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CHAPTER 6 BONDS

Learn polyatomic ions, Lewis dot diagrams, chemical formulas, and different types of chemical bonds with flashcards. Understand metallic, ionic, and covalent bonds, and practice writing formulas for ionic and molecular compounds.

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CHAPTER 6 BONDS

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  1. CHAPTER 6 BONDS

  2. Polyatomic ions Flashcards-due Tomorrow-you can make them out of cut paper if you don’t have index cards

  3. Lewis DOT DIAGRAMS A model of an atom in which each dot represents a valence e- Max # of dots is 8 Li He Ne C X

  4. DOT DIAGRAMSDirections Draw dot diagrams for the following elements. On your paper Name Dot Diagrams 1.

  5. CHEMICAL FORMULA Tells what elements a compound contains & the ratio of those elements. Ex: H2O

  6. subscript- means “written below” Tells how many atoms of that element • superscript-means “written above” Tells charge (oxidation #) of element or compound • Ex: PO43- or PO4-3

  7. Ex: List elements & give ratio Your paper Name Elements & ratios My paper • CuSO4 = • Li2S = 11. Mg(OH)2= 19. C2H5OH= • CuSO4 • Li2S 11. Mg(OH)2 19. C2H5OH

  8. Answers • Ex: H2O = Hydrogen, Oxygen 2:1 • Fe2O3 = Iron, Oxygen 2:3 • Al(C2H3O2)3 = Aluminum, Carbon, Hydrogen, Oxygen 1:6:9:6 • HC2H3O2 = Hydrogen, Carbon, Oxygen 1:2:3:2

  9. Star questions • How many dots would Helium receive? • 2 • Define Chemical Formula • Tells what elements a compound contains & the ratio of those elements. • Subscript means? • Written below • Superscript means? • Written above

  10. CHEMICAL BONDS Occur through interactions between the valence electrons!!! • Three major types of chemical bonds: • Metallic • Ionic • Covalent

  11. METALLIC BONDS Metal + Metal = Metallic Bonds “SEA of ELECTRONS”=valence e- are not held tightly. They are freely moving or swimming around the atom nucleus’ at all times. Forms a lattice structure

  12. METALLIC BONDS • Characteristics: • Malleable • Ductile • Ex: Aluminum foil: crumpling, wont tear due to strong bonds! • More swimming electrons = stronger bonds!

  13. IONIC BONDS Formed when elements give up or take e- Formed between Metal & NonMetal

  14. IONIC BONDS • Protons no longer equal electrons!! • Particles formed by ionic bonds are called ions (a charged atom) • Anion—An ion w/ a negative charge (take e- , more negative) • Cation—An ion w/ a positive charge (give up e-, more positive)

  15. IONIC BONDS • EX: Na + Cl = Na+Cl- Na+ = Cation Cl- = Anion

  16. Write the purple words on your reference table! Charge, AKA: Oxidation # Group 1AGroup 2A 1 outer shell e- 2 outer shell e- gives 1 e- gives 2 e- +1 charge+2 charge Group 3AGroup 4A 3 outer shell e-*special group gives 3 e- can give, take +3 charge or share +/- 4 usually Carbon is -4

  17. Group 5AGroup 6A 5 outer shell e- 6 outer shell e- takes 3 e- takes 2 e- -3 charge-2 charge Group 7AGroup 8A 7 outer shell e- 8 outer shell e- takes 1 e- *already stable -1 charge0 charge *Goal is to be stable by having 8 electrons (octet rule)

  18. Covalent Bonds • Formed when 2 atoms share electrons • You complete me! • Only between NONMETALS

  19. Particles formed by covalent bonds are called molecules (ex: O2 & H2O) • Polar molecules have a separated + area & a - area b/c the e- are not shared equally! *most common covalent bond • Ex: HCl, NH2 & WATER (H20)

  20. Nonpolar molecules have the same charge (+ or -) because the e- are shared equally! • Ex: Cl2, CO2, O2

  21. 1. Mg F2 Mg + F + F MgF2 • Ionic Diagrams • Identify each element as a metal or nonmetal • State if Ionic or Covalent • Draw the diagram for the formation of the compound • Ionic Diagrams Need 4 things: • Equation • Dots • Arrows • Charges Your notes paper

  22. 2. H F H F • Covalent Diagrams • Identify each element as a metal or nonmetal • State if Ionic or Covalent • Draw the diagram for the formation of the compound • If covalent, state if Polar or nonpolar • Covalent Diagrams Need 2 things: • Dots • Circles Your notes paper

  23. Ionic and Covalent Diagramsmore examples My paper Your paper Name I/C Diagrams • LiCl • Cl2 • LiF • Cl2

  24. STAR questions • What type of bond would a metal and nonmetal be? • Ionic • What is the name of the particles formed by a covalent bond? • Molecules • What type of bond holds atoms of Au together? • metallic

  25. NamingBinary Ionic Compounds Composed of 2 elements 1. Write the name of 1st element 2. Write the root of the 2nd element, changing the ending to –ide ****(Name of cation, then anion) *See chart on page 171 One Nonmetal and One Metal!

  26. Examples: • MgO=Magnesium Oxide • NaCl=Sodium Chloride • Al2O3=

  27. Writing Formulas Binary Ionic Compounds 1. Write symbol for 1st element 2. Write symbol for 2nd element 3. Find the oxidation # (charge) for each element

  28. 4. drop n’ swap the oxidation # (drop=w/out the + or - ) (swap=give the # to the other element) 5. Reduce if possible

  29. Examples: • Lead Oxide • Pb • O • Pb +/-4 and O -2 • Pb2O4 • PbO2 • Aluminum Sulfide = Al S Al=+3, S=-2 , drop charges & swap #s Al2S3 • Lithium Fluoride • Calcium Oxide

  30. Molecular BinaryCovalent Compounds That means 2nonmetals only! • The name & formula of a molecular compound describes the type & # of atoms in a molecule of the compound

  31. Naming molecular compounds ex: 1. N2O4 dinitrogen tetraoxide 2. CO2 carbon dioxide

  32. Writing Molecular Formula ex: 1. Diphosporous tetraflouride P2F4 2.Carbon dioxide CO2

  33. More Binary and Molecular compounds examples • P2F4 • Li2S • MgF2 • Carbon Dioxide • Aluminum Oxide • Calcium Bromide

  34. STAR questions • Another word for oxidation # is? • Charge • What is the difference between an Anion and a Cation? • An Anion w/ a negative charge, a Cation is an ion w/ a positive charge • How many elements are in Binary compounds? • 2

  35. Naming Polyatomic Compounds Polyatomic ion-positive or negative group of atoms 1. Write name of first element 2. Write name of the polyatomic ion

  36. Examples: • CaCO3 = Calcium Carbonate • Mg(ClO3)2

  37. Writing FormulasPolyatomic Compounds 1. Write symbol of first element 2. Write symbol of polyatomic ion 3. Find the oxidation #’s 4. drop n’ swap! Use parenthesis around the polyatomic ion if crossing more than one! 5. Reduce if possible

  38. Examples: Lithium Sulfate • Li • SO4 • Li +1, SO4-2 • Li2(SO4) • Magnesium Nitrate • Ammonium Bromide

  39. STAR questions • Another word for oxidation # is? • Charge • What does a subscript tell me? • The #s of atoms of each element • What does the superscript tell me? • The charge for the elements or compound • What type of elements are Molecular compounds? • Covalent (nonmetals) binary (2 elements)

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