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Chapter 8 Test Review

Chapter 8 explores the essential concepts of covalent bonds, discussing the sharing of electrons, electronegativity, and the properties associated with these bonds. It delves into polar versus non-polar bonds, bond lengths, and strengths, along with the characteristics of sigma and pi bonds. The chapter also reviews the formation of covalent bonds in various groups of the periodic table, examines diatomic molecules, and provides insights regarding molecular shapes and Lewis structures. This comprehensive review equips students with the foundational knowledge needed for advanced studies in chemistry.

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Chapter 8 Test Review

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  1. Chapter 8 Test Review

  2. Polar- unequal sharing of electrons • Non-polar - equal sharing of electrons • Electronegativity- ability to attract electrons

  3. Properties of Covalent bonds • Bond length decreases as number of covalent bonds increases. • Bond strength increases as number of covalent bonds increases • Bond length increases as number of covalent bonds decreases • Bond strength decreases as number of covalent bonds decreases.

  4. Sigma and Pi bonds • Sigma- • Single covalent bond • Single bond- 1 sigma • Pi • Multiple covalent bonds • Double bond- 1 sigma, 1 pi bond • Triple bond- 1 sigma, 2 pi bonds

  5. 28. Which diagram correctly depicts the trend in electronegativity?

  6. How many atoms in each formula? • CH3OH • CH4 • PF3 • OF2 • NO2- • BH3 • SO42- • CN- • N2H2

  7. Covalent Bonds • How many covalent bonds can elements in the following groups form: • Group 1 (alkali metals) • Group 2 (alkali earth metals) • Group 3 • Group 4 • Group 5 • Group 6 • Group 7 (halogens) • Group 8 ( noble gases)

  8. Polar or non-polar • Shares equally • Does not share equally

  9. Diatomic Molecules • List the 7 diatomic molecules:

  10. Naming Molecules • SiS4 • PCl5 • CCl4 • NO

  11. Writing Formulas • Sulfur difluoride • Silicon tetrachloride • Chlorine trifluoride • Tetrasulfur heptanitride

  12. Lewis structures • CH3OH • BH3 • N2H2

  13. Lewis Structures with polyatomic ions • SO42- • CN-

  14. Molecular Shapes • CH4 • PF3 • OF2 • NO2-

  15. Lewis Structures with resonance • NO3– • CO32-

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