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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)
diatomic ions
hydrogen, nitrogen, oxygen, bromine, chlorine, iodine, fluorine
allotropes
molecules with different formulas whose atoms are all of the same element (ex. O2 and O3; S6, S8, and S12)
charge of NH4==+== (ammonium)
+1
charge of H3O==+== (hydronium)
+1
charge of Hg22+ (mercury I)
+1
charge of H2PO3==-== (dihydrogen phosphite)
-1
charge of H2PO4==-== (dihydrogen phosphate)
-1
charge of HCO3==-== (hydrogen carbonate)
-1
charge of HSO3==-== (hydrogen sulfite)
-1
charge of HSO4==-== (hydrogen sulfate)
-1
charge of NO2==-== (nitrite)
-1
charge of NO3==-== (nitrate)
-1
charge of OH==-== (hyrdoxide)
-1
charge of CH3COO==-== (acetate)
-1
charge of CrO2==-== (chromite)
-1
charge of CN==-== (cyanide)
-1
charge of CNO==-== (cyanate)
-1
charge of CNS==-== (thiocyanate)
-1
charge of MnO4==-== (permanganate)
-1
charge of ClO==-== (hypochlorite)
-1
charge of ClO2==-== (chlorite)
-1
charge of ClO3==-== (chlorate)
-1
charge of ClO4==-== (perchlorate)
-1
charge of BrO==-== (hypobromite)
-1
charge of BrO2==-== (bromite)
-1
charge of BrO3==-== (bromate)
-1
charge of BrO4==-== (perbromate)
-1
charge of IO==-== (hypoiodite)
-1
charge of IO2==-== (iodite)
-1
charge of IO3==-== (iodate)
-1
charge of IO4==-== (periodate)
-1
charge of N3==-== (azide)
-1
charge of HPO32- (hydrogen phosphite)
-2
charge of HPO42- (hydrogen phosphate)
-2
charge of CO32- (carbonate)
-2
charge of SO32- (sulfite)
-2
charge of SO42- (sulfate)
-2
charge of S2O32- (thiosulfate)
-2
charge of C2O42- (oxalate)
-2
charge of CrO42- (chromate)
-2
charge of Cr2O72- (dichromate)
-2
charge of O22- (peroxide)
-2
charge of S22- (disulfide)
-2
charge of O2- (oxide)
-2
charge of S2- (sulfide)
-2
charge of PO43- (phosphate)
-3
charge of AsO33- (arsenite)
-3
charge of AsO43- (arsenate)
-3
charge of N3- (nitride)
-3
SI unit: terra
10^12
SI unit: giga
10^9
SI unit: mega
10^6
SI unit: kilo
10^3
SI unit: centi
10^-2
SI unit: milli
10^-3
SI unit: micro
10^-6
SI unit: nano
10^-9
p-orbitals have __ shapes/p-orbitals per shell
3
d-orbitals have __ shapes/p-orbitals per shell
5
f-orbitals have __ shapes/p-orbitals per shell
7
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
paramagnetic
has unpaired electrons, attracted to magnets, odd or even number of electrons (ex. O2)
diamagnetic
has no unpaired electrons, repelled by magnets, even number of electrons (ex. N2)
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
kinetic energy of electrons equation
E photon- work function
work function= the minimum amount of energy required to ionize the electrons
types of compounds
ionic, molecular, network covalent, and metallic
features of ionic compounds
high melting points, high boiling points, brittle, hard, held together by ionic interactions (lattice energy), examples include NaCl and MgO
features of molecular compounds
low melting points, do not conduct electricity, held together by IMFs, examples include H2O and Cl-Cl and CH2
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)
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
lattice energy equation
[(cation charge) x (anion charge)]/bond distance
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
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
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
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
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
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
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
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
features to know about noble gases
group 8 on PT, unreactive gases, they have a full octet so are happy
features to know about transition metals
found in the d-block of PT, often form brightly colored compounds, can have multiple oxidation states
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
boyle’s law
as pressure decreases, volume increases and vice versa
charles’ law
as volume decreases, temperature decreases; as volume increases, temperature increases
avogadro’s law
as volume decreases, the number of moles decreases; as volume increases, the number of moles increases
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
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)
Heisenberg uncertainty principle
you cannot simultaneously know everything about an electron’s location and momentum
dalton’s law
total pressure inside a container filled with multiple gases = sum of the gases’ individual pressures
kinetic energy equation
(1/2 x mass) x (velocity)^2
graham’s law
effusion rate 1/effusion rate 2= sqaure root of mw2/mw1
unit cells: simple cubic
only one total atom inside the cell
unit cells: body centered cubic
two atoms per cell
unit cells: face centered cubic
four atoms per cell
sublimation
solid -→ gas (endothermic, +deltaH; create disorder, +deltaS)
melting (fusion)
solid -→ liquid (endothermic, +deltaH; create disorder, +deltaS)
boiling (vaporization)
liquid -→ gas (endothermic, +deltaH; create disorder, +deltaS)
deposition
gas -→ solid (exothermic, -deltaH; create order, -deltaS)
condensation
gas -→ liquid (exothermic, -deltaH; create order, -deltaS)