1. Bonding

2. Why do elements bond? Bonding results in greater stability
Through sharing electrons- covalent
Through transfer of electrons- ionic
Compounds have different properties than elements
Sodium Chloride vs. Sodium and Chlorine

3. Covalent Bonds Covalent Bonds- sharing of electrons to become stable
Results in a molecule- 2 or more atoms covalently bonded
Occurs between 2 nonmetals
Have relatively low melting points so often liquid or gas at room temperature
No ions, so do not conduct if dissolved in water
Single Covalent bond- sharing of 2 electrons
Longest and weakest of the 3 covalent bonds
Double Covalent bond- sharing of 4 electrons
Triple Covalent bond- sharing of 6 electrons
Shortest and strongest

4. Covalent bonding
Fluorine has seven valence electrons (but would like to have 8) F

5. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven F F

6. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons… F F

7. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons… F F

8. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons… F F

9. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons… F F

10. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons… F F

11. F F Covalent bonding …both end with full orbitals
Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons…
…both end with full orbitals F F

12. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons…
…both end with full orbitals F F
8 Valence electrons

13. F F Covalent bonding Fluorine has seven valence electrons
A second atom also has seven
By sharing electrons…
…both end with full orbitals F F
8 Valence electrons

14. B. Covalent Bond
covalent bonds result in discrete molecules
NH3
H2O
Cl2

15. Covalent Bonds

16. Covalent Bonds

17. Covalent Bonds

18. Covalent Bonds

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

21. Dot diagram for Carbon dioxide
CO2 - Carbon is central atom ( more metallic )
Carbon has 4 valence electrons
Wants 4 more
Oxygen has 6 valence electrons
Wants 2 more C O

22. Carbon dioxide
Attaching 1 oxygen leaves the oxygen 1 short, and the carbon 3 short C O

23. Carbon dioxide
Attaching the second oxygen leaves both of the oxygen 1 short, and the carbon 2 short O C O

24. Carbon dioxide
The only solution is to share more O C O

25. Carbon dioxide
The only solution is to share more O C O

26. Carbon dioxide
The only solution is to share more O C O

27. Carbon dioxide
The only solution is to share more O C O

28. Carbon dioxide
The only solution is to share more O C O

29. O C O Carbon dioxide The only solution is to share more
Requires two double bonds
Each atom can count all the electrons in the bond O C O

30. O C O Carbon dioxide The only solution is to share more
Requires two double bonds
Each atom can count all the electrons in the bond
8 valence electrons O C O

31. O C O Carbon dioxide The only solution is to share more
Requires two double bonds
Each atom can count all the electrons in the bond
8 valence electrons O C O

32. O C O Carbon dioxide The only solution is to share more
Requires two double bonds
Each atom can count all the electrons in the bond
8 valence electrons O C O

33. N H C H C N HCN has a triple bond! H needs 1 electron
C needs 4 electrons
N needs 3 electrons
Bond between H and C is a single bond
Bond between C and N is a triple bond
Single bonds 1 pair shared
Double bonds 2 pairs shared
Triple bonds 3 pairs shared C N N H C

34. B. Covalent Bond Nonpolar Covalent Bond e- are shared equally
usually identical atoms

35. + - B. Covalent Bond Polar Covalent Bond
e- are shared unequally between 2 different atoms
results in partial opposite charges + -

36. B. Covalent Bond
Nonpolar
Polar
Ionic
View Bonding Animations.

37. Polar vs. Nonpolar

39. Video! Ionic and Covalent Bonding.

40. C. Comparison Chart IONIC COVALENT transferred from metal to nonmetal
shared between nonmetals
Electrons
Melting
Point
high
low
Soluble in
Water
yes
usually not
yes (solution or liquid)
Conduct Electricity no
crystal lattice of ions, crystalline solids
molecules, odorous liquids & gases
Other
Properties

41. Metallic bonding: The bonding between atoms within metals
Metallic bonding: The bonding between atoms within metals. The sharing of many free electrons.
Copyright © 2010 Ryan P. Murphy

43. Remember:
Covalent – Sharing an Electron many of the SPONCH elements.

44. Remember:
Covalent – Sharing an Electron many of the SPONCH elements.
Ionic – Opposite charges + / -

45. Remember:
Covalent – Sharing an Electron many of the SPONCH elements.
Ionic – Opposite charges + / -
Metallic – Many electrons

48. Metallic

49. Metallic

50. Metallic
Ionic

51. Metallic
Ionic

52. Covalent
Metallic
Ionic

53. Covalent
Metallic
Ionic

54. Chemical Formulas
Chemical formula- used to tell us how many of each element are in a compound
Consists of element symbols and subscripts
Water has 2 hydrogen atoms and 1 oxygen atom

55. Chemical Formulas SiO2 silicon- 1 Oxygen-2 C12H22O11
Carbon- 12 Hydrogen-22 Oxygen-11
N2O
Nitrogen- 2 Oxygen-1

56. Ionic Compounds Ionic compound - composed of cations and anions
Metal (cation) & nonmetal (anion) OR metal & polyatomic ion
Polyatomic Ions- groups of atoms that are covalently bonded and collectively have a charge
Examples of polyatomic ions: SO42- PO43-

57. Ionic Compounds Ionic compound - composed of cations and anions
Metal (cation) & nonmetal (anion) OR metal & polyatomic ion
Neutral overall
Total positive charge = total negative charge
Solid crystals at room temperature
Melt only at very high temperatures
Ionic Bond: The electrostatic forces that hold ions together in ionic compounds

58. Properties of Ionic Compounds
7.2
Properties of Ionic Compounds
The orderly arrangement of component ions produces the beauty of crystalline solids.
The beauty of crystalline solids, such as these, comes from the orderly arrangement of their component ions.

59. Sodium Chlorine Sodium Chloride
CLICK FOR ANIMATION OF IONIC and COVALENT BONDING

60. Writing Lewis Dot Structures for covalent compounds
Count up total number of valence electrons
Determine the central atom
C is often the central atom
For now, the single atom will be the central atom
Bond atoms to satisfy the octet rule first
Fill in valence electrons
If all atoms are not stable, you’ll need to try double or triple bonds
If you have extra electrons, put them on the central atom
For more detailed rules: