1. Notes – Chemical Bonding and Electron Transfer Assign # 30 pt.

2. Chemical Bonding Chemical Bonds – Chemical forces which hold atoms together and form complete electrons shells Atoms of elements will transfer or share electrons to reach the stable octet number. Inert (Noble) Gases have 8 valence electrons (2 for He) and are stable Nonmetals –Groups 5a to 7a will gain electrons to become stable Metals – Groups 1a to 3a will lose electrons to become stable

3. Chemical Bonds – Chemical forces which hold atoms together and form complete electrons shells Ionic Bond – Positive (+) and negative (-) ions attract – formed by the transfer of valence electrons. Na11p+11p+ 11e-10e- =+1 Na Cl17p+17p+ 17e-18e- =-1 Cl Na +1 + Cl -1 = NaCl o

4. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)

5. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)

6. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-) Na = 11 p+ 11 e - 10 e-

7. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)

8. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-) Cl = 17 p+ 17 e - 18 e-

9. Ionic Bonds Ion – is an atom or group of atoms that have an electric charge. Atoms become charged when they lose or gain electrons to become stable Atoms which lose electrons become positive (+) Atoms which gain electrons become negative (-) Na +1 + Cl -1 = NaCl o

10. Ionic bond Atoms which lose electrons become positive (cations) Lose 1 = +1 Lose 2 = +2 Lose 3 = + 3 Atoms which gain electrons become negative (anions) Gain 1 = - 1 Gain 2 = - 2 Gain 3 = -3

11. Ionic Bond Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions Na + plus Cl - combining to form NaCl is an example

12. Ionic Bond Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions Na + plus Cl - combining to form NaCl is an example

13. Ionic Bond Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions Na + plus Cl - combining to form NaCl is an example

14. Ionic Bond Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions Na + plus Cl - combining to form NaCl is an example

15. Ionic Bond Ionic Bond – a type of chemical bond formed from the attraction of two oppositely charged ions Na + plus Cl - combining to form NaCl is an example A compound consisting of positive and negative ions such as NaCl = sodium chloride is an Ionic Compound Sodium Chloride Ionic Compound

18. Table Salt

22. Oxidation – Reduction Reactions Reduction – Any reaction in which a reactant can be considered to gain one or more electrons. Elements or ions which lose electrons are said to be reduced. Cu 2+ + 2e - = Cu Copper II ion Copper metal Reduction Reaction. Copper ions are reduced

23. Oxidation – Reduction Reactions Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons. Elements or ions which gain electrons are said to be oxidized. Cu = Cu 2+ + 2e - Copper metal Copper II ion Oxidation Reaction. Copper ions are oxidized

24. Oxidation – Reduction Reactions Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons. Elements or ions which gain electrons are said to be oxidized. Cu = Cu 2+ + 2e - Copper metal Copper II ion Oxidation Reaction. Copper ions are oxidized Oil Rig : Oxidation is Loss (of electrons), Reduction is Gain (of electrons)

25. Oxidation – Reduction Reactions Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons. Elements or ions which gain electrons are said to be oxidized. Cu = Cu 2+ + 2e - Copper metal Copper II ion Oxidation Reaction. Copper ions are oxidized Oil Rig : Oxidation is Loss (of electrons), Reduction is Gain (of electrons) Cu + O 2 = 2CuO Copper is Oxidized Oxygen is Reduced

26. Oxidation – Reduction Reactions Oxidation – Any reaction in which a reactant can be considered to lose one or more electrons. Elements or ions which gain electrons are said to be oxidized. Cu = Cu 2+ + 2e - Copper metal Copper II ion Oxidation Reaction. Copper ions are oxidized Oil Rig : Oxidation is Loss (of electrons), Reduction is Gain (of electrons) Cu + O 2 = 2CuO Copper is Oxidized Oxygen is Reduced Copper loses electrons Oxygen gains electrons

27. Metals can be changed to ions by oxidation. Mg Mg 2+ + 2e - Metallic ions can be changed to metals by reduction. Al 3+ + 3e - Al Oxidation – Reduction Reactions

28. Metals and Metal ions will react in a Redox, Reduction- Oxidation reaction. The more active metal will react with a less active ion in a replacement reaction Cu + Ag + Ag + Cu + Cu is oxidized, Ag + is reduced Cu loses an e -, Ag gains an e - Oxidation – Reduction Reactions

29. Metallic bonding Metal atoms combine in regular patterns in which valence electrons are free to move from atom to atom. Most metals have from 1 to 3 valence electrons and are positive ions. Metal ions are held in place by a metallic bond an attraction between a positive metal ion and the many electrons surrounding it.

30. Metallic bonding Most metals have from 1 to 3 valence electrons and are positive ions. Metal ions are held in place by a metallic bond an attraction between a positive metal ion and the many electrons surrounding it.

31. Metal Properties Metals properties are attributed to the “sea of electrons” flowing over the positive ions Malleable and ductile – metal’s positive ions are attracted to electrons and can slide into different positions

32. Metal Properties Luster – When light strikes the valence electrons they absorb it than give it off again Electrical and Thermal conductivity – valence electrons move freely and cause electric current to flow or heat to flow easily from hot to cold

33. 1 2 3456 7 8 1 2 3 4 5 6 7

34. Covalent Bonding Covalent Bond – the chemical bond formed when atoms share electrons The force holding them together is the attraction of the nucleus and the shared electrons

35. Covalent Bonding Covalent Bond – the chemical bond formed when atoms share electrons The force holding them together is the attraction of the nucleus and the shared electrons Usually forms between atoms of nonmetals

36. Covalent Bonding Covalent Bond – the chemical bond formed when atoms share electrons The force holding them together is the attraction of the nucleus and the shared electrons Usually forms between atoms of nonmetals The neutral group of atoms joined by covalent bonds is called a molecule

37. Covalent Bonding The neutral group of atoms joined by covalent bonds is called a molecule Molecular compounds is a compound composed of covalently bonded molecules

38. v v

39. Covalent bonding – Sharing of valence electrons to fill electron shells Follows octet rule, except for H and He Common elements- H, C, N, 0 Lines show shared electrons H O H

40. H 2 0 – Molecular formula H O H - Structural formula – shows the number and position of atoms O NC Show the bonds formed when these atoms combine with Hydrogen (H. )

41. H 2 0 – Molecular formula H O H - Structural formula – shows the number and position of atoms Show the bonds formed when these atoms combine with each other H + H= Cl + Cl = Br + Br =

42. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons O + O =

43. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons O + O =

44. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons O + O = O + C + O =

45. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons O + O = O + C + O =

46. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 3 atoms sharing 2 pairs of electrons O + O = O + C + O =

47. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons O + O =

48. Covalent Bonding Double bond – Some covalent bonds involve 2 atoms sharing 2 pairs of electrons Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons O + O = O + C + O = N + N =

49. Covalent Bonding Triple bond – Some covalent bonds involve 2 atoms sharing 3 pairs of electrons N + N = C + O =

50. Table Salt NaCl- Sodium Chloride Sugar - glucose

51. Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound. Ex: Al 2 O 3 = 2 aluminum and 3 oxygen Examples- NaCl MgCl 2 Li 2 Cl Al 2 O 3 K 2 SO 4 Chemical formulas

52. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound Ex: Al 2 O 3 = 2 aluminum and 3 oxygen When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Examples- NaCl = MgCl 2 Li 2 Cl Al 2 O 3 K 2 SO 4 Types of Matter

53. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound Ex: Al 2 O 3 = 2 aluminum and 3 oxygen When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Examples- NaCl = Sodium Chloride MgCl 2 Li 2 Cl Al 2 O 3 K 2 SO 4 Types of Matter

54. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound Ex: Al 2 O 3 = 2 aluminum and 3 oxygen When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Examples- NaCl = Sodium Chloride MgCl 2 =Magnesium Chloride Li 2 Cl Al 2 O 3 K 2 SO 4 Types of Matter

55. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound Ex: Al 2 O 3 = 2 aluminum and 3 oxygen When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Examples- NaCl = Sodium Chloride MgCl 2 =Magnesium Chloride Li 2 Cl = Lithium Chloride Al 2 O 3 K 2 SO 4 Types of Matter

56. Chemical formulas – Abbreviated form of compound showing the element symbols and ratio of atoms A subscript shows you the number and ratio of atoms in a compound Ex: Al 2 O 3 = 2 aluminum and 3 oxygen When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Examples- NaCl = Sodium Chloride MgCl 2 =Magnesium Chloride Li 2 Cl = Lithium Chloride Al 2 O 3 = Aluminum Oxide K 2 SO 4 Types of Matter

57. Chemical formulas – When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Ions that are made of more than one atom are called polyatomic ions. Ex: SO 4 = sulfate Examples- NaCl = Sodium Chloride MgCl 2 =Magnesium Chloride Li 2 Cl = Lithium Chloride Al 2 O 3 = Aluminum Chloride K 2 SO 4 = Potassium Sulfate Types of Matter

58. Chemical formulas – When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Ions that are made of more than one atom are called polyatomic ions. Ex: SO 4 = sulfate Examples- LiCl = K 2 S = CaF 2 = MgO 2 = Na 2 PO 4 = Types of Matter

59. Chemical formulas – When naming ionic compounds the positive ion comes first, followed by the name of the negative ion Ions that are made of more than one atom are called polyatomic ions. Ex: SO 4 = sulfate Examples- LiCl = Lithium Chloride K 2 S = Potassium Sulfide CaF 2 = Calcium Flouride MgO 2 = Magnesium Oxide Na 2 PO 4 = Sodium Phosphate Types of Matter

60. Table Salt NaCl- Sodium Chloride Sugar - glucose