2. 1 + - + - + - BONDING

3. 2

4. 3 + - + - + - IONIC BONDING

5. 4 IONIC RADII + - Z eff

6. 5 MONOATOMIC CATIONS LOW IONIZATION ENERGY ELEMENTS ELECTROPOSTIVE ELEMENTS LOSE SOME OR ALL OF THEIR VALENCE ELECTRONS  LOSE HIGHEST n QUANTUM NUMBER FIRST TRANSITION ELEMENTS: HIGHEST ns FIRST; THEN d Na: [Ne]3s 1 Na 1+ : [Ne] Ca: [Ar]4s 2 Ca 2+ : [Ar] Fe: [Ar]3d 6 4s 2 Fe 2+ : [Ar]3d 6 Fe 3+ : [Ar]3d 5  LOSE HIGHEST SUBLEVEL ( l ) FIRST Sn: [Kr]4d 10 5s 2 5p 2 Sn 2+ : [Kr]4d 10 5s 2 Sn 4+ : [Kr]4d 10 REMINDER: CATION RADIUS < ATOM RADIUS

7. 6 MONOATOMIC ANIONS ELECTRONEGATIVE ELEMENTS GAIN ELECTRONS NUMBER GAINED IS AMOUNT NEEDED TO FILL VALENCE ORBITALS....HIGHEST p SUBLEVEL O: [He]2s 2 2p 4 O 2- : [He]2s 2 2p 6 O 2- : [Ne] I: [Kr]4d 10 5s 2 5p 5 I 1- : [Kr]4d 10 5s 2 5p 6 I 1- : [Xe] REMINDER: ANION RADIUS > ATOM RADIUS TO HELP REMEMBER MONOATOMIC ANION CHARGE: GROUP NUMBER - EIGHT …….OR EIGHTEEN - GROUP NUMBER

8. 7 IONIC COMPOUNDS ELECTROPOSITIVE ELEMENT TRANSFERS OR LOSES ELECTRON(S) TO THE ELECTRONEGATIVE ELEMENT METAL LOSES ELECTRON(S) TO NON-METAL NaFCaF 2 FeF 3

9. 8

10. 9 COVALENT BONDS

11. 10 IONIC BONDS: TRANSFER ELECTRONS FROM HIGHER E ORBITALS TO LOWER E ORBITALS USUALLY: METAL + NON-METAL NOT INDIVIDUAL MOLECULES SPHERICAL, NON-DIRECTIONAL CHARGE NaCl MgF 2 BaO COVALENT BONDS SHARING OF ELECTRONS USUALLY: BETWEEN NON-METALS DIRECTIONAL BONDS INDIVIDUAL MOLECULES CO CO 2 C 2 H 5 OH

12. 11 POLAR COVALENT BONDS ELECTRONEGATIVITY (  ): MEASURE OF ATOM ’ S ABILITY TO ATTRACT BONDING ELECTRONS NON-POLAR COVALENT BOND:  = 0 H 2, Cl 2, O 2 POLAR COVALENT BOND:  > 0 HCl, H 2 O, ICl H Cl  = 2.1  3.0  = 0.9  BOND DIPOLE BOND POLARITY INCREASES AS  INCREASES ROUGH RULE:  > 1.8, BOND IS CLASSIFIED AS IONIC METAL + NON-METAL = IONIC NON-METAL + NON-METAL = COVALENT...

13. 12 IN EACH OF THE FOLLOWING, IDENTIFY THE MORE POLAR BOND AND INDICATE THE DIRECTION OF THE DIPOLE. P-F OR S-F N-F OR P-F C-H OR O-H Al-Cl OR Si-Cl REMEMBER:  INCREASES UP A GROUP AND ACROSS THE PERIOD  S >  P  P-F >  S-F P-F IS MORE POLAR DIPOLE TOWARDS F  N >  P P-F IS MORE POLAR DIPOLE TOWARDS F  O >  C O-H MORE POLAR DIPOLE TOWARDS O  Si >  Al Al-Cl MORE POLAR DIPOLE TOWARDS Cl IONIC

14. 13 LEWIS SYMBOLS: PICTORIAL REPRESENTATIONS OF VALENCE SHELL ELECTRONS SHOWS OUTERMOST ELECTRONS IN 4 “ ORBITALS ” FOLLOWING HUND ’ S RULE C H He Li Be B C N O F NeNa Mg Al Si P S Cl Ar OCTET DUET

15. 14 F FFFF F FF BONDING PAIR NONBONDING PAIRS (LONE PAIRS) TO DETERMINE LEWIS STRUCTURES, YOU NEED: ELECTRONS REQUIRED: ER = 8 x NON-H ATOMS + 2 x H ATOMS VALENCE ELECTRONS AVAILABLE VE =  (VALENCE ELECTRONS IN ALL ATOMS) SHARED PAIRS (NUMBER OF BONDS) SP = ½ (ER-VE) LONE PAIRS = ½ (VE) - SP

16. 15 GUIDES FOR DETERMINING LEWIS STRUCTURES OF SYSTEMS OBEYING THE OCTET (DUET) RULE  DETERMINE ER, VE, SP, & LP  DRAW MOLECULE WITH SINGLE BONDS UNLESS NOTED: FIRST ATOM IS CENTRAL ADD OTHER BONDS TO SATISFY SP ADD LONE PAIRS TO SATISFY OCTET(S) ON MOST ELECTRONEGATIVE ATOMS FIRST WORTH NOTING: H ATOMS CAN ONLY HAVE 1 BOND (TERMINAL ATOMS) HALOGENS: 1 BOND UNLESS CENTRAL ATOM

17. 16 DRAW LEWIS STRUCTURES FOR: CH 4 H2OH2O ER = VE = SP = ER = VE = SP = LP =

18. 17 DRAW LEWIS STRUCTURES FOR: F2F2 HCl ER = VE = SP = ER = VE = SP = LP =

19. 18 DRAW LEWIS STRUCTURES FOR: PF 3 NH 3 ER = VE = SP = F P F F ER = VE = SP = LP =

20. 19 WHAT IS THE LEWIS STRUCTURE OF O 2 ? ER = 8 x # O ATOMS 16 ELECTRONS NEEDED VE =2 O ATOMS x 6 e - PER ATOM 12 ELECTRONS AVAILABLE SP = ½(ER-VE) = ½ (16-12) 2 SHARED PAIRS 2 BONDS O O WHAT IS THE LEWIS STRUCTURE OF C 2 H 2 ? ER =2 x 8 e - + 2 x 2 e - 20 e - VE =2 C ATOMS x 4 e - + 2 H ATOMS x 1 e - 10e - SP = 1/2 (20 e - - 10e - ) 5 SHARED PAIRS H C C H LONE PAIRS = ½ (VE) - SP = ½ (12) - 2 =4

21. 20 BOND ORDER:NUMBER OF SHARED ELECTRON PAIRS C BO = 1 OR SINGLE BOND BO = 2 OR DOUBLE BOND BO = 3 OR TRIPLE BOND BOND STRENGTH OF A SPECIFIC BOND INCREASES AND BOND LENGTH DECREASES AS BOND ORDER INCREASES C  O C O C O STRENGTH LENGTH < > 358 799 1058 kJ/MOLE 1.43 1.23 1.13 A o

22. 21 MOLECULAR STRUCTURE VSEPR

23. 22 V ALENCE S HELL E LECTRON P AIR R EPULSION VSEPR ELECTRON REGIONS OR GROUPS OF NEGATIVE CHARGE AROUND AN ATOM REPEL ON ANOTHER ATTAIN POSITION TO MINIMIZE REPULSION 1 ELECTRON GROUP OR ELECTRON REGION IS A: LONE PAIR SINGLE BOND DOUBLE BOND TRIPLE BOND THE MOLECULAR SHAPE IS DETERMINED USING THESE ELECTRON GROUPS

24. 23 What does it mean to hybridize? Hybridization is the “ chemistry word ” for promoting electrons to an empty orbital 3 62 6 2 4 5 3 1 7 1 7 5 84 8 The #2 “ s ” electron becomes a “ p ” and #5 “ p ” becomes a “ s ” !

25. Hybridization Summary Table GeometryHybridization Total e - pairs Shared pairs Lone pairs AngleSketch Linearsp220 Trigonal Planar sp 2 330 Bentsp 2 321 Linearsp 2 312 Tetrahedralsp 3 440 Trigonal Pyramidal sp 3 431 Bent Angular sp 3 422 Linear sp 3 413

26. Hybridization Summary Table GeometryHybridization Total e - pairs Shared pairs Lone pairs AnglesSketch Trigonal bipyramidal sp 3 d550 See-Sawsp 3 d541 T-shapedsp 3 d532 Linearsp 3 d523 Linearsp 3 d514

27. Hybridization Summary Table GeometryHybridization Total e - pairs Shared pairs Lone pairs AnglesSketch ocatahedral sp 3 d 2 660 Square pyramidal sp 3 d 2 651 Square planar sp 3 d 2 642 T-shaped sp 3 d 2 633 Linear sp 3 d 2 624 Linear sp 3 d 2 615

28. 27 OBEY OCTET RULE:2, 3, OR 4 ELECTRON GROUPS 180 o 120 o 109 o THE “ MOLECULAR SHAPE ” ANALYSIS INCLUDES: DETERMINE NUMBER OF ELECTRON GROUPS DETERMINE APPLICABLE SHAPE NAME THE SHAPE LINEAR TRIGONAL PLANER TETRAHEDRAL

29. 28 WHAT IS THE SHAPE OF THE FOLLOWING: PF 3 CH 4 O 3 F P F F TRIGONAL PYRAMIDAL ~109 o BOND ANGLE P F F F H H C H H TETRAHEDRAL 109 o BOND ANGLE C H H H H O O O BENT ~120 o BOND ANGLE O

30. 29 MORE THAN 4 ELECTRON REGIONS? 5 = TRIGONAL BIPYRAMIDAL 6 = OCTAHEDRAL

31. 30 LARGE MOLECULES? DIFFERENT REGIONS! CAEFFINE LINEAR TETRAHEDRAL TRIGONAL PLANAR

32. 31 BOND ORDER (AGAIN)! FF ELECTRON DENSITY INTERNUCLEAR AXIS  BOND NODAL PLANE  BOND EVERY BOND CONTAINS 1  BOND MULTIPLE BONDS CONTAIN 1  BOND +  BONDS FF SINGLE BOND =  BOND O DOUBLE BOND =  BOND + 1  BOND H C C H TRIPLE BOND =  BOND + 2  BONDS

33. 32 HYBRIDIZATION RULES ONLY FORM IN MOLECULES; NOT ATOMS COVALENTLY BONDED POLYATOMIC MOLECULESONLY MIX NON-DEGENERATE ORBITALS sp, spd BUT NOT ss OR ppREQUIRES ENERGY INPUT O O H H C O H C O H H O C H H C O C H sp 3 4  BONDS sp 2 1  C-C 1  C-H 1  C-O OTHER p ORBITAL IS IN  BOND 3  C-O

34. 33 VALENCE BOND THEORY LOCALIZES BONDING ELECTRONS DIFFICULT TO EXPLAIN RESONANCE MOLECULAR ORBITAL THEORY DELOCALIZES  ELECTRONS C FREEDOM TO MOVE FREEDOM TO SPREAD

35. 34

36. 35 + - + - + - METALLIC BONDING

37. Metallic Bonding With atoms of the same metallic element Delocalized electron clouds caused by metallic atoms being so physically close to each other Known as a “sea of electrons” Reason why metals are such good conductors 36