1. CHEMICAL BONDING
IONIC BONDS
COVALENT BONDS
HYDROGEN BONDS

2. IONIC BONDING

3. 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

4. IONIC BONDING IS THE COMPOUND AN IONIC COMPOUND? Mg 3 N2 METAL
NONMETAL
SUBSCRIPTS

5. IONIC BOND FORMATION Non-Metal Metal
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.

6. ION – any atom with more or less electrons that it is
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

7. Metals will tend to lose electrons and become
IONIC BONDING
Metals will tend to lose electrons and become
POSITIVE CATIONS = Na
11 p
10 e + -
to become sodium ion + -
11 p
11 e Na
Normal sodium atom - 1e
loses one electron

8. Nonmetals will tend to gain electrons and become
IONIC BONDING
Nonmetals will tend to gain electrons and become
NEGATIVE ANIONS
17 p
17 e + - Cl
Normal chlorine atom = Cl
17 p
18 e + -
to become a chloride ion + 1e -
gains an electron

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

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

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

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

13. NH4+1 ammonium ion CO3-2 carbonate ion PO4-3 phosphate ion
IONIC BONDING
POLYATOMIC IONS--a group of atoms that act like one ion
NH ammonium ion
CO carbonate ion
PO phosphate ion

14. POLYATOMIC IONS ACT JUST LIKE ANY OTHER NEGATIVE ION WHEN BONDING
IONIC BONDING
POLYATOMIC IONS ACT JUST LIKE ANY OTHER NEGATIVE ION WHEN BONDING
Na1+ SO42-

15. IONIC BONDING
Na2 SO4
SODIUM SULFATE

16. IONIC BONDING
Al3+ NO1-3
Al1(NO3)3

17. 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.

18. Crystalline structure
The POSITIVE CATIONS stick to the NEGATIVE ANIONS, like a magnet. + + - - - - + + - + - + + - - - + +

19. COVALENT BONDING

20. When an atom of one nonmetal shares one or more electrons
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

21. 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

22. COVALENT BONDING IS THE COMPOUND A COVALENT COMPOUND? C O2 NONMETAL
YES since it is made of only nonmetal elements

23. Covalent bonding
Fluorine has seven valence electrons F

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

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

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

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

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

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

30. 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

31. 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

32. 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

33. 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.

34. 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.

35. H O Water 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 H O

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

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

38. 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.

39. C O Carbon dioxide CO2 - Carbon is central atom ( I have to tell you)
Carbon has 4 valence electrons
Wants 4 more
Oxygen has 6 valence electrons
Wants 2 more C O

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

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

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

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

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

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

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

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

48. O C O Carbon dioxide The only solution is to share more
Requires two double bonds
Each atom gets to count all the atoms in the bond O C O

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

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

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

52. N H Examples NH3 N - has 5 valence electrons wants 8
H - has 1 valence electrons wants 2
NH3 has 5+3(1) = 8
NH3 wants 8+3(2) = 14
(14-8)/2= 3 bonds
4 atoms with 3 bonds H

53. H H N H Examples Draw in the bonds All 8 electrons are accounted for
Everything is full H H N H

54. H C N HCN Put in single bonds Need 2 more bonds
Must go between C and N H C N

55. H C N HCN Put in single bonds Need 2 more bonds
Must go between C and N
Uses 8 electrons - 2 more to add H C N

56. H C N HCN Put in single bonds Need 2 more bonds
Must go between C and N
Uses 8 electrons - 2 more to add
Must go on N to fill octet H C N

57. H C N H C O H Structural Examples
C has 8 electrons because each line is 2 electrons
Ditto for N
Ditto for C here
Ditto for O
H C N H
C O H

58. Polar Bonds
When the atoms in a bond are the same, the electrons are shared equally.
This is a nonpolar covalent bond.
When two different atoms are connected, the atoms may not be shared equally.
This is a polar covalent bond.
How do we measure how strong the atoms pull on electrons?

59. How to show a bond is polar
Isn’t a whole charge just a partial charge
d+ means a partially positive
d- means a partially negative
The Cl pulls harder on the electrons
The electrons spend more time near the Cl d+ d- H Cl

60. Polar Molecules
Molecules with ends

61. Polar Molecules Molecules with a positive and a negative end
Requires two things to be true
The molecule must contain polar bonds
This can be determined from differences in electronegativity.
Symmetry can not cancel out the effects of the polar bonds.
Must determine geometry first.

62. Is it polar? HF
H2O
NH3
CCl4
CO2

63. Hydrogen bonding
Are the attractive force caused by hydrogen bonded to F, O, or N.
F, O, and N are very electronegative so it is a very strong dipole.
The hydrogen partially share with the lone pair in the molecule next to it.
The strongest of the intermolecular forces.

64. Hydrogen Bonding H O d+ d- H O d+ d-

65. Hydrogen bonding H O H O H O H O H O H O H O