1. Chapter 8 Covalent Bonding

2. Covalent bonding ……. Usually forms between two nonmetals (takers) Neither want to give up their electrons but are willing to share electrons

3. Exception: Hydrogen Hydrogen and a nonmetal …..neither wants to give up their electrons and neither has enough pull to take the other’s so they share a pair of electrons Hydrogen has one electron, but only needs one more to be “happy”

4. In a covalent bond the… -shared electrons are attracted to adjacent nuclei ++

5. Covalent Bonding

6. Covalent Bonds form molecules (* remember: Ionic Compounds form formula units) Molecule = smallest part of a covalent compound

7. That’s why…….Covalent compounds are also called molecular compounds

8. Binary (2-element) compounds -similar to ionic, but indicate the number of atoms using prefixes Naming Covalent Compounds

9. Prefix Meaning Mono-1 Di-2 Tri-3 Tetra-4 Penta-5 Hexa-6 Hepta-7 Octa-8 Nona9 Deca-10

10. -if only 1 atom of 1 st element, then no prefix is used Ex. CO Carbon monoxide CO 2 Carbon dioxide

11. -if more than 1 atom of 1 st element, then use prefix N2O4N2O4 Dinitrogen tetraoxide

12. Ws. Naming Molecular Compounds Ws. Name the following Molecular Compounds

13. Hydrogen Compounds can form Acids Remember…..Hydrogen is the exception to most rules Hydrogen has 1 electron but only needs 1 more to be happy so it acts like a nonmetal

14. Hydrogen doesn’t want to give up it’s one electron but it is willing to share it. When hydrogen combines with an anion a covalent compound is formed

15. When these compounds are dissolved in water….. …..they become acids.

16. What makes them an acid? Hydronium ions are formed

17. Start with ionic compound name. Then follow the 3 rules How to Name Acids

18. Naming Acids Rule #1 (Binary Acids) When anion ends in “ide”, the acid name begins with “hydro” and then ends in “ic”, then “acid” Ex. Hydrogen chloride (HCl)= hydrochloric acid Hydrogen sulfide (H 2 S) =hydrosulfuric acid

19. Naming Acids Rule #2 (Tertiary Acids) If anion ends in “ate”, the acid name is the stem of the anion with the suffix “-ic” followed by the word “acid” Ex. Hydrogen nitrate (HNO 3 ) = nitric acid

20. Naming Acids Rule #3 (Tertiary Acids) When anion ends in “ite”, the acid name is the stem of the anion with suffix “-ous” followed by the word “acid” Ex. Hydrogen sulfite (H 2 SO 3 ) = sulfurous acid

22. Ws. Name the Following Acids Ws. Formula Writing

23. Molecule Ex. CO H 2 O 1 molecule of carbon monoxide 1 molecule of water

24. Coefficient – the # of molecules or # of formula units. H2OH2O 4 molecules of water How many molecules of water??? 4

25. The number covalent bonds that will form depends on the # of valence electrons *Remember each atom is trying to achieve noble gas configuration (full outer shell) 7 valence electrons wants to share 1 pair 6 valence electrons wants to share 2 pair 5 valence electrons wants to share 3 pair

26. Chlorine atoms each have 7 valence electrons ….they each want one more so they will share one pair of electrons

28. Formation of Bonds

29. Single Covalent Bonds – 1 shared pair of electrons Cl 2

30. Single bond- 1 shared pair of electrons F and FF Double bond-2 shared pairs of electrons O and OO Triple bond-3 shared pairs of electrons N and N N

31. - you show the shared pair(s) of electrons between symbols Ex. Cl 2 Lewis Dot Diagram of Covalent Compounds Cl

32. Structural Formulas Each pair of shared electrons is shown as a dash( - ) Ex. Cl 2 Cl Cl - Cl Lewis Dot DiagramStructural Formula

33. *Remember hydrogen only needs to share one pair Be careful with Hydrogen (H 2 )

34. Hydrogen (H 2 ) H-H

35. Diatomic Molecules Two different atoms covalently bonded Ex. CO OH -

36. Diatomic Elements Ex. Cl and ClCl -when atoms of same element covalently bond

37. Diatomic Elements -elements that exist in pairs when not bonded to other atoms (“BrINClHOF”) Br 2 bromine I 2 iodine N 2 nitrogen Cl 2 chlorine H 2 hydrogen O 2 oxygen F 2 fluorine

38. More examples of single covalent bonds…

39. Water H 2 O Water H 2 O (2 single covalent bonds) H O H

40. Hydrogen and chlorine H - Cl

41. Methane CH 4 ( 4 single covalent bonds) H H C H H

42. PCl 3 Phosphorus trichloride ( 3 single covalent bonds) Cl P Cl Cl

43. Double Bonds O O

44. Lewis Dot Diagram of carbon dioxide O C O Carbon dioxide O C O

45. Triple bonds NN

46. Coordinate Covalent Bonds A coordinate covalent bond is formed when one atom donates both electrons to be shared.

47. Ammonium NH 4 + NH H H H Ammonia NH 3 Hydrogen Coordinate covalent bond

48. In coordinate bond structural formula…… An arrow points from the atom donating the pair of electrons toward the atom receiving them. NHH H H

49. When drawing electron dot diagrams…….. if an atom is “short” 2 electrons – try a coordinate covalent bond

50. H 3 (PO 4 )

51. PO O O O H H H Coordinate covalent bond

52. Bond Polarity Nonpolar - When bonding electrons are equally shared (same electronegativity) Ex. Diatomic elements Polar – When one atom has higher electronegativity ( attractive force) and pulls electron closer to it. It gains a slight negative charge and the other atom gains a slight positive charge Ex. H 2 O

53. Ws. What is Electronegativity?

54. .4 and belowNonpolar covalent Between.4 to 2.0Polar covalent Greater than 2.0ionic If the difference is….. the type of bond will be.. Electronegativity Differences !!!!!

55. Describing each bond in the molecule as …. Even pull= Nonpolar Uneven pull = polar Strong uneven pull = ionic

56. Showing polarity of individual bonds Use differences in electronegativities Indicated with δ ( lower case Greek letter delta) and charge.

57. Overall polarity of Molecules equals the sum of all the bond polarities

58. The arrow points to the atom with the higher electronegativity

59. Symmetry in Molecules Symmetrical molecules are usually nonpolar. Polar bonds cancel each other out Ex. CO 2

60. Carbon Tetrachloride

61. Bonds can be polar, yet overall molecular polarity is nonpolar

62. Asymmetrical Molecules Asymmetrical molecules are polar if there are polar bonds in the structure. Ex. H 2 O

63. Polarity of Water H H O δ - δ +

64. VSEPR Theory Valence shell electron-pair repulsion theory Because electron pairs repel, molecules adjust shapes so that pairs are as far away from each other as possible

65. Domains Single bond Double bond Triple bond Lone unshared pair

66. The # of Electron Domains determines the Basic Electron Domain shape Linear – 1 or 2 domains Trigonal Planar – 3 domains Tetrahedral – 4 domains Trigonal bipyramidal – 5 domains Octrahedral – 6 domains

67. Linear

68. Trigonal Planar ( flat)

69. Tetrahedral

70. Trigonal bipyramidal

71. Octahedral

72. Determining the Electron Domain Shape Count up all valence electrons Start with central atom (C, or Lowest EN, never H) Place other atoms around with maximum repulsion Put 8 electrons around outside atoms Any extra electrons go around the central atom Count the number of domains to determine the basic shape **** some compounds do NOT follow the octet rule

73. Let’s try some CS 2 BeH 2 CO 2 CH 4 CCl 4 NO 3 - NH 4 + SiF 4 SF 4

74. Molecular geometry Shapes are altered if there are non- bonding pairs of electrons surrounding the central atom

75. Bent – can be formed from a trigonal planar or tetrahedral Ex. H 2 O Ex. SO 2

76. Trigonal Pyramidal- can be formed from a tetrahedral Ex. NH 3

77. Ws. Electron Domain and Molecular Geometries

78. Structures and Models

79. Covalent Bonding: Molecular Model Building Lab

80. Model Colors Black – Carbon family Blue – Nitrogen family Red - Oxygen family Green or Purple - Halogens Yellow - Hydrogen

81. Use sticks to show single bonds Use springs to show multiple bonds

82. FormulaElectron domain shape/ Molecular shape Lewis Dot diagram * be careful of shape Single, double or triple bond ( list each bond EN Difference- list for for each bond Bond Type ( polar or nonpolar – list for each bond) Polarity of Molecule (polar or nonpolar) H 2 EA= D= NBD= BD= Cl 2 EA= D= NBD= BD= EA= valenceelectrons available D = electron domains NBD= non-bonding domainsBD= bonding domains

83. Electron –Domain Basic Bond Shapes Linear Bent Trigonal Planar Trigonal Pyramidal Tetrahedral

84. Hints for Lab

85. Start with Central Atom If it has carbon, use “C” as central atom If no carbon, use single atom or atom with lowest EN as central atom Never put hydrogen as central atom

86. Hints about the Acids Do polyatomic ion groups first, then add the hydrogens Use single atom, except Hydrogen, as central atom Usually contain coordinate covalent bonds

87. Last Hint !!!! If an atom is “short” 2 electrons – try a coordinate covalent bond

88. H 2 (CO 3 ) CO O O Double bond HH

89. H 3 (PO 4 ) PO O O O H H H Coordinate covalent bond

90. H 2 (SO 4 ) S O OO O H H Coordinate covalent bonds

91. H(NO 3 ) NO O O H Coordinate covalent bond

92. Properties of Covalent Compounds Low melting points (usually below 300 o C) Boiling points usually lower than ionic compounds Many are liquids or gases at room temperature High to low solubility Poor to non-conducting

93. Covalent Compounds form Network Solids Most covalently bonds substances melt easily because you just have to break the weak attractions between molecule and molecule Ex. Ice – Water –Sugar (C 12 H 22 O 11 )

94. Covalent crystals Covalent crystals If covalent compound forms crystals (repeating pattern)…….. Requires a lot of energy to break all the covalent bonds Have high melting points Ex. diamonds

95. A diamond ( pure carbon)

96. Solubility of Covalent Compounds “Like dissolves Like” Polar compounds will dissolve in polar solvents Nonpolar compounds will dissolve in nonpolar solvents

97. Why don’t water and oil mix? -Water is polar, oil is nonpolar. -Water is more attracted to itself than to the oil. Why do detergents cause water and oil to mix? -detergents are long molecules with one polar and one nonpolar end. -the water is attracted to the polar end and the oil is attracted to the nonpolar end.

98. Soap and Detergent Nonpolar end –attracts nonpolar oil or grease Polar end –attracts (polar)water

99. Chapter Review Covalent Bonding

100. Ionic vs. Covalent Electrons transferElectrons shared Metal and Non metalNonmetal and Nonmetal Formula unitsmolecules No prefixes in namesPrefixes in names Neutral compound Called saltsIf starts with “H” it could be an acid when dissolved in H 2 O High melting points, easily dissolved and conduct when dissolved Low melting points, not easy to dissolve, don’t conduct electricity

101. Ws. Bond Prediction Ws.Naming Compounds Ws. Name the Following Compounds Ws. Naming Compounds Reference Sheet

102. Diatomics = 2 atoms of same element bonded to each other BrINClHOF Diatomic element is linear and Nonpolar

103. Covalent Bonds – 4 Types Single- 1 shared pair of electrons (1 from each atom) Double – 2 shared pairs of electrons (two from each atom) Triple- 3 shared pairs of electrons, ( three from each atom) Coordinate covalent – both electrons of shared pair come from 1 atom

104. Structural Formula Structural Formula- shows arrangement of bonds Cl Cl single O O double N N triple C O coordinate covalent

105. Electron Dot Diagrams Every atom MUST have 8 electrons drawn around it except “H”. “H” needs 2 electrons

106. Polar vs. Nonpolar – depends on EN ( electronegativity) difference Nonpolar – shared evenly – EN difference below.4 Polar – shared unevenly – EN.4 – 2.0 Ionic – pulls electron off of atom. EN above 2.0

107. Polarity of Bond Depends on electronegativity difference

108. Polarity of Molecule Look at symmetry, then polarity of the bonds

109. Know how to name ionic compounds, covalent compounds and acids

110. The End