Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
30 Cards in this Set
- Front
- Back
crystalline solids
|
highly regular atomic arrangements
|
|
amorphous solids
|
disordered atomic arrangements
|
|
lattice
|
a three-dimensional array of points designating the centers of the components (atoms, ions, or molecules) that shows the repetitious pattern of the components
|
|
unit cell
|
the smalles repeating unit of the lattice
|
|
X-ray diffraction
|
the scattering of light from a regular array of points or lines. the spacing between the points or lines (planes for atoms) are related to the wavelength of the light. x-rays are used because there wavelengths are similar to distances between the atomic nuclei
|
|
ionic solids
|
form electrolytes when dissolved in water (NaCl) [brittle, high melting temp]
|
|
molecular solids
|
do not form electrolytes when dissolved (H20 - ice) [strong forces within molecules and weak inter molecular forces between molecules]
|
|
atomic solid
|
contains atoms of only one element, which are covalently bonded together (Diamond)
|
|
Bragg Equation
|
n(wavelength) = 2d sin (angle), where d is the distance between the atoms and angle is angle of incidence and reflection
|
|
protein crystallography
|
if a protein can be turned into a crystal then its structure can bet studied this way.
|
|
constructive interference
|
when waves are in phase (peaks on top of each other), the addition of these two waves has an amplitude equal to the sum of each
|
|
destructive interference
|
when waves are not in phase, the sum of the waves equals zero
|
|
closest (or close) packed
|
spheres packed as efficiently together as possible
|
|
hexagonal closest packed (hcp) structure
|
the resulting structure formed by an aba arrangement, with a hexagonal unit cell
(coordination number is 12) |
|
cubic closest packed (ccp) structure
|
the resulting structure formed by an abc arrangement, with a face-centered cubic unit cell (coordination number is 12)
|
|
body centered cubic structure
|
spheres are not closest packed, (coordination number is 8, 2 spheres per unit cell [1 full + 8 1/8)
|
|
simple cubic
|
formed by packing spheres on top of each other, not closest packed (each unit cell contains 8 1/8 spheres, = 1 total sphere, coordination number =8)
|
|
band model
|
molecular orbital model for metals, electrons are assumed to travel around the metal crystal in MOs formed from the valence atomic orbitals of the metal atoms
|
|
holes
|
spaces left by the packing of atoms that define the unit cell [trigonal < tetrahedral < octahedral < cubic)
|
|
substitutional alloy
|
some of the host metal atoms are replaced by the other metal atoms of a similar size (ex. brass)
|
|
interstitial alloy
|
formed when some of the holes in the closest packed metal structure are occupied by small atoms
|
|
CO2 vs SiO2
|
CO2 forms one sigma bond a one pi bond with oxygen
SiO2 (silica), however due to the large size of 3p orbitals, cannot form good pi bonds, so it froms networks build from single bonds |
|
silica
|
SiO2, where each O is shared between two Si
ex. quartz |
|
silicates
|
have O-Si ratios greater than 2:1 and thus some O are not fully bonded to the ions
ex. Feldspar, and many minerals |
|
N-type semiconductors
|
formed by adding small amounts of atoms with extra valence electrons, allowing for easier movement of conductions
|
|
P-type semiconductors
|
formed by adding a small amount of an element that has less valence electrons than silicon, forming positively charged holes that become occupied by electrons from neighboring atoms
|
|
mass percent
|
grams solute/ total grams (solute + solvent) = (grams/grams) x 100%
|
|
molarity
|
moles solute / volume of solution = M = (mol/L)
|
|
p-n junction
|
a small number of electrons migrate from the N-type region to the P-type region, where there are vacancies in the lower MOs.
|
|
critical temperature
|
the temperature above which the vapor cannot be liquified no matter how much pressure is applied
|