electron configuration

Question 1

orbitals

Answer 1

a region around the nucleus that can only hold two electrons with opposite spins

Question 2

what are the sub levels

Answer 2

1st- s sublevel
2nd- s+p sublevel
3rd- s+p+d sublevel
4th- s+p+d+f

Question 3

how many orbitals and electrons can each sublevel hold

Answer 3

s= 1 orbital, 2 electrons
p= 3 orbitals, 6 electrons
d= 5 orbitals, 10 electrons
f= 7 orbitals, 14 electrons

Question 4

why do the outer shell electrons have more energy?

Answer 4

-because they are further away from the nucleus, therefore meaning the nucleus charge is weaker. So, the outer shell electrons would require more energy to stay in there shells.
-they experience repulsion from the inner electrons, adding to the energy needed to stay in the shells

Question 5

how to find the number of electrons in a shell

Answer 5

2n^2

Question 6

what are the exceptions in electron configuration

Answer 6

transition metals such as chromium and copper will include the 3d sub shell. if the element doesn’t have enough electrons to fill in the 3d sub shell. the 4s electrons will move to the 3d sub shell, as its more stable than having empty orbitals

Question 7

why do electrons tend to prefer being unpaired in orbitals

Answer 7

because they are electrons and tend to repel each other

Question 8

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

Answer 8

the 4s orbital is lower in energy

Question 9

what happens during the ionisation of transition metals

Answer 9

the 3d will initially have more energy than the 4s so it will act as a shield, protecting the 4s, and it will lose energy. So, the 4s will have more energy. So, during ionization they will get lost first