Tetravalence Of Carbon: Shapes Of Organic Compounds
Chapter Name : Organic Chemistry - Some Basic Principles And Techniques |
Sub Topic Code : 102_11_12_02_02 |
Topic Name : Tetravalence Of Carbon: Shapes Of Organic Compounds |
|
Sub Topic Name : Some Characteristic Features Of ∏ Bonds |
|
Introduction
Organic chemistry is a chemistry sub discipline involving the scientific study of the structure, properties, and reactions of organic compounds and organic materials, i.e., matter in its various forms that contain carbon atoms.
Pre-Requisites:
Organic chemistry
Activity:
Aromatic compounds.
Real Life Question:
What is organic chemistry?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| Organic compound | An organic compound is any member of a large class of gaseous, liquid, or solid chemical compounds whose molecules contain carbon. |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|---|
| Alcohols | Alcohols (R-OH) take the suffix "-ol" with an infix numerical bonding position: CH3CH2CH2OH is propan-1-ol. The suffixes -diol, -triol, -tetraol, etc., are used for multiple -OH groups: Ethylene glycol CH2OHCH2OH is ethane-1, 2-diol. |
Real life uses :
Study the nature of chemicals.
Places to visit :
Chemistry laboratory.
Practical examples around us
| Examples | Explainations |
|---|---|
| ketones | In general ketones (R-CO-R) take the suffix "-one" with an infix position number: CH3CH2CH2COCH3 is pentan-2-one. If a higher precedence suffix is in use, the prefix "oxo-" is used: CH3CH2CH2COCH2CHO is 3-oxohexanal. |
What you learn in Theory:
Pi bonds (? bonds) are covalent chemical bonds where two lobes of one involved atomic orbital overlap two lobes of the other involved atomic orbital. These orbitals share a nodal plane which passes through both of the involved nuclei.
What you learn in Practice:
Pi bonds are usually weaker than sigma bonds; the C-C double bond has bond energy less than twice the C-C single bond energy; which leads to the conclusion that the p orbital overlap to form molecular orbitals is a weaker bond than when s orbitals overlap to form molecular orbitals.