Study Set Content:
Listing of Orbitals occupied by an atom’s electron
Ground-state electron configuration
· Lowest-energy orbitals fill first, in the order of 1S, 2S,
3S, 3p...
Aufbau principle
· Only two electrons can occupy an orbital and they must be of opposite spin
Pauli exclusion principle
· If two or more empty orbitals of equal energy are available, electrons occupy each with parallel spins until all orbitals have one electron.
Hund's rule
Indicates type and ratio of atoms in a compound.
– For example: CH2 , May represent either C2H4 or c4H8
Empirical formula
– Indicated actual number of atoms in a compound.
– Example: CH4, C2H4, C6H6
Molecular Formula
Indicated the actual number of atoms and how they are
bonded each other. The most comprehensive formula.
Structural formula
· This theory explains how atoms are connected
together in an organic compound. It was developed by
independent studies of Butlerov, Kekule and Couper
between 1857-1861.
Structural theory Organic Compounds
ll atoms form a certain number of bonds. It can be
explained by
valency concept
Carbon
Tetravalent
Hydrogen
Monovalent
Two compounds may have same molecular formula
but different
structural formula
· Idea that acids are solutions containing a lot of “H+” and bases are solutions containing a lot of “OH” is not very useful in organic chemistry.
Acid and Base (Bronsted-Lowry Definition)
· Substance that donate a hydrogen ion, H+
Bronsted-Lowry Acid
· Substance that accepts a hydrogen ion, H+
Bronsted-Lowry Base
Products that results forms deprotonation of a Bronsted=Lowry Acid
Conjugate base
· Products that results forms protonation of a Bronsted-Lowry Base
Conjugate acid
For the reaction of an acid (HA) with water to form
hydronium ion.
Ka
is a measure related to the strength
of the acid.
Conjugate-base
indicate concentration in moles per liter.
Brackets
