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My Name is Bond…

My Name is Bond…. Chemical Bond. Chemical Bonding. Chapter 6. Covalent Compounds. Nonmetal bonding with another nonmetal Electronegativity difference less than 1.7 Electrons being shared. Draw the MO diagram for Chlorine and Hydrogen…. Diatomic Molecules. You must memorize these!!

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My Name is Bond…

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  1. My Name is Bond… Chemical Bond

  2. Chemical Bonding Chapter 6

  3. Covalent Compounds Nonmetal bonding with another nonmetal Electronegativity difference less than 1.7 Electrons being shared

  4. Draw the MO diagram for Chlorine and Hydrogen…

  5. Diatomic Molecules You must memorize these!! H2 N2 O2 F2 Cl2 Br2 I2 (At2) Magnificent 7— I won’t hold you responsible for astatine, just know that trends in a group apply!

  6. Formation of Covalent Bond

  7. Bond stability

  8. Octet Rule • Noble gases: have filled valence shells = 2 (He) or 8 e- • Octet Rule tells us that chemical compounds tend to form so that atoms obtain an octet of e- in its highest energy level. Visual Concepts

  9. Exceptions • Boron trifluoride BF3 • PF5 and SF6 can expand the shell and share more electrons. (10 and 12 respectively)

  10. Electron – Dot Notation • Dots are used to represent valence electrons around an atom. • Visual Concepts

  11. Lewis Structure Rules • Add up total number of valence e- • Pick central atom and create the bonds • Surround the adjacent atoms. • Put extra electrons on the central atom. • Beg, borrow or steal so that all the atoms are stable (have a complete octet). • Make sure the number of valence e- you started with are the number you used!

  12. Lets do… CH4 SiF4 NCl3

  13. Forming Multiple Bonds CO2 N2O

  14. Warm Up Draw the Lewis Structure for CS2 Circle each atom showing a complete octet.

  15. Exceptions • Boron Ex: Boron trifluoride BF3 • PF5 and SF6 can expand the shell and share more electrons. (10 and 12 respectively)

  16. Let’s talk about your WS Remind me to talk about the polyatomic ions!! Let’s add some Dipoles!

  17. Polyatomic ions Examples

  18. Naming Covalent Compounds Covalent compounds are molecules or molecular compounds… Indicate the number of each atom using prefixes….. …change the end of the name to “ide”

  19. Covalent Prefixes Use the prefixes! 1- mono 6- hexa 2- di 7- hepta 3- tri 8- octa 4- tetra 9- nona 5- penta 10- deca Examples: NO SiCl4

  20. Practice Formulas to names Names to formulas 1. Carbon tetrachloride 2. Dinitrogen monoxide 3. Dinitrogen tetroxide 4. Phosphorus triiodide 5. Sulfur heptafluoride • SO3 • ICl3 • PBr5 • CO • CO2

  21. Homework… Name all the molecular compounds on the Lewis Structure WS…. Remember to get your ions names from the polyatomic ion sheet!

  22. Multiple Covalent Bonds • Bond length and strength • Triple bonds are the shortest (pm), have the most Energy (kJ/mol) and are most unstable. • Single bonds are the longest (pm), have the least amount of Energy (kJ/mol), and are most stable

  23. Sigma s and Pi p bonds • Sigma (s) bonds are single bonds • Pi (p) bonds are the bonds that follow in a multiple bond situation

  24. Resonance Structures • Some molecules cannot be correctly identified by a single Lewis structure • When you can draw two mirror images, you probably have a resonance structure • For example: Ozone O3 Visual Concepts

  25. Draw the Resonance Structures for Silicon Trioxide with a 2- charge.

  26. Properties of Covalent Compounds • low melting point • low boiling point • many are gas and liquid at room temp • typically do not conduct electricity when dissolved in water This is due to the fact that forces of attraction between molecules are much weaker .

  27. Ionic vs covalent Visual Concepts

  28. Conductivity Demo

  29. Types of Bonds Lab Pre-lab- 8 minutes 1. Make a list of the characteristics of ionic and covalent compounds. 2. Discuss what makes the compounds different.

  30. Purpose- To classify 3 unknown samples as being either ionic of molecular using the known characteristics. Procedure: Design an experiment that would help you identify if an unknown sample is ionic or covalent. Would it be helpful to test your known compounds and compare results? t

  31. Materials Available Equipment Bunsen Burner Ring Stand Wire holder Test tubes Test tube racks Conductivity meter Chemicals Distilled water Sodium Chloride Sugar (C6H12O6) Unknown 1 Unknown 2 Unknown 3

  32. Warm Up- Draw the Lewis Structure Cl2O, SiCl3Br and ONCl • Draw the dipoles. • Count the number of shared and unshared electron pairs. • Count the number of shared and unshared pairs on the central atom. • How many sigma and pi bonds in each molecule? • Do any of them need resonance structures?

  33. Quiz Friday! Know your diatomics…. Draw Lewis Structures- understand polarity, draw dipoles, shared and unshared electrons. Naming covalents…

  34. Naming Acids Acids are molecular compounds that have hydrogen atoms…usually at the start of the formula! Binary Acids- have 2 elements HCl- HydrochloricAcid

  35. Oxyacids- Acids containing H,O, and a Nonmetal. (Polyatomic ion) If the poly ends in ate- change the end to ic and add “acid” H3PO4 If the poly ends in ite- change the end to “ous” and add “acid” HNO2

  36. Practice… • HI • HSO3 • HNO3 • HClO2 • HClO3 • H2CO3 Can we figure out the formula from the name?

  37. Metallic Bonding • This is an extremely strong bond Gives metal: luster, malleability, ductility, conduct electricity and heat d-orbital electrons

  38. Electron behavior explains the properties! Share a sea of electrons…otherwise known as “delocalized electrons” Explains why so many of them are good conductors of electricity.

  39. Alloys • Mixture of metals • Bronze: copper and tin • Brass: zinc and copper • Coin metal: copper and nickel • Solder: lead and tin

  40. Substitutional Alloy • Some of the main metal atoms are replaced by other metal atoms of similar size. An example is brass where one-third of the atoms of the host copper are replaced with zinc atoms.

  41. Interstitial Alloy • Formed when some of the holes in the closest packed metal structure are occupied by small atoms. • Steel is an interstitial alloy, containing carbon atoms in the holes of an iron crystal.

  42. Stainless steel is a substitutional/interstitial alloy

  43. Practice Naming Test…

  44. Work on your Naming WS Do about 10 and compare with your neighbor!

  45. Naming Race…

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