OAT Gen Chem

Strong acids

HBr, HI, HCl, HClO3, HClO4, H2SO4, HNO3

Strong bases

group 1 metal hydroxides, Ba(OH)2, Sr(OH)2, Ca(OH)2

Soluble salts

group 1 metal cations, NO3-, NH4+, C2H3O2-, ClO4- (NNCCL- nickel)

Insoluble salts

Hg2+, OH-, Pb2+, PO43-, S2-, Ag+, CO32- (HOPPSAC)

Solubles trump insolubles T/F

T

Diatomic gases (x2)

H2, N2, F2, O2, I2, Cl2, Br2 (have no fear of ice cold beer)

Ionization energy

energy to remove e-

Ionization energy exceptions

group 2>13, group 15>16

Transition metal color exception

row 4 is colorless

e- affinity

energy released when e- added

e- affinity exceptions

group 2 low, group 14>15, noble gases=0

increases up, right

electronegativity, ionization energy, e- affinity (higher is more neg), nonmetallic character

increases down, left

metallic character, atomic radius

atomic radius higher in anions or cations?

anions

increases down, right

acidity

increases up, left

basicity

Boyle

P1V1=P2V2

Charles

V1/T1=V2/T2

Avogadro

V1/n1=V2/n2

Gay-Lussac

P1/T1=P2/T2

Combined

P1V1/T1=P2V2/T2

Ideal

PV=nRT (R= 0.0821 atm, 8.314 KPa)

Does strength of acids and bases depend on concentration?

No

Standard T, P, 1mol

T=273k, P=1 atm, 1 mol= 22.4L

Density

m/v=PM/RT

What type of collisions occur in an ideal gas?

Collisions are elastic, no energy is lost.

What is the motion of gas particles in an ideal gas?

Gas is in continuous, rapid, random motion.

What kind of forces exist between gas particles in an ideal gas?

There are no attractive or repulsive forces between gas particles.

Does an ideal gas have volume?

An ideal gas has no volume.

How do gas particles relate to each other in terms of distance in an ideal gas?

Gas particles are spread far apart from each other relative to their size.

Buffers

1. weak A +CB 1:1

2. weak B+ CA 1:1

3. strong A + weak base 1:2

4. strong B + weak acid 1:2

effusion

rate1/rate2=radical M2/M1

diluted/conc equation

M1V1=M2V2

Zeff

P-shield e-

Moles (n)

mass/molar mass

% error

(A-T)/T x 100

Bond order

(bonding-anti bonding)/2

Molarity (M)

moles solute/L solution

Absorption

(molar extinction coefficient)(conc- M)(path- cm)

vapor-pressure depression

x*p, x=mole fraction of solvent (mol solv/(mol solvent + mol solute)), p=pure vapor pressure of solvent

freezing pt depression

-kfim, m=molality

bp elevation

kbim, m=molality

osmotic pressure

iMRT, R=0.0821

Pressure

F/A

1/2 life

initial(1/2)^n, n=# half lives

Single step rxn rule

halogens higher up are more reactive

ex. won't see CaF2+Br2->CaBr2+F2

Endothermic

heat absorbed, solid to gas

Exothermic

heat released, gas to solid

Deposition

gas to solid

Sublimation

solid to gas

Trigonal planar

Tetrahedral

Trigonal pyramidal

Trigonal bipyrimidal

Octahedral

alpha decay

A-4, Z-2

beta+ (positron)

A, Z-1

beta- (beta)

A, Z+1

e- capture

A, Z-1

gamma decay

A, Z

Enthalpy

△H=Hprod-Hreact

=n(△Hprod)-m(△React), don't include mol in standard state (ex. O2, Cl2)

=bonds broken (react)-bonds formed (prod)

△H>0

Endothermic, break bonds

△H<0

Exothermic, form bonds

Entropy

Does increase dissolution (aq) increase/decrease entropy?

Increase

Does #product mol>#reactant mol increase/decrease entropy?

Increase

Positive work (+w)

Compressed, work done on system, △V<0

Negative work (-w)

Expansion, work done by system, △V>0

Internal energy △U

△U=q+w

Work given pressure and volume

w=-p△V, p=pressure

heat given mass and heat fusion/vap

q=m△H

Calorimetry equations

qrxn=-qcal, qcal=C△T

Reaction rate, Aa+Bb→Cc+Dd

Rate and order, A+B→C+D

rate=K[A]^m[B]^n

order=m+n (if 0, then not depend on reactants)

k and rate when temp increases

both increase

k and rate when decrease in Ea (add catalyst)

both increase

k and rate when reactants increase

k same, rate increase

Free energy (△G)

△G=△H-T△S

△G>0

Endergonic, not spontaneous

△G<0

Exergonic, spontaneous

-△H, △S, -△G

Spontaneous

-△H, -△S, -/+△G

Spontaneous (low T), not spontaneous (high T)

△H, △S, -/+△G

Spontaneous (high T), not spontaneous (low T)

△H, -△S, △G

Not spontaneous

keq and result when -△G

keq>1, product fav

keq and result when △G

keq<1, reactants fav

keq and result when △G=0

keq=1, equilibrium (not spontaneous or spontaneous)

0 order

rate=k

k=m/s

conc/t graph straight w negative slope

[A]/t graph straight w negative slope

slope=-k

decrease concentration is decrease 1/2 life

1st order

rate=k[A]

k=s^-1

conc/t graph curved w negative slope (exponential)

ln[A] graph curved w negative slope

slope=-k

1/2 life=0.693/k

2nd order

rate=k[A]^2

if A+B→C+D, rate=k[A][B]

k=M^-1S^-1

conc/t graph curved w negative slope (exponential)

1/[A] graph straight w positive slope

slope=k

decrease conc, increase 1/2 life

equation to work out k for order reaction

k=m^1-n, s^-1

k=Ae^(-Ea/RT), Ae=frequency factor, Ea=activation energy

pH

-log[H+]

pKa+log[A-]/[HA]

pOH

-log[OH-]

[H+]

10^-pH

[OH-]

10^-pOH

pKa

-logKa=([H+][A])/[HA]

Kw

=1 x 10^-14 at 25C

=[H+][OH-], 1x10^-7 each

=Ka(Kb)

Reducing agent

Oxidized, oxidation # increases, gains oxygen, loses H

H2, Fe, Zn, alkali metals

Oxidizing agent

Reduced, oxidation # decreases, gains H, loses oxygen

O2, O3, H2SO4, halogens

Oxidation number for oxygen

-2