1. 10.7.00 6:16 PM 1 Lewis Structure Tutorial Drawing Lewis Structures A Tutorial on Writing Lewis Dot Structure

2. 10.7.00 6:16 PM 2 Lewis Structure Tutorial Lewis Structure by Bond Determination 1. Know how to determine the valence electrons for all elements. 2.(Connectivity) From the chemical formula, determine the atom connectivity for the structure. i. Given a chemical formula, AB n, A is the central atom and B flanks the A atom. i.e., NH 3, NCl 3, NO 2. In these examples, N is central in the structure. ii. H and F are never central atoms. 2.(# of electrons in Bonding) Determine the number of bonds in the compound, by calculating the theoretical Octet electrons (Oe) minus the total valence electrons (TVe) and dividing by 2 (2 electrons = 1 bond). Oe is the theoretical number of electrons necessary for each atom in the structure to obtain a Noble Gas electron configuration, while TVe is the actual number of total valence electron for each atom in the structure. 3.(Remaining e-) Calculate the number of remaining electrons in the compound by taking the total valence electron (TVe) minus the number of electrons that was used to form bonds.

3. 10.7.00 6:16 PM 3 Lewis Structure Tutorial Valence electrons for Elements Recall that the valence electrons for the elements can be determined based on the elements position on the periodic table. Lewis Dot Symbol

4. 10.7.00 6:16 PM 4 Lewis Structure Tutorial Valence electrons and number of bonds Number of bonds elements prefers depending on the number of valence electrons. In general - X Family  # Covalent Bonds* Halogens F, Br, Cl, I Calcogens O, S Nitrogen N, P Carbon C, Si  O N C    1 bond often 2 bond often 3 bond often 4 bond always The above chart is a guide on the number of bonds formed by these atoms.

5. 10.7.00 6:16 PM 5 Lewis Structure Tutorial Lewis Structure, Octet Rule Guidelines When compounds are formed they tend to follow the Octet Rule. Octet Rule: Atoms will share electrons (e - ) until it is surrounded by eight valence electrons. Rules of the (VSEPR) game- i) O.R. works mostly for second period elements. Many exceptions especially with 3rd period elements (d-orbitals) ii) H prefers 2 e - (electron deficient) iii) :C:N::O::F: 4 unpaired 3unpaired2unpaired1 unpaired up = unpaired e- 4 bonds3 bonds2 bonds1 bond O=C=ON  NO = OF - F iv) H & F are terminal in the structural formula (Never central)........

6. 10.7.00 6:16 PM 6 Lewis Structure Tutorial Atomic Connectivity The atomic arrangement for a molecule is usually given. CH 2 ClF HNO 3 CH 3 COOH H 2 Se H 2 SO 4 O 3 HC F Cl H H N OO O H O S O H O O OO O H C C O H H H O HSe H In general when there is a single central atom in the molecule, CH 2 ClF, SeCl 2, O 3 (CO 2, NH 3, PO 4 3- ), the central atom is the first atom in the chemical formula. Except when the first atom in the chemical formula is Hydrogen (H) or fluorine (F). In which case the central atom is the second atom in the chemical formula. Find the central atom for the following: 1) H 2 Oa) Hb) O2) PCl 3 a) Pb) Cl 3) SO 3 a) Sb) O4) CO 3 2- a) Cb) O 5) BeH 2 a) Beb) H6) IO 3- a) Ib) O

7. 10.7.00 6:16 PM 7 Lewis Structure Tutorial Setting up the bond table requires the chemical formula, and determining the number of electrons around each atom. A) Chemical Formula I.e., HNO 3 B) Oe - Octet Electrons. This is always either 8 or 2 (for H) C) Tve - Total Valence Electron. Setting up Bond Table ChemFormulaOctet e-Tot Val e- HNO 3 OeTve H N O 1 x 2 = 2 1 x 8 = 8 3 x 8 = 24 1 x 1 = 1 1 x 5 = 5 3 x 6 = 18 3424 Note this recipe works only if the chemical specie obeys the octet rule. For chemical specie which violates the octet rule, this method must be modified.

8. 10.7.00 6:16 PM 8 Lewis Structure Tutorial After setting up the bond table, calculate the number of bonds in the chemical specie and the number of electrons. The remaining electrons are place around the atoms in the chemical specie such that each atom obeys the octet rule Calculating the Number of Bonds and the Remaining electrons HNO 3 OeTve# Bonding e - Bond Table # of Bonds Remaining e - 34 - 24 = 10 10/2 = 5 Tve(24) - electrons in Bond (10) = 14

9. 10.7.00 6:16 PM 9 Lewis Structure Tutorial 1) Chemical formula: 2) Atomic sequence: HNO3 HNO3 HNO3 HNO3 3) Number of bonds = 5 4) Remaining electrons = 14 5) Lewis Structure with 5 bonds: 6) Complete Lewis Structure 6) Complete Lewis Structure with 14 remaining electrons Putting it Together H NOO O HNOO O HNOOO

10. 10.7.00 6:16 PM 10 Lewis Structure Tutorial Lewis Dot Structure of CO 2 by Bonds Table B. Calculate the number of bonds in compound structure. # bonds = (Oe - TVe) 2 = (24- 16) = 8 = 4 bonds 22 C. Calculate the remaining electrons to add to structure to complete Lewis dot structure. Remaining e- = TVe - e - used in bonding. = 16 - 8 = 8 e - Remaining Writing Lewis Structure: First determine atom connectivity keeping in mind that H and F can never be central atoms. Generally when given the formula, ABn, A is the central atom in the structure (but not always), and B atoms flank the central atom. Next use information from the above calculations. Total of 16e- in CO 2, of which 8 electrons are used to form 4 bonds and 8 remaining electrons are used to complete Lewis structure. OCO 6. Place the remaining 8 electrons in the structure to complete the Lewis Structure A. Calculate Octet electrons (Oe-) and Total Valence electrons to determine number of bonds CO 2 OeTVe 1 C1(8)= 81(4) = 4 2 O2(8)=162(6)=12 Chg 2416 1,2. Write atom connectivity for CO 2. 3,4,5. Draw the four bonds in the structure. OCOOCO

11. 10.7.00 6:16 PM 11 Lewis Structure Tutorial Lewis Dot Structure of ClO 4 - by Bonds Table B. Number of Bonds. # bonds = (40- 32) = 8 = 4 bonds 22 C. Remaining electrons. Remaining e- = 32 - 8 = 24 e - Remaining Writing Lewis Structure: 6. Place the remaining 24 electrons in the structure such that each atom has an octet to complete the Lewis Structure A. Calculate (Oe-) and (TVe) ClO 4 - OeTVe 1 Cl1(8)= 81(7) = 7 4 O4(8)= 324(6)= 24 Chg 1 4032 1,2. Write atom connectivity for ClO 4 -. 3.4.5. Draw the four bonds in the structure.

12. 10.7.00 6:16 PM 12 Lewis Structure Tutorial Lewis Structures: Examples Example a) CH 2 ClF b)SO 2 c)SO 4 2- d) H 3 PO 4 H P O O O O H H

13. 10.7.00 6:16 PM 13 Lewis Structure Tutorial SummarySummary Lewis Structure Determination: Molecular Formula Molecular Formula Atomic Sequence (H and F are terminal) Atomic Sequence (H and F are terminal) Determine the # of bonds Determine the # of bonds Oe - and TVe - # of Bonds = (Oe - TVe - ) / 2 Determine remaining electrons Determine remaining electrons Re = (TVe - ) - (# e - in bonding) Make sure all atoms satisfy octet rule (Except H which is satisfied with 2 electrons Make sure all atoms satisfy octet rule (Except H which is satisfied with 2 electrons )

14. Polarity-Unequal Sharing of Electrons Even though all atoms want the same number of electrons as the Noble Gases, some want to get or give them more than others. The magnitude of this attraction for electrons is called “Electronegativity”. The more electronegative an atom is, the more it wants the electrons. Some atoms want to gain electrons so bad, they take them altogether to form negative ions. Some want to lose them so bad that they become positive ions.

15. Examples of Polar and Non- Polar Compounds H 2 O Water is a bent molecule. The lone pair of electrons from the Lewis structure distorts its shape and it becomes a very polar molecule. NaCl Since Na is a metal it gives up its electron to form Na + and Cl takes the electron completely to form Cl -. HCl The Chlorine wants the electrons more than the Hydrogen. Thus we have +δ HCl -δ. Cl 2 (Cl—Cl) The Chlorine molecules want the electrons equally so they form a non-polar molecule with NO partial or full charges. CO 2 Carbon Dioxide is a linear molecule. It has no lone pairs of electrons from the Lewis structure. The two oxygen atoms pull equally and make it a non-polar molecule... :O:H ●● H.. O::C::O ●● ●●

16. Let’s Practice! Name the following. CaF 2 K2SK2S CoI 2 SnF 2 SnF 4 OF 2 CuI 2 CuI SO 2 SrS LiBr Strontium Sulfide Lithium Bromide Copper ( I ) Iodide or Cuprous Iodide Sulfur dioxide Copper ( II ) Iodide or Cupric Iodide Oxygen diflouride Tin ( IV ) Flouride or Stannic Flouride Tin ( II ) Flouride or Stannous Flouride Cobalt ( II ) Iodide or Cobaltous Iodide Potassium Sulfide Calcium Flouride

17. Polyatomic Ions (partial list from page 195 (193 2 nd edition)) Ammonium……………... Nitrate…………………… Permanganate………….. Chlorate………………… Hydroxide………………. Cyanide…………………. Sulfate…………………... Carbonate………………. Chromate……………….. Acetate………………….. Phosphate………………. NH 4 + NH 4 + NO 3 - NO 3 - MnO 4 - MnO 4 - ClO 3 - ClO 3 - OH - OH - CN - CN - SO 4 2 - SO 4 2 - CO 3 2- CO 3 2- CrO 4 2- CrO 4 2- C 2 H 3 O 2 - C 2 H 3 O 2 - PO 4 3- PO 4 3-

18. Acids (with H in front) Binary acids (without oxygen in formula) Hydro _________ ic Acid HCl Hydrochloric acid HBr Hydrobromic acid Oxy acids (with oxygen in formula) -ate goes to –ic and –ite goes to -ous HNO 3 Nitric acid HNO 2 Nitrous acid H 2 SO 4 Sulfuric acid H 2 SO 3 Sulfurous acid H 3 PO 4 Phosphoric acid H 3 PO 3 Phosphorous acid

19. Lets Practice! HF Na 2 CO 3 H 2 CO 3 KMnO 4 HClO 4 H2SH2S NaOH CuSO 4 PbCrO 4 H2OH2O NH 3 Hydrooxic acid (no……just water) Nitrogen trihydride (no..just ammonia) Copper ( II ) sulfate or Cupric sulfate Lead ( II ) chromate or Plubous chromate Sodium hydroxide Hyrdogen sulfuric acid Perchloric acid Potassium permanganate Sodium carbonate Hydroflouric acid Carbonic acid