Unit 3 - Multielectron & Periodic Table Flashcards
What are the features of orbital enegry in multielectron atoms ?
- as z increases, enegry of 1s and orbital size decrease
- n values are** not degenerate **
- as l value increases in a shell, energy increases
What is the Pauli Exclusion Principle?
Electrons cannot have the same set of quantaum numbers, 2 electrons per orbital
How many orbitals does each subshell have?
- ns = 1
- np = 3
- nd = 5
- nf = 7
What is the Aufbau Procedure?
What are the exceptions?
- Orbitals are filled in a certain order (n + l)
- cronium and copper
What is Hund’s Rule?
- each orbital gets one electron (with parallel spins) before any get two
What trends in the periodic table relate to orbital filling?
- periods indicate value of n
- group number indicates number of valence electrons
- certain blocks correspond with subshell of last electron
Which groups are located in each block?
- s-block: 1-2 + hydrogen
- d-block: 3-12
- p-block: 13-18
- f-block: the bottom part
What happens to the n value when crossing blocks?
- crossing s-block to d-block: n -1
- crossing d-block to p-block: n + 1 (back to original)
What is the ground state electron configuration of Cr (cronium)?
[Ar] 4s^1 3d^5
What is the ground state electron configuration of Cu (copper)?
[Ar] 4s^1 3d^10
How are electrons removed when writing electron configurations of cations?
- Remove electrons with highest n-value
- Remove electrons with highest l-value
Define diagmagnetic.
All electrons are paired
Define paramagnetic.
atom has unpaired electrons and a magnetic moment
Describe periodic table trends for atomic radius.
- increases: going down a group
- decreases: going down a period
What is ionization energy?
enegry required to remove an electron
