3. CHEMICAL BONDING IONIC BONDS COVALENT BONDS

5. IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence electrons

6. IONIC BONDING IS THE COMPOUND AN IONIC COMPOUND?METAL NONMETAL SUBSCRIPTS

7. IONIC BOND FORMATION Neutral atoms come near each other. Electron(s) are transferred from the Metal atom to the Non-metal atom. They stick together because of electrostatic forces, like magnets.

8. IONIC BONDING ION – any atom with more or less electrons that it is supposed to have* *Remember that the number of electrons is supposed to be equal to the number of Protons if the atom has a neutral charge

9. IONIC BONDING Metals will tend to lose electrons and become POSITIVE CATIONS Normal sodium atom loses one electron to become sodium ion

10. IONIC BONDING Nonmetals will tend to gain electrons and become NEGATIVE ANIONS Normal chlorine atom gains an electron to become a chloride ion

11. Na +1 is called a sodium ion The +1 symbol means it has lost one electron IONIC BONDING

12. Mg +2 is called a magnesium ion The +2 symbol means it has lost two electron IONIC BONDING

13. S -2 is called a sulfide ion The -2 symbol means it has gained two electron IONIC BONDING

14. Cl -1 is called a chloride ion The -1 symbol means it has gained one electron IONIC BONDING

15. POLYATOMIC IONS--a group of atoms that act like one ion NH 4 +1 --ammonium ion CO 3 -2 --carbonate ion PO 4 -3 --phosphate ion IONIC BONDING

16. POLYATOMIC IONS ACT JUST LIKE ANY OTHER NEGATIVE ION WHEN BONDING IONIC BONDING

17. SODIUM SULFATE

18. IONIC BONDING

19. Properties of Ionic Compounds Crystalline structure. A regular repeating arrangement of ions in the solid. Ions are strongly bonded. Structure is rigid. High melting points- because of strong forces between ions.

21. COVALENT BONDING When an atom of one nonmetal shares one or more electrons with an atom of another nonmetal so both atoms end up with eight valence electrons

22. COVALENT BOND FORMATION When one nonmetal shares one or more electrons with an atom of another nonmetal so both atoms end up with eight valence electrons

23. COVALENT BONDING IS THE COMPOUND A COVALENT COMPOUND?NONMETAL NONMETAL YES since it is made of only nonmetal elements

24. Covalent bonding Fluorine has seven valence electrons F

25. Covalent bonding Fluorine has seven valence electrons A second atom also has seven FF

26. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons FF

27. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons FF

28. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons FF

29. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons FF

30. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons FF

31. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons l Both end with full orbitals FF

32. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons l Both end with full orbitals FF 8 Valence electrons

33. Covalent bonding l Fluorine has seven valence electrons l A second atom also has seven l By sharing electrons l Both end with full orbitals FF 8 Valence electrons

34. Single Covalent Bond A sharing of two valence electrons. Only nonmetals and Hydrogen. Different from an ionic bond because they actually form molecules. Two specific atoms are joined. In an ionic solid you can’t tell which atom the electrons moved from or to.

35. How to show how they formed It’s like a jigsaw puzzle. I have to tell you what the final formula is. You put the pieces together to end up with the right formula. For example- show how water is formed with covalent bonds.

36. Water H O Each hydrogen has 1 valence electron Each hydrogen wants 1 more The oxygen has 6 valence electrons The oxygen wants 2 more They share to make each other happy

37. Water Put the pieces together The first hydrogen is happy The oxygen still wants one more H O

38. Water The second hydrogen attaches Every atom has full energy levels H O H

39. Covalent Bonds

40. LET’S FIRST REVIEW IONIC BONDING

41. In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds. FK

42. FK

43. FK

44. FK

45. FK

46. FK

47. FK

48. FK + _

49. FK + _ The compound potassium fluoride consists of potassium (K + ) ions and fluoride (F - ) ions

50. FK + _ The ionic bond is the attraction between the positive K + ion and the negative F - ion

51. So what are covalent bonds?

52. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule).

53. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair.

54. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair

55. Cl 2 Chlorine forms a covalent bond with itself

56. Cl How will two chlorine atoms react?

57. Cl Each chlorine atom wants to gain one electron to achieve an octet

58. Cl Neither atom will give up an electron – chlorine is highly electronegative. What’s the solution – what can they do to achieve an octet?

59. Cl

63. octet

64. Cl circle the electrons for each atom that completes their octets octet

65. Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

66. Cl circle the electrons for each atom that completes their octets The octet is achieved by each atom sharing the electron pair in the middle

67. Cl circle the electrons for each atom that completes their octets This is the bonding pair

68. Cl circle the electrons for each atom that completes their octets It is a single bonding pair

69. Cl circle the electrons for each atom that completes their octets It is called a SINGLE BOND

70. Cl circle the electrons for each atom that completes their octets Single bonds are abbreviated with a dash

71. Cl circle the electrons for each atom that completes their octets This is the chlorine molecule, Cl 2

72. O2O2 Oxygen is also one of the diatomic molecules

73. How will two oxygen atoms bond? OO

74. OO Each atom has two unpaired electrons

75. OO

76. OO

77. OO

78. OO

79. OO

80. OO

81. Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

82. Oxygen atoms are highly electronegative. So both atoms want to gain two electrons. OO

83. OO

84. OO

85. OO

86. OO

87. O O Both electron pairs are shared.

88. 6 valence electrons plus 2 shared electrons = full octet O O

89. 6 valence electrons plus 2 shared electrons = full octet O O

90. two bonding pairs, O O making a double bond

91. O O = For convenience, the double bond can be shown as two dashes. O O

92. O O = This is the oxygen molecule, O 2 this is so cool! !

94. Multiple Bonds Sometimes atoms share more than one pair of valence electrons. A double bond is when atoms share two pair (4) of electrons. A triple bond is when atoms share three pair (6) of electrons.