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Covalent Bonding

Covalent Bonding. Covalent Bond. Atoms are held together by SHARING electrons. Terms. Molecule Neutral group of atoms joined together by covalent bonds. Compounds. Diatomic Molecule. Molecule consisting two of the same atom Never exist by themselves Example: Oxygen (O2). Also Known As:

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Covalent Bonding

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  1. Covalent Bonding

  2. Covalent Bond • Atoms are held together by SHARING electrons

  3. Terms • Molecule • Neutral group of atoms joined together by covalent bonds Compounds

  4. Diatomic Molecule • Molecule consisting two of the same atom • Never exist by themselves • Example: Oxygen (O2) Also Known As: The Magnificent Seven

  5. Diatomic Molecules Nitrogen Oxygen Flourine Clorine Bromine Iiodine

  6. Compounds Molecular Compound Ionic Compound • Compound composed of molecules • Collection of +ve and –ve charged ions repeating in a 3D pattern

  7. Molecular Compound • Lower melting and boiling points compared to ionic compounds • Composed of two or more non-metals

  8. Practice Worksheet: Identifying Ionic versus Molecular Compounds

  9. Writing Formulas for Molecular Compounds

  10. Binary Molecular Compounds • Composed of two elements • Metal and non-metal

  11. Molecular Formula • Chemical formula of a molecular compound • Example: Water H2O

  12. Molecular Formula • Represents the ACTUAL number of atoms in each molecule • (NOT the lowest ratio) • Example: Ethane C2H6

  13. Naming Molecular Compounds

  14. PreFixes

  15. Rules: • The name of a molecular compound indicates: • # of atoms • type of elements • Prefix “mono” ONLY used on the second element • For example: • CO is carbon monoxide rather than carbon oxide.

  16. Let’s Practice SO2 SF6 CCl4 NI3

  17. More Practice… CF4 SiO2 SO3 P4S3

  18. Practice Worksheet Naming Ionic and Covalent Bonds

  19. The Nature of Covalent Bonding Grab a WHITEBOARD, MARKER AND TOWEL

  20. The Nature of Covalent Bonding • Electrons are shared so that each atom: • gets eight electrons • Or • attains the noble gas configuration)

  21. Hint • The atom with the LEAST amount of valence electrons normally is in the middle… • Exception: • Hydrogen is ALWAYS on the outside • Example: HOCl

  22. Hint • Sometimes the molecular formula tells you the arrangement of atoms • Example: CH3COOH

  23. Single Covalent Bond • Two atoms held together by sharing ONE PAIR of electrons • Pair of shared e- can be represented by a dash • Structural formula • Example: • Hydrogen Molecule (H2) • Water (H2O)

  24. Unshared Pair • Not shared between atoms • Also known as: • Lone Pair • Non-Bonding • Example: A fluorine molecule (F2)

  25. Practice • H2O2 • PCl3

  26. Practice • Bromine • Chlorine • Iodine

  27. Other Covalent Bonds Double Covalent Bond Triple Covalent Bond • Atoms share two pairs of electrons • Atoms share three pairs of electrons

  28. Double and Triple Bonds • O2 • N2

  29. Double and Triple Bonds • C2H6O • NH3

  30. Try These… • CO • CF4

  31. Coordinate Covalent Bonds

  32. Coordinate Covalent Bond • A covalent bond in which one atom contributes BOTH bonding electrons • Example: • CO2

  33. Coordinate Covalent Bonding • SO3 • ClO3

  34. Try this one… • NH4

  35. Drawing Polyatomic Ions • REVIEW: • A tightly bound group of covalently bonded atoms that have a positive or negative charge and behave as a unit • Example: [SO3]2-

  36. Polyatomic ions • Contain both covalent and coordinate covalent bonds • Electronegativity: • The ability of an atom to attract electrons when the atom is in a compound • More electronegative elements will GAIN electrons • Less electronegative elements will LOSE electrons • [OH]-

  37. Practice • [BF4]- • [SO4]2- • [CO3]2-

  38. Practice Problems • [BF4]-

  39. Practice Problems • [SO4]2-

  40. Practice Problems • [CO3]2-

  41. Bonding Videos… • Ionic vs. Covalent Bonding

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