Chapter 6 Covalent bonding

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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
  bondexo
• There are no _____ ___ or ___ions______ formed

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Types of Covalent Cmpds

• 1. _Nonpolar__covalent(npc)share ___equally
  same element (diatomics)
• En diff0-.5
• Examples En diff
• H H ?
• O O ?
• N N ?

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• 2. ___Polar___covalent (pc) share _unequally____
• (hoggerhigher En)have and __area____(not
  ionic called dipole) En diff___.6 -1.6____
• H Cl ?
• Note the higher the En diffmore polarstronger
  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 Danceelectrons 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

• 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

• ___Linear_________-any __2____ atom molecule is
  linear
• Ex HCl O2 N2
• Exception CO2 molecular formula

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• ____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

• 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 atomsdipole if bondpolar
• Dipoles are asymmetrical (not a mirror image)
• Dipoles are examples of molecular atttraction
• Ex. HCl CH3Cl

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• ______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

• Prefixes
• 1 mono 2 di 3 tri 4tetra
• 5 penta 6hexa
• 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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• 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

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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