Section 1
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doping
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Last updated
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Date created
Mar 1, 2020
Cards (83)
Section 1
(50 cards)
doping
the addition of an impurity to an existing lattice
n-doping
add a substance with one MORE valence e- which leaves a free e- to travel freely i.e. si + p
resonance structures
structures that occur when it is possible to draw two or more valid lewis electron dot diagrams that have the same number of electron pairs for a molecule or ion
substitutional alloy
metal atoms with similar radii combine; ex. brass
paper chromatography
the separation of a mixture by passing it through a medium in which the components of the solution move at different rates
double bonds
one sigma bond, one pi bond; two e- pairs
p-doping
create a hole (positively charged) that draws electrons through the substance (add a substance with one LESS valence e-) i.e. si + al
column chromatography
a column is packed with stationary substance, then the solution to be separated (analyte) is injected into the column where it adheres to the stationary phase, then the eluent solution is injected into the column. as the eluent solution passes through the stationary phase the analyte molecules will be attracted to it with varying degrees of strength based on polarity
network covalent bonds
lattice of covalent bonds; network solid (acts similar to one molecule); very hard, high melting/boiling points; poor conductors
isotope
element with a different number of neutrons
distillation
the process that separates the substances in a solution based on their boiling points
octahedral geometry
6 e- pairs, sp5 hybridization 0 lone pairs: octahedral (6 bonds) [SF6] 1 lone pair: square pyramidal (5 bonds) [BrF5, IF5] 2 lone pairs: square planar (4 bonds) [XeF4]
tetrahedral geometry
4 e- pairs, sp3 hybridization angles 109.5 0 lone pairs: tetrahedral (four bonds) [CH4, NH4+, ClO4-, SO4 2-, PO4 3-] 1 lone pair: trigonal pyramidal (3 bonds) [NH3, PCl3, SO3 2-] 2 lone pairs: bent (2 bonds) [H2O, OF2, NH2-]
ionic bond
bond between metal and nonmetal; electrons are NOT shared: the cation gives an e- up to the anion
more polar molecule....
.... larger dipole moment
maxwell-boltzmann diagrams
shows the range of velocities for molecules of a gas
molecular formula
actual formula for a substance
substances with only london dispersion forces usually...
... are gases at room temp, and boil/melt at extremely low temps
hydrogen bonding
strong IMF between two moelcules; F, O, N; have higher melting and boiling points than molecules with other IMFs
empirical formula
simplest ratio of the molecules making up a compound
dipole-dipole forces
the positive end of one polar molecule is attracted to the negative end of another molecule; relatively weak attraction force
trigonal planar geometry
sp2 hybridization bond angles 120 0 lone pairs: trigonal planar (three bonds) 1 lone pair: bent (two bonds)
formal charge
used to find which structure is most likely to occur; valence - assigned
triple bonds
one sigma bond, two pi bonds; 3 e- pairs; shortest bond, most energy
interstitial alloy
metal atoms with vastly different radii combine; ex. steel
retention factor
stronger the attraction between the solute and the solvent front is, the larger the Rf value will be
dipole moment
the measurement of the polarity of a molecule; the unit of measurement is a debye (D)
intermolecular forces (IMFs)
forces that exist between molecules in a covalently bonded substance; not bonds
polarity
exists when a molecule has a clustering of negative charge on one side due to unequal sharing of electrons (e- are pulled to the more electronegative side); creates dipoles in molecules
trigonal bipyramidal geometry
5 e- pairs, sp4 hybridization 0 lone pairs: trigonal bipyramidal (5 bonds) [PCl5, PF5] 1 lone pair: seesaw (4 bonds) [SF4, IF4+] 2 lone pairs: t-shaped (3 bonds) [ClF3, ICl3] 3 lone pairs: linear (2 bonds) [XeF2, I3-]
avogadros number
6.022 E23
mass spectrometry
mass of various isotopic elements to create a mass spectrum graph
london dispersion forces
IMFs that occur between all molecules; occur because of the random motions of electrons on atoms within molecules to create instantaneous polarities; molecules with more e- will have greater _________________ forces
coulombs law
the amount of energy that an electron has depends on its distance from the nucleus of an atom; e=k(q1*q20)/r
periodic trend: down a group
periodic trend: atomic radius increases; shells of electrons are added which shield the more distant shells and valence e- get farther away ionization energy decreases (shells of e- added, each inner shell shields more and reduces the pull on valence e- so they are easier to remove)
covalent bonds
bond in which two atoms share electrons; each atom counts the e- as a part of its valence shell
effusion
the rate at which a gas will escape from a container through microscopic holes in the surface of the container
the common network solids
SiO2,
melting & boiling points of a covalent substance is almost always _____________ than that of ionic substances
lower
ionization energy
amount of energy necessary to remove electrons from an atom (electromagnetic energy exceeds binding energy)
metallic bonding
bond between two metals; sea of electrons that make metals such good conductors; delocalized structure allows for malleability and ductility
linear geometry
sp hybridization 0 lone pairs ex. BeCl2 & CO2
? L/mol
22.4 L
shielding electrons
electrons between a valence electron and the nucleus that decreases the attraction between the nucleus and the valence electron
dissociation
when ionic substances break up into ions into solution
vapor pressure
the pressure exerted by a vapor over a liquid
single bonds
one sigma bond, one e- pair; longest bond, least energy
mole fraction
moles of substance/total moles in solution
electrolytes
free ions in solution that conduct electricity
periodic trend: left to right
periodic trend: atomic radius decreases; protons are added to the nucleus so valence electrons are more strongly attracted ionization energy increases (protons are added to the nucleus)
Section 2
(33 cards)