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Covalent Bonding

Covalent Bonding

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Covalent Bonding

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  1. Covalent Bonding Chapter 8

  2. Molecular Compounds • These toy models are made from circular pieces joined together in units by sticks. Atoms can also be arranged in different ways to make a variety of products.

  3. 8.1 Molecules and Molecular Compounds • Molecules and Molecular Compounds • How are the melting points and boiling points of molecular compounds different from those of ionic compounds?

  4. Molecules and Molecular Compounds • In nature, matter takes many forms. The noble gases, including helium and neon, are monatomic. That means they exist as single atoms.

  5. Molecules and Molecular Compounds • Some compounds are so different from ionic compounds that attractions between ions fail to explain their bonding. • The atoms held together by sharing electrons are joined by a covalent bond.

  6. Molecules and Molecular Compounds • A molecule is a neutral group of atoms joined together by covalent bonds. Air contains oxygen molecules. • A diatomic molecule is a molecule consisting of two atoms. An oxygen molecule is a diatomic molecule.

  7. Molecules and Molecular Compounds • A compound composed of molecules is called a molecular compound. Water and carbon monoxide are molecular compounds.

  8. Molecules and Molecular Changes • Molecular compounds tend to have relatively lower melting and boiling points than ionic compounds. • Unlike ionic compounds, many molecular compounds are liquids or gases at room temperature. • Unlike ionic compounds, molecular compounds usually contain only nonmetal atoms.

  9. Molecules and Molecular Compounds

  10. Molecules and Molecular Changes • Ethane, a component of natural gas, is also a molecular compound.

  11. Molecular Formulas • Molecular Formulas • What information does a molecular formula provide?

  12. Molecular Formulas • A molecular formula is the chemical formula of a molecular compound. • A molecular formula shows how many atoms of each element a molecule contains.

  13. Molecular Formulas

  14. Molecular Formulas • Formulas of Some Molecular Compounds

  15. The Nature of Covalent Bonding • The colors in this map indicate the concentrations of ozone in various parts of Earth’s atmosphere. Oxygen atoms can join in pairs to form the oxygen you breathe and can also join in groups of three oxygen atoms to form ozone.

  16. 8.2 The Octet Rule in Covalent Bonding • The Octet Rule in Covalent Bonding • What is the result of electron sharing in covalent bonds?

  17. 8.2 The Octet Rule in Covalent Bonding • In covalent bonds, electron sharing usually occurs so that atoms attain the electron configurations of noble gases.

  18. 8.2 Single Covalent Bonds • Single Covalent Bonds • How do electron dot structures represent shared electrons?

  19. Single Covalent Bonds • Two atoms held together by sharing a pair of electrons are joined by a single covalent bond.

  20. 8.2 Single Covalent Bonds • An electron dot structure such as H:H represents the shared pair of electrons of the covalent bond by two dots. • A structural formula represents the covalent bonds by dashes and shows the arrangement of covalently bonded atoms.

  21. Single Covalent Bonds • The halogens form single covalent bonds in their diatomic molecules. Fluorine is one example.

  22. 8.2 Single Covalent Bonds • A pair of valence electrons that is not shared between atoms is called an unshared pair, also known as a lone pair or a nonbonding pair.

  23. Single Covalent Bonds • The hydrogen and oxygen atoms attain noble-gas configurations by sharing electrons.

  24. Single Covalent Bonds • The ammonia molecule has one unshared pair of electrons.

  25. Single Covalent Bonds • Methane has no unshared pairs of electrons.

  26. Pg. 220 Conceptual Problem

  27. for Conceptual Problem 8.1 Pg. 220 Practice Problems

  28. 8.2 Double and Triple Covalent Bonds • Double and Triple Covalent Bonds • How do atoms form double or triple covalent bonds?

  29. 8.2 Double and Triple Covalent Bonds • Atoms form double or triple covalent bonds if they can attain a noble gas structure by sharing two pairs or three pairs of electrons.

  30. 8.2 Double and Triple Covalent Bonds • A bond that involves two shared pairs of electrons is a double covalent bond. • A bond formed by sharing three pairs of electrons is a triple covalent bond.

  31. Double and Triple Covalent Bonds • Oxygen shares two pairs of electrons.

  32. Double and Triple Covalent Bonds

  33. 8.2 Double and Triple Covalent Bonds • Carbon dioxide gas is soluble in water and is used to carbonate many beverages. A carbon dioxide molecule has two carbon-oxygen double bonds.

  34. Double and Triple Covalent Bonds • Carbon dioxide is an example of a triatomic molecule.

  35. 8.2 Coordinate Covalent Bonds • Coordinate Covalent Bonds • How are coordinate covalent bonds different from other covalent bonds?

  36. Coordinate Covalent Bonds • In carbon monoxide, oxygen has a stable configuration but the carbon does not.

  37. 8.2 Coordinate Covalent Bonds • As shown below, the dilemma is solved if the oxygen donates one of its unshared pairs of electrons for bonding.

  38. 8.2 Coordinate Covalent Bonds • A coordinate covalent bond is a covalent bond in which one atom contributes both bonding electrons. • In a structural formula, you can show coordinate covalent bonds as arrows that point from the atom donating the pair of electrons to the atom receiving them.

  39. 8.2 Coordinate Covalent Bonds • In a coordinate covalent bond, the shared electron pair comes from one of the bonding atoms.

  40. Coordinate Covalent Bonds • A polyatomic ion, such as NH4+, is a tightly bound group of atoms that has a positive or negative charge and behaves as a unit. • Most plants need nitrogen that is already combined in a compound to grow.

  41. Coordinate Covalent Bonds

  42. Conceptual Problem pg. 225

  43. for Conceptual Problem 8.2 Section Assessment pg. 225

  44. Bond Dissociation Energies • Bond Dissociation Energies • How is the strength of a covalent bond related to its bond dissociation energy?

  45. Bond Dissociation Energies • The energy required to break the bond between two covalently bonded atoms is known as the bond dissociation energy. • A large bond dissociation energy corresponds to a strong covalent bond.

  46. Resonance • Resonance • How are oxygen atoms bonded in ozone?

  47. Resonance • Ozone in the upper atmosphere blocks harmful ultraviolet radiation from the sun. At lower elevations, it contributes to smog.

  48. Resonance • The actual bonding of oxygen atoms in ozone is a hybrid, or mixture, of the extremes represented by the resonance forms.

  49. Resonance • A resonance structure is a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion.

  50. Exceptions to the Octet Rule • Exceptions to the Octet Rule • What are some exceptions to the rule?