Lewis Structures Formal Charge

Lewis Structures Formal Charge - LEWIS STRUCTURES General...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
LEWIS STRUCTURES General Rules for Drawing Lewis Structures 1. All valence electrons of the atoms in Lewis structures must be shown. 2. Generally electrons are paired. Unpaired electrons are observed in odd electron molecules such as NO and NO 2 . 3. Generally each atom acquires eight electrons in its valence shell except hydrogen acquires only two electrons. 4. Multiple bonds (double and triple bonds) can be formed by C, N, O, P, and S. 5. Hydrogen atoms are terminal atoms. Hydrogen can accommodate a maximum of two electrons in its valence shell. It can therefore only make one bond to one other atom. There are only very few exceptions to this rule (for example, diborane, B 2 H 6 , shown in Fig. 18.9, Pg. 879 of your text). 6. Central atoms are generally less electronegative then terminal atoms. For example, HCN is more stable than HNC because carbon is less electronegative then nitrogen. Carbon atoms are generally central atoms. Oxygen has a relatively high electronegativity and is observed to be a terminal atom in many molecules. In alcohols, the –O–H group is attached to a carbon and eventhough hydrogen is less electronegative it must be a terminal atom. Also, in peroxides such as hydrogen peroxide, H 2 O 2 , the oxygen atoms are in the center (H–O–O–H). 7.
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 08/06/2008 for the course CHEM 1C taught by Professor Hooker during the Summer '06 term at UCSB.

Page1 / 2

Lewis Structures Formal Charge - LEWIS STRUCTURES General...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online