Bonding Flashcards
each type has a specific shape, which describes the probability of finding an electron in a given region of space
atomic orbitals
spherical and symmetrical orbital , centered around nucleus
s-orbital
orbital composed of two lobes located symmetrically around nucleus and contains a node at the nucleus, like a dumbbell; x, y, or z axis
p-orbital
area where the probability of finding an electron is zero
node
orbital with four symmetrical lobes and two nodes
d-orbital
formed when two atomic orbitals combine
molecular orbitals
produced when sign of wave functions is the same, lower energy, more stable
bonding orbitals
produced when signs of wave functions are different, higher energy, less stable
antibonding orbitals
molecular orbital formed by head-to-head or tail-to-tail overlap; includes all single bonds (accommodating two electrons)
sigma (σ) bond
molecular orbital formed when two p-orbitals line up in parallel and their electron clouds overlap
pi (π) bond
individual pi bonds are _____ than sigma bonds
weaker
one π bond on top of an existing σ bond
double bond
a σ bond and two π bonds
triple bond
formed by mixing different types of orbitals
hybrid orbitals
atom with all single bonds; 25% s character, 75% p character
sp^3