chapter 6 covalent bonding i.covalent cmpds-____share_____ valence electrons sharing can be...
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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
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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
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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
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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
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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+
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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
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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)
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IV. Shapes of Molecules
A. ___Linear_________-any __2____ atom molecule is linear
Ex HCl O2 N2
Exception: CO2 = molecular formula
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B. ____Bent/Angular___= 3 atoms
Ex. H2O
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C. ___Trigional _ ___Pyramid_______- 4 atoms make it up.
Ex CH3
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• D. ____Tetrahedral__- 5 atoms make it up
• Ex. CH4
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V. Lewis Dot Diagrams
A. Cl + Cl
B. H + I
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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
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B. ______Nonpolar___molecules are symmetrical (mirror images)
• Molecules of more than two atoms maybe nonpolar, even if the bonds are polar
• Ex. CH4
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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!!!
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Writing Formulas
Phosphorus(III) chloride diphosphorus pentcholride carbon(IV) nitride
Hexafluorine decaoxide Carbon (IV) oxide Sulfur (VI) oxide
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____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
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____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+
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_______1. N + H (3x)
_______2. Hg + Hg
Draw the following, list the shape and state type of molecule
CCl4 H2O CO2
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• P2O10
• N5P4
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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
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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
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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
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19. OF2 oxygen difluoride oxygen(II) fluoride
20. PBr3phosphorus tribromide phosphorus (III) bromide