quangtum chem Flashcards
(22 cards)
electron configuration
the way in which electrons are distributed among the various orbitals
ionization energy
energy required to remove an electron and form an ion. how tightly an electron is held by the nucleus
electronegativity
the power of an atom in a molecule to attract electrons to itself
wavelength
distance between points of two consecutive waves
frequency
how often a wave occurs
speed of light
speed at which electromagnetic radiation travels through a vacuum
energy
electromagnetic radiation. travels through space by electromagnetic waves
VSEPR theory
valence shell electron pair repulsion theory
- predicts bond angle based on the repulsion of electrons
types molecular geometry
2linear, 3trigonal planar, 4tetrahedral, 5trigonal bipyramidal, 6octahedral
molecular structure
structure of the electron pair geometry
polar covalent bond
unequal sharing
covalent bonds
sharing of a pair of valence electrons
ionic bonds
electrons from one atom attach to another, positive and negative ions attract
why does atomic size decrease going up a family
fewer energy levels, less shielding, stronger pulling towards nucleus
non polar covalent bond
equal sharing
going down a group/family
- More energy levels
- Farther from nucleus
- Better shielding due to more core electrons.
- Decreasing ionization energy and electronegativity
- increasing radii
going across a period
- More protons
- Increased nuclear charge, pulling closer to nucleus
- Poor shielding (same-level electrons)
- Decreasing radii
- Increasing lonization energy and electronegativity
polarity
unequal sharing of electrons in a bond
Can a molecule have polar bonds but have an overall neutral (non-polar) charge?
yes
atoms with full shell
stable, unwilling to give up electrons. takes more ionization energy to remove
atoms with valence electrons
willing to give up electrons, less ionization energy to remove
resonance
electrons spread across the location of the bonds
