Textbook Question
Draw the Lewis structure for each organic compound from its condensed structural formula. b. CH3OCH3
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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 99
Draw the Lewis structure for each organic compound from its condensed structural formula. a. C2H4 b. CH3NH2 c. HCHO d. CH3CH2OH e. HCOOH
Verified step by step guidance1
Identify the total number of valence electrons for each compound by adding the valence electrons of each atom present in the formula.
For each compound, determine the central atom (usually the least electronegative atom, except hydrogen) and arrange the other atoms around it.
Draw single bonds between the central atom and surrounding atoms, using a pair of electrons for each bond.
Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the outer atoms and then the central atom. Remember that hydrogen only needs two electrons.
If any atoms do not have a complete octet, consider forming double or triple bonds by sharing more pairs of electrons between atoms.
Related Practice
Textbook Question
Draw the Lewis structure for each organic compound from its condensed structural formula. c. CH3COCH3
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Textbook Question
Draw the Lewis structure for each organic compound from its condensed structural formula. e. CH3CHO
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Textbook Question
Use Lewis structures to explain why Br3- and I3- are stable, while F3- is not.
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Open Question
Draw the Lewis structure for HCSNH2. The carbon and nitrogen atoms are bonded together, and the sulfur atom is bonded to the carbon atom. Label each bond in the molecule as polar or nonpolar.
Textbook Question
Draw the Lewis structure for urea, H2NCONH2, one of the compounds responsible for the smell of urine. (The central carbon atom is bonded to both nitrogen atoms and to the oxygen atom.) Does urea contain polar bonds? Which bond in urea is most polar?
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