Organic Chemistry Notes

Organic Chemistry

studies the structure, properties, preparation, and reactions of organic compounds

Chemical Compounds

contain one or more carbon atoms bonded together to other \n elements such as hydrogen, oxygen, nitrogen, or halogens. Examples of organic compounds, \n are methane (CH4), ethanol (C2H5OH), and glucose (C6H12O6)

To classify compounds into organic or inorganic, follow these steps:

1\.Check the Molecular Formula , does it contain carbon?


2. Yes-Organic No=Inorganic

Examples: H20=NO

C2H6=YES

HCL=NO (Chlorine)

C2H4O2 (YES)

Chemical Bond

A chemical bond is the force of attraction that holds atoms together and helps them to stay intact

Why do elements make bonds?

They want to get more saturated/more stable

Covalent Bonds

\-Formed when non-metals bond together. -Elements share one or more pairs of electrons. Examples: H2O, CH4 , CO2 , C2H4

Ionic Bonds

\-Formed between metals and non-metals.

• Metal loses electrons to form a cation.

• Non-metal gains electrons to form an anion. Examples: NaCl, CaH2 , TiCl4 , Fe2O3 .

(common all have metals)

To classify compounds into ionic or covalent, follow these steps:

1. Check the chemical formula
2. Does it contain a metal?
3. YES=IONIC
4. NO=COVALENT

Examples: LiO =YES, IONIC

C2H2= NO,COVALENT

SO2= NO, COVALENT

Ca3N2=YES, IONIC

In organic compounds, the most common elements

are carbon, hydrogen, oxygen, nitrogen, sulfur and halogens “mostly non-metals”, so covalent bonds dominate in organic compounds.

Types of Covalent Bonds

Elements that are bonded together by covalent bonds can:

• Share one electron pair → single bond

• Two electron pairs → double

• Three electron pairs → triple bond

The bond length and strength depend on the number of shared electrons (similar elements)

• As the number of shared electrons increases.

• Attraction between the bonded elements increases.

• Bond strength increases & bond length

Longest to Shortest (Bond Length)

Single>Double>Triple

Weakest to Strongest (Bond Strength)

Single > Double > Triple