is destabilized. Notice the two adjacent + charges. In general, carbocations are destabilized by neighboring electron-withdrawing groups if: Contain an atom more electronegative than C There is no atom with an electron pair that is directly attached to the carbocation (-CF 3 , -CCl 3...