The two redox half reactions are taking place as follows:

Cr --> Cr³⁺ + 3e^-

3e^- + 4H⁺ + NO₃^- --> NO + 2H₂O

covalently bonded oxides bubbled into water make?

(SO₂ + H₂O --> ?)

acids

(H₂SO₃₎

Ionically bonded oxides bubbled into water form what?

(CaO + H₂O --> ?)

bases

(Ca(OH)₂)

exothermic, and product

(a negative relationship produces an ex)

an acid with a difference of 1 between H and O is (strong/weak)

(ex: H₂SO₃)

group I and II elements + OH^- make ____ bases

(Ca(OH)₂)

a base with N & H together is _______

(NH₃)

could act as an acid or a base

(ex: HPO₄^2-)

when something is introduced into a system, the reaction proceeds to use that something up

can be used to explain the effect that temperature, concentration, or pressure changes have on a reaction

produced and used up in a mechanism

can't be used in rate law

ln(P₁/P₂) = (-ΔH_vap/R)((1/T₂)-(1/T₁))

ln(k₁/k₂) = (-E_a/R)((1/T₂)-(1/T₁))

R=8.31 J/molxK

zero order: [A] = -kt+[A]_o

first order: ln[A] = -kt+ln[A]_o

second order: 1/[A]=kt+(1/[A]_o)

zero order: [A]_o/2k

first order: .693/k

second order: 1/[A]_ok

lowered

P_soln=(mols of solvent/(mols solvent + (mols solute x i)))(P_solvent)

goes down as radius goes up

low bond length means high BE

triple>double>single

BERP -> Bond Energy = Reactants - Products

0 is ideal

if not ^, then most electronegative is -, while least is +

each atom gets 2 per lone pair, and 1 per bond

valence electrons - electrons controlled in the molecule

ex: CF₄ - each bond is :::F-C

F: 7-7=0

C: 4-4=0

0(1) + 0(4)=0

large radii, low electronegativity, low zeff

ex: Xe, Kr, I, Br, S, Se, P

n - period # for s & p orbitals, period-1 for d, -2 for f

l - orbital, s=0, p=1, d=2, f=3

m - can be any number between -l and l (pick 0 to be safe)

s - can be 1/2 or -1/2, doesn't matter which

must fill to next level before jumping to n=1

(all of 2s and 2p must be filled before going to 3s)

place 1 e^- in each orbital before doubling up

(this creates magnetic field in molecules with any unfilled orbitals)

isotope - same protons, different neutrons

isoelectronic - different elements, same e^-

isomer - same formula, different structure

-ane -> only single bonds in backbone

-ene -> has a double bond in backbone

-yne -> has a triple bond in backbone

meth- one

eth- two

prop - three

but - four

pent - five

hex - six

hept - seven

oct - eight

when hydrogen bonds to N,O,F

only in a polar molecule

form of IMF

strongest type of bond

Si forms a network covalent

element is 0

Monatomic ion is same as charge

F = -1

O = -2, except in peroxides = -1

H = +1

colors:

Cr

MnO₄^-

Fe

Co

Ni

Cu

Pb as solid

Cr - orangeish

MnO₄^- - purple

Fe - orange

Co - pink

Ni - green

Cu - blue

Pb as solid - yellow

metal-ic ions reduced produces _____________

(Fe³⁺)

metal-ous ions

(Fe²⁺)

Free halogens reduced produces ______________

(I₂)

halide ions

(I^-)

Halide ions oxidized produces _________

(I^-)

free halogens

(I₂)

free metals oxidized produces _________

(Fe)

metal ions

(Fe²⁺)

hypohalite ions

metal-ous ions oxidized produces _________

(Fe²⁺)

metal-ic ions

(Fe³⁺)

Lewis Acid/Base combination

(BF₃ + NH₃ --> ?)

addition

(BF₃NH₃)

metallic oxides + P₄O₁₀ --> ?

(CaO + P₄O₁₀ --> ?)

metallic phosphates

(Ca₃(PO₄)₂)

metallic oxides + CO₂ --> ?

(CaO + CO₂ --> ?)

metallic carbonates

(CaCO₃)

metallic oxides + SO₃ --> ?

(CaO + SO₃ --> ?)

metallic sulfates

(CaSO₄)

metals + gases --> ?

(Na + O₂ --> ?)

ionic crystals

(Na₂O)

metallic oxides + SO₂ --> ?

(CaO + SO₂ --> ?)

metallic sulfites

(CaSO₃)

metallic carbonates --> ?

(CaCO₃ --> ?)

metallic oxides + CO₂

(CaO + CO₂)

metallic chlorates --> ?

(NaClO₃)

metallic chlorides + O₂

(NaCl + O₂)

metallic sulfides + O₂ --> ?

(CaS + O₂ --> ?)

metallic oxide + SO₂

(CaO + SO₂)