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CHAPTER 6 BONDS

CHAPTER 6 BONDS. Polyatomic ions. Flashcards-due Tomorrow-you can make them out of cut paper if you don’t have index cards. 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. DOT DIAGRAMS Directions.

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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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