PRELIM 01 - Introduction to Organic Chemistry & Structure and Bonding Flashcards
Is the chemistry of the compounds present in living organisms
Organic chemistry
The ability of atoms in forming stable bonds with itself
Catenation
Is defined as an atom or a group of atoms that effectively determines the chemical properties of an organic compound
Functional group
Is a series of compounds that have the same funcitonal group
Homologous series
Is the idea of an electron “orbiting” the nucleus like planets orbiting the sun
Orbit
Are electron clouds that represent the shape of probability for an electron’s location
Orbital
Tells about the detailed location of electrons in an atom and the specific electron orbitals that the electrons are found
Electron configuration
He is credited as the father of modern atomic theory
John Dalton
Proposed the planetary model of the atom
Niels Bohr
Principle that states that there is an inherent uncertainty in the act of measuring a variable of a particle
Heisenberg uncertainty principle
Atoms of the same element with different number of neutrons
Isotopes
Is weighted average mass in atomic mass units of an element’s naturally occuring isotopes
Atomic mass/Atomic weight
4 quantum numbers
Principal, Angular momentum, Magnetic, Spin
Orbital size and energy level (n)
Principal
Orbital shape (l)
Angular momentum
Orbital orientation (ml)
Magnetic
Electron spin direction (ms)
Spin
4 different kinds of orbitals for electrons
s, p, d, f
Spherical; nucleus at the center
s orbitals
Dumbbell-shaped; nucleus at middle
p orbitals
Elongated dumbbell-shaped; nucleus at center
d orbitals
Tetrahedral; nucleus at center
f orbitals
Lobes of a p orbital are separated by region of zero electron density, which is called a __________
Node
Lowest energy arrangement of an atom
Ground-state electron configuration
Principle that states that lowest energy orbitals must be filled first
Aufbau ‘build-up’ principle
Principle that states that only two electrons can occupy an orbital, and they must be of opposite spin
Pauli exclusion principle
Principle that states that if two or more empty orbitals of equal energy are available, electrons occupy each with spins parallel until all orbitals have one electron
Hund’s rule
Shows the valence electrons of atoms as dots
Lewis structures
Have a line drawn between two atoms indicating a covalent bond
Kekule structures
Valence electrons that are not used in bonding
Nonbonding electrons/Lone-pair electrons
Forms when two atoms approach each other closely so that a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom
Covalent bond
2 models to describe covalent bonding
Valence bond theory, Molecular orbital theory
Theory that states that electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms
Valence bond theory
Is where electrons are most likely to be found in a molecule
Molecular orbital
Theory that states that bonds results from combination of atomic orbitals to give molecular orbitals
Molecular orbital (MO) theory
Circular cross-section and are formed by head-on interaction
Sigma (σ) bond
“Dumbbell” shape from sideways interaction of p orbitals
Pi (π) bond
