Module 1: Introduction Flashcards
What century was organic chemistry?
18th Century
What was the assumption for organic chemistry?
It was assumed that compounds was only found in living organisms and cannot be sythesized in laboratories.
What was this concept called?
The Vital Force Theory
Who proposed this concept?
Jon Jacob Berzelius
When and who proved it incorrect?
In 1828 by Friedrich Wohler
What was the aqueous solution of two inorganic compounds?
Ammonium Chloride and Silver Cyanate= Urea-Compound of Urine
What is the study of hydrocarbons and their derivatives?
Organic Chemistry
What are the common additional elements found in hydrocarbon derivatives?
F P O N S Cl Br
What discipline is organic chemistry normally used?
Pharmaceuticals
Biochemistry
Material Science
Metallurgy
It is known for a seemingly unlimited number of compounds
Carbon
Chemical compounds are divided into two
Organic and Inorganic Compounds
What are examples of Organic Compounds?
DNA
Gasoline
Sugar
Alcohol
What are examples of Inorganic Compounds?
Salt
Quartz
Hydrochloric Acid
Water
What is stronger? Ionic or Covalent?
Ionic
Give some characteristics of organic compounds
Low melting point
Low Boiling Point
Low solubility in water
high solubility in non-polar solvents
flammable
aqueous solution does not conduct electricity
exhibit covalent bonding
Give some characteristics of inorganic compounds
High melting point
High Boiling Point
High solubility in water
Low solubility in non-polar solvents
non-flammable
aqueous solution conducts electricity
exhibit ionic bonding
Organic Compounds compromise how many percent?
90
What is catenation?
Self Linking of Ion
What is the tetravalency of carbon?
It needs 4 bonds
What is isomerism?
Same chemical formula but different chemical structures.
What are the kinds of isomerism?
Structural Isomerism
Stereoisomerism
What configuration is the opposite side?
E
What configuration is on the same side?
Z
Three types of bonds
Purely Covalent or Non Polar
Polar Covalent
Ionic
The bonding electrons are shared equally between two bonding atoms.
Purely Covalent or Non Polar
The electrons are shared between atoms, but unequally, with the electrons spending more time around the morte electronegative form.
Polar Covalent
The electrons are not shared.
Ionic
Is a measure of the tendency of an atom to attract electrons.
Electronegativity
How would you know which has a greater electronegativity value?
From bottom to top
What is the highest electronegativity value element?
Fluorine 4.0
0-0.4
Nonpolar Covalent
0.5-1.4
Polar Covalent
1.5-2.0 (NM + NM)
Polar Covalent
1.5-2.0 (NM + M)
Ionic
2.0+
Ionic
Which is stronger? Intermolecular or Intramolecular?
Intramolecular (connection between two elements)
Strongest to weakest intermolecular forces
Ionic Interactions
Hydrogen Bonding
Dipole-dipole Interactions
Dispersion Forces
Are interactions between charged atoms and molecules
Ionic Forces
Occurs in molecules containing the highly electronegative elements F, O, N directly bound to hydrogen
Hydrogen Bonding
Other groups besides hydrogen can be involved in polar covalent bonding with F O N.
Dipole-Dipole Interaction
Weakest Intermolecular forces
London forces
Ion-Ion Forces
Ionic Bond
Ion-Dipole Forces
Ionic and Polar
Hydrogen Bonding Forces
H + FON
Dipole-dipole Forces
Polar and not H
London Dispersion Forces
Non-Polar
Most common models used in representing molecules in organic chemistry?
Lewis Structure
What is usually the central element?
Thee least electronegativity
Total number of electrons shared in the molecule
S
Total number of valence electrons needed by all the atoms in the molecules to achieve noble gas configuration.
N
Number of electrons available in the valence shells of all atoms.
A
It is the charge assigned to an atom in a molecule
Formal Charge
Also known as mixture of orbitals
Hybridization of the Carbon Atom
The property of carbon that makes it unique is its ability to form bonds with itself
Catenation
What is stronger? Sigma bond or Pi bond?
Sigma Bond
C-H Single Bond, how many no. of sigma and pi bonds?
1 Sigma bond
C-C Double bond, how many no. of sigma and pi bonds?
1 Sigma bond and 1 Pi bond
C-C Triple bond, how many no. of sigma and pi bonds?
1 Sigma bond and 2 Pi bond
What hybridization is 2 steric number?
sp, linear, 180
What hybridization is 3 steric number?
sp2, trigonal planar, 120
What hybridization is 4 steric number?
sp3, tetrahedal, 109.5
Are specific groupings of atoms within molecules that have their own characteristic properties, regardless of the other atoms present in a molecule.
Funcitional Groups
What does R represent in molecular structures?
Rest of the molecule
A compound that contains only carbon atoms and hydrogen atoms.
Hydrocarbon
Hydrocarbons may be divided into two large classes.
Saturated and unsaturated hydrocarbon
Is a hydrocarbon in which all carbon-carbon bonds are single bonds.
Saturated Hydrocarbons
Is a hydrocarbon in which one or more carbon-carbon multiple bonds are present.
Unsaturated Hydrocarbons
Give three examples of saturated hydrocarbons.
Alkanes
Cycloalkanes
Haloalkanes
Give three examples of unsaturated hydrocarbons.
Alkenes
Alkynes
Aromatic
A saturated hydrocarbon in which the carbon atom arrangement is acyclic.
Alkanes
Is a saturated hydrocarbon in which carbon atoms are connected to one another in a cyclic (ring) arrangement.
Cycloalkanes
Also known as alkyl halides, are a group of chemical compounds comprised of an alkane with one or more hydrogens replaced by a halogen atom.
Haloalkanes
Are hydrocarbons that contain one or more double bonds between neighboring carbon atoms.
Alkenes
Are hydrocarbons that contain one or more triple bonds between neighboring carbon atoms.
Alkynes
Is a six-carbon ring with alternative double bonds.
Aromatic Hydrocarbons or Benzene
A functional group that involves an oxygen atom that is bonded to one hydrogen atom and one carbon atom.
Alcohol
A functional group consisting of an oxygen atom that forms single bonds with two carbon atoms.
Ethers
A functional group that contains a sulfur atom bonded to a hydrogen atom.
Thiols
A functional group that consists of a nitrogen atom bonded to some combination of carbons and hydrogens.
Amines
A carbon atom and an oxygen atom are connected by a double bond.
Carbonyl Group
Is a carbonyl in which carbon atoms is bonded to at least one hydrogen atom.
Aldehyde
Involves a carbonyl in which the carbon atom makes single bonds with two r-groups
Ketones
Are another carbonyl-containing functional group, in which the carbon atom is bonded to an OH group on one side and either a carbon or hydrogen atom on the other.
Carboxylic Acids
It contains a carbonyl where the carbon is bonded to one additional oxygen atom and one carbon or hydrogen atom.
Esters
A carbonyl in which the carbon is attached to one nitrogen atom and one carbon or hydrogen atom.
Amides
Sulfur replaces the oxygen and is connected to one atom and one r group.
Thioether
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