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Electron Distribution in Molecules

G. N. Lewis 1875 - 1946. Electron Distribution in Molecules. Electron distribution is depicted with Lewis (electron dot) structures This is how you decide how many atoms will bond covalently! (In ionic bonds, it was decided with charges). ••. H. Cl. •. •. ••. lone pair (LP).

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Electron Distribution in Molecules

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  1. G. N. Lewis 1875 - 1946 Electron Distribution in Molecules • Electron distribution is depicted withLewis (electron dot) structures • This is how you decide how many atoms will bond covalently! (In ionic bonds, it was decided with charges)

  2. •• H Cl • • •• lone pair (LP) shared or bond pair Bond and Lone Pairs • Valence electrons are distributed as shared orBOND PAIRS and unshared orLONE PAIRS. This is called a LEWIS structure.

  3. •• •• Cl H H Cl • • + • • •• •• Bond Formation A bond can result from anoverlapof atomic orbitals on neighboring atoms. Overlap of H (1s) and Cl (2p) Note that each atom has a single, unpaired electron.

  4. Review of Valence Electrons • Remember from the electron chapter that valence electrons are the electrons in the OUTERMOST energy level… that’s why we did all those electron configurations! • B is 1s2 2s2 2p1; so the outer energy level is 2, and there are 2+1 = 3 electrons in level 2. These are the valence electrons! • Br is [Ar] 4s2 3d10 4p5How many valence electrons are present?

  5. Review of Valence Electrons Number of valence electrons of a main (A) group atom = Group number

  6. Steps for Building a Dot Structure Ammonia, NH3 1. Decide on the central atom; never H. Why? If there is a choice, the central atom is atom of lowest affinity for electrons. (Most of the time, this is the least electronegative atom…in advanced chemistry we use a thing called formal charge to determine the central atom. But that’s another story!) Therefore, N is central on this one 2. Add up the number of valence electrons that can be used. H = 1 and N = 5 Total = (3 x 1) + 5 = 8 electrons / 4 pairs

  7. H H N H •• H H N H Building a Dot Structure 3. Form a single bond between the central atom and each surrounding atom (each bond takes 2 electrons!) 4. Remaining electrons form LONE PAIRS to complete the octet as needed (or duet in the case of H). 3 BOND PAIRS and 1 LONE PAIR. Note that N has a share in 4 pairs (8 electrons), while H shares 1 pair.

  8. •• H H N H Building a Dot Structure • Check to make sure there are 8 electrons around each atom except H. H should only have 2 electrons. This includes SHARED pairs. 6. Also, check the number of electrons in your drawing with the number of electrons from step 2. If you have more electrons in the drawing than in step 2, you must make double or triple bonds. If you have less electrons in the drawing than in step 2, you made a mistake!

  9. Carbon Dioxide, CO2 1. Central atom = 2. Valence electrons = 3. Form bonds. C 4 e-O 6 e- X 2 O’s = 12 e-Total: 16 valence electrons This leaves 12 electrons (6 pair). 4. Place lone pairs on outer atoms. 5. Check to see that all atoms have 8 electrons around it except for H, which can have 2.

  10. Carbon Dioxide, CO2 C 4 e-O 6 e- X 2 O’s = 12 e-Total: 16 valence electrons How many are in the drawing? 6. There are too many electrons in our drawing. We must form DOUBLE BONDS between C and O. Instead of sharing only 1 pair, a double bond shares 2 pairs. So one pair is taken away from each atom and replaced with another bond.

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