1. Chemical Bonding 1/7/11 – “C” day Objective: Describe the interactions that occur between atoms when bonding occurs Do Now: Do you remember – what is the name of LiCl or MgBr 2 ?

2. Chemical Bonding 1/10/11 – “D” day Objective: Describe the interactions that occur between atoms when bonding occurs Do Now: Draw the lewis dot structures to determine how the following bond: Li & Cl Mg & N

3. What’s due` Due by the end of class pages 1-8 of Naming Compounds Packet Due tomorrow before quiz – Review Sheet

4. Valence Electrons Chemical bonds result from the sharing or transfer of valence electrons Valence electrons are those in the outermost energy level (think Bohr model) http://hyperphysics.phy- astr.gsu.edu/hbase/pertab/perlewis. html#c1http://hyperphysics.phy- astr.gsu.edu/hbase/pertab/perlewis. html#c1

5. Central concept The interaction between atoms (bonding) = ONLY involves valence electrons Think of the inner electrons as being “locked” tightly in filled energy level

6. Electron Dot Structures Represent valence electron configurations of atom/ions of an element Electrons are represented by dots and arranged in pairs around the elemental symbol along the four sides of a square Can be anywhere from 1 to 8 dots around an atom

7. Electron Dot Structures Electrons are arranged unpaired until they must be paired (only if there is more than 4 valence electrons) **He is the only element that does not follow this rule!

8. Electron Dot Structures Why? Because we will use dot structures of atoms to show bonding. Try dot structures for these: LiKr MgGa SiS

9. Electron Dot Structures LiKr MgGa SiS

10. Class Work Electron Dot Structures Hydrogen Calcium Aluminum Neon Sulfur Barium Silicon Oxygen Xenon Helium Tin Iodine Radon Potassium Krypton Strontium Arsenic

11. Valence Bonding Theory explains How many atoms are connected How these atoms are connected Shape of the structure –IONIC = geometry of the structure –MOLECULAR = shape of the molecule Strength of the bond (bond energy) –Ionic, nonpolar covalent, polar covalent

12. The Octet Rule Atoms in compounds tend to gain or lose electrons (what’s this called?) to achieve the e- configurations of a noble gas 8 valence electrons!

13. Cation: atom with a + charge The LOSS of valence e- produces a cation produced from metals lose 1, 2, or 3 electrons easily atoms become cations to satisfy the octet rule

14. Anion: atom with a - charge The GAIN of valence e- produces an anion produced from nonmetals gains 1, 2, or 3 electrons readily atoms become anions in order to satisfy the octet rule

15. AGENDA May 13: Submit HW Notes – Ionic Compounds & Metals CW – Properties of Ionic Compounds WS HW – Types of Bonds Packet – highlight, complete all “Reading Checks”and “Picture This” in margins and 1& 2 on last page

16. Ionic bonds and properties of ionic compounds An ionic compound is the result of the transfer of electrons from one set of atoms to another and consists entirely of ions Ionic bond - forces of attraction that bind oppositely charged ions together THEY MUST BE NEUTRAL!

17. NaCl and ionic bonding http://web.jjay.cuny.edu/~acarpi/N SC/5-bonds.htmhttp://web.jjay.cuny.edu/~acarpi/N SC/5-bonds.htm http://www.visionlearning.com/librar y/module_viewer.php?mid=55http://www.visionlearning.com/librar y/module_viewer.php?mid=55

18. Electron Dot Structures and Ionic Bonding Let’s determine the correct ratio of atoms that will come together and form an ionic bond. 1)K & O 2)Li & Cl 3)Mg & N

19. Electron Dot Structures and Ionic Bonding Then complete Ionic Bonding WS

20. Ionic bonds and properties of ionic compounds Properties of ionic bonds Conduct electricity when dissolved in water High MP due to crystalline structure Net charge of zero Salts Composed of Formula units Crystals at room temperature

21. Get out your notes and questions!! –What questions do you have?

22. Properties of ionic compounds 1. Conduct electricity when dissolved in water (melt) What needs to be present in order to conduct a current? when ionic solids dissolve in water, they break apart into their component ions these ions act as electrical conductors in water

23. Properties of ionic compounds 2. Salts - most ionic compounds are called salts because of their crystalline structure Crystal - a solid that contains atoms, ions or molecules in a regular repeating three dimensional pattern

25. Notice Each Li+ ion is surrounded by four F- ions Each F- ion is surrounded by four Li+ ions

26. Lithium Fluoride Again..

27. Properties of ionic compounds 3. High melting point due to crystalline structure it will take a lot of energy to break these highly organized bonds

28. Properties of ionic compounds 4. Net charge of zero anions and cations connect in a ratio such that the overall charge of the ionic compound is zero Example: Al +3 + Cl -1 ==> AlCl 3

29. Properties of ionic compounds 5. Composed of formula units a formula unit represents a compound that is ionically bound The lowest whole number ratio of ions represented in an ionic compound ex. NaCl instead of Na 2 Cl 2

30. Let’s do this together… Draw electron dot structures to illustrate the formation of the following two ionic compounds… –Magnesium Chloride –Aluminum Sulfide

31. Metallic Bonds Definition : Consist of the attraction of the free-floating valence electrons for the positively charged metal ions. Properties : Metallic bonds involve “moveable” electrons - this explains many of the properties of metals –conductivity –malleability –ductility

32. Metallic Bonds http://www.drkstreet.com/resources /metallic-bonding-animation.swfhttp://www.drkstreet.com/resources /metallic-bonding-animation.swf

33. AGENDA 25-APR: Submit HW Notes – Properties of Covalent Compounds CW – Properties of covalent compounds WS HW – pp. 406-408 KT #3, 7-9 RQ # 6, 17-22

34. Covalent bonds and properties of covalent compounds Covalent bond - forms when electrons are shared between two atoms H + H ==> H 2 (H H) Atoms can have SINGLE, DOUBLE, or TRIPLE covalent bonds

35. Covalent bonds Atoms share electrons in a covalent bond so that each atom has 8 valence electrons & more stability

36. Covalent bonds http://web.jjay.cuny.edu/~acarpi/NS C/5-bonds.htm

37. Covalent bonds and their properties Properties of covalent bonds Share bonding electrons Low MP and BP Not very soluble in water; poor/non conducting Can be gas, liquid, or solid at room temperature Composed of molecules No charged particles here!

38. Covalent bonds can be... 1. SINGLE - one pair of e- is shared between two atoms - shown as a dash (-) instead of two dots F - F dash is always used in covalent bonds to show shared electrons - NEVER for ionic bonds

39. Covalent bonds can be... Dots represent UNSHARED pairs of electrons –lone pairs (around the central bonding atom & affect molecular shape) –nonbonding pairs (around the bonded atoms)

40. Covalent bonds can be... 2. DOUBLE - two pair of e- is shared between two atoms oxygen = common example –O 2 - each O has 6 valence electrons so when the O 2 bond is formed, it must share TWO pair of electrons to satisfy the Octet Rule –O = O

41. Covalent bonds can be... 3. TRIPLE - three pair of e- is shared between two atoms nitrogen = common example –N 2 - each nitrogen has 5 valence electrons so to fulfill the Octet Rule, three pairs of electrons must be shared N

42. AGENDA 28-APR: Submit HW Notes – Drawing Covalent Compounds CW – Covalent bonding WS HW – Covalent bonding WS; TEST NEXT MONDAY!

43. Drawing covalent bonds Some atoms form single, double, or triple bonds when forming compounds to achieve an octet of electrons

44. Drawing covalent bonds HCl: H + Cl ==> H Cl = shared pair Shared pairs can be represented with a DASH H-Cl HCl has THREE unshared pairs of electrons

45. Drawing covalent bonds H 2 O: 2H + O ==> O H or O H H H Water has two shared pairs and two lone pairs of electrons

46. Drawing covalent bonds Draw the following covalent compounds in your notebooks now: NH 3 CH 4 CO 2

47. AGENDA 29-APR: Submit HW Notes - Polarity CW – Polarity of Molecules WS HW – pp. 406-408 KT #10-13, RQ # 23-28; TEST MONDAY!

48. Ionic vs. Covalent bonds and electronegativity W hat if one atom has a greater electronegativity than the other but not enough strength to pull the electron away all together (form an ionic bond)? We land somewhere in the middle with – polar covalent bonds – non polar covalent bonds

49. Polar vs. Nonpolar Covalent Bonds Electronegativtiy measures the nucleus’ ability to attract electrons When bonding atoms approach each other a tug of war begins Example: HCl Cl nucleus is stronger so bonding e- are closer to Cl H Cl H : Cl

50. Non polar covalent bonds Forms when atoms share electrons equally (like in the H 2 example or CH 4 ) Each atom or BONDED atom has equivalent electronegativity values

51. Non polar covalent bonds

52. Polar vs. Non-polar http://web.jjay.cuny.edu/~acarpi/NS C/5-bonds.htm Hydrogen – non-polar Water - polar

53. AGENDA 30-April: Submit HW Notes – Molecular Geometry CW – Shapes of Molecules WS #1-6 HW – Shapes of Molecules #7-12; TEST MONDAY!

54. Three dimensional chemistry REMEMBER –electrons = same charge = repel each other –Lone pair electrons also repel because electron pairs repel, molecules adjust their shape so that the valence electron pairs are as far apart as possible = VSEPR theory

56. Methane (tetrahedral, CH 4 )

57. Pyramidal (ammonia, NH 4 )

58. Bent (water, H 2 O)

59. AGENDA 1-April: Submit HW Molecular Geometry Activity HW – Review Study Guide; TEST MONDAY!

60. 2-MAY: Questions from Study Guide? CW: Web Quest ReviewWeb Quest Review