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CHEMISTRY SAMPLE DATA SHEET
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Chemistry Sample Data Sheet 2016
2014/10138
Table of contents
Periodic table of the elements........................................................................................................ 3
Formulae........................................................................................................................................ 4
Units............................................................................................................................................... 4
Constants....................................................................................................................................... 4
Solubility rules for ionic solids in water........................................................................................... 4
Colours of selected substances..................................................................................................... 5
α-amino acids........................................................................................................................... 6 – 7
Standard reduction potentials......................................................................................................... 8
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3
[Data source: The International Union of Pure and Applied Chemistry Periodic Table of the Elements (May 2013)]
Periodic table
Formulae
Number of moles
n
=
m
=
M
Number of moles of solute
n
=
cV
Number of moles of a gas at STP
n
=
Parts per million
ppm =
pH of a solution
pH
mass
molar mass
V
22.71
mass of solute (mg)
mass of solution (kg)
= - log [H+]
Units
Volumes are given in the units of litres (L), or millilitres (mL)
Temperatures are given in the units of degrees Celsius (°C) or kelvin (K).
It may be assumed that 0.0 °C = 273.15 K
Energy changes are given in kilojoules (kJ)
Pressures are given in kilopascals (kPa)
Solution concentrations are given in the units moles per litre (mol L-1),
grams per litre (g L-1) or parts per million (ppm).
Constants
Universal gas constant, R = 8.314 J K-1 mol-1
Avogadro constant, N = 6.022×1023 mol-1
Volume of 1.00 mol of an ideal gas at 0.0 °C and 100.0 kPa is 22.71 L
S.T.P. is 0.0 °C and 100.0 kPa
Equilibrium constant for water at 25 °C, Kw = 1.00×10–14
Solubility rules for ionic solids in water
Soluble in water
Exceptions
Soluble
Most chlorides
Most bromides
Most iodides
Slightly soluble
PbCℓ2
PbBr2
Insoluble
AgCℓ
AgBr
AgI, PbI2
All nitrates
No exceptions
All ethanoates
Most sulfates
CaSO4, Ag2SO4
SrSO4, BaSO4, PbSO4
Insoluble in water
Insoluble
Exceptions
Soluble
Slightly soluble
Most hydroxides
NaOH, KOH, Ba(OH)2
NH4OH*, AgOH**
Ca(OH)2, Sr(OH)2
Most carbonates
Na2CO3, K2CO3, (NH4)2CO3
Most phosphates
Na3PO4, K3PO4, (NH4)3PO4
Most sulfides
Na2S, K2S, (NH4)2S
*
** NH3 dissolves in water to form both NH3 (aq) and NH4+(aq)/OH–(aq)
Ag+(aq) reacts with OH–(aq) to form insoluble Ag2O
Soluble = more than 0.1 mole dissolves per litre
Slightly soluble = between 0.01 and 0.1 mole dissolves per litre
Insoluble = less than 0.01 mole dissolves per litre
4
Colours of selected substances
In general, ionic solids have the same colour as that of any coloured ion they contain.
Two colourless ions in general produce a white solid.
Selected exceptions to these two basic rules are noted below.
Ionic Solid
Colour
Other coloured substances
copper(II) carbonate
green
copper(II) chloride
green
copper(II) oxide
black
Most gases and liquids are colourless, and most metals are
silvery or grey. Selected exceptions to these basic rules are
noted below.
copper(II) sulfide
black
lead(II) iodide
yellow
lead(II) sulfide
grey
manganese(IV) oxide
black
silver carbonate
yellow
silver iodide
pale yellow
silver oxide
brown
silver sulfide
black
Substance
State
Colour
copper
solid
salmon pink
gold
solid
yellow
nitrogen dioxide
gas
brown
sulfur
solid
yellow
Coloured halogens
Halogen
Colour of free element
F2(g)
yellow
Cℓ2(g)
greenish-yellow
Br2(ℓ)
red
I2(s)
purple
Halogen
Colour of halogen in aqueous solution
Cℓ2(aq)
pale yellow
Br2(aq)
orange
I2(aq)
brown
Halogen
Colour of halogen in organic solvent
Br2
red
I2
purple
Coloured ions in aqueous solution
Cation
2+
Co
pink
Cu2+
blue
Fe
2+
pale green
Fe
3+
pale brown
Mn
pale pink
2+
Ni2+
green
Anion
Colour
CrO42–
yellow
Cr2O7
orange
2–
MnO4
5
Colour
deep green
Cr
3+
–
purple
α–amino acids
Name
Symbol
alanine
Ala
Structure
CH3
H 2N
arginine
COOH
Arg
NH
H 2N
asparagine
CH
CH2
CH2
CH
COOH
CH2
NH
Asn
O
CH2
H 2N
aspartic acid
Asp
Cys
COOH
CH
COOH
CH2
SH
CH
COOH
Gln
O
CH2
H2 N
glutamic acid
H 2N
Gly
histidine
His
CH2
CH
Glu
glycine
NH2
COOH
CH2
H 2N
glutamine
C
CH
H2N
cysteine
C
CH2
CH2
CH
COOH
H 2N
NH2
COOH
CH2
COOH
COOH
N
CH2
H 2N
isoleucine
C
Ile
CH
N
H
COOH
CH3
CH
CH2
H2N
CH
COOH
6
CH3
NH2
α–amino acids
Name
Symbol
leucine
Leu
Structure
CH3
CH
CH3
CH2
H 2N
lysine
Lys
H2N
methionine
CH2
CH2
CH
COOH
Met
H2N
phenylalanine
CH
CH2
CH
COOH
serine
Ser
threonine
tryptophan
CH2
S
CH3
CH2
H2N
Pro
CH2
CH2
Phe
proline
COOH
CH
H
N
CH2
Thr
COOH
COOH
OH
H2N
CH
COOH
CH3
CH
OH
H 2N
CH
COOH
H
N
Trp
CH2
H 2N
tyrosine
Tyr
COOH
CH2
H2 N
valine
CH
Val
7
CH
OH
COOH
CH3
CH
CH3
H 2N
CH
COOH
NH2
Standard Reduction Potentials at 25 °C
Half-reaction
F2(g) + 2 e
H2O2(aq) + 2 H (aq) + 2 e
+
PbO2(s) + SO4 (aq) + 4 H (aq) + 2 e
2–
+
2 F (aq)
+ 2.89
–
2 H2O(ℓ)
+ 1.76
–
2 HCℓO(aq) + 2 H+(aq) + 2 e–
MnO4–(aq) + 8 H+(aq) + 5 e–
Au3+(aq) + 3 e–
HCℓO(aq) + H (aq) + 2 e
–
PbO2(s) + 4 H (aq) + 2 e
–
+
+
Cℓ2(g) + 2 e
Cr2O7 (aq) + 14 H (aq) + 6 e
2–
+
O2(g) + 4 H (aq) + 4 e
+
E°(volts)
–
–
PbSO4(s) + 2 H2O(ℓ) + 1.69
Cℓ2(g) + 2 H2O(ℓ)
+ 1.63
Mn2+(aq) + 4 H2O(ℓ) + 1.51
Au(s)
+ 1.50
Cℓ (aq) + H2O(ℓ)
+ 1.49
–
Pb (aq) + 2 H2O(ℓ)
2+
+ 1.46
–
2 Cℓ (aq)
–
2 Cr (aq) + 7 H2O(ℓ) + 1.36
–
+ 1.36
–
3+
2 H2O(ℓ)
+ 1.23
–
–
2 Br (aq)
+ 1.08
Ag (aq) + e
–
Ag(s)
+ 0.80
Fe (aq) + e
–
Fe (aq)
+ 0.77
O2(g) + 2 H (aq) + 2 e
–
H2O2(aq)
+ 0.70
Br2(ℓ) + 2 e
+
3+
+
I2(s) + 2 e
2+
2 I (aq)
+ 0.54
–
4 OH (aq)
+ 0.40
Cu (aq) + 2 e
–
Cu(s)
+ 0.34
S(s)+ 2 H (aq) + 2 e
–
+ 0.17
2 H (aq) + 2 e
H2S(aq)
–
Pb (aq) + 2 e
–
Pb(s)
– 0.13
Sn (aq) + 2 e
–
Sn(s)
– 0.14
Ni (aq) + 2 e
–
Ni(s)
– 0.24
Co (aq) + 2 e
–
Co(s)
–
O2(g) + 2 H2O(ℓ) + 4 e
2+
+
+
2+
2+
2+
2+
PbSO4(s) + 2 e
–
–
–
H2(g)
0 exactly
– 0.28
Pb(s) + SO4 (aq)
2–
– 0.36
Cd (aq) + 2 e
–
Cd(s)
– 0.40
2 CO2(g) + 2 H (aq) + 2 e
–
– 0.43
Fe2+(aq) + 2 e–
H2C2O4(aq)
Fe(s)
– 0.44
Cr (aq) + 3 e
–
Cr(s)
– 0.74
Zn (aq) + 2 e
–
Zn(s)
2+
+
3+
2+
2 H2O(ℓ) + 2 e
–
Mn 2+(aq) + 2 e–
– 0.76
H2(g) + 2 OH (aq)
–
– 0.83
Mn(s)
– 1.18
Aℓ (aq) + 3 e
–
Aℓ(s)
– 1.68
Mg (aq) + 2 e
–
Mg(s)
– 2.36
Na (aq) + e
–
Na(s)
– 2.71
Ca2+(aq) + 2 e–
Ca(s)
– 2.87
Sr (aq) + 2 e
–
Sr(s)
– 2.90
Ba (aq) + 2 e
–
Ba(s)
– 2.91
K (aq) + e
–
K(s)
– 2.94
3+
2+
+
2+
2+
+
[Data source: Aylward, G.H., & Findlay, T. (2008). SI Chemical Data (6th ed.). Queensland: John Wiley & Sons Australia, Ltd.]
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