Unit 1 topic B with the goofy orbitals n stuff Flashcards
ja very goofy i don't like this so much
what are orbitals
an area of space around the nucleus where we are likely to find an electron
what quantum number determines the main energy level and size of orbital
the principal quantum number (n)
what quantum number determines the shape of the subshell
angular momentum quantum number (l)
what quantum number determines the orientation of the orbital
the magnetic quantum number (ml)
what quantum number determines the spin of the orbital
spin magnetic number
what are atomic orbitals
the areas with a high probability of finding electrons
what is the maximum electrons that an orbital can hold
2
what is Aufbau’s principle
Electrons fill orbitals in order of increasing energy
What is Pauli’s principle
in an atom no 2 electrons can have the same 4 quantum numbers and an orbital cannot contain more than 2 electrons and they must have opposite spin
what is Hund’s principle
when electrons occupy degenerate orbitals, the electrons fill each one singly with spins parallel before pairing up
define degenerate
same energy
what are the orbitals within each subshell in an isolated atom
degenerate
what is the special stability associated with half filled and full sub-shells
The more stable the electronic configuration, the higher the ionisation energy meaning those with full sub-shells are more stable and have a higher ionisation energy
what can be used to predict the shape of molecules and polyatomic ions
Valence shell electron pair repulsion aka VSEPR
what is spectroscopic notation
it is a type of shorthand used to represent the arrangement of the electrons
define ionisation energy
the energy needed to remove 1 mole of electrons from one mole of gaseous atoms
what are quanta
the fixed amount of energy that electrons have
how are electrons pairs arranged
to minimise repulsion and to maximise seperation
what is the arrangement of electron pairs around a central atom for two electron pairs
linear
what is the arrangement of electron pairs around a central atom for three electron pairs
trigonal planar
what is the arrangement of electron pairs around a central atom for four electron pairs
tetrahedral
what is the arrangement of electron pairs around a central atom for five electron pairs
trigonal bi pyramidal
what is the arrangement of electron pairs around a central atom for six electron pairs
octahedral
which has a greater repulsive effect, bonded pairs or lone pairs
lone pairs
what accounts for the slight deviations from expected bond angles
the different strength of electron pair repulsion
