Ch4 Chem Concepts Flashcards
Ionization energy
The energy necessary to remove an electron from a gas-phase atom or ion.
Ionization energy increases across a period. Ionization energy increases up a group.
Electron affinity
The energy change that occurs when an electron is added to a gas-phase atom.
Halogens have large, negative electron affinities.
Noble gases have positive electron affinities.
Alkaline earth metals have electron affinities that are approximately equal to zero.
Lattice energy strength
bigger charges lead to larger lattice energies.
bigger ions lead to smaller lattice energies.
Electronegativity
the extent to which an atom attracts shared electrons.
Bond polarity
the degree to which bonding electrons are transferred.
Relative Importance of Resonance structures
- each atom should satisfy the octet rule.
- Like charges on adjacent atoms are unfavorable.
- Smaller formal charges, either positive or negative, are preferable.
- A more negative formal charge should reside on a more electronegative atom.
Removing electrons from metals w/ variable charge
Remove from highest p subshell for first charge, then remove from s subshell for 2nd charge.
Diamagnetic materials
are slightly repelled by a magnet.
All of the electrons in diamagnetic materials are paired.
Paramagnetic materials
are attracted by a magnet.
Paramagnetic materials contain at least one unpaired electron.
VB Theory
Atom centered, better with localized electrons, easy to visualize; good at justifying molecular shapes.
MO Theory
Molecule centered, better with delocalized electrons, better at explaining energies, bond orders, and magnetic properties.