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Understanding Chemical Bonding: Atoms, Ions, and Bonds

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Explore the fundamentals of chemical bonding in this comprehensive guide. Start with the basics of atoms, including their structure and the significance of valence shells. Learn how atoms bond to achieve stability through ionic and covalent bonds. Discover how bonds are formed, the differences between conductive and non-conductive compounds, and the practical implications of these bonds. Utilize Lewis Dot Diagrams for a clear visual representation of bonding. Perfect for students seeking to understand the chemical interactions that shape our world.

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Understanding Chemical Bonding: Atoms, Ions, and Bonds

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  1. Let’s Bond Notes on Chemical Bonding 8/15/13 p. 31 in ILL

  2. Warm-Up • What’s an atom? • Draw the atomic structure. • What is bonding? • What is 3 great things about your track-out?

  3. Announcements • Redos • Website: mpatberg.wordpress.com • Trays • Discipline Tier • Warm-Up

  4. Agenda • Warm-Up • Notes/Videos • Essential Learning

  5. Quick Review: • What’s an atom? • Smallest unit of matter • Made of protons (+), electrons (-), and neutrons • Has a nucleus and energy shells • Outermost energy shell is called a valence shell

  6. Valence Shells: • Determine how an atom behaves when it encounters other atoms • reactivity • Determined by group number in periodic table • Desired number of valence electrons is 8 (octet rule)

  7. Chemical Bonding: • Just like the 26 letters of alphabet combine to form words, the 100+ elements combine to form compounds (2 or more different elements) • http://www.brainpop.com/science/matterandchemistry/chemicalbonds/

  8. Chemical Bonding: • an attempt to fill valence shells to “feel noble” • Two types— • Ionic bonds • Covalent bonds

  9. Lewis Dot Diagrams: A quick simple way to show valence electrons 1 2 13 14 15 16 17 18 H He:      LiBe B  C  N  O : F :Ne :            Na Mg AlSiPS:Cl :Ar:    

  10. Learning Check: A. X would be the electron dot formula for 1) Na 2) K3) Al   B.  X  would be the electron dot formula  1) B 2) N 3) P

  11. Review Ions: Sodium atom Sodium ion Na  – e Na +(feels like Ne) 11 p+ 11 p+ 11 e- 10 e- 01+

  12. Review Ions: Fluorine atom Fluorine ion :F: + e:F:-(feels like Ne) 9 p+ 9 p+ 9 e- 10 e- 01-

  13. Ionic Bonds: • Ions are the result of atoms gaining or losing electrons • An ionicbond forms when one atom transfers an electron to another atom • Occurs when a metal reacts with a non-metal • The number of electrons lost must be equal to the number of electrons gained

  14. Ionic Bonds cont… • Great conductors of electricity when dissolved in water • Have very high melting points • Metals will lose electrons, non-metals will gain electrons • Held together by strong attraction of (+) to (-)

  15. Learning Check: A. Number of valence electrons in aluminum 1) 1 e-2) 2 e-3) 3 e- B. Change in electrons for octet (8 valence) 1) lose 3 e- 2) gain 3 e- 3) gain 5 e- C. Ionic charge of aluminum 1) 3- 2) 5- 3) 3+

  16. Covalent Bonds: • A bond formed when electrons are shared between two atoms • Occurs between non-metallic atoms • Not good conductors of electricity

  17. Covalent Bonds cont… • Low melting points • Mostly liquids and gases at room temp (solids are like plastics) • Individual groups of like atoms formed by covalent bonds are called molecules

  18. Learning Check: A. Covalent bonds are formed when atoms __________ electrons. 1) give up2) take on3) share B. Oxygen would most likely form a covalent bond with 1) Na 2) N 3) Ca

  19. Comparison of Bonds covalent ionic molecules ions conductive Non-conductive valence electrons Transfers electrons Sharing electrons metals/non-metals non-metals only solids/crystals liquids/gases low mp high mp

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