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Chapter 6 Covalent bonding

Chapter 6 Covalent bonding. 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____

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Chapter 6 Covalent bonding

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  1. Chapter 6 Covalent bonding 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: 4Which represents a sea of mobile electrons? a. Chlorine b. nitrogen c. oxygen d. mercury

  5. 4. ____Coordinate Covalent_:_Donate____!!!! electrons from one __ion____are used by another without ____providing_(donate)_____any to ______share___!!!!Usually seen with polyatomic NH4+ or H3O+

  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 • 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. ___1. Ionic A. Unequally sharing of electrons___2. NPC B. Transfer of electrons___3. PC C. Donate the electrons to be shared___4. Metallic D. Form a continuous pattern___5. Network solid E. Equal sharing of electrons___6. Coordinate Covalent F. Sea of mobile electrons

  9. ___1.Ionic A. Rh + Pd___2. NPC B. H3O+___3.PC C. SiC___4. Metallic D. F + F___5. Network solid E. GaI3___6. Coordinate Covalent F. H + Br

  10. IV. Shapes of Molecules • ___Linear_________-any __2____ atom molecule is linear Ex HCl O2 N2 Exception: CO2 = molecular formula

  11. ____Bent/Angular___= 3 atoms Ex. H2O

  12. C. ___Trigional ____Pyramid_______- 4 atoms make it up. Ex CH3

  13. D. ____Tetrahedral__- 5 or more atoms make it up • Ex. CH4

  14. V. Lewis Dot Diagrams • Cl + Cl  B. H + I 

  15. 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 CH3Cl

  16. ______Nonpolar___molecules are symmetrical (mirror images) • Molecules of more than two atoms maybe nonpolar, even if the bonds are polar • Ex. CH4

  17. 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!!!

  18. Prefix System Stock System CO2 P2O3 N2S3 CCl4 N2O

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

  20. ____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

  21. ____1. network solid A. W + Rh ____2. metallic B. CI4 ____3. coordinate covalent bonding C. H3N ____4. polar covalent D. SiC ____5. nonpolar covalent E. HgCl2 ____6. ionic F. H3O+

  22. _______1. S + O (2x)  _______2. Hg + Hg Draw the following, list the shape and state type of molecule CCl4 H2O CO2

  23. P2O10 • N5P4

  24. CO2 carbon dioxide carbon (IV) oxide • CO carbon monoxide carbon( II) oxide • SO2 sulfur dioxide sulfur (IV) oxide • SO3 sulfur trioxide sulfur (VI) oxide • N2O dinitrogen monoxide nitrogen (I) oxide • NO nitrogen monoxide nitrogen (II) oxide • N2O3 dinitrogen trioxide nitrogen (III)oxide • NO2 nitrogen dioxide nitrogen (IV) oxide

  25. 9. N2O4 dinitrogen tetraoxide nitrogen (IV) oxide 10. N2O5 dinitrogen pentaoxide nitrogen (V) oxide 11. PCl3phosphorus trichloride phosphorus (III) chloride 12. PCl5phosphorus pentachloride phosphorus (V) chloride 13. NH3nitrogen trihydride nitrogen (III) hydride

  26. 14. SCl6 sulfur hexachloride sulfur (VI) chloride 15. P2O5 diphosphorus pentaoxide phosphorus (V) oxide 16. CCl4 carbon tetrachloride carbon (IV) chloride 17. SiO2 silicon dioxide silicon (IV) oxide 18. CS2 carbon disulfide carbon (IV) sulfide

  27. 19. OF2 oxygen difluoride oxygen(II) fluoride 20. PBr3phosphorus tribromide phosphorus (III) bromide

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