Organic Chemistry Flashcards
heated inorganic compound
ammonium cyanate produced urea
Wöhler synthesis
AKA Carbamide
Urea
German chemist, disproved the
“Vitalism” and isolate urea
Friedrich Wohler
Urea was isolated from an inorganic compound ______
ammonium cyanate
states that electrons fill lower-energy atomic orbitals before
filling higher-energy ones
AUFBAU PRINCIPLE
maximum of 2 electrons can occupy the same orbital only if
they have opposite spins
PAULI’S EXCLUSION PRINCIPLE
atoms of the same element with different
numbers of neutrons and thus different mass
number (A).
ISOTOPES
region of space where there is a
certain probability of finding an
electron
ORBITALS
- Also known as WAVE FUNCTION
ORBITALS
for degenerate orbitals, electrons fill the orbitals singly
before they pair up
HUND’S RULE
No 2 electrons can have the same set of 4 quantum numbers
HEISENBERG’S UNCCERTAINTY PRINCIPLE
- symbolic notation of the manner in which the electrons of its atoms are distributed over different
atomic orbitals
Electron Configuration
The tendency among atoms of group 1A-7A
elements to react in ways that achieve an outer shell of
eight valence electrons.
Octet Rule
– an atom or group of atoms bearing a negative
charge.
Anion
an atom or group of atoms bearing a positive charge.
Cation
-Electron dot structure
-Valence shell electrons of an atom are represented as dot
LEWIS STRUCTURE
-Line bond structure
-Each shared electron is represented by line
between the atom
symbols
KEKULE STRUCTURE
Associated with any atom that does not exhibit the appropriate number of valence electrons.
Formal Charge
Measure of the ability of an atom to attract electrons
ELECTRONEGATIVITY
withdrawal of electrons towards a highly
electronegative atom which causes the formation of
partial charges
INDUCTION
is a complex interaction that
includes dipole-dipole, as well as orbital interactions
and the transfer of electron density between
molecules.
Hydrogen bonding
These are the strongest of the IMFs and range from 5 –
25 kJ/mol
Hydrogen bonding
forces arise from the attraction of
oppositely charged atoms (other than H) in
molecules.
Dipole-dipole
- These are generally weaker than H-bonding, ranging
from about 5-10 kJ/mol.
Dipole-Dipole
forces arise
from the movement of electrons within a molecule. This natural motion can produce an uneven
distribution of the electrons (polarization of the distribution) resulting in a temporary dipole
moment in the molecule. This will induce the
movement of electrons in adjacent molecules
Van der Waals or (London) dispersion
forces are very brief and weak, only 2-5 kJ/mol.
Van der Waals or (London) dispersion forces
A _______ reaction involves the displacement of one
atom or group in a molecule by another atom or group.
SUBSTITUTION
