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

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

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

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

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 NH4

+ or H3O+

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

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)

IV. Shapes of Molecules

A. ___Linear_________-any __2____ atom molecule is linear

Ex HCl O2 N2

Exception: CO2 = molecular formula

B. ____Bent/Angular___= 3 atoms

Ex. H2O

C. ___Trigional _ ___Pyramid_______- 4 atoms make it up.

Ex CH3

• D. ____Tetrahedral__- 5 atoms make it up

• Ex. CH4

V. Lewis Dot Diagrams

A. Cl + Cl

B. H + I

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

B. ______Nonpolar___molecules are symmetrical (mirror images)

• Molecules of more than two atoms maybe nonpolar, even if the bonds are polar

• Ex. CH4

VII. Naming Molecular(2 nonmetals) must use prefix system or the stock system

• Prefixes1= mono 2= di 3= tri 4=tetra

5= penta 6=hexa

** mono not used for first element only!!!

Writing Formulas

Phosphorus(III) chloride diphosphorus pentcholride carbon(IV) nitride

Hexafluorine decaoxide Carbon (IV) oxide Sulfur (VI) oxide

____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

____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+

_______1. N + H (3x)

_______2. Hg + Hg

Draw the following, list the shape and state type of molecule

CCl4 H2O CO2

• P2O10

• N5P4

1. CO2 carbon dioxide carbon (IV) oxide

2. CO carbon monoxide carbon( II) oxide

3. SO2 sulfur dioxide sulfur (IV) oxide

4. SO3 sulfur trioxide sulfur (VI) oxide

5. N2O dinitrogen monoxide nitrogen (I) oxide

6. NO nitrogen monoxide nitrogen (II) oxide

7. N2O3 dinitrogen trioxide nitrogen (III)oxide

8. NO2 nitrogen dioxide nitrogen (IV) oxide

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

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

19. OF2 oxygen difluoride oxygen(II) fluoride

20. PBr3phosphorus tribromide phosphorus (III) bromide