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Ch 7 PowerPoint Notes

Ch 7 PowerPoint Notes. Section 7.1 - Ions. OBJECTIVES: Determine the number of valence electrons in an atom of a representative element. Section 7.1 - Ions. OBJECTIVES: Explain how the octet rule applies to atoms of metallic and nonmetallic elements. Section 7.1 - Ions. OBJECTIVES:

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Ch 7 PowerPoint Notes

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  1. Ch 7 PowerPoint Notes

  2. Section 7.1 - Ions • OBJECTIVES: • Determine the number of valence electrons in an atom of a representative element.

  3. Section 7.1 - Ions • OBJECTIVES: • Explain how the octet rule applies to atoms of metallic and nonmetallic elements.

  4. Section 7.1 - Ions • OBJECTIVES: • Describe how cations and anions form.

  5. Why do some elements react to form compounds and others do not?Is there any way to predict if atoms might react with each other?Is there any way to predict what chemical formulas might be formed?

  6. Ionic and Metallic Bonding Na 1+,Na +1 or Na+ = cation , missing 1 e- O2- = anion, gained 2 e- (the number is the charge on ion, not # of e- gained or lost,, i.e., +1 means 1 electron lost, not 1 gained.)

  7. Ion definitions • Valence electrons: Outermost electrons. The s and p electrons in the outer energy level. The highest occupied energy level. • Core electrons: are those in the energy levels below. • Ion: An atom that has lost or gained an electron. Ions have a + or - charge. • (Atoms are always neutral, # of p+ = # of e-) • Cation: Positive Ion or metals, gained e-. • Anion: Negative Ion or non-metals, Lost e-.

  8. Valence Electrons are…? • The electrons responsible for the chemical properties of atoms, and 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 – are those in the energy levels below.

  9. Keeping Track of Electrons • Atoms in the same column (group)... • Have the same outer electron configuration. • Have the same valence electrons. • The number of valence electrons are easily determined. It is the group number for representative. • Group 2A: Be, Mg, Ca, etc. • have 2 valence electrons Group 8A, Noble gases has 8.

  10. Electron Dot diagrams are… • DEF: Shows the 8 valence electrons as dot pairs around the chemical symbol. • A way of showing & keeping track of valence electrons. • How to write them? • Write the symbol - it represents the nucleus and inner (core) electrons • Put one dot for each valence electron (8 maximum) • They don’t pair up until they have to (Hund’s rule). Do 4 singles before pairs. X

  11. Electron Dot diagramsSingle dots can be on any side. 1A 2A 3A 4A 5A 7A 6A 8A

  12. Valence e- highest electron energy level of an atom(ns np…where n is the same number)Nitrogen 1s22s2 2p3 5 Valence e-

  13. e- dot structures show only valence e-(single per side/then pair up)2 dots Mg –[Ne]3s2 3p0

  14. Need to Memorize!! EASY!

  15. valence e- determine the chemical properties of an elementAlkali metals (1 ve-) - ns1np0

  16. Remember s, p, d, f blocks S p 1S1 1S2 2S1 2S2 3S1 3S2 1 2 3 4 5 6 7 1 2 3 4 5 6 7 2p1 2p2 2p32p4 2p5 2p6

  17. Write the e dot structuresO = 1s22s2 2p4Ne = Na =

  18. Write the e dot structuresO = 1s22s2 2p4Ne = 1s22s2 2p6Na = 1s2 2s2 2p63s1 3p

  19. e dot structures – show valence e- as dotsO = 1s22s2 2p4Ne = 1s22s2 2p6Na = 1s2 2s2 2p63s1 3p

  20. octet rule – ions tend to have pseudo noble gas configuration (8 valence e-)full s and p orbitals

  21. Formation of Cations • Metals lose electrons to attain a 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 This is a noble gas configuration with 8 electrons in the outer level.

  22. Electron Dots For Cations • Metals will have few valence electrons (usually 3 or less); calcium has only 2 valence electrons Ca

  23. Electron Dots For Cations • Metals will have few valence electrons • Metals will lose the valence electrons Ca

  24. Electron Dots For Cations • Metals will have few valence electrons • Metals will lose the valence electrons • Forming positive ions Ca2+ This is named the “calcium ion”. NO DOTS are now shown for the cation.

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

  26. Electron Dots For Anions • Nonmetals will have many valence electrons (usually 5 or more) • They will gain electrons to fill outer shell. 3- P (This is called the “phosphide ion”, and should show dots)

  27. Stable Electron Configurations • All atoms react to try and achieve a noble gas configuration. • Noble gases have 2 s and 6 p electrons. • 8 valence electrons = already stable! • This is the octet rule (8 in the outer level is particularly stable). Ar

  28. ATOMNa = 1s2 2s2 2p63s1 3p0IONNa+1 = 1s22s2 2p6

  29. a. What is the charge of an e-?b. What is the e- config for N 3- ion? c. How many e- does (B) have?d. how many valence e- does (B) have?

  30. Why don’t the noble gases form ions?

  31. When writing S2-, what does the 2- indicate?Does this ion have more or less e than the original atom?

  32. Section 7.2 Ionic Bonds and Ionic Compounds • OBJECTIVES: • Explain the electrical charge of an ionic compound.

  33. Section 7.2 Ionic Bonds and Ionic Compounds • OBJECTIVES: • Describe three properties of ionic compounds.

  34. Ionic Compounds – compounds formed from cations and anions Usually a metal and a nonmetal (the charges always cancel)Na+, Cl- = NaCl

  35. Ionic Bonding • Anions and cations are held together by opposite charges (+ and -) • Ionic compounds are called salts. • Simplest ratio of elements in an ionic compound is called the formula unit. • The bond is formed through the transfer of electrons (lose and gain) • Electrons are transferred to achieve noble gas configuration (Octet Rule).

  36. Ionic Compounds • Also called SALTS • Made from: a CATION with an ANION (or literally from a metal combining with a nonmetal)

  37. Ionic Bonding Na Cl The metal (sodium) tends to lose its one electron from the outer level. The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.

  38. Ionic Bonding Na+ Cl - Note: Remember that NO DOTS are now shown for the cation!

  39. Chemical formula = number of atoms in a formula unit of an ionic compound (and not the charges on the ions)Formula unit = NaCl

  40. Ionic Bonding Lets do an example by combining calcium and phosphorus: • All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable). Ca P

  41. Ionic Bonding Ca P

  42. Ionic Bonding Ca2+ P

  43. Ionic Bonding Ca2+ P Ca

  44. Ionic Bonding Ca2+ P 3- Ca

  45. Ionic Bonding Ca2+ P 3- Ca P

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

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

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

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

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