Valence electrons octet rule. Lewis structure Lewis structures

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2 Lewis Dot Diagrams Valence electrons are the electrons in the outermost energy level of an atom. An element with a full octet of valence electrons has a stable configuration. The tendency of bonded atoms to have octets of valence electrons is called the octet rule. A Lewis structure is a structural formula in which valence electrons are represented by dots. In Lewis structures, dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.

3 Electron Dot Notation 1) Find the element s # of Valence Electrons by looking at its Group #. 2) Write the element s chemical symbol. 3) Starting at the top and moving clockwise, add valence electrons until all sides are filled. 4) If each side is filled, begin pairing the electrons.

4 Lewis Structures Lewis structures are representations of molecules showing all electrons, bonding and nonbonding.

5 Writing Lewis Structures 5 PCl 3 + 3(7) = Find the sum of valence electrons of all atoms in the polyatomic ion or molecule. If it is an anion, add one electron for each negative charge. If it is a cation, subtract one electron for each positive charge.

6 Writing Lewis Structures Keep track of the electrons: 2. The central atom is the least electronegative element (that isn t hydrogen). Connect the outer atoms to it by single bonds. 26 (total from P + 3Cl) 6 (2 from each single bond) = 20

7 Writing Lewis Structures 3. Fill the octets of the outer atoms. Keep track of the electrons: 26 6 = (lone pairs around Cl atoms) = 2

8 Writing Lewis Structures 4. Fill the octet of the central atom. Keep track of the electrons: 26 6 = = 2 2 (lone pairs on P) = 0

9 Writing Lewis Structures 5. If you run out of electrons before the central atom has a full octet form multiple bonds until it does.

10 Resonance Resonance is a way of describing delocalized electrons within certain molecules or polyatomic ions where the bonding cannot be expressed by one single Lewis Diagram. Delocalized electrons are (essentially) those that are shared covalently by more than 2 adjacent nuclei.

11 Resonance In truth, the electrons that form the second C O bond in the double bonds below do not always sit between that C and that O, but rather can move among the two oxygens and the carbon. They are not localized, but rather are delocalized.

12 Resonance This is the Lewis structure we would draw for ozone, O

13 Resonance But this is at odds with the true, observed structure of ozone, in which both O O bonds are the same length. both outer oxygens have a charge of 1/2.

14 Resonance One Lewis structure cannot accurately depict a molecule such as ozone. We use multiple structures, resonance structures, to describe the molecule.

15 Resonance Just as green is a synthesis of blue and yellow ozone is a synthesis of these two resonance structures.

16 How many resonance structures can be drawn for NO 3 -?

17 How many resonance structures can be drawn for NO 3 -?

18 Resonance The organic compound benzene, C 6 H 6, has two resonance structures. It is commonly depicted as a hexagon with a circle inside to signify the delocalized electrons in the ring.

19 Exceptions to the Octet Rule There are three types of ions or molecules that do not follow the octet rule: Ions or molecules with an odd number of electrons. Ions or molecules with less than an octet. Ions or molecules with more than eight valence electrons (an expanded octet).

20 Odd Number of Electrons Though relatively rare and usually quite unstable and reactive, there are ions and molecules with an odd number of electrons. Such as: ClO 2, NO, NO 2, & O 2 -

21 Fewer Than Eight Electrons Consider BF 3 : Giving boron a filled octet places a negative charge on the boron and a positive charge on fluorine. This would not be an accurate picture of the distribution of electrons in BF 3.

22 Fewer Than Eight Electrons Filling boron s octet results in a negative charge on boron and a positive charge on the fluorine, which is much more electronegative. Therefore, the structures that put a double bond between boron and fluorine are much less important than the one that leaves boron with only 6 valence electrons.

23 Fewer Than Eight Electrons The lesson is: If filling the octet of the central atom results in a negative charge on the central atom and a positive charge on the more electronegative outer atom, don t fill the octet of the central atom.

24 More Than Eight Electrons The only way PCl 5 can exist is if phosphorus has 10 electrons around it. It is allowed to expand the octet of atoms on the 3rd row or below. Presumably d orbitals in these atoms participate in bonding.

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