DAT GEN CHEM

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 Hg2==2+== (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 HPO3==2-== (hydrogen phosphite)

\-2

charge of HPO4==2-== (hydrogen phosphate)

\-2

charge of CO3==2-== (carbonate)

\-2

charge of SO3==2-== (sulfite)

\-2

charge of SO4==2-== (sulfate)

\-2

charge of S2O3==2-== (thiosulfate)

\-2

charge of C2O4==2-== (oxalate)

\-2

charge of CrO4==2-== (chromate)

\-2

charge of Cr2O7==2-== (dichromate)

\-2

charge of O2==2-== (peroxide)

\-2

charge of S2==2-== (disulfide)

\-2

charge of O==2-== (oxide)

\-2

charge of S==2-== (sulfide)

\-2

charge of PO4==3-== (phosphate)

\-3

charge of AsO3==3-== (arsenite)

\-3

charge of AsO4==3-== (arsenate)

\-3

charge of N==3-== (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)