Topic 1- Lecture 3 Flashcards
Every electron under one of these labels (1s,2p,3d…) in a given atom is at the same quantized…
Energy level
Electrons are added to…
The lowest energy orbital available
1s2, 2s1 (lithium) is an example of…
Electron configuration
Place one unpaired electron in each degenerate orbital
Orbital Diagram
Unpaired electrons cause a magnetic moment
-lone atoms with one or more unpaired electrons are attracted by magnetic fields
Paramagnetic Atom
Lone atoms with no unpaired electrons are not attracted by magnetic fields
Diamagnetic Atom
Zeff= Z-σ
Ζeff= charge experienced by electron Z= actual nuclear charge (atomic #) σ= shielding constant
Large to small from left to right on periodic table
Atomic Radius
- new shells added with larger orbitals
- valence electrons have more energy, are less stable, and are farther from nucleus
- valence electrons experience greater shielding
- force of attraction decreases as distance from nucleus increases (Coulomb’s law)
Atomic Radius
Lose electrons
- Creates positive atoms
- Creates smaller ionic radius
Cations
Gain electrons
- creates negative atoms
- creates larger ionic radius
Anions
Energy must always be added to remove an electron
Endothermic Processes
Increases from left to right on periodic table
- increases as atomic radii decrease
- some exceptions apply
First Ionization Energy
An elements ability to attract electrons in a chemical bond
Electronegativity
Increases left to right across periodic table
-increases as atomic radius decreases
Electronegativity
