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Chapter 15 Ionic Bonding and Ionic Compounds

Chapter 15 Ionic Bonding and Ionic Compounds. Section 15.1 Electron Configuration in Ionic Bonding. OBJECTIVES: Use the periodic table to infer the number of valence electrons in an atom, and draw it’s electron dot structure. Section 15.1 Electron Configuration in Ionic Bonding. OBJECTIVES:

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Chapter 15 Ionic Bonding and Ionic Compounds

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  1. Chapter 15Ionic Bonding and Ionic Compounds

  2. Section 15.1Electron Configuration in Ionic Bonding • OBJECTIVES: • Use the periodic table to infer the number of valence electrons in an atom, and draw it’s electron dot structure.

  3. Section 15.1Electron Configuration in Ionic Bonding • OBJECTIVES: • Describe the formation of cations from metals, and of anions from nonmetals.

  4. Valence Electrons • The electrons responsible for the chemical properties of atoms are those in the outer energy level. • Valence electrons - The s and p electrons in the outer energy level • the highest occupied energy level • Core electrons -those in the energy levels below.

  5. Keeping Track of Electrons • Atoms in the same column... • Have the same outer electron configuration. • Have the same valence electrons. • Easily found: group number on the periodic table for representative elem. • Group 2A: Be, Mg, Ca, etc. • 2 valence electrons

  6. Electron Dot diagrams • A way of keeping track of valence electrons. • How to write them? • Write the symbol. • Put one dot for each valence electron • Don’t pair up until they have to (Hund’s rule) X

  7. The Electron Dot diagram for Nitrogen • Nitrogen has 5 valence electrons. • First we write the symbol. N • Then add 1 electron at a time to each side. • Until they are forced to pair up.

  8. Write electron dot diagrams: • Na • Mg • C • O • F • Ne • V

  9. Electron Configurations for Cations • Metals lose electrons to attain noble gas configuration. • They make positive ions (cations) • If we look at the electron configuration, it makes sense to lose electrons: • Na 1s22s22p63s1 1 valence electron • Na1+1s22s22p6 noble gas configuration

  10. Electron Dots For Cations • Metals will have few valence electrons (usually 3 or less) Ca

  11. Electron Dots For Cations • Metals will have few valence electrons • These will come off Ca

  12. Electron Dots For Cations • Metals will have few valence electrons • These will come off • Forming positive ions Ca2+ Pseudo-noble gas configuration Now make Sc an ion.

  13. Electron Configurations for Anions • Nonmetals gain electrons to attain noble gas configuration. • They make negative ions (anions) • Halide ions- ions from chlorine or other halogens that gain electrons • S 1s22s22p63s23p4 6 valence electrons • S2-1s22s22p63s23p6 noble gas configuration.

  14. Electron Dots For Anions • Nonmetals will have many valence electrons (usually 5 or more) • They will gain electrons to fill outer shell. P P3-

  15. Stable Electron Configurations • All atoms react to achieve noble gas configuration. • Noble gases have 2 s and 6 p electrons. • 8 valence electrons . • Also called the octet rule. Ar

  16. Section 15.2Ionic Bonds • OBJECTIVES: • List the characteristics of an ionic bond.

  17. Section 15.2Ionic Bonds • OBJECTIVES: • Use the characteristics of ionic compounds to explain the electrical conductivity of ionic compounds when melted and when in aqueous solution.

  18. Ionic Bonding • Anions and cations are held together by opposite charges. • Ionic compounds are called salts. • Simplest ratio is called the formula unit. • The bond is formed through the transfer of electrons. • Electrons are transferred to achieve noble gas configuration.

  19. Ionic Bonding Na Cl

  20. Ionic Bonding Na+ Cl-

  21. Ionic Bonding • All the electrons must be accounted for! Ca P

  22. Ionic Bonding Ca P

  23. Ionic Bonding Ca2+ P

  24. Ionic Bonding Ca2+ P Ca

  25. Ionic Bonding Ca2+ P 3- Ca

  26. Ionic Bonding Ca2+ P 3- Ca P

  27. Ionic Bonding Ca2+ P 3- Ca2+ P

  28. Ionic Bonding Ca Ca2+ P 3- Ca2+ P

  29. Ionic Bonding Ca Ca2+ P 3- Ca2+ P

  30. Ionic Bonding Ca2+ Ca2+ P 3- Ca2+ P 3-

  31. Ionic Bonding = Ca3P2 Formula Unit Sample Problem 15-1, page 421

  32. Properties of Ionic Compounds • Crystalline structure, usually solids • A regular repeating arrangement of ions in the solid: Fig. 15.9, p.423 • Ions are strongly bonded together. • Structure is rigid. • High melting points • Coordination number- number of ions of opposite charge surrounding it

  33. Crystalline structure

  34. Do they Conduct? • Conducting electricity is allowing charges to move. • In a solid, the ions are locked in place. • Ionic solids are insulators. • When melted, the ions can move around. • Melted ionic compounds conduct. • NaCl: must get to about 800 ºC. • Dissolved in water they conduct (aqueous)

  35. Section 15.3Bonding in Metals • OBJECTIVES: • Use the theory of metallic bonds to explain the physical properties of metals.

  36. Section 15.3Bonding in Metals • OBJECTIVES: • Describe the arrangements of atoms in some common metallic crystal structures.

  37. Metallic Bonds • How atoms are held together in the solid. • Metals hold on to their valence electrons very weakly. • Think of them as positive ions (cations) floating in a sea of electrons: Fig. 15.13, p.427

  38. + + + + + + + + + + + + Sea of Electrons • Electrons are free to move through the solid. • Metals conduct electricity.

  39. Metals are Malleable • Hammered into shape (bend). • Also ductile - drawn into wires. • Both malleability and ductility explained in terms of the mobility of the valence electrons • Fig. 15.14, p.427

  40. + + + + + + + + + + + + Malleable

  41. + + + + + + + + + + + + Malleable • Electrons allow atoms to slide by.

  42. + - + - - + - + + - + - - + - + Ionic solids are brittle

  43. - + - + - + - + + - + - - + - + Ionic solids are brittle • Strong Repulsion breaks crystal apart.

  44. Crystalline structure of metal • If made of one kind of atom, metals are among the simplest crystals • Note Fig. 15.16, p.428 for types: 1. Body-centered cubic: • every atom has 8 neighbors • Na, K, Fe, Cr, W

  45. Crystalline structure of metal 2. Face-centered cubic: • every atom has 12 neighbors • Cu, Ag, Au, Al, Pb 3. Hexagonal close-packed • every atom also has 12 neighbors • different pattern due to hexagonal • Mg, Zn, Cd

  46. Alloys • We use lots of metals every day, but few are pure metals • Alloys - mixtures of 2 or more elements, at least 1 is a metal • made by melting a mixture of the ingredients, then cooling • Brass: an alloy of Cu and Zn • Bronze: Cu and Sn

  47. Why use alloys? • Properties often superior to element • Sterling silver (92.5% Ag, 7.5% Cu) is harder and more durable than pure Ag, but still soft enough to make jewelry and tableware • Steels are very important alloys • corrosion resistant, ductility, hardness, toughness, cost

  48. Why use alloys? • Table 15.3, p.429 - common alloys • Types? a) substitutional alloy- the atoms in the components are about the same size • b) interstitial alloy- the atomic sizes quite different; smaller atoms fit into the spaces between larger • Amalgam- dental use, contains Hg

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