electron configuration quiz

Aufbaus Principal

electrons enter orbitals of the lowest energy first

Hunds Rule

orbitals of equal energy all must have 1 electron with parallel spin before the orbital can have a 2nd electron with opposite spin

paulis exclusion principal

no two electrons can be in the same orbital without opposite spin

orbitals=

shapes

orbital type S # of shapes and maximum number of electrons

1, 2

orbital type P # of shapes and maximum number of electrons

3,6

orbital type D # of shapes and maximum number of electrons

5,10

orbital type F # of shapes and maximum number of electrons

7,14

each orbital can hold a maximum of

2 electrons

why does the 4s orbital fill before the 3d orbital

the 4s orbital has less energy than the 3d orbital

1s² what do they all stand for

1- energy level

s-orbital shape

² - number of electrons

1s² 11 why’s that incorrect

i violated paulis exclusion principle which says no two electrons can be in the same orbital without opposite spin

1| _ _ whys this incorrect

it violates hunds rule because it says orbitals of equal energy all must have 1 electron with parallel spin before the orbital can have a 2nd electron with opposite spin