Unit 1-Electronic Configurations And The Periodic table Flashcards
What is the Aufbau principle?
Orbitals are filled in order of increasing energy. 1s before 2s
What is the order of orbital filling from 1s to 4d?
1s 2s 2p 3s 3p 4s 3d 4p 4d
What is the Pauli exclusion principle?
This states that an orbital cannot contain more than two electrons and they must have opposite spins.
What is Hund’s rule of maximum multiplicity?
Electrons fill each degenerate orbital singly with spins parallel before pairing occurs.
What are the 2 types of notation used to represent the electron configurations of elements?
Spectroscopic notation and orbital box notation
What is the spectroscopic notation for a lithium atom?
What is the spectroscopic notation for a magnesium 2+ ion?
1s2 2s1
1s2 2s<span>2 </span>2p6
Which element has atoms with [Ar]4s1?
Potassium
How many electrons are there in the 2p sub-shell of the oxygen atom?
4
Which number would complete this spectroscopic notation for a nitrogen atom?
1s2 2s2 2p?
1s2 2s2 2p3
Carbon has two unpaired electrons. How many unpaired electrons would boron have?
1
What is the spectroscopic notation of a lithium ion?
1s2
Which element does this orbital box notation represent?
Hydrogen
Which element does this orbital box notation represent?
Fluorine
How would lithium be represented as orbital box notation?
How would oxygen be represented as orbital box notation?
Which areas represent elements which have s, p, d or f electrons in the outermost sub-shell?
Why is there a slight dip in first ionisation energy from beryllium to boron?
Beryllium is 1s2 2s2 and boron is 1s2 2s2 2p1
Beryllium has a full sub-shell and is more stable. Boron has a single 2p electron and is less stable.
Why is there a dip in first ionisation energy in the middle of the p-block from nitrogen to oxygen?
Nitrogen is 1s2 2s2 2p3 and oxygen is 1s2 2s2 2p4
Half filled sub-shells are relatively stable and it is easier to remove the fourth ‘p’ electron from the 2p shell of oxygen.
