2.2.1 Electron Structure Flashcards
what is the order of the subshell
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s
what does sub shell s look like
its just one sphere
what does sub shell p look like
3 dumbell shapes
What property of electrons is represented by the direction of the arrows in the bus diagram
Opposite spins
how many electrons are there in each shell
1- 2
2 - 8
3 - 18
4 - 32
5 - 50
how many electrons can each type of sub shell hold
s 2
p 6
d 10
f 14
which block does … belong to
group 1 or 2 = s block
transition metals = d block
group 3 - 8 = p block
Electron configuration of ions
O = [He] 2s2 2p4 What is O2-
[He] 2s2 2p6
Electron configuration exceptions Cu29 Cr24
Cr24 - [Ar] 4s1 3d5
Cu25 - [Ar] 4s1 3d10
As the distance of each Electron from the nucleus decreases, nuclear attraction
Increases. so more energy is needed to remove each successive electron
the more electrons - smaller or bigger
The bigger the substance so negative ions are bigger
Why does 4S fill before 3D
4S has a lower energy than 3D
How many electrons in total occupy the P subshells inGr32
6+6+2 = 14
What is an orbital?
A region around the nucleus that can hold up to 2 electrons with opposite spins
eg p has 3 orbitals
What are subshells?
group of Orbitals of the same type
eg p subshell
What are the number of unpaired electrons in a sulphur16 atom?
Has six in outer shell uses two to pair in s subshell and 2 in p subshell so has 2 left
What are the number of full shells in a krypton 36 atom?
Three
Why do isotopes have the same chemical properties?
They have the same number of electrons in the outer shell so they have the same overall configuration of electrons which determine how they react the same
Describe the relative energy of the 2S orbital and two of the 2P orbitals
S orbital has a lower energy level then P
Both P orbitals have equal energy
