Organic Chemistry: Functional Groups

Functional groups is a specific group that gives the molecule ability to react in a specific manner. And are usually in organic compound other than Carbon and Hydrogen, such as Nitrogen, Chlorine, Florine.

•Halides & Nitro Compounds

Naming rule is just attached to the Alkane and Alkene, but we have to follow the new prefixes:

F = Fluro

Br= Bromo

Cl = Chloro

NO3 = Nitro

Notes: 

We use prefixes such as di-, tri-, tetra-.... to indicate that if there is one more Compounds.

Alcohols:

1: It contains OH- and we have to name it as the lowest number as possible (start counting it from the closest way)

2: End in  - ol

3: If there is more than one OH- in it, we use prefixes such as di-, tri- to indicate it.

Aldehydes and Ketones :

The difference between aldehydes and ketones is that

1: Aldehydes contains double bond Oxygen at the end of its chain

2: Ketones contains double bond Oxygen at the MIDDLE of its chain

Aldehydes:

1: End in "-al"

 "Ketones"

1: End in "-one"

Organic Chemistry.

Organic chemistry is responsible for many everyday products of the everyday products that are used around the world, as it's composed of only organic matters like Oxygen, Hydrogen... that's naturally come from the nature in order to decrease the pollution from chemical product.

•Properties

•Low melting points

•Weak or No-electrolytes

Types of Carbon Atom Chains:

A straight-line

Circular Pattern.

Branch Pattern.

Single Bond:

Alkanes are saturated hydrocarbon which have all carbon atoms bonded by single bonds.

To name them, we have to end in "-ane" as they are Alkanes.

1: Count how many carbon is there in the LONGEST CHAIN, (usually from left to right)

2: According to the numbers of carbon, we can record the name as a symbol " Methane, Ethane...."

3: Then, use the general formula to show the Alkane.

Double Bond (Alkene):

Generally it's the same as Alkane in the naming way, but now it's Double Bond

1: End in "-ene" instead

2: Be aware the double bonding location and name it specificly according to the information has provided!

3: Draw a double line to show it's a double bond~

Triple Bond (Alkyne):

Same method of naming to Alkene, but

1: End in "-yne" instead.

2: Draw a triple line to show it's a triple bond~

Chemical Bonding

There are three types of chemical bonding:
1) Ionic bonding- the transfer between 2 atoms to form a positive ion and negative ion.
2) Non-polar covalent bonding- equal sharing of electrons
3) Polar covalent bonding- unequal sharing of electrons


The first two bondings we have already learned from previous classes, so lets started with the new bonding - Polar covalent bonding


First, we have to know the electronegativity. The difference in electronegativity will determine the electron sharing. To determine the difference, there's a formula we have to notice!: 

ENeg Diff. = lENeg1 - ENeg 2l

If ENeg Diff <0.5 it's a non polar covalent bond

If ENeg Diff > 0.5 and <1.8 it's a polar covalent bond

If ENeg Diff > 1.8 it's an ionic bond

Atoms with Higher Electronegativity
will form a PARTIAL NEGATIVE charge

•δ- (between 0 and -1)

Atoms with Lower 

Electronegativity
will form a PARTIAL
POSITIVE charge

•δ+(between 0 and +1)

INTRAmolecular forces are found within a molecule, responsible for holding the atoms of a molecule together

INTERmolecular forces are found between the molecules, responsible for the bonding between molecules

Polarity - 

 Describes a molecule's electrical balance.

According to the electronegativity from each element. By subtracting two atoms in the compound. The number as a result will tell us that what kind of bonding it is. 

For example: 

 

H2O:

H: 2.20
O:3.44


3.44-2.20= 1.24

Which mean H20 is a polar covalent bond according to the electronegativity.

Drawing Electron Dot and Lewis Diagrams

When Drawing Electron Dot and Lewis Diagrams, keep that in mind that 
-the nucleus represents the symbol
-The dot represents the electrons
-There are four orbitals in each side, each orbital can only hold 2 maximum electrons
-Each shell can only hold 8 electrons

 Electron dot diagrams help us to understand and represent the process of ion formation, and also illustrate that ionic bonds tend to produce full outer orbits of electron


Covalent Bonds:

Lets use water as an example, covalent bonds are composed by 2 non-metal atom as we've learned from previous classes. When we are doing it, remember:

- Fill each orbital into full shell
- Use line instead to replace the dot to represent the orbital is full
- Use the symbol to represent the nucleus.


Lets move on in to Ion bond.

Basically it's the same format, but please remember both elements are not SHARING electrons. So we use "+" to represents that they are joined together still, but not covalent bonds.