Atoms and electrons Flashcards
how many electrons can each energy level hold
1= 2
2= 8
3= 18
4= 32
what is the formula to calculate the maximum number of electrons each energy level can hold
2n^2
what is atomic orbital
an atomic orbital is a region around the nuclues that can hold up to two electrons with opposite spins
what are the types of spins
up spin
down spin
what is an electron
it is a cloud of negative charge and it hhas the shape of the orbital occupied by the electron
what are the types of atomic orbital
s
p
d
f
list the features of the s orbital
s= has a spherical shape
every electron shell has a s orbital
1 in each energy level
list the features of the p orbitals
p= every electron shell apart from the 1st one has a p orbital
shaped like a dumb bell
they are 3 in each energy level
what are te features of the d orbitals
d= 5 in each shell
in every shell except the first and second one
what are the fetures of the f orbitals
f= 7 in the 4th shell
only in the 4th shell
what are sublevels
all of the orbitals of the same type in the same shell
explain and visualise electron configuration (use nitrogen with 7 electrons ) as an example
for example nitrogen has 7 electrons therefore starting from the smallest (1s) we place 2 electrons in opposite spins
then we place 2 electrons again in opposite spins on 2s and lastly 1 electron each on 3 boxes of 2p
what are the rules for filling atomic orbitals
orbitals with the lowest energy are filled first
we can have up to 2 electrons in the same orbital but they must have opposite spin
if we have orbitals with the same energy then we put electrons into individual orbitals before we pair them
why do we put electrons in the same energy in individual orbitals
because the electrons will repel
what is special about the 4s sublevel
teh energy is less than the 3d sublevel therefore we fill that first before he 3d sublevel
what happens in an actual configuration
the 3d sublevel always has 2 electrons because it makes it more stable
explain the process of electron configuration in the d block
in the d block if it requires ions u remove or add electron starting from 4s not 3d
explain electron configuration in ions
add or minus from the level with the highest energy
explain the shorthand electron configuration
start with putting the configuration of the element down then take the configuration of the previous element and remove it from the current one leaving what is left
what is the first ionisation energy
this is needed to remove one mole of electrons from one mole of atoms in their gaseous state to form one mole of 1+ ions also in their gaseous state
what is second ionisation energy
this is the energy needed to remove one mole of electrons from one mole of 1+ ions in their gaseous state to form one mole of 2+ ions in their gaseous state
what is successive ionisation energies
this is the process of continually removing electrons and measuring the ionisation energy each time
