Chapter 1 Atomic Structures Flashcards
(20 cards)
Organic Chemistry
The study of carbon compounds
Isotope
Atoms of the same element that have different mass numbers
Shell
A group of an atom’s electrons with the same principal quantum number
Node
A surface of zero electron density within an orbital
Ground state electron configuration
The most stable, lowest energy electron configuration of a molecule or an atom
Valence Shell
The outermost electron shell of an atom
Covalent Bond
A bond formed by sharing electrons between atoms
Forms molecules
Lewis structures or electron dot structures
A representation of a molecule showing valence electrons as dots
Lone pair or nonbonding electrons
Nonbonding valence shell electron pairs
Valence Bond Theory
A bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Sigma Bond
A covalent bond formed by head-on overlap of atomic orbitals
Bond strength
An alternative name for bond dissociation energy
Bond length
The equilibrium distance between the two nuclei of two atoms that are bonded to each other
sp3 hybrid orbitals
Hybrid orbitals formed from combination of an s orbital with three p atomic orbitals
Directed towards the corners of a tetrahedron with an angle of 109.5 degrees to each other
Bond angle
The angle formed between two adjacent bonds
sp2 hybrid orbitals
A hybrid orbital derived by the combination of an s orbital with two p orbitals.
The three sp2 orbitals are in a plane at angles of 120 degrees from each other
sp hybrid orbitals
Hybrid orbitals formed when an s orbital hybridizes with only on p orbital.
sp orbitals are at 180 degrees from each other
Molecular Orbital Theory
A description of covalent bond formation resulting from the combination of atomic orbitals to form molecular orbitals
Bonding MO
A molecular orbital that is lower in energy that the atomic orbitals from which it is formed
Antibonding MO
A molecular orbital that is higher in energy than the atomic orbitals from which it is formed
