1. Chemical Bonding

2. Chemical Bonding is the mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.

3. chemical formula.
The composition of a formula is given by its chemical formula.
A chemical formula indicates the relative number of atoms combined using atomic symbols and numeric subscripts
H2O, C6H12O8, FeCl3, CaS, Li3P

4. Diatomic molecules Di = two Atomic = atoms two atoms
Diatomic molecules contain only two atoms. F2 H2
NaCl

5. Learn the following diatomic elements
Cl2
Br2 I2
At2 H2 O2 N2
HalHON
All the hologens plus Hydrogen, Oxygen and Nitrogen

6. Lewis Structures Lewis Structures only show the valence electrons.
Write the element symbol C

7. Lewis Structures
Place one dot to the right of the symbol
C 

8. Lewis Structures
Then add the next electron below the symbol
C  

9. Lewis Structures
The next electron goes to the left
C  

10. Lewis Structures
Continue moving around the symbol until all electrons have been added.
 
N  

11. Lewis Structures
Using electron dot diagrams, a diatomic molecule of hydrogen can be represented as H
 H
B period ¼

12. Write the Lewis Structures for the following elements
Li Be B C
N O F Ne

13. Lewis Structures are useful in seeing where an atom is willing to make a bond
Atoms can not bond when electrons are paired

14. Helium has full shell with two electrons So it is written

15. N has 5 valence electrons
 N:
It can only bond in three spots

16. Chemical Bonding There are several types of bonds – Ionic Covalent
Metallic

17. Covalent bonds
Covalent bonds are when nonmetallic elements share an electron pair.
Nm Nm

18. This can be two hydrogen atoms, H2 or many different elements such as in sucrose (C6H12O6)

19. Molecular compound
Molecular compound is the simplest unit for molecules.
Remember that only the valance electron are involved in bonding.
A molecule is a neutral group of atoms that are held together by covalent bonds.
Atoms share electrons

20. Covalent bonds are when nonmetallic elements share an electron pair.
Nm Nm
1s 2s p
F      .
F      .
F           F
F          F
 This is the octet rule for covalent bonding.

21. There are several types of covalent bonds.
Polar
Nonpolar
Coordinate
They tell how well elements share electrons

22. Polar Covalent
is a covalent bond that does not share the electrons equally.
One side is slightly + and the other is slightly –
Because there are two poles of charge involve, the bond is a dipole.
H O

23. A dipole caused by the polar covalent bond of the water molecule

24. Nonpolar Covalent
is a covalent bond where the electrons are evenly shared.
F F

25. Electronegativity! So how do we know what type of bond we have?
Covalent
Nonpolar Polar Ionic
E %

26. Sulfur’s electronegativity is 2.5 Hydrogen’s electronegativity is 2.1
Use the electronegative difference to determine the bond type. The electronegativity can be found on the periodic table
Sulfur and Hydrogen
Sulfur’s electronegativity is 2.5
Hydrogen’s electronegativity is 2.1
S – H = = 0.4
Where does it fall?
Polar covalent

27. Which element is least negative?
So it is written first in the formula

28. Try some more F2 or F – F, SF4, LiF Compound F2 SF4 LiF
Electronegativity Difference
Type of Bond

29. The HF (Hydrofluoric) can be written: + -
+ -
H – F HF
The '+' and '-' symbols indicate partial positive and negative charges.

30. Coordinate covalent
bond is a bond formed when one atom provides both electrons in a shared pair.
H N H H

31. How do we know if a double or triple bond in needed?
Using the equations to correctly draw the Lewis Structure and Structural Formula for each of the following.
All Single Bonds
6(N) + 2 = VE
N= number of atoms (not counting H)
VE = # of valence electrons

32. No interaction between atomsp+ e- p+ e-

33. Attraction begins p+ e- p+ e-

34. Covalent bond forms
p p+ e-

35. Network Solids
"Covalent Crystals" (crystal is used to describe Ionic structures) (Diamonds)
Hard
Good insulators
Transparent
High Melting Point

36. Properties of Covalent Compounds
These are poor conductors of electricity in the fused or dissolved state
Nonelectrolytes-do not conduct electricity in water
Poor conductors of heat and electricity
Brittle or cleave rather than deform

37. Covalent Compounds Exist as neutral molecules (C6H12O2)
Solids, liquids, or gases (C6H12O2(s), H2O(l), CO2(g))
Lower melting and boiling points (i.e., often exist as a liquid or gas at room temperature)

38. Covalent Compounds
Relatively weak force of attraction between molecules
Remain as same molecule in water and will not conduct electricity
H2O(l),
C6H12O2(s) → C6H12O2(aq)

39. Naming Covalent Compounds
All covalent compounds have two word names.  The first word is the first element in the formula and the second corresponds to the second element in the formula except that "-ide" is substituted for the end. 

40. Rules for Naming Binary Covalent Compounds
A binary covalent compound is composed of two different nonmetal elements. For example, a molecule of chlorine trifluoride, ClF3 contains 1 atom of chlorine and 3 atoms of fluorine.

41. Rules for Naming Binary Covalent Compounds
Rule 2. The second element in the name is named as if it were an anion, i.e., by adding the suffix -ide to the name of the element.

42. Rules for Naming Binary Covalent Compounds
Rule 3. If both elements are in the same group, the element with the bigger period number is written first in the name. So , BrF is named “bromine fluoride", because bromine is the first element and fluorine is the second element.

43. Rules for Naming Binary Covalent Compounds
Rule 4. Greek prefixes are used to indicate the number of atoms of each nonmetal element in the chemical formula for the compound.
Exception: The only time “mono” is used is with oxygen

44. Naming Covalent Compounds
If there is more than one atom of an element in a molecule, we need to add prefixes to these words to tell us how many are present.  Here are the prefixes you'll need to remember:

45. mono- (use only for oxygen)
Prefixes for Covalent
Number of atoms
Prefix 1
mono- (use only for oxygen) 2
di- 3
tri- 4
tetra- 5
penta- 6
hexa- 7
hepta- 8
octa- 9
Nona- 10
Deca-

46. Naming Practice SH2 P2S3 C4F10 NO sulfur dihydride diphosphorous
trisulfide
tetracarbon
decafluoride
nitrogen
monoxide

47. Some important exceptions
To the naming scheme occur because the compounds were originally named before the methodical naming scheme above became widespread.  Nowadays, these names are so common that they're officially recognized:
H2O is "water"
NH3 is "ammonia"
CH4 is "methane"