Exam 2 Lecture 8 Flashcards
Hydrogen atom orbitral energiesdon’t have any
crossover or splitting
Multi-electron atoms have…
crossover and splitting
…..are lower in multielectron atom
Principle energies
•Energies of subshells are____ in multielectron atoms
“split”
Some _______in multielectron atoms results in certain subshells having_________
crossover of energy levels
lower energies than subshells with lower “n” values
What is responsible fo rthe differences in energies for the single- and multielectron atoms?
ELECTROSTATIC INTERACTIONS
ms describes electron …..
spin
The Pauli exclusion principle:
No two electrons in an atom can have the same set of four quantum numbers four quantum numbers
What’s the 1st orbital to experience crossover?
What’s the 2nd orbital to experience crossover?
What’s the 3rd orbital to experience crossover?
What does this represent?
direction of electron spin
Populate Lithium orbitals
Populate Berillium orbitals
Populate Boron orbitals
Hund s’ rule
For degenerate orbitals the lowest energy is attained when the number of electrons with the same spin is maximized
complete the sentence, name the rule…
For _____the lowest energy is attained when ________
degenerate orbitals,
the number of electrons with the same spin is maximized
HUND’s RULE
Populate the Carbon atom
12
Populate the Nitrogen atom
Write the electron configuration for Oxygen
Where is the s block?
Where is the p block?
Where is the d block?
transition metals
Where is the f block?
Lanthanides and Actinides
Auf-Bau Principle:
Lower electron orbitals fill before higher orbitals do, “building up” the electron shell. The end result is that the atom, ion, or molecule forms the most stable electron configuration.
(The periodic table color coded by principle quantum number of the orbital being filled)
Auf-Bau Principle periodic table
Auf-Bau Rule
