BSES 26 Flashcards
they represent the probability of finding an electron in any one place. they correspond to the different energies. so an electron in an orbital has definite energy. orbitals are best described with quantum mechanics
orbitals
the region in space just outside the nucleus of the atom where the probability of finding the electrons is at the highest (95%)
atomic orbitals
formed as a result from the overlap of two atomic orbitals, wherein a pair of electrons occupying.
molecular orbitals
a measure of the probability of finding an electron in an orbital.
electron density
mathematical description of the volume of space occupied by an electron having a certain amount of energy
wave function
is the place where a crest and a trough of energy
a node in an orbital
is based on the wave properties of matter. quantization of energy is the consequence of these properties
quantum mechanics
the energy levels about the nucleus contain group
atomic orbitals
atomic orbitals are designates as
s, p, d, and f
what are the three p orbitals of equal energy
px, py, and pz
the number describes the energy level that the electron occupies. it can have a value of 1-7. this defines the “level” of the electron
principal quantum number
this number describes the shape of the orbital that the electron is found in. it can have a value from 0-3. this defines the “sublevel” of the electron. also, the numbers can be replaced by letters according to the following:
0 = S
1 = P
2 = D
3 = F
orbital (azimuthal) quantum number
this number describes the orientation of the electron in the orbitals. this defines the “orbital” of the electron. there are 2L+1 orbitals in each sublevel.
magnetic quantum number
this number describes the direction of spin of the electron in the orbital
spin quantum number
are spherical regions where the probability of finding an electron is zero
radial nodes
it states that no two electrons may have the same set of quantum numbers
pauli exclusion and the build up principles
result from the combination of atomic orbitals
molecular orbitals
is an indicator of the bond strength and length. a bond order of 1 is equivalent to a single bond. fractional bond orders are possible
bond order
hybridization is a major players in this approach to bonding
valence bond theory
there are two ways orbitals can overlap to form bonds between atoms
valence bond theory
head-to-head overlap
sigma bonds
cylindrical symmetry of an electron density about the internuclear axis
sigma bonds
side-to-side overlap
pi bonds
electron density above and below the internuclear axis
pi bonds
defined as the concept of mixing two atomic orbitals to give rise to a new type of hybridized orbitals. this intermixing usually results in the formation of hybrid orbitals having entirely different energy, shapes, etc.
hybridization
an extension of the valence bond theory, and it helps us to understand the formation of bonds, bond energies, and bond lengths
hybridization
redistribution of the energy of the energy of orbitals of individual atoms to give orbitals of equivalent energy happens when two atomic orbitals combine to form a hybrid orbital in a molecule.
hybridization
observed when one s and one p orbital in the same main shell of an atom mix to form two new equivalent orbitals
sp hybridization
observed when one s and two p orbitals of the same shell of an atom mix to form 3 equivalent orbitals
sp2 hybridization
when one s orbital and 3 p orbitals belonging to the same shell of an atom mix together to form four new equivalent orbitals
sp3 hybridization
involves the mixing of 1s orbitals, 3p orbitals, and 1d orbital to form 5
sp3d hybridization
arrangement of sp
linear
arrangement of sp2
triangular planar
arrangement of sp3
tetrahedron
arrangement of sp3d
triangular bipyramid
sp measurement
180 degrees
sp2 measurement
120 degrees
sp3 measurement
109.5 degrees
sp3d measurement
90 and 120 degrees
