DAT GEN CHEM

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239 Terms

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equation for density of gas
p= PM/RT

p= density of gas (g x L^-1)

P= pressure (atm)

M= molar mass (g)

R= ideal gas constant \[0.0821 (L x atm/mol x K)\]

T= temperature (K)
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diatomic ions
hydrogen, nitrogen, oxygen, bromine, chlorine, iodine, fluorine
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allotropes
molecules with different formulas whose atoms are all of the same element (ex. O2 and O3; S6, S8, and S12)
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charge of NH4==+== (ammonium)
\+1
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charge of H3O==+== (hydronium)
\+1
6
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charge of Hg2==2+== (mercury I)
\+1
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charge of H2PO3==-== (dihydrogen phosphite)
\-1
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charge of H2PO4==-== (dihydrogen phosphate)
\-1
9
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charge of HCO3==-== (hydrogen carbonate)
\-1
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charge of HSO3==-== (hydrogen sulfite)
\-1
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charge of HSO4==-== (hydrogen sulfate)
\-1
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charge of NO2==-== (nitrite)
\-1
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charge of NO3==-== (nitrate)
\-1
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charge of OH==-== (hyrdoxide)
\-1
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charge of CH3COO==-== (acetate)
\-1
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charge of CrO2==-== (chromite)
\-1
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charge of CN==-== (cyanide)
\-1
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charge of CNO==-== (cyanate)
\-1
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charge of CNS==-== (thiocyanate)
\-1
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charge of MnO4==-== (permanganate)
\-1
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charge of ClO==-== (hypochlorite)
\-1
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charge of ClO2==-== (chlorite)
\-1
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charge of ClO3==-== (chlorate)
\-1
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charge of ClO4==-== (perchlorate)
\-1
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charge of BrO==-== (hypobromite)
\-1
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charge of BrO2==-== (bromite)
\-1
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charge of BrO3==-== (bromate)
\-1
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charge of BrO4==-== (perbromate)
\-1
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charge of IO==-== (hypoiodite)
\-1
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charge of IO2==-== (iodite)
\-1
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charge of IO3==-== (iodate)
\-1
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charge of IO4==-== (periodate)
\-1
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charge of N3==-== (azide)
\-1
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charge of HPO3==2-== (hydrogen phosphite)
\-2
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charge of HPO4==2-== (hydrogen phosphate)
\-2
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charge of CO3==2-== (carbonate)
\-2
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charge of SO3==2-== (sulfite)
\-2
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charge of SO4==2-== (sulfate)
\-2
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charge of S2O3==2-== (thiosulfate)
\-2
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charge of C2O4==2-== (oxalate)
\-2
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charge of CrO4==2-== (chromate)
\-2
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charge of Cr2O7==2-== (dichromate)
\-2
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charge of O2==2-== (peroxide)
\-2
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charge of S2==2-== (disulfide)
\-2
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charge of O==2-== (oxide)
\-2
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charge of S==2-== (sulfide)
\-2
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charge of PO4==3-== (phosphate)
\-3
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charge of AsO3==3-== (arsenite)
\-3
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charge of AsO4==3-== (arsenate)
\-3
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charge of N==3-== (nitride)
\-3
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SI unit: terra
10^12
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SI unit: giga
10^9
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SI unit: mega
10^6
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SI unit: kilo
10^3
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SI unit: centi
10^-2
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SI unit: milli
10^-3
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SI unit: micro
10^-6
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SI unit: nano
10^-9
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p-orbitals have __ shapes/p-orbitals per shell
3
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d-orbitals have __ shapes/p-orbitals per shell
5
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f-orbitals have __ shapes/p-orbitals per shell
7
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quantum numbers formula
n, l, ml, ms

n= principal; the energy level/distance from nucleus; range is 1-infinity

l= azimuthal; the type of orbital it is (l=0=s, l=1=p, l=2=d, l=3=f); range is 0, 1, 2, or 3

ml= magnetic; shares which p, d, or f orbital you have (oriental space); range is \[-l -→ +l\]

ms= spin; shares the electrons spin; range is either +1/2 or -1/2
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paramagnetic
has unpaired electrons, attracted to magnets, odd or even number of electrons (ex. O2)
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diamagnetic
has no unpaired electrons, repelled by magnets, even number of electrons (ex. N2)
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equation for the energy of a photon
E photon= hf= hc/w

h= Planck’s constant= 6.63 x 10^-34 J x sec

f= photon’s frequency= c/w

c= speed of light= 3.0 x 10^8 m/sec

w= photon’s wavelength
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kinetic energy of electrons equation
E photon- work function

\
work function= the minimum amount of energy required to ionize the electrons
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types of compounds
ionic, molecular, network covalent, and metallic
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features of ionic compounds
high melting points, high boiling points, brittle, hard, held together by ionic interactions (lattice energy), examples include NaCl and MgO
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features of molecular compounds
low melting points, do not conduct electricity, held together by IMFs, examples include H2O and Cl-Cl and CH2
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features of network covalent compounds
high melting points, high boiling points, hard, do not conduct electricity, held together by a network of covalent bonds, examples include C (diamond and graphite) and SiO2 (quartz)
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features of metallic compounds
variable hardness and melting points, conducts electricity, conducts heat, lustrous (shiny), malleable, ductile, held together by metallic bonding, examples include Fe and Mg
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lattice energy equation
\[(cation charge) x (anion charge)\]/bond distance
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if there are two “things” surrounding the atom…
electron domain: 2

hybridization: sp

bond angles: 180 degrees

electron-domain geometry: linear

non-bonding electron pairs: 0

molecular geometry: linear
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if there are three “things” surrounding the atom…
electron domain: 3

hybridization: sp2

bond angles: 120 degrees

electron-domain geometry: trigonal planar

non-bonding electron pairs: 0 or 1

molecular geometry: trigonal planar or bent
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if there are four “things” surrounding the atom…
electron domain: 4

hybridization: sp3

bond angles: 109.5 degrees

electron-domain geometry: tetrahedral

non-bonding electron pairs: 0, 1, or 2

molecular geometry: tetrahedral, trigonal pyramid, bent
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if there are five “things” surrounding the atom…
electron domain: 5

hybridization: sp3d

bond angles: 90, 120, or 180 degrees

electron-domain geometry: trigonal bipyramid

non-bonding electron pairs: 0, 1, 2, or 3

molecular geometry: trigonal bipyramid, see-saw, t-shaped, linear
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if there are six “things” surrounding the atom…
electron domain: 6

hybridization: sp3d2

bond angles: 90 degrees

electron-domain geometry: octahedral

non-bonding electron pairs: 0, 1, or 2

molecular geometry: octahedral, square pyramid, square planar
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features to know about alkali metals
group 1 on PT, low ionization energies, very reactive with water, readily form compounds

\
reaction with water: M (s) + H2O (l) -→ MOH (aq) + 1/2H2 (g); VERY exothermic reaction
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features to know about alkaline earth metals
group 2 on PT, low ionization energies (not as low as alkali metals), reacts with H2O (not as violently as alkali metals), becomes more reactive with H20 as you go down the group
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features to know about halogens
group 7A on PT, high electronegativities and electron affinities, easily reduced because they really want an extra electron, highly reactive with metals, good oxidizing agents
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features to know about noble gases
group 8 on PT, unreactive gases, they have a full octet so are happy
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features to know about transition metals
found in the d-block of PT, often form brightly colored compounds, can have multiple oxidation states
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features to know about oxygen group/chalcogens
group 6A on PT, two forms of molecular oxygen: O2 and O3, metals like to react with oxygen to form metal oxides
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boyle’s law
as pressure decreases, volume increases and vice versa
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charles’ law
as volume decreases, temperature decreases; as volume increases, temperature increases
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avogadro’s law
as volume decreases, the number of moles decreases; as volume increases, the number of moles increases
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combined gas law
P1 x V1/n1 x T1=P2 x V2/ n2 x T2

\
P= pressure

V= volume

n= number of moles

T= temperature
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ideal gas law
PV=nRT

P= pressure (atm)

V= volume (L)

n= number of moles

R= ideal gas constant= 0.0821 L x atm/ mol x K

T= temperature (Kelvins)
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Heisenberg uncertainty principle
you cannot simultaneously know everything about an electron’s location and momentum
90
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dalton’s law
total pressure inside a container filled with multiple gases = sum of the gases’ individual pressures
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kinetic energy equation
(1/2 x mass) x (velocity)^2
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graham’s law
effusion rate 1/effusion rate 2= sqaure root of mw2/mw1
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unit cells: simple cubic
only one total atom inside the cell
only one total atom inside the cell
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unit cells: body centered cubic
two atoms per cell
two atoms per cell
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unit cells: face centered cubic
four atoms per cell
four atoms per cell
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sublimation
solid -→ gas (endothermic, +deltaH; create disorder, +deltaS)
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melting (fusion)
solid -→ liquid (endothermic, +deltaH; create disorder, +deltaS)
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boiling (vaporization)
liquid -→ gas (endothermic, +deltaH; create disorder, +deltaS)
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deposition
gas -→ solid (exothermic, -deltaH; create order, -deltaS)
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condensation
gas -→ liquid (exothermic, -deltaH; create order, -deltaS)