1. Chemical Bonding

2. A Chemical Bond is a mutual electrical attraction between the nuclei of one atom and the valence electrons of another atom.
This attraction binds the atoms together.

3. Bonding between atoms occurs because:
Bonding between atoms occurs because: *it creates a more stable arrangement for atoms *all atoms want to be like the noble gases and have a completely filled outer shell

4. 3 Types of Bonding Metallic bonding – “metal to metal”
Results from the attraction between metal atoms and the surrounding sea of electrons
Ionic bonding – “nonmetal to metal”
Results from the electrical attraction between large number of cations and anions. It involves the transfer of electrons from one atom to another
Covalent bonding – “nonmetal to nonmetal”
Results from the sharing of electron pairs between two atoms

5. Ionic Bonding sodium atom chlorine atom Na Cl
Many atoms transfer electrons and other atoms accept them. This creates cations (positive ions) and anions (negative ions).
sodium atom chlorine atom
Na Cl
sodium ion - Na+1 chlorine ion – Cl-1
Na Cl

6. Ionic Bonding
Ionic bonding is the electrostatic attraction between positive cations and negative anions. This is the strongest bond type.

7. Covalent Bonding a “tug-of-war”
In many cases electrons do not completely transfer from one atom to another. The electrons between atoms are shared -like a “tug of war”
Consider two hydrogen atoms:
Hydrogen Hydrogen
H H
The two hydrogen atoms SHARE the 2 electrons equally, giving each atom 2 electrons
H:H

8. NON-POLAR Covalent Bonding: an EQUAL “tug-of-war”
the electron orbitals overlap or “share” electrons
When electrons are shared equally the bond is called a nonpolar or pure covalent bond

9. POLAR Covalent Bonding: an UNEQUAL “tug-of-war”
A polar covalent bond is when the electrons between two atoms are NOT shared equally. It is an unequal tug-of- war.
Each Atom donates one electron to be shared to give each a stable, filled outer energy level

10. POLAR Covalent Bonding an UNEQUAL “tug-of-war”
But sometimes, the two electrons are shared UNEQUALLY…one atom “tugs” harder on the shared electron pair (in this case the Cl is stronger). This creates an uneven distribution of charge. The H will have a partial positive charge ( ) and the Cl will have a partial negative charge ( ).

11. POLAR Covalent Bonding an UNEQUAL “tug-of-war”
Since this bond has two “poles” – a positive pole and a negative pole – it is called a
Polar Covalent Bond
H Cl

12. Ionic, Polar Covalent or Non-Polar Covalent ??????
We use electronegativities to determine whether we have an ionic, polar or non-polar bond
An electronegativity value is a number ranging from 0.0 to 4.0 that shows the tendency of an atom to attract electrons towards itself.

13. Electronegativity Chart
The electronegativity values for the elements are found on an “electronegativity chart”, which looks like the periodic table. The numbers on the chart are the electronegativity values for that element. The HIGHER the number, the STRONGER the attraction for the electrons.

14. Ionic, Polar or Non-Polar ??????
How do we determine what type of bond will occur between two atoms?
The DIFFERENCE between their electronegativity values (EN) will tell us:
electronegativity bond
difference ( EN) type
1.7 and higher ionic
0.3 – polar
0.0 – non-polar

15. Ionic, Polar or Non-Polar ??????
What type of bond will occur between Iodine (EN= 2.7) and the following elements: cesium (EN=0.8), iron (EN=1.8) and sulfur (EN=2.5)
Bond between Iodine
and
Electronegativity difference
Bond Type
More negative atom
cesium
2.7 – 0.8 = 1.9
iron
2.7 – 1.8 = 0.9
sulfur
2.7 – 2.5 = 0.2

16. Determine the type of bond between the following pairs:
Bonding between:
EN difference
Bond Type
More negative atom
Na and Cl
S and O
Ca and Br
P and H
Si and Cl
S and Br
1.7 and greater IONIC
0.3 – 1.7 Polar
0.0 – 0.3 Non-Polar

17. What if the electronegativity difference is 0. 3 or 1. 7
What if the electronegativity difference is 0.3 or 1.7? What type of bond is it?
The cut-off numbers are guidelines, not definite delineation points. It is more of a gradual change from one bond type to another.

18. Draw pictures of the bonds in the previous table
Draw pictures of the bonds in the previous table. Show the distribution of charge.
Sodium and chlorine ionic bond Sulfur and oxygen polar covalent S O

19. Draw these bonds. Show the distribution of charge if polar
Calcium and Bromine
Phosphorus and hydrogen
Silicon and chlorine
Sulfur and bromine