Stuff I Should Know (Page 2)
2nd DRAFT
Complex Ions & Common Ligands
Ligands
polar molecules & anions
Central Ions transition metals and Al3+
Examples
usually twice the number of ligands as
the charge on the central ion.
Key Words: “excess, concentrated”
Organic Chemistry & Functional Groups
alkanes
alkenes
Cn H2n+2
Cn H2n
alcohol
NH3 , H2 O, OH−, CN−, Cl−
Ag +, Cu 2+, Ni2+, Zn2+, etc. & Al3+
Ag(CN)2 −, Cu(NH3 )4 2+,
Ni(OH)4 2−, Zn(NH3 )4 2+,
Al(OH)6 3−
alkynes
Cn H2n−2
aromatics (benzene)
C6 H6
ketone
ether
aldehyde
Odd example:
Fe3+ + SCN−
FeSCN2+
Reaction with Acid:
Cu(NH3 )4 2+ + H+ → Cu 2+ + NH4 +
nuclear chem
alpha
4
2
He
beta/electron
0
−1
carboxylic acid
ester
amine
amide
e
neutron
1
0
n
positron
Substituted benzene:
ortho = 1,2
meta = 1,3
0
+1
para = 1,4
e
Lewis Acids & B ases
BF3 + NH3 → BF3 NH3
acid anhydrides (oxides of nonmetals, CO2 )
basic anhydrides (oxides of metals, MgO)
MgO + CO2 → MgCO3
decomposition reactions: MgCO3 → MgO + CO2
Strange Examples:
P4 O10 + H2 O → H3 PO4
Electrochemical Cells
anode
cathode
oxidation
reduction
+ side
− side
lower E°
higher E°
e− leave
e− enter
Strange Ions: (nitride, N3−) (hydride, H−)
Li + N2 → Li3 N
LiH + H2 O → H2 + Li+ + OH−
SN & hybridization & shape
Steric Number
hybridization
1
s
2
sp
3
sp2
4
sp3
5
sp3 d
6
sp3 d2
Flame Test Colors
Barium – green
Sodium – yellow
Copper – blue (w/ green)
Potassium – lavender
Strontium – red
Lithium – red
Calcium – orange
Quantum Numbers
1, 2, 3, …
n
l
0 … (n−1)
ml
−l … +l
ms
+½, −½
l
IMF’s
London
dipole−dipole
hydrogen bonding
0 = s, 1 = p,
2 = d, 3 = f
Writing Lewis Structures
hint: use one valence electron to connect F’s or Cl’s then
determine lone pairs (Ex: XeF4 )
metallic
ionic
Product−Favored Reactions
∆G < 0
E° > 0
Keq > 1
covalent network
IMF BP FP Hvap Hfus
IMF
BP
FP
Hvap
H fus
VP
VP
Orders of Reactions & Graphs That Give Straight Lines
0 Order
1st Order
2nd Order
[R] vs. Time
ln[R] vs. Time
1/[R] vs. Time
slope = -k
slope = -k
slope = k
Bond Orders
bond
B.O.
single
1
σ
double
2
σ+π
triple
3
σ+π+π
basic shape
−−
linear
r planar
tetrahedral
r bipyramidal
octahedral
nonpolar molecules, ex: CH4 , He
polar molecules, ex: H2 S, SO2
H−F, H−O−, H−N−, NH3 , H2 O
amines and alcohols
metals, Ag, Pb
salts, NaCl, Ca CO3
(Note: “ates” contain covalent bonds)
C(graphite), C(diamond), SiO2 , WC,
Si, SiC (Note: graphite = London, too)
Activity of Metals (Four Groups)
Metals
React with…
Groups I & II H2 O ex: Li + H2 O → Li+ + OH− + H2
Non-oxidizing Acid, ex: HCl
all others
Zn + 2HCl → H2 + ZnCl2
Oxidizing Acid, HNO3 or H2 SO4 (conc.)
Cu, Ag, Hg
Cu + HNO3 → NO2 + H2 O + Cu 2+
Au, Pt, Ir
Aqua Regia (HNO3 + HCl)