1 / 38

Covalent Bonding

Covalent Bonding . Sharing of Electron Pairs: Non-metal with Non-metal Atoms. Covalent Bonding . Compounds that are NOT held together by an electrical attraction, but instead by a sharing of electrons. Occur between nonmetal atoms with electronegativity differences less than 1.67.

rhett
Télécharger la présentation

Covalent Bonding

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Covalent Bonding Sharing of Electron Pairs: Non-metal with Non-metal Atoms

  2. Covalent Bonding • Compounds that are NOT held together by an electrical attraction, but instead by a sharing of electrons. • Occur between nonmetal atoms with electronegativity differences less than 1.67

  3. Covalent Bonding H••H

  4. Covalent Bonding

  5. Covalent Bonding A neutral group of atoms joined together by covalent bonds is called a molecule. A compound composed of molecules is called a molecular compound. The chemical formula for a molecule is called the molecular formula.

  6. Covalent Bonding Properties of Molecular Compounds: • Composed of two or more nonmetals. • Usually gases or liquids at room temperature. But can be found in any physical state at STP. • Molecular compounds tend to have lower melting and boiling points than do ionic compounds. • Do not conduct electricity. They form nonelectrolytes.in solution.

  7. Covalent Bonding Do not conduct electricity. They form nonelectrolytes. • Reason: Molecular compounds do not break apart into ions in solutions.

  8. Covalent Bonding Molecular compounds tend to have lower melting and boiling points than do ionic compounds. • Reason: There are no (or few and weak) bonds holding the molecules together in molecular compounds. Molecular Compound (H2O) Ionic Compound (NaCl)

  9. intermolecular bonds Dispersion forces - caused by motion of electrons (weakest intermolecular force). More electrons = stronger dispersion forces. Diatomic halide molecules are held together by dispersion forces. gas gas liquid solid

  10. intermolecular bonds dipole interactions

  11. hydrogen bonds Weak bonds between bonded hydrogen and some electron dense species. (F,O,N)

  12. polar covalent bonds Polar bonds have more electrons on one side of the bond than the other. Electrons concentrate around electronegative elements.

  13. polar covalent molecules Polar molecules have polar bonds. A molecule with two poles is called a dipole.

  14. non-polar covalent bonds

  15. Covalent Bonding • Predicting Molecular Geometries & Polarity: • Atoms attain an octet (also called noble gas electron configurations) by sharing electrons. • The bonds that form from this sharing can be single, double or triple. Triple bonds are shorter and stronger than double bonds, which are shorter and stronger than single bonds.

  16. Covalent Bonding • How Do We Proceed? Determine total number of valence electrons Based on usual bond numbers, identify reasonable layout for atoms <VSEPR> Place bonding electrons between atoms to make usual number of bonds Place remaining electrons as lone pairs around atoms still lacking an octet

  17. hybrid orbital geometries

  18. hybrid orbital geometries

  19. Covalent Bonding · · · C · Outer e- only shown H + C 1e- 2e- 1H 6C 4e- Equivalent to: H·

  20. Covalent Bonding · · · C · H + C H· H· H· H· Outer e- only shown

  21. Covalent Bonding H + C Positive nuclei H 2 e- at each H : H: :H C : H Negative electrons 8 e- at carbon all atoms closed shell Outer e- only shown

  22. Covalent Bonding H + C Final Structure: Tetrahedral

  23. Covalent Bonding : · · N · H + N H· H· H· Outer e- only shown

  24. Covalent Bonding H + N 2 e- at each H : H: :H N : H 8 e- at nitrogen all atoms closed shell Outer e- only shown

  25. Covalent Bonding H + N Final Structure: Trigonal Pyramidal

  26. Covalent Bonding : O : · · H + O H· H· Outer e- only shown

  27. Covalent Bonding H + O 2 e- at each H : H: : O : H 8 e- at oxygen all atoms closed shell Outer e- only shown

  28. Covalent Bonding H + O Final Structure: Bent

  29. Covalent Bonding : : F : · H + F H· Outer e- only shown

  30. Covalent Bonding H + F 8 e- at fluorine all atoms closed shell : : : F : H 2 e- at H Outer e- only shown

  31. Covalent Bonding H + F Final Structure: Linear

  32. Covalent Bonding Patterns for Major Elements: • CH4 C = 4 bonds; all electrons shared • NH3 N = 3 bonds; one lone pair • H2O O = 2 bonds; two lone pairs • HF F = 1 bond; three lone pairs

  33. Covalent Bonding Patterns for Major Elements: 4 Bonds All e-shared • Carbon, group IV 3 Bonds 1 Lone Pair • Nitrogen, Group V 2 Bonds 2 Lone Pairs • Oxygen, Group VI 1 Bond 3 Lone pairs • Fluorine, Group VII

  34. Covalent Bonding Other Compounds Have Same Pattern: C = 4 bonds; Cl (like F) = 1 bond P (like N = 3 bonds; Br (like F) = 1 bond

  35. Covalent Bonding Other Compounds Have Same Pattern: S (like Oxygen) = 2 bonds, 2 lone pairs C = 4 bonds; O = 2 bonds, 2 lone pairs

  36. Covalent Bonding Multiple Bonds • Atoms may share more than one pair of electrons • a DOUBLE BOND forms when atoms share two pairs of electrons (4 e-) • a TRIPLE BOND forms when atoms share three pairs of electrons (6 e-) • Total number of bonds per atom unchanged

  37. Covalent Bonding 4 Bonds, each carbon Two bonds at oxygen Multiple Bonds • C2H4 Valence e-= 12 • H2CO Valence e- = 12

  38. Covalent Bonding Multiple Bonds Total valence e-= 16 (Oxygen = 6 e-, each; Carbon = 4 e-. Four bonds/C; 2 bonds oxygen Total valence e- = 10 (H = 1, C = 4, N = 5) Bonds: C = 4, N = 3, H = 1 Total valence e- = 18 (O = 6, Cl = 7, P = 5) Bonds: Cl = 1, P = 3, O = 2

More Related