1. Chapter 6 Covalent bonding I.Covalent Cmpds-____share_____ valence electrons Sharing can be __equal_________, ___unequal_________ or can ___donate_____the e- to be shared. Bonds happen between 2 __metals____ or 2 __nm____ Form bonds to be more ____stable_____and come closer to being an ____octet_____. Form a bond=exo There are no _____[ ]___ or ___ions______ formed

2. Types of Covalent Cmpds 1. _Nonpolar__covalent(npc)=share ___equally= same element (diatomics) En diff=0-.5 Examples En diff= H + H  O + O  N + N 

3. 2. ___Polar___covalent (pc)= share _unequally____ (hogger=higher En)have – and + __area____(not ionic called dipole) En diff=___.6 -1.6____ H + Cl  Note: the higher the En diff=more polar=stronger bond = harder to break

4. 3. __Metallic______Bonding; __2____ metals, __+__ “ ions in a ___sea__ of mobile e-’s” Cu + Cu  Question: 4 Which represents a sea of mobile electrons? a. Chlorine b. nitrogen c. oxygen d. mercury

5. 4. ____Coordinate Covalent_:___USER____!!!!{Like the Winter Dance}electrons from one __ion____are used by another without ____providing______any to ______share___!!!!Usually seen with polyatomic NH 4 + or H 3 O +

6. 5 ___Network___________ Solids- many, many bonding sites. Bonds extend to form a continous pattern. Ex diamond, carbon, silicon dioxide or any cmpd that begins with silicon

7. III. Properties of Covalent compounds 1.Low melting and boiling points 2. Do not conduct electricity 3. Form a product called a molecule ( a group held together by covalent bonds)

8. IV. Shapes of Molecules A.___Linear_________-any __2____ atom molecule is linear Ex HCl O 2 N 2 Exception: CO 2 = molecular formula

9. B.____Bent/Angular___= 3 atoms Ex. H 2 O

10. C. ___Trigional _ ___Pyramid_______- 4 atoms make it up. Ex CH 3

11. D. ____Tetrahedral__- 5 atoms make it up Ex. CH 4

12. V. Lewis Dot Diagrams A.Cl + Cl  B. H + I 

13. VI. Type of Molecule-based on symmetry ( Must draw out) A.___Polar______ Molecules are also known as ___Dipoles______. Molecules of 2 atoms=dipole if bond=polar Dipoles are asymmetrical (not a mirror image) Dipoles are examples of molecular atttraction Ex. HCl CH 3 Cl

14. B.______Nonpolar___molecules are symmetrical (mirror images) Molecules of more than two atoms maybe nonpolar, even if the bonds are polar Ex. CH 4

15. VII. Naming Molecular(2 nonmetals) must use prefix system or the stock system Prefixes 1= mono 2= di 3= tri 4=tetra 5= penta 6=hexa ** mono not used for first element only!!!

16. Writing Formulas Phosphorus(III) chloride diphosphorus pentcholride carbon(IV) nitride Hexafluorine decaoxide Carbon (IV) oxide Sulfur (VI) oxide

17. ____1. network solid A. bonds formed by donating e-’s ____2. metallic B. covalent bonds that form a continuous pattern ____3. coordinate covalent bonding C. unequal sharing ____4. polar covalent D. sea of mobile e-’s ____5. nonpolar covalnt E. transfer of e-’s ____6. ionic F. equal sharing of e-’s

18. ____1. network solid A. W + Rh ____2. metallic B. CI 4 ____3. coordinate covalent bonding C. H 3 N ____4. polar covalent D. SiC ____5. nonpolar covalent E. HgCl 2 ____6. ionic F. H 3 O +

19. _______1. N + H (3x)  _______2. Hg + Hg  Draw the following, list the shape and state type of molecule CCl 4 H 2 O CO 2

20. P 2 O 10 N 5 P 4

21. 1.CO 2 carbon dioxide carbon (IV) oxide 2.CO carbon monoxide carbon( II) oxide 3.SO 2 sulfur dioxide sulfur (IV) oxide 4.SO 3 sulfur trioxide sulfur (VI) oxide 5.N 2 O dinitrogen monoxide nitrogen (I) oxide 6.NO nitrogen monoxide nitrogen (II) oxide 7.N 2 O 3 dinitrogen trioxide nitrogen (III)oxide 8.NO 2 nitrogen dioxide nitrogen (IV) oxide

22. 9. N 2 O 4 dinitrogen tetraoxide nitrogen (IV) oxide 10. N 2 O 5 dinitrogen pentaoxide nitrogen (V) oxide 11. PCl 3 phosphorus trichloride phosphorus (III) chloride 12. PCl 5 phosphorus pentachloride phosphorus (V) chloride 13. NH 3 nitrogen trihydride nitrogen (III) hydride

23. 14. SCl 6 sulfur hexachloride sulfur (VI) chloride 15. P 2 O 5 diphosphorus pentaoxide phosphorus (V) oxide 16. CCl 4 carbon tetrachloride carbon (IV) chloride 17. SiO 2 silicon dioxide silicon (IV) oxide 18. CS 2 carbon disulfide carbon (IV) sulfide

24. 19. OF 2 oxygen difluoride oxygen(II) fluoride 20. PBr 3 phosphorus tribromide phosphorus (III) bromide