2. Chapter 6 Chemical Compounds 6-1 Ionic Bonding

3. Stable Electron Configurations When the highest occupied energy level of an atom is filled with electrons, the atom is ___________ and not likely to react Chemical properties of an element depend on the number of _________ electrons

4. Electron Dot Diagram An ____________ is a model of an atom in which each dot represents a _____________ electron The symbol is in the center represents the_________ and all the other electrons in the atom

5. Electron Dot Diagrams Group 1 Group 2 Group 3

6. Electron Dot Diagrams Group 4 Group 5 Group 6

7. Electron Dot Diagrams Group 7 Group 8

8. Ionic Bonds Some elements achieve stable electron configurations through the __________ of electrons between atoms. Ex Chlorine atom has________electron fewer than an argon atom Chlorine _________ a valence electron, it would have the same stable electron arrangement as _________

9. Formations of Ions When an atom ______ or _________an electron, the number of protons is no longer _________ to the number of electrons. An atom that has a net________ or ________ electric charge is called an_______. The charge on an ion is represented by a ______ or__________ sign

10. Na: Cl: Na +1 sodium ion Cl -1 chloride ion [Ne] [Ar]

11. Anion verses cation An ion with a __________ charge is an ________ Ex: Cl -1 An ion with a_________ charge is a __________ Ex: Na +1

12. Formation of Ionic Bonds 6-1 continued When an anion and a cation are close together, a chemical_________ forms A __________ bond is the force that holds atoms or ions together as a__________. An _________ bond is the force that holds cations and anions together An ________ bond forms when electrons are transferred from one atom to another

13. Ionization energy The amount of energy used to remove an_____ is called_________energy Ionization energy tends to_______ from left to right________ a period. They tend to_______ going down a_________

14. Ionic Compounds A chemical ___________ is a notation that shows what elements a compound contains and the_________ of the atoms or ions these elements in the compound. Ex: chemical formula =_________ (sodium chloride) Ex: MgCl 2

15. Crystal Lattices Solids whose particles are arranged in a lattice structure are called___________

16. Ionic bonding within a crystal lattice Covalent bonding forms a “molecule”

17. Properties of Ionic Compounds The properties of an ionic compound can be explained by the__________ attractions among ions within a crystal ________. Have _________ melting points Ions with same charges (- and -) or (+ and +) __________ each other Ions with the opposite charges (+ and -) _________ each other.

18. 6-2 Covalent Bonding _________ bond is a chemical bond in which two atoms_______ a pair of valence electrons When two atoms share one pair of electrons, the bond is called a _________ bond

19. Molecular Models Electron Dot diagram of H 2

20. Molecular Models Structural formula of H 2

21. Molecular Models Space-filling model of H 2

22. Molecular Models Electron Cloud Model of H 2

23. Molecules of Elements A _______ is a neutral group of atoms that are joined together by one or more covalent bonds The __________ between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond Diatomic means ________atoms

25. Lewis structure Single bond: covalent bond produced by the sharing on ONE pair of electrons between 2 atoms

26. Multiple Covalent Bonds DOUBLE BOND –sharing of________ pairs of electrons between 2 atoms TRIPLE BOND –sharing of __________ pairs of electrons between 2 atoms Bond Energies: triple > double > single …..triple bonds are stronger and shorter

27. Think Pair Share You and your partner think of situations that serve as analogies for ionic and covalent bonding.

28. Draw the Lewis structure for carbon tetrachloride CCl 4 Total # of valence electrons: –C: 1 x 4 e - = _______ e - –Cl: 4 x 7 e - = _______ e - Total # = ______ e -

29. or…..

30. Practice Draw the Lewis structure of IBr

31. Beaker Breaker Draw the Lewis structure showing bonds for HBr CH 4

32. 6-2 Continued A ____________bond in which electrons are not shared equally is called a _______ covalent bond. _________ – opposite in character, nature, or direction When atoms form a polar covalent bond, the atom with the __________ attraction for electrons has a partial __________ charge. The other atom has a partial _________ charge.

33. Polar and Nonpolar Molecules If a molecule has only______atoms, it will be _________ When molecules have more than______atoms, the answer is not as obvious. The _______ of atoms in a molecule and its ________are factors that determine whether a molecule is_______ or ______ See figure 12 page 168

34. Attraction between Molecules Attractions between polar molecules are _______ than attractions between __________ molecules Ex: water verses methane (CH 4 ) Methane = ________ Water = _______ Boiling point of water is _______

35. Practice Complete Section 6-2 Review page 169 Questions 1-8

36. 6-3 Naming Compounds and Writing Formulas Chemists use a system for naming compounds that is based on ________ The chemical name for lime is calcium oxide and the chemical formula is ______ ______ to_____ ratio of calcium ions to oxide ions in calcium oxide

37. Describing Ionic Compounds The name of an_______ compound must distinguish the compound from other ionic compounds containing the _______ elements. The formula of an ionic compound describes the ______ of the ions in the compound

38. Binary Ionic Compounds A compound made from only two elements is a _______ compound The names have a predictable pattern; the name of the________ followed by the name of the ______ Name for the cation is the name of the_______ without any change Name of the anion used part of the name of the _________with the suffix “_______” Ex : NaCl = ____________

39. Metals with Multiple Ions The alkali metals, alkaline earth metals, and aluminum form ions with___________charges equal to the _______ number Ex: potassium = ______ : calcium = ______ : aluminum = _______

40. Transition Metals When a metals forms more than one ion, the name of the ion contains a_______ numeral to indicate the ______ on the ion Example Copper(I)oxide = Cu +1 O -2 The formula balanced equals _____ Copper (II) oxide = Cu +2 O -2 The formula balanced equals _______

41. Polyatomic Ions What does the prefix “poly” mean? A covalently bonded group of atoms that has a positive or negative charge and acts as a unit is a___________ See figure 19 on page 173

42. Practice What are the names of these binary ionic compounds: LiCl BaO Na 3 N PbSO 4 use table on 173

43. Practice The charge on a chloride ion in AlCl 3 is? Write the formulas for the following compounds: Copper(I)chloride Copper(II)chloride

44. Homework/More Practice Name the following Binary compounds: 1.Na 2 S = 2.Li 2 O = 3.MgBr 2 = 4.H 2 S = 5.AlN =

45. Homework/More Practice Name the following using the Roman Numeral system 1.SnO = 2.TiO = 3.TiCl 3 = 4.CuCl = 5.NiBr 2 =

46. 6-3 continued Describing Molecular Compounds The name and formula of a ________ compound describes the ________ and ______ of atoms in a molecule of the compound

47. Naming Molecular Compounds Consists of two _________ in a compound The name of the________element is changed to end in the suffix “ide” You use Greek _______ to describe how many atoms of each element there is present (see handout) Ex: carbon dioxide = ______ or can be named as ________________, mono is usually not used for the first element

48. Writing Molecular Formulas Write the ________ for the elements in the order the elements appear in the name The _________ indicate the number of atoms of each element in the molecule Prefixes appear as __________ in the formulas. Ex: diphosphorus tetrafluoride = ________

49. Molecular Compounds Practice Write the name of the following compounds: Cl 2 O = __________ NO =____________ S 2 F 10 = ____________ P 2 S 3 = _____________

50. More Molecular Compounds Practice Write the formula of the following: Carbon tetrabromide =_________ Dinitrogen hexafluoride =________ Nitrogen Trichloride = _________ Phosphorus trihydride = _________

51. Homework/More Practice Write the following name for the compound or write the correct formula CI 4 = _________ N 2 F 6 = ________ Carbon trioxide = __________ Carbon monoxide =___________

52. Homework/More Practice P 2 O 5 = ____________ Nitrogen monoxide = __________ CCl 4 = ____________ CBr 3 = ___________ Carbon tetraiodide = ___________

53. 6-4 The Structure of Metals A________ bond is the attraction between a metal_______ and the shared ________ that surround it. The cation in a metal form a_______ that his held in place by the ________metallic bonds between the cations and the surrounding valence ___________

54. Metallic bonding Although the electrons are moving amoung the atoms, the _________number of electrons does not change The overall metal is __________ Metallic bonds in some metals are________ than in other _________metals are weaker compared to __________ metals

55. Explaining Properties of Metals The _________ of electrons within a metal lattice explains some of the___________ of metals _________ and ability conduct an_________current are two properties An electric current can be carried through a metal by the flow of the shared _________ ___________ – being able to be drawn into a thin wire is another property

56. Review Questions What holds metal ions together in a metal lattice? What characteristic of a metallic bond explains some of the properties of metals?

57. 6-4 Continued Alloys An _________ is a mixture of two or more elements, at least one of which is a _______. Alloys have the characteristic__________ of metals

58. Copper Alloys _________ was the first important alloy and is associated with the bronze era. Bronze contains only _______ and _______, which are relatively soft metals Mixed together in bronze, the metals are much _________ and ___________ than either metal alone. Scientists can design alloys with specific properties by varying the________ and_______ of elements in an alloy

59. Steel Alloys 1900’s was the Age of Steel because of skyscrapers, automobiles, and ships were built from _________. Steel is an alloy of________ that contains small quantities of ______ Stainless steels are durable because_________ forms an oxide that protects the steel from rusting _________ steel is more brittle than steels that contain more _______

60. Other Alloys Airplane parts are made of many different________ _______aluminum is lighter than most metals, it ______ and______ too easily _______ and __________ is added to make the material stronger

61. Review Questions 1.How can scientists design alloys with specific properties? 2.Explain why the metallic bonds in some metals are stronger than the bonds in other metals