1. Covalent Bonding
Chapter 7:

2. What is covalent bonding?
Covalent bonding is the force that holds two or more atoms together when electrons are shared between atoms to achieve a stable number of electrons in the outer shell.
The shared electrons continually move between the two atoms acting to fill two outer shell orbitals at once.
Covalent molecules usually have a zero charge and individual molecules are held together by intermolecular forces.

3. Electron shell diagrams
Both Chlorine atoms want one more electron in their outer shell.
By sharing their unpaired electrons both atoms achieve a full outer shell.

4. Electron dot diagrams – Lewis diagrams
Electrons occur in pairs in their shells. In the outer shell the first four electrons will fill singularly creating four single electrons and the opportunity for four bonds.
After this, the electrons start to pair up, so the number of bonds that can be formed decreases until the outer shell is full.

5. Single, double and triple bonds
Some covalent molecules can form double bonds. These are stronger than a single bond.
Triple bonds may also be formed.

6. Drawing covalent molecules
The symbol for each atom is represented with lines branching from it to the atom(s) it is bonded to. This should be done so as to represent the 3D shape of the molecule.
Benzene

7. Shapes of common molecules

8. Naming covalent molecules
SO3 would be called Sulphur trioxide
N2O5 would be called dinitrogen pentoxide
OCl2 would be called oxygen dichloride

9. Naming covalent molecules
Have a go at naming the following: NCl3 SF6 CO PH3 SiH4 N2O

10. Polar and non polar bonds
A bond is considered polar if there is an unequal sharing of electrons in the bond This is due to the difference in electronegativity (ability to attract an electron) Keep in mind that just because a molecule has polar bonds within it, it does not necessarily become classed as a polar molecule

11. Polar and non polar molecules
To add to the confusion many covalent molecules are what we call polar.
This means that one end of the molecule has a slightly positive ( + ) charge and the other end a slightly negative ( - ) charge.
This is because some atoms
attract electrons more than
others. This is called
electronegativity.

12. Draw a dot diagram and a structural diagram of the following polar molecules and identify the polar bond/s:
HCl
H2O
CH3Cl

13. Identifying polarity Does the molecule have a dipole covalent bond?
Can dipole charges be assigned to the ends of the molecule?
Do these dipole charges cancel each other out?
Is there 0 or 1 line of symmetry?
Does the dipole charges have a direction?

14. Intramolecular forces
So far we have been talking about forces within a molecule. Is the molecule polar? Or non-polar? However, most covalent substances are made up of more than one singular molecule so we also need to talk about forces that hold these individual molecules together. Eg. Water is made up of many H2O molecules, how are these molecules held together??

15. Intermolecular attractions
Covalent molecules can form liquids and solids which means there must be some kind of forces holding these molecules together.
Dispersion forces are very weak forces of attraction between all molecules.

16. Dispersion Forces (Van der Waals) Weakest Intermolecular force
In a sample of molecules, the nuclei of atoms in one molecule are able to attract the electrons of atoms in neighbouring molecules.
All electrons are attracted by neighbouring nuclei, thus, dispersion forces are present in all molecules.
Instantaneous dipoles can also contain dispersion forces

17. Dispersion Forces (Van der Waals) Weakest Intermolecular force
Two factors influence the strength of dispersion forces:
The number of electrons in the molecules. In general, the more electrons the molecules of a substance have, the stronger the dispersion forces between them.
The shapes of the molecules. Shape affects how closely the molecules may approach each other. The closer the molecules can get, the stronger the attraction will be.

18. Dipole – Dipole interactions
Polar molecules attract one another as the positive dipole will be attracted to the negative dipole of another molecule.
This will result in compounds with higher boiling points.
Polarity also determines which covalently bonded liquids will mix and which will not.
Water is a polar molecule and oil is non polar. These liquids will not mix – immiscible.

19. Hydrogen Bonding
Hydrogen bonding is a special case of Dipole-dipole attraction
When H bonds to a more electronegative atom, its sole electron is drawn to the other atom, leaving its nucleus exposed. This forms a dipole and as the H nucleus in unshielded, other molecules can approach far more closely.
This is especially the case when hydrogen is bonded to Nitrogen, Fluorine and Oxygen.
It creates a much stronger dipole bond, known as a Hydrogen bond.
High melting and boiling points
Hydrogen bonds are vitally important for life as they keep water as a liquid at room temperature, give proteins their unique shape and hold the two DNA strands together.

20. Properties of Covalent structures
A great variety of physical properties occurs due largely to the differences in the strength of the intermolecular attractions.
Don’t conduct electricity in sold/molten form as molecules are electrically neutral
Some molecules dissolve in water to form ions and thus can conduct electricity
Like dissolves like (polar molecules dissolve in polar solvents and non-polar dissolves in non-polar solvents)
Low melting and boiling points due to weak forces
Substances are soft and easily scratched
Mostly gas or liquid at room temperature

21. Covalent lattices Carbon and Silicon can form covalent lattices.
These are often extremely hard and durable substances such as diamond, graphite and quartz.

22. Covalent lattices
Covalent Network Lattice -Some non-metals form giant structures in which no individual molecules exist. They consist of countless numbers of atoms covalently bonded to each other, forming a 3D lattice. Eg Diamond, Silicon dioxide
Covalent Layer Lattice - Each layer is held together covalently (strong bonds) and the layers are held together by dispersion forces (weak bonds) Eg Graphite

23. Properties of Covalent lattices
Network Lattice:
Large amount energy to break lattice so high boiling and melting points
No free moving electrons so no conductivity
Hard, as lattice holds atoms in fixed positions
Unreactive
Layer Lattice:
Graphite has a single free electron so does conduct electricity
Forces between layers weak so layers slide over each other, graphite appears soft.

25. Your Task
“online testing” link “students – direct access: enter here” Organisation = rochestersc Password = student “chemistry” “Bonding”